1. Quantum Mechanics, electron configurations, Shape of PT

2. Classical vs. Quantum Mechanics
Wave or particle, wave continuous, macroscopic level
Quantum
Wave and particle, wave quantized, nanoscopic level
Behavior of objects at the microscopic level

3. Heisenberg & Schrodinger
Uncertainty principle
Location & momentum cannot be known at the same time
Schrodinger
Created mathematical description of e- in an orbital
4 principle quantum numbers

4. Principle Quantum Numbers
Principle QN: n
Describes distance from nucleus
Angular momentum: (L)
Describes shape of an orbital
Magnetic QN: (Ml)
Describes orientation in space of orbitals, # of suborbitals in shell
Electron Spin QN: (Ms)
Describes the “spin” of an electron

5. Orbital Shapes S orbital- holds 2 e- P orbital- holds 6 e-
D orbital- holds 10 e-
F orbital- holds 14 e-

6. Valence Electrons Electrons in the outermost orbital Octet Rule
Focus more on S and P orbitals

7. Aufbau Principles Orbitals only hold 2 e- with opposite spin
Fill lower energy levels before filling higher energy orbitals
“Hund's Rule”
If two or more degenerate energy levels are available one e- goes in each until they are half full by pairing e- up

8. Order of the Orbitals Looking at shape of periodic table
Memorize 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, and 7p Or

10. Electron Configurations
Configuration for Oxygen Mg Sn

11. Shape of Periodic Table
Rows: Same principle
QN (n-size)
Columns: Same set
Of valence e-, similar
Physical & chemical
properties

12. Size of Molecules on the Periodic Table
-Across a row, molecules decrease in size. Ex: Al is larger than Cl
-Down a column, molecules increase in size. Ex: O is smaller than Te
-Neutral atoms are always going to be bigger than cations, but will be smaller than anions.
Ionization energy: As the size of the molecule gets smaller across a row, the ionization energy grows. As you move down a column and the molecules get bigger, ionization energy gets smaller.
Removing electrons from a complete octet, from a lower energy level takes a much larger amount of ionization energy.