acs practice exam general chemistry

General Chemistry II Sample Test bank

Page 1of 27

1. According to the Bronsted—Lowry definition,

8. The weakest of the bases listed is

which chemical species can function both as an
acid and as a base?
a. Cl—
b. SO42—
c. NH4+
d. HCO3—
e. H3O+

Acid

HCl
HSO4—
SO42—
H2S
HS—
HS—
S2—
a. Cl—
b. CN—
c. HS—
d. S2—
e. SO42—

2. In the reaction CN— + H2O  HCN + OH—
which is an acid—base conjugate pair?
a. H2O and HCN
b. H2O and OH—
c. CN— and H2O
d. HCN and OH—

Period
First
Second
Third
a.
b.
c.
d.
e.

4. The pH of a 0.03 M HCl solution is
a. 1.5
b. 2.5
c. 3.5
d. 12.5
solution at

6. Which is the strongest acid?
a.
b.
c.
d.

HClO
HClO2
HClO3
HClO4

7. Which salt reacts with water (hydrolyzes) to
produce a basic solution?
a.
b.
c.
d.

NaC2H3O2
NaNO3
NH4Cl
BaSO4

Ka (Ionization
Constant of Acid)
100% ionized
1.2 x 10-2
5.7x10-8
1.2x10-13

9. The oxide of which element will react with water
to form the strongest acid?

3. Given that HX is a stronger Bronsted acid than
HY in aqueous solution, which is true of a 1 M
solution of NaX

a. It is less basic than a 1 M solution of NaY.
b. It is more basic than a 1 M solution of NaY.
c. It yields a neutral solution.
d. It is more concentrated than a 1 M solution
of NaY.

5. The pH of a 1.0 x 10—3 M Ba(OH)2
25oC is
a. 2.7
b. 3.0
c. 11.0
d. 11.3

Conjugate
Base
Cl—

10.

Main Groups
I
II II IV
I
X
W

Y

Z

P

V

VI

VII

O

Q
R

S
T

U
M

W
M
P
R
Z

Which statement is a logical inference from the
fact that a 0.10 M solution of potassium acetate
KC2H3O2, is less alkaline than a 0.10 M solution
of potassium cyanide, KCN?
a.

b.
c.
d.

Hydrocyanic acid is a weaker acid than
acetic acid.
Hydrocyanic acid is less soluble in water
than acetic acid.
Cyanides are less soluble than acetates
Acetic acid is a weaker acid than
hydrocyanic acid

11.In the titration of 50.0 mL of 0.100 M
benzoic acid (a monoprotic acid) with 50.0 mL of
0.100 M NaOH, the properties of the solution at
the equivalence point will correspond exactly to
the properties of
a. a 0.100 M sodium solution.
b. a 0.0500 M sodium hydroxide solution.
c. a 0.0500 M benzoic acid solution.
d. a 0.0500 M sodium benzoate solution.


12.

13.

A mixture of which pair of 0.1 M aqueous
solutions would constitute a buffer?
a. NaOH and NaCl

b. HCl and NaOH
c. HCl and NaCl
d. NH3 and NH4NO3

Which electron transition is associated with the
largest emission of energy?
a.
b.
c.
d.

What do these have in common?
20

a.
b.
c.
d.
14.

19.

19 1-

Ne

F

24

Mg2+

20.

the same number of protons
the same number of neutrons
the same number of electrons
the same size

The number of neutrons in the nucleus of
13

a.
b.
c.
d.
e.

n=2 to n=1
n=2 to n=4
n=2 to n=3
n=3 to n=2

If an electron moves from one energy level in an
atom to another energy level more remote from
the nucleus of the same atom
a. energy is absorbed.
b. energy is liberated.
c. there is no energy change.
d. the atom must assume a different ionic

valence
an 2
e. light of a
at
definite wave
o
length is
m
emitted.
of
4
21.
A
0
photon
1
of light
3
of 450
2
nm,
7
when
1
compar
4
ed to
9
light of
wavele

ngth
300
nm, has
(1nm =
10-9 m)
a.

15.

16.

The orbitals of 2p
electrons are often
represented as being
a. elliptical.
b. Pyramidal
c. Tetrahedral
d. dumbbell
shaped
e. spherical.
The element in
Period 5, Group 3A,
has the outer
electron
configuration
a. 5s25p1
b. 3s23p5
c. 3s23p3

d.

a higher
frequency.

5s25p3

17.

Which
electron
configuration
is
impossible?
a. 1s22s22p63s2
b. 1s22s22p63s23p6
c. 1s22s22p62d2
d. 1s22s22p53s1

18.

The element X occurs
naturally to the extent
of 20.0% 12X and
80.0% 13X. The atomic
mass of X is nearest


a.
b.
c.

d.

12.2
12.5
12.8
13.0

b.
c.
d.
22.

lower energy.
a greater
velocity.
a shorter
wavelength

Which set of
quantum
numbers is
possible for
an electron in
an atom?
a. n=3, l=0,
ml=1, ms = -½
b. n=2, l=2,ml=
-2, ms = -½
c. n=5, l=2,
ml=2, ms =+½

d. n=4, l=3, ml=
-4, ms= -½

23.

A compound
consisting of
an element
having a low
ionization
potential
and a second
element
having a
high
electron
affinity is
likely to
have
a.
b.
c.
d.

24.

covalent bonds
metallic bonds
coordinate
covalent bonds

ionic bonds.

According
to modern
bonding
theory the
number of
sigma (σ)
and pi (π)
bonds in
the
ethylene
molecule
H2C=CH2 is
a. l π and 4 σ

b.
c.

l π and 1 σ
l π and 5 σ

d.
e.

2 π and 4 σ
l π and 6 σ


25.

