Unit 3 Practice Questions
I.
Ionic Bonding
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
X+
X+2
X+3
XO3-2
XO4-2
1. A type of ion found in sodium acetate
2. A type of ion found in aluminum oxide
3. A type of ion found in potassium phosphate
1
Questions 1-2 refer to the following:
(A)
(B)
(C)
(D)
(E)
1
7
9
10
14
1. The atomic number of an atom with an electron
dot arrangement similar to iodine
2. The number of atoms represented in the formula
Al(OH)3
2
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Na+
Al
F
Ti
Br--
1. Has 7 valence electrons
2. Has the electron configuration 1s22s22p63s23p1
3. Has the same electron configuration as a neon
atom
4. Has valence electrons in d orbitals
3
Questions 1-5 refer to the following:
(A)
(B)
(C)
(D)
(E)
Ca+ and K
H+ and He
Cl- and F
O- and S+
Na+ and O--
1.
2.
3.
4.
5.
Difference of 6 electrons
Same number of electrons
Difference of 9 electrons
Difference of 2 electrons
Difference of 1 electron
4
II
I
Molten sodium
chloride is a good
electrical
conductor
Sodium chloride is
an example of
ionic bonding
BECAUSE
Sodium chloride in the
molten state allows ions to
move freely
BECAUSE
Sodium and chlorine
have the same
electronegativity
5
II
I
An ionic solid is a
good conductor of
electricity
When a chlorine
atom gains an
electron, it
becomes a
positively charged
ion
BECAUSE
An ionic solid is composed
of positive and negative
ions joined together in a
lattice structure held
together by electrostatic
forces
BECAUSE
A neutral atom has
equal numbers of
protons and electrons
6
II
I
Crystals of sodium
chloride go into
solution in water as
ions
For an element
with an atomic
number of 17, the
most probable
oxidation number
(charge) is +1
BECAUSE
The sodium ion has a 1+
charge and the chloride ion
has a 1- charge and they
are hydrated by the water
molecules
BECAUSE
The outer energy level
of the halogen family
has a tendency to add
one electron to itself
7
II
I
The ionic bond is
the strongest bond
Atom A with 7
valence electrons
forms AB2 with
atom B with two
valence electrons
BECAUSE
Ionic bonds have
electrostatic attraction due
to the loss and gain of
electrons
BECAUSE
B donates its electrons
to fill the outer shell of
A
8
II
I
MgO has a high
melting point
A solution of NaCl
will conduct
electricity
BECAUSE
Highly charged ions result
in strong ionic forces and
high lattice energies
BECAUSE
NaCl will not form ions
in solution
9
The correct formula for calcium hydrogen sulfate is
(A)
(B)
(C)
(D)
(E)
CaH2SO4
CaHSO4
Ca(HSO4)2
Ca2HSO4
Ca2H2SO4
10
Which sample below has its atoms arranged in a
regular, geometric pattern?
(A)
(B)
(C)
(D)
(E)
NaC2H3O2 (s)
H2O (l)
Ar (g)
NaCl (aq)
CH4 (g)
11
How many electrons does a 37Cl ion with a charge of
-1 contain?
(A)
(B)
(C)
(D)
(E)
16
17
18
37
38
12
Which element is most likely represented by X in
the oxygen-containing ion, XO4-3?
(A)
(B)
(C)
(D)
(E)
C
N
P
S
Cl
13
Which of the following is NOT true of the element
sodium?
(A) It takes the oxidation state (charge) +1
(B) It reacts with water to form a basic solution
(C) It forms metallic bonds in its solid uncombined
form
(D) It is found in nature as a diatomic gas
(E) It reacts with a halogen to form an ionic salt
14
How many atoms are present in the formula
KAl(SO4)2?
(A)
(B)
(C)
(D)
(E)
7
9
11
12
13
15
Which sample has atoms that are arranged in a
regular geometric pattern?
(A)
(B)
(C)
(D)
(E)
KCl (l)
NaC2H3O2 (s)
Fe (l)
NaCl (aq)
HCl (aq)
16
When an ionic compound is dissolved in water, the
ions in solution can best be described as
(A)
(B)
(C)
(D)
(E)
Hydrated molecules only
Dehydrated ions and molecules
Both hydrated molecules and hydrated ions
Neither hydrated ions nor hydrated molecules
Hydrated ions only
17
What is the chemical formula for iron(III) sulfate?
