Download Regents Chemistry - New York Science Teacher

Regents Chemistry
REVIEW - 2
*Questions from NYS Chemistry Regents exams
Kenneth E. Schnobrich
Just a Note
• The questions in Review-2 generally do not
involve reference to a major diagram.
• All questions are taken from Regents Exams,
parts A and B-1.
• In most cases, it will help to have your
“Reference Tables for Physical
Setting/CHEMISTRY” available.
2
1/07-1
• Which subatomic particles are located in the nucleus of a neon atom?
(1) Electrons and positrons
(2) Electrons and neutrons
(3) Protons and neutrons
(4) Protons and electrons
3
1/07-1
• Which subatomic particles are located in the nucleus of a neon atom?
(1) Electrons and positrons
(2) Electrons and neutrons
(3) Protons and neutrons
(4) Protons and electrons
correct
4
1/07-2
• The total mass of the protons in an atom of gold-198 is approximately
(1) 79 atomic mass units
(2) 119 atomic mass units
(3) 198 atomic mass units
(4) 277 atomic mass units
5
1/07-2
• The total mass of the protons in an atom of gold-198 is approximately
(1) 79 atomic mass units
(3) 198 atomic mass units
correct
(2) 119 atomic mass units
(4) 277 atomic mass units
6
1/07-3
• In a calcium atom in the ground state, the electrons that possess the
least amount of energy are located in the
(1) First electron shell
(2) Second electron shell
(3) Third electron shell
(4) Fourth electron shell
7
1/07-3
• In a calcium atom in the ground state, the electrons that possess the
least amount of energy are located in the
(1) First electron shell
(3) Third electron shell
correct
(2) Second electron shell
(4) Fourth electron shell
8
1/07-4
• Which group of atomic models is listed in historical order from the earliest
to the most recent?
(1) hard-sphere model, wave-mechanical
model, electron-shell model
(2) hard-sphere model, electron-shell
model, wave-mechanical model
(3) electron-shell model, wavemechanical model, hard-sphere model
(4) electron-shell model, hard-sphere
model, wave-mechanical model
9
1/07-4
• Which group of atomic models is listed in historical order from the earliest
to the most recent?
(1) hard-sphere model, wave-mechanical
model, electron-shell model
(2) hard-sphere model, electron-shell
model, wave-mechanical model correct
(3) electron-shell model, wavemechanical model, hard-sphere model
(4) electron-shell model, hard-sphere
model, wave-mechanical model
10
1/07-5
• Which isotopic notation represents an atom of carbon-14?
(1) 8C6
(2) 6C8
(3) 14C8
(4) 6C14
11
1/07-5
• Which isotopic notation represents an atom of carbon-14?
(1) 8C6
(2) 6C8
(3) 14C8
(4) 6C14
correct
12
1/07-6
• An atom of argon rarely bonds to an atom of another element because an
argon atom has
(1) 8 valence electrons
(2) 2 valence electrons
(3) 3 valence electrons
(4) 22 valence electrons
13
1/07-6
• An atom of argon rarely bonds to an atom of another element because an
argon atom has
(1) 8 valence electrons
(3) 3 valence electrons
correct
(2) 2 valence electrons
(4) 22 valence electrons
14
1/07-7
• The elements on the Periodic Table are arranged in order of increasing
(1) Boiling point
(2) electronegativity
(3) Atomic number
(4) Atomic mass
15
1/07-7
• The elements on the Periodic Table are arranged in order of increasing
(1) Boiling point
(3) Atomic number
(2) electronegativity
correct
(4) Atomic mass
16
1/07-8
• Which element is classified as a nonmetal?
(1) Be
(2) Al
(3) Si
(4) Cl
17
1/07-8
• Which element is classified as a nonmetal?
(1) Be
(2) Al
(3) Si
(4) Cl
correct
18
1/07-9
• Solid samples of the element phosphorous can be white, black, or red in
color. The variations in the color are due to different
(1) Atomic masses
(2) Molecular structures
(3) Ionization energies
(4) Nuclear charges
19
1/07-9
• Solid samples of the element phosphorous can be white, black, or red in
color. The variations in the color are due to different
(1) Atomic masses
(2) Molecular structures
(3) Ionization energies
(4) Nuclear charges
correct
20
1/07-10
• Given the balanced equation representing a reaction between propane
and oxygen:
C3H8 + 5O2 -> 3CO2 + 4H2O
According to this equation, which ratio of oxygen to propane is correct?
(1) 5 grams O2/1 gram of C3H8
(2) 10 grams O2/11 grams C3H8
(3) 5 moles O2/1 mole C3H8
(4) 10 moles O2/11 moles C3H8
21
1/07-10
• Given the balanced equation representing a reaction between propane
and oxygen:
C3H8 + 5O2 -> 3CO2 + 4H2O
According to this equation, which ratio of oxygen to propane is correct?
(1) 5 grams O2/1 gram of C3H8
(3) 5 moles O2/1 mole C3H8
(2) 10 grams O2/11 grams C3H8
correct
(4) 10 moles O2/11 moles C3H8
22
1/07-11
• Lithium and potassium have similar chemical properties because the
atoms of both elements have the same
(1) Mass number
(2) Atomic number
(3) Number of electron shells
(4) Number of valence electrons
23
1/07-11
• Lithium and potassium have similar chemical properties because the
atoms of both elements have the same
(1) Mass number
(2) Atomic number
(3) Number of electron shells
(4) Number of valence electrons
correct
24
1/07-12
• Which two substances are covalent compounds?
(1) C6H12O6(s) and KI(s)
(2) C6H12O6(s) and HCl(g)
(3) KI(s) and NaCl(s)
(4) NaCl(s) and HCl(g)
25
1/07-12
• Which two substances are covalent compounds?
(1) C6H12O6(s) and KI(s)
(2) C6H12O6(s) and HCl(g)
(3) KI(s) and NaCl(s)
(4) NaCl(s) and HCl(g)
correct
26
1/07-13
• which substance when dissolved in water, forms a solution that conducts
and electric current?
(1) C2H5OH
(2) C6H12O6
(3) C12H22O11
(4) CH3COOH
27
1/07-13
• Which substance when dissolved in water, forms a solution that conducts
and electric current?
(1) C2H5OH
(2) C6H12O6
(3) C12H22O11
(4) CH3COOH
correct
28
1/07-15
• Compared to a phosphorous atom, a P3- ion has
(1) More electrons and a larger radius
(2) More electrons and a smaller radius
(3) Fewer electrons and a larger radius
(4) Fewer electrons and a smaller radius
29
1/07-15
• Compared to a phosphorous atom, a P3- ion has
(1) More electrons and a larger radius
(2) More electrons and a smaller radius
(3) Fewer electrons and a larger radius
(4) Fewer electrons and a smaller radius
correct
30
1/07-16
• The balanced equation below represents a molecule of bromine
separating into two bromine atoms.
Br2 -> Br + Br
What occurs during the change?
(1) Energy is absorbed and a bond is
formed
(2) Energy is absorbed and a bond is
broken
(3) energy is released and a bond is
formed
(4) Energy is released and a bond is
broken
31
1/07-16
• The balanced equation below represents a molecule of bromine
separating into two bromine atoms.
Br2 -> Br + Br
What occurs during the change?
(1) Energy is absorbed and a bond is
formed
(2) Energy is absorbed and a bond is
correct
broken
(3) energy is released and a bond is
formed
(4) Energy is released and a bond is
broken
32
1/07-17
• Which substance can be decomposed by chemical means?
(1) tungsten
(2) antimony
(3) krypton
(4) methane
33
1/07-17
• Which substance can be decomposed by chemical means?
(1) tungsten
(2) antimony
(3) krypton
(4) methane
correct
34
1/07-18
• Bronze contains 90 to 95% copper and 5 to 10% tin. Because these
percentages can vary, bronze is classified as
(1) A compound
(2) An element
(3) A mixture
(4) A substance
35
1/07-18
• Bronze contains 90 to 95% copper and 5 to 10% tin. Because these
percentages can vary, bronze is classified as
(1) A compound
(3) A mixture
(2) An element
correct
(4) A substance
36
1/07-19
• Compared to a 2.0 M aqueous solution of NaCl at 1 atmosphere, a 3.0 M
aqueous solution of NaCl at 1 atmosphere has a
(1) Lower boiling point and a higher
freezing point
(2) Lower boiling point and a lower
freezing point
(3) Higher boiling point and a higher
freezing point
(4) Higher boiling point and lower freezing
point
37
1/07-19
• Compared to a 2.0 M aqueous solution of NaCl at 1 atmosphere, a 3.0 M
aqueous solution of NaCl at 1 atmosphere has a
(1) Lower boiling point and a higher
freezing point
(2) Lower boiling point and a lower
freezing point
(3) Higher boiling point and a higher
freezing point
(4) Higher boiling point and lower freezing
correct
point
38
1/07-20
• In which reaction are the electrons transferred from one reactant to
another?
(1) 2Ca(s) + O2(g) -> 2CaO(s)
(2) AgNO3(aq) + KCl(aq) ->
AgCl(s) + KNO3
(3) HCl(aq) + NaOH(aq) -> NaCl(aq) +
H2O(l)
(4) H3O+(aq) + OH-(aq) -> 2H2O(l)
39
1/07-20
• In which reaction are the electrons transferred from one reactant to
another?
(1) 2Ca(s) + O2(g) -> 2CaO(s)
correct
(3) HCl(aq) + NaOH(aq) -> NaCl(aq) +
H2O(l)
(2) AgNO3(aq) + KCl(aq) ->
AgCl(s) + KNO3
(4) H3O+(aq) + OH-(aq) -> 2H2O(l)
40
1/07-21
• Which statement must be true for any chemical reaction at equilibrium?
