Download Practice MSL Multiple Choice 1. Compared to the charge and mass

Practice MSL Multiple Choice
1. Compared to the charge and mass of a proton,
an electron has
a.
b.
c.
d.
the same charge and a smaller mass
the same charge and the same mass
an opposite charge and a smaller mass
an opposite charge and the same mass
2. When alpha particles are used to bombard gold
foil, most of the alpha particles pass through
undeflected. This result indicates that most of the
volume of a gold atom consists of ____.
a.
b.
c.
d.
deuterons
neutrons
protons
unoccupied space
3. A proton has approximately the same mass as
a.
b.
c.
d.
a neutron
an alpha particle
a beta particle
an electron
4. When electrons in an atom in an excited state
fall to lower energy levels, energy is
a.
b.
c.
d.
absorbed, only
released, only
neither released nor absorbed
both released and absorbed
5. A neutron has approximately the same mass as
a.
b.
c.
d.
an alpha particle
a beta particle
an electron
a proton
6. Which symbols represent atoms that are
isotopes?
a.
b.
c.
d.
C-14 and N-14
O-16 and O-18
I-131 and I-131
Rn-222 and Ra-222
7. Which element's ionic radius is smaller than its
atomic radius?
a.
b.
c.
d.
neon
nitrogen
sodium
sulfur
8. Which atom contains exactly 15 protons?
a.
b.
c.
d.
P-32
S-32
O-15
N-15
9. An ion with 5 protons, 6 neutrons, and a
charge of 3+ has an atomic number of
a.
b.
c.
d.
5
6
8
11
10. What is the mass number of an atom which
contains 28 protons, 28 electrons, and 34
neutrons?
a.
b.
c.
d.
28
56
62
90
11. Which three groups of the Periodic Table
contain the most elements classified as metalloids
(semimetals)?
a.
b.
c.
d.
1, 2, and 13
2, 13, and 14
14, 15, and 16
16, 17, and 18
12. Which element has the highest first ionization
energy?
a.
b.
c.
d.
sodium
aluminum
calcium
phosphorus
13. Which compound forms a colored aqueous
solution?
a.
b.
c.
d.
CaCl22
CrCl3
NaOH
KBr
14. When a metal atom combines with a
nonmetal atom, the nonmetal atom will
a.
b.
c.
d.
lose electrons and decrease in size
lose electrons and increase in size
gain electrons and decrease in size
gain electrons and increase in size
15. Which of the following elements has the
smallest atomic radius?
a.
b.
c.
d.
nickel
cobalt
calcium
potassium
16. Which element in Group 15 has the strongest
metallic character?
a.
b.
c.
d.
Bi
As
P
N
17. Which halogens are gases at STP?
a.
b.
c.
d.
chlorine and fluorine
chlorine and bromine
iodine and fluorine
iodine and bromine
18. When combining with nonmetallic atoms,
metallic atoms generally will
a.
b.
c.
d.
lose electrons and form negative ions
lose electrons and form positive ions
gain electrons and from negative ions
gain electrons and form positive ions
19. Which set of elements contains a metalloid?
a.
b.
c.
d.
K, Mn, As, Ar
Li, Mg, Ca, Kr
Ba, Ag, Sn, Xe
Fr, F, O, Rn
20. Atoms of elements in a group on the Periodic
Table have similar chemical properties. This
similarity is most closely related to the atoms'
a.
b.
c.
d.
number of principal energy levels
number of valence electrons
atomic numbers
atomic masses
21. As atoms of elements in Group 16 are
considered in order from top to bottom, the
electronegativity of each successive element
a. decreases
b. increases
c. remains the same
22. What is the concentration of hydroxide ions if
the pH is 3.75?
a.
b.
c.
d.
5.6 x 10-11 M
1.78 x 10-4 M
10.25 M
3.9 M
23. An atom of which of the following elements
has the greatest ability to attract electrons?
a.
b.
c.
d.
silicon
sulfur
nitrogen
chlorine
24. At STP, which substance is the best
conductor of electricity?
a.
b.
c.
d.
nitrogen
neon
sulfur
silver
25. Which metal is obtained commercially by the
electrolysis of salt?
a.
b.
c.
d.