The number of σ bonds in N=N is
a. 1
b. 2
c. 3
d. 4

26.

The elements in an ionic compound are held
together by

Standard Potentials
Mg Mg2++2e
Al  Al3++3e
Zn  Zn2++2e
FeFe2++2e
Cu  Cu2++2e
Ag Ag++ e
31.

o
E
2.37V
1.66V
0.76V
0.44V
0.34V
-0.80V

Using only the metals Mg, Al, Zn, Fe, Cu
a.

27.

electrostatic
forces of
attraction.
b. van der
Waals
forces
c. the spin of
paired
electrons.
d. the
formation
of hybrid
orbitals.
e. an electron
pair.
In every
electrolytic and
galvanic
(voltaic) cell
the anode is
that electrode
a.
b.
c.

d.

28.

at which
oxidation
occurs.
which
attracts
cations.
at
whi
ch
elec
tron
s
are
sup
plie
d to
the
solu
tion.
at which
reduction
occurs.

Metal X was
plated from a
solution

containing cations
of X. The passage
of 48.25 C
deposited 31 mg of
X on the cathode.
What is the mass
of X (in grams) per
mole of electrons?
a. 47
b. 62
c. 93
d. 186
29.

In a galvanic
(voltaic) cell
in which the
reaction is
Cd +
2+
Cu  Cu +
Cd2+
and the ions are at
unit concentration
(activity), the cell
potential is
C
d


C
d
2+

+
2
e
-

0
.
4
0
2
1
V
C
u

C
u


2

and Ag,
together
with their 1
M salt
solutions, a

voltaic cell
of the
highest
possible
voltage
would be
constructed
using
electrodes of
these
metals.
a. Mg and Ag
b. Mg and Fe
c. Zn and Cu
d. Al and Ag
e. Mg and Al

+

+
2
e
-

0
.
3
4
4
V

a
.
32.

0
.
1
3
8
3
V
b.
c.
d.
e.
30.

0.4021 V
0.344 V
0.7461 V
0.3677 V

In which
reaction will
an increase in
total pressure
at constant
temperature
favor
formation of

the products?
a. CaCO3(s)

CaO(s) +
CO2(g)
b. H2(g) +
Cl2(g) 
2HCl(g)
c. 2NO(g) +
O (g)  2NO
(g)

c. +
]
33.

b.

E = Eo 0.059/n
log Q
(Nernst
equation
) [H+] =
1.0 M
initially,
P02 = 1.0
atm
4e + O2(g)+4H+
(aq) 2H2O(l)
Eo=1.23V

Based on
the
information
above,
which
statement is
correct?
a.

n=
1,
sin
ce
on
e
mo
le
of
ox
yg
en
is

d.

The
equilibri
um
constant
for the

gaseous
reaction
C+D
 E +
2F is 3.0
at 50 oC.
In a
2.0 L flask
at 50 oC are
placed 1.0
mol of C,
1.0 mol of
D, 1.0 mol
of E, and
3.0 mol of
F.
Initially, the
reaction will
a. proceed at
equal rates
in both
directions.
b. proceed
more
rapidly to
form E and
F.
c. proceed
more
rapidly to

form C and
D.
d. not occur
in either
direction.
Compound
H2O(l)
H2O(g)

34.
[
O
2

value,]
which
less [
1.23 H

At
298
K
the
equi
libri
um
cons
tant
for

∆Go
—237
—229

H2(g) +
½
O2(g)

H2O(l)
a.

i
s
l
a
r
g
e
r
t
h
a
n
t
h
e
K
e
q
f

o
r
H
2

(
g
)
+
½
O
2

(
g
)


H
2

O
(
g
)


b.

d.

will have
a value of

1 0 at
equilibrium.
2
2
c.
cannot be
computed since data on O2
and
COCl2(g)  CO(g) + Cl2(g)


H2 are not provided.
will have the same value as the Keq for
2 H2(g) + O2(g) 2 H2O(l)

b.

Consider the reversible system at
equilibrium:
2CO + O2  2CO2 + heat
When the temperature is increased at constant
pressure

d.

d.

35.

a.
b.
c.
d.
e.
36.

37.

The numerical value of the equilibrium
constant for any chemical change is affected by
changing
a. the catalyst.
b. the concentration of the products.
c. the concentration of reacting substances.
d. the pressure.
e. the temperature

39.

At a certain temperature, the equilibrium
constant for the reaction 2HI(g)  H2(g) +
I2(g) is 0.49. Calculate the number of moles of
hydrogen produced when one mole of HI is
placed in a 1 L vessel at this temperature.
a. 0.41
b. 0.25
c. 0.29

d. 3.45

40.

What is the [OH-] of a solution which is
0.18 M in ammonium ion and 0.10 M in
ammonia? Kb = 1.8 x 10-5
a. 1.3x10-3
b. 1.0x10-3
c. 1.3x10-5
d. 1.0x10-5

41.

What is the pH of a 0.10 M solution of a
monoprotic acid, HA, with a Ka = 1.0 x 10-6?
a. 1.6
b. 3.5
c. 5.0
d. 6.0

42.

When 0.10 mol of a weak acid HA was diluted
to one liter, experiment showed the acid to be
1% dissociated.
HA + H2O  H3O+ + AWhat is the acid dissociation constant, Ka?
a. 1 x10-6
b. 1 x10-5
c. l x10-3

d. 1 x105
Which solution has a pH less than 7.0?
a. 1 M NH4Cl
b. 1 M K2CO3
c. 1 M NaOCl
d. 1 M NaOH

What is the equilibrium constant expression for
the gas phase oxidation of CO to CO2 by O2?
a.
b.

