1. Electron configurations
Where they go and why.

2. Orbitals
What are they?
S, P, D and F sublevels hold different numbers of orbitals
What does each one hold?
S sublevel: 2 electrons of opposite spin (1 orbital)
P sublevel: 6 electrons of 3 clockwise 3 counterclockwise spin (3 orbitals)
D sublevel: 10 electrons of 5 clockwise and 5 counterclockwise spin (5 orbitals)
F sublevel: 14 electrons of 7 clockwise and 7 counterclockwise spin (7 orbitals)

3. S P D and F orbitals

4. Examples What is the outer orbital in Helium?
What orbital is filling in Nitrogen?
What orbital is the outside of Copper?
What is the outside of Europium?

5. Drawing orbital filling
Draw Arsenic.
How do we use the shortcut?
You can skip up to the Nobel Gas right before your element.

6. Pauli exclusion principle
What does it say?
An atomic orbital may only hold 2 electrons at one time.
Each electron has to have a different spin (clockwise or counterclockwise).

7. Electron orbital filling
What determines their order?
The aufbau principle states that electrons occupy the orbitals of lowest energy first.
How do we find this order?

8. Spin rules What determines the spin of the electron? Hund’s rule.
This rule states that electrons fill the orbitals in a way that gives the atom the largest number of electrons with the same spin.
What does this mean?

9. Stability What adds to the stability of the atom?
Not all atoms follow the aufbau principle.
Cr and Cu

10. Quantum numbers What are quantum numbers?
Quantum numbers give us a different way to look at energy levels, sublevels, orbitals and spin.
3, 2, 2, ½
First is energy level
Second is sublevel
third is orbital
Forth is electron spin

11. What are the rules for quantum numbers?
First is a whole number 1-7 (n)
Second is 0 to (n-1) (L)
Third is +/- L (m)
Fourth is +/- 1/2