Zn
K
Fe
Ag
26. Which element can be found in nature in the
free (uncombined) state?
a.
b.
c.
d.
Ca
Ba
Au
Al
27. Which of the following is a binary
compound?
a.
b.
c.
d.
hydrogen sulfide
hydrogen sulfate
ammonium sulfide
ammonium sulfate
28. What is the formula for sodium oxalate?
a.
b.
c.
d.
NaClO
Na2ClO
Na2C2O4
NaC2H3O2
29. Given the unbalanced equation:
Al + O2
Al2O3
When this equation is completely balanced using
the smallest whole numbers, what is the sum of
the coefficients?
a.
b.
c.
d.
9
7
5
4
30. What is the empirical formula of the
compound whose molecular formula is P4O10?
a.
b.
c.
d.
PO
PO2
P2O5
P8O20V
31. Which of the following is a binary
compound?
a.
b.
c.
d.
potassium chloride
ammonium chloride
potassium chlorate
ammonium chlorate
32. Which is the correct formula for nitrogen
monoxide?
a.
b.
c.
d.
NO
N2O
NO2
N2O3
33. What is the total number of atoms represented
in the formula CuSO4 . 5H2O?
a.
b.
c.
d.
8
13
21
27
34. What is the gram formula mass of K2CO3?
a.
b.
c.
d.
138 g
106 g
99 g
67 g
35. What is the total number of atoms contained
in 2.00 moles of nickel?
a.
b.
c.
d.
58.9
118
6.02 x 1023
1.2 x 1024
a.
b.
c.
d.
36. What is the percent by mass of oxygen in
magnesium oxide, MgO?
a.
b.
c.
d.
20%
40%
50%
60%
1.5 moles
2.00 moles
6.02 moles
9.03 moles
a.
b.
c.
d.
CH
CH2
CH3
CH4
a.
b.
c.
d.
40. What is the mass in grams of 3.0 x 10
molecules of CO2?
a.
b.
c.
d.
22 g
44 g
66 g
88 g
23
113 g
121 g
149 g
404 g
45. What is the empirical formula of a compound
that contains 85% Ag and 15% F by mass?
a.
b.
c.
d.
2.5
5.0
10
20
1.00 M
2.00 M
3.00 M
4.00 M
44. What is the gram formula mass of
(NH4)3PO4?
a.
b.
c.
d.
39. What is the total number of moles of H2SO4
needed to prepare 5.0 liters of a 2.0 M solution of
H2SO4?
22.4 L Ar
28.0 L of N2
32. 0 L of H2
44.8 L of He
43. What is the molarity of a KF (aq) solution
containing 116 grams of KF in 1.00 liter of
solution?
a.
b.
c.
d.
38. A compound is 86% carbon and 14%
hydrogen by mass. What is the empirical formula
for this compound?
6.89%
14.5%
26.1%
62.9%
42. At STP, 32.0 liters of O2 contain the same
number of molecules as
a.
b.
c.
d.
37. What is the total number of moles of
hydrogen gas contained in 9.03 x 1023 molecules?
a.
b.
c.
d.
41. What is the percent by mass of water in the
hydrate Na2CO3 * 10H2O (formula mass = 286)?
AgF
Ag2F
AgF2
Ag2F2
46. Given the reaction CH4 + 202 --> C02 + 2H20,
What amount of oxygen is needed to completely
react with 1 mole of CH4?
a.
b.
c.
d.
2 moles
2 atoms
2 grams
2 molecules
47. Which formula represents a molecular
substance?
a.
b.
c.
d.
CaO
CO
Li2O
Al2O3
53. Which gas is monatomic at STP?
a.
b.
c.
d.
chlorine
fluorine
neon
nitrogen
54. What Kelvin temperature is equal to 25°C?
48. Which sequence of Group 18 elements
demonstrates a gradual decrease in the strength of
the Van der Waals forces? All the choices are
elements in the liquid state.
a.
b.
c.
d.
