Download Chapter 7 Handout 1 Atomic Orbitals Quantum Numbers: Principal

Chapter 7
Handout 1
Atomic Orbitals
Quantum Numbers:
Principal Quantum Number (n) = Whole numbers only, determines the energy of an orbital
Angular Momentum Quantum Number (l) = Sublevels = determines shape of orbital (s, p, d, f)
Magnetic Quantum Number (ml) = describes the orientation of the orbital
Electron Spin Quantum Number (ms)= describes electron spin
Sublevel
Max Amount of Electrons
s
2
p
6
d
10
f
14
Electron Configuration:
How the electrons are distributed among the various atomic orbitals.
Energy Level Diagram
7p
6d
5f
5d
4f
7s
6p
6s
5p
4d
5s
4p
3d
4s
3p
3s
2p
2s
1s
Orbital Diagram Notation:
Electron Configuration Notation:
1s2
Rules for filling orbitals:
1. Aufbau Principle:
a. Electrons fill up orbitals of lowest energy first
b. Orbitals in the same sublevel are equal in energy
c. Sometimes energy levels overlap
2. Pauli Exculsion Principle
a. There is a max of 2 electrons in any one orbital
b. These 2 electrons must have opposite spins
3. Hund’s Rule
a. When filling orbitals of equal energy, one enters each orbital first
b. Then, second electron will enter each orbital to form paired opposite spins.
Diagonal Rule (Aufbau Principal) : Orbitals fill upward right to left.
Diamagnetism and Paramagnetism (Pauli Exclusion Principal):
Diamagnetic:
Paramagnetic:
The Shielding Effect: https://www.boundless.com/chemistry/textbooks/boundless-chemistrytextbook/periodic-properties-8/electron-configuration-68/the-shielding-effect-and-effective-nuclearcharge-319-7515/