1. Which statement describes the particles of an ideal
gas based on the kinetic molecular theory?
A) The gas particles are relatively far apart and have
negligible volume.
B) The gas particles are in constant, nonlinear
motion.
C) The gas particles have attractive forces between
them.
D) The gas particles have collisions without
transferring energy.
2. A sample of a gas is contained in a closed rigid
cylinder. According to kinetic molecular theory, what
occurs when the gas inside the cylinder is heated?
A) The number of gas molecules increases.
B) The number of collisions between gas molecules
per unit time decreases.
C) The average velocity of the gas molecules
increases.
D) The volume of the gas decreases.
3. An assumption of the kinetic theory of gases is that
the particles of a gas have
A) little attraction for each other and a significant
volume
B) little attraction for each other and an
insignificant volume
C) strong attraction for each other and a significant
volume
D) strong attraction for each other and an
insignificant volume
6. A cylinder with a tightly fitted piston is shown in the
diagram below.
As the piston moves downward, the number of
molecules of air in the cylinder
A) decreases
C) remains the same
B) increases
7. What volume will a 300.-milliliter sample of a gas at
STP occupy when the pressure is doubled at constant
temperature?
8. When a base is dissolved in water it releases
A) hydrogen ions
C) hydroxide ions
B) hydronium ions
D) oxide ions
9. A base reacts with an acid to produce
A)
B)
C)
D)
ammonia and methane
ammonia and a salt
water and methane
water and a salt
10. What are the relative ion concentrations in an acid
solution?
A)
B)
C)
D)
more H + ions than OH – ions
fewer H+ ions than OH – ions
an equal number of H + ions and OH– ions
H+ ions but no OH – ions
4. A cylinder with a movable piston contains a sample of 11. The OH– ion concentration is greater than the H + ion
concentration in a water solution of
gas having a volume of 6.0 liters at 293 K and 1.0
atmosphere. What is the volume of the sample after
A) CH 3OH
B) Ba(OH) 2
the gas is heated to 303 K, while the pressure is held
C) HCl
D) H2SO 4
at 1.0 atmosphere?
12. Which solution reacts with LiOH(aq) to produce a
5. Which two samples of gas at STP contain the same
salt and water?
total number of molecules?
A) KCl(aq)
B) CaO(aq)
A) 1 L of CO(g) and 0.5 L of N2(g)
C) NaOH(aq)
D) H2SO 4(aq)
B) 2 L of CO(g) and 0.5 L of NH 3(g)
13. The attraction between water molecules and an Na +
C) 1 L of H2(g) and 2 L of Cl2(g)
ion or a Cl– ion occurs because water molecules are
D) 2 L of H2(g) and 2 L of Cl2(g)
A) linear
B) symmetrical
C) polar
D) nonpolar
14. Under which conditions of temperature and pressure
is a gas most soluble in water?
A)
B)
C)
D)
high temperature and low pressure
high temperature and high pressure
low temperature and low pressure
low temperature and high pressure
15. At room temperature, the solubility of which solute
in water would be most affected by a change in
pressure?
A) methanol
C) carbon dioxide
B) sugar
D) sodium nitrate
16. The molarity of an aqueous solution of NaCl is
defined as the
A)
B)
C)
D)
grams of NaCl per liter of water
grams of NaCl per liter of solution
moles of NaCl per liter of water
moles of NaCl per liter of solution
17. What is the molarity of 1.5 liters of an aqueous
solution that contains 52 grams of lithium fluoride,
LiF, (gram-formula mass = 26 grams/mole)?
18. Which preparation produces a 2.0 M solution of C 6H
12O 6 ? [molecular mass = 180.0]
A) 90.0 g of C 6H12O6 dissolved in 500.0 mL of
solution
B) 90.0 g of C 6H12O6 dissolved in 1000. mL of
solution
C) 180.0 g of C 6H12O6 dissolved in 500.0 mL of
solution
D) 180.0 g of C 6H12O6 dissolved in 1000. mL of
solution
19. A barium atom attains a stable electron configuration
when it bonds with
A)
B)
C)
D)
one chlorine atom
two chlorine atoms
one sodium atom
two sodium atoms
A)
B)
C)
D)
22. Based on electronegativity values, which type of
elements tends to have the greatest attraction for
electrons in a bond?
