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Unit 3 Review

Total questions: 106

Worksheet time: 2hrs 1mins

Name
Class
Date
1.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
2.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
3.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
4.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
5.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
6.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
7.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
8.

What shape would PH3 have?

a)

Trigonal Planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

9.
What is the bond angle for this molecule?
a)
109.5
b)
120
c)
107
d)
90
10.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
11.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
12.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
13.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
14.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
15.
What is the molecular shape of a silicon dioxide molecule?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
16.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

17.

Which of the following images represents a Trigonal Planar molecular geometry?

a)
b)
c)
d)
18.

What is the hybridization of this molecule shown above

a)

sp

b)

sp2

c)

sp3

d)

sp4

19.

What is the bond angle for the CH4 molecule?

a)

120°

b)

107°

c)

109.5°

d)

90°

20.

What is the hybridization of the central atom of a bent molecule? (AB2E2)

a)

sp

b)

sp2

c)

sp3

d)

sp3d

21.
The molecule shown in the diagram can best be classified as a
a)
polar covalent molecule
b)
nonpolar covalent molecule
c)
ionic compound
d)
nonpolar ionic compound
22.

The polarity of a bond between two elements can be best determined by

a)

The difference in electronegativity between the elements

b)

The difference in first ionization energy between the elements

c)

The number of electrons shared in the bond

d)

The difference in atomic radius between the elements

23.
Which bond is most polar?
a)
H-F
b)
H-Cl
c)
H-Br
d)
H-I
24.
What kind of bond do you have: Li and Cl
a)
Non-polar covalent
b)
Polar covalent
c)
ionic
d)
James Bond
25.
What are the hybridization and the approximate bond angles in CS2?
a)
sp2, 1070
b)
sp3, 1200
c)
sp2, 1200
d)
sp, 1800
26.

Which of the following is a covalent compound?

a)

SrI2

b)

P4O10

c)

LiOH

d)

ZnS

27.
What type of bonding typically exhibits the greatest melting point and boiling point?
a)
ionic
b)
metallic
c)
polar covalent
d)
nonpolar covalent
28.

When forming an ionic bond, a metal atom

a)

Gains electrons to form a cation

b)

Loses electrons to form a cation

c)

Gains electrons to form an anion

d)

Loses electrons to form an anion

29.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
30.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
31.

In chemical compounds, covalent bonds form when

a)

the electronegativity difference between two atoms is very large.

b)

electrons are completely transferred between two metals.

c)

pairs of electrons are shared between two nonmetal atoms.

d)

two nonmetal atoms are attracted to each other by opposite charges.

32.

An ionic bond forms when

a)

Valence electrons are shared

b)

a sea of mobile electrons surround the cations

c)

valence electrons are transferred between atoms

d)

none of the above

33.

Predict the bond that will form between Cu and F.

a)

Ionic

b)

Covalent

c)

Metallic

34.

Predict the bond that will form between Se and Cl.

a)

Ionic

b)

Covalent

c)

Metallic

35.

Predict the bond that will form between Sr and S.

a)

Ionic

b)

Covalent

c)

Metallic

36.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
37.

Ca3(PO4)2

a)

ionic bond

b)

covalent bond

c)

metallic bond

d)

cannot be determined

38.

NaCl

a)

covalent bonding

b)

ionic bonding

c)

hydrogen bonding

d)

metallic bond

39.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Polar Covalent
c)
Metallic
d)
Nonpolar Covalent
40.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

41.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

42.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

43.

When you have Be-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

44.

When you have Si-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

45.

When you have F-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

46.

When you have C-H, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

47.

When you have Zn-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

48.

When you have Mn-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

49.

When you have Ga-Se, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

50.

How would the melting point and boiling point for polar covalent bond?

a)

High

b)

Low

51.

How would the melting point and boiling point for nonpolar covalent bond?

a)

High

b)

Low

52.
The force of attraction between nonpolar molecules:
a)
Hydrogen Bonding
b)
Dipole - Dipole Forces
c)
LDF
d)
Ionic Forces
53.

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

54.

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

55.

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

56.

A strong IMF increases

a)

boiling point

b)

solubility

c)

flammability

d)

malleability

57.

A weak IMF will result in a

a)

high melting point

b)

high viscosity

c)

high surface tension

(hard to break apart)

d)

low surface tension (easy to break apart)

58.

What letter on the diagram represents the substance only in the gas phase?

a)

A

b)

B

c)

C

d)

D

59.

What letter on the diagram represents a substance only in the liquid?

a)

A

b)

B

c)

C

d)

D

60.

What letter on the diagram represents a substance only in the solid phase?

a)

A

b)

B

c)

C

d)

D

61.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

62.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
63.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
64.

A molecule is polar when

a)

it is asymmetrical with at least one polar bond

b)

it is symmetrical

c)

it is asymmetrical

d)

it is symmetrical with at least one polar bond

65.

