TN Ch 9.1 Date
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EQ:
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it (Highlight answer) based on from what you read.
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TN Ch 9.1
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DRAW ANY PICTURES, FIGURES,
AND WRITE OUT ANY PRACTICE
PROBLEMS/QUESTIONS.
WE WILL ANSWER THEM TOGETHER.
LEAVE SPACES SO WE CAN ANSWER
QUES.
LEFT Side – PICTURES, PRACTICE PROBLEMS, ETC
Ch 9.1-9.2 Notes
Topic: Light & Electromagnetic
Radiation
EQ: How does light interact with
atoms?
READ Ch 9.1 – 9.2 (pg. 285-288)
Write Questions & Answer Questions #1-5
(notes side) Highlight answer
Electrons in Atoms and the Periodic Table
• We examine two important models—the Bohr
model and the quantum-mechanical
model—that propose explanations for the
inertness of helium, the reactivity of hydrogen,
and the periodic law.
• These models explain how electrons exist in
atoms and how those electrons affect the
chemical and physical properties of elements.
• (Remember – elements in same group have
similar phy/chem prop’s) - Learned this in
Ch 4!!
Electromagnetic Radiation
• The interaction of light with atoms helped to
shape scientists’ models of the atom.
• Light is a form of electromagnetic radiation.
• Light has properties of both waves and
particles.
Light: Electromagnetic Radiation
When a water surface is disturbed, waves are created that
radiate outward from the site. The wave carries energy as
it moves through the water.
• Wavelength: The wavelength of light, λ (lambda), is defined as the distance between adjacent wave crests.
Draw with notes
Light: Color of Light • White light, as produced by the sun or by a lightbulb,
contains a spectrum of wavelengths and therefore a
spectrum of color.
• We see these colors—red, orange, yellow, green,
blue, indigo, and violet—in a rainbow or when white
light is passed through a prism.
• Red light, with a wavelength of 750 nm (nanometers),
has the longest wavelength of visible light.
• Violet light, with a wavelength of 400 nm, has the
shortest wavelength of visible light
(1 nm = 1 × 10–9 m).
• The presence of color in white light is responsible for
the colors we see in our everyday vision.
Components of white light
R O Y G B I V
• Light is separated into its constituent colors—red, orange, yellow, green, blue, indigo, and violet—when it is passed through a prism.
Draw with notes
• A red shirt appears red because it reflects red
light; the shirt absorbs all of the other colors of
light except the red light. Our eyes see only the
reflected light, making the shirt appear red.
• Frequency: The frequency of light, ν (nu),
is defined as the number of cycles or
crests that pass through a stationary point
in one second.
• Wavelength and frequency are inversely
related—the shorter the wavelength, the
higher the frequency.
Electromagnetic Radiation
(Photons—Particles of Light)
• Light can be viewed as a stream of particles.
• A particle of light is called a photon.
– Photon = packet (bundle) of light energy.
• The amount of energy carried in the packet depends
on the wavelength of the light—the shorter the
wavelength, higher frequency, the greater the
energy.
• Violet light (shorter wavelength) carries more energy
per photon than red light (longer wavelength).
Ch 9.3 Notes
Topic: Electromagnetic Spectrum
EQ: What are the 7 types of radiation?
READ Ch 9.3 (pg. 288-291)
Write Questions & Answer Questions #6-12
(notes side) Highlight answer
• The entire electromagnetic spectrum, with short-
wavelength, high-frequency radiation on the right and
long-wavelength, low-frequency radiation on the left, is
shown below. Visible light is the small sliver in the middle.
Ch 9.3: The Electromagnetic Spectrum
Draw LEFT side (color)
• The shortest wavelength(λ) and most energetic photons are those of gamma rays.
– produced by the sun, by stars, and by certain unstable atoms on Earth.
– Excessive exposure is dangerous: high energy photons can damage biological molecules.
• X-rays, familiar to us from their medical
and dental uses.
– used to image internal bones and
organs.
– Can damage biological molecules.
– While yearly exposures to X-rays are
relatively harmless, excessive exposure
to X-rays increases cancer risk.