(1) The concentration of the products is
greater than the concentration of the
reactants.
(2) The concentration of the products is
less than the concentration of the
reactants.
(3) The concentration of the products and
the concentration of the reactants are
equal.
(4) The concentration of the products and
the concentration of the reactants are
constant.
41
1/07-21
• Which statement must be true for any chemical reaction at equilibrium?
(1) The concentration of the products is
greater than the concentration of the
reactants.
(2) The concentration of the products is
less than the concentration of the
reactants.
(3) The concentration of the products and
the concentration of the reactants are
equal.
(4) The concentration of the products and
the concentration of the reactants are
correct
constant.
42
1/07-24
• Which group of emissions is listed in order of increasing charge?
(1) Alpha particle, beta particle, gamma
radiation
(2) Gamma radiation, alpha particle, beta
particle
(3) positron, alpha particle, neutron
(4) neutron, positron, alpha particle
43
1/07-25
• Two substances have different physical and chemical properties. Both
substances have molecules that contain two carbon atoms, one oxygen
atom, and six hydrogen atoms. These two substances must be
(1) Isomers of each other
(2) Isotopes of each other
(3) The same compound
(4) The same hydrocarbon
44
1/07-25
• Two substances have different physical and chemical properties. Both
substances have molecules that contain two carbon atoms, one oxygen
atom, and six hydrogen atoms. These two substances must be
(1) Isomers of each other
(3) The same compound
correct
(2) Isotopes of each other
(4) The same hydrocarbon
45
1/07-26
• Given the balanced equation representing a reaction:
CH3CH2CH3 + Br2 -> CH3CH2CH2Br + HBr
This organic reaction is best classified as
(1) An addition reaction
(2) An esterification reaction
(3) A polymerization reaction
(4) A substitution reaction
46
1/07-26
• Given the balanced equation representing a reaction:
CH3CH2CH3 + Br2 -> CH3CH2CH2Br + HBr
This organic reaction is best classified as
(1) An addition reaction
(2) An esterification reaction
(3) A polymerization reaction
(4) A substitution reaction
correct
47
1/07-27
• In terms of energy and entropy, systems in nature tend to undergo
changes toward
(1) Higher energy and higher entropy
(2) Higher energy and lower entropy
(3) Lower energy and higher entropy
(4) Lower energy and lower entropy
48
1/07-27
• In terms of energy and entropy, systems in nature tend to undergo
changes toward
(1) Higher energy and higher entropy
(2) Higher energy and lower entropy
(3) Lower energy and higher entropy
(4) Lower energy and lower entropy
correct
49
1/07-29
• Which compound has hydrogen bonding between its molecules?
(1) CH4
(2) KH
(3) CaH2
(4) NH3
50
1/07-29
• Which compound has hydrogen bonding between its molecules?
(1) CH4
(2) KH
(3) CaH2
(4) NH3
correct
51
1/07-30
• Which ion is the only negative ion produced by an Arrhenius base in
water?
(1) NO3-
(2) Cl-
(3) OH-
(4) H-
52
1/07-30
• Which ion is the only negative ion produced by an Arrhenius base in
water?
(1) NO3(3) OH-
(2) Cl-
correct
(4) H-
53
1/07-31
• When the elements in Group 1 are considered in order from top to
bottom, each successive element at standard pressure has
(1) A higher melting point and a higher
boiling point
(2) A higher melting point and a lower
boiling point
(3) A lower melting point and a higher
boiling point
(4) A lower melting point and a lower
boiling point
54
1/07-31
• When the elements in Group 1 are considered in order from top to
bottom, each successive element at standard pressure has
(1) A higher melting point and a higher
boiling point
(2) A higher melting point and a lower
boiling point
(3) A lower melting point and a higher
boiling point
(4) A lower melting point and a lower
correct
boiling point
55
1/07-32
• Which isotopic notation identifies a metalloid that is matched with the
corresponding number of protons in each of its atoms
(1)
24Mg
and 12 protons
(3) 75As and 75 protons
(2) 28Si and 14 protons
(4) 80Br and 80 protons
56
1/07-32
• Which isotopic notation identifies a metalloid that is matched with the
corresponding number of protons in each of its atoms
(1)
24Mg
and 12 protons
(3) 75As and 75 protons
(2) 28Si and 14 protons
correct
(4) 80Br and 80 protons
57
1/07-33
• At STP, which list of elements contains a solid, liquid, and a gas?
(1) Hf, Hg, He
(2) Cr, Cl2, C
(3) Ba, Br2, B
(4) Se, Sn, Sr
58
1/07-33
• At STP, which list of elements contains a solid, liquid, and a gas?
(1) Hf, Hg, He
(2) Cr, Cl2, C
(3) Ba, Br2, B
(4) Se, Sn, Sr
59
1/07-33
• At STP, which list of elements contains a solid, liquid, and a gas?
(1) Hf, Hg, He
(3) Ba, Br2, B
correct
(2) Cr, Cl2, C
(4) Se, Sn, Sr
60
1/07-34
• Element X reacts with iron to form two different compounds with the
formulas FeX and Fe2X3. To which group on the Periodic Table does
element X belong?
(1) Group 8
(2) Group 2
(3) Group 13
(4) Group 16
61
1/07-34
• Element X reacts with iron to form two different compounds with the
formulas FeX and Fe2X3. To which group on the Periodic Table does
element X belong?
(1) Group 8
(2) Group 2
(3) Group 13
(4) Group 16
correct
62
1/07-35
• The molar mass of Ba(OH)2 is
(1) 154.3 g
(2) 155.3 g
(3) 171.3 g
(4) 308.6 g
63
1/07-35
• The molar mass of Ba(OH)2 is
(1) 154.3 g
(3) 171.3 g
(2) 155.3 g
correct
(4) 308.6 g
64
1/07-36
• Given the balanced equation representing a reaction:
4NH3 + 5O2 -> 4NO + 6H2O
What is the minimum number of moles of O2 that are needed to completely
react 1ith 16 moles of NH3?
(1) 16 mol
(2) 20. mol
(3) 64 mol
(4) 80. mol
65
1/07-36
• Given the balanced equation representing a reaction:
4NH3 + 5O2 -> 4NO + 6H2O
What is the minimum number of moles of O2 that are needed to completely
react 1ith 16 moles of NH3?
(1) 16 mol
(2) 20. mol
(3) 64 mol
(4) 80. mol
correct
66
1/07-38
• A 10.0-gram sample of which element has the smallest volume at STP?
(1) aluminum
(2) magnesium
(3) titanium
(4) zinc
67
1/07-38
• A 10.0-gram sample of which element has the smallest volume at STP?
(1) aluminum
(2) magnesium
(3) titanium
(4) zinc
correct
68
1/07-39
• A which temperature would atoms of a He(g) sample have the greatest
average kinetic energy?
(1) 25°C
(2) 37°C
(3) 273 K
(4) 298 K
69
1/07-39
• A which temperature would atoms of a He(g) sample have the greatest
average kinetic energy?
(1) 25°C
(2) 37°C
(3) 273 K
(4) 298 K
correct
70
1/07-41
• At room temperature, a mixture of sand and water can be separated by
(1) ionization
(2) combustion
(3) filtration
(4) sublimation
71
1/07-41
• At room temperature, a mixture of sand and water can be separated by
(1) ionization
(3) filtration
(2) combustion
correct
(4) sublimation
72
1/07-42
• Given a balanced equation representing a reaction at 101.3 kPa and
298 K:
N2(g) + 3H2(g) -> 2NH3(g) + 91.8 kJ
Which statement is true about this reaction?
(1) It is exothermic and the ∆H equals 91.8 kJ
(2) It is exothermic and the ∆H equals
+91.8 kJ
(3) it is endothermic and the ∆H equals 91.8 kJ
(4) It is endothermic and the ∆H equals
+91.8 kJ
73
1/07-42
• Given a balanced equation representing a reaction at 101.3 kPa and
298 K:
N2(g) + 3H2(g) -> 2NH3(g) + 91.8 kJ
Which statement is true about this reaction?
(1) It is exothermic and the ∆H equals correct
91.8 kJ
(2) It is exothermic and the ∆H equals
+91.8 kJ
(3) it is endothermic and the ∆H equals 91.8 kJ
(4) It is endothermic and the ∆H equals
+91.8 kJ
74
1/07-43
• Which balanced equation represents a phase equilibrium?
(1) 1
(2) 2
(3) 3
(4) 4
75
1/07-43
• Which balanced equation represents a phase equilibrium?
(1) 1
(3) 3
(2) 2
correct
(4) 4
76
1/07-44
• Given the system at equilibrium:
2POCl(g) + Energy = 2PCl3(g) + O2(g)
Which changes occur when O2(g) is added to the system?
(1) The equilibrium shifts to the right and
the concentration of PCl3(g) increases
(2) The equilibrium shifts to the right and
the concentration of PCl3(g) decreases
(3) The equilibrium shifts to the left and
the concentration of PCl3(g) increases
(4) The equilibrium shifts to left and the
concentration fo PCl3(g) decreases
77
1/07-44
• Given the system at equilibrium:
2POCl(g) + Energy = 2PCl3(g) + O2(g)
Which changes occur when O2(g) is added to the system?
(1) The equilibrium shifts to the right and
the concentration of PCl3(g) increases
(2) The equilibrium shifts to the right and
the concentration of PCl3(g) decreases
(3) The equilibrium shifts to the left and
correct
the concentration of PCl3(g) increases
(4) The equilibrium shifts to left and the
concentration fo PCl3(g) decreases
78
1/07-45
• What is the oxidation number of chromium in the chromate ion, CrO42-?