(A)
(B)
(C)
(D)
(E)
Fe2SO4
Fe3SO4
Fe(SO4)3
Fe2(SO4)3
Fe2S3
18
The name of the compound MgBr2 is
(A)
(B)
(C)
(D)
(E)
Manganese bromite
Manganese bromide
Magnesium bromite
Magnesium bromide
Magnesium dibromide
19
The anion S2- is called
(A)
(B)
(C)
(D)
(E)
Sulfide
Sulfite
Sulphorous
Sulfuron
Sulfate
20
Element X forms the compounds XCl3 and X2O3.
Element X would most likely belong to the group
called
(A)
(B)
(C)
(D)
(E)
Alkali metals
Alkaline earth metals
Group 13
Halogens
Noble gases
21
A nonmetal (X) reacts with a metal (M) to give the
formula M2X. Which pairing below is most like
elements represented by M and X?
(A)
(B)
(C)
(D)
(E)
Ca and N
Li and S
Si and O
Rb and F
Mg and Cl
22
In the Lewis dot structure X: , what is the
predictable oxidation number (charge)?
(A)
(B)
(C)
(D)
(E)
+1
-1
+2
-2
+3
23
Which of the following compounds would be
expected to have the greatest lattice binding
energy?
(A)
(B)
(C)
(D)
(E)
LiNO3
LiF
KI
NH4Br
CsNO3
24
Which of the following is true regarding an Ne atom
with a mass number of 20 and an O2- ion with a
mass number of 16?
(A) They contain the same number of protons
(B) They contain the same number of neutrons
(C) They contain the same number of protons plus
neutrons
(D) They are isoelectronic
(E) They are isomers
25
Which bonds are ionic?
I. HCl
II. SCl
III. CsF
(A)
(B)
(C)
(D)
(E)
I only
III only
I and II only
II and III only
I, II and III
26
II. Covalent Bonding
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
CH4
CO2
NH3
N2
O2
1. Forms hydrogen bonds
2. Is polar
3. Has a triple bond
27
II
I
A pi bond is formed
between the lobes
of adjacent p
orbitals in the same
plane of two atoms
that contain only
one electron each
BECAUSE
Each of the two lobes of a
single p orbital can hold
two electrons of opposite
spin
Ammonia (NH3)
has a trigonal
pyramidal
molecular
structure
BECAUSE
Ammonia has a
tetrahedral electron pair
geometry with three
atoms bonded to the
central atom
28
II
I
Maximum
repulsion between
two electron pairs
in a molecular
compound will
result in a linear
structure
BECAUSE
The VSEPR model says that
like charges will orient
themselves so as to
diminish the repulsion
between them
The structure of
SO3 is shown by
using more than
one structural
formula
BECAUSE
SO3 is very unstable and
resonates between
these possible
structures
29
II
I
The hybrid orbital
form of carbon in
acetylene (C2H2) is
believed to be the
sp form
The weakest of
the bonds
between
molecules are
coordinate
covalent bonds
BECAUSE
BECAUSE
C2H2 is a linear compound
with a triple bond between
the carbons
Coordinate covalent
bonds represent the
weak attractive force of
the electrons of one
molecule for the
positively charged
nucleus of another
30
II
I
Water is a polar
substance
Water is a good
solvent for ionic
and/or polar
covalent
substances
BECAUSE
BECAUSE
The sharing of the bonding
electrons in water is equal
Water shows hydrogen
bonding between
oxygen atoms
31
II
I
The N-N bond
distance in N2 is
shorter than the NN bond distance in
N2H4
Elemental iodine
has a higher
boiling point than
elemental
bromine
BECAUSE
BECAUSE
The atomic radius of H is
smaller than the atomic
radius of N
Iodine forms stronger
covalent bonds than
bromine
32
II
I
The boiling point of
H2O is higher than
the boiling point of
H2S
Bromine has a
higher boiling
point than
chlorine
BECAUSE
BECAUSE
H2S has a greater molecular
mass than H2O
Bromine has higher
dispersion forces than
chlorine
33
II
I
Some covalent
bonds are polar in
nature
A nonpolar
molecule can have
polar bonds
BECAUSE
BECAUSE
Atoms of different
electronegativities are
unequal in the degree to
which they attract electrons
Polar bonds can be
symmetrically arranged
in a molecule so that
there are no net poles
34
II
I
The bond in an O2
molecule is
nonpolar
BF3 has a
tetrahedral
geometry
BECAUSE
BECAUSE
The oxygen atoms in an O2
molecule share the bonding
electrons equally
The central B atom does
not have a complete
stable octet
35
II
I
Substances with
hydrogen bonding
tend to have
unusually low
boiling points
CCl4 is a nonpolar
compound
BECAUSE
BECAUSE
Extra energy is necessary to
break the hydrogen bonds
The dipole moments are
canceled out
36
A tetrahedral molecule, XY4, would be formed if X
were using the orbital hybridization
(A)
(B)
(C)
(D)
(E)
p2
s2
sp
sp2
sp3
37
Which of the elements below is most likely to form
compounds in which it has an incomplete octet?