38.

the CO2 concentration will be increased.
the CO2 concentration will be decreased.
the amount of each substance will be
unchanged.
the amount of each substance will be
increased.
the result cannot be predicted from the
information given.

c.

K = [CO2]2
[CO][O2]
K= [CO]2 [O2]
[CO2]
c.

K= [CO2]2
[CO]2 [O2]

d.

K= [CO] [O2]
[CO2]

43.

Into an empty vessel COCl2(g) is
introduced at 1.0 atm pressure whereupon it
dissociates until equilibrium is established:
2COCl2(g)  C(graphite) +CO2(g) + 2Cl2(g)
44.

a.

If x represents the partial pressure of
CO2(g) at equilibrium, what is the value of
the equilibrium constant, Kp?
x.2x2
(1.0-2x)2

x x 2x2
(1.0-2x2)
x (2x)2
(1.0- 2x)2
x (2x)2

(1.0—x)2

What is the pH of a 0.1 M NaF solution?
Ionization constant for HF, Ka = 7 x 10-4
a. 2.1
b. 5.9
c. 8.1
d. 9.1


45.

a.
b.
c.
d.
46.

1.6x10-2
1.6x10-9
4.0x10-5
6.2x10-5

The addition of solid Na2SO4 to an aqueous
solution in equilibrium with solid BaSO4 will
cause
a.
b.
c.
d.

48.

2.2x10-4M
9.0 x 10-4 M
4.5 x 10-4 M
9.5 x 10-3M

Assume that standardized aqueous solutions of
each of these are available.

NaOAc
RNH3+ClRNH2
HOAc

52.

The correct IUPAC name of N2O3 is
a. nitrogen oxide.
b. nitrogen(II) oxide.
c. nitrous oxide
d. dinitrogen trioxide.

53.

In which case is the substance with the
given formula followed by its correct name?
a. KNO2 — potassium nitrate
b. FeCl3 — iron(III) chloride
c. FeS — iron(II) sulfite

d. Mg3N2 — magnesium nitrite
e. HClO — hydrochloric oxide

54.

Balance the equation for the following
reaction, using no fractional coefficients.
? C +? HNO3  ? CO2 +? NO2 +? H2O

Ionization
Constant
Kb = 5.6 x 10-10
Ka = 5.6 x 10-10
Kb=1.8x10-5
Ka=1.8x10-5

A buffer with a desired pH is 5.0 would be
conveniently prepared by appropriate mixtures of
a. NaOAc and HOAc
b. HOAc and water
c. NaOAc and RNH2
d. HOAc and RNH2

50.

Which is the correct expression for the
solubility product constant for Ag2CrO4?
a. Ksp = [Ag+]2 [CrO4 2-]
b. Ksp = [2Ag+]2 [CrO4 2-]
c. Ksp = [Ag+] [CrO42-]

d. Ksp = [Ag+] [CrO42-]2
e. Ksp = [2Ag+] [CrO42-]

no change in [Ba2+] in solution.
more BaSO4 to dissolve.
precipitation of more BaSO4.
an increase in the Ksp of BaSO4.

Substance

49.

51.

The solubility of BaCO3 is 7.9 x 10-3 g/L.
Calculate the solubility product, Ksp ignoring
hydrolysis. MW of BaCO3 197 g/mol
a.
b.
c.
d.

47.

BaCrO4 253 g/mol
a. 1.2x10-10
b. 2.2x10-5
c. 2.8x10-3
d. 7.8 xl0-6

What is the hydrogen ion concentration of a
buffer solution containing 0.10 M NO 21- and 0.20
M HNO2?
Ionization constant for Nitrous
Acid, Ka = 4.5x 10-4

Which substance is most soluble in water?
a. C6H6
b. CaCO3
c. C2H5OH
d. CO2
The solubility of BaCrO4 in water is 2.8 x 10-3
g/L what is the Ksp of the salt? MW of

55.

The sum of the coefficients in the balanced
equation is
a. 5
b. 7
c. 9
d. 12
e. 16
Complete and balance the equation for the
reaction, where the reactants are in aqueous
solution. Use no fractional coefficients.
? Na3PO4 + ? Ba(NO3)2  ? +

?

The number of moles and formula of the product
containing Ba are
a. 3NaNO3
b. BaPO4
c. Ba(PO4)2
d. Ba2P3
e. Ba3(PO4)2


56.

According to the kinetic molecular theory,
a.
b.
c.
d.
e.

57.

b.
c.
d.

e.

59.

attractive forces between gas molecules are
negligible.

attractive forces between gas molecules are
appreciable.
the average kinetic energy of the molecules
of a gas is proportional to the absolute
temperature.
increasing the molecular concentration, at
constant temperature, means increasing the
number of collisions between molecules
and container.
collisions between gas molecules are
perfectly elastic.

The Kelvin temperature of one liter of gas is
doubled and its pressure is tripled, volume will
then be
a. l/6 L
b. 2/3 L
c. 3/2 L
d. 6 L
Which gas, present in the same closed system,
has the greatest average kinetic energy at a given
temperature?
a.
b.
c.
d.

A sample of neon occupies a volume of
27.3 L at STP. What would be the neon volume
at 177 oC and 0.100 atm pressure?

a.
b.
c.
d.

177 L
350 L
422 L
450 L

61.

Under the same conditions of temperature and
pressure, the gas whose molecules possess the
highest average speed is
a. H2O
b. O2
c. F2
d. Ne

62.

What is the volume of 2.00 mol of helium gas
at 27 oC and 3.00 atm?

The volume of a given mass of gas varies
inversely with pressure, provided that the
temperature remains constant because
a.