(1) +6
(2) +2
(3) +3
(4) +8
79
1/07-45
• What is the oxidation number of chromium in the chromate ion, CrO42-?
(1) +6
(3) +3
correct
(2) +2
(4) +8
80
1/07-46
• Given the balanced equation representing a reaction:
Which type of reaction is represented by this equation?
(1) decomposition
(2) neutralization
(3) single replacement
(4) synthesis
81
1/07-46
• Given the balanced equation representing a reaction:
Which type of reaction is represented by this equation?
(1) decomposition
(2) neutralization
(3) single replacement
(4) synthesis
correct
82
1/07-47
• In which 0.01 M solution is phenolphthalein pink?
(1) CH3OH(aq)
(2) Ca(OH)2(aq)
(3) CH3COOH(aq)
(4) HNO3(aq)
83
1/07-47
• In which 0.01 M solution is phenolphthalein pink?
(1) CH3OH(aq)
(2) Ca(OH)2(aq)
(3) CH3COOH(aq)
(4) HNO3(aq)
correct
84
1/07-48
• As the pH of a solution is changed from 3 to 6, the concentration of the
hydronium ions
(1) Increases by a factor of 3
(2) Increases by a factor of 1000
(3) Decreases by a factor of 3
(4) Decreases by a factor of 1000
85
1/07-48
• As the pH of a solution is changed from 3 to 6, the concentration of the
hydronium ions
(1) Increases by a factor of 3
(2) Increases by a factor of 1000
(3) Decreases by a factor of 3
(4) Decreases by a factor of 1000
correct
86
1/07-49
• If 1/8 of an original sample of krypton-74 remains unchanged after 34.5
minutes, what is the half-life of krypton-74?
(1) 11.5 min
(2) 23.0 min
(3) 34.5 min
(4) 46.0 min
87
1/07-49
• If 1/8 of an original sample of krypton-74 remains unchanged after 34.5
minutes, what is the half-life of krypton-74?
(1) 11.5 min
(3) 34.5 min
correct
(2) 23.0 min
(4) 46.0 min
88
1/07-50
• Given the nuclear equation:
•Which particle is represented by X?
(1) 2He4
(2) -1e0
(3) 0n1
(4) +1e0
89
1/07-50
• Given the nuclear equation:
•Which particle is represented by X?
(1) 2He4
(3) 0n1
correct
(2) -1e0
(4) +1e0
90
6/07-1
• According to the wave-mechanical model of the atom, electrons in an
atom
(1) Travel in defined circles
(2) Are most likely found in an excited
state
(3) Have a positive charge
(4) Are located in orbitals outside the
nucleus
91
6/07-1
• According to the wave-mechanical model of the atom, electrons in an
atom
(1) Travel in defined circles
(2) Are most likely found in an excited
state
(3) Have a positive charge
(4) Are located in orbitals outside the
correct
nucleus
92
6/07-2
• What is the total charge of the nucleus of a carbon atom?
(1) -6
(2) 0
(3) +6
(4) +12
93
6/07-2
• What is the total charge of the nucleus of a carbon atom?
(1) -6
(2) 0
(3) +6
(4) +12
correct
94
6/07-3
• A sample composed only of atoms having the same atomic number is
classified as
(1) A compound
(2) A solution
(3) An element
(4) An isomer
95
6/07-3
• A sample composed only of atoms having the same atomic number is
classified as
(1) A compound
(3) An element
(2) A solution
correct
(4) An isomer
96
6/07-4
• Which two particles each have a mass approximately equal to one atomic
mass unit?
(1) Electron and neutron
(2) Electron and positron
(3) Proton and electron
(4) Proton and neutron
97
6/07-4
• Which two particles each have a mass approximately equal to one atomic
mass unit?
(1) Electron and neutron
(2) Electron and positron
(3) Proton and electron
(4) Proton and neutron
correct
98
6/07-5
• Which two characteristics are associated with metals?
(1) Low first ionization energy and low
electronegativity
(2) Low first ionization energy and high
electronegativity
(3) High first ionization energy and low
electronegativity
(4) Low first ionization energy and high
electronegativity
99
6/07-5
• Which two characteristics are associated with metals?
(1) Low first ionization energy and low
correct
electronegativity
(2) Low first ionization energy and high
electronegativity
(3) High first ionization energy and low
electronegativity
(4) Low first ionization energy and high
electronegativity
100
6/07-6
• Which element is most chemically similar to chlorine?
(1) Ar
(2) F
(3) Fr
(4) S
101
6/07-6
• Which element is most chemically similar to chlorine?
(1) Ar
(2) F
(3) Fr
(4) S
correct
102
6/07-7
• Which substance can be decomposed by chemical means?
(1) ammonia
(2) oxygen
(3) phosphorous
(4) silicon
103
6/07-7
• Which substance can be decomposed by chemical means?
(1) ammonia
(3) phosphorous
correct
(2) oxygen
(4) silicon
104
6/07-8
• When an atom loses one or more electrons, this atom becomes a
(1) Positive ion with a radius smaller than
the radius of this atom
(2) Positive ion with a radius larger than
the radius of this atom
(3) Negative ion with a radius smaller than (4) Negative ion with a radius larger than
the radius of this atom
the radius of this atom
105
6/07-8
• When an atom loses one or more electrons, this atom becomes a
(1) Positive ion with a radius smaller than
correct
the radius of this atom
(2) Positive ion with a radius larger than
the radius of this atom
(3) Negative ion with a radius smaller than (4) Negative ion with a radius larger than
the radius of this atom
the radius of this atom
106
6/07-9
• What is the name of the polyatomic ion in the compound Na2O2?
(1) hydroxide
(2) oxalate
(3) oxide
(4) peroxide
107
6/07-9
• What is the name of the polyatomic ion in the compound Na2O2?
(1) hydroxide
(2) oxalate
(3) oxide
(4) peroxide
correct
108
6/07-10
• Given the balanced equation:
I + I -> I2
Which statement describes the process represented by this equation?
(1) A bond is formed and energy is
absorbed
(2) A bond is formed and energy is
released
(3) A bond is broken and energy is
absorbed
(4) A bond is broken and energy is
released
109
6/07-10
• Given the balanced equation:
I + I -> I2
Which statement describes the process represented by this equation?
(1) A bond is formed and energy is
correct
absorbed
(2) A bond is formed and energy is
released
(3) A bond is broken and energy is
absorbed
(4) A bond is broken and energy is
released
110
6/07-11
• An oxygen molecule contains a double bond because two atoms of
oxygen share a total of
(1) 1 electron
(2) 2 electrons
(3) 3 electrons
(4) 4 electrons
111
6/07-11
• An oxygen molecule contains a double bond because two atoms of
oxygen share a total of
(1) 1 electron
(2) 2 electrons
(3) 3 electrons
(4) 4 electrons
correct
112
6/07-12
• Which term is defined as a measure of the average kinetic energy of the
particles in a sample?
(1) temperature
(2) pressure
(3) thermal energy
(4) chemical energy
113
6/07-12
• Which term is defined as a measure of the average kinetic energy of the
particles in a sample?
(1) temperature
(3) thermal energy
correct
(2) pressure
(4) chemical energy
114
6/07-13
• A 3.0 M HCl(aq) solution contains a total of
(1) 3.0 grams of HCl per liter of water
(2) 3.0 grams of HCl per mole of solution
(3) 3.0 moles of HCl per liter of solution
(4) 3.0 moles of HCl per mole of water
115
6/07-13
• A 3.0 M HCl(aq) solution contains a total of
(1) 3.0 grams of HCl per liter of water
(2) 3.0 grams of HCl per mole of solution
(3) 3.0 moles of HCl per liter of solution
(4) 3.0 moles of HCl per mole of water
correct
116
6/07-14
• A dilute, aqueous potassium nitrate solution is best classified as a
(1) Homogeneous compound
(2) Homogeneous mixture
(3) Heterogeneous compound
(4) Heterogeneous mixture
117
6/07-14
• A dilute, aqueous potassium nitrate solution is best classified as a
(1) Homogeneous compound
(2) Homogeneous mixture
correct
(3) Heterogeneous compound
(4) Heterogeneous mixture
118
6/07-15
• Given the equation representing a phase change at equilibrium:
C2H5OH(l) = C2H5OH(g)
Which statement is true?
(1) The forward process proceeds faster
than the reverse process
(2) The reverse process proceeds faster
than the forward process
(3) The forward and reverse processes
proceed at the same rate
(4) The forward and reverse processes
both stop
119
6/07-15
• Given the equation representing a phase change at equilibrium:
C2H5OH(l) = C2H5OH(g)
Which statement is true?
(1) The forward process proceeds faster
than the reverse process
(2) The reverse process proceeds faster
than the forward process
(3) The forward and reverse processes
correct
proceed at the same rate
(4) The forward and reverse processes
both stop
120
6/07-16
• A 5.0-gram sample of zinc and a 50. –milliliter sample of hydrochloric acid
are used in a chemical reaction. Which combination of these samples has
the fastest reaction rate?
(1) A zinc strip and 1.0 M HCl(aq)
(2) A zinc strip and 3.0 M HCl(aq)
(3) Zinc powder and 1.0 M HCl(aq)
(4) Zinc powder and 3.0 M HCl(aq)
121
6/07-16
• A 5.0-gram sample of zinc and a 50. –milliliter sample of hydrochloric acid
are used in a chemical reaction. Which combination of these samples has
the fastest reaction rate?
