1. Quantum Theory

2. Werner Heisenberg Heisenberg Uncertainty Principle
You cannot know the location and velocity of an electron (or any other particle) at any given time
Electrons are located using photons
Because they are about the same size, the photon knocks the electron off course.

3. Schrödinger Created equation that treated electrons as waves
Only worked for waves of certain frequencies
Showed quantization
Schrödinger and Heisenberg basis of Quantum Theory

4. Where are electrons?

5. Quantum Numbers
Describe the properties of orbitals and electrons around the nucleus
Kind of like an address for where and in what state you are likely to find electrons
There are 4 quantum numbers

6. Principle Quantum Number
Symbol = n
Gives the main energy level
1-7
Lower numbers closer to nucleus

7. Angular Momentum Number
Symbol = l
Gives the shape of the sublevel
s,p,d,f
s= 1 orbital
p = 3 orbitals
d = 5 orbitals
f = 7orbitals

9. Magnetic Quantum Number
Symbol = m
Gives the orientation around the nucleus
Indicates which orbital

10. Spin Number
If 2 electrons in the same orbital spin in the same direction, they will create a magnetic field
So electrons sharing an orbital must spin in opposite directions
Spin number shows which direction each is spinning

11. Electron configurations

12. Rules Aufbau principle- fill from lowest energy to highest energy
Hunds Rule- place 1 electron in all orbitals of equal energy before putting 2 electrons in any 1 orbital
Paulie Exclusion Principle - 2 electrons sharing an orbital must spin in opposite directions

13. Energy Diagrams

14. Examples