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Covalent Bonding Test Review

Total questions: 108

Worksheet time: 2hrs 43mins

Name
Class
Date
1.

How are atoms held together in covalent bonds?

a)

By gaining and losing electrons

b)

By sharing electrons

2.

Which of the following has the highest melting point?

a)

O2

b)

F2

c)

Na2O

d)

CCl4

3.

In forming covalent bonds, why do atoms share electrons?

a)

To achieve noble-gas notation

b)

To become charged

c)

To form ions

4.

If the bond between two atoms has the electronegativity difference of 0.4, what type of bond do the atoms have?

a)

Ionic

b)

Polar Covalent

c)

Non-polar covalent

5.

What types of elements combine to form ionic bonds?

a)

Metals and metalloids

b)

Metals and non metals

c)

Non metals only

d)

Metalloids only

e)

Metals only

6.

When diatomic fluorine creates a molecule, what type of bond is used? (Hint, you may have to draw the Lewis structure)

a)

Single bond

b)

Double bond

c)

Triple bond

7.

What are atoms used to complete an octet but not used in bonding called?

a)

Shared pair

b)

Lone pair

c)

Bonded pair

d)

unshared pair

8.

Which of the following is NOT one of the seven diatomic molecules?

a)

Hydrogen

b)

Carbon

c)

Bromine

d)

Iodine

e)

Oxygen

9.

A compound has a boiling point of  8915°C8915\degree C , dissolves in water, and makes an electrolyte.  Which of the following compounds is most likely being described?

a)

Ionic Compound

b)

nonpolar covalent Compound

c)

polar covalend compound

10.

What type of bond will N - H form?

a)

Polar Covalent

b)

Non-polar Covalent

c)

Ionic

11.

If the bond between two atoms has an electronegativity difference of 0.6, what type of bond do the atoms have?

a)

Ionic

b)

Polar Covalent

c)

Non-polar Covalent

12.

Which group has no electronegativity value?

a)

Halogen

b)

Transition Metals

c)

Noble Gases

d)

Alkaline Earth Metals

13.

In a polar covalent bond, electrons are shared ____________ between two atoms.

a)

equally

b)

unequally

14.

Which of the following has the greatest electronegativity?

a)

O

b)

S

c)

Br

d)

Si

15.

How many electrons are shared between two atoms in a double covalent bond?

a)

1

b)

2

c)

4

d)

6

16.

The compound CBr4 has a tetrahedral shape, what is the molecular polarity?

a)

Polar

b)

Nonpolar

17.

If a bond between two atoms has an electronegativity difference of 1.9, we can assume that bond is ________________

a)

Ionic

b)

Polar Covalent

c)

Non Polar Covalent

18.

What is the molecular geometry (shape) of NH3?

a)

Bent

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Linear

19.

What is the correct molecular geometry AND molecular polarity of HCN?

a)

Tetrahedral, nonpolar

b)

Tetrahedral, polar

c)

Bent, polar

d)

Linear, polar

e)

Linear, nonpolar

20.

Which of the following bonds is the most polar?

a)

O-F

b)

N-F

c)

H-F

d)

S-F

21.

When drawing the structure of diatomic oxygen (O2), what type of bond is used?

a)

single

b)

double

c)

triple

d)

quadruple

22.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
23.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
24.
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
25.
How many electrons should Carbon have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
26.
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a)
1
b)
4
c)
3
d)
2
27.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
28.

Which of the following elements will NOT be surrounded by an octet of electrons in a correctly drawn Lewis structure?

a)

carbon

b)

oxygen

c)

chlorine

d)

hydrogen

29.

Which of the following has an ionic bond?

a)

H3N

b)

CaCl2

c)

NO2

d)

SCl

30.
How many valence electrons do elements in Group 2A have?
a)
12
b)
4
c)
1
d)
2
31.
Which is the correct structure for ammonia?
Pictures correspond with a-d.
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D. 
32.

Choose the structure that forms a double bond (draw the Lewis structure).

a)

Carbon monoxide (CO)

b)

Carbon dioxide (CO2)

c)

Water (H2O)

d)

Cyanic Acid (HCN)

33.

Choose the structure that forms a triple bond (remember these exist in diatomic form in nature). (draw the Lewis structures)

a)

Hydrogen

b)

Fluorine

c)

Oxygen

d)

Nitrogen

34.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
35.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
36.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
37.

