1. Electron Configuration
Radiant Energy

2. Waves Light travels as both Waves and Packets of energy.
Light is a form of Electromagnetic Radiation.
EM Radiation has waves in the electric and magnetic fields
All waves (Water or Electromagnetic) have 4 key characteristics:
Amplitude
Wavelength
Frequency
Speed

3. Wave Characteristics Amplitude. Wavelength.
Height of a wave from origin to a peak/crest.
Affects brightness and intensity.
Wavelength.
Distance from crest to crest. Distance for one full cycle.
Visible light: nm.

4. Wave Characteristics Frequency. Speed.
How fast a wave oscillates (moves up and down).
Units: s-1, 1/s or Hz.
Speed.
Speed of light a constant:
3.00 X 108 m/s.
Frequency and Wavelength related by the equation:  = c / 

5. Try this…
If the frequency of a wave is 93.1 x 106 s-1, what is the wavelength?
Answer: m
If the wavelength of a wave is 1.54 mm, what is it’s frequency?
Answer: x 1011 Hz (s-1)

6. Have a Problem? Rearranging the equation:
First, multiply by  (frequency):
   = (c/)  
Now, divide by  (wavelength):
() /  = c / 
Leaving:  = c/
Moving on….

7. Electromagnetic Spectrum
Many parts including:
Gamma Rays (10-11 m)
X-Rays (10-9 m)
Ultra-violet (10-8 m)
Visible (10-7 m)
Infared (10-6 m)
Microwave (10-2 m)
TV/Radio (10-1 m)

8. Electromagnetic Spectrum
Visible Spectrum:
ROY G BIV
Red
Orange
Yellow
Green
Blue
Indigo
Violet

9. Electromagnetic Spectrum (once more)

10. Electron Configuration
Quantum Theory

11. Early Puzzlements
Wave model for light was originally accepted by scientific community.
This couldn’t explain why metals heating first emitted invisible radiation and then visible radiation.
Other questions included why elements only emitted certain characteristic colors of light.

12. Plank’s Theory
Every object can only absorb or emit a fundamental amount of energy.
This amount is called a quantum.
The amount is like moving up or down steps.

13. Plank’s Theory
Plank’s Theory is based on the relationship between frequency and the energy of the particle.
E = h
Plank’s Constant:
h = X J-s

14. Quick Practice
If a wave has a frequency of 9.33x106 Hz, what is it’s energy?
6.18x10-27 J
What is the frequency of a wave if its energy is 4.32x10-31 J?
652 Hz

15. Photoelectric Effect
Einstein used Plank’s equation to explain a puzzling phenomenon, the Photoelectric Effect.
Electrons ejected from metal when light shines on it.
Metal need’s certain frequency of light to release electrons. In Sodium, red light is no good, violet releases them off easily.
Photons: Tiny particles of light providing energy to “knock off” electrons.

16. Dual Nature of Radiant Energy
Proven in 1923 by Arthur Compton
Showed photon could collide with an electron like tiny balls.
Summary:
Light behaves as a wave ( = c/)
Light behaves as a particle (E = h)

17. Electron Configuration
Another Look at the Atom

18. Line Spectra
Def: A spectrum that contains only certain colors/wavelengths.
AKA: The Atomic Emission Spectrum
Each element has it’s own “fingerprint” emission spectrum.

19. The Bohr Model
Bohr drew the connection between Rutherford's model of the atom and Planks idea of quantization.
Energy levels labeled with Quantum Numbers (n)
Ground state, or lowest energy level – n=1
Excited State – level of higher energy

20. Matter Waves If energy has dual nature, why not matter?
De Broglie thought so.
Matter Waves – the wavelike behavior of waves.
Didn’t stand without experimental proof
Davison and Germer proved this with experiments in 1927.
Why don’t we see these matter waves? Mass must be very small to observe wavelength.

21. Heisenberg Uncertainty
Uncertainty Principle
The position and momentum of a moving object cannot simultaneously be measured and known exactly.
Translation:
Cannot know exactly where and how fast an electron is moving at the same time.

22. Electron Configurations
A New Approach to the Atom

23. Quantum-mechanics Model
Includes all the ideas of the atom we have covered:
Energy of electrons is quantized
Electrons exhibit wavelike behavior
Electrons position and momentum cannot be simultaneously known
Model does describe the probable location of electrons around the nucleus

24. Probability and Orbitals
Electron Density:
The density of an electron cloud.
Atomic Orbitals:
A region around the nucleus of an atom where an electron with a given energy is likely to be found.
Kinds of orbitals:
Each kind has own different basic shape.
Given letter designations of s, p, d and f.
s-orbitals are spherical
p-orbitals are dumbbell
d- and f-orbitals more complex.

25. Orbitlas and Energy
Principle energy levels (n) can be divided into sublevels.
Number of sublevels is equal to the number of the principle energy level.

26. Orbitals and Energy Each sublevel has one or more orbitals
P – three
d – five
f – seven
Summary provided in figure 4-28 (pg 145)

27. Electron Spin Electrons have two spins:
Up or clockwise
Down or counterclockwise
Only two electrons (one of each spin) can occupy an orbital. These electrons are said to be “paired”.

28. Electron Configurations