A) metals
C) nonmetals
B) metalloids
D) noble gases
23. The bonds in BaO are best described as
A) covalent, because valence electrons are shared
B) covalent, because valence electrons are
transferred
C) ionic, because valence electrons are shared
D) ionic, because valence electrons are transferred
24. What is the total number of electrons shared in a
double covalent bond?
A) 1
B) 2
C) 3
D) 4
25. Which two substances are covalent compounds?
A)
B)
C)
D)
C6 H12 O6 (s) and KI(s)
C6 H12 O6 (s) and CO 2(g)
KI(s) and NaCl(s)
NaCl(s) and HCl(g)
26. Covalent bonds are formed when electrons are
A)
B)
C)
D)
transferred from one atom to another
captured by the nucleus
mobile within a metal
shared between two atoms
27. Which type of bond is found between atoms of solid
cobalt?
20. When a sodium atom reacts with a chlorine atom to
form a compound, the electron configurations of the
ions forming the compound are the same as those in
which noble gas atoms?
A) krypton and neon
C) neon and helium
21. Which is the correct electron-dot formula for a
molecule of chlorine?
B) krypton and argon
D) neon and argon
A) nonpolar covalent B) polar covalent
C) metallic
D) ionic
28. A solid substance is an excellent conductor of
electricity. The chemical bonds in this substance are
most likely
A) ionic, because the valence electrons are shared
between atoms
B) ionic, because the valence electrons are mobile
C) metallic, because the valence electrons are
stationary
D) metallic, because the valence electrons are
mobile
29. An atom in the ground state has two electrons in its
first shell and six electrons in its second shell. What
is the total number of protons in the nucleus of this
atom?
A) 5
B) 2
C) 7
D) 8
30. An ion that consists of 7 protons, 6 neutrons, and 10
electrons has a net charge of
A) 4–
B) 3–
C) 3+
D) 4+
31. Every chlorine atom has
A)
B)
C)
D)
7 electrons
17 neutrons
a mass number of 35
an atomic number of 17
A) total mass of all the protons and neutrons in an
atom of Ti
B) total mass of all the protons, neutrons, and
electrons in an atom of Ti
C) weighted average mass of the most abundant
isotope of Ti
D) weighted average mass of all the naturally
occurring isotopes of Ti
33. If an element, X, can form an oxide that has the
formula X2O3, then element X would most likely be
located on the Periodic Table in the same group as
B) Cd
C) Al
D) Na
34. Bronze contains 90 to 95 percent copper and 5 to 10
percent tin. Because these percentages can vary,
bronze is classified as
A) a compound
C) a mixture
A)
B)
C)
D)
homogeneous compound
homogeneous mixture
heterogeneous compound
heterogeneous mixture
36. A 1.0-mole sample of krypton gas has a mass of
A) 19 g B) 36 g C) 39 g D) 84 g
37. What is the total number of moles of oxygen atoms
in 1 mole of N 2O3?
A) 1
B) 2
B) an element
D) a substance
C) 3
D) 5
38. What is the total mass of oxygen in 1.00 mole of
Al 2(CrO4) 3?
A) 192 g
C) 64.0 g
B) 112 g
D) 48.0 g
39. What is conserved in the reaction shown below?
N2(g) + 3F2(g)
2NF 3(g)
A) atoms only
C) mass and atoms
32. The atomic mass of titanium is 47.88 atomic mass
units. This atomic mass represents the
A) Ba
35. A sample is prepared by completely dissolving 10.0
grams of NaCl in 1.0 liter of H 2O. Which
classification best describes this sample?
B) mass only
D) moles only
40. How many moles of aluminum are needed to react
completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s)
3Fe(s) + Al2O3(s)
A) 1.2 mol
C) 1.6 mol
B) 0.8 mol
D) 2.4 mol
41. Methane and hydrogen sulfide form when hydrogen
reacts with carbon disulfide. Identify the excess
reagent and calculate how much remains after 36 L
of H reacts with 12 L of CS.
