2014 unit 8
TRANSCRIPT
Letrsquos look at our goalObjectives 1-4 possibly 5
Unit 8 Outline
Pg 365 1-6 amp pg 370 1-6 (assigned at the end of day 1)
Models thus far
What was wrong with Rutherfordrsquos model First came Bohrhellip then
Electrons ndash are they waves or particles Yes
e- how do they lets us see light of different colors Whatrsquos up with that
e- and their location in atoms Ions Etc
NEXT What is e- configuration
bull1 EVOLUTION OF MODELDalton Thomson Rutherford Bohr
The Development of Atomic Models
The timeline shoes the development of atomic models from 1803 to 1911
51
bullDaltonSolid indivisible (no parts inside)
Combine in simple ratios
Same element are identicalhellipcanrsquot change chemically into other element
Can mix chemically but elements are not changed into other atoms
DID EXPERIMENTS TO PROVE HIS THEORIES AS OPPOSED TO PREDICESSORS
bullTHOMSONUsed CRT to discover electrons because it bent
toward a positive plate
Later discovered proton too
Plum pudding model
Unit 8 Outline
Pg 365 1-6 amp pg 370 1-6 (assigned at the end of day 1)
Models thus far
What was wrong with Rutherfordrsquos model First came Bohrhellip then
Electrons ndash are they waves or particles Yes
e- how do they lets us see light of different colors Whatrsquos up with that
e- and their location in atoms Ions Etc
NEXT What is e- configuration
bull1 EVOLUTION OF MODELDalton Thomson Rutherford Bohr
The Development of Atomic Models
The timeline shoes the development of atomic models from 1803 to 1911
51
bullDaltonSolid indivisible (no parts inside)
Combine in simple ratios
Same element are identicalhellipcanrsquot change chemically into other element
Can mix chemically but elements are not changed into other atoms
DID EXPERIMENTS TO PROVE HIS THEORIES AS OPPOSED TO PREDICESSORS
bullTHOMSONUsed CRT to discover electrons because it bent
toward a positive plate
Later discovered proton too
Plum pudding model
bull1 EVOLUTION OF MODELDalton Thomson Rutherford Bohr
The Development of Atomic Models
The timeline shoes the development of atomic models from 1803 to 1911
51
bullDaltonSolid indivisible (no parts inside)
Combine in simple ratios
Same element are identicalhellipcanrsquot change chemically into other element
Can mix chemically but elements are not changed into other atoms
DID EXPERIMENTS TO PROVE HIS THEORIES AS OPPOSED TO PREDICESSORS
bullTHOMSONUsed CRT to discover electrons because it bent
toward a positive plate
Later discovered proton too
Plum pudding model
The Development of Atomic Models
The timeline shoes the development of atomic models from 1803 to 1911
51
bullDaltonSolid indivisible (no parts inside)
Combine in simple ratios
Same element are identicalhellipcanrsquot change chemically into other element
Can mix chemically but elements are not changed into other atoms
DID EXPERIMENTS TO PROVE HIS THEORIES AS OPPOSED TO PREDICESSORS
bullTHOMSONUsed CRT to discover electrons because it bent
toward a positive plate
Later discovered proton too
Plum pudding model
bullDaltonSolid indivisible (no parts inside)
Combine in simple ratios
Same element are identicalhellipcanrsquot change chemically into other element
Can mix chemically but elements are not changed into other atoms
DID EXPERIMENTS TO PROVE HIS THEORIES AS OPPOSED TO PREDICESSORS
bullTHOMSONUsed CRT to discover electrons because it bent
toward a positive plate
Later discovered proton too
Plum pudding model
bullTHOMSONUsed CRT to discover electrons because it bent
toward a positive plate
Later discovered proton too
Plum pudding model
bullRutherfordGold foil exp Discovered nucleus large positive
mass and that atom was mostly empty space
Rutherfordrsquos model had problems though Could not explain why metals like iron changed colors when they were heated
The Development of Atomic Models
Rutherfordrsquos atomic model could not explain the chemical properties of elements Rutherfordrsquos atomic model could
not explain why objects change color when heated
51
bullBohrPlanetary model with electrons in fixed energy
locations (but as we will soon see his model could only describe some things)
It is like the 2 8 8 that we described earlier this year See video if time
The Bohr ModelEach possible electron orbit in Bohrrsquos model has
a fixed energyThe fixed energies an electron can have are called
energy levelsA quantum of energy is the amount of energy
required to move an electron from one energy level to another energy level
51
The Bohr ModelLike the rungs of the
strange ladder the energy levels in an atom are not equally spaced
The higher the energy level occupied by an electron the less energy it takes to move from that energy level to the next higher energy level
51
Wave LectureThe current model could not describe emission
spectra which were not continuous (like the gas spectrum tubes)pg 364-369
SEE DEMOS of colors from salts spectroscopy video