Ar, Kr, Ne, Xe
Kr, Xe, Ar, Ne
Ne, Ar, Kr, Xe
Xe, Kr, Ar, Ne
49. Which substance is an example of a network
solid?
a.
b.
c.
d.
nitrogen dioxide
sulfur dioxide
carbon dioxide
silicon dioxide
50. Which combination of atoms can form a polar
covalent bond?
a.
b.
c.
d.
H and H
H and Br
N and N
Na and Br
51. A strontium atom differs from a strontium ion
in that the atom has a greater
a.
b.
c.
d.
number of electrons
number of protons
atomic number
mass number
52. Which bond has the greatest ionic character?
a.
b.
c.
d.
H---Cl
H---F
H---O
H---N
a.
b.
c.
d.
248 K
298 K
100 K
200 K
55. When the external pressure is 101.3 kPa,
water will boil at what temperature?
a.
b.
c.
d.
12.8°C
14.5°C
100°C
18°C
56. As ice cools from 273 K to 263 K, the
average kinetic energy of its molecules will
a. decrease
b. increase
c. remain the same
57. The phase change represented by the equation
I2 (s) ----> I2 (g) is called
a.
b.
c.
d.
sublimation
condensation
melting
boiling
58. The heat of fusion is defined as the energy
required at constant temperature to change 1 unit
mass of a
a.
b.
c.
d.
gas to a liquid
gas to a solid
solid to a gas
solid to a liquid
59. As the pressure of a gas at 2 atm is changed
to 1 atm at constant temperature, the volume of
the gas
a. decreases
b. increases
c. remains the same
60. What is the total number of joules of heat
energy absorbed by 15 grams of water when it is
heated from 30°C to 40°C?
a.
b.
c.
d.
10
63
150
630
61. A compound differs from a mixture in that a
compound always has a
a.
b.
c.
d.
homogeneous composition
maximum of two components
minimum of three components
heterogeneous composition
62. Which substance cannot be decomposed into
simpler substances?
a.
b.
c.
d.
ammonia
aluminum
methane
methanol
63. How many joules are equivalent to 35
kilojoules?
a.
b.
c.
d.
0.035 joules
0.35 joules
3,500 joules
35,000 joules
64. Which statement describes a chemical
property?
a.
b.
c.
d.
Its crystals are a metallic gray.
It dissolves in alcohol.
It forms a violet-colored gas.
It reacts with hydrogen to form a gas.
65. A solution in which the crystallizing rate of
the solute equals the dissolving rate of the solute
must be
a.
b.
c.
d.
saturated
unsaturated
concentrated
dilute
66. A sample of unknown gas at STP has a
density of 0.630 g per liter. What is the gram
molecular mass of this gas?
a.
b.
c.
d.
2.81 g
14.1 g
22.4 g
63 g
67. The heat of fusion of a compound is 30 joules
per gram. What is the total number of joules of
heat that must be absorbed by a 15.0 gram sample
to change the compound from a solid to a liquid at
its melting point?
a.
b.
c.
d.
15 cal
45 cal
150 cal
450 cal
68. How many joules of heat are absorbed when
70.0 grams of water is completely vaporized at its
boiling point?
a.
b.
c.
d.
23, 352
7, 000
15, 813
158, 130
69. Under which conditions are gases most
soluble in water?
a.
b.
c.
d.
high pressure and high temperature
high pressure and low temperature
low pressure and high temperature
low pressure and low temperature
d. potential energy of the products
70. A student investigated the physical and
chemical properties of a sample of unknown gas
and then investigated the gas. Which statement
represents a conclusion rather than an
experimental observation?
a. The gas is colorless.
b. The gas is carbon dioxide.
c. When the gas is bubbled in limewater, the
liquid becomes cloudy.
d. When placed in the gas, a flaming splint
stops burning.
71. A student determined the heat of fusion of
water to be 366.9 J/g. If the accepted value is
333.3J/g, what is the student's percent error?
a.
b.
c.
d.
8.0%
10.0%
15%
30.0%
72. What occurs as potassium nitrate is dissolved
in a beaker of water, indicating that the process is
endothermic?
a.
b.
c.
d.
The temperature of the solution decreases.
The temperature of the solution increases.
The solution changes color.
The solution gives off a gas.
