outline of topics 1. a light wave – what is light? 2. history of the periodic table 3. electron...

OUTLINE OF TOPICS

1.A Light Wave – What is light?2.History of the Periodic Table3.Electron Configuration4.Quantum Number – Atom’s

Address5.Quantum Power – What is energy?6.Atom is Bohr-ed – The story of

Atom Part II

1. A Light Wave

What is light?

What is color?

What does the word “frequency” mean?

1. A Light Wave

OBJECTIVE: To understand what light and colors are

1. A Light Wave

Light is a WAVE

This wave has electrical properties

AND

This wave has magnetic properties

So we call light an electro-magnetic wave

1. A Light Wave

Spectrum = a range

This picture is a range of waves from long to short

1. A Light Wave

1. A light wave

Wavelength Frequency

What is it

Symbol:

Unit:

2 quantitative properties of a wave

1. A Light Wave

Wavelength: distance between two waves

“crest to crest” or “trough to trough”

1. A Light Wave

What does it mean to do something frequently?

1. Quantum Model

Frequency: how many waves in 1 second

1. Quantum Model

2 properties of waves

Wavelength: distance between two waves

either crests or troughs

Symbol: lUnits = meters, m

1. Quantum Model


Frequency: How many waves in 1 second

Symbol: vUnits = Hz, or sec-1

1. Quantum Model

1. Quantum Model

Which has a longer wavelength: radio or ultraviolet?

1. Quantum Model

Which has a higher frequency: radio or ultraviolet?

1. A Light Wave

Heat energy in the form

ofInfrared waves

1. A Light Wave

X-Ray Sunburn from UV rays

1. Quantum Model


Wavelength: is…

Symbol: ?Units = ?

Frequency: is…

Symbol: ?Units = ?

What does it mean for wavelength and frequency to have an inverse relationship?

1. Quantum Model

2 properties of wavesl= Wavelengthv = Frequency

C = Speed of light = 3.0 x 108 meters/seconds <- this

number never changes

lv = cl

1. Quantum Model

Calculations using lv = c

Your favorite radio station broadcasts the signal at 99.5 MHz. This is equal to 9.96 x 107 Hz. Calculate the wavelength in meters.

1. Write the equation: lv = c2. Plug in values. C = 3.0 x 108 m/s ALWAYS3. Rearrange equation to solve for unknown. 4. Solve

Answer = 3.01 meters

1. Quantum Model

Calculations using lv = c

Photosynthesis uses light waves with a wavelength of 660 nm to convert CO2 and H2O into glucose and O2. 660 nm = 6.6 x 10-7m. Calculate the frequency.

1. Write the equation: lv = c2. Plug in values. C = 3.0 x 108 m/s ALWAYS3. Rearrange equation to solve for unknown. 4. Solve

Answer = 4.5 x 1014 Hz or 4.5 x 1014 sec-1

1. A Light Wave

Answer on Warmup Paper. Label it as “WAVES”

Your favorite FM radio station broadcasts at a frequency of 101.1 MHz. This is equal to 1.011 x 108 Hz. What is the wavelength of this station in meters?

A police officer is using a radar gun for speeding citations. The gun uses waves with a wavelength of 8.45 nanometers. This is equal to 8.45 x 10-9 meters. What is the frequency in Hz?

1.Make sure that l is in METERS, or that v is in Hz2. If not, then convert to METERS or Hz using the

conversion factors given to you.3.Solve: Step-by-step instructions on how to solve

should be in your notes4.Does your final answer have the units that is

asked for in the problem?

1. A Light Wave

1. What is light?

2. What are the symbols and units for the two quantitative properties of a wave?

3. What is the relationship between the two quantitative properties?

4. Explain why we have different colors using the two quantitative properties

5. What does a high frequency mean in terms of energy?

Summary & Review

2. Quantum Power

What is energy? What are some examples of energy?

What is energy made out of?

What do you think the word “quantum” means?

How is walking up stairs different from walking up a hill?

2. Quantum Power

OBJECTIVE: To understand what energy is

2. Quantum Power

Energy as massless waves

2. Quantum Power

Relationship between

ENERGY and WAVELENGTH

1. Quantum Model

2. Quantum PowerWhat does it mean for

energy to be quantized?What does it mean for light to be quantized?

What is a quantum? What is a photon?

2. Quantum Power

Max Plank

Discovered that

Energy is QUANTIZED

Quantized?