• Ultraviolet or UV light - sunlight that
produces a sunburn or suntan.
• Not as energetic as gamma-ray or X-ray
photons,
• Still can damage biological molecules.
• Excessive exposure to UV increases the
risk of skin cancer, cataracts and causes
premature wrinkling of the skin.
• Visible light, only radiation we can see with eyes.
• ranging from violet (shorter λ, higher E) to red (longer λ, lower E).
• Do not damage biological molecules.
• Do cause molecules in our eyes to rearrange, which sends a signal to our brains that results in vision.
• R O Y G B I V
• Infrared (IR) light - The heat you feel when you place your hand near a hot object is infrared light.
• All warm objects, including human bodies, emit infrared light.
• Can’t see with our eyes, infrared sensors can detect it and are often used in night-vision technology to “see” in the dark.
– warm objects—such as human bodies—glow light a lightbulb glows in the visible region of the spectrum.
In the infrared photograph, the warmest areas
appear as red and the coolest as dark blue.
(Note the cold noses.)
• Microwaves, used for radar and in
microwave ovens.
– Substances that contain water, such as
food, are warmed by the radiation of a
microwave oven, but substances that do
not contain water, such as a plate, are
not.
• The longest wavelengths of light are radio
waves, which are used to transmit the
signals used by AM and FM radio, cellular
telephones, television, and other forms of
communication.
Practice #1
• Arrange the three types of electromagnetic
radiation—visible light, X-rays, and
microwaves—in order of increasing:
(a) Wavelength
(b) Frequency
(c) Energy per photon
Write LEFT side
Chemistry and
Health Radiation
Treatment for
Cancer
• In radiation therapy, doctors aim
X-ray or gamma-ray beams at
cancerous tumors.
• The ionizing radiation damages
the molecules within the tumor’s
cells that carry genetic information,
and the cell dies or stops dividing.
• Healthy cells often sustain damage
during treatments, resulting in side
effects such as fatigue, skin
lesions, and hair loss.
• Doctors try to minimize the
exposure of healthy cells by
appropriate shielding and by
targeting the tumor from multiple
directions, minimizing the
exposure of healthy cells.
Ch 9.4-9.5 Notes
Topic: Atoms with Orbitals
EQ: How do electrons orbit around
the nucleus?
READ Ch 9.4-9.5 (pg. 291-295)
Write Questions & Answer Questions #13-16
(notes side) Highlight answer
• Ne atoms inside a
glass tube absorb
electrical energy
and then reemit
the energy as red
light.
• Light emitted from
a Hg lamp (left) and
light emitted from a
H lamp (right).
Emission Spectra of the Elements Are Not Continuous
A white-light spectrum is continuous, with some
radiation emitted at every wavelength.
The emission spectrum of an individual element
includes only certain specific wavelengths.
Niels Bohr Developed a Simple Model to Explain
These Results
Draw with notes
The energy of each Bohr
orbit, specified by a
quantum number n = 1, 2, 3
is fixed, or quantized.
Bohr orbits are like steps of
a ladder, each at a specific
distance from the nucleus
and each at a specific
energy.
The Energy Is Quantized Draw with notes
Excitation and Emission
(Lab next week)
• When a hydrogen
atom absorbs
energy, an electron
is excited to a
higher-energy
orbit. The electron
then relaxes back
to a lower-energy
orbit, emitting a
photon of light.
Draw with notes
Hydrogen Emission Lines
The Bohr Model: Atoms with Orbits
• Bohr model - predicted the lines of the
hydrogen emission spectrum.
• However, it failed to predict the emission
spectra of other elements that contained
more than one electron.
• Bohr model was replaced with the
quantum-mechanical or wave-mechanical
model.
• In the quantum-mechanical model,
Bohr orbits are replaced with quantum-
mechanical orbitals.
• Orbitals are different from orbits - they
represent probability maps that show a
where the electron is likely to be found.
Baseball Paths and Electron Probability Maps
(Read only)
• Baseball vs an
electron.
• Imagine a baseball
thrown from the
pitcher’s mound to a
catcher at home plate.
• The baseball’s path
can easily be traced as
it travels from the
pitcher to the catcher.
