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Advanced Chem Covalent Bonding and Intermolecular Forces Review

Total questions: 84

Worksheet time: 2hrs 37mins

Name
Class
Date
1.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
2.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
3.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
4.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
5.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
6.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
7.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
8.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
9.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
10.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

11.
A molecule with a lone pair on the central atom would have the same electron and molecular geometry
a)
True
b)
False
12.

Is this molecule polar?

a)

No

b)

Yes

13.

What is the molecular shape of ICl3 ? (You have to draw this)

a)

T Shaped

b)

See Saw

c)

Octahedral

d)

Trigonal Bipyramidal

14.

What is the molecular shape of SeH4 ? (You have to draw this)

a)

T Shaped

b)

See Saw

c)

Octahedral

d)

Trigonal Bipyramidal

15.

What type of bond is formed when atoms share two pairs of electrons?

a)

Coordinate covalent bond

b)

Triple covalent bond

c)

Single covalent bond

d)

Double covalent bond

16.
What is the best explanation of VSEPR theory?
a)
It explains the shapes that electrons make around atoms when they repel
b)
It explains how many electrons fit into an element's valent shell
c)
It explains why electrons pair up
d)
It explains why electrons repel each other
17.

By looking at the chart, determine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .

a)

eg = tetrahedral, mg = tetrahedral

b)

eg = linear, mg = linear

c)

eg = octahedral, mg = square planar

d)

eg = trigonal bipyramidal, mg = tetrahedral

18.
Name CCl4
a)
carbon carbon tetraiodide
b)
carbon tetrachloride
c)
monocarbon tetrachloride
d)
water
19.
Give the formula for oxygen dichloride
a)
OCl2
b)

O2Cl2

c)
OCl
d)
O2Cl
20.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
21.

Which of the following is NOT formed by a covalent bond?

a)

K2S

b)

H2O

c)

I2

d)

CO2

22.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
23.
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
24.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
25.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
26.

Which sample has hydrogen bonding?

a)

H2S

b)

CH4

c)

NH3

d)

HI

27.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

28.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

29.

Can NEVER conduct electricity

a)

ionic

b)

covalent

c)

metallic

30.

Ammonia, NH3, adopts a tetrahedral geometry. However, the non-bonding pair on the central nitrogen atom distorts the bond angle away from the expected 109.5°. Which of the following statements correctly describes how the bond angle is distorted?

a)

The actual bond angle is reduced: it is less than 109.5°

b)

The actual bond angle is increased: it is more than 109.5°

31.

Apply the VSEPR model to XeF4. Which of the following molecular shapes is consistent with the model?

a)

Disphenoidal

b)

Square planar

c)

Tetrahedral

d)

Square pyramidal

32.

Choose the molecule that is incorrectly matched with the electronic geometry about the central atom.

a)

CF4 - tetrahedral

b)

BeBr2 - linear

c)

H2O - tetrahedral

d)

PF3 - pyramidal

33.
Bromine monofluoride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
34.
Weak Bonds
a)
Ionic
b)
Covalent
35.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
36.
What molecular shape is this? 
a)
Trigonal Planar
b)
Trigonal Bipyramidal
c)
Tetrahedral
d)
Pyramidal
37.
Which of the following describes water?
a)
Linear structure, nonpolar
b)
Linear structure, polar
c)
Bent structure, nonpolar
d)
Bent structure, polar
38.
Will this molecule be polar or nonpolar? CCl4
a)
polar
b)
nonpolar
39.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
40.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
41.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
42.

What is the difference between a polar and nonpolar covalent bond?

a)

The difference lies in the formation of ionic bonds.

b)

The difference lies in the equal sharing of electrons.

c)

The difference lies in the unequal sharing of electrons.

d)

The difference lies in the transfer of electrons.

43.

What are intermolecular forces?

a)

Forces that exist within a molecule

b)

Forces that exist between molecules

c)

Forces that exist between atoms within a molecule

d)

Forces that exist between ions

44.

What is a dipole?

a)

A) A molecule with a single charge.

b)

B) A molecule with no charge.

c)

C) A molecule with two poles, one positive and one negative.

d)

D) A molecule with multiple charges.

45.

What type of intermolecular force exists between polar molecules due to the uneven sharing of electrons?

a)

London dispersion forces

b)

Hydrogen bonding

c)

Dipole-dipole interactions

d)

Ionic bonding

46.

What type of bond is described as a strong dipole-dipole interaction formed when hydrogen is bonded to oxygen, nitrogen, or fluorine?

a)

Covalent bond

b)

Ionic bond

c)

Hydrogen bond

d)

Metallic bond

47.

Which of the following elements can form a hydrogen bond with hydrogen?

a)

Carbon

b)

Sulfur

c)

Oxygen

d)

Chlorine

48.

What does a diatomic molecule contain?

a)

1 atom

b)

2 atoms

c)

3 atoms

d)

4 atoms

49.

Which of the following is an example of a diatomic molecule?

a)

H2O

b)

CO2

c)

O2

d)

CH4

50.

How many of the following molecules are polar?

BH3 CH4 H2O HF H2

a)

1

b)

2

c)

3

d)

4

e)

5

51.

Which molecule has a Dipole?

a)
b)
c)
d)
52.

What type of bond in shown in this picture?

a)

Non-Polar Covalent

b)

Polar Covalent

c)

Ionic

d)

Metallic

53.

What type of bond in shown in this picture?

a)

Non-Polar Covalent

b)

Polar Covalent

c)

Ionic

d)

Metallic

54.

What type of bond in shown in this picture?

a)

Non-Polar Covalent

b)

Polar Covalent

c)

Ionic

d)

Metallic

55.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
56.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
57.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
58.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
59.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
60.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
61.
Intermolecular force present in Cl2?
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
62.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

63.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

64.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

65.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
66.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

67.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

68.

How much Ce2(SO4)3 solute is saturated at 80 degrees?

a)

20

b)

15

c)

30

d)

2

69.

How much NaBr solute is saturated at 70 degrees?

a)

110

b)

120

c)

130

d)

140

70.

Which solute is MOST likely a gas?

a)

KNO3

b)

NaNO3

c)

KCl

d)

Ce2(SO4)3

71.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

72.

What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

73.

What type of a solution is 100g KNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

74.

What type of a solution is 260g sugar at 50ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

75.

What type of a solution is 25g NaCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

76.

What type of a solution is 55g KCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

77.

At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?

a)

60 ºC

b)

30 ºC

c)

50 ºC

d)

83 ºC

78.

25 grams of NaCl are dissolved in 100 mL of water at 60 C. How many more grams need to be dissolved for the solution to be saturated?

a)

13 grams

b)

25 grams

c)

6 grams

d)

38 grams

79.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
80.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
81.
Which of these solutes does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
82.
What conclusion can be made using this solubility curve?
a)
Decreasing temperatures always increases solubility 
b)
Increasing temperatures always increases solubility
c)
Increasing temperatures usually increases solubility
d)
Temperature has no affect on solubility
83.

The substance that does the dissolving

a)

Solute

b)

Solvent

c)

Solution

d)

Miscibility

84.

Which of the following will allow for more solute than normal to be dissolved in a solvent?

a)

freezing the solution

b)

shaking the solute

c)

cooling the solution

d)

heating the solution

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