4H2(g) + CS 2(g)
CH 4(g) + 2H 2S(g)
A) 3 L
B) 6 L
C) 9 L
D) 12 L
42. Given the reaction
N2(g) + 3 H2(g) ® 2 NH3(g)
How many liters of ammonia, measured at STP, are
produced when 28.0 grams of nitrogen is completely
consumed?
A) 5.60 B) 11.2 C) 22.4 D) 44.8
43. Which formula represents strontium phosphate?
A) SrPO4
C) Sr 2(PO4) 3
B) Sr 3PO 8
D) Sr 3(PO4) 2
44. What is the chemical formula for iron(III) oxide?
A) FeO
C) Fe 3O
B) Fe 2O3
D) Fe 3O2
45. The formula for nitrogen dioxide is
A) N4O B) N2O2 C) N2O D) NO 2
46. Base your answer to the following question on the information below.
A 1.0-gram strip of zinc is reacted with hydrochloric acid in a test tube. The unbalanced equation
below represents the reaction.
____ Zn(s) + ____HCl(aq) ____H2(g) + ____ ZnCl2(aq)
Balance the equation for the reaction of zinc and hydrochloric acid, using the smallest whole-number
coefficients.
47. Which compound can be classified as an electrolyte?
A)
B)
C)
D)
carbon tetrachloride
sugar
hydrochloric acid
distilled water
A) 3.0 M
C) 0.75 M
49. A gas occupies a volume of 444 mL at 273 K and
79.0 kPa. What is the final kelvin temperature when
the volume of the gas is changed to 1880 mL and the
pressure is changed to 38.7 kPa?
50. Given the equation:
OH–(aq)
NH 3(g) + H 2O( ) -->
+
+
The reactant that donates a H ion in the reaction is
51. What are the products of a reaction between
KOH(aq) and HCl(aq)?
A) H2O and KCl
C) KH and HClO
B) 0.33 M
D) 6.0 M
53. A solution at 25°C with a pH of 7 contains
48. A cylinder with a movable piston contains a sample
of gas having a volume of 6.0 liters at 293 K and 1.0
atmosphere. What is the volume of the sample after
the gas is heated to 303 K, while the pressure is held
at 1.0 atmosphere?
NH 4+ (aq)
52. What is the molarity of an H 2SO 4 solution if 0.25
liter of the solution contains 0.75 mole of H 2SO 4?
B) H2 and KClO
D) KOH and HCl
A)
B)
C)
D)
more H 3O+ ions than OH – ions
fewer H3O+ ions than OH – ions
an equal number of H 3O+ ions and OH– ions
no H3O+ ions or OH – ions
54. What is the correct formula for nitrous acid?
A) H3N
C) HNO2
B) HNO3
D) H2NO 2
55. The products of a neutralization reaction between a
base and an acid are
A)
B)
C)
D)
ammonia and methane
ammonia and a salt
water and methane
water and a salt
56. The attraction between water molecules and a K + ion
or a Br – ion occurs because water molecules are
A) linear
C) polar
B) symmetrical
D) nonpolar
57. The bonds in CaO are best described as
A) covalent, because valence electrons are shared
B) covalent, because valence electrons are
transferred
C) ionic, because valence electrons are shared
D) ionic, because valence electrons are transferred
58. Which formula represents iron(III) phosphate?
A) FePO 4
C) Fe 2(PO4) 3
B) Fe 3PO 8
D) Fe 3(PO4) 2
59. What is the chemical formula for dinitrogen
trioxide?
A) NO
B) N2O3 C) N3O D) N3O2
60. A student tested a 0.1 M aqueous solution and made
the following observations:
• conducts electricity
• turns blue litmus to red
• reacts with Zn(s) to produce gas bubbles
66. An atom of argon rarely bonds to an atom of another
element because an argon atom has
A)
B)
C)
D)
2 electrons in the first shell
8 valence electrons
3 electron shells
22 neutrons
67. The bonds in P 2O5 are best described as
A) covalent, because valence electrons are shared
B) covalent, because valence electrons are
transferred
C) ionic, because valence electrons are shared
D) ionic, because valence electrons are transferred
68. When ionic bonds are formed, metallic atoms tend to
A)
B)
C)
D)
lose electrons and form anions
lose electrons and form cations
gain electrons and form anions
gain electrons and form cations
69. Which substance is not an electrolyte?
Which compound could be the solute in this
solution?
