Unit 6 Review
Question 1

How many valence electrons does
sulfur have?
a. 1
b. 2
c. 6
d. 16
Question 1

How many valence electrons does
sulfur have?
a. 1
b. 2
c. 6
d. 16
Question 2

How many fluorine atoms can form
covalent bonds with one silicon atom?
a. 1
b. 2
c. 3
d. 4
Question 2

How many fluorine atoms can form
covalent bonds with one silicon atom?
a. 1
b. 2
c. 3
d. 4
Question 3

Why do atoms share electrons in covalent
bonds?
a. To become ions and attract each other
b. To attain a noble-gas electron
configuration
c. To become more polar
d. To increase their atomic numbers
Question 3

Why do atoms share electrons in covalent
bonds?
a. To become ions and attract each other
b. To attain a noble-gas electron
configuration
c. To become more polar
d. To increase their atomic numbers
Question 4

Covalent molecular compounds are usually
_____________.
a. Composed of two or more transition
metals
b. Composed of positive and negative ions
c. Composed of two or more nonmetals
d. Exceptions to the law of conservation of
mass
Question 4

Covalent molecular compounds are usually
_____________.
a. Composed of two or more transition
metals
b. Composed of positive and negative ions
c. Composed of two or more nonmetals
d. Exceptions to the law of conservation of
mass
Question 5

What is the name for N2H4?
a. Dinitrogen tetrahydride
b. Nitrogen hydride
c. Mononitrogen dihydride
d. Pentahydride dinitride
Question 5

What is the name for N2H4?
a. Dinitrogen tetrahydride
b. Nitrogen hydride
c. Mononitrogen dihydride
d. Pentahydride dinitride
Question 6

How many valence electrons does
chlorine have?
a. 1
b. 2
c. 7
d. 8
Question 6

How many valence electrons does
chlorine have?
a. 1
b. 2
c. 7
d. 8
Question 7

How many pairs of electrons must two
nitrogen atoms share in order for each atom
to have eight valence electrons?
a. Zero
b. One
c. Two
d. Three
Question 7

How many pairs of electrons must two
nitrogen atoms share in order for each atom
to have eight valence electrons?
a. Zero
b. One
c. Two
d. Three
Question 8

Which of the following molecules
contain polar covalent bonds?
a. Phosphorus, P4
b. Ozone, O3
c. Oxygen, O2
d. Hydrogen Fluoride, HF
Question 8

Which of the following molecules
contain polar covalent bonds?
a. Phosphorus, P4
b. Ozone, O3
c. Oxygen, O2
d. Hydrogen Fluoride, HF
Question 9

Which of the following molecules
contain nonpolar covalent bonds?
a. Cl2
b.CCl4
c. SiBr4
d.H2O
Question 9

Which of the following molecules
contain nonpolar covalent bonds?
a. Cl2
b.CCl4
c. SiBr4
d.H2O
Question 10

What is the formula for
diphosphorous pentoxide?
a. P2O5
b.P5O2
c. P3O2
d. P2O3
Question 10

What is the formula for
diphosphorous pentoxide?
a. P2O5
b.P5O2
c. P3O2
d. P2O3
Question 11

Which type of covalent bond is found
in Carbon Monoxide?
a. Single bond
b. Double bond
c. Triple bond
d. Not enough information
Question 11

Which type of covalent bond is found
in Carbon Monoxide?
a. Single bond
b. Double bond
c. Triple bond
d. Not enough information
Question 12

How many electrons are being
shared in carbon monoxide?
a. 1
b.2
c. 3
d.6
Question 12

How many electrons are being
shared in carbon monoxide?
a. 1
b.2
c. 3
d.6
Question 13

What is a property of covalent
molecules?
a. Low melting point
b. Only exists as a solid at room
temperature
c. Malleability
d. Brittle (easy to break)
Question 13

What is a property of covalent
molecules?
a. Low melting point
b. Only exists as a solid at room
temperature
c. Malleability
d. Brittle (easy to break)
Question 14

Which of the following correctly shows a
prefix used in naming molecular compounds
with its corresponding number?
a. hexa-, 8
b. octa-, 4
c. deca-, 7
d. nona-, 9
Question 14

Which of the following correctly shows a
prefix used in naming molecular compounds
with its corresponding number?
a. hexa-, 8
b. octa-, 4
c. deca-, 7
d. nona-, 9
Question 15

Which of the following formulas
represents a covalent molecular
compound?
a. ZnO
b. Xe
c. SO
d. BeF
Question 15

Which of the following formulas
represents a covalent molecular
compound?
a. ZnO
b. Xe
c. SO
d. BeF
Question 16

What is the molecular formula for
the following structure?
a. OH
b.HO2
c. H2O
d.HO
Question 16

What is the molecular formula for
the following structure?
a. OH
b.HO2
c. H2O
d.HO
Question 17