73. To determine the density of an irregularly
shaped object, a student immersed the object in
21.2 milliliters of H2O in a graduated cylinder,
causing the level of the H2O to rise to 27.8
milliliters. If the object had a mass of 22.4 grams,
what was the density of the object.
a.
b.
c.
d.
27.8 g / mL
6.6 g / mL
3.0 g / mL
3.4 g/ mL
74. When a catalyst is added to a system at
equilibrium, a decrease occurs in the
a. activation energy
b. heat of reaction
c. potential energy of the reactants
75. In a chemical reaction, a catalyst changes the
a.
b.
c.
d.
potential energy of the products
potential energy of the reactants
heat of reaction
activation energy
76. Which element is present in all organic
compounds?
a.
b.
c.
d.
carbon
nitrogen
oxygen
phosphorous
77. In which pair of hydrocarbons does each
compound contain only one double bond per
molecule?
a.
b.
c.
d.
C2H2 and C2H6
C2H2 and C3H6
C4H8 and C2H4
C6H6 andC7H8
78. What is the maximum number of covalent
bonds that an atom of carbon can form?
a.
b.
c.
d.
1
2
3
4
79. What is the net ionic equation for the
following:
2Na3PO4 (aq) + 3 CaCl2 (aq)  6 NaCl (aq) +
Ca3(PO4)2 (s)
a.
b.
c.
d.
6Na+(aq) + 6Cl-(aq)  NaCl (aq)
2PO43-(aq) + 3Ca+2(aq)  Ca3(PO4)2(s)
6Na+(aq) + 2PO43-(aq) Ca3(PO4)2(s)
6Cl-(aq) + 3Ca+2NaCl(aq)
80. Which substance functions as the electrolyte
in an automobile battery?
a.
b.
c.
d.
PbO2
PbSO4
H2SO4
H2O
81. Consider the equation, 2H2 + O2 ↔ 2H2O. If
hydrogen was added, in which direction would we
see a shift?
a.
b.
c.
d.
toward left
toward right
toward left and right
no shift
82. What are the spectator ions in the following
equation:
AgNO3(aq) + LiBr(aq) ↔ AgBr(aq) + LiNO3(s)
a.
b.
c.
d.
Ag+(aq) and Br-(aq)
Li+(aq) and NO3-(aq)
Ag+(aq) and NO3-(aq)
Li+(aq) and Br-(aq)
83. If a flask contains 5.90 mL of NH3 at 100 C,
what would the new temperature be if the volume
was changed to 13.7 mL?
a.
b.
c.
d.
0.00115C
0.217C
593C
866C
84. Given the reaction:
2Li(s) + Cl2(g) -> 2LiCl(s)
As the reaction takes place, the Cl2(g) will
a.
b.
c.
d.
gain electrons
lose electrons
gain protons
lose protons.
85. Given the reaction:
__Mg + __Cr3+ -> __Mg2+ + __Cr
When the equation is correctly balanced using
smallest whole numbers, the sum of the
coefficients will be
a.
b.
c.
d.
10
7
5
4
86. How many grams of KCl are needed at STP if
volume is 152mL?
a.
b.
c.
d.
0.00678 g
0.506 g
6.78 g
506 g
87. Which formula represents a salt?
a.
b.
c.
d.
KOH
KCl
CH3OH
CH3COOH
88. Which substance can be classified as an
Arrhenius acid?
a.
b.
c.
d.
HCl
NaCl
LiOH
KOH
89. Which solution will change red litmus to
blue?
a.
b.
c.
d.
HCl(aq)
NaCl(aq)
CH3OH(aq)
NaOH(aq)
90. An acidic solution could have a pH of
a.
b.
c.
d.
7
10
3
14
91. What is the pH of a 0.00001 molar HCl
solution?
a.
b.
c.
d.
1
9
5
4
92. What is the pH of a solution with a
hydronium ion concentration of 0.01 mole per
liter?
a.
b.
c.
d.
1
2
10
14
93. There are alternate acid base theories that
define an acid as any species that can
a.
b.
c.
d.
donate a proton
donate an electron
accept a proton
accept an electron
94. Which 0.1 M solution will turn
phenolphthalein pink?
a.
b.
c.
d.
