Quantum Mechanics

Can only refer to the probability of finding an e- in a region of space. Cannot specify the path 4 Quantum #’s are required to describe the energy of any electron in an atom (Pauli Exclusion Principle) No 2 e-’s can have the same 4 #’s

Quantum Mechanics Heisenberg Uncertainty Principle Impossible to know both the velocity and position of an electron at the same time

1st Quantum Number (n) Given by the energy level n= 1,2,3,4 to infinity Value of n is the main factor in determining the energy of an electron therefore, its average distance from the nucleus.

2nd Quantum Number (l) p s d f Angular momentum Gives the sublevel (l) l= n-1 n=1,2,3,4 l =0,1,2,3 Value of l= 0 1 2 3 letter s p d f f d s p

Magnetic Quantum Number ( ml ) Orientation of orbital Specifies the exact orbital within each sublevel

3rd Quantum Number (ml) Magnetic quantum number l=0 s sublevel ml=0 only one suborbital l=1 p sublevel ml=-1,0,+1 3 suborbitals l=2 d sublevel ml=-2,-1,0,1,2 5 suborbitals l=3 f sublevel m1=-3,-2,-1,0,1,2,3 7 suborbitals

4th Quantum Number (ms) Spin Number ½ or -1/2

Feeling overwhelmed? Read Section 4-2!

For example Orbital Diagram 1s 2s 2p O 8e-