A) NH 3
C) HBr
B) LiBr
D) LiOH
61. Which compounds can be classified as electrolytes?
A)
B)
C)
D)
Carbon tetrachloride
sugar
hydrochloric acid
distilled water
A) True B) False
63. What property of water enables a water strider to
walk on water?
B) High heat capacity
D) Universal solvent
64. Which property of water allows nutrients from food
to be carried by the blood to all of the body's cells?
A) High heat capacity B) Universal solvent
C) Cohesion
D) Adhesion
65. Which formula represent hydroiodic acid?
A) HBr B) HCl
C) HF
70. What is the correct name for NH 4Cl
A)
B)
C)
D)
nitrogen hydrochloric (IV) acid
nitrogen hydrogen choride
ammonium chloride
nitrogen tetrahydrochloride
71. ________ gain electrons and _________ lose
electrons when forming ionic bonds.
62. Always add acid to water when diluting acids.
A) Transparency
C) Cohesion
A) K2O B) CO 2 C) NaCl D) KOH
D) HI
A)
B)
C)
D)
cations; anions
metals; non-metals
anions; cations
none of the above
72. What is the mass in grams of 5.90 mol C 8H18?
A) 0.0512 g
C) 389 g
B) 19.4 g
D) 673 g
73. Which equation represents a decomposition
reaction?
A) CaCO 3(s)
CaO(s) + CO 2(g)
B) Cu(s) + 2AgNO 3(aq)
2Ag(s) + Cu(NO3) 2(aq)
C) 2H2(g) + O 2(g)
2H2O(l)
D) KOH(aq) + HCl(aq)
KCl(aq) + H 2O(l)
74. The total number of molecules in 34.0 grams of NH 3
is equal to
A)
B)
C)
D)
22.4 molecules of NH 3
44.8 molecules of NH 3
6.02 × 10 23 molecules of NH 3
1.20 × 10 24 molecules of NH 3
75. What is the total mass in grams of 0.75 mole of
sulfur dioxide?
A) 16 g B) 24 g C) 32 g D) 48 g
76. A covalent bond is formed when a chemical reaction
occurs between atoms of
A)
B)
C)
D)
chlorine and potassium
chlorine and zinc
oxygen and fluorine
oxygen and magnesium
77. Given the Lewis structure for nitrogen:
What is the total number of electrons shared between
the atoms represented in this diagram?
A) 1
B) 2
C) 4
D) 6
78. Which element consists of positive ions immersed in
a "sea" of mobile electrons?
A) oxygen
C) gold
B) nitrogen
D) chlorine
79. Chlorine gas is bubbled through a solution of sodium
bromide to form bromine gas and sodium chloride.
Which equation represents this reaction?
A)
B)
C)
D)
Cl 2 + 2NaBr --> 2NaCl + Br 2
Cl 2 + 2NaBr --> 2NaCl + 2Br
2Cl + 2NaBr --> 2NaCl + Br 2
Cl + Na2Br --> Na 2Cl + Br
80. The sum of the atomic masses of the atoms in one
molecule of C3H6Br 2 is called the
A)
B)
C)
D)
molar mass
isotopic mass
percent abundance
percent composition
81. Given the unbalanced equation:
When the equation is balanced using the smallest whole-number coefficients, what is the mole ratio
of aluminum to copper?
A)
B)
C)
D)
1 mole of aluminum : 1 mole of copper
2 moles of aluminum : 3 moles of copper
3 moles of aluminum : 2 moles of copper
2 moles of aluminum : 1 mole of copper
82. Given the balanced equation:
86. Given the unbalanced equation:
F2(g) + H 2(g) 2HF(g)
How many grams of HF would be produced if 4
moles of H 2 reacted with excess F 2?