58.

gaseous molecules are continuously in
random motion and collisions are perfectly
elastic.
the absolute temperature of a gas depends
on its molar mass.
the pressure exerted on a gas affects the
speed of its molecules.
gaseous molecules can travel in straight or
curved paths.
all gaseous molecules are diatomic.

60.

a.
b.
c.
d.
63.

6.1x10-2L
1.48L
16.4L
44.8 L

Real gases are most like ideal gases at
a.
b.
c.

d.

high pressure and high temperature.
low pressure and low temperature.
high pressure and low temperature.
low pressure and high temperature.

64.

500 mL of a gaseous compound has a mass of
0.9825 g at 0oC and 760 mmHg. What is the
approximate molar mass of the compound?
a. 19.7
b. 38.7
c. 44.0
d. 58.9

65.

The partial pressures of a gaseous mixture are
given in the table. What is the mole percent of
hydrogen?

Hydrogen
neon
carbon dioxide
None; the average kinetic energy is the
same for each gas.
a.
b.

c.
d.

hydrogen
carbon dioxide
methane
ethylene
20.0
25.8
38.8
41.7

Partial Pressures
200 mmHg
150 mmHg
320 mmHg
105 mmHg


66.

67.

It is desired to collect enough oxygen over water
at 25 oC and 750 mmHg barometric pressure to
be equivalent to 1 L of pure oxygen at 0 oC and
760 mmHg. The vapor pressure of water at 25 oC
is 23.5 mm. The volume collected is
a. 1 L (298/273)(750/760)
b. 1 L (273/298)((750-23.5)/(760-23.5))

c. 1 L (273/298)((750-23.5)/760)
d. 1 L (298/273)(760/(750-23.5))

71.

The following mechanism has been
proposed for the formation of ethylbenzene:
CH3CH2Br + AlBr3  AlBr -4+ CH3CH +2
+
CH3CH2+ + C 6H 6 C H6 CH
CH
6
2
3
+
C6H6CH2CH 3 + AlBr 4 AlBr3 + HBr +
C6H5CH2CH3
Which substance serves as the catalyst?

Methane, CH4, diffuses in a given apparatus at
the rate of 30 mL/min. At what rate would a

a. AlBr3
b. CH3CH2+
gas with a molar
mass of 100 diffuse
under the same
conditions? MW of
CH4 = 16 g/mol
a. 0.77 mL/min

b. 30 mL/min
c. 6.7 mL/min
d. 75 mL/min
e. 12.0 mL/min
68.

The Arrhenius
equation, k= AeE/RT
expresses the
relationship
between the
reaction rate
constant, k, and
the energy of
activation, E. The
probability that
colliding
molecules will
react
a. increa
ses
with
increa
sing
energ
y of
activa
tion.
b. depends only
on the

empirical
constant, A.
c. increases with
decreasing
temperature.
d. decrea
ses
with
increa
sing

energy of
activatio
n.
69.

The rate law for the
reaction A+BC+D is
first order in [A] and
second order in [B]. If
[A] is halved and [B]
is doubled, the rate of
the reaction will
a.
b.
c.
d.

70.

remain the same
be increased by a
factor of 2.
be increased by a
factor of 4.
be increased by a
factor of 8.

The addition of a
catalyst in a
chemical reaction
a. increases the
concentration
of products at
equilibrium.
b. increases the
fraction of
reactant
molecules with a
given kinetic
energy.
c. provides an
alternate path
with a different
activation
energy.
d. lowers the
enthalpy
change in the
overall

reaction.


c.
d.

AlBr C6H6CH2CH
+

72.

Which
substanc
e has the
highest
boiling
point?

proceeds by
this
mechanism:
2A  A2
(equilibrium)
A
2

+
B

a.

b.
c.
d.
73.

74.

CH4
He
HF
Cl2

The
table
presents
data for the
reaction:
The
temperature
of
the
reaction is
constant.
The initial
rate is in
arbitrary
units.
2H2(g)
2NO(g)
2H2O(g)

N2(g)


X
+
C
(
r
a
t
e

d
e
t
+
e

r
+
m
i
n
Initial Concentration i
Exp. [NO] x 10-3 [H
n
I
6.0
1.0
g

II
6.0
2.0
)
III
1.0
6.0
X
IV
2.0
6.0
+
B

What is the rate
law for this
D
reaction?
a. rate = k1
(
[H2][NO]
r
b. rate = k1
a
[H2]2 [NO]2
p
c. rate = k1
i
[H2]2 [NO]
d

d. rate = k1
)
[H2] [NO]2
The rate equation for
the reaction is
The
reaction 2A
a. rate = k[A] [B]
+ 2B  C
b. rate = k[A]2
[B]2/[C][D]
+D

c.

rate =4 k[A]2
[B]2[D]

d.
3

rate = k[A]2 [B]


75.

What is the correctly reported mass of
water based on this data?

a.

Mass of beaker and water
29.62 g
Mass of beaker only 28.3220 g

b.

a.
b.
c.
d.
76.

c.
d.
e.

80.

the metal is less dense than the acid.
the metal gets hot and expands and
decreases its density markedly as it reacts
with the acid
the magnesium sulfate formed increases the
density of the solution.
gas bubbles attached to the metal buoy the
metal to the top.
convection currents set up in the acid carry
the metal to the top.

The stronger the intermolecular forces in a
substance
a.
b.
c.
d.

81.

a.
b.
c.
d.
82.

HF>H2>NaF
NaF>H2>HF
HF>NaF>H2
NaF>HF>H2

The fact that H2O has a dipole moment
suggests that the water molecule is
a.
b.
c.
d.

65.4
92.0
184

238

the higher the boiling point.
the lower the boiling point.
the higher the vapor pressure.
the smaller the deviation from ideal gas
behavior.