(1) A zinc strip and 1.0 M HCl(aq)
(2) A zinc strip and 3.0 M HCl(aq)
(3) Zinc powder and 1.0 M HCl(aq)
(4) Zinc powder and 3.0 M HCl(aq)
correct
122
6/07-17
• For a given reaction, adding a catalyst increases the rate of the reaction
by
(1) Providing an alternate reaction
pathway that has a higher activation
energy
(2) Providing an alternate reaction
pathway that has a lower activation
energy
(3) Using the same reaction pathway and
increasing the activation energy
(4) Using the same reaction pathway and
decreasing the activation energy
123
6/07-17
• For a given reaction, adding a catalyst increases the rate of the reaction
by
(1) Providing an alternate reaction
pathway that has a higher activation
energy
(2) Providing an alternate reaction
pathway that has a lower activation
correct
energy
(3) Using the same reaction pathway and
increasing the activation energy
(4) Using the same reaction pathway and
decreasing the activation energy
124
6/07-18
• Which reaction releases the greatest amount of energy per 2 moles of
product?
(1) 1
(2) 2
(3) 3
(4) 4
125
6/07-18
• Which reaction releases the greatest amount of energy per 2 moles of
product?
(1) 1
(2) 2
(3) 3
(4) 4
correct
126
6/07-19
• What is the total number of carbon atoms in a molecule of ethanoic acid?
(1) 1
(2) 2
(3) 3
(4) 4
127
6/07-19
• What is the total number of carbon atoms in a molecule of ethanoic acid?
(1) 1
(2) 2
(3) 3
(4) 4
correct
128
6/07-21
• A double carbon-carbon bond is found in a molecule of
(1) pentane
(2) pentene
(3) pentyne
(4) pentanol
129
6/07-21
• A double carbon-carbon bond is found in a molecule of
(1) pentane
(2) pentene
(3) pentyne
(4) pentanol
correct
130
6/07-22
• Which changes occur when Pt2+ is reduced?
(1) The Pt2+ gains electrons and its
oxidation number increases
(2) The Pt2+ gains electrons and its
oxidation number decreases
(3) The Pt2+ loses electrons and its
oxidation number increases
(4) The Pt2+ loses electrons and its
oxidation number decreases
131
6/07-22
• Which changes occur when Pt2+ is reduced?
(1) The Pt2+ gains electrons and its
oxidation number increases
(2) The Pt2+ gains electrons and its
oxidation number decreases correct
(3) The Pt2+ loses electrons and its
oxidation number increases
(4) The Pt2+ loses electrons and its
oxidation number decreases
132
6/07-23
• Which balanced equation represents an oxidation-reduction reaction?
(1) 1
(2) 2
(3) 3
(4) 4
133
6/07-23
• Which balanced equation represents an oxidation-reduction reaction?
(1) 1
(2) 2
(3) 3
(4) 4
correct
134
6/07-24
• Which energy conversion occurs during the operation of a voltaic cell?
(1) Chemical energy is spontaneously
converted to electrical energy
(2) Chemical energy is converted to
electrical energy only when an external
power source is provided
(3) Electrical energy is spontaneously
converted to chemical energy
(4) Electrical energy is converted to
chemical energy only when an external
power source is provided
135
6/07-24
• Which energy conversion occurs during the operation of a voltaic cell?
(1) Chemical energy is spontaneously
converted to electrical energy correct
(2) Chemical energy is converted to
electrical energy only when an external
power source is provided
(3) Electrical energy is spontaneously
converted to chemical energy
(4) Electrical energy is converted to
chemical energy only when an external
power source is provided
136
6/07-25
• An Arrhenius base yields which ion as the only negative ion in an
aqueous solution?
(1) Hydride ion
(2) Hydrogen ion
(3) Hydronium ion
(4) Hydroxide ion
137
6/07-25
• An Arrhenius base yields which ion as the only negative ion in an
aqueous solution?
(1) Hydride ion
(2) Hydrogen ion
(3) Hydronium ion
(4) Hydroxide ion
correct
138
6/07-26
• According to the acid-base theory, a water molecule acts as an acid when
the water molecule
(1) Accepts H-
(2) Accepts OH-
(3) Donates a H+
(4) Donates an OH-
139
6/07-26
• According to the acid-base theory, a water molecule acts as an acid when
the water molecule
(1) Accepts H(3) Donates a H+
(2) Accepts OH-
correct
(4) Donates an OH-
140
6/07-27
• Which list of radioisotopes contains an alpha emitter, a beta emitter, and
a positron emitter?
(1) C-14, N-16, P-32
(2) Cs-137, Fr-220, Tc-99
(3) Kr-85, Ne-19, Rn-222
(4) Pu-239, Th-232, U-238
141
6/07-27
• Which list of radioisotopes contains an alpha emitter, a beta emitter, and
a positron emitter?
(1) C-14, N-16, P-32
(3) Kr-85, Ne-19, Rn-222
(2) Cs-137, Fr-220, Tc-99
correct
(4) Pu-239, Th-232, U-238
142
6/07-28
• Which nuclear decay emission consists of energy, only?
(1) alpha particle
(2) Beta particle
(3) gamma radiation
(4) positron
143
6/07-28
• Which nuclear decay emission consists of energy, only?
(1) alpha particle
(3) gamma radiation
(2) Beta particle
correct
(4) positron
144
6/07-29
• Which balanced equation represents nuclear fusion?
(1) 1
(2) 2
(3) 3
(4) 4
145
6/07-29
• Which balanced equation represents nuclear fusion?
(1) 1
(2) 2
(3) 3
(4) 4
correct
146
6/07-30
• The energy released by a nuclear reaction results primarily from the
(1) Breaking of bonds between atoms
(2) Formation of bonds between atoms
(3) Conversion of mass into energy
(4) Conversion of energy into mass
147
6/07-30
• The energy released by a nuclear reaction results primarily from the
(1) Breaking of bonds between atoms
(2) Formation of bonds between atoms
(3) Conversion of mass into energy
(4) Conversion of energy into mass
correct
148
6/07-33
• What is the total number of neutrons in an atom of 26Fe57?
(1) 26
(2) 31
(3) 57
(4) 83
149
6/07-33
• What is the total number of neutrons in an atom of 26Fe57?
(1) 26
(2) 31
(3) 57
(4) 83
correct
150
6/07-34
• At STP, which element is brittle and not a conductor of electricity?
(1) S
(2) K
(3) Na
(4) Ar
151
6/07-34
• At STP, which element is brittle and not a conductor of electricity?
(1) S
(3) Na
correct
(2) K
(4) Ar
152
6/07-35
• What is the total number of electrons in a Mg2+ ion?
(1) 10
(2) 12
(3) 14
(4) 24
153
6/07-35
• What is the total number of electrons in a Mg2+ ion?
(1) 10
(3) 14
correct
(2) 12
(4) 24
154
6/07-36
• Which formula represents lead(II) chromate?
(1) PbCrO4
(2) Pb(CrO4)2
(3) Pb2CrO4
(4) Pb2(CrO4)3
155
6/07-36
• Which formula represents lead(II) chromate?
(1) PbCrO4
(3) Pb2CrO4
correct
(2) Pb(CrO4)2
(4) Pb2(CrO4)3
156
6/07-37
• Compared to an electron in the first electron shell of an atom, an electron
in the third shell of the same atom has
(1) Less mass
(2) Less energy
(3) More mass
(4) More energy
157
6/07-37
• Compared to an electron in the first electron shell of an atom, an electron
in the third shell of the same atom has
(1) Less mass
(2) Less energy
(3) More mass
(4) More energy
correct
158
6/07-38
• Which pair consists of a molecular formula and its corresponding
empirical formula?
(1) C2H2 and CH3CH3
(2) C6H6 and C2H2
(3) P4O10 and P2O5
(4) SO2 and SO3
159
6/07-38
• Which pair consists of a molecular formula and its corresponding
empirical formula?
(1) C2H2 and CH3CH3
(3) P4O10 and P2O5
(2) C6H6 and C2H2
correct
(4) SO2 and SO3
160
6/07-41
• At STP, fluorine is a gas and bromine is a liquid because, compared to
fluorine, bromine has
(1) Stronger covalent bonds
(2) Stronger intermolecular forces
(3) Weaker covalent bonds
(4) Weaker intermolecular forces
161
6/07-41
• At STP, fluorine is a gas and bromine is a liquid because, compared to
fluorine, bromine has
(1) Stronger covalent bonds
(2) Stronger intermolecular forces
correct
(3) Weaker covalent bonds
(4) Weaker intermolecular forces
162
6/07-41
• At STP, fluorine is a gas and bromine is a liquid because, compared to
fluorine, bromine has
(1) Stronger covalent bonds
(2) Stronger intermolecular forces
correct
(3) Weaker covalent bonds
(4) Weaker intermolecular forces
163
6/07-42
• The boiling point of a liquid is the temperature at which the vapoir
pressure of the liquid is equal to the pressure on the surface of the liquid.
What is the boiling point of propanone if the pressure on its surface is 48
kilopascals?
(1) 25°C
(2) 30.°C
(3) 35°C
(4) 40.°C
164
6/07-42
• The boiling point of a liquid is the temperature at which the vapoir
pressure of the liquid is equal to the pressure on the surface of the liquid.
What is the boiling point of propanone if the pressure on its surface is 48
kilopascals?
(1) 25°C
(3) 35°C
(2) 30.°C
correct
(4) 40.°C
165
6/07-42
• The boiling point of a liquid is the temperature at which the vapoir
pressure of the liquid is equal to the pressure on the surface of the liquid.
What is the boiling point of propanone if the pressure on its surface is 48
kilopascals?
(1) 25°C
(3) 35°C
(2) 30.°C
correct
(4) 40.°C
166
6/07-43
• At which Celsius temperature does lead change from a solid to a liquid?