Baseball Paths and Electron Probability
Maps (Read only)
• To describe the
behavior of a
“pitched” electron,
you would have to
construct a
probability map of
where it would
cross home plate.
• We cannot describe their exact paths.
– Best probability of where the electron is
likely to be found (90% of the time)
The Quantum-Mechanical Model: Atoms with
Orbitals
Ch 9.5 Quantum Mechanics • Electrons do not behave like particles
flying through space.
• Orbital (“electron cloud”)
– Region in space where there is 90%
probability of finding an electron
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Orbital
90% probability of
finding the electron The greater dot density near
the middle represents a
higher probability of finding
the electron near the
nucleus. Draw with notes
Electron capacities
Copyright © 2006 Pearson Benjamin Cummings. All rights reserved.
Electron capacities
Principal Quantum Numbers for Orbitals
• The lowest-energy orbital 1s orbital.
• Number = 1 and the letter = s (shape of
orbital).
• The number is called the principal
quantum number (n) and specifies the
principal shell of the orbital.
• n can range from n=1….7 (why? Because
there are 7 periods)
Ground States and Excited States
• ground state - lowest energy state
• When the e- is in a higher-energy orbital,
the hydrogen atom is said to be in an
excited state.
Energy Increases with Principal
Quantum Number • The higher the principal
quantum number (n), the
higher the energy (E) of the
orbital. (direct relationship)
• The possible principal
quantum numbers are
n = 1, 2, 3, etc… to 7
• Since the 1s orbital has the
lowest possible n , it is in
the lowest-energy shell and
has the lowest possible E.
Draw with notes
Ch 9.6 Notes (Part 1)
Topic: Atoms with Orbitals
EQ: How do electrons orbit around
the nucleus?
1s22s22p63s23p64s23d104p65s24d104p65s24d105p66s24f145d106p6…
READ Ch 9.6 (pg. 295-301)
Write Questions & Answer Questions #19-22
(notes side) Highlight answer
Shapes of Orbitals
• The letter indicates the subshell of the
orbital and specifies its shape.
• The possible letters are s, p, d, and f, each
with a different shape.
• Orbitals can be drawn as geometric
shapes
The 2s Orbital Is Similar to the 1s Orbital, but
Larger in Size
The s Orbitals: called spheres
There are one s orbitals Draw with notes
The p Orbitals: called dumbbells
There are three p orbitals
Draw with notes
The d Orbitals: called clovers
There are five d orbitals Draw with notes
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Copyright © 2006 Pearson Benjamin Cummings. All rights reserved.
The Number of Subshells in a Given
Principal Shell = Equal to the n
Draw LEFT side
General Rules
• Pauli Exclusion Principle
– Each orbital can hold TWO electrons with
opposite spins.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Wolfgang Pauli
Orbital diagram (box)
Electron spins =
arrows in
opposite
direction
Draw with notes
General Rules
Aufbau Principle
– Electrons fill the
lowest energy
orbitals first.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
2s
3s
4s
5s
6s
7s
1s
2p
3p
4p
5p
6p
3d
4d
5d
6d
4f
5f
1s
2s
2p
3s
3p
4s
4p
3d
4d 5s
5p
6s
7s
6p
6d
4f
5f
5d
En
erg
y
Don’t Draw
RIGHT WRONG
General Rules
• Hund’s Rule
– Within a sublevel, place one electron
per orbital before pairing them.