HBr(aq)
CO2(aq)
LiOH(aq)
CH3OH(aq)
95. As the hydrogen ion concentration of an
aqueous solution increases, the hydroxide ion
concentration of this solution will
a. decrease
b. increase
c. remain the same
96. Which radioactive emanations have a charge
of -1?
a.
b.
c.
d.
neutrons
gamma rays
alpha particles
beta particles
97. As the temperature of a sample of a
radioactive element decreases, the half-life will
a. decrease
b. increase
c. remain the same
98. What kind of radiation will travel through an
electric field on a pathway that remains unaffected
by the field?
a.
b.
c.
d.
a proton
a gamma ray
an electron
an alpha particle
99. Which particle cannot be accelerated in a
magnetic field?
a.
b.
c.
d.
alpha particle
beta particle
neutron
proton
100. In the reaction 4Be9 + X -> 6C12 + 0n1, the X
represents
a.
b.
c.
d.
an alpha particle
a beta particle
an electron
a proton
101. Which substance has chemical properties
similar to those of radioactive 235U?
a.
b.
c.
d.
235
Pa
Pa
233
U
206
Pb
233
102. Which reaction illustrates fusion?
a.
b.
c.
d.
2
2
4
1H + 1H -> 2He
1
27
24
4
0n + 13Al - > 11Na + 2He
27
4
30
1
13Al + 2He -> 15P + 0n
14
4
1
17
7N + 2He -> 1H + 8O
103. Which statement describes characteristics of an endothermic reaction?
a.
b.
c.
d.
The sign of H is positive, and the products have less potential energy than the reactants.
The sign of H is positive, and the products have more potential energy than the reactants.
The sign of H is negative, and the products have less potential energy than the reactants.
The sign of H is negative, and the products have more potential energy than the reactants.
104. Which statement explains why the speed of some chemical reactions is increased when the surface
area of the reactant is increased?
a.
b.
c.
d.
This change increases the density of the reactant particles.
This change increases the concentration of the reactant.
This change exposes more reactant particles to a possible collision.
This change alters the electrical conductivity of the reactant particles.
105. Which conditions will increase the rate of chemical reaction?
a.
b.
c.
d.
decreased temperature and decreased concentration of reactants?
decreased temperature and increased concentration of reactants?
increased temperature and decreased concentration of reactants?
increased temperature and increased concentration of reactants?
106. Which procedure will increases the solubility of KCl in water?
a.
b.
c.
d.
stirring the solute and solvent mixture
increasing the surface area of the solute
raising the temperature of the solvent
increasing the pressure on the surface of the solvent
107. Given the reaction:
Mg(C2H3O2)2 (aq) + K2CO3(aq)  MgCO3 (s) + 2KC2H3O2 (aq)
What is the net ionic equation?
a.
b.
c.
d.
Mg+2(aq) + 2C2H3O2-(aq) MgCO3(s)
2C2H3O2-(aq) + 2K+(aq)  MgCO3(s)
2C2H3O2-(aq) + CO3-2(aq) MgCO3(s)
Mg+2(aq) + CO3-2(aq) MgCO3(s)
108. The following data were collected at the endpoint of a titration performed to find the molarity of an
HCl solution.
Volume of acid (HCl) used = 14.4 mL
Volume of base (NaOH) used = 22.4 mL
Molarity of standard base (NaOH) = 0.20 M
What is the molarity of the acid solution?
a.
b.
c.
d.
1.6 M
0.64 M
0.31M
0.13M
109. In a fusion reaction, reacting nuclei must collide. Collisions between two nuclei are difficult to achieve
because the nuclei are
a.
b.
c.
d.
both negatively charged and repel each other
both positively charged and repel each other
oppositely charged and attract each other
oppositely charged and repel each other
110. A particle accelerator can increase the kinetic energy of
a.
b.
c.
d.
an alpha particle and a beta particle
an alpha particle and a neutron
a gamma ray and a beta particle
a neutron and a gamma ray
111. Which solution is the most concentrated?
a.
b.
c.
d.
1 mole of solute dissolved in 1 liter of solution?
2 moles of solute dissolved in 3 liters of solution?