(1) 874°C
(2) 601°C
(3) 328°C
(4) 0°C
167
6/07-43
• At which Celsius temperature does lead change from a solid to a liquid?
(1) 874°C
(3) 328°C
(2) 601°C
correct
(4) 0°C
168
6/07-44
• Given the equation representing a reaction at equilibrium:
N2(g) + 3H2(g) = 2NH3(g) + energy
Which change causes the equilibrium to shift to the right?
(1) Decreasing the concentration of H2(g)
(2) Decreasing the pressure
(3) Increasing the concentration of N2(g)
(4) Increasing the temperature
169
6/07-44
• Given the equation representing a reaction at equilibrium:
N2(g) + 3H2(g) = 2NH3(g) + energy
Which change causes the equilibrium to shift to the right?
(1) Decreasing the concentration of H2(g)
(2) Decreasing the pressure
(3) Increasing the concentration of N2(g)
(4) Increasing the temperature
correct
170
6/07-45
• Which compound is an unsaturated hydrocarbon?
(1) hexanal
(2) hexane
(3) Hexanoic acid
(4) hexyne
171
6/07-45
• Which compound is an unsaturated hydrocarbon?
(1) hexanal
(2) hexane
(3) Hexanoic acid
(4) hexyne
correct
172
6/07-46
• The organic compound represented by the condensed structural formula
CH3CH2CH2CHO is classified as an
(1) alcohol
(2) aldehyde
(3) ester
(4) ether
173
6/07-46
• The organic compound represented by the condensed structural formula
CH3CH2CH2CHO is classified as an
(1) alcohol
(2) aldehyde
(3) ester
(4) ether
correct
174
6/07-47
•
(1) Al to Mg2+
(2) Al3+ to Mg
(3) Mg to Al3+
(4) Mg2+ to Al
175
6/07-47
•
(1) Al to Mg2+
(3) Mg to Al3+
(2) Al3+ to Mg
correct
(4) Mg2+ to Al
176
6/07-48
• Which two formulas represent Arrhenius acids?
(1) 1
(2) 2
(3) 3
(4) 4
177
6/07-48
• Which two formulas represent Arrhenius acids?
(1) 1
(2) 2
(3) 3
(4) 4
178
6/07-49
• Information about a titration experiment is given in the balanced equation
and table below.
correct
Based on the equation and results, what is the concentration of
H2SO4(aq)?
(1) 0.12 M
(2) 0.24 M
(3) 0.16 M
(4) 0.96 M
179
6/07-49
• Information about a titration experiment is given in the balanced equation
and table below.
correct
Based on the equation and results, what is the concentration of
H2SO4(aq)?
(1) 0.12 M
(2) 0.24 M
(3) 0.16 M
(4) 0.96 M
correct
180
6/07-50
• Which radioisotope is used in medicine to treat thyroid disorders?
(1) cobalt-60
(2) iodine-131
(3) phosphorous-32
(4) uranium-238
181
6/07-50
• Which radioisotope is used in medicine to treat thyroid disorders?
(1) cobalt-60
(2) iodine-131
(3) phosphorous-32
(4) uranium-238
correct
182
8/07-1
• What was concluded about the structure of the atom as a result of the
gold foil experiment?
(1) A positively charged nucleus was
surrounded by positively charged
particles
(2) A positively charged nucleus was
surrounded by mostly empty space
(3) A negatively charged nucleus is
surrounded by positively charged
particles
(4) A negatively charged nucleus is
surrounded by mostly empty space
183
8/07-1
• What was concluded about the structure of the atom as a result of the
gold foil experiment?
(1) A positively charged nucleus was
surrounded by positively charged
particles
(2) A positively charged nucleus was
surrounded by mostly empty space
(3) A negatively charged nucleus is
surrounded by positively charged
particles
(4) A negatively charged nucleus is
surrounded by mostly empty space
correct
184
8/07-2
• An atom is electrically neutral because
(1) Number of protons equals number of
electrons
(2) Number of protons equals number of
neutrons
(3) Ratio of the number of neutrons to the (4) Ratio of the number of neutrons to the
number electrons is 1:1
number of protons is 2:1
185
8/07-2
• An atom is electrically neutral because
(1) Number of protons equals number of
correct
electrons
(2) Number of protons equals number of
neutrons
(3) Ratio of the number of neutrons to the (4) Ratio of the number of neutrons to the
number electrons is 1:1
number of protons is 2:1
186
8/07-3
• How do energy and the most probable location of an electron in the third
shell of an atom compare to the energy and most probable location of an
electron in the first shell of the same atom?
(1) In the third shell, the electron has
more energy and is closer to the
nucleus
(2) In the third shell, an electron has more
energy and is farther from the nucleus
(3) In the third shell, an electron has less
energy and is closer to the nucleus
(4) In the third shell, an electron has less
energy and is farther from the nucleus
187
8/07-3
• How do energy and the most probable location of an electron in the third
shell of an atom compare to the energy and most probable location of an
electron in the first shell of the same atom?
(1) In the third shell, the electron has
more energy and is closer to the
nucleus
(2) In the third shell, an electron has more
energy and is farther from the nucleus
(3) In the third shell, an electron has less
energy and is closer to the nucleus
(4) In the third shell, an electron has less
energy and is farther from the nucleus
correct
188
8/07-4
• Which element is a solid at STP and a good conductor of electricity?
(1) iodine
(2) mercury
(3) nickel
(4) sulfur
189
8/07-4
• Which element is a solid at STP and a good conductor of electricity?
(1) iodine
(3) nickel
(2) mercury
correct
(4) sulfur
190
8/07-5
• Which element has both metallic and nonmetallic properties?
(1) Rb
(2) Rn
(3) Si
(4) Sr
191
8/07-5
• Which element has both metallic and nonmetallic properties?
(1) Rb
(3) Si
(2) Rn
correct
(4) Sr
192
8/07-6
• The carbon atoms in graphite and the carbon atoms in diamond have
different
(1) Atomic numbers
(2) Atomic masses
(3) electronegativities
(4) Structural arrangements
193
8/07-6
• The carbon atoms in graphite and the carbon atoms in diamond have
different
(1) Atomic numbers
(2) Atomic masses
(3) electronegativities
(4) Structural arrangements correct
194
8/07-7
• Which element has the greatest tendency to gain electrons?
(1) bromine
(2) chlorine
(3) fluorine
(4) iodine
195
8/07-7
• Which element has the greatest tendency to gain electrons?
(1) bromine
(3) fluorine
(2) chlorine
correct
(4) iodine
196
8/07-8
• Which statement describes a chemical property of the element
magnesium?
(1) Magnesium is malleable
(2) Magnesium conducts electricity
(3) Magnesium reacts with an acid
(4) Magnesium has a high boiling point
197
8/07-8
• Which statement describes a chemical property of the element
magnesium?
(1) Magnesium is malleable
(2) Magnesium conducts electricity
(3) Magnesium reacts with an acid
(4) Magnesium has a high boiling point
correct
198
8/07-9
• Matter that is composed of two or more different elements chemically
combined in a fixed proportion is classified as
(1) A compound
(2) An isotope
(3) A mixture
(4) A solution
199
8/07-9
• Matter that is composed of two or more different elements chemically
combined in a fixed proportion is classified as
(1) A compound
(2) An isotope
(3) A mixture
(4) A solution
correct
200
8/07-10
• Given the balanced equation representing a reaction:
2CO(g) + O2(g) -> 2CO2(g)
What is the mole ratio of CO(g) to CO2(g) in this reaction?
(1) 1:1
(2) 1:2
(3) 2:1
(4) 3:2
201
8/07-10
• Given the balanced equation representing a reaction:
2CO(g) + O2(g) -> 2CO2(g)
What is the mole ratio of CO(g) to CO2(g) in this reaction?
(1) 1:1
(3) 2:1
correct
(2) 1:2
(4) 3:2
202
8/07-11
• Given the balanced equation representing a reaction:
H+(aq) OH-(aq) -> H2O(l) + 58 kJ
In this reaction there is conservation of
(1) Mass, only
(2) Mass and charge, only
(3) Mass and energy, only
(4) mass, charge, and energy
203
8/07-11
• Given the balanced equation representing a reaction:
H+(aq) OH-(aq) -> H2O(l) + 58 kJ
In this reaction there is conservation of
(1) Mass, only
(2) Mass and charge, only
(3) Mass and energy, only
(4) mass, charge, and energy
correct
204
8/07-12
• Which polyatomic ion contains the greatest number of oxygen atoms?
(1) acetate
(2) carbonate
(3) hydroxide
(4) peroxide
205
8/07-12
• Which polyatomic ion contains the greatest number of oxygen atoms?
(1) acetate
(2) carbonate
(3) hydroxide
(4) peroxide
correct
206
8/07-13
• Which formula represents an ionic compound?
(1) H2
(2) CH4
(3) CH3OH
(4) NH4Cl
207
8/07-13
• Which formula represents an ionic compound?
(1) H2
(2) CH4
(3) CH3OH
(4) NH4Cl
correct
208
8/07-14
• An ion of which element has a larger radius than an atom of the same
element?
(1) aluminum
(2) chlorine
(3) magnesium
(4) sodium
209
8/07-14
• An ion of which element has a larger radius than an atom of the same
element?
(1) aluminum
(2) chlorine
(3) magnesium
(4) sodium
correct
210
8/07-15
• Which statement must be true when solution equilibrium occurs?
(1) The solution is at STP
(2) The solution is supersaturated
(3) The concentration of the solution
remains constant
(4) The masses of the dissolved solute and
the undissolved solute are equal
211
8/07-15
• Which statement must be true when solution equilibrium occurs?
