Multiple Choice
Identify 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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As independent particles, most atoms are
a. | at relatively high potential energy. | c. | very stable. | b. | at relatively low
potential energy. | d. | part of a
chemical bond. |
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3.
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As atoms bond with each other, they
a. | increase their potential energy, thus creating less-stable arrangements of
matter. | b. | decrease their potential energy, thus creating less-stable arrangements of
matter. | c. | increase their potential energy, thus creating more-stable arrangements of
matter. | d. | decrease their potential energy, thus creating more-stable arrangements of
matter. |
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4.
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If the atoms that share electrons have an unequal attraction for the electrons,
the bond is called
a. | nonpolar. | c. | ionic. | b. | polar. | d. | dipolar. |
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5.
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Nonpolar covalent bonds are not common because
a. | one atom usually attracts electrons more strongly than the other. | b. | ions always form
when atoms join. | c. | the electrons usually remain equally distant from both atoms. | d. | dipoles are rare in
nature. |
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6.
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The greater the electronegativity difference between two bonded atoms, the
greater the percentage of ____ in the bond.
a. | ionic character | c. | metallic character | b. | covalent character | d. | electron
sharing |
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7.
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The pair of elements that forms a bond with the least ionic character is
a. | Na and Cl. | c. | O and Cl. | b. | K and Cl. | d. | Mg and Cl. |
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8.
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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. | metallic. |
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9.
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In the three molecules, O2, HCl, and F2, what atom would
have a partial negative charge?
a. | oxygen | c. | chlorine | b. | hydrogen | d. | fluorine |
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10.
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The percentage ionic character and the type of bond in Br2
(electronegativity for Br is 2.8) is
a. | 0%; nonpolar covalent. | c. | 0%; pure ionic. | b. | 100%; polar covalent. | d. | 100%; pure
ionic. |
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11.
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A neutral group of atoms held together by covalent bonds is a
a. | molecular formula. | c. | polyatomic ion. | b. | chemical formula. | d. | molecule. |
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12.
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Which of the following shows the types and numbers of atoms joined in a single
molecule of a molecular compound?
a. | molecular formula | c. | covalent bond | b. | potential energy diagram | d. | ionic bond |
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13.
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Which of the following is not an example of a molecular formula?
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14.
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The energy released when a covalent bond forms is the difference between zero
and the
a. | maximum potential energy. | c. | minimum potential
energy. | b. | kinetic energy of the atom. | d. | bond length expressed in nanometers. |
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15.
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In a molecule of fluorine, the two shared electrons give each fluorine atom how
many electron(s) in the outer energy level?
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16.
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The electron configuration of nitrogen is 1s2
2s2 2p3. How many more electrons does nitrogen need to satisfy
the octet rule?
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17.
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In drawing a Lewis structure, the central atom is generally the
a. | atom with the greatest mass. | b. | atom with the highest atomic
number. | c. | atom with the fewest electrons. | d. | least electronegative
atom. |
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18.
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To draw a Lewis structure, one must know the
a. | number of valence electrons in each atom. | b. | atomic mass of each
atom. | c. | bond length of each atom. | d. | ionization energy of each
atom. |
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19.
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Multiple covalent bonds may occur in atoms that contain carbon, nitrogen,
or
a. | chlorine. | c. | oxygen. | b. | hydrogen. | d. | helium. |
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20.
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What is the correct Lewis structure for hydrogen chloride, HCl?  
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21.
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Bonding in molecules or ions that cannot be correctly represented by a single
Lewis structure is
a. | polyatomic. | c. | single bonding. | b. | resonance. | d. | double bonding. |
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22.
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In the NaCl crystal, each Na+ and Cl– ion has how
many oppositely charged ions clustered around it?
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23.
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In an ionic compound, the orderly arrangement of ions in a crystal is the state
of
a. | maximum potential energy. | c. | average potential
energy. | b. | minimum potential energy. | d. | zero potential energy. |
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24.
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The ions in most ionic compounds are organized into a
a. | molecule. | c. | polyatomic ion. | b. | Lewis structure. | d. | crystal. |
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25.
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In a crystal, the electrons of adjacent ions
a. | repel each other. | c. | neutralize each other. | b. | attract each
other. | d. | have no effect on
each other. |
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26.
