Chemistry - Quantum Mechanics

if n = 1, the possible value(s) of l = ____

0

if n = 2, the possible value(s) of l = ____

0, 1

if n = 3, the possible value(s) of l = ____

0, 1, 2

if n = 4, the possible value(s) of l = ____

0, 1, 2, 3

if n = 1, and l = 0, ml = ___

0

if n = 2, and l = 0, ml = ___

0

if n = 2, and l = 1, ml = ___

-1, 0, 1

if n = 3, and l = 0, ml = ___

0

if n = 3, and l = 1, ml = ___

-1, 0, 1

if n = 3, and l = 2, ml = ___

-2, -1, 0, 1, 2

if n = 4 and l = 0, ml = ___

0

if n = 4 and l = 1, ml = ___

-1, 0, 1

if n = 4 and l = 2, ml = ___

-2, -1, 0, 1, 2

if n = 4 and l = 3, ml = ___

-3, -2, -1, 0, 1, 2, 3

1s, 2s, 2p, 3s, 3p… name the next 5 orbitals

4s, 3d, 4p, 5s, 4d

S-Ville = Groups:

1, 2

P-Ville = Groups:

13-18

D-Ville = Groups:

3-12

F-Ville = Groups:

lanthanides and actinides  

no two e- in the same atom can have identical quantum numbers, spin up/spin down

Pauli Exclusion Principle

orbital first has to be filled up by a single e- before doubling up

Hund’s Rule

filling orbitals from lowest energy to highest energy

Aufbau’s Rule

Size of atoms/ions __________ moving to the left and ___________ moving down

decrease, increase

Ionization energy __________ moving to the left and ___________ moving down

increases, decreases

Electron affinity (more negative) __________ moving to the left and ___________ moving down

increases, decreases

Electronegativity __________ moving to the left and ___________ moving down

increases, decreases

Ionization energy has exceptions in Groups:

2/3, 5/6

Electron affinity has exceptions in Groups:

1/2, 4/5

Reactivity for metals ___________ moving to the left and ___________ moving down

decreases, increases

Reactivity for nonmetals ___________ moving to the left and ___________ moving down

increases, decreases

Zeff = Z - S, Z =

atomic number

Zeff = Z - S, S =

screening constant (noble gas before it)

Lattice energy ________ with charge of ions and ________ with decreasing size of ions

increases, increases

(val e-) - 1/2(bond e-) - (nonbond e-)

Formal Charge

Determined by number of bonding pairs and number of lone e- pairs (number of electron pairs)

electron domain

2 e- pairs

Linear

3 e- pairs

Trigonal Planar

4 e- pairs

Tetrahedral

5 e- pairs

Trigonal Bipyramidal

6 e- pairs

Octahedral

3 e- groups, 1 lone pair

MDG: bent

4 e- groups, 1 lone pair

trigonal pyramidal

4 e- groups, 2 lone pairs

bent