What is the formula for sulfur
hexachloride?
a. SCl6
b.S6Cl
c. SCl2
d.S2Cl
Question 17

What is the formula for sulfur
hexachloride?
a. SCl6
b.S6Cl
c. SCl2
d.S2Cl
Question 18

When atoms form a polar covalent bond, the
atom with the greater attraction for electrons
has a partial ________________ charge.
a. Positive
b. Negative
c. Neutral
d. Not enough information
Question 18

When atoms form a polar covalent bond, the
atom with the greater attraction for electrons
has a partial ________________ charge.
a. Positive
b. Negative
c. Neutral
d. Not enough information
Question 19

Polarity is determined by
___________________.
a. Atomic Number
b. Atomic Radius
c. Electronegativity
d. Atomic Mass
Question 19

Polarity is determined by
___________________.
a. Atomic Number
b. Atomic Radius
c. Electronegativity
d. Atomic Mass
Question 20

What is the name of NO?
a. Nitrogen oxide
b.Mononitrogen oxide
c. Mononitrogen monoxide
d.Nitrogen monoxide
Question 20

What is the name of NO?
a. Nitrogen oxide
b.Mononitrogen oxide
c. Mononitrogen monoxide
d.Nitrogen monoxide
Question 21

What do the two dots between the “N” and
“H” represent?
a. Bonded pairs of electrons
b. Lone pairs of electron
c. Ionic bonds
d. Not enough information
Question 21

What do the two dots between the “N” and
“H” represent?
a. Bonded pairs of electrons
b. Lone pairs of electron
c. Ionic bonds
d. Not enough information
Question 22

What is the formula for tetraphosphorus
hexoxide?
a. P6O4
b. P5O7
c. P4O6
d. P3O7
Question 22

What is the formula for tetraphosphorus
hexoxide?
a. P6O4
b. P5O7
c. P4O6
d. P3O7
Question 23

What is the electronegativity of an
atom?
a. Ability to attract electrons
b.Ability to attract neutrons
c. Ability to repel electrons
d. Ability to attract protons
Question 23

What is the electronegativity of an
atom?
a. Ability to attract electrons
b.Ability to attract neutrons
c. Ability to repel electrons
d. Ability to attract protons
Question 24

What element on the periodic table
has the highest electronegativity?
a. Francium
b.Oxygen
c. Bromine
d.Fluorine
Question 24

What element on the periodic table
has the highest electronegativity?
a. Francium
b.Oxygen
c. Bromine
d.Fluorine
Question 25

Which is more polar: a carbon-oxygen bond or a
carbon-nitrogen bond?
a. Carbon-oxygen bond because it has a lower
electronegativity difference.
b. Carbon-nitrogen bond because it has a lower
electronegativity difference.
c. Carbon-oxygen bond because it has a higher
electronegativity difference.
d. Carbon-nitrogen bond because it has a higher
electronegativity difference.
Question 25

Which is more polar: a carbon-oxygen bond or a
carbon-nitrogen bond?
a. Carbon-oxygen bond because it has a lower
electronegativity difference.
b. Carbon-nitrogen bond because it has a lower
electronegativity difference.
c. Carbon-oxygen bond because it has a higher
electronegativity difference.
d. Carbon-nitrogen bond because it has a higher
electronegativity difference.
Question 26

What is the name of S2O3?
a. Sulfur trioxide
b.Disulfur trioxide
c. Sulfur oxide
d.Trisulfur dioxide
Question 26

What is the name of S2O3?
a. Sulfur trioxide
b.Disulfur trioxide
c. Sulfur oxide
d.Trisulfur dioxide
Question 27

Which atom carries the negative partial
charge (-δ) in Br-F?
a. Bromine
b. Fluorine
c. They are equal
d. Not enough information
Question 27

Which atom carries the negative partial
charge (-δ) in Br-F?
a. Bromine
b. Fluorine
c. They are equal
d. Not enough information
Question 28

Which pair of elements listed below
is likely to form a covalent bond?
a. Lithium and oxygen
b.Sodium and copper
c. Calcium and neon
d. Sulfur and chlorine
Question 28

Which pair of elements listed below
is likely to form a covalent bond?
a. Lithium and oxygen
b.Sodium and copper
c. Calcium and neon
d. Sulfur and chlorine
Question 29

What is the name for the H2O?
a. Dihydrogen monoxide
b.Hydrogen dioxide
c. Hydrogen oxide
d.Dihydrogen oxide
Question 29

What is the name for the H2O?
a. Dihydrogen monoxide
b.Hydrogen dioxide
c. Hydrogen oxide
d.Dihydrogen oxide
Question 30

What is the name of IF7?
a.Heptaiodine fluoride
b.Heptaiodine monofluoride
c. Iodine heptafluoride
d.Monoiodine heptafluoride
Question 30

What is the name of IF7?
a.Heptaiodine fluoride
b.Heptaiodine monofluoride
c. Iodine heptafluoride
d.Monoiodine heptafluoride
Question 31