Is light a Wave or a particle SEE BOOK PG 363Light is like a particle (cathode ray)Light is like a wave too
Plank and Einstein described this
Wave TermsWavelength
Frequency
speed
Spectroscopy demoUse gas tubes amp flames
Mr K will insert a little about the electromagnetic spectrum here
Basically Shorter wavelength = more energy = violet or UV
or gammaLonger wavelength = less energy ndash red IR
microwave radio
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
bullBohrPlanetary model with electrons in fixed energy
locations (but as we will soon see his model could only describe some things)
It is like the 2 8 8 that we described earlier this year See video if time
The Bohr ModelEach possible electron orbit in Bohrrsquos model has
a fixed energyThe fixed energies an electron can have are called
energy levelsA quantum of energy is the amount of energy
required to move an electron from one energy level to another energy level
51
The Bohr ModelLike the rungs of the
strange ladder the energy levels in an atom are not equally spaced
The higher the energy level occupied by an electron the less energy it takes to move from that energy level to the next higher energy level
51
Wave LectureThe current model could not describe emission
spectra which were not continuous (like the gas spectrum tubes)pg 364-369
SEE DEMOS of colors from salts spectroscopy video
Is light a Wave or a particle SEE BOOK PG 363Light is like a particle (cathode ray)Light is like a wave too
Plank and Einstein described this
Wave TermsWavelength
Frequency
speed
Spectroscopy demoUse gas tubes amp flames
Mr K will insert a little about the electromagnetic spectrum here
Basically Shorter wavelength = more energy = violet or UV
or gammaLonger wavelength = less energy ndash red IR
microwave radio
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
The Bohr ModelEach possible electron orbit in Bohrrsquos model has
a fixed energyThe fixed energies an electron can have are called
energy levelsA quantum of energy is the amount of energy
required to move an electron from one energy level to another energy level
51
The Bohr ModelLike the rungs of the
strange ladder the energy levels in an atom are not equally spaced
The higher the energy level occupied by an electron the less energy it takes to move from that energy level to the next higher energy level
51
Wave LectureThe current model could not describe emission
spectra which were not continuous (like the gas spectrum tubes)pg 364-369
SEE DEMOS of colors from salts spectroscopy video
Is light a Wave or a particle SEE BOOK PG 363Light is like a particle (cathode ray)Light is like a wave too
Plank and Einstein described this
Wave TermsWavelength
Frequency
speed
Spectroscopy demoUse gas tubes amp flames
Mr K will insert a little about the electromagnetic spectrum here
Basically Shorter wavelength = more energy = violet or UV
or gammaLonger wavelength = less energy ndash red IR
microwave radio
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
The Bohr ModelLike the rungs of the
strange ladder the energy levels in an atom are not equally spaced
The higher the energy level occupied by an electron the less energy it takes to move from that energy level to the next higher energy level
51
Wave LectureThe current model could not describe emission
spectra which were not continuous (like the gas spectrum tubes)pg 364-369
SEE DEMOS of colors from salts spectroscopy video
Is light a Wave or a particle SEE BOOK PG 363Light is like a particle (cathode ray)Light is like a wave too
Plank and Einstein described this
Wave TermsWavelength
Frequency
speed
Spectroscopy demoUse gas tubes amp flames
Mr K will insert a little about the electromagnetic spectrum here
Basically Shorter wavelength = more energy = violet or UV
or gammaLonger wavelength = less energy ndash red IR
microwave radio
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Wave LectureThe current model could not describe emission
spectra which were not continuous (like the gas spectrum tubes)pg 364-369
SEE DEMOS of colors from salts spectroscopy video
Is light a Wave or a particle SEE BOOK PG 363Light is like a particle (cathode ray)Light is like a wave too
Plank and Einstein described this
Wave TermsWavelength
Frequency
speed
Spectroscopy demoUse gas tubes amp flames
Mr K will insert a little about the electromagnetic spectrum here
Basically Shorter wavelength = more energy = violet or UV
or gammaLonger wavelength = less energy ndash red IR
microwave radio
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Wave TermsWavelength
Frequency
speed
Spectroscopy demoUse gas tubes amp flames
Mr K will insert a little about the electromagnetic spectrum here
Basically Shorter wavelength = more energy = violet or UV
or gammaLonger wavelength = less energy ndash red IR
microwave radio
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Spectroscopy demoUse gas tubes amp flames
Mr K will insert a little about the electromagnetic spectrum here