– “Empty Bus Seat Rule”
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Draw with notes
Electron Filling in Periodic Table
1
2
3
4
5
6
7
s
d
p
s
f
1
2
3
4
5
6
7
s
d
p
s
f
*
W
W
*
Electron Filling in Periodic Table
Li
2s1
H
1s1
He
1s2
C
2p2
N
2p3
O
2p4
F
2p5
Ne
2p6
Na
3s1
B
2p1
Be
2s2
H
1s1
Al
3p1
Si
3p2
P
3p3
S
3p4
Cl
3p5
Ar
3p6
K
4s1
Ca
4s2
Sc
3d1
Ti
3d2
V
3d3
Cr
3d5
Mn
3d5
Fe
3d6
Co
3d7
Ni
3d8
Cu
3d10
Zn
3d10
Ga
4p1
Ge
4p2
As
4p3
Se
4p4
Br
4p5
Kr
4p6
Rb
5s1
Sr
5s2
Y
4d1
Zr
4d2
Nb
4d4
Mo
4d5
Tc
4d6
Ru
4d7
Rh
4d8
Pd
4d10
Ag
4d10
Cd
4p1
In
5p1
Sn
5p2
Sb
5p3
Te
5p4
I
5p5
Xe
5p6
Cs
6s1
Ba
6s2
Hf
5d2
Ta
5d3
W
5d4
Re
5d5
Os
5d6
Ir
5d7
Pt
5d9
Au
5d10
Hg
5d10
Tl
6p1
Pb
6p2
Bi
6p3
Po
6p4
At
6p5
Rn
6p6
Fr
7s1
Ra
7s2
Rf
6d2
Db
6d3
Sg
6d4
Bh
6d5
Hs
6d6
Mt
6d7
Mg
3s2
Ce
4f2
Pr
4f3
Nd
4f4
Pm
4f5
Sm
4f6
Eu
4f7
Gd
4f7
Tb
4f9
Dy
4f10
Ho
4f11
Er
4f12
Tm
4f13
Yb
4f14
Lu
4f114
Th
6d2
Pa
5f2
U
5f3
Np
5f4
Pu
5f6
Am
5f7
Cm
5f7
Bk
5f8
Cf
5f10
Es
5f11
Fm
5f14
Md
5f13
No
5f14
Lr
5f14
La
5d1
Ac
6d1
1
2
3
4
5
6
7
s
d
p
s
f
*
W
W
*
s2 s1 Elements in the s - blocks
He
s2
Label the top of the groups on your PT
1s1
1s22s1
1s22s22p63s1
1s22s22p63s23p64s1
1s22s22p63s23p64s23d104p65s1
1s22s22p63s23p64s23d104p65s24d10
5p66s1
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1
H 1
Li 3
Na
11
K
19
Rb
37
Cs
55
Fr
87
Do you notice any similarity in these
configurations of the alkali metals?
The P-block p1 p2 p3 p4 p5 p6
Label the top of the groups on your PT
He
2
Ne
10
Ar
18
Kr
36
Xe
54
Rn
86
1s2
1s22s22p6
1s22s22p63s23p6
1s22s22p63s23p64s23d104p6
1s22s22p63s23p64s23d104p65s24d105p6
1s22s22p63s23p64s23d104p65s24d10
5p66s24f145d106p6
Do you notice any similarity in the
configurations of the noble gases?
Transition Metals - d block
d1 d2 d3 s1
d5 d5 d6 d7 d8 s1
d10 d10
Note the change in configuration.
Label the top of the groups on your PT
F - block
• Called the “inner transition elements”
f1 f5 f2 f3 f4
f6 f7 f8 f9 f10 f11 f12 f14
f13
Label the top of the groups on your PT
Maximum Number of Electrons In Each Sublevel Maximum Number of Electrons
In Each Sublevel
Maximum Number
Sublevel Number of Orbitals of Electrons
s 1 2
p 3 6
d 5 10
f 7 14
LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 146
Draw LEFT side
Principal Quantum Number ( n )
– Energy level
– Size of the orbital
– PERIOD # (except
Transition/Inner Tran’s
Metals)
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
1s
2s
3s
Draw with notes
Electron Configurations:
How Electrons Occupy Orbitals
• An electron configuration (e.c.) shows the
location of every orbital, # of e- in each orbital for
a particular atom.
• The e.c. formula is the following:
nL#
PQ# = period # Orbital
shape =
s, p, d, f
Valence e- =
outer most
electrons
s-block 1st Period
1s1 # of valence
electrons
1
2
3
4
5
6
7
Periodic Patterns
• Example - Hydrogen
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Electron Configurations: Orbital Diagrams
• The orbital diagram for a ground-state hydrogen
atom is as follows:
• The box represents the 1s orbital, and the arrow
within the box represents the electron in the 1s
orbital.