(A)
(B)
(C)
(D)
(E)
B
C
N
O
F
38
Which substance has a polar covalent bond
between its atoms?
(A)
(B)
(C)
(D)
(E)
K3N
Ca3N2
NaCl
F2
NH3
39
Which molecule is a polar molecule?
(A)
(B)
(C)
(D)
(E)
N2
H2O
CH4
CO2
KCl
40
In which of the following compounds are hydrogen
bonds between molecules the strongest?
(A)
(B)
(C)
(D)
(E)
HF
HCl
HBr
HI
HAt
41
The compound PF5 is called
(A)
(B)
(C)
(D)
(E)
Monophorofluoride
Phosphorus pentafluoride
Pentaphosphoro fluoride
Phosphorus tetrafluoride
Potassium pentafluoride
42
How many sigma and pi bonds are found in the
following molecule?
H—C
(A)
(B)
(C)
(D)
(E)
C—CH2—CH=CH2
6 sigma, 2 pi
2 sigma, 6 pi
10 sigma, 3 pi
5 sigma, 3 pi
11 sigma, 2 pi
43
Which of the following statements is false?
(A) H2 has just one sigma bond
(B) HCl has just one sigma bond
(C) H—C
C—H has four pi and three sigma
bonds
(D) CH2=CH2 has five sigma bonds and one pi bond
(E) H2O has two sigma bonds and two lone pairs
44
How many pi bonds are there in a molecule of
N
(A)
(B)
(C)
(D)
(E)
C—CH2—CH2—NH—CH=CH2
6
4
12
10
3
45
Which of the following species has a molecular
shape most similar to that of ammonia, NH3?
(A)
(B)
(C)
(D)
(E)
BH3
H2O
H3O+
CH4
NH4+
46
Which compound below has a bent molecular
geometry?
(A)
(B)
(C)
(D)
(E)
H2SO4
CH4
CO2
H2S
C2H2
47
Which compound of oxygen is most likely to contain
an O-O bond?
(A)
(B)
(C)
(D)
(E)
CO2
NO2
SO2
H2O2
TiO2
48
How many single bonds are in a molecule of carbon
dioxide, CO2?
(A)
(B)
(C)
(D)
(E)
None
One
Two
Three
Four
49
All of the following have covalent bonds EXCEPT
(A)
(B)
(C)
(D)
(E)
HCl
CCl4
H2O
CsF
CO2
50
Which of the following molecules is polar?
(A)
(B)
(C)
(D)
(E)
BH3
NF3
C2H6
SF6
CCl4
51
The shape of a PCl3 molecule can be described as
(A)
(B)
(C)
(D)
(E)
Bent
Trigonal pyramidal
Linear
Trigonal planar
Tetrahedral
52
Which of the following is a nonpolar molecule?
(A)
(B)
(C)
(D)
(E)
CO2
H2O
NH3
NO
HI
53
The structure of SiO2 can best be described as
(A)
(B)
(C)
(D)
(E)
Linear
Bent
Trigonal
Tetrahedral
Square
54
Which of the following molecules has a trigonal
pyramidal geometry?
(A)
(B)
(C)
(D)
(E)
BH3
H2O
CH4
NH3
AlCl3
55
Which of these resembles the molecular structure
of the water molecule?
