Which is a typical characteristic of
an ionic compound?
 Electron pairs are shared among atoms.
 The ionic compound has a low solubility in water.
 The ionic compound is described as a molecule.
 The ionic compound has a high melting point.
 The ionic compound has a high melting point.
What is shown by the structural
formula of a molecule or
polyatomic ion?
 the arrangement of bonded atoms
 the number of metallic bonds
 the number of ionic bonds
 the shapes of molecular orbitals
 the arrangement of bonded atoms
Which of these elements does not exist as a
diatomic molecule?
 Ne
H
F
I
 Ne
How do atoms achieve noble-gas
electron configurations in single
covalent bonds?
 One atom completely loses two electrons to the other
atom in the bond.
 Two atoms share two pairs of electrons.
 Two atoms share two electrons.
 Two atoms share one electron.
 Two atoms share two electrons.
Why do atoms share electrons in
covalent bonds?
 to become ions and attract each other
 to attain a noble-gas electron configuration
 to become more polar
 to increase their atomic numbers
 to attain a noble-gas electron configuration
Which of the following elements can form diatomic
molecules held together by triple covalent bonds?
 carbon
 fluorine
 oxygen
 nitrogen
 nitrogen
Which noble gas has the same
electron configuration as the
oxygen in a water molecule?
 helium
 argon
 neon
 xenon
 neon
Which elements can form diatomic
molecules joined by a single
covalent bond?
 hydrogen only
 halogens only
 halogens and members of the oxygen group only
 hydrogen and the halogens only
 hydrogen and the halogens only
Which of the following is the name given to the pairs of
valence electrons that do not participate in bonding in
diatomic oxygen molecules?
 unvalenced pair
 inner pair
 outer pair
 unshared pair
 unshared pair
A molecule with a single covalent
bond is ____.
 CO2
 CO
 Cl 2
 N2
 Cl 2
Once formed, how are coordinate
covalent bonds different from
other covalent bonds?
 They are stronger.
 They are weaker.
 They are more ionic in character.
 There is no difference.
 There is no difference.
When H forms a bond with H2 O to form the hydronium ion H 3O +, this bond is
called a coordinate covalent bond because ____.
 both bonding electrons come from the oxygen atom
 it forms an especially strong bond
 the electrons are equally shared
 the oxygen no longer has eight valence electrons
 both bonding electrons come from the oxygen atom
How many valid electron dot formulas—having the same number
of electron pairs for a molecule or ion—can be written when a
resonance structure occurs?
0
 2 only
 1 only
 2 or more
0
How many electrons can occupy a
single molecular orbital?
0
2
1
4
2
According to VSEPR theory, molecules adjust their shapes
to keep which of the following as far apart as possible?
 pairs of valence electrons
 mobile electrons
 inner shell electrons
 the electrons closest to the nuclei
 pairs of valence electrons
What causes water molecules to have a bent shape,
according to VSEPR theory?
 repulsive forces between unshared pairs of electrons
 interaction between the fixed orbitals of the unshared
pairs of oxygen
 ionic attraction and repulsion
 the unusual location of the free electrons
 repulsive forces between unshared pairs of electrons
What type of hybrid orbital exists in the methane
molecule?
 sp
 sp 3
 sp 2
 sp 3d 2
 sp 3
What is the shape of a molecule
with a triple bond?
 tetrahedral
 bent
 pyramidal
 linear
 linear
What is thought to cause the
dispersion forces?
 attraction between ions
 sharing of electron pairs
 motion of electrons
 differences in electronegativity
 motion of electrons
What are the weakest attractions
between molecules?
 ionic forces
 covalent forces
 Van der Waals forces
 hydrogen forces
 Van der Waals forces
What causes hydrogen bonding?
 attraction between ions
 motion of electrons
 sharing of electron pairs
 bonding of a covalently bonded hydrogen atom with
an unshared electron pair
 bonding of a covalently bonded hydrogen atom with
an unshared electron pair