When drawing a Lewis structure, after drawing in your bonds and lone pairs, what do you do if you don't have enough electrons to get each atom to its octet? (this is for the counting method I showed later)

a)

Place dots until everything has eight

b)

Place dots only around the terminal atoms

c)

Add a multiple bond

d)

Have eight only around the central atom

38.
In a Lewis structure, what do you do  with the total number of valence if your ion is + charged?
a)
Divide the valence number by 1
b)
Multiply the valence number by 1
c)
Add 1 to the valence number
d)
Subtract 1 from the valence number
39.

How many covalent bonds does carbon need to form in order to have a full octet?

a)

2

b)

3

c)

4

d)

5

40.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
41.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

42.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

43.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

44.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
45.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
46.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
47.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
48.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
49.

Will this molecule be polar or nonpolar? H2S

a)

polar

b)

nonpolar

50.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
51.

What is the molecular geometry for this molecule?

a)

Bent

b)

Trigonal pyramidal

c)

Trigonal planar

d)

Linear

52.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
53.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

54.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

55.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

56.

In a nonpolar covalent bond, the electrons spread around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

57.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

58.

Molecules that contain whole number charges on atoms (+1,-3, etc.) must be...

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

d)

Polar Covalent or Ionic

59.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that attracts electrons less

b)

The atom with the greater electronegitivity

c)

The atom that attracts more electrons

d)

The atom with the lower electronegativity

60.

What must be the approximate difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less or equal to 0.4

b)

greater than 1.8

c)

greater than 0.4 and less than 2.0

d)

exactly 0

61.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

62.
Which molecule contains bonds of GREATER polarity?
a)
H2O
b)
OF2
63.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
64.

A bond with a partially negative end and a partially positive end is:

a)

ionic

b)

polar

c)

non-polar

d)

called a dipole

65.

A diatomic molecule like O2 is always_______ because electrons are shared ________.

a)

nonpolar; equally

b)

polar; equally

c)

nonpolar; unequally

d)

nonpolar; unequally

66.
If Bromine bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
67.
When you are asked to find bond polarity, compare EN values of each bonding atom to the central atom
a)
true
b)
false
68.

The electronegativity difference in the bonds of CH4 (methane) is:

a)

0.4

b)

5.9

c)

-0.4

d)

1.7

69.

The electronegativity difference in the bonds of CCl4 (carbon tetrachloride) is:

a)

0.4

b)

0.5

c)

9.5

d)

5.5

70.
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
71.

According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?

a)

groups of valence electrons

b)

Inner shell electrons

c)

Mobile Electrons

d)

Electrons closest to the nucleus

72.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

73.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

74.

Use your knowledge and electronegativity sheet to predict what type of bond would form between calcium and bromine.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

75.

Use your knowledge and electronegativity sheet to predict what type of bond would form between phosphorus and fluorine.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

76.

What causes a partial charge on a molecule?

a)

unequal sharing of electrons

b)

an electronegativity difference between 0.4 and 1.8.

c)

the shape of the molecule

d)

all of the above

77.

Which of the following types of compounds will likely dissolve in water, since it is polar?

a)

ionic compounds

b)

polar molecules

c)

nonpolar molecules

d)

metallic compounds

78.
Polarity of a molecule is determined by
a)
shape and charge
b)
shape and difference in EN value
c)
difference in EN value and size
d)
difference in EN value and charges
79.
CCl4 has polar bonds but is a non polar molecule. Why?
a)
bond polarity exist between atoms
b)
bond polarity between atoms cancel
c)
dipole moment exist between atoms in molecule
d)
difference in EN between C and Cl
80.
Which of the following is FALSE about intermolecular forces between molecules?
a)
It is also called London or Van Der Waals forces
b)
Dipole dipole attraction between molecule
c)
Also due to instantaneous dipole attraction between molecule
d)
Must have permanent dipole moment before it can exist
81.
The following statement is true for hydrogen bonding EXCEPT
a)
It is a dipole dipole forces of attraction
b)
Electronegative element like N, O and F must be present
c)
Hydogen bonding is stronger than covalent bonding
d)
ESF attraction bet H atom with lone pair electron from N,O,F
82.

The following are requirement for hydrogen bonding EXCEPT

a)

H atom bonded to electronegative N, O and F

b)

Electronegative element like N, O and F must be present

c)

H atom bonded with lone pair electrons from any Gp 7 element

d)

Attraction between H atom with lone pair electron from N,O,F

83.