Means WHOLE NUMBERS

Energy is quantized = energy is gained or lost in WHOLE NUMBERS

2. Quantum PowerMax Plank

Energy is quantized = energy is gained or lost in WHOLE NUMBERS

Similar Examples:

1. Musical instruments are “quantized” in that they can only produce certain notes, like C or F#.

2. US Dollars is “quantized” in whole number of pennies.

2. Quantum Power

http://www.google.com/url?sa=i&rct=j&q=&esrc=s&frm=1&source=images&cd=&cad=rja&docid=ii225UFuOIFEJM&tbnid=gw6YwJ9JqkovzM:&ved=0CAUQjRw&url=http://www.elephantjournal.com/2012/12/my-solsbury-hill-revelation-maureen-andrade/&ei=1_VvUu37BYHeiALesYCQDQ&bvm=bv.55123115,d.cGE&psig=AFQjCNGCotHU61a6KBGjxvhKY0zvMaAKEQ&ust=1383155527232503

2. Quantum PowerWhat does it mean for energy to be quantized?

Whole numbers of what?Whole numbers of quantum

What is a quantum?The smallest UNIT of energy.

A penny is similar to a quantum because…

2. Quantum PowerEinstein and the Photoelectric Effect

Photoelectric Effect:

when metals loseelectrons when it is hit with light

2. Quantum Power

Einstein and the Photoelectric Effect

Why does nothing happenwhen red light makes contact

with the metal?

Why does only violet lightrelease an electron?

2. Quantum Power


It was thought that color should not matter, only intensity

But experiment showed that color does matter.

2. Quantum Power


Einstein applied Plank’s idea, and said

Light is also quantized

Light is made up of particles called

PHOTONS PHOTON: a particle of light

2. Quantum PowerWhy Plank and Einstein are important

Plank’s and Einstein's postulate that energy is quantized is in many ways similar to Dalton’s

description of atoms. Both theories are based on the existence of simple building blocks, atoms in one case, and quanta in the other. The work of Plank and Einstein thus suggested a connection between the quantized nature of energy and the properties of individual atoms. In fact, Einstein's

Nobel Prize was awarded for his work in the photoelectric effect and demonstrating its

fundamental important, not for his famous E=mc2 equation.

2. Quantum PowerWhy Plank and Einstein are important

1. Light is as BOTH waves and particles.

simulation




How is a penny or steps on a stair like a quantum of energy/a photon of light?

2. Quantum Power

Summary & Review

What is a quantum?A package of energy, the smallest unit of energy

How is a photon like a quantum?A photon is like a quantum because a photon is the

basic unit of light

Explain what it means for energy to be quantized by using one of the examples used in class: stairs, hills,

penny, music notes

1. Quantum ModelWhat does it mean for energy to be quantized?

It means that energy is transferred in whole numbers.

Example: Stairs vs a hill, music, US Dollars

What does it mean for light to be quantized?

It means that light is also transferred in whole numbers because light is made up of

particles

What is a quantum?Smallest unit of energy

What is a photon?A particle of light

How is a penny like a quantum of energy?Just like the penny is the smallest unit, a quantum

is the smallest unit of energy.

1. Quantum ModelMax Plank

E = hv

h = Plank’s Constant

h = 6.626 x 10-34 J•sec

(J = Joule, the unit for measuring energy)

1. Quantum Model

Plank + Einstein = Calculating the Energy of one Photon

E = (hc)/l

h = Plank’s Constant

h = 6.626 x 10-34 J•secThis number NEVER changes

(J = Joule, the unit for measuring energy)

1. Quantum ModelPlank + Einstein = Calculating the Energy of a Photon

E = (hc)/l

The blue color in fireworks results when copper is heated to about 1200°C. The blue light has a

wavelength of 450 nm. What is the unit of energy emitted?

1. Write equation2. Plug in values. h = 6.626 x 10-34 J•sec ALWAYS3. Solve

ANSWER = 4.42 x 10-19 J


E = (hc)/l

A ruby laser emits a red light at a wavelength of 694.3 nm. What is the energy in J?

1. Write equation2. Make sure l is in METERS. Plug in values. h = 6.626

x 10-34 J•sec ALWAYS 3. Plug in values. h = 6.626 x 10-34 J•sec ALWAYS4. Solve

ANSWER = 2.861 x 10-19 J


E = (hc)/l

An x-ray generator, such as those used in hospitals, emits radiation with a wavelength of 1.544 angstrom.

What is the energy of a single proton?