Which of the following would experience dipole-dipole forces of attraction between molecules?

a)
b)
c)
d)
66.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

67.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
68.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
69.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

70.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

71.

List the strongest to weakest IMFs.

a)

Hydrogen Bond, London Dispersion, Dipole-dipole

b)

London Dispersion, Dipole-dipole,

Hydrogen Bond

c)

Hydrogen Bond, Dipole-dipole, London Dispersion

d)

Dipole-dipole, Hydrogen Bond, London Dispersion

72.

A strong IMF increases

a)

boiling point

b)

solubility

c)

flammability

d)

malleability

73.

A weak IMF will result in a

a)

high melting point

b)

high viscosity

c)

high surface tension

d)

low surface tension

74.

Which substance in the table below has the strongest intermolecular forces?

a)

HF

b)

HCl

c)

HBr

d)

HI

75.

Which statement explains why Br2 is a liquid at STP and I2 is a solid at STP?

a)

Molecules of Br2 are polar, and molecules of I2 are nonpolar.

b)

Molecules of I2 are polar, and molecules of Br2 are nonpolar.

c)

Molecules of Br2 have stronger intermolecular forces than molecules of I2.

d)

Molecules of I2 have stronger intermolecular forces than molecules of Br2.

76.

A molecule of HCl contains polar covalent bonds and displays dipole-dipole interactions when it encounters other HCl molecules. Which of these two forces is stronger?

a)

Polar covalent, because it is an intermolecular force.

b)

Polar covalent, because it is an intramolecular force.

c)

Dipole-dipole, because it is an intermolecular force.

d)

Dipole-dipole, because it is an intramolecular force.

77.

If a substance has a high boiling point, this indicates that the substance has ____________ IMFs.

a)

Weak

b)

Moderate

c)

Strong

78.

Which of the following does NOT experience hydrogen bonding?

a)

HF

b)

HI

c)

NH3

d)

H2O

79.

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.

80.

Which one has higher melting point, CO2 or NH3?

a)

CO2

b)

NH3

81.

Which statement is true?

a)

IMFs occur within molecules, and one example is hydrogen bonding.

b)

IMFs occur between molecules, and one example is ionic bonding.

c)

IMFs occur within molecules, and one example is Van der Waal's forces.

d)

IMFs occur between molecules, and one example is dipole-dipole interaction.

82.

How many TOTAL electron domains are around the C on the left?

a)

1

b)

2

c)

3

d)

4

83.

What type of electron domains are around the N in the middle?

a)

2 bonding, 0 non-bonding

b)

0 bonding, 2 non-bonding

c)

4 bonding, 0 non-bonding

d)

0 bonding, 4 non-bonding

84.

What type of electron domains are around the C on the left?

a)

3 bonding, 0 non-bonding

b)

4 bonding, 0 non-bonding

c)

0 bonding, 3 non-bonding

d)

0 bonding, 4 non-bonding

85.

How many TOTAL electron domains are around the middle oxygen?

a)

2

b)

3

c)

4

d)

5

86.

What type of electron domains are around the middle oxygen?

a)

2 bonding, 1 non-bonding

b)

3 bonding, 1 non-bonding

c)

3 bonding, 2 non-bonding

d)

1 bonding, 2 non-bonding

87.

How many TOTAL electron domains are around the S in the midde?

a)

2

b)

3

c)

4

d)

5

88.

What type of electron domains are around the S in the midde?

a)

3 bonding, 1 non-bonding

b)

3 bonding, 2 non-bonding

c)

2 bonding, 3 non-bonding

d)

1 bonding, 3 non-bonding

89.

What type of electron domains are around one of the oxygen atoms on the left (either one...they are the same)?

a)

2 bonding, 2 non-bonding

b)

1 bonding, 3 non-bonding

c)

2 bonding, 4 non-bonding

d)

4 bonding, 2 non-bonding

90.

What type of electron domains are around the N?

a)

2 bonding, 1 non-bonding

b)

3 bonding, 1 non-bonding

c)

3 bonding, 2 non-bonding

d)

2 bonding, 3 non-bonding

91.

How many valence electrons does Hydrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

92.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

93.

How many valence electrons does Magnesium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

94.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

95.

How many valence electrons does Potassium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

96.

How many valence electrons does Silicon Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

97.

How many valence electrons does Phosphorus Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

98.

How many valence electrons does Boron Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

99.

How many valence electrons does Neon Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

100.

How many valence electrons does Fluorine Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

101.

According to the Octet Rule, atoms want ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

102.

When atoms LOSE electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

103.

What does Neon need to do fulfill the Octet Rule?

a)

Gain 2

b)

Lose 2

c)

Nothing - it already fulfills the Octet Rule.

104.

When atoms GAIN electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

105.

Which 2 atoms are EXCEPTIONS to the Octet Rule and only need 2 valence electrons?

a)

H, Na

b)

H, He

c)

He, Ne

d)

There are no exceptions to the Octet Rule

106.

When anions and cations join together, what kind of bond is formed?

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

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