Unit 3

Question 1

Pauli Exclusion Principle

Answer 1

2e- within same orbital must have opposite spins

Question 2

Hounds Rule

Answer 2

Give each orbital 1e- before pairing (within same energy level)

Question 3

Aufbow Principle

Answer 3

Fill lower energy orbitals first

Question 4

Magnetic Quantum Number, Ml

Answer 4

Orientation of e- orbitals
Values: -l:+l

Question 5

Spin Quantum Number Ms

Answer 5

Relates to the spin of e-
Values: +1/2 or -1/2

Question 6

Principle Quantum Number, n

Answer 6

Relates to energy of e-
Values: integer

Question 7

Secondary Quantum Number, L

Answer 7

Relates to the shape
Values: 0 to (n-1)

Question 8

Ferromagnetic

Answer 8

Strong magnet
Less atoms = stronger magnetism

Question 9

Paramagnetic

Answer 9

Weak magnet
Not noticed unless interacting with strong magnet

Question 10

Hybridization

Answer 10

Atomic orbital -> molecular orbitals
- Shapes resemble combinations of atomic orbitals
- Make covalent bonds

Question 11

Energy levels and their max e-

Answer 11

S^2, P^6, D^10, F^

Question 12

How does a molecule hybridize?

Answer 12

Takes from s orbital
Fills p orbitals via hunds Rule
P orbitals extend and overlap tp make pi bonds

Question 13

Sigma bonds

Answer 13

Overlap of SP orbital
Triple bond(?)

Question 14

Bond Order

Answer 14

= (#bonding e-) - (#antibonding e-) / 2

Question 15

AX2

Answer 15

SP hybridized
180
Linear

Question 16

AX3

Answer 16

120
Trigonal Planar
SP2

Question 17

AX4

Answer 17

SP3
109.5
Tetrahedral

Question 18

AX5

Answer 18

sp3d
Trigonal bipyramidal
90
105

Question 19

AX6

Answer 19

sp3d2
Octahedral

Question 20

Determining its geometry

Answer 20

1. # e- orbitals
2. Hybridization of A
3. Geometry

Question 21

AX3E

Answer 21

SP3
Trigonal pyramidal
107

Question 22

AX2E2

Answer 22

SP3
Bent

Question 23

Lone pairs on geometry

Answer 23

Lone pairs take up less space and push away

Question 24

VSEPR

Answer 24

Valence
Shell
Electron
Pair
Repulsion