Basically Shorter wavelength = more energy = violet or UV
or gammaLonger wavelength = less energy ndash red IR
microwave radio
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Electromagnetic spectrum
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Pictures of spectroscopyWhen atoms and molecules are exposed to
light or some form of energy they are said to be excited
They absorb that energy and can produce a unique energy change that can identify that atom or molecule
This study of substances that are exposed to some sort of continuous exciting energy is called spectroscopy
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Na (see pg 374)
Bright line spectra (made from a element (this gives us an atomic emission spectrum)
In lab wersquoll see an image of a flame and determine the wavelength
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Stair step model
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
What happens
in spectroscopy
Longer jumps mean higher energy and shorter wavelengths
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Light amp spectraC= (speed of light = wavelength
frequency)
Red light is longer amp lower freq
Blueviolet light is shorter amp higher freq amp HAS MORE ENERGY
Diff color = diff freq
e-s in atoms are what give off diff colors
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Photo electric effect amp quantum mechanics
Planckrsquos constant discussion Diff colors meant diff e-s jumps in atoms (Fe when heated goes from black to red yellow white blue)
Einstein proved it with photoelectric effect Blue light higher energy
Simulation httpphetcoloradoeduensimulationphotoelectric
DEMO w LED and ldquoglow in the dark materialrdquo
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Again Bohr could explain only the mathematical model for H so the model changed
SEE pg 367
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
See Phethttpphetcoloradoeduensimulationdischarge
-lamps
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
AssignmentBegin vocab and page 3 in packet as well ashellip
IN OUR BOOK
Read pg 360-365 do 1-6
Read pg 366-370 do 1-6(these will be collected at our next class meeting
after a brief discussion)
Nexthellip the quantum model amp e- configuration
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Collect and discuss questions
365 amp 370 1-6 amp 1-6 (collect walk by)
Packet pages 3 discuss
Lecture configuration
Key things thus far NEXT SLIDE
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
KEY IDEASLight observations led to the model change
Rutherford couldnrsquot explain light amp color changes Bohr could only explain hydrogen Pg 367
Bohr used Quantized energy levels 368
colors are determined by wavelength Shorter wavelength has more energy (wavelength and frequency are inverses of each other)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
NOTEWhen more energy is absorbed that means there
are larger quantum leaps and more energy that can be given off
When atoms become ions they must gain energy to lose an electron That is called the ionization energy More on this later
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Move on to the model now
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
The Quantum Mechanical Model
Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
51
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
The Quantum Mechanical Model
Austrian physicist Erwin Schroumldinger (1887ndash1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom
The modern description of the electrons in atoms the quantum mechanical model comes from the mathematical solutions to the Schroumldinger equation
51
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
The Quantum Mechanical ModelThe propeller blade has the same probability of
being anywhere in the blurry region but you cannot tell its location at any instant The electron cloud of an atom can be compared to a spinning airplane propeller
51
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
The Quantum Mechanical ModelItrsquos the probability of finding an
electron within a certain volume of space surrounding the nucleus See pg 370 of our book about the lightning bug
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Atomic OrbitalsAn atomic orbital is often thought of
as a region of space in which there is a high probability of finding an electronEach energy sublevel corresponds to an
orbital of a different shape which describes where the electron is likely to be found
Each energy level we go out away from the nucleus we add an energy level and also add an additional sublevel
51
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Atomic OrbitalsDifferent atomic orbitals are denoted by letters The s
orbitals are spherical and p orbitals are dumbbell-shaped
51
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Where are electrons (a new approach S2012)