A) 80g HF
C) 40g HF
B) 160g HF
D) 20g HF
83. Based on the equation:
2 Al + 3 Ni(NO 3) 2
A) 6
2 Al(NO 3) 3 + 3 Ni
If 50 grams of Al react with 100 grams of Ni(NO 3) 2,
what is the limiting reactant?
84. Given the unbalanced chemical equation:
K + Br2
KBr
If 100 grams of K react with 100 grams of Br 2, how
many grams of KBr will be formed?
A) 200 grams
C) 149 grams
B) 100 grams
D) 74 grams
85. Given the unbalanced chemical equation:
____ Zn(s) + ____HCl(aq)
ZnCl2(aq)
____H2(g) + ____
If a student began an experiment with 9.74 grams of
zinc and produced an experimental (actual) yield of
0.227 grams of H2, what is the percent yield of H 2?
A) 73.5%
C) 61.3%
When this equation is correctly balanced using
smallest whole numbers, what is the coefficient of O
2 (g)?
B) 2.2%
D) 33.9%
B) 2
C) 3
D) 4
87. Given the balanced reaction:
2 C2H2(g) + 5 O 2(g)
4 CO 2(g) + 2 H 2O(g)
What is the total number of grams of O 2(g) needed
to react completely with 0.50 mole of C 2H2(g)?
A) 10. g
C) 80. g
B) 40. g
D) 160 g
88. Given the balanced reaction:
C6H6 + Br 2
C6H5Br + HBr
If 2 moles of benzene (C 6H6) are combined with 3
moles of bromine, what is the theoretical yield of
HBr?
A) 81 grams
C) 243 grams
B) 162 grams
D) 405 grams
89. Which of the following pH values indicates the
highest concentration of hydrogen ions in a solution?
A) pH = 1
C) pH = 9
B) pH = 5
D) pH = 14
90. When a base is dissolved in water it yields
A) hydrogen ions
C) hydroxide ions
B) hydronium ions
D) oxide ions
91. Base your answer to the following question on the
following balanced equation representing a reaction:
Show your work!!!
2H2 + O2 2H2O
What is the Limiting Reactant/ Reagent if 20 grams
of oxygen with 7 grams of hydrogen to produce
water?
92. According to solubility graph, which compound is
least soluble in water at 60. °C?
A) KClO 3
C) NaCl
B) KNO3
D) NH 4Cl
93. According to the solubility graph, which substance
forms an unsaturated solution when 80 grams of the
substance is dissolved in 100 grams of H2O at 10°C?
A) KI
C) NaNO3
B) KNO3
D) NaCl
94. Which equation represents a single replacement
reaction?
A)
B)
C)
D)
95. Given the balanced equations representing two
chemical reactions:
Cl 2 + 2NaBr
2NaCl + Br2
2NaCl
2Na + Cl2
Which type of chemical reactions are represented by
these equations?
A)
B)
C)
D)
single replacement and decomposition
single replacement and double replacement
synthesis and decomposition
synthesis and double replacement
96. The volume of a sample of a gas at 273°C is 200.
liters. If the volume is decreased to 100. liters at
constant pressure, what will be the new temperature
of the gas?
A) 0 K
C) 273 K
B) 137. K
D) 546 K
97. Which set of values represents standard pressure and
standard temperature?
A)
B)
C)
D)
1 atm and 101.3 K
1 kPa and 273 K
101.3 kPa and 0°C
101.3 atm and 273°C
98. At 25ºC, gas in a rigid cylinder with a movable
piston has a volume of 145 mL and a pressure of 125
kPa. Then the gas is compressed to a volume of 80.
mL. What is the new pressure of the gas if the
temperature is held at 25ºC?
A) 69 kPa
C) 160 kPa
B) 93 kPa
D) 230 kPa
99. A rigid cylinder contains a sample of gas at STP.
What is the pressure of this gas after the sample is
heated to 410 K?
A) 1.0 atm
C) 0.67 atm
B) 0.50 atm
D) 1.5 atm
100. Which graph represents the relationship between
pressure and volume for a sample of an ideal gas at
constant temperature?
A)
B)
C)
D)