Let’s Practice
• The following slides we will do in
class!!
• Don’t write them in notes yet
• Get out PT
• List the first 20 elements (symbols)
• Leave space between each element.
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1
2
3
4
5
6
7
OK, so we’re going to use arrows pointing up or down to
represent the electrons. Can you guess into which box the first
electron would go given that it is attracted to the nucleus?
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s1
1
2
3
4
5
6
7
That’s right: it goes in the 1s sublevel. And its el. config is 1s2.
Notice in the table above where H is – in the area designated
as 1s. So where does the next electron go?
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
If you were thinking it went in the 2s, then you forgot that each
orbital can hold up to two electrons. Note how He is right here
in the area designated as 1s2 and so its el. config. is 1s2. +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Now that the 1s is filled, the next electron goes in the
next sublevel – the 2s. Again note how Li is in 2s1.
Its full el. conf. is 1s2 2s1. What is Be’s el. conf? +
Energy Level Diagram A
rbitra
ry E
nerg
y S
cale
1s
2s 2p
3s 3p
4s 4p 3d
5s 5p 4d
6s 6p 5d 4f
NUCLEUS
Bohr Model
Electron Configuration
CLICK ON ELEMENT TO FILL IN CHARTS
N
Li = 1s22s1
Lithium
H He Li C N Al Ar F Fe La
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Is this what you were thinking? Good. Now look at the
periodic table above, what comes after the 2s sublevel?
The 2p sublevel. So what will the next el. conf. be? +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Is this what you were thinking? Notice how B is
in the 2p1 spot.
So its full el. conf. is 1s2 2s2 2p1. What’s next? +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Is this what you were thinking? Notice how C is
in the 2p2 spot. So its el. conf. is 1s2 2s2 2p2
Notice also how when we fill a sublevel… +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p3
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
…we put one electron in each orbital until the
sublevel is half filled…
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p4
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
… and then we go back and start pairing off
This is called “Hund’s Rule, but it also referred to
as the bus seat rule. Can you figure out why? +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p5
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Look at F. It’s just one electron away from having
filled 2p sublevel…
And it’s just one square away from the end of the 2p block. +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
And then Ne has a completely filled outer level.
Na is next. Can you guess where the next
electron is going to go? +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
That’s right: in the 3s sublevel. Right now,
write down in your notebook what you
think the next three el configs will be. +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Did you get this one right?
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
How about Al’s? See how Al is
in the 3p1 spot on the per table
and its el config ends with 3p1 +
Energy Level Diagram A
rbitra
ry E
nerg
y S
cale
1s
2s 2p
3s 3p
4s 4p 3d
5s 5p 4d
6s 6p 5d 4f
NUCLEUS
Bohr Model
Electron Configuration
CLICK ON ELEMENT TO FILL IN CHARTS
N
Al = 1s22s22p63s23p1
Aluminum
H He Li C N Al Ar F Fe La
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Now just advance through the
next 23 slides, but as you do,
make sure you are understanding +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p3
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Exactly what is going on… how
the el configs simply follow the
sequence of the periodic table. +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p4
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
Your goal by the end of this slide
show is to be able to write el
configs for any element using just
the periodic table – and your brain! +
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p5
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d3
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s1 3d5
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d5
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d6
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d7
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d8
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s1 3d10
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
5s
+
1s
2s
3s
4s
2p
3p
4p
3d
4d 5s
s
p
d
f
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
1
2
3
4
5
6
7
1 2
1 2 3 4 5 6 7 8 9 10
1 2 3 4 5 6 7 8 9 10 11 12 13 14
1 2 3 4 5 6
+
Ch 9.6 Notes (Part 2)
Topic: Atoms with Orbitals
EQ: How do electrons orbit around
the nucleus?
