Unit 7

Question 1

2 electron domains, no lone pairs
EDG and MG

Answer 1

linear

Question 2

3 electron domains, no lone pairs
EDG and MG

Answer 2

trigonal planar

Question 3

4 electron domains, no lone pairs
EDG and MG

Answer 3

tetrahedral

Question 4

5 electron domains, no lone pairs
EDG and MG

Answer 4

trigonal bipyramidal

Question 5

6 electron domains, no lone pairs
EDG and MG

Answer 5

octahedral

Question 6

3 electron domains, 1 lone pair EDG and MG

Answer 6

EDG: trigonal planar
MG: bent

Question 7

4 electron domains, 1 lone pair
EDG and MG

Answer 7

EDG: tetrahedral
MG: trigonal pyramidal

Question 8

4 electron domains, 2 lone pairs
EDG and MG

Answer 8

EDG: tetrahedral
MG: bent

Question 9

5 electron domains, 1 lone pair
EDG and MG

Answer 9

EDG: trigonal bipyramidal
MG: seesaw

Question 10

5 electron domains, 2 lone pairs
EDG and MG

Answer 10

EDG: trigonal bipyramidal
MG: T-shaped

Question 11

5 electron domains, 3 lone pairs
EDG and MG

Answer 11

EDG: trigonal bipyramidal
MG: linear

Question 12

6 electron domains, 1 lone pair
EDG and MG

Answer 12

EDG: octahedral
MG: square pyramid

Question 13

6 electron domains, 2 lone pairs
EDG and MG

Answer 13

EDG: octahedral
MG: square planar

Question 14

6 electron domains, 3 lone pairs
EDG and MG

Answer 14

EDG: octahedral
MG: T-shaped

Question 15

6 electron domains, 4 lone pairs
EDG and MG

Answer 15

EDG: octahedral
MG: linear

Question 16

molecular polarity depends on…

Answer 16

bond polarity and molecular geometry.

Question 17

bond polarity

Answer 17

A measure ofhow evenly electrons are shared in a chemical bond, determined by the difference in electronegativity between the bonded atoms.

Question 18

To be a polar MOLECULE a molecule must…

Answer 18

1. have polar bonds.
2. have the polar bonds arranged in a way that their polarity is not cancelled out (unsymmetrical electron cloud) –> non-symmetrical charge distribution –> dipole moment = polar molecule.

Question 19

To determine molecular polarity…

Answer 19

1. Determine the VSEPR shape.
2. Determine the bond polarity, draw the dipole moments.
3. Sum all the dipole moments to determine the net dipole.

Question 20

Resonance structures

Answer 20

(Multiple) hybrid Lewis structures that show different possible arrangements of electrons in a molecule.

Question 21

When do resonance structures occur?

Answer 21

When there is more than one possible position of a double bond in a molecule.

Question 22

Resonance hybrid

Answer 22

An intermediate form of a molecule which exists when more than one valid Lewis formula can be drawn.
This form is more stable, as it has equal bond length and strength for each bond.

Question 23

What is one molecule that has resonance

Answer 23

Benzene (C6H6)

Question 24

Formal charge definition

Answer 24

The charge an atom would have if all the bonding electrons in the molecule were shared equally.

Question 25

Formal charge equation

Answer 25

FC = V - (B+L) V = number of valence electrons in the unbonded atom (determined by the group number) B = number of bondinng pairs L = number of lone/non-bonded electrons

Question 26

Which atom should have the more negative formal charge?

Answer 26

More electronegative atom.

Question 27

Which atom should have the more positive formal charge?

Answer 27

Less electronegative atom.

Question 28

Which atom should be the central atom?

Answer 28

The less electronegative atom (the atom with the ability to form the most bonds).

Question 29

3 types of intermolecular forces

Answer 29

London dispersion forces Dipole-dipole (permanent or permanent-induced) Hydrogen bonding