Bonding

Question 1

CO2

Answer 1

linear
180

Question 2

BF3

Answer 2

trigonal planar
120

Question 3

SO2

Answer 3

V-Shaped / bent
119

Question 4

CH4

Answer 4

Tetrahedral
109.5

Question 5

NH3

Answer 5

trigonal pyramidal
107

Question 6

H2O

Answer 6

v-shaped
104.5

Question 7

PCl5

Answer 7

trigonal bipyramidal
90 and 120

Question 8

SF4

Answer 8

seasaw
<90 and <120

Question 9

ClF3

Answer 9

T shaped
87.5

Question 10

XeF2

Answer 10

linear
180

Question 11

SF6

Answer 11

octahedral
90

Question 12

BrF5

Answer 12

square pyramidal
<90

Question 13

XeF4

Answer 13

square planar
90

Question 14

Electronegativity Definition

Answer 14

• the measure of tendency
• an atom has to attract a pair of electrons
• in a covalent bond

Question 15

Factors effecting electronegativity

Answer 15

• nuclear charge
• distance
• shielding

Question 16

Types of intermolecular forces (weakest to strongest)

Answer 16

• van der Waal’s forces
• permanent dipole-dipole
• hydrogen bonds

Question 17

van der Waal’s forces

Answer 17

• instantaneous dipoles
• which can induce a dipole in another molecule
• causing a temporary attraction

Question 18

permanent dipole-dipole

Answer 18

• between δ+ αnd δ- ends of a molecule

Question 19

hydrogen bonding

Answer 19

• when H is bonded to either: N, O, or F
• creates permanent dipoles (due to large electronegativity difference)

Question 20

Octet Rule exceptions

Answer 20

Incomplete octet: not enough electrons (B and Be)

Expansion of the Octet: (Period 3+, groups 5-7)

Question 21

Cations and Anions charge

Answer 21

Cations = +
Anions = -

Question 22

VESPR Theory

Answer 22

• pairs of electrons in out shell repel
• so electrons are as spread out as possible
• lone and bond pairs are charge clouds
• lone pairs repel more than bond pairs

Question 23

macromolecular meaning

Answer 23

large covalent structure

giant molecule with covalent bonding