Which group of substances is correctly
arranged in order from the highest to the lowest
melting point?

the mass of the liquid.
the surface area of the liquid
the temperature only
the volume of the liquid

The edge of a unit cube of an element Y,
containing two atoms per unit cube, was found
(by X- ray diffraction) to be 3.16 x 10-8 cm. The
density of the metal is 19.35 g/cm3. What is the
approximate atomic molar mass of Y?
a.
b.
c.
d.

79.

d.

e.

The equilibrium vapor pressure of a few liters
of a liquid is dependent on
a.
b.
c.
d.

78.

1.3g
1.30g
1.298g
1.2980g

When a small single piece of magnesium ribbon
is dropped into a test tube half filled with dilute
sulfuric acid, the metal soon floats to the
surface of the liquid. The best explanation for
this is that, (Densities, Mg, 1.79 g/cm3;
H2SO4(dilute) 1.2 g/cm3)
a.
b.

77.

c.

the electron affinity of X is small in

magnitude and the ionization potential of M
is large in magnitude.
the heat of vaporization of crystalline M is
small.
the heat of vaporization of crystalline M is
large.
the effective radii of M+ and X- are large.
the effective radii of M+ and X- are small.

83.

dimeric
symmetrical.
bent.
nonpolar.
Which pair is geometrically similar?

a.
b.
c.
d.

SO2 and CO2
CO2 and OF2
PH3 and BF3
SO2 and O3

84.
The bond type and molecular polarity of
SiCl4 are

+

-

When a hypothetical ionic crystal M X is
heated, it vaporizes to form separate M+(g) and
X-(g) ions. The energy required for this
vaporization (the lattice energy) will be greatest
when

a.
b.
c.
d.

Bond Type
polar
polar
nonpolar
nonpolar

Polarity of Molecule
nonpolar
polar
polar
nonpolar


85.

The fact that BCl3 is a planar molecule while
NCl3 is pyramidal can be explained several
different ways. Which is the best rationalization?
a.
b.
c.
d.

86.

Nitrogen is more electronegative than
boron.
The nitrogen atom in NCl3 has a lone
pair of electrons whereas the boron atom
in BCl3 does not.
The nitrogen atom is smaller than the boron
atom
The boron atom in BCl3 is sp3
hybridized, while the nitrogen atom in
NCl3 is sp2 hybridizes

The geometry for SeF + is
a. trigonal pyramidal.
b. tetrahedral.
c. square planar.
d. rectangular planar.

isotope?
a.

b.
c.
d.
91.

Which of these molecules is the most polar?
(X and Y are two different elements, Y being
the more electronegative.)
a.
b.
c.
d.

X2
Y2
X—Y—X
X—Y
X
X
e.
Y—X
X

3

92.
87.

4 days
8 days

12 days
16 days

The Lewis structure of BrF5 is
F
F
F
Br
F
F

In the beta emission of a species such as
14
6C the process may be considered as
a.
b.
c.
d.

the change of a proton into a neutron.
the change of a neutron into a proton.
the same mode of decay as electron capture.
neutrino absorption by the nucleus.

The molecular structure of BrF5 is
a.
b.
c.
d.
88.

90.

93.

PCl3
ClO3CO32NH3
PH3

A molecule of the type ML4 consists of four
bonding pairs of electrons and no lone pairs.
Which structure would it be expected to assume?
a. square planar
b. tetrahedral
c. linear
d. square pyramidal
A sample of a radioactive isotope initially
contains 20 x 1010 atoms. After 16 days, 5 x 1010
atoms remain. What is the half-life of the

Which compound is a paraffin (methane
series) hydrocarbon?
a.
b.
c.
d.
e.

Which is planar?
a.

b.
c.
d.
e.

89.

square pyramidal.
trigonal pyramidal.
trigonal bipyramidal.
octahedral.

94.

lsobutane differs from butane in that the
former
a.
b.
c.
d.
e.

95.

C5H12
C5H11OH
(C2H5)2O
C6H6
C6H5Cl

has a higher molecular weight.
has a different percentage composition.
is not a saturated hydrocarbon.
has a different empirical formula.
has a different structural formula.

Which has the highest boiling point?
a.
b.
c.
d.

n-butane C4H10
n-heptane C7H16
n-hexane C6H14
n-pentane C5H12


General Chemistry II Sample Test bank

96.

Page 14of 27

The reaction between acetic acid and ethyl
alcohol is classified as

the magnesium acts as a reducing agent. How
many electrons does each magnesium atom
lose?

CH3COOH + C2H5OH  CH3COOC2H5 + H2O
97.
a.
b.
c.
d.

saponification
addition
esterification
hydrolysis
Manganese has the oxidation number of +5

most polarizable?
a. 1
b. in 2
c. 3
a. Na+
3b. O2d. a.4 [MnF6]
c. Fe. b.6 Mn2O7
c. [MnO4]2d. Mg2+
1102. d.Which
of these
[Mn(CN)
6] isoelectronic ions is the
103.

98.

The highest
oxidation number
of vanadium is
exhibited in
a.
b.
c.
d.
e.

6

99.

VO2+
VBr4
NH4VO3
V2(SO4)3
V(CN) 3—
Fe(s) +
Cu2+ (aq)
 Cu(s) +
Fe2+ (aq)
Which
statement
is true for
the
reaction?

a.

b.
c.
d.
100.

The greatest
oxidizing
power
(tendency to
gain
electrons) is
shown by

a.
b.
c.
d.
104.

Cu2+ is
oxidized.
Cu2+ gains in
oxidation
state.
Cu2+ is
reduced.
Fe(s) is
reduced.

