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Unit 7 Review

Total questions: 68

Worksheet time: 3hrs 24mins

Name
Class
Date
1.

What are valence electrons?

a)

The innermost electrons

b)

The outermost electrons

2.

How many valence electrons does Carbon have

a)

1

b)

4

3.

How many valence electrons does Argon have

a)

8

b)

11

4.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
5.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
6.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
7.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
8.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
9.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
10.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
11.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
12.

Which of the following compounds has only single bonds?

a)

I only

b)

II only

c)

III only

d)

I and III

e)

III and IV

13.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
14.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
15.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

16.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

17.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

18.

What would be the bond angle between atoms in this molecule?

a)

180

b)

120

c)

90

d)

109.5

19.

What would be the bond angle between atoms in this molecule?

a)

109.5

b)

120

c)

180

d)

90

20.

What is the name of this molecule's shape?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal pyramidal

21.

What 3-D shape would this molecule have: H2S ?

a)

bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

22.

What is the name of this molecular shape?

a)

trigonal pyramid

b)

tetrahedral

c)

bent

d)

trigonal planar

23.

What 3-D shape would this molecule have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

24.

What 3-D shape would this molecule have?

a)

tetrahedral

b)

trigonal planar

c)

pyramidal

d)

bent

25.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
26.

What shape would a molecule have if it has 4 bonded pairs around its central atom? (It may help if you sketch this out)

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Bent

27.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
28.
Does HCl have hydrogen bonding?
a)
yes
b)
no
29.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
30.

All molecules have London dispersion forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London dispersion forces.  Which of these has ONLY London dispersion forces?

a)

I2

b)

NH3

c)

OCl2

d)

SH2

31.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

32.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

33.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
34.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

35.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

36.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

37.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
38.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
39.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
40.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
41.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
42.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
43.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
44.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
45.

Which is an example of an ionic crystal?

a)

Graphite (lead in a lead pencil)

b)

Sodium Chloride (NaCl)

c)

Ammonia (NH3)

d)

Iron (Fe)

46.

Which type of solid is hard, brittle, has a high melting point, but ONLY conducts electricity if dissolved in H2O or melted.

a)

Ionic Crystal

b)

Covalent Molecular Crystal

c)

Metallic Crystal

d)

Covalent Network Crystal

47.
Which type of solid typically has the lowest melting point of the four types of crystals?
a)
Ionic Crystal
b)
Covalent Molecular Crystal
c)
Metallic Crystal
d)
Covalent Network Crystal
48.

Which type of solid has very strong covalent bonds between neighboring atoms?

a)

Ionic Crystal

b)

Covalent Molecular Crystal

c)

Metallic Crystal

d)

Covalent Network Crystal

49.

Identify the covalent molecular solid crystal.

a)

Diamond (Carbon)

b)

Sodium chloride (NaCl)

c)

Ammonia (NH3)

d)

Iron (Fe)

50.

Identify the metallic crystal.

a)

Graphite (carbon)

b)

NaCl

c)

Ammonia (NH3)

d)

Iron (Fe)

51.

High melting points, good conductors of electricity in the solid state, does not dissolve in water.

a)

Ionic

b)

Metallic

c)

Covalent Network

d)

Covalent Molecular

52.

Very hard, very high melting point, nonconductors of electricity, low density.

a)

Ionic

b)

Metallic

c)

Covalent Network

d)

Covalent Molecular

53.

Identify the property that gives metallic solids the ability to conduct electricity well, but not covalent network solids.

a)

Electrons in metallic solids are strongly bound in place

b)

Electrons in covalent network solids are freely moving around

c)

Covalent network solids are not bound to other atoms

d)

Metallic solids have a sea of electrons that are not bound and can move about the solid freely.

54.

Which of the following is an example of covalent network solid.

a)

Diamond (carbon)

b)

Graphite (carbon in a lead pencil)

c)

copper

d)

silver chloride

55.

Between which points is the temperature of the substance remaining constant?

a)

A-B only

b)

A-B, C-D, and E-F

c)

B-C only

d)

B-C and D-E

56.

__________ show the change in state of matter as heat is added.

a)

Phase diagrams

b)

Heating curves

c)

Density graphs

d)

Temperature plots

57.

The melting point of the sample is

a)

-60 ºC

b)

20 ºC

c)

60 ºC

d)

100 ºC

58.

Which letter indicates where water is in both the solid and liquid phase at the same time?

a)

A

b)

B

c)

C

d)

D

e)

E

59.

A measure of the average kinetic energy of the particles in an object is called

a)

Heat

b)

Temperature

c)

Kinetic energy

d)

Enthalpy

60.

In which region(s) does temperature increase?

a)

Region C only

b)

Regions B and D

c)

Regions A, C, and E

d)

Regions A and B

61.

____________, or temperature, does not chance during a ____________.

a)

Kinetic energy, phase change

b)

Potential energy, phase change

c)

Kinetic energy, heat addition

d)

Potential energy, heat addition

62.

When heat is added to water, temperature increases until

a)

the power of heat expires

b)

the water is hotter than anything else

c)

the water reaches its boiling point

63.

Liquids with very high viscosity flow very _______________________.

a)

fast

b)

not at all

c)

slow

d)

whenever it wants

64.

The best example of high viscosity would be?

a)

Honey

b)

Soap

c)

Marbles

d)

Water

65.

Surface tension is the property of water in which...

a)

water molecules at the surface tend to stick together.

b)

water spills easily.

c)

water tends to be see-through.

66.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

67.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

68.

Liquids with high volatility will

a)

probably not have an odor

b)

have weak intermolecular forces

c)

have strong intermolecular forces

d)

have high surface tension

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