Bonding Practice Test
Multiple Choice
Identify the choice that best completes the statement or answers the question.
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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.
When atoms share electrons, the electrical attraction of an atom for the shared electrons is called the atom's
a.
electron affinity.
c.
resonance.
b. electronegativity.
d. hybridization.
What are shared in a covalent bond?
a.
ions
c.
electrons
b. Lewis structures
d. dipoles
Most chemical bonds are
a.
purely ionic.
c.
partly ionic and partly covalent.
b. purely covalent.
d. metallic.
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.
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
In the three molecules, F2, HFl, and N2, what atom would have a partial negative charge?
a.
oxygen
c.
chlorine
b. hydrogen
d. fluorine
After drawing a Lewis structure, one should
a.
determine the number of each type of atom in the molecule.
b. add unshared pairs of electrons around nonmetal atoms.
c.
confirm that the total number of valence electrons used equals the number available.
d. determine the electronegativity of each atom.
Multiple covalent bonds may occur in atoms that contain carbon, nitrogen, or
a.
chlorine.
c.
oxygen.
b. hydrogen.
d. helium.
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.
Chemists once theorized that a molecule that contains a single bond and a double bond split its time existing as one of these two structures. This effect
became known as
a.
alternation.
c.
multiple bonding.
b. resonance.
d. single-double bonding.
The Lewis structure for the ammonium ion, NH4, has
a.
nonpolar covalent bond.
c.
polar covalent bond.
b. ionic bond.
d. metallic bond.
How many extra electrons are in the Lewis structure of the phosphate ion, PO 43–?
a.
0
c.
3
b. 2
d. 4
How many electrons must be shown in the Lewis structure of the hydroxide ion, OH –?
a.
1
c.
9
b. 8
d. 10
Compared with nonmetals, the number of valence electrons in metals is generally
a.
smaller.
c.
about the same.
b. greater.
d. almost triple.
To appear shiny, a material must be able to
a.
form crystals.
b. absorb and re-emit light of many wavelengths.
c.
absorb light and change it all to energy as heat.
d. change light to electricity.
The shiny appearance of a metal is most closely related to the metal's
a.
highly mobile valence electrons.
c.
brittle crystalline structure.
b. covalent bonds.
d. positive ions.
As light strikes the surface of a metal, the electrons in the electron sea
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a.
allow the light to pass through.
b. become attached to particular positive ions.
c.
fall to lower energy levels.
d. absorb and re-emit the light.
If a material can be shaped or extended by physical pressure, such as hammering, which property does the material have?
a.
conductivity
c.
ductility
b. malleability
d. luster
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.
Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.
a.
tetrahedral
c.
bent
b. linear
d. trigonal-planar
Use VSEPR theory to predict the shape of the chlorate ion, ClO3–.
a.
trigonal-planar
c.
trigonal-pyramidal
b. octahedral
d. bent
Use VSEPR theory to predict the shape of carbon dioxide, CO2.
a.
tetrahedral
c.
bent
b. linear
d. octahedral
Which hybrid orbitals help explain the bonding in methane, CH4?
a.
sp3 orbitals
c.
pd3 orbitals
b. sp orbitals
d. df3 orbitals
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.
The reason 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.
The following molecules contain polar bonds. The only polar molecule is
a.
CCl4.
c.
NH3.
b. CO2.
d. CH4.
Short Answer
28.
Why do most atoms form chemical bonds?
29.
Explain why scientists use resonance structures to represent some molecules.
30.
Differentiate between an ionic compound and a molecular compound.
31.
Explain why metals are good conductors of electricity.
32.
Draw a Lewis structure for carbon disulfide, CS2.
33.
Draw a Lewis structure for the nitrate ion,
Problem
. Use VSEPR theory to predict its molecular geometry.
Bonding Practice Test
Answer Section
MULTIPLE CHOICE
1.
2.
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26.
27.
ANS:
OBJ:
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SHORT ANSWER
28.
ANS:
C
1
B
3
C
3
C
4
A
4
A
4
C
5
C
4
C
5
B
5
B
5
C
4
C
4
B
4
A
1
B
2
A
2
D
2
B
3
C
3
A
2
C
2
B
2
A
3
D
3
D
4
C
5
PTS:
1
DIF:
I
REF:
1
PTS:
1
DIF:
I
REF:
1
PTS:
1
DIF:
I
REF:
1
PTS:
1
DIF:
I
REF:
1
PTS:
1
DIF:
I
REF:
1
PTS:
1
DIF:
I
REF:
1
PTS:
1
DIF:
III
REF:
1
PTS:
1
DIF:
I
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
I
REF:
2
PTS:
1
DIF:
I
REF:
2
PTS:
1
DIF:
I
REF:
3
PTS:
1
DIF:
III
REF:
3
PTS:
1
DIF:
III
REF:
3
PTS:
1
DIF:
I
REF:
4
PTS:
1
DIF:
I
REF:
4
PTS:
1
DIF:
I
REF:
4
PTS:
1
DIF:
I
REF:
4
PTS:
1
DIF:
I
REF:
4
PTS:
1
DIF:
I
REF:
4
PTS:
1
DIF:
III
REF:
5
PTS:
1
DIF:
III
REF:
5
PTS:
1
DIF:
III
REF:
5
PTS:
1
DIF:
I
REF:
5
PTS:
1
DIF:
II
REF:
5
PTS:
1
DIF:
II
REF:
5
PTS:
1
DIF:
III
REF:
5
Atoms form chemical bonds to establish a more-stable arrangement. As independent particles, they are at high potential energy. By bonding, they
decrease their potential energy, thus becoming more stable.
29.
PTS:
1
DIF:
II
REF:
1
OBJ:
2
ANS:
Resonance structures represent the bonding in molecules that cannot be adequately represented with a single Lewis structure.
30.
PTS:
1
DIF:
II
REF:
2
OBJ:
2
ANS:
Atoms in a molecular compound share electrons to achieve stability. Atoms in an ionic compound gain or lose electrons to form ions, which combine
so that the number of positive and negative charges is equal.
31.
PTS:
1
DIF:
II
REF:
3
OBJ:
1
ANS:
The valence electrons in a metal's structure are delocalized, so they can move freely and carry an electric charge throughout the metal.
PTS:
1
DIF:
II
REF:
3
OBJ:
3
1
DIF:
III
REF:
3
OBJ:
5
DIF:
III
REF:
3
OBJ:
5
PROBLEM
32.
ANS:
33.
PTS:
ANS:
trigonal-planar
PTS:
1