Standard Potentials

Na Na+ + e
Al  Al3++3e
Sn2+Sn4++2e
21—  l2+2e
2F—F2 + 2e
Na+
Al
Sn4+
F2

Which metal
will reduce
copper(ll) ions
but not zinc
ions?

Which is the
strongest
oxidizing
agent?

Standard Potentials
Na  Na+ + e
Cd  Cd2+ + 2e
H2  2H+ + 2e
Ag Ag+ + e

Eo
2.71 V
0.40 V

0.00 V
-0.80 V

o
E
2.7
1.6
-0.1
-0.5
-2.8


General Chemistry II Sample Test bank

a.
b.

Na
c. + Cd0
Hd.2 Ag+
101.
In this
reaction
3Mg +
2HNO3(dilute) +
6H 3Mg2+ +
2NO + 4H2O

a.
b.

c.
d.

Na
Hg
Pb
Ag

Standard Potentials
Na  Na+ +e
Zn  Zn2++2e
Fe  Fe2+ + 2e
Pb  Pb2++2e
H2  2H++ 2e
Cu  Cu2++2e
Hg  Hg2++2e
Ag  Ag+ +e

o
E
2.71 V
0.76 V
0.4 V
0.13 V
0.00 V
-0.34.V
-0.85 V
-0.80 V

Page 15of 27

105.

A metal, M, forms an oxide of formula M2O3.
The ground state valence shell electron
configuration of the M atom is
a.
b.
c.
d.

106.

109.

Based on their positions in the periodic table,
which is most likely to replace selenium, Se,
in a biological system?
a. Te
b. Br
c. As
d. I

113.

Which conditions favor the high solubility of a
gas in a liquid?
a. high pressure, high temperature
b. high pressure, low temperature

c. low pressure, high temperature
d. low pressure, low temperature

114.

Ionic compounds in the solid state at room
temperature are generally characterized by their
a. ability to conduct an electric current.
b. high vapor pressures.
c. solubility in polar solvents.
d. solubility in nonpolar solvents.
e. low melting points.

115.

Which precipitate will not dissolve in
aqueous HCl solution?
a. AgBr
b. BaCO3
c. CaSO3
d. Fe(OH)3
e. ZnS

116.

A cellophane bag, which acts as a membrane
permeable only to water, contains a 2 M sugar
solution. The bag is immersed in a 1 M sugar
solution. What will happen?

A3N
A3N2
AN
AN2

In which pair of particles is the first
member larger than the second member?
a.
b.
c.
d.

Li+ ; Be2+
Li+ ; Na+
Li+ ; Li
Be ; Mg

Which would be expected to be the most
electronegative?
a.
b.
c.
d.

P
As
Si
Al

a.

110.

Predict which element would have the largest
difference between its first and second
ionization energies.
a. Sodium
b. Phosphorus
c. Silicon
d. magnesium

NaCl(crystal) + energy  Na+(g) + Cl—(g)
Cl(g) + energy Cl+ + e
Cl(g) + e  Cl—(g) + energy
Cl— g) + H+(g)  HCl(g) + energy

112.

Use this section of a periodic table.
A
E
Q
R
If atoms of R have one “d” type electron, what
is the formula for a nitride of element A?
a.
b.
c.
d.

108.

ns np
np6
4s13d10
4f7

GaSe
GaSe2
Ga2Se
Ga2Se3

In which reaction is the energy term
referred to as the ionization energy?
a.
b.
c.
d.

1

From your knowledge of the periodic nature
of the elements, what formula would be
anticipated for gallium selenide?
a.
b.
c.
d.

107.

2

111.

b.
c.
d.
e.

The bag will soon contain more solution
that will be are concentrated than 2 M.
The bag will soon contain more solution
that will be less concentrated than 2 M.
The bag will lose sugar and the solution in
it will become less concentrated.
The bag will lose water and the solution in
it will become more concentrated.
There will be no change.


117.

a.
b.
c.
d.
118.

4.00x10–3 m
5.00x10–2 m

5.00 x 10–3 m
4.00 x 10–1 m

123.

What is the mole fraction of water in 200. g of
95% (by mass) ethanol, C2H5OH (mw = 46.0
g/mol)?
a.
b.
c.
d.

119.

a.
b.
c.
d.
e.

If 0.400 g of a substance R (MW = 80.0 g/mol)
is dissolved in 100 g of liquid Q, what is the
molality of the solution?

0.050
0.12
0.56
0.88

When dilute aqueous solutions of lead(II)
nitrate and potassium bromide are mixed, a
precipitate is observed. The products of this
reaction are
a.
b.
c.
d.

124.

A 0.10 m aqueous solution of HF shows a
freezing point of - 0.198 oC. What is the percent
dissociation of HF? Molal freezing point

40 g./mol
200 g/mol
100 g./mol
400 g/mol
128 g./mol

Pb2+(aq) + Br 1- (aq) + KNO3(s)
Br2(aq) + NO2(g) + PbK2(s)
PbO(s) + K+(aq) + Br1-(aq) + NO2(g)
PbBr2(s) + K+(aq) + NO3 1-(aq)

Assuming ideal behavior, what is the vapor
pressure of a solution of 16.0 mol of carbon
tetrachloride and 4.00 mol of dioxane at 23 oC?
constant, Kf for water = 1 .86 oC/m

a.
b.
c.
d.

6.4%
10%
20%
98%

120.
A 0.10 m solution of MgSO4 freezes
at -0.245oC instead
of 2 x (- 0.186 oC)
122.
When one mole of
as predicted for
naphthalene is
ideal behavior. This
dissolved in 1000 g of
deviation from
benzene, the freezing
ideality can best be
point changes from
explained on the
5.51 oC to 0.41 oC.
basis of
When 20 g of an
unknown organic
a. interionic

compound is dissolved
attraction.
in 500 g of benzene,
b. hydrogen
the freezing point of
bonding.
this solution is
c. the Le
5.00 oC. What is the
Chatelier
molar mass of the
principle.
unknown organic
d. the solubility
compound?
product
constant
121.