6 moles of solute dissolved in 4 liters of solution?
4 moles of solute dissolved in 8 liters of solution?
112. Under the same conditions of temperature and pressure, a liquid differs from a gas because the
particles of the liquid
a.
b.
c.
d.
are in constant straight-line motion
take the shape of the container they occupy
have no regular arrangement
have stronger forces of attraction between them
113. The volume of a given mass of an ideal gas at constant pressure is
a.
b.
c.
d.
directly proportional to the Kelvin temperature.
directly proportional to the Celsius temperature.
inversely proportional to the Kelvin temperature.
inversely proportional to the Celsius temperature.
114. How are the boiling and freezing points of a sample of water affected when salt is dissolved in the
water?
a.
b.
c.
d.
The boiling point decreases and the freezing point decreases.
The boiling point decreases and the freezing point increases.
The boiling point increases and the freezing point decreases.
The boiling point increases and the freezing point increases.
115. A solid is dissolved in a beaker of water. Which observation suggests that the process is endothermic?
a.
b.
c.
d.
The solution gives off a gas.
The solution changes color.
The temperature of the solution decreases.
The temperature of the solution increases.
116. Salt A and salt B were dissolved separately in 100 mL beakers of water. The water temperatures were
measured and recorded as shown in the table below:
Salt A: initial water temp. 25.1°C final water temp. 30.2°C
Salt B: initial water temp. 25.1°C final water temp. 20.0°C
Which statement is a correct interpretation of these data?
a.
b.
c.
d.
The dissolving of only salt A was endothermic.
The dissolving of only salt B was exothermic
The dissolving of both salt A and salt B was endothermic.
The dissolving of salt A was exothermic and the dissolving of salt B was endothermic.
117. Which statement explains why the element carbon forms so many compounds?
a.
b.
c.
d.
Carbon atoms combine readily with oxygen.
Carbon atoms have very high electronegativity.
Carbon readily forms ionic bonds with other carbon atoms.
Carbon readily forms covalent bonds with other carbon atoms.
118. When HCl(aq) is exactly neutralized by NaOH(aq), the hydrogen ion concentration in the resulting
mixture is
a.
b.
c.
d.
always less than the concentration of the hydroxide ions
always greater than the concentration of the hydroxide ions
always equal than the concentration of the hydroxide ions
sometimes greater and sometimes less than the concentration of the hydroxide ions
119. A student wishes to prepare approximately 100 milliliters of an aqueous solution of 6M HCl using 12
M HCl. Which procedure is correct?
a.
b.
c.
d.
adding 50 mL of 12 M HCl to 50 mL of water while stirring the mixture steadily.
adding 50 mL of 12 M HCl to 50 mL of water and then stirring the mixture steadily.
adding 50 mL of water to 50 mL of 12 M HCl while stirring the mixture steadily.
adding 50 mL of water to 50 mL of 12 M HCl and then stirring the mixture steadily.
Answer Sheet: Practice MSL
1.______
25._____
49._____
73._____
2.______
26._____
50._____
74._____
3.______
27._____
51._____
75._____
4.______
28._____
52._____
5.______
29._____
53._____
6.______
30._____
54._____
97._____
98._____
99._____
7.______
8.______
9.______
31._____
32._____
33._____
11._____
35._____
59._____
12._____
36._____
60._____
13._____
37._____
61._____
14._____
38._____
62._____
15._____
39._____
63._____
16._____
40._____
64._____
19._____
42._____
43._____
101.____
78._____
102.____
79._____
103.____
80._____
104.____
81._____
105.____
82._____
106.____
83._____
107.____
84._____
108.____
85._____
109.____
86._____
110.____
87._____
111.____
88._____
112.____
89._____
113.____
90._____
114.____
91._____
115.____
92._____
116.____
93._____
117.____
94._____
118.____
95._____
119.____
96._____
120.____
57._____
58._____
18._____
77._____
56._____
34._____
41._____
100.____
55._____
10._____
17._____
76._____
65._____
66._____
67._____
20._____
44._____
68._____
21._____
45._____
69._____
22._____
46._____
70._____
23._____
47._____
71._____
24._____
48._____
72._____
121.____