Chapter 3- Bonding And Chemical Interactions

Question 1

Elements with expanded octet

Answer 1

Any element in period 3 and greater
Phosphorus (10)
Sulfur (12)
Chlorine (14)

Question 2

Elements with odd numbers of electrons

Answer 2

Any molecule with an odd number of valence electrons cannot distribute those electrons to give eight to each atom

Ex: NO (nitric oxide) has 11 valence electrons

Question 3

Elements with incomplete octet

Answer 3

Hydrogen (2) 
Helium (2) 
Lithium (2) 
Beryllium (4)
Boron (6)

Question 4

Ionic bonds

Answer 4

Usually formed between metal and nonmetal because it requires a large difference in electronegativity

Very strong so high melting and boiling points

Question 5

Dipole moment

Answer 5

P = qd

P - dipole moment
q - magnitude of charge
d - displacement vector separating 2 partial charges

Question 6

Lewis acid and Lewis base

Answer 6

Acid - accepts lone pair of electrons

Base - donates a pair of electrons to form a covalent bond

Question 7

Coordinate covalent bonds

Answer 7

Both of shared electrons come from same atom

Question 8

Formal charge equation

Answer 8

FC = V - Nnonbonding - (1/2)Nbonding

V - valence electrons in neutral atom

Question 9

VSEPR theory

Answer 9

Valence shell electron pair repulsion theory.
Predicts molecular geometry of covalent lay bonded molecules.
3-D arrangement is determined by repulsion a between bonding and nonbonding electron pairs in valence shell.

Question 10

Linear shape

Answer 10

Electron density- 2
Shape- linear
Angle b/w electron pairs- 180

Question 11

Trigonal planar

Answer 11

Electron density- 3
Shape- trigonal planar
Angle b/w electron pairs- 120

Question 12

Tetrahedral

Answer 12

Electron density- 4
Shape- tetrahedral
Angle b/w electron pairs- 109.5

Question 13

Trigonal bipyramidal

Answer 13

Electron density- 5
Shape- trigonal bipyramidal
Angle b/w electron pairs- 90, 120, 180

Question 14

Octahedral

Answer 14

Electron density- 6
Shape- octahedral
Angle b/w electron pairs- 90, 180

Question 15

Difference b/w electronic and molecular geometry

Answer 15

Electronic- spatial areangement of all Paris of electrons around central atom (lone and bonding)

Molecular- spatial arrangement of only bonding pairs of electrons

Question 16

Order of intermolecular interactions from weakest to strongest

Answer 16

1. London forces (dispersion)
2. Dipole-dipole interactions
3. Hydrogen bond

Question 17

London dispersion forces

Answer 17

Electron density being rapidly/randomly unequal causes quick dipole moments that cause a domino effect of more quick dipole moments in neighboring molecules
liquify noble gases

Question 18

Dipole-dipole interactions

Answer 18

Same as London dispersion, but they last longer and have higher melting and boiling points

Question 19

Hydrogen bonds

Answer 19

Only with F, O, and N

Question 20

In acid base reactions we are most concerned with…

Answer 20

Hydrogen ions

Question 21

In oxidation reduction reactions we are most concerned with….

Answer 21

Concentration of electrons