(A)
(B)
(C)
(D)
(E)
H—H—O, linear
H—O—H, bent, 30o angle
H—O—H, bent, 90o angle
H—O—H, bent, 105o angle
H—O—H, linear
56
The shape of a PCl3 molecule is described as
(A)
(B)
(C)
(D)
(E)
Bent
Trigonal planar
Linear
Trigonal pyramidal
tetrahedral
57
The bond that includes an upper and a lower
sharing of electron orbitals is called
(A)
(B)
(C)
(D)
(E)
A pi bond
A sigma bond
A hydrogen bond
A covalent bond
An ionic bond
58
What is the structure associated with the BF3
molecule?
(A)
(B)
(C)
(D)
(E)
Linear
Trigonal planar
Tetrahedron
Trigonal pyramidal
Bent
59
Which of these statements is the best explanation
for the sp3 hybridization of carbon’s electrons?
(A) The new orbitals are one s orbital and three p
orbitals
(B) The s electron is promoted to the p orbitals
(C) The s orbital is deformed into a p orbital
(D) Four new and equivalent orbitals are formed
(E) The s orbital electron loses energy to fall back
into a partially filled p orbital
60
The intermolecular force that is most significant in
explaining the variation of the boiling point of water
from the boiling points of similarly structured
molecules is
(A)
(B)
(C)
(D)
(E)
Hydrogen bonding
Van der Waals forces
Covalent bonding
Ionic bonding
Coordinate covalent bonding
61
Which of the following properties can be attributed
to water?
I. It has a permanent dipole moment attributed
to its molecular structure
II. It is a very good conductor of electricity
III. It has polar covalent bonds with hydrogen on
opposite sides of the oxygen atom, so that
the molecule is linear
(A)
(B)
(C)
(D)
(E)
I only
III only
I and II only
II and III only
I, II and III
62
III. All Types of Bonding
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
Ionic substance
Metallic substance
Polar covalent molecule
Nonpolar covalent molecule
Aromatic organic molecule
1. Carbon tetrachloride
2. Cesium chloride
3. Hydrogen chloride
63
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Ionic
Covalent
Polar covalent
Metallic
Hydrogen bonding
1. When the electronegativity difference between 2
atoms is 2
2. If two atoms are bonded in such a way that both
members of the pair equally share one electron
with the other
3. Which of the 5 choices is the weakest bond?
4. If an electron is lost by one atom and completely
captured by another
64
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
Water
Hydrogen bromide
Iron
Argon
Sodium chloride
1. Hydrogen bonding
2. Highly polar
3. Dispersion forces
65
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
Ionic
Covalent
Polar covalent
Metallic
Hydrogen bonding
1. Bonding that explains water’s high boiling point
2. If the sharing of an electron pair is unequal and the
atoms have an electronegativity difference of 1.4
to 1.6
3. If one or more valence electrons become detached
from the atoms and migrate in a “sea” of free
electrons among the positive metal ions
66
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
Hydrogen gas, H2
Carbon monoxide, CO
Potassium, K
Aluminum oxide, Al2O3
Bromine, Br2
1. Substance held together by metallic bonds
2. Substance held together by ionic bonds
3. Consists of polar molecules
67
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Hydrogen bond
Ionic bond
Polar covalent bond
Nonpolar covalent bond
Metallic bond
1. The type of bond between atoms of potassium and
chloride
2. The type of bond between the atoms in a nitrogen
molecule
3. The type of bond between the atoms in CO2
(electronegativity difference = 1)
4. The type of bond between the atoms of calcium in
a crystal of calcium
68
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Ionic substance
Polar covalent substance
Nonpolar covalent substance
Amorphous substance
Metallic network
1.
2.
3.
4.