1s22s22p63s23p64s23d104p65s24d104p65s24d105p66s24f145d106p6…
READ Ch 9.6 (pg. 295-301)
NO BQ’s
1
2
3
4
5
6
7
Periodic Patterns
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Draw LEFT side
Order in which subshells are filled
with electrons
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
3d
4d
5d
6d
4f
5f
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d … 2 2 6 2 6 2 10 6 2 10
Draw LEFT side
Electron Filling in Periodic Table
K
4s1
Ca
4s2
Sc
3d1
Ti
3d2
V
3d3
Mn
3d5
Fe
3d6
Co
3d7
Ni
3d8
Cr
3d4
Cu
3d9
Zn
3d10
Ga
4p1
Ge
4p2
As
4p3
Se
4p4
Br
4p5
Kr
4p6
1
2
3
4
s
d
p
s
Cr 4s13d5
Cu 4s13d10
4f
4d
4p
4s
n = 4
3d
3p
3s
n = 3
2p
2s n = 2
1s n = 1
Energ
y
4s 3d
Cr 4s13d5
4s 3d
Cu 4s13d10
Cr
3d5
Cu
3d10
Transition Metals - d block
d1 d2 d3 s1
d5 d5 d6 d7 d8 s1
d10 d10
Note the change in configuration.
Label the top of the groups on your PT
Draw LEFT side
A Pattern Exists for the Entire Periodic Table
Ch 9.7 Notes
Topic: Valence Electrons &
Noble Gas e.c.
EQ: What are Val. E- & how do you
write noble gas e.c.?
1s22s22p63s23p64s23d104p65s24d104p65s24d105p66s24f145d106p6…
READ Ch 9.7 (pg. 302-305)
Write Questions & Answer Questions #23-25
(notes side) Highlight answer
1
2
3
4
5
6
7
Periodic Patterns
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Review
Energy Ordering of Orbitals for Multi-
Electron Atoms
• The subshells (s,p,d,f) within a principal
shell (n) do not have the same energy
because of e - interactions.
• Different subshells within the same
principal shell have different energies.
– Increasing Energy:
3s < 3p <3d (more e-)
Core electrons: Inside Electrons closet to nucleus
Valence Electrons: electrons in the _________-_______ energy
level (or shell). (MOST IMPORTANT FOR BONDING!!)
• V.E. = “___” electrons and “___” electrons only.
(V.E. = A Groups only on PT )
Counting Valence Electrons
• MAXIMUM NUMBER OF VALENCE ELECTRONS = 8 e-
(only exception Helium = __ e-’s)
Examples: Ca = __ e-’s Nitrogen = __ e-’s Argon = __ e-’s
• d-block and f-block = _________ valence e-’s
Ch 9.7: Core and Valence Electrons
outer most
s p
2 5 8
2 or 1
2
Electron Configurations and the Periodic Table
The elements within “A” groups (not “B”
groups) of the P.T. all have the same
number of v.e. and similar outer e.c.
With notes - Make a “sketch” with boxes. Label symbols and label “A”
groups
Valence Electrons and Core Electrons
What is e.c. for Si?
Silicon has 4 v.e. (those in the n = 3 principal
shell) and 10 core electrons.
Draw with notes
Valence Electrons and Core Electrons
What is e.c. for Se?
Selenium has 6 v.e. (those in the n = 4 principal shell).
All other electrons, including those in the 3d orbitals, are
core electrons.
Draw with notes
Periodic Trends in Electron Configurations of the
Transition Series Elements
• The transition metals (“B” groups) have
e.c. differ from “A” group elements.
– For the 1st row of trans. metals (in period 4),
they all have the outer configuration of 4s23dx
(x = number of d electrons).
• So, valence e- are always 2 (or
sometimes 1 for two special groups in
the d-block…hint, hint)!!
• Two exceptions groups: Cr is 4s13d5 and
Cu is 4s13d10.
