1. Arrangement of Electrons

2. Bohr Model
Electron orbit nucleus like planets orbit the sun.

3. Draw Bohr model for the following:Mg Cl

4. What is an atom at ground state?
When all the electrons around the atom is at the lowest level they can be

5. What is an excited state?
When one or more electrons jump to a higher level.
When the electrons fall back to ground state they give off energy, usually in the form of light.
We can usually determine the element by color given off or by its line spectrum.

6. Shapes or Areas that electrons fill
s shape (Alkali metals and Alkaline Earth metals)
p shape (Boron family to Noble gases)
d shape (transition metals)
f shape (Actinide and Lanthanide series)

7. Heisenberg Uncertainty Principle
It is impossible to determine simultaneously both the position and velocity of an electron

8. Aufbau Principle
Electrons occupy the lowest-energy orbital that can receive it.

9. Hund’s rule
Orbitals with the same energy must receive one electron before receiving the second one

10. Orbital Notation for Oxygen

11. d and f shapes Things that are in the d shape are 1 level off
Things that are in the f shape are 2 levels off

12. Electron Configuration Notation for Oxygen
1s2 2s2 2p4

13. Noble Gas Notation for Oxygen
[He] 2s2 2p4
You always start with the noble gas before the element you are looking for.

14. Quantum Numbers Principle Quantum Number (Level)
Angular Quantum Number (Shape)
Magnetic Quantum Number (Seat)
Spin Quantum number (1st or 2nd Electron)

15. Principle Quantum number
What level of the Periodic Table you are in

16. Angular Quantum Number
This number is based on what shape.
s = 0
p = 1
d = 2
f = 3

17. Magnet Quantum Number This is based off of the Angular Quantum Number
If Angular Quantum Number is 1 your possible seats will be -1,0,1
0 is 0
1 is -1,0,1
2 is -2,-1,0,1,2
3 is -3,-2,-1,0,1,2,3

18. Spin Quantum Number Is based on the electron in that seat
If it is the 1st electron you will put + ½
If it is the 2nd electron you will put – ½

19. Quantum Numbers for the last electron in Oxygen
2,1,-1,- ½

20. Pauli exclusion Principle
No two electrons of the same atom have the same Quantum Numbers.