Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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A
mutual electrical attraction between the nuclei and valence electrons of different atoms that binds
the atoms together is called a(n) a. | dipole. | c. | chemical bond. | b. | Lewis
structure. | d. | London
force. | | | | |
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2.
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A
chemical bond resulting from the electrostatic attraction between positive and negative ions is
called a(n) a. | covalent
bond. | c. | charged
bond. | b. | ionic bond. | d. | dipole bond. | | | | |
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3.
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If
two covalently bonded atoms are identical, the bond is a. | nonpolar
covalent. | c. | nonionic. | b. | polar covalent. | d. | coordinate covalent. | | | | |
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4.
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Purely ionic bonds do not occur because the atom that gives up an electron in such a
bond a. | is not an
ion. | b. | still has some
attraction for the electron. | c. | has a negative charge. | d. | shares the
electron equally with the other atom in the bond. | | |
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5.
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The
B—F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0)
is a. | polar
covalent. | c. | nonpolar
covalent. | b. | ionic. | d. | pure covalent. | | | | |
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6.
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In
which of these compounds is the bond between the atoms NOT a nonpolar covalent bond?
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7.
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Which
of the following is NOT an example of a molecular formula?
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8.
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How
many extra electrons are in the Lewis structure of the phosphate ion,
PO43–?
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9.
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What
is the Lewis structure for carbon tetraiodide, which contains one carbon atom and four iodine
atoms?
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10.
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Bonding in molecules or ions that cannot be correctly represented by a single Lewis
structure is a. | covalent
bonding. | c. | single
bonding. | b. | resonance. | d. | double bonding. | | | | |
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11.
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The
ions in an ionic compound are organized into a(n) a. | molecule. | c. | polyatomic ion. | b. | Lewis
structure. | d. | crystal. | | | | |
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12.
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Which
of the following is NOT a property of an ionic compound? a. | low boiling
point | c. | hardness | b. | brittleness | d. | molten compound conducts electricity | | | | |
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13.
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In
metals, the valence electrons a. | are attached to particular positive
ions. | c. | are
immobile. | b. | are shared by all of the atoms. | d. | form covalent bonds. | | | | |
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14.
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Metals are malleable because the metallic bonding a. | holds the layers
of ions in rigid positions. | b. | does not produce ions. | c. | allows one plane
of ions to slide past another. | d. | is easily broken. | | |
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15.
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According to VSEPR theory, the electrostatic repulsion between electron pairs
surrounding an atom causes a. | an electron sea to form. | b. | positive ions to
form. | c. | these pairs to be separated as far as
possible. | d. | light to reflect. | | |
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16.
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Use
VSEPR theory to predict the shape of the carbon tetraiodide molecule,
CI4. a. | tetrahedral | c. | bent | b. | linear | d. | trigonal planar | | | | |
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17.
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Use
VSEPR theory to predict the shape of the chlorate ion,
ClO3–. a. | trigonal planar | c. | trigonal pyramidal | b. | octahedral | d. | bent | | | | |
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18.
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Use
VSEPR theory to predict the shape of the hydrogen sulfide molecule, H2S. a. | tetrahedral | c. | bent | b. | linear | d. | octahedral | | | | |
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19.
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Use
VSEPR theory to predict the shape of carbon dioxide, CO2. a. | tetrahedral | c. | bent | b. | linear | d. | octahedral | | | | |
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20.
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Dipole-dipole forces are considered the most important forces in polar substances
because the London dispersion forces a. | act only in nonpolar substances. | b. | are usually much
weaker than the dipole-dipole forces. | c. | are too unpredictable. | d. | act only in
solids. | | |
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21.
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The
strength of London dispersion forces between molecules depends on a. | only the number
of electrons in the molecule. | b. | only the number of protons in the
molecule. | c. | both the number of electrons in the molecule and the mass of
the molecule. | d. | both the number of electrons and the number of neutrons in the
molecule. | | |
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22.
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Compared with molecular bonds, the strength of intermolecular forces
is a. | weaker. | c. | about the
same. | b. | stronger. | d. | too variable to compare. | | | | |
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23.
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That
the boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide
(H2S) is partially explained by a. | London forces. | c. | ionic bonding. | b. | covalent
bonding. | d. | hydrogen
bonding. | | | | |
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24.
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The
following molecules contain polar bonds. The only polar molecule is a. | CCl4. | c. | NH3. | b. | CO2. | d. | CH4. | | | | |
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25.
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Choose the species that is incorrectly matched with the electronic
geometry about the central atom.
a. |
Molecule Electronic
Geometry
H2O
tetrahedral
| c. |
Molecule Electronic
Geometry
CF4
tetrahedral
| b. | Molecule
Electronic Geometry
BeBr2
linear
| d. |
Molecule Electronic
Geometry
PF3
pyramidal | | | | |
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Short Answer
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26.
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Describe the
force referred to as London force
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27.
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Draw
the Lewis structures of the following molecules; name the shape of the molecule (not of the
electrons) and state whether the molecule is polar or non-polar.
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