KCl (s)
HCl (g)
CH4 (g)
Li (s)
69
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Hydrogen bonding
Ionic bonding
Metallic bonding
Nonpolar covalent bonding
Polar covalent bonding
1. Holds a sample of barium iodide, BaI2, together
2. Allows solids to conduct electricity
3. Attracts atoms of hydrogen to each other in an H2
molecule
4. Responsible for relatively low vapor pressure of
water
70
Questions 1-5 refer to the following:
(A)
(B)
(C)
(D)
(E)
Hydrogen bonding
Ionic bonding
Network bonding
London dispersion force
Metallic bonding
1. Chiefly responsible for the relatively high boiling
point of water
2. Is present in liquid oxygen
3. Is primarily responsible for the hardness of
diamond
4. Allows copper to conduct electricity
5. Is present in solid KCl
71
II
I
Most atoms are
less stable in the
bonded state than
in the unbonded
state
Ionic bonds are
always stronger
than covalent
bonds
BECAUSE
Both ionic and covalent
bonds fail to provide the
participating atoms with a
stable electron
configuration
BECAUSE
They break only when
bombarded with
electrons
72
I
The most
important factor in
determining the
chemical properties
of an element is
the number of
electrons in the
outermost shell
Helium will have
fewer dispersion
forces between its
atoms than the
other noble gases
II
BECAUSE
BECAUSE
The number of electrons in
the outer shell determines
the bonding characteristics
of the element
As the mass of nonpolar
atoms and molecules
increases, dispersion
forces increase
73
Which of the following are the WEAKEST attractive
force?
(A)
(B)
(C)
(D)
(E)
Dipole-dipole forces
Coordinate covalent bonding
Covalent bonding
Polar covalent bonding
Ionic bonding
74
The complete loss of an electron of one atom to
another atom with the consequent formation of
electrostatic charges is referred to as
(A)
(B)
(C)
(D)
(E)
A covalent bond
A polar covalent bond
An ionic bond
A coordinate covalent bond
A pi bond between p orbitals
75
Which of the following compounds would be
predicted to have the highest melting point?
(A)
(B)
(C)
(D)
(E)
CS2
HI
H2S
H2O
MgO
76
Which compound is not paired with its correct
name?
(A)
(B)
(C)
(D)
(E)
FeCl2 / iron(II) chloride
K2O / potassium oxide
NO2 / nitrogen dioxide
PCl3 / potassium trichloride
NH4Cl / ammonium chloride
77
Which of the following statements about bonding is
correct?
(A) Van der Waals forces exist between polar
molecules
(B) Dipoles are the result of the equal sharing of
electrons
(C) Cu(s) is a network solid
(D) Hydrogen bonds exist between the molecules of
HCl
(E) NaCl (aq) has attraction between the molecules
and the ions
78
Which kinds of bonding can be found in a sample of
H2O (l)?
(A)
(B)
(C)
(D)
(E)
Hydrogen bonds only
Nonpolar covalent bonds only
Ionic and nonpolar hydrogen bonds
Both polar covalent and hydrogen bonds
Metallic and ionic bonds
79
Which compound contains no ionic character?
(A)
(B)
(C)
(D)
(E)
NH4Cl
CaO
K2O
Li2O
CO
80
The forces of attraction that exist between nonpolar
molecules are called
(A)
(B)
(C)
(D)
(E)
Van der Waals/ dispersion forces
Ionic bonds
Covalent bonds
Electrovalent bonds
Metallic bonds
81
When a salt dissolves in water, the water molecules
are attracted by ions in solution. This attraction is
called
(A)
(B)
(C)
(D)
(E)
Atom-atom
Molecule-molecule
Molecule-ion
Ion-ion
Atom-ion
82
Which element is expected to have a “sea” of
electrons?
(A)
(B)
(C)
(D)
(E)
Hydrogen
Nitrogen
Cobalt
Chlorine
Oceanium
83
In which of the following liquids are the Van der
Waals forces of attraction between the molecules
weakest?
(A)
(B)
(C)
(D)
(E)
Xe
Kr
Ar
Ne
He
84
Which molecule has both nonpolar intramolecular
and nonpolar intermolecular bonds?
(A)
(B)
(C)
(D)
(E)
CCl4
CO
HF
HCl
F2
85
If two atoms that differ in electronegativity combine
by chemical reaction and share electrons, the bond
that joins them will be
(A)
(B)
(C)
(D)
(E)
Metallic
Ionic
A hydrogen bond
Nonpolar covalent
Polar covalent
86
The reactivity and chemical behavior of an atom is
governed by many factors. The most important
factor is
(A) The number of protons in the nucleus
(B) The number of neutrons in the nucleus
(C) The number of protons and neutrons in the
nucleus
(D) The ratio of protons and neutrons in the nucleus
(E) The number of electrons in the valence shell
87