• So, valence e- will be 1!! (only for those
2 groups in d-block)
(2e–) for 4s23dx
(1e–) for 4s13d5 or 4s13d10
Periodic Trends in Electron Configurations of the
Transition Series Elements
neon's e.c. (1s22s22p6)
Noble Gas Configuration
[Ne] 3s1 third energy level
one electron in the s orbital
orbital shape
Na = [1s22s22p6] 3s1 electron configuration
A
B
C
D
Draw with notes
[Ar]
1
2
3
4
5
6
7
4s2 3d10 4p2
Noble Gas Electron Configuration
• Example - Germanium
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Ge 72.61
32
• Noble Gas (Shorthand) Configuration
S 16e-
Valence Electrons Core Electrons
S 16e- [Ne] 3s2 3p4
1s2 2s2 2p6 3s2 3p4
Notation
• Longhand Configuration
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
S 32.066
16
Practice
[Ar] 4s2
Electron configuration Element symbol
[He] 2s2 2p5
[Kr] 5s2 4d10 5p6
V
Sg
Ag
I
[Ar] 4s23d6
Valence e-
LEFT side
Ch 9.8 Notes
Topic: Ions and E.C.
EQ: How does the e.c. change if the
atom loses/gains v.e.?
1s22s22p63s23p64s23d104p65s24d104p65s24d105p66s24f145d106p6…
READ Ch 9.8 (pg. 305-307)
Write Questions & Answer Questions #27
(notes side) Highlight answer
• The chemical properties of elements
are largely determined by the number
of valence electrons they contain.
Ch 9.8 Electron Configuration and Ions
• Alkali metals (Group 1) are
among the most reactive
metals since their outer e.c.
(ns1)
• If they lose the 1 valence e-,
they attain a Noble Gas e.c.
• This is why whole group has
a 1+ charge.
The Alkali Metals Draw with notes
• The alkaline earth
metals (Group 2) all
have e.c. ns2 and have
2 v. e.
• In their reactions, they
tend to lose 2 e -,
forming 2+ ions and
attaining a NG
configuration.
The Alkaline Earth Metals Draw with notes
• The halogens (Group 7) all
have ns2np5 e. c. (short 1
valence e- to noble gas
config)
• Halogens tend to gain 1 e-,
forming 1− ions and
attaining a NG configuration.
The Halogens Draw with notes
• All have 8 v. e. (or 2 for
helium).
• The noble gases are
chemically stable, and are
nonreactive.
The Noble Gases Draw with notes
Elements That Form
Predictable Ions
Ch 9.8 - ELECTRONIC CONFIGURATION OF IONS
• Positive ions (cations) are formed by losing e-.
• Negative ions (anions) are formed by gaining e-.
• Electrons are removed first from the HIGHest occupied orbitals
Practice: (leave 4 lines of space for each)
1. SODIUM
2. CHLORINE
With notes
ELECTRONIC CONFIGURATION OF IONS
Electrons are removed first from the
HIGHest occupied orbitals (be careful
transition metals!!)
Practice: (leave 4 lines of space for each)
1. TITANIUM
2. Germanium
With notes
Ch 9.9 Notes
Topic: Periodic Trends
EQ: What are the 3 trends on the PT?
READ Ch 9.9 (pg. 307-312)
Write Questions & Answer Questions #28
(notes side) Highlight answer
Periodic Trends #1: Atomic Size
• #1: As you move to the right across a period in
the PT, atomic size decreases.
– atomic size determined by the distance
between the outermost electrons and the
nucleus.
– # of protons in the nucleus is increasing,
which results in a greater pull on the e- from
the nucleus, causing atomic size to decrease.
• #2: As you move down a column in the periodic
table, atomic size increases.
– highest principal quantum number, n,
increases.
– orbital increases with increasing PQ#, the e-
that occupy the outermost orbitals are farther
from the nucleus as you move down a
column.
Periodic Trends #1: Atomic Size
Periodic Properties: Atomic Size
With notes - Make a “sketch” with boxes. Draw Arrows
Periodic Trends #2: Ionization Energy
• Ionization Energy – ability to lose electrons
• Ionization energy increases as you move
to the right across a period and decreases
as you move down a column in the
periodic table.
Periodic Trends #2: Ionization Energy
With notes - Make a “sketch” with boxes. Draw Arrows
Periodic Properties #3: Metallic Character
• Metals tend to lose electrons in their chemical
reactions, while nonmetals tend to gain
electrons.
• Metallic character decreases as you move to
the right across a period and increases as you
move down a column in the periodic table.
Periodic Properties: Metallic Character
With notes - Make a “sketch” with boxes. Draw Arrows