(1) The solution is at STP
(2) The solution is supersaturated
(3) The concentration of the solution
correct
remains constant
(4) The masses of the dissolved solute and
the undissolved solute are equal
212
8/07-16
• Which liquid has the highest vapor pressure at 75°C?
(1) ethanoic acid
(2) ethanol
(3) propanone
(4) water
213
8/07-16
• Which liquid has the highest vapor pressure at 75°C?
(1) ethanoic acid
(2) ethanol
(3) propanone
(4) water
correct
214
8/07-17
• What is the total number of different elements present in NH4NO3?
(1) 7
(2) 9
(3) 3
(4) 4
215
8/07-17
• What is the total number of different elements present in NH4NO3?
(1) 7
(2) 9
(3) 3
(4) 4
correct
216
8/07-18
• Which sample of matter is a single substance?
(1) Air
(2) Ammonia gas
(3) Hydrochloric acid
(4) Salt water
217
8/07-18
• Which sample of matter is a single substance?
(1) Air
(2) Ammonia gas
(3) Hydrochloric acid
(4) Salt water
correct
218
8/07-19
• At STP, which sample contains the same number of molecules as 11.2
liters of CO2(g) at STP
(1) 5.6 liters of NO(g)
(2) 11.2 liters of N2(g)
(3) 7.5 liters of H2(g)
(4) 22.4 liters of CO(g)
219
8/07-19
• At STP, which sample contains the same number of molecules as 11.2
liters of CO2(g) at STP
(1) 5.6 liters of NO(g)
(2) 11.2 liters of N2(g)
(3) 7.5 liters of H2(g)
(4) 22.4 liters of CO(g)
correct
220
8/07-20
• A sample of gas is held at a constant pressure. Increasing the Kelvin
temperature of this gas sample causes the average kinetic energy of its
molecules to
(1) Decrease and the volume of the gas
sample to decrease
(2) Decrease and the volume of the gas
sample to increase
(3) Increase and the volume of this gas
sample to decrease
(4) Increase and the volume of this gas
sample to increase
221
8/07-20
• A sample of gas is held at a constant pressure. Increasing the Kelvin
temperature of this gas sample causes the average kinetic energy of its
molecules to
(1) Decrease and the volume of the gas
sample to decrease
(2) Decrease and the volume of the gas
sample to increase
(3) Increase and the volume of this gas
sample to decrease
(4) Increase and the volume of this gas
correct
sample to increase
222
8/07-21
• Given the balanced equation representing a reaction:
Cl2(g) -> Cl(g) + Cl(g)
What occurs during this change?
(1) Energy is absorbed and a bond is
broken
(2) Energy is absorbed and a bond is
formed
(3) Energy is released and a bond is
broken
(4) Energy is released and a bond if
formed
223
8/07-21
• Given the balanced equation representing a reaction:
Cl2(g) -> Cl(g) + Cl(g)
What occurs during this change?
(1) Energy is absorbed and a bond is
correct
broken
(2) Energy is absorbed and a bond is
formed
(3) Energy is released and a bond is
broken
(4) Energy is released and a bond if
formed
224
8/07-22
• A molecule of butane and a molecule of 2-butene both have the same
total number of
(1) Carbon atoms
(2) Hydrogen atoms
(3) Single bonds
(4) Double bonds
225
8/07-22
• A molecule of butane and a molecule of 2-butene both have the same
total number of
(1) Carbon atoms
(2) Hydrogen atoms
correct
(3) Single bonds
(4) Double bonds
226
8/07-23
• Which general formula represents the homologous series of
hydrocarbons that includes the compound 1-heptyne?
(1) CnH2n-6
(2) CnH2n-2
(3) CnH2n
(4) CnH2n+2
227
8/07-23
• Which general formula represents the homologous series of
hydrocarbons that includes the compound 1-heptyne?
(1) CnH2n-6
(2) CnH2n-2
correct
(3) CnH2n
(4) CnH2n+2
228
8/07-24
• Which two compounds are isomers of each other?
(1) 1
(2) 2
(3) 3
(4) 4
229
8/07-24
• Which two compounds are isomers of each other?
(1) 1
(2) 2
correct
(3) 3
(4) 4
230
8/07-26
• Which formula represents the hydronium ion?
(1) H3O+
(2) NH4+
(3) OH-
(4) HCO3-
231
8/07-26
• Which formula represents the hydronium ion?
(1) H3O+
(3) OH-
correct
(2) NH4+
(4) HCO3-
232
8/07-27
• Which compound is an Arrhenius acid?
(1) H2SO4
(2) KCl
(3) NaOH
(4) NH3
233
8/07-27
• Which compound is an Arrhenius acid?
(1) H2SO4
(3) NaOH
correct
(2) KCl
(4) NH3
234
8/07-28
• What is the decay mode of 37K?
(1) beta
(2) positron
(3) gamma
(4) alpha
235
8/07-28
• What is the decay mode of 37K?
(1) beta
(2) positron
(3) gamma
(4) alpha
correct
236
8/07-29
• Which nuclear emission has the greatest penetrating power?
(1) Alpha particle
(2) Beta particle
(3) Gamma radiation
(4) Positron
237
8/07-29
• Which nuclear emission has the greatest penetrating power?
(1) Alpha particle
(3) Gamma radiation
(2) Beta particle
correct
(4) Positron
238
8/07-30
• What is the mass number of an alpha particle?
(1) 1
(2) 2
(3) 0
(4) 4
239
8/07-30
• What is the mass number of an alpha particle?
(1) 1
(2) 2
(3) 0
(4) 4
correct
240
8/07-31
• What is the net charge on an ion that has 9 protons, 11 neutrons, and 10
electrons?
(1) 1+
(2) 2+
(3) 1-
(4) 2-
241
8/07-31
• What is the net charge on an ion that has 9 protons, 11 neutrons, and 10
electrons?
(1) 1+
(3) 1-
(2) 2+
correct
(4) 2-
242
8/07-32
• Which two particles make up most of the mass of a hydrogen-2 atom?
(1) Electron and neutron
(2) Electron and proton
(3) Proton and neutron
(4) Proton and positron
243
8/07-32
• Which two particles make up most of the mass of a hydrogen-2 atom?
(1) Electron and neutron
(3) Proton and neutron
(2) Electron and proton
correct
(4) Proton and positron
244
8/07-33
• Which statement explains why sulfur is classified as a Group 16 element?
(1) A sulfur atom has 6 valence electrons
(2) A sulfur atom has 16 neutrons
(3) Sulfur is a yellow solid at STP
(4) Sulfur reacts with most metals
245
8/07-33
• Which statement explains why sulfur is classified as a Group 16 element?
(1) A sulfur atom has 6 valence electrons
(2) A sulfur atom has 16 neutrons
(3) Sulfur is a yellow solid at STP
(4) Sulfur reacts with most metals
correct
246
8/07-34
• How do the atomic radius and metallic properties of sodium compare to
the atomic radius and metallic properties of phosphorous?
(1) Sodium has a larger atomic radius and
is more metallic
(2) Sodium has a larger atomic radius and
is less metallic
(3) Sodium has a smaller atomic radius
and is more metallic
(4) Sodium has a smaller atomic radius
and is less metallic
247
8/07-34
• How do the atomic radius and metallic properties of sodium compare to
the atomic radius and metallic properties of phosphorous?
(1) Sodium has a larger atomic radius and
correct
is more metallic
(2) Sodium has a larger atomic radius and
is less metallic
(3) Sodium has a smaller atomic radius
and is more metallic
(4) Sodium has a smaller atomic radius
and is less metallic
248
8/07-35
• A compound has a molar mass of 90. grams per mole and the empirical
formula CH2O. What is the molecular formula for this compound?
(1) CH2O
(2) C2H4O2
(3) C3H6O3
(4) C4H8O4
249
8/07-35
• A compound has a molar mass of 90. grams per mole and the empirical
formula CH2O. What is the molecular formula for this compound?
(1) CH2O
(3) C3H6O3
(2) C2H4O2
correct
(4) C4H8O4
250
8/07-36
• At standard pressure, a certain compound has a low boiling point and is
insoluble in water. At STP, this compound most likely exists as
(1) Ionic crystals
(2) Metallic crystals
(3) Nonpolar molecules
(4) Polar molecules
251
8/07-36
• At standard pressure, a certain compound has a low boiling point and is
insoluble in water. At STP, this compound most likely exists as
(1) Ionic crystals
(3) Nonpolar molecules
(2) Metallic crystals
correct
(4) Polar molecules
252
8/07-38
• Which group on the Periodic Table of the Elements contains elements
that react with oxygen to form compounds with the general formula X2O?
(1) Group 1
(2) Group 2
(3) Group 14
(4) Group 18
253
8/07-38
• Which group on the Periodic Table of the Elements contains elements
that react with oxygen to form compounds with the general formula X2O?
(1) Group 1
(3) Group 14
correct
(2) Group 2
(4) Group 18
254
8/07-39
• A unsaturated solution is formed when 80. grams of a salt is dissolved in
100 grams of water at 40.°C. This salt could be
(1) KCl
(2) KNO3
(3) NaCl
(4) NaNO3
255
8/07-39
• A unsaturated solution is formed when 80. grams of a salt is dissolved in
100 grams of water at 40.°C. This salt could be
(1) KCl
(2) KNO3
(3) NaCl
(4) NaNO3
correct
256
8/07-40
• Which Kelvin temperature is equal to 56°C?
(1) -329 K
(2) -217 K
(3) 217 K
(4) 329 K
257
8/07-40
• Which Kelvin temperature is equal to 56°C?