Bohr originally thought e-s were in shells
Because of the light experiments (spectroscopy) we actually have sublevels
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
See text pg 371-374Kicker draw the overlapping orbitals here
Student should know these two shapesS shaped like a sphereP like a dumbell
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Each sublevel adds a new orbital shape Each
orbital holds 2 electrons (see book for filling order)
Atomic OrbitalsFour of the five d orbitals have the same shape but
different orientations in space
51
Orbital diagram template
Filling rules
1Fill a sublevel before going to another (except S before D amp F)
2Single up before doubling up
3Opposite spinAufbau amp poly Rules
You try Oxygenorbital diagram then list configuration
Here are the energy levels with the sub levels labeled s p d amp f
BOOK IMAGESee the book for the filling order
PG 382
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Atomic OrbitalsFour of the five d orbitals have the same shape but
different orientations in space
51
Orbital diagram template
Filling rules
1Fill a sublevel before going to another (except S before D amp F)
2Single up before doubling up
3Opposite spinAufbau amp poly Rules
You try Oxygenorbital diagram then list configuration
Here are the energy levels with the sub levels labeled s p d amp f
BOOK IMAGESee the book for the filling order
PG 382
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Orbital diagram template
Filling rules
1Fill a sublevel before going to another (except S before D amp F)
2Single up before doubling up
3Opposite spinAufbau amp poly Rules
You try Oxygenorbital diagram then list configuration
Here are the energy levels with the sub levels labeled s p d amp f
BOOK IMAGESee the book for the filling order
PG 382
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Filling rules
1Fill a sublevel before going to another (except S before D amp F)
2Single up before doubling up
3Opposite spinAufbau amp poly Rules
You try Oxygenorbital diagram then list configuration
Here are the energy levels with the sub levels labeled s p d amp f
BOOK IMAGESee the book for the filling order
PG 382
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
You try Oxygenorbital diagram then list configuration
Here are the energy levels with the sub levels labeled s p d amp f
BOOK IMAGESee the book for the filling order
PG 382
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Here are the energy levels with the sub levels labeled s p d amp f
BOOK IMAGESee the book for the filling order
PG 382
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
BOOK IMAGESee the book for the filling order
PG 382
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
See pg 378 amp look at sample 11-2 page 379
Try a couple
C
N
O
Mg
Ti (4s fills before the 3d)
Hey Kicker there has to be an easier way
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Letrsquos make this easy by using our PT to write configurations
See moodle
Where are e-s located
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
s pd
f
sAreas or Blocks
Shade in these areas or notate them on the PT I will give you
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
s pd
f
sFilling Order
1 2
3 4 5 6 7 8 9 10
11
12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34
35 36
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Another picture
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Keep in mind that this is not as difficult as it may seem
Basically we go in order from left to right across a period
Letrsquos try a couple
N
Si
K
Ti
Cl
The only problem with this method when we get to d filling we subtract one from the energy level at f we subtract 2 Because they are actually further inside S amp P are the valence electrons
Try Ti
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
YOU TRYZn
Fe
Mg
Br
K
Hg
Rb
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Orbital diagramsHow about an orbital diagram for the ones we
just did N Si K Ti Cl
See textbook pg 378
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Valence electrons (see pg 384) are the outer electron shell which we learned
earlier can only hold up to 8 total electrons
Valence is the outer shell ndash only s amp p
How about the valence configuration for these
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Most atomsWant to have a full valence of 8 electrons (called
octet) this would be s2 amp p 6
Metals lose electrons when there is sufficient energy to ldquopull one offrdquo this is called the Ionization energy
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Configuration for ionsWrite these configurations
Ca
Ca +2
F
F-1
O-2
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Spring 2014Discuss notes pg 3-5
Discuss answers pg 6-7 -Try pg 11 (valence pg 384 image is wrong)
Highlight spectroscopy steps
Discuss vocab
