1.2 Atomic Orbitals, Electronic Configurations and the Periodic Table

Question 1

Quanta

Answer 1

Fixed amount of energy of electrons in an atom

Question 2

Principal Quantum Number (n)

Answer 2

Main energy level of an electron

Question 3

Angular Momentum Quantum Number (l)

Answer 3

Shape of the subshell (s=0, p=1, d=2, f=3)

Question 4

Magnetic Quantum Number (ml)

Answer 4

Orientation of orbital (between -l and +l)

Question 5

Spin Magnetic Quantum Number

Answer 5

Direction of spin (+1/2 or -1/2)

Question 6

Aufbau Principle

Answer 6

Electrons fill orbitals in order of increasing energy

Question 7

Hund’s Rule

Answer 7

When degenerate orbitals are available, electrons fill each singly and with parallel spins before pairing up to fill orbitals

Question 8

Pauli Exclusion Principle

Answer 8

No two electrons in one atom can have the same set of four quantum numbers

Question 9

Isoelectronic

Answer 9

Particles which have the same electronic configuration

Question 10

VSEPR (Valence Shell Electron Pair Repulsion) Theory

Answer 10

Used to predict the shapes of molecules and polyatomic ions

Question 11

Calculating Electron Pairs

Answer 11

• Take total number of outer electrons of central atom and add one for every atom attached
• Add an electron for negative charge
• Remove an electron for positive charge
• Divide by two

Question 12

Strength of Electron Pair Repulsions (strongest to weakest)

Answer 12

Non-bonding pair/non-bonding pair > non-bonding pair/bonding pair > bonding pair/bonding pair