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The energy released when 1 mol of an ionic crystalline compound is formed from
gaseous ions is called the
a. | bond energy. | c. | lattice energy. | b. | potential energy. | d. | energy of
crystallization. |
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27.
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Compared with energies of neutral atoms, a crystal lattice has
a. | higher potential energy. | c. | equal potential
energy. | b. | lower potential energy. | d. | less stability. |
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28.
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Compared with ionic compounds, molecular compounds
a. | have higher boiling points. | c. | have lower melting
points. | b. | are brittle. | d. | are harder. |
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29.
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The forces of attraction between molecules in a molecular compound are
a. | stronger than the forces among formula units in ionic bonding. | b. | weaker than the
forces among formula units in ionic bonding. | c. | approximately equal to the forces among formula
units in ionic bonding. | d. | zero. |
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30.
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The properties of both ionic and molecular compounds are related to the
a. | lattice energies of the compounds. | b. | strengths of attraction between the particles
in the compounds. | c. | number of covalent bonds each
contains. | d. | mobile electrons that they contain. |
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31.
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The Lewis structure for the ammonium ion, NH4, has
a. | nonpolar covalent bond. | c. | polar covalent
bond. | b. | ionic bond. | d. | metallic bond. |
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32.
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How many extra electrons are in the Lewis structure of the phosphate ion,
PO43–?
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33.
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A chemical bond formed by the attraction between positive ions and surrounding
mobile electrons is a(n)
a. | nonpolar covalent bond. | c. | polar covalent
bond. | b. | ionic bond. | d. | metallic bond. |
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34.
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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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35.
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Metals are malleable because the metallic bonding
a. | holds the layers of ions in rigid positions. | b. | maximizes the
repulsive forces within the metal. | c. | allows one plane of ions to slide past
another. | d. | is easily broken. |
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36.
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Malleability and ductility are characteristic of substances with
a. | covalent bonds. | c. | Lewis structures. | b. | ionic bonds. | d. | metallic bonds. |
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37.
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Shifting the layers of an ionic crystal causes the crystal to
a. | be drawn into a wire. | c. | become metallic. | b. | shatter. | d. | emit light. |
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38.
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According to VSEPR theory, an AB2 molecule is
a. | trigonal-planar. | c. | linear. | b. | tetrahedral. | d. | octahedral. |
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39.
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According to VSEPR theory, the shape of an AB3 molecule is
a. | trigonal-planar. | c. | linear. | b. | tetrahedral. | d. | bent. |
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40.
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Use VSEPR theory to predict the shape of the hydrogen chloride molecule,
HCl.
a. | tetrahedral | c. | bent | b. | linear | d. | trigonal-planar |
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41.
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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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42.
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The mixing of two or more atomic orbitals of similar energies on the same atom
to produce new orbitals of equal energies is called
a. | VSEPR theory. | c. | hybridization. | b. | malleability. | d. | dipole-dipole
interaction. |
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43.
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Which hybrid orbitals help explain the bonding in methane,
CH4?
a. | sp3 orbitals | c. | pd3
orbitals | b. | sp orbitals | d. | df3 orbitals |
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44.
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Four hybrid sp3 orbitals are formed from
a. | two s orbitals and two p orbitals. | b. | an s orbital
and a p orbital. | c. | three s orbitals and one p
orbital. | d. | one s orbital and three p orbitals. |
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45.
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Dipole-dipole forces are considered the most important forces in polar
substances because the London dispersion forces present in polar substances
a. | are no longer present. | b. | are usually much weaker than the dipole-dipole
forces. | c. | are too unpredictable. | d. | act only in
solids. |
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46.
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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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47.
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The strong forces of attraction between the positive and negative regions of
molecules are called
a. | dipole-dipole forces. | c. | lattice forces. | b. | London forces. | d. | orbital forces. |
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48.
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The equal but opposite charges present in the two regions of a polar molecule
create a(n)
a. | electron sea. | c. | crystal lattice. | b. | dipole. | d. | ionic bond. |
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49.
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A polar molecule contains
a. | ions. | b. | a region of positive charge and a region of
negative charge. | c. | only London forces. | d. | no bonds. |
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50.
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Iodine monochloride (ICl) has a higher boiling point than bromine
(Br2) partly because iodine monochloride is a(n)
a. | nonpolar molecule. | c. | metal. | b. | polyatomic ion. | d. | polar molecule. |
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