Discuss exceptions amp ions (See page 8 for notes and probs)
Assign pg 12-13 amp colored PT areas
IF TIME ndashwavelength lab (pg 9-10) else ndashread and do tomorrow
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Ready for OVERKILL
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
B) Quantum numbers
1 s 2
Energy level Refered to as n
Sublevel (orbital shape)
electrons
Discuss
2p4
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
VOCABULARY NOTES electromagnetic radiation Wavelength
Frequency Photons
Quantized wave mechanical model
Orbital principal energy levels
Sublevels Pauli exclusion principle
electron configuration orbital diagram
valence electrons core (shielding) electrons
Groups representative elements
atomic size ionization energy
Electronegativity stability
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Continuous spectrumWhat is seen when white light
goes through a prism (not discrete lines) ROYGBIV
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Bright line spectra Also called emission spectra
This is the fingerprint of the atom Electrons are excited and jump to a higher energy level when the return to ground state they give off a discrete line of a particular wavelength Each atoms spectrum is different
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
What is the explanation for the discrete lines in atomic emission
spectra
Electrons absorb energy and leap from one orbital in an atom to an orbital of higher energy When these excited electrons fall back down to lower energy levels they emit light The lines result from the fact that the electrons can move only between discrete energy levels they cannot have intermediate energies Electron energies are quantized not continuous (LIKE STAIRSTEPS amp A BALL)
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
The process pg 366-367
1 The atom gets excited
2 an e- jumps to a higher energy level
3 it comes back to its ground state
4 and a photon of light is emitted (maybe in the visible spectrum or not)
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
+
Ground state is where the electron is normally located
1
2
3
Emitted photon
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
WavelengthDistance from crest to crest
INVERSE OF FREQUENCY
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Photondiscrete bundle of
electromagnetic energy
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Photoelectric effectThis is the situation where light hits a
photo cell and creates a direct current (electron flow)
What happens In the photoelectric effect Electrons are ejected by metals when light shines on them The effect is only observed if the frequency of the incident light is above a certain threshold frequency
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Energy levelLocations where electrons can
be Each has a specific orbital
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Quantumenergy needed to move an
electron from one energy level to another
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Quantum mechanical model
It is a model that describes the motions of electrons in atoms as probabilistic motions within a certain region It is depicted as electron clouds the density of which represents the probability of finding the electron in that region The electron cloud of the quantum mechanical model is centered on the atomic orbital as proposed by Bohr but Bohr could not describe the discrete spectral lines on an emission spectrum with his planetary model
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Atomic orbitalsThe shapes of the clouds that electrons tend to
make There are specific shapes and numbers of orbitals for each atom SHAPES An s orbital has the shape of a sphere and is the orbital having the lowest energy A p orbital is dumbbell-shaped and has the next highest energy
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Electron configurationThe filling order of electrons
into the orbitals
Two methods Orbital fillingElectron config (1s2 2s3 sp6hellip
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Ground stateThe lowest energy state of the
atom (The original location of electrons in their orbitals)
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Valence electronsThis is the highest energy
levels S amp P electrons
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Octet ruleAll atoms want a full valence of
electrons This is the highest energy levels S amp P electrons
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Still to discuss this unit
Valence of ions
Exceptions to electron configuration
Do the Na wavelength lab amp practice worksheets
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Packet Pg 8 Stability levels (ordered from most stable to least stable)
1 full octet s2p6
2 full sub level s2 d10 F14
3 frac12 filled sub level d5
Which is more stable
2S2 or 2s1
3s2 3p3 or 3s2 3p4
2s1 2p6 or 2s1 2p2
