1. Bellwork (…to be done when you walk in)
Write down three facts that you know about electrons.

2. Unit 2: Electrons in Atoms
Mr. Gates
Ch. 5
Prentice Hall Chemistry

3. Learning objective I can define “electron configuration.”
I can write the electron for a given element.

4. Orbitals
Schrodinger developed the Quantum Mechanical Model which described the location of electrons based on probability.
Atomic orbitals are regions in space with the highest probability of finding an electron.

5. Main Types of Orbitals
Dumbbell

6. Electron Configuration
Electron Configuration: the way electrons are arranged around the nucleus of an atom.

7. Aufbau Diagrams

8. Electron Configurations Rule #1
Aufbau Principle: electrons enter orbitals with the lowest energy first

9. Electron Configurations Rule #2
Pauli Exclusion Principle: a suborbital can hold a maximum of TWO electrons each of opposite spins.

10. Electron Configurations Rule #3
Hund’s Rule: When electrons occupy suborbitals of equal energy, one electron enters each suborbital until each has an electron of parallel spins, before entering a second electron into the suborbital.
Half fill each suborbital before completely filling any suborbital of the same energy.

11. Example of Hund’s Rule

12. Practice
Fill in the energy level diagram (aufbau diagram) on the right for a neutral oxygen atom.

13. Practice… solution
Fill in the energy level diagram (aufbau diagram) on the right for a neutral oxygen atom.

14. Bellwork…
Draw an Aufbau diagram for a chlorine atom.

15. Writing Electron Configurations

16. Examples K
1s22s22p63s23p64s1 O
1s22s22p4 Cl
1s22s22p63s23p5

17. Exit task Write down the electron configuration of Nitrogen.
Show Mr. Gates, the correct electron configuration of Nitrogen to get a copy of the homework.

18. Noble Gas Notation K O Cl 1s22s22p63s23p64s1 [Ar] 4s1 1s22s22p4
[He] 2s22p4 Cl
1s22s22p63s23p5
[Ne] 3s23p5

19. Learning Objective
I can identify the trend of electron configurations on the periodic table.

21. Tricks of the Trade
s = same as period number
p = same as period number
d = period number minus 1
f = period number minus 2

22. Periodic Table and Orbitals

23. Represents how orbitals fill using lines and arrows
Orbital Notation
Represents how orbitals fill using lines and arrows

24. Orbital Notation

25. *Exceptional Electron Configurations
All elements up to V follow the normal e- configurations
After that there are exceptions
Sometimes electrons rearrange themselves so orbitals are full or half-full instead of partially full

26. *Exceptional Electron Configurations
Expected e- configuration
Cr 1s22s22p63s23p64s23d4
Cu 1s22s22p63s23p64s23d9
Predicted e- configuration
Cr 1s22s22p63s23p64s13d5
Cu 1s22s22p63s23p64s13d10

27. Bellwork… start working on as soon as you get to class.
Work with a partner to brainstorm as many sources of light as you can think of that you have encountered in your life.
Examples: sun, light bulbs, fireworks, etc.
Answer the question: is all light visible?

28. Light… particle or wave?
Early scientists believed that light behaved as a wave.
Later evidence suggested that light behaves like a particle.
PLJicmE8fK0EiEzttYMD1zYkT-SmNf323z&v=Hk3fgjHNQ2Q

29. Parts of a Wave Wavelength ( λ - lambda )- the distance between crests
Amplitude- the height of a wave from the origin to the crest

30. Frequency (v)
Frequency is the number of wave cycles to pass a given point per unit of time.
Units are usually cycles per second
The SI unit of cycles per second is called a hertz (Hz)
Hertz can also be expressed as inverse seconds (s-)

31. Assessment for learning
Draw a line about 5in long in your notes and draw two waves on this line with the same amplitude, but different frequencies.
Draw a line about 5in long and draw two waves on the line with the same wavelengths, but with different amplitudes.

32. Relationship between (v) and (λ)
Frequency and Wavelength are inversely proportional.
As one goes up, the other goes down.
The speed of all light is constant.
c (speed of light) = 3.0 x 108 m/s
c = vλ

33. Practice
What is the frequency of light that has the wavelength of 1.2 x 10-5m?
2.5 x 1013 s-
What is the wavelength of light that has a frequency of 4.35 x 1018s- ?
6.9 x 10-11m

34. Mo’ Practice, Mo’ Perfect
A red light has a wavelength of 728 nm.  What is the frequency of the light? (1 nm = 10-9 m)
A purple light has a frequency of 7.42 x Hz.  What is its wavelength?
4.12 x 1014 or x 1017
4.04 x 10-7

35. Electromagnetic Spectrum

36. Homework
Pg. 146
# 16, 21
Pg. 149
# 40, 42, 45, 46,

37. Energy and Light
Energy of a light wave is directly related to the frequency.
Higher energy = higher frequency
E = h x v
Where:
E = Energy (J)
h = x Js
v = Frequency (Hz)

38. Practice Calculations
What is the energy of a photon whose frequency is 3.0 X 1012 Hz?
Calculate the photon energy of light (in J) with a wavelength of 254 nm
1.98 x J
7.826 x 10-19

39. Let’s get excited!!!
When people get excited, their level of energy as displayed to those around them increases.
When electrons get excited, their level of energy increases as well
When electrons become de-excited, their level of energy drops.

40. Started from the bottom…
An electron in its lowest possible energy state is in its ground state.

41. Excited Electrons
As electrons become excited, they jump up to an orbital of a higher energy level.
This is caused by an absorbance of energy.
As electrons become de-excited, they drop to an orbital of a lower energy level.
This causes a release or emission of energy.

42. To Excite or Not Excite
An electron must absorb/emit exactly the energy equal to the difference between the energy level it is at and the energy level it will be excited/de- excited into, in order for the electron to move between orbitals.
More or less than exactly the energy gap will result in NO CHANGE.

43. Energy Emissions Energy is emitted in the form of light.
The type of light that is emitted depends on how far an electron falls.
The farther an electron falls, the greater the energy and the frequency of the light it emits.

44. Light and the Atom
If there are multiple electrons, then multiple frequencies of light can be emitted.
Different elements release different colors of light.

45. Atomic Emission Spectrum
The different frequencies of light that are released can be observed and recorded to produce an Atomic Emission Spectrum.
This can be used as a “signature” for an element

46. Homework
Pg. 146
# 17, 18,
Pg. 149
# 47,
Pg. 151
# 76