How many hydrogen atoms does it take
for the carbon atom to form a stable
octet?
a. 1
b. 2
c. 3
d. 4
Question 31

How many hydrogen atoms does it take
for the carbon atom to form a stable
octet?
a. 1
b. 2
c. 3
d. 4
Question 32

The bonds between carbon and oxygen
atoms shown in the figure below would
be best classified as:
a. Nonpolar covalent bonds
b. Polar covalent bonds
c. Ionic bonds
d. Metallic bonds
Question 32

The bonds between carbon and oxygen
atoms shown in the figure below would
be best classified as:
a. Nonpolar covalent bonds
b. Polar covalent bonds
c. Ionic bonds
d. Metallic bonds
Question 33

For the diatomic molecule Cl2, how many
electrons does each chlorine atom
contribute to the sharing?
a. 1
b. 2
c. 3
d. 4
Question 33

For the diatomic molecule Cl2, how many
electrons does each chlorine atom
contribute to the sharing?
a. 1
b. 2
c. 3
d. 4
Question 34

What is the formula for carbon
monoxide?
a. CO
b.CO2
c. C2O
d.C2O4
Question 34

What is the formula for carbon
monoxide?
a. CO
b.CO2
c. C2O
d.C2O4
Question 35

How many total electrons are shared
between two oxygen atoms in a covalent
double bond?
a. 2
b. 4
c. 6
d. 8
Question 35

How many total electrons are shared
between two oxygen atoms in a covalent
double bond?
a. 2
b. 4
c. 6
d. 8
Question 36

Nitrogen and oxygen can form a covalent
compound. In this example, electrons
are:
a. Lost
b. Gained
c. Shared
d. Unchanged
Question 36

Nitrogen and oxygen can form a covalent
compound. In this example, electrons
are:
a. Lost
b. Gained
c. Shared
d. Unchanged
Question 37

What does this symbol represent?
a. Dipole
b. Electronegativity
c. Nonpolar bond
d. Transfer of electrons
Question 37

What does this symbol represent?
a. Dipole
b. Electronegativity
c. Nonpolar bond
d. Transfer of electrons
Question 38

How many double bonds are in the
molecule SiO2?
a. 0
b.1
c. 2
d.3
Question 38

How many double bonds are in the
molecule SiO2?
a. 0
b.1
c. 2
d.3
Question 39

Water has a higher boiling point than carbon
dioxide because attractions between polar
molecules are _________________ than
attractions between nonpolar molecules.
a. Weaker
b. Stronger
c. The same
d. Not enough information
Question 39

Water has a higher boiling point than carbon
dioxide because attractions between polar
molecules are _________________ than
attractions between nonpolar molecules.
a. Weaker
b. Stronger
c. The same
d. Not enough information
Question 40

Which atom carries the positive partial
charge (+δ) in H-Cl?
a. Hydrogen
b. Chlorine
c. They are equal
d. Not enough information
Question 40

Which atom carries the positive partial
charge (+δ) in H-Cl?
a. Hydrogen
b. Chlorine
c. They are equal
d. Not enough information
Question 41

Which of the following is an example
of an intramolecular force?
a. Covalent bonding
b.Ionic bonding
c. Hydrogen bonding
d.Both a & b
Question 41

Which of the following is an example
of an intramolecular force?
a. Covalent bonding
b.Ionic bonding
c. Hydrogen bonding
d.Both a & b
Question 42

What is a polar covalent bond?
a. A covalent bond where the protons are shared
equally.
b. A covalent bond where the protons are shared
unequally.
c. A covalent bond where the electrons are shared
equally.
d. A covalent bond where the electrons are shared
unequally.
Question 42

What is a polar covalent bond?
a. A covalent bond where the protons are shared
equally.
b. A covalent bond where the protons are shared
unequally.
c. A covalent bond where the electrons are shared
equally.
d. A covalent bond where the electrons are
shared unequally.
Question 43

Which of the following is not an
example of a diatomic molecule?
a. Hydrogen
b.Sulfur
c. Oxygen
d.Bromine
Question 43

Which of the following is not an
example of a diatomic molecule?
a. Hydrogen
b.Sulfur
c. Oxygen
d.Bromine
Question 44

What is the name given to the pairs of
valence electrons not involved in
bonding?
a. Lone pair
b. Shared pair
c. Bonded pair
d. Paired electrons
Question 44

What is the name given to the pairs of
valence electrons not involved in
bonding?
a. Lone pair
b. Shared pair
c. Bonded pair
d. Paired electrons
Question 45

What forces are between 2 different
molecules?
a. Intramolecular forces
b.Dipole forces
c. Intermolecular forces
d. Bonding forces
Question 45

What forces are between 2 different
molecules?
a. Intramolecular forces
b.Dipole forces
c. Intermolecular forces
d. Bonding forces