Fe or Mn Si or P Ca or Sc
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Work thru pg 8Then assign pg 12-13 amp colored packet
Lab tomorrow
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Exception for e- configuration
Some atoms rearrange their electrons from what we would predict the e- configuration to be to become more stableEx Cu
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Stable ions- explain themElements will lose e-s to become more stable It
takes energy to do this though Some elements take on a couple different oxidation numbers because of the options in stability
Be able to predict stable ions OR What are possible oxidation numbers that these atoms can have)
Ca Ti Sc Ta
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
What information does the PT give us
Demo trend of Alkali metals discuss (assign) label a table and periodically yours unit 8 quiz ws
Discuss why they react and why the trend Lecture lots discuss periodic table ws 1 pg 18 packet Ionization energy amp atomic size ws Review using worksheets
Layout various metals Si Non metals Alkali metals Ca Show locations amp variety
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Goals Describe the history of the design of PT
How location of certain groupsregions
Size of atoms (AR) Cations Anions
How do they become ions (cations) IETrend of IE (exceptions)EN
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Periodic table
bullDesigned by Mendeleev and put in increasing atomic mass He put elements that had similar properties in vertical columnsbullLater it was put in order of increasing atomic number (moseley)
bullPacket pg 15 (some notes can be filled in as we go
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Terms amp concepts TO KNOWMendeleev amp his processPeriodGroupPeriodic law Metal nonmetals metalloids and some of their
propertiesAlkali metalsAlkaline earth metalsHalogensNoble gasesTransition metalsInner transition metalsRepresentative elements
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Terms amp concepts TO KNOWMendeleev amp his process ndashmass order periodicityPeriod - rowGroup (family ndash vertical column)Periodic law when elements are arranged in atomic number a
repeating pattern of chemical AND physical properties existMetal nonmetals metalloids and some of their properties
Metals conduct heat amp electricity maleable ductile luster left sideNon-metals donrsquot conduct brittle dull right sideMetalloids (semi-metals) some properties of both
Alkali metals (group 1A)Alkaline earth metals (group II A)Halogens (group VII A)Noble gases (group VIII A)Transition metals (d filling)Inner transition metals (f filling) Representative elements ( s amp p filling)
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
categories
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
See the mini PT pages
Metalloids HalogensAlkali metals Alkaline Earth MetalsTransition Metals Representative elements Inner transition metals noble gases
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
More from LABEL THE TABLEatom size trend
ion size trend
How does the size of a cation compare to itrsquos atom (explain why)
How does the size of a anion compare to itrsquos atom (explain why)
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Reactivity of Alkali Metals
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Alkali metalsSee video
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
KEY IDEA
The periodic table position and the chemical properties of the elements arise from their electron configuration
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Predict PAIR SHARE
What do you think happens to atom size as you
A) go down a family
B) go across a period
WHY
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Atomic Size (AR)General trends
Atoms get larger as you add more energy levels
Atoms tend to get smaller as you go across a period from left to right ( Be able to explain WHY)
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
ATOM Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the electron cloud making the atom smaller
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
So which is largerCa or Mg
F or Br
Si or C
Sr or Ne
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
What about the size of ionsWhen atoms gain or lose electrons the
atom becomes an ion
What would you predict would be true about the size of cations compared to their atom What about the anionsTrend of ions going across Going down
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Ion size from atom size You need to think about if it is a cation or an anion
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Can you explain which is larger of each of these pairs
Li to Li+1
Li+1 to Be +2
F to F-1
O-2 to F-1
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
ION Size Trend RationalAs you go down we add an energy level