1. Write equation2. Make sure l is in METERS. Plug in values. h = 6.626

x 10-34 J•sec ALWAYS 3. Plug in values. h = 6.626 x 10-34 J•sec ALWAYS4. Solve

ANSWER = 1.287 x 10-15 J

1. Quantum ModelPlank + Einstein = Calculating the Energy of a

Photon

E = (hc)/l

1. Write equation2. Make sure l is in METERS. If not, then

convert it to METERS using sideways T 3. Plug in values h = 6.626 x 10-34 J•sec

ALWAYS Plug in values. c = 3.0 x 108 m/sec ALWAYS

4. Solve

3. History, Period.

What is atomic number?Where is the atomic number found on the

Periodic Table?

What is atomic mass?Where is the atomic mass found on the

Periodic Table?

3. History, Period.

OBJECTIVE: History of the Periodic Table

3. History, Period.

Brief History of the Table

Just like class activity many different versions• 1860 - John Newlands & Octaves• 1869 – Dimitri Mendeleev

• Compare Mendeleev’s table with the modern one.

• List two similarities and two differences

3. History, Period.• 1869 – Dimitri Mendeleev

3. History, Period.• 1869 – Dimitri Mendeleev• put elements into ROWS by ATOMIC MASS.• made columns by PROPERTY• Left blank spaces • Blanks = elements not yet discovered• Predicted properties of undiscovered elements• AND PREDICTIONS WERE CORRECT!

3. History, Period.

Brief History of the Table

• Just like class activity, different versions• 1860 - John Newlands & Octaves• 1869 – Dimitri Mendeleev

So how did we get from Mendeleev’s table to today’s table?

3. History, Period.

3. History, Period.

Modern (YOUR) Periodic Table

Arranged by ROWS By ATOMIC NUMBER

3. History, Period.

Modern (YOUR) Periodic Table

Arranged by COLUMNSBy SIMILAR PROPERTIES

3. History, Period.

Brief History of the Table• Just like class activity, different versions• 1860 - John Newlands & Octaves• 1869 – Dimitri Mendeleev• 1913 – J. Moseley & Protons & Atomic #

• Nickel vs Cobalt

Classwork: Textbook pg 122, #2,5,6,7,8

3. History, Period.Summary & Review

1. In what two ways is today’s periodic table organized?

2. List 2 ways Mendeleev and your table are different. List 2 ways how they are similar

3. Why is Nickel and Cobalt placed in a different order in your PT than it was in Mendeleev’s?

4. In 2013, a new element was created, element 115. Use your periodic table to predict

1. Its possible mass2. Its period and group3. Elements with similar property

4. Atom is Bohr-ed

Draw our solar system on your warmup paper

Draw a hydrogen atomIt was one proton and one electron

Draw a helium atomIt has two protons, two neutrons and two electrons

Draw a lithium atomIt has three protons, three neutrons, three

electrons

4. Atom is Bohr-ed

OBJECTIVE: Another model of the Atom

4. Atom is Bohr-ed

Bohr said that electrons ORBIT the nucleus

Okay…how is this different from Rutherford’s model?

4. Atom is Bohr-edBohr’s Model

Bohr said that electrons ORBIT the nucleus,

ORBITS are QUANTIZED

What does this mean???

4. Atom is Bohr-ed

You MUST be ON a step

You CANNOT beBETWEEN steps

4. Atom is Bohr-ed

Orbits are “quantized”

means…

electrons MUST

be ON an orbit

Electrons CANNOT beBETWEEN

orbits


You CANNOT be BETWEEN

steps

4. Atom is Bohr-ed

Orbits are “quantized”

means…

The orbits are like steps!

Notice the “steps”/orbits are not all the

same distance?

4. Atom is Bohr-ed

Orbits are “quantized” means…

electrons MUST be ON an orbit

Electrons CANNOT be BETWEEN

orbits


You CANNOT be BETWEEN

steps

4. Atom is Bohr-edWhy did Bohr say

atoms have quantized orbits?

Evidence?

LINE SPECTRUMS was Neil Bohr’s evidence

that atoms have quantized orbits

4. Atom is Bohr-edWhat is a line spectrum?

RedOrangeYellowGreenBlue

+ Purple/VioletWhite Light

4. Atom is Bohr-ed

What is a line spectra?

4. Atom is Bohr-edEnergy, Photons and Line Spectrum

What is a line spectra?

4. Atom is Bohr-ed

Why do we get line spectrums?

