Unit 4 Chemistry

The Principal Quantum Number (n)

describes the size or energy of the atomic orbital

The Angular Quantum Number (l)

described the shape of the orbital

The Magnetic Quantum Number (ml)

describes the orientation of the orbital in space

the Spin Magnetic Quantum Number (ms)

describes the spin of an electron

Value of L = 0

S - sphere

Value of L = 1

P - dumbbell

value of L = 2

D = 4 orbitals and a donut

value of L = 3

f = 5 orbitals and 2 donuts 

Aufbau Principle

electrons in ground state atoms always fill low energy orbitals before high energy orbitals

Pauli Exclusion Principle

only two spin paired electrons can occupy a single orbital

Core electrons

Valence Electrons 

Hund’s Rule

the lowest energy electron configurations has the maximum number of unpaired electrons, and all unpaired electrons in atom have the same spin