As we go across from L to R we add protons which make the nuclear charge stronger and effectively sucking in the atom to make it smaller
The pattern is the same as for atoms however when you get to where atoms become anions there is a big jump in size
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
You predictWhich is larger
Use only your periodic table
Na Na +1
Cl Cl-1
Na+1 Cl-1
H+ H H-1
F -1 Na+1 Ne
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Put these in order from largest to smallest and be able to justify
your answerMg+2 Na+1 Ne F-1 O-2
When an atom or ion has an equal number of electrons or has the same number of electrons when compared to the atoms of another element the two species are called isoelectronic
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Ionization Energy packet pg 23-24 See chapter
IE is the energy required to lose one electron
TWO THINGS EFFECT IESize of atom (shielding) and nuclear charge
More shielding
less shielding
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
So letrsquos think about thisThose valence electrons that
are closer to the nucleus are harder to pull away So an e- from Na is harder to pull away than it is to steal an e- from K Therefore K is more reactive
What would you predict is true as you go across a period Which has lower IE Mg or Na
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
IE
1312 2371
520 900 800 1086 1402 1314 1681 2080
4958 7376 5774 7862 10120 9996 12550 15200
4180 5895
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
We have various IErsquosFirst IE Second IE Third IE as you try to take away a second electron from an atom the IE increases even more
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Generally IE increases as we go across a period from left to right What happened between N amp O Why
Also IE1 and IE 2 what seems to be true Why is there a huge jump from the first to the second IE for lithium
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Are there other areas where the trend (increasing IE to the right) does not fit
Remember the exceptions to configurationOctetFilled sub levelHalf filled sublevel
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Show my Straw Example
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
A closer look at ionizationBoron is further to the
right on the PT but it has a lower IE Why
Because it would rather have a more stable config so it lets the e- go with a little more ease than Be does
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
AlsoLook at the activity
chart (single replacement rxns) on your Periodic table With the exception of Lithium what trend exists for the first 5 or 6 metals
bull Ionization tends to decrease as we go down the periodic table This is because the atoms become so big that the attraction of the outer e- is so small
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Use your PT to predictWhich has the higher IE Ca or Mg
B or N
Why would IE for a nonmetal such as Cl be higher than that of a metal such as K
REMEMBER WHAT IE IS
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
ElectronegativityEN Is the affinity for electrons
What would be characteristics of an element with a high EN
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Metallic TrendsAn element is more metallic if it tend to lose
electrons easier
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Test will have a different PT
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Predict the most reactive
Metal (low IE and lots of shielding)
Non metal (high IE and not much shielding)
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
summary
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Time in class to try Unit 8 WS 1 pg 15 (15 mins)
You will have about 10 minutes or so to work through this page and wersquoll discuss it So get to it Pg 69 amp 386 might help
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Unit 8 WS 1 pg 15 ANSWERS
Who did the pioneer work on the periodic table we used today
DEMETRI MENDELEEV later it was Moseley
In what order are the elements listed in our present periodic table
BY ATOMIC (originally by atomic mass)
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
State the periodic law
When the elements are arrange in order of increasing atomic there is a periodic repetition of their physical and chemical properties
What is the name given to the elements in a vertical column of the periodic table
GROUP (or Family)
What name is given to the elements in a horizontal row on the periodic table
PERIOD
Unit 8 WS 1 pg 15 ANSWERS
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
What part of the periodic table represents the filling of the d sublevel
Transition metals
Which groups by number are the representative elements
A GROUPS
What part of the periodic table represents the filling of the f sublevel
INNER TRANSITION METALS
Unit 8 WS 1 pg 15 ANSWERS