Which aqueous
solution has the
smallest freezing
point
depression?
a.
b.
c.
d.

0.2 m Ca(NO3)2

0.2 m MgSO4
0.2 m CH3OH
0.2 m K3PO4

a.
b.
c.
d.


125.

b.
c.
d.

What
is the
empi
rical
form
ula
for
the
subst
ance
with
this
analy
sis:

Na=5
4.0%
,
B=8.
50%,
O=3
7.5%
a.

126.

Na3BO3

Na4BO4
Na2B2O3
NaB2O2

A
hydrocarbon
undergoes
complete
combustion
to give 0.44g
of CO2 and
0.27 g of
H2O. What is
the simplest
(empirical)
formula of
the

hydrocarbon?
a.
b.
c.
d.

C44H27
CH4
C2H3
CH3


127.

128.

A 6.80 g coin was dissolved in nitric acid and
6.21 g of AgCl was precipitated by the addition
of excess sodium chloride, Calculate the
percentage silver in the coin.
Ag+(aq) + Cl1-(aq) AgCl(s)
a. 24.7%
b. 68.7%
c. 75.3%
d. 91.3%

133.

Which change is likely to be accompanied by
the greatest increase in entropy?

a.
b.
c.
d.

134.

A 40- mL portion of a 0.1 M MgSO4 solution
contains how many grams of MgSO4?
a. 120 g

N2(g) + 3H2(g)  2NH3(g) (at 25 oC)
Ag+(aq) + Cl1-(aq)  AgCl(s) (at 25 oC)
CO2(s)  CO2(g) (at - 70 oC)
H2O(g)  H2O(l) (at 100 oC)

When 45.0 g of an alloy at 100.0 oC is dropped
into 100.0 g of water at 25.0 oC the final
temperature is 37.0 oC. What is the specific heat
of the alloy? (for water, specific heat = 4.184 J g1o

-1
b.C )24 g
c. 0.96 g
d. 0.6 g
e. 0.48 g

a.
b.
c.

d.

129.
An aqueous solution containing 49 g of
135.
d. 112
sulfuric acid per
liter has a
132.
What volume of ammoni
concentration of
a. 0.50 M
measured at STP, will
b. 1.0M
be produced by the
c. 4.9% by
decomposition of two
mass
moles of ammonium
d. 4.9M
carbonate?
(NH4)2CO3(s) 
130.
One hundred
2NH3(g) + CO2(g) +
milliliters of a
H2O(g)
solution of oxalic
a. 22.4 L
acid, (COOH)2, is

b. 33.6 L
neutralized with
c. 44.8 L
50.0 mL of 0.750
d. 89.6 L
M KOH solution.
e. 112 L
What is the
molarity of the
oxalic acid
solution?
a. 0.099 M
b. 0.375 M
c. 0.188 M
d. 0.750 M
e. 0.333 M
131.

How many L of
CO2 gas at STP
can be obtained
by burning one
mole of C3H8?
C3H8(g) + 5
O2(g) 3 CO2(g)
+ 4H2O(g)
a. 11.2
b. 44.8
c. 67.2

combustion of
C2H6 in kJ mol1
?

rived
from
coolin
g one
gram
of
steam
at 100
o
C to
water
at 50
o
C
than
from
coolin
g one
gram
of
liquid
water
at 100
o
C to

50 oC
becau
se

Reaction
H2(g) + ½ O2(g)  H2
C2H4(g) + H2(g)  C
C2H4(g) + 3 O2(g) 2 CO
H2O(g)

a.
b.
c.
d.
136.

–1275 kJ
–31561 kJ
–1558 kJ
+1834 kJ
Given
these
equations

SO2(
g) 
O2(g)
+
S(s)
∆Ho

=
+300
kJ
2SO2
(g) +
O2(g)

2SO3
(g)
∆Ho
=200
kJ

a.
b.
c.

calculate the
heat of
formation of
SO3(g).
a. –500
kJ.mol-1
b. +100
kJ.mol-1
c. –400
kJ.mol-1
d. +200
kJ.mol-1
137.

M
or
e
he
at
is
de

d.

water is a
poor thermal
conductor.
the steam is
hotter than
the water.
the
stea
m
occu
pies
a
great
er
volu
me
than
the
water

.
the
densi
ty of
water
is
great
er
than
that
of

stea
m.

e.

the heat of
condensation is
evolved.


138.

Calculate the value of (in kJmol-1) for the
reaction

142.

N2(g) + 3H2(g) 2NH3(g)

Bond Energies
H—H
N=N
N—H

Which nuclear equation is properly
balanced?
a. 4He + 9Be  12C + 1H
b. 4He + 14N  17O + 1H
c. 4He + 24Mg  27Si + 1H

(kJ. mol-1)
435
946 (in N2)
389

d.

-1

14

N
+ 0 e

14
O
143.
What is the correct reading for the buret? 32
a.

b.
c.
d.

139.

140.

2340 kJ of heat
absorbed
213 kJ of heat
absorbed
2340 kJ of heat
evolved
83 kJ of heat
evolved

When Al2O3(s) is
formed from the
elements at standard
conditions, the
values of ∆Ηo and
∆Go at 298 K are
-1617 kJ.mol-1 and
-1577 kJ.mol-1,
respectively. The
standard entropy of
formation per mole,
in joules per degree,
will be

a. -315
b. -134
c. - 93.3
d. 0.0933
e. +15.7
Vaporization of a
liquid is an
example of a
process for which
a. ∆H,
∆S,
and
∆G
are
posit
ive
at all

b.
c.

d.
141.

tempera
tures.
∆H and ∆S are
positive.
∆G is
negative

at low
temperat
ures,
positive
at high
temperat
ures.
∆H=∆S

Consider the
boiling point of a
series of hydrogen
compounds. The
abnormally high
boiling point for
water is due to


33
a.
b.
c.
d.
144.

a.