4. Atom is Bohr-ed

4. Atom is Bohr-edBohr’s Model

4. Atom is Bohr-edOrbits represent

ENERGY LEVELS

Closer to nucleus = lower energy levelFarther from nucleus = higher EL

Period = Energy Level

Period 1 = LowestPeriod 7 = Highest

4. Atom is Bohr-ed

IMPORTANTBohr’s idea of orbit is correct

…kind of

After more discovery, we call it an orbital,and yes, there is a BIG difference

BUT, for us, we will treat it similarly

4. Atom is Bohr-edThere are 4 types of orbits/orbitals

S orbital

P orbital


D orbital


F orbital


We are only going to use the

s p

d orbitals

4. Atom is Bohr-ed

4. Atom is Bohr-ed

What is the difference between

1s orbital and 2s orbital??

size (draw)

4. Atom is Bohr-ed

1. What do the orbits/orbitals represent?

2. What does it mean for orbits to be quantized?

3. What are the three orbitals we will use?

4. What is the different between a 1s orbital and a 2s orbital?

5. What is the difference between a 2p and a 3p orbital?

6. What do the number and the letter represent in “1s” and “2p”?

5. Electron Configuration

So what do we do with the orbitals and

the energy levels?


OBJECTIVE: Learn how electrons are organized inside an atom

5. Electron ConfigurationEach orbital can have

2 electrons MAX

1s orbital and 2s orbital

5. Electron ConfigurationEach orbital can have 2 electrons

S orbital 2 electrons


p orbital

2

2

2

6 electrons


d orbital

2 + 2 + 2 + 2 + 2 = 10 electrons


f orbital

5. Electron ConfigurationHow to write Electron Configurations

1. Find element on PT2. Write symbol of element3. Write number of electrons4. Start counting from Hydrogen. 5. you MUST start at Hydrogen, ALWAYS6. Count from left to right, in this direction 7. Use H.O. to help remember the different

blocks.8. Check your work


Write electron configurations for the following elements

H He Be C O Ne

Mg Al Si Sc V Co


What are valence electrons?

electrons in its outermost orbital are called the

valence electrons


How do we know which are the valence electrons?

electrons in the HIGHEST ENERGY LEVEL are

valence electrons


Write electron configuration for Silicon, Si

Si = 1s22s22p63s23p2

Si = 1s22s22p63s23p2


Write electron configuration for Gallium, Ga

Ga = 1s22s22p63s23p24s23d104p1

Ga = 1s22s22p63s23p24s23d104p1

Ge has 3 valence electrons


1.Write electron configurations

2.Underline valence electrons

Do you notice a pattern?

Lithium Mg Boron Sulfur Fluorine Neon

Sodium Ca Aluminum Sellenium Chlorine Krypton


1. Write electron configurations for the following2. Underline the valence electrons

Barium

[Xe]6s2

Carbon

[He]2s22p2

Nitrogen

[He]2s22p3

Oxygen

[He]2s22p4

Fluorine

[He]2s22p5

Neon

[He]2s22p6

Aluminum Tin Phosphorus Tellurium Chlorine Krypton


How many valence electrons do you predict the last row will have?

Do you notice a pattern?

Barium Carbon Nitrogen Oxygen Fluorine Neon

Aluminum Tin Phosphorus Tellurium Chlorine Krypton

Indium Silicon Arsenic Selenium Bromine Argon


EXAMPLE:Sodium 1s22s22p63s1 = [Ne]3s1

Lithium 1s22s1 = [He]2s1

This pattern is seen in columns 1-2 and 13-18 of the PT

What other patterns might exist within the PT?Maybe there is a reason why the PT has that weird shape!

5. Electron ConfigurationSummary & Review

1. How many electrons can the s, p, and d orbitals hold?

2. What are valence electrons

3. How do you know which electrons are the valence electrons?

4. Write the EC for Calcium and Titanium5. How many valence electrons do calcium and

titanium have? What is their energy levels?

Periodic Table

Important GROUPS

1.Alkali Metals2.Alkali Earth Metals3.Halogens4.Noble Gases5.Transition Metals6.Lanthanides7.Actinides8.Metalloids

Periodic Table

1. Alkali Metalsmetalsvery reactive

2. Alkali Earth Metalsmetaldoes NOT dissolve quickly in waterhigh melting point

Periodic Table

3. Halogensnon-metalvery reactive

4. Noble Gasesgasesstablenot reactive – why?

Periodic Table

5. Metalsconducts heat and electricitymalleable – like Playdoh ductile

Periodic Table

6. Lanthanidesextremely rare

7. Actinidesalso rareradioactive

Periodic Table 8. Metalloids

solid, but not metalhas properties of metals

outline of topics 1. a light wave – what is light? 2. history of the periodic table 3. electron...

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