Arrange the boiling point of molecules from lowest to highest.

a)

lowest H2 - N2 - H2O - CI2 highest

b)

lowest H2 - H2O - N2 - CI2 highest

c)

lowest H2 - N2 - CI2 - H2O highest

d)

lowest H2O - N2 - H2 - CI2 highest

84.

Arrange the boiling point for molecules (RMM given) from lowest to highest.

a)

lowest A - B - C- D highest

b)

lowest A - C - B - D highest

c)

lowest D - A - B - C highest

d)

lowest D - A - C - B highest

85.
Why BCI3 is non polar while NCI3 is polar?
a)
BCI3 is symmetrical and bond polarity exist
b)
BCI3 does not have polar bonds, while NCI3 does
c)
BCI3 is asymmetrical and bond polarity exist
d)
BCI3 is symmetrical and bond polarity cancel
86.
Does H2O have hydrogen bonding?
a)
yes
b)
no
87.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

88.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

LDF

c)

Hydrogen Bonds

89.

Intermolecular forces for: CO2

a)

LDF

b)

Dipole dipole

c)

Hydrogen bonding

90.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
91.
What explains the very high melting and boiling point of water?
a)
Dipole-dipole forces between water molecules
b)
Hydrogen bonds between water molecules
c)
London dispersion forces between water molecules
d)
Molecule-ion attractions between water molecules
92.
In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces
a)
Higher
b)
Lower
c)
The same
93.

Which of the following molecules would have the lowest boiling point?

a)

CH4

b)

C2H6

c)

C3H8

d)

C4H10

94.

HCl and F2 both have a molecular mass of approximately 36 g/mol. Based on IMF, which will have a lower boiling point?

a)

HCl

b)

F2

95.

Which of these has the strongest London forces?

a)

F2

b)

Br2

c)

Cl2

d)

I2

96.
a)

Polar covalent bond

b)

Nonpolar covalent bond

c)

Hydrogen bond

d)

London dispersion forces

97.
a)

C4H10, because it has more H atoms, resulting in more H-bonding

b)

C4H10, because it has more electrons, resulting in greater polarizability and stronger LDFs

c)

C2H6, because its molecules are smaller and they can get closer to each other, resulting in stronger LDFs

d)

C2H6, because its molecules are more polar, resulting in stronger dipole-dipole attractions

98.
Rank the IM forces from strongest to weakest.
a)
dipole, hydrogen bonding, dispersion
b)
dispersion, dipole, hydrogen bonding
c)
hydrogen bonding, dipole, dispersion
d)
hydrogen bonding, dispersion, dipole
99.

Which of the following will take the longest to evaporate?

a)

CH3CH2OH

b)

CH3OH

c)

CH3CH3

100.
Which type of solid is hard, brittle, and nonconducting unless dissolved in H2O?
a)
Ionic Crystal
b)
Covalent Molecular Crystal
c)
Metallic Crystal
d)
Covalent Network Crystal
101.

Which molecule will exhibit resonance?

a)

SO2

b)

CO2

c)

NH3

d)

CCl4

102.

When both shared electrons originate from only one atom, it is called a/an

a)

ionic bond

b)

London covalent bond

c)

coordinate covalent bond

d)

resonance bond

103.

A polar covalent bond is an example of an ____________ force while a hydrogen bond is an example of ________________ force.

a)

intermolecular/intramolecular

b)

intermolecular/intermolecular

c)

intramolecular/ionic

d)

intramolecular/intermolecular

104.

The intermolecular force that holds DNA strands together and helps determine the folded structure of proteins is

a)

dipole-dipole forces

b)

London dispersion forces

c)

H-bonds

d)

ionic forces

105.

We tend to draw the extreme resonance solutions for Lewis structures but in reality a _______________________ exists in which the double bond electrons are delocalized over the entire molecule.

a)

resonance isomer

b)

resonance hybrid

c)

ionic hybrid

d)

dipole isomer

106.

All molecules and atoms will have London Forces occur between them.

a)

True

b)

False

107.

Molecules have to have permanent polarity in order to experience dipole-dipole forces between them.

a)

True

b)

False

108.

When you boil a molecular substance, you are interrupting

a)

only intramolecular forces

b)

only intermolecular forces

c)

both intermolecular and intramolecular forces

d)

neither intermolecular nor intramolecular forces

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