32 mL
32.2 mL
32.26 mL

33.74 mL

e
m
pe
ra
tu
re
s.
b.

A
particular
chemical
reaction
has a
negative
∆H and
negative
∆S. Which
statement
is correct?
T
h
e
r
e
a
c
t

i
o
n
i
s
s
p
o
n
t
a
n
e
o
u
s
a
t
a
l
l
t

c.

T
h
e
r
e

a
c
ti
o
n
i
s
n
o
n
s
p
o
n
t
a
n
e
o
u
s
a
t
a
ll
t
e
m
p
e

r
a
t
u
r
e
s
.
T
h
e
r
e
a
ct

d.

io
n
be
co
me
s
sp
on
tan
eo
us
as

te
m
pe
rat
ur
e
inc
rea
ses
.
Th
e

reacti
on
beco
mes
spont
aneo
us as
temp
eratur
e
decre
ases.
145.

Which line in
the diagram
represents the

activation
A energyDfor a
forward
reaction?

B
a.
b.
c.

A
B
C

E
C

BP
d.
D

Reaction
Coordinate

H2O
H2S
H2Se
H2Te
a.
b.

c.

d.

extensive
hydrogen
bonding
its low
dipole
moment.
the extreme
stability of
the
compound.
the high
electronegat
ivity of
hydrogen.

H
146.

The group —C=O is
characteristic of
a. aldehydes.
b. ketones.
c. alcohols
d. esters
e. acids

147.

Uranium—234 undergoes spontaneous
radioactive decay to give an alpha particle and a
new nucleus, X.
U  4He + X

234

What is X?

150.
Consider the phase diagram of a pure
compound. Which statement applies?
a. 230 U
90
b. 230 Th
P
90
c. 238 U
238 94
d.
Pu
AC
94

148.

a.

b.
c.

d.

Which
is
classifi
ed as
an
alkene
?
O

B

CH3—
CH2—
C—H
CH3C
H2CH3
CH3—
C=C
H
CH2
HC
CH2
H
C
C

H
2

C
H
2

149.

a.

An
exampl
e of an
organi
c acid
is
O
CH3C
H2CO
CH3
O

b.

CH3CH2COH
O

c.

CH3CH2CNH2
O

d.

CH3 CH2CH


o
u
l
d

Temper
ature
a.

b.

The
pat
hA
C
repr
ese
nts
subl
ima
tion
.

f
i
r
s
t
l
i
q
u
e
f
y

F
o
l
l
o
w
i
n
g

a
n
d
t
h
e

n

t
h
e
p
a
t
h
A

B

C
t
h
e
c
o
m
p
o
u
n
d
w

c.

v

a
p
o
r
i
z
e
.
I
f
t
h
e
c
o
m
p
o
u
n
d
i
s
i
n
s
t
a

te

A
,
c
o
nt
in
u
e
d
re
d
u
ct
io
n
of
th
e
pr
es
su
re
(a
t
c
o
ns
152.

d.

151.

a.
b.

c.
d.
e.

Which is the
formula of an
alcohol?
CH3CH2CH2 —
O—CH3
CH3CH2CH2C
H2 – O H
O

c.

CH3 CH2 —C
—CH3
O

d.

CH3CH2CH2C
—H

Which choice best indicates the degree
of correctness of this statement? “The
boiling point of normal propanol is
lower than the boiling point of
turpentine.”

Temperature
n-propanol
Water
Turpentine
a.
b.

tant
temp
eratu
re)
will
cause
it to
melt.
None of these
statements is
correct.

0oC
3.4
4.6
2.1

Vapor Pressure of Substances in mm
20oC
50oC
80oC
95oC
14.5
87.2
376
697
17.6
92.0
354.9
4.4
17.0
61.3

The statement is true.
The statement is probably true; additional data
would be needed for a final decision.
It is impossible to judge the statement because the
data are insufficient.
The statement is probably false; additional data
would be needed for a final decision.
The statement is false.


153.

For the reaction 2H2O2 2H2O +O2 Which plot confirms that the rate is first order with respect to
H2O2?

a.

b.

[H2O2]

d.

[H2O2]2

1/[H2O2]
time

154.

c.

time

log[H2O2]
time

time

Sulfur dioxide can be described by the structures:
S
O

S
O

O

O

This implies that
a.
b.
c.
d.
155.

the two bonds in SO2 are of equal length, and the electronic distribution in the two SO bonds is
identical.
the single bond is longer than the double bond and the electronic distribution in the two SO bonds is
different.
an electron pair in the SO2 molecule alternates back and forth between the two sulfur— oxygen
electron pairs so that the two different bonds seem to exchange positions.
the SO2 molecule revolves so that the two different bonds seem to exchange positions.
The graph shows how the vapor pressure of liquid A and of liquid B changes with the temperature.
Select the choice that best indicates the degree of correctness of this statement: “The normal boiling
point of liquid B is 78 0C.”

1000
900
Va 800
po
r
pr
es

su
re
m
m

A

600

B

400
300
200
100
0

20

40

60

80

100

120

Temperature oC

a.
b.
c.
d.
e.

The statement is true.
The statement is probably true; additional data would be needed for a final decision.
It is impossible to judge the statement because data are insufficient.
The statement is probably false; additional data would be needed for a final decision.
The statement is false.