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
What is true of the valence electron configuration of the elements with similar properties
THEY ARE THE SAME
State the octet rule (or when atoms become un-reactive)
ALL ATOMS THAT HAVE A FULL VALENCE (mainly 8 e-)
Unit 8 WS 1 pg 15 ANSWERS
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Atoms of the alkali group have 1 valence electron and tend to LOSE 1 e-s
Alkaline earth metals have 2 valence electrons and tend to LOSE 2 e-s
Halogens have 7 valence electrons and tend to GAIN 1 e-s
Unit 8 WS 1 pg 15 ANSWERS
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Isoelectronic refers to ions that have the same electron configuration of each other (usually that of a noble gas For example Mg+ 2 Na +1 Ne F-1 O-2)
Can you tell me some that are isoelectronic to Kr
Unit 8 WS 1 pg 15 ANSWERS
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Unit 8 WS 1 pg 15 ANSWERSWhat is the basic trend as you go across a period
Increase an electron in the valence and increase nuclear charge The atom size becomes smaller as a result
What can be said about elements that are in the same family or group
They have similar chemical and physical properties
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
LAB (s)Na vapor wavelength (collect data complete
and turn in)
Alkaline Earth LAB
Homework plantet quack pages
Pg 25
Next day in class (26-27 and discussion) begin the next lab
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-
Discussion ProtocolSee the handout
Expectations everyone participates
Each one write some
Groups 1 amp 2 (oral protocol)
Discuss part 11amp2
Discuss part 2
- Letrsquos look at our goal
- Unit 8
- 1 EVOLUTION OF MODEL
- The Development of Atomic Models
- Dalton
- THOMSON
- Rutherford
- The Development of Atomic Models (2)
- Bohr
- The Bohr Model
- The Bohr Model (2)
- Wave Lecture
- Wave Terms
- Slide 15
- Spectroscopy demo
- Electromagnetic spectrum
- Pictures of spectroscopy
- Na (see pg 374)
- The process pg 366-367
- Slide 21
- Stair step model
- Slide 23
- What happens in spectroscopy
- Light amp spectra
- Photo electric effect amp quantum mechanics
- Again Bohr could explain only the mathematical model for H so
- NOTE
- See Phet
- Assignment
- Collect and discuss questions
- KEY IDEAS
- NOTE (2)
- Move on to the model now
- The Quantum Mechanical Model
- The Quantum Mechanical Model (2)
- The Quantum Mechanical Model (3)
- The Quantum Mechanical Model (4)
- Atomic Orbitals
- Atomic Orbitals (2)
- Where are electrons (a new approach S2012)
- See text pg 371-374
- Each sublevel adds a new orbital shape Each orbital holds 2 e
- Slide 44
- Atomic Orbitals (3)
- Orbital diagram template
- Filling rules
- You try Oxygen orbital diagram then list configuration
- Slide 49
- BOOK IMAGE
- See pg 378 amp look at sample 11-2 page 379
- Letrsquos make this easy by using our PT to write configurations
- Areas or Blocks
- Filling Order
- Another picture
- Keep in mind that this is not as difficult as it may seem
- YOU TRY
- Orbital diagrams
- Valence electrons (see pg 384)
- Most atoms
- Configuration for ions
- Spring 2014
- Slide 63
- Slide 64
- Ready for OVERKILL
- B) Quantum numbers
- Slide 67
- Slide 68
- Slide 69
- VOCABULARY NOTES
- Continuous spectrum
- Bright line spectra
- What is the explanation for the discrete lines in atomic emissi
- The process pg 366-367 (2)
- Slide 75
- Wavelength
- Photon
- Photoelectric effect
- Energy level
- Quantum
- Quantum mechanical model
- Atomic orbitals
- Electron configuration
- Ground state
- Valence electrons
- Octet rule
- Still to discuss this unit
- Packet Pg 8 Stability levels (ordered from most stable to le
- Work thru pg 8
- Exception for e- configuration
- Stable ions- explain them
- Slide 92
- What information does the PT give us
- Goals
- Periodic table
- Terms amp concepts TO KNOW
- Terms amp concepts TO KNOW (2)
- categories
- See the mini PT pages
- More from LABEL THE TABLE
- Reactivity of Alkali Metals
- Alkali metals
- KEY IDEA
- Predict PAIR SHARE
- Atomic Size (AR)
- ATOM Size Trend Rational
- So which is larger
- Slide 108
- What about the size of ions
- Slide 110
- Slide 111
- Slide 112
- Can you explain which is larger of each of these pairs
- ION Size Trend Rational
- You predict
- Put these in order from largest to smallest and be able to just
- Ionization Energy packet pg 23-24 See chapter
- So letrsquos think about this
- IE
- Slide 120
- Slide 121
- Slide 122
- Are there other areas where the trend (increasing IE to the rig
- Show my Straw Example
- A closer look at ionization
- Also
- Use your PT to predict
- Electronegativity
- Metallic Trends
- Test will have a different PT
- Predict the most reactive
- summary
- Time in class to try Unit 8 WS 1 pg 15 (15 mins)
- Unit 8 WS 1 pg 15 ANSWERS
- Slide 135
- Slide 136
- Slide 137
- Slide 138
- Slide 139
- Unit 8 WS 1 pg 15 ANSWERS (2)
- LAB (s)
- Discussion Protocol
-