(1) -329 K
(2) -217 K
(3) 217 K
(4) 329 K
correct
258
8/07-42
• Given the balanced equation representing the reaction occuring in a
voltaic cell:
Zn(s) + Pb2+(aq) -> Zn2+(aq) + Pb(s)
In the completed external circuit, the electrons flow from
(1) 1
(2) 2
(3) 3
(4) 4
259
8/07-42
• Given the balanced equation representing the reaction occuring in a
voltaic cell:
Zn(s) + Pb2+(aq) -> Zn2+(aq) + Pb(s)
In the completed external circuit, the electrons flow from
(1) 1
(3) 3
(2) 2
correct
(4) 4
260
8/07-43
• Which balanced equation represents a redox reaction?
(1) 1
(2) 2
(3) 3
(4) 4
261
8/07-43
• Which balanced equation represents a redox reaction?
(1) 1
(2) 2
(3) 3
(4) 4
correct
262
8/07-44
• Given the unbalanced ionic equation:
3Mg + ____Fe3+ -> 3Mg2+ + ____Fe
When this equation is balanced, both Fe3+ and Fe have a coefficient of
(1) 1, because a total of 6 electrons is
transferred
(2) 2, because a total of 6 electrons is
transferred
(3) 1, because a total of 3 electrons is
transferred
(4) 2, because a total of 3 electrons is
tranferred
263
8/07-44
• Given the unbalanced ionic equation:
3Mg + ____Fe3+ -> 3Mg2+ + ____Fe
When this equation is balanced, both Fe3+ and Fe have a coefficient of
(1) 1, because a total of 6 electrons is
transferred
(2) 2, because a total of 6 electrons is
correct
transferred
(3) 1, because a total of 3 electrons is
transferred
(4) 2, because a total of 3 electrons is
tranferred
264
8/07-45
• A student collects the materials and equipment below to construct a
voltaic cell
•Two 250-mL beakers
•Wire and a switch
•One strip of magnesium
•One strip of copper
•125 mL of 0.20 M Mg(NO3)2(aq)
•125 mL of 0.20 M Cu(NO3)2(aq)
Which additional item is required for the construction of the voltaic cell?
(1) An anode
(2) A battery
(3) A cathode
(4) A salt bridge
265
8/07-45
• A student collects the materials and equipment below to construct a
voltaic cell
•Two 250-mL beakers
•Wire and a switch
•One strip of magnesium
•One strip of copper
•125 mL of 0.20 M Mg(NO3)2(aq)
•125 mL of 0.20 M Cu(NO3)2(aq)
Which additional item is required for the construction of the voltaic cell?
(1) An anode
(2) A battery
(3) A cathode
(4) A salt bridge
correct
266
8/07-48
• What is the pH of a solution that has hydronium ion concentration 100
times greater than a solution with a pH of 4?
(1) 5
(2) 2
(3) 3
(4) 6
267
8/07-48
• What is the pH of a solution that has hydronium ion concentration 100
times greater than a solution with a pH of 4?
(1) 5
(2) 2
(3) 3
(4) 6
correct
268
8/07-49
• Which nuclear equation represents a natural transmutation?
(1) 1
(2) 2
(3) 3
(4) 4
269
8/07-49
• Which nuclear equation represents a natural transmutation?
(1) 1
(2) 2
(3) 3
(4) 4
correct
270
8/07-50
• A nuclear fission reaction and a nuclear fusion reaction are similar
because both reactions
(1) Form heavy nuclides from light
nuclides
(2) Form light nuclides from heavy
nuclides
(3) Release a large amount of energy
(4) Absorb a large amount of energy
271
8/07-50
• A nuclear fission reaction and a nuclear fusion reaction are similar
because both reactions
(1) Form heavy nuclides from light
nuclides
(2) Form light nuclides from heavy
nuclides
(3) Release a large amount of energy
(4) Absorb a large amount of energy
correct
272
1/09-1
• On the modern Periodic Table, the elements are arranged in order of
increasing
(1) atomic mass
(2) mass number
(3) atomic number
(4) oxidation number
273
1/09-1
• On the modern Periodic Table, the elements are arranged in order of
increasing
(1) atomic mass
(2) mass number
(3) atomic number
(4) oxidation number
correct
274
1/09-2
• Which particle has a mass that is approximately the same as the mass of
a proton?
(1) an alpha particle
(2) a neutron
(3) a beta particle
(4) a positron
275
1/09-2
• Which particle has a mass that is approximately the same as the mass of
a proton?
(1) an alpha particle
(2) a neutron
(3) a beta particle
(4) a positron
correct
276
1/09-3
• An atom of an element forms a 2+ ion. In which group on the Periodic
Table could this element be located?
(1) 1
(2) 13
(3) 2
(4) 14
277
1/09-3
• An atom of an element forms a 2+ ion. In which group on the Periodic
Table could this element be located?
(1) 1
(3) 2
(2) 13
correct
(4) 14
278
1/09-4
• Which statement describes the relative energy of the electrons in the
shells of a calcium atom?
(1) An electron in the first shell has more
energy than an electron in the second
shell.
(2) An electron in the first shell has the
same amount of energy as an electron in
the second shell.
(3) An electron in the third shell has more
energy than an electron in the second
shell.
(4) An electron in the third shell has less
energy than an electron in second shell.
279
1/09-4
• Which statement describes the relative energy of the electrons in the
shells of a calcium atom?
(1) An electron in the first shell has more
energy than an electron in the second
shell.
(2) An electron in the first shell has the
same amount of energy as an electron in
the second shell.
(3) An electron in the third shell has more
energy than an electron in the second
correct
shell.
(4) An electron in the third shell has less
energy than an electron in second shell.
280
1/09-5
• According to the electron-cloud model of the atom, an orbital is a
(1) circular path traveled by an electron
around the nucleus
(2) spiral path traveled by the electron
toward the nucleus
(3) region of the most probable proton
location
(4) region of the most probable electron
location
281
1/09-5
• According to the electron-cloud model of the atom, an orbital is a
(1) circular path traveled by an electron
around the nucleus
(2) spiral path traveled by the electron
toward the nucleus
(3) region of the most probable proton
location
(4) region of the most probable electron
correct
location
282
1/09-6
• What can be determined if only the atomic number of an atom is known?
(1) the total number of neutrons in the
atom, only
(2) the total number of protons in the
atom, only
(3) the total number of protons and the
total number of neutrons in the atom
(4) the total number of protons and the
total number of electrons in the atom
283
1/09-6
• What can be determined if only the atomic number of an atom is known?
(1) the total number of neutrons in the
atom, only
(2) the total number of protons in the
atom, only
(3) the total number of protons and the
total number of neutrons in the atom
(4) the total number of protons and the
total number of electrons in the atom
correct
284
1/09-7
• The most common isotope of chromium has a mass number of 52.
Which notation represents a different isotope of chromium?
52
24Cr
(2) 24Cr54
(3) 54Cr24
(4) 52Cr24
(1)
285
1/09-7
• The most common isotope of chromium has a mass number of 52.
Which notation represents a different isotope of chromium?
52
24Cr
(2) 24Cr54
(3) 54Cr24
(4) 52Cr24
(1)
correct
286
1/09-8
• Which Group 14 element is a metalloid?
(1) tin
(2) silicon
(3) lead
(4) carbon
287
1/09-8
• Which Group 14 element is a metalloid?
(1) tin
(2) silicon
(3) lead
(4) carbon
correct
288
1/09-9
• Samples of four Group 15 elements, antimony, arsenic, bismuth, and
phosphorous, are in the gaseous phase. An atom in the ground state of
which element requires the least amount of energy to remove its most
loosely held electron?
(1) As
(2) Bi
(3) P
(4) Sb
289
1/09-9
• Samples of four Group 15 elements, antimony, arsenic, bismuth, and
phosphorous, are in the gaseous phase. An atom in the ground state of
which element requires the least amount of energy to remove its most
loosely held electron?
(1) As
(2) Bi
(3) P
(4) Sb
correct
290
1/09-10
• Which substance cab be broken down by chemical means?
(1) CO
(2) Ce
(3) Ca
(4) Cu
291
1/09-10
• Which substance cab be broken down by chemical means?
(1) CO
(3) Ca
correct
(2) Ce
(4) Cu
292
1/09-11
• During all chemical reactions, mass, energy, and charge are
(1) absorbed
(2) conserved
(3) formed
(4) released
293
1/09-11
• During all chemical reactions, mass, energy, and charge are
(1) absorbed
(2) conserved
(3) formed
(4) released
correct
294
1/09-12
• Which formula represents a molecular compound?
(1) Kr
(2) LiOH
(3) N2O4
(4) NaI
295
1/09-12
• Which formula represents a molecular compound?
(1) Kr
(3) N2O4
(2) LiOH
correct
(4) NaI
296
1/09-13
• The bonds in BaO are best described as
(1) covalent, because valence electrons
are shared
(2) covalent, because valence electrons
are transferred
(3) ionic, because valence electrons are
shared
(4) ionic, because valence electrons are
transferred
297
1/09-13
• The bonds in BaO are best described as
(1) covalent, because valence electrons
are shared
(2) covalent, because valence electrons
are transferred
(3) ionic, because valence electrons are
shared
(4) ionic, because valence electrons are
correct
transferred
298
1/09-14
• In which sample of water do the water molecules have the highest
average kinetic energy?
(1) 20. mL at 100°C
(2) 40. mL at 80°C
(3) 60. mL at 60°C
(4) 80. mL at 40°C
299
1/09-14
• In which sample of water do the water molecules have the highest
average kinetic energy?
(1) 20. mL at 100°C
(3) 60. mL at 60°C
correct
(2) 40. mL at 80°C
(4) 80. mL at 40°C
300
1/09-15
• Which compound is insoluble in water?
(1) calcium bromide
(2) potassium bromide
(3) silver bromide
(4) sodium bromide
301
1/09-15
• Which compound is insoluble in water?
(1) calcium bromide
(3) silver bromide
(2) potassium bromide
correct
(4) sodium bromide
302
1/09-16
• Which element is a brittle solid with low conductivity at STP?
(1) sulfur
(2) sodium
(3) argon
(4) aluminum
303
1/09-16
• Which element is a brittle solid with low conductivity at STP?
(1) sulfur
(3) argon
correct
(2) sodium
(4) aluminum
304
1/09-17
• Which two samples of gas at STP contain the same total number of
molecules?
(1) 1 L of CO(g) and 0.5L of N2(g)
(2) 2 L of CO(g) and 0.5L of NH3(g)
(3) 1 L of H2(g) and 2 L of Cl2(g)
(4) 2 L of H2(g) and 2 L of Cl2(g)
305
1/09-17
• Which two samples of gas at STP contain the same total number of
molecules?
(1) 1 L of CO(g) and 0.5L of N2(g)
(2) 2 L of CO(g) and 0.5L of NH3(g)
(3) 1 L of H2(g) and 2 L of Cl2(g)
(4) 2 L of H2(g) and 2 L of Cl2(g)
correct
306
1/09-18
• A reaction is most likely to occur when reactant particles collide with
(1) proper energy, only
(2) proper orientation, only
(3) both proper energy and proper
orientation
(4) neither proper energy nor proper
orientation
307
1/09-18
• A reaction is most likely to occur when reactant particles collide with
(1) proper energy, only
(2) proper orientation, only
(3) both proper energy and proper
correct
orientation
(4) neither proper energy nor proper
orientation
308
1/09-19
• The net energy released or absorbed during a reversible chemical
reaction is equal to
(1) the activation energy of the
endothermic reaction
(2) the activation energy of the
exothermic reaction
(3) the difference between the potential
energy of the reactants and the potential
energy of the products
(4) the sum of the potential energy of the
reactants and the potential energy of the
products
309
1/09-19
• The net energy released or absorbed during a reversible chemical
reaction is equal to
(1) the activation energy of the
endothermic reaction
(2) the activation energy of the
exothermic reaction
(3) the difference between the potential
energy of the reactants and the potential
correct
energy of the products
(4) the sum of the potential energy of the
reactants and the potential energy of the
products
310
1/09-20
• A catalyst lowers the activation energy of a reaction by
(1) providing an alternate energy pathway (2) decreasing the heat of reaction
(3) increasing the mass of the reactants
(4) changing the mole ratio of the
reaction
311
1/09-21
• Which element is present in every organic compound?
(1) carbon
(2) fluorine
(3) nitrogen
(4) oxygen
312
1/09-21
• Which element is present in every organic compound?
(1) carbon
(3) nitrogen
correct
(2) fluorine
(4) oxygen
313
1/09-22
• Given the balanced equation representing a reaction:
2Fe + 3Cu2+ -> 2Fe3+ + 3Cu
When the iron atoms lose six moles of electrons, how many moles of
electrons are gained by the copper ions?
(1) 12 moles
(2) 2 moles
(3) 3 moles
(4) 6 moles
314
1/09-22
• Given the balanced equation representing a reaction:
2Fe + 3Cu2+ -> 2Fe3+ + 3Cu
When the iron atoms lose six moles of electrons, how many moles of
electrons are gained by the copper ions?
(1) 12 moles
(2) 2 moles
(3) 3 moles
(4) 6 moles
correct
315
1/09-23
• Which statement describes electrolysis?
(1) chemical energy is used to produce an
electrical change
(2) chemical energy is used to produce a
thermal change
(3) electrical energy is used to produce a
chemical change
(4) thermal energy is used to produce a
chemical change
316
1/09-23
• Which statement describes electrolysis?
(1) chemical energy is used to produce an
electrical change
(2) chemical energy is used to produce a
thermal change
(3) electrical energy is used to produce a
correct
chemical change
(4) thermal energy is used to produce a
chemical change
317
1/09-24
• During which process does the atom gain one or more electrons?
(1) transmutation
(2) reduction
(3) oxidation
(4) neutralization
318
1/09-24
• During which process does the atom gain one or more electrons?
(1) transmutation
(2) reduction
(3) oxidation
(4) neutralization
correct
319
1/09-25
• Which substance is an Arrhenius base?
(1) CH3OH
(2) CH3Cl
(3) LiOH
(4) LiCl
320
1/09-25
• Which substance is an Arrhenius base?
(1) CH3OH
(3) LiOH
(2) CH3Cl
correct
(4) LiCl
321
1/09-26
• Which statement describes an alternate theory of acids and bases?
(1) Acids and bases are both H+ acceptors
(2) Acids and bases are both H+ donors
(3) Acids are H+ acceptors and bases are
H+ donors
(4) Acids are H+ donors and bases are H+
acceptors
322
1/09-26
• Which statement describes an alternate theory of acids and bases?
(1) Acids and bases are both H+ acceptors
(2) Acids and bases are both H+ donors
(3) Acids are H+ acceptors and bases are
H+ donors
(4) Acids are H+ donors and bases are H+
correct
acceptors
323
1/09-27
• Which two compounds are electrolytes?
(1) C6H12O6 and CH3CH2OH
(2) C6H12O6 and HCl
(3) NaOH and HCl
(4) NaOH and CH3CH2OH
324
1/09-27
• Which two compounds are electrolytes?
(1) C6H12O6 and CH3CH2OH
(3) NaOH and HCl
(2) C6H12O6 and HCl
correct
(4) NaOH and CH3CH2OH
325
1/09-28
• The only positive ion found in H2SO4(aq) is the
(1) ammonium ion
(2) hydronium ion
(3) hydroxide ion
(4) sulfate ion
326
1/09-28
• The only positive ion found in H2SO4(aq) is the
(1) ammonium ion
(2) hydronium ion
(3) hydroxide ion
(4) sulfate ion
correct
327
1/09-29
• Which risk is associated with using nuclear fission to produce energy in a
power plant?
(1) depletion of hydrocarbon
(2) depletion of atmospheric oxygen
(3) exposure of workers to radiation
(4) exposure of workers to sulfur dioxide
328
1/09-29
• Which risk is associated with using nuclear fission to produce energy in a
power plant?
(1) depletion of hydrocarbon
(2) depletion of atmospheric oxygen
(3) exposure of workers to radiation
(4) exposure of workers to sulfur dioxide
correct
329
1/09-30
• An unstable nucleus loses most mass if the nucleus emits
(1) an alpha particle
(2) a beta particle
(3) a positron
(4) a gamma ray
330
1/09-30
• An unstable nucleus loses most mass if the nucleus emits
(1) an alpha particle
(3) a positron
correct
(2) a beta particle
(4) a gamma ray
331
1/09-33
• What is the total number of valence electrons in an atom of germanium in
the ground state?
(1) 8
(2) 2
(3) 14
(4) 4
332
1/09-33
• What is the total number of valence electrons in an atom of germanium in
the ground state?
(1) 8
(2) 2
(3) 14
(4) 4
correct
333
1/09-34
• In the formula X2O5, the symbol X could represent an element in Group
(1) 1
(2) 2
(3) 15
(4) 18
334
1/09-35
• A 50.0-gram block of copper at 10.0°C is carefully lowered into 100.0
grams of water at 90.0°C in an insulated container. Which statement
describes the transfer of heat in this system?
(1) The water loses heat to the block until
both are at 10.0°C.
(2) The block gains heat from the water
until both are at 90.0°C.
(3) The water loses heat and the block
gains heat until both are at the same
temperature that is between 10.0°C and
90.0°C.
(4) The water gains heat and the block
loses heat until both are at the same
temperature that is between 10.0°C and
90.0°C.
335
1/09-35
• A 50.0-gram block of copper at 10.0°C is carefully lowered into 100.0
grams of water at 90.0°C in an insulated container. Which statement
describes the transfer of heat in this system?
(1) The water loses heat to the block until
both are at 10.0°C.
(2) The block gains heat from the water
until both are at 90.0°C.
(3) The water loses heat and the block
gains heat until both are at the same
temperature that is between 10.0°C and
correct
90.0°C.
(4) The water gains heat and the block
loses heat until both are at the same
temperature that is between 10.0°C and
90.0°C.
336
1/09-36
• The compounds C2H4 and C4H8 have the same
(1) freezing point at standard pressure
(2) boiling point at standard pressure
(3) molecular formula
(4) empirical formula
337
1/09-36
• The compounds C2H4 and C4H8 have the same
(1) freezing point at standard pressure
(2) boiling point at standard pressure
(3) molecular formula
(4) empirical formula
correct
338
1/09-37
• The chemical bond between which two atoms is most polar?
(1) C-N
(2) H-H
(3) S-Cl
(4) Si-O
339
1/09-37
• The chemical bond between which two atoms is most polar?
(1) C-N
(2) H-H
(3) S-Cl
(4) Si-O
correct
340
1/09-38
• What is the total amount of heat absorbed by 100.0 grams of water when
the temperature of the water is increased from 30.0°C to 45.0°C?
(1) 418 J
(2) 6270 J
(3) 12,500 J
(4) 18,800 J
341
1/09-38
• What is the total amount of heat absorbed by 100.0 grams of water when
the temperature of the water is increased from 30.0°C to 45.0°C?
(1) 418 J
(2) 6270 J
(3) 12,500 J
(4) 18,800 J
correct
342
1/09-39
• Which process is exothermic?
(1) boiling water
(2) melting copper
(3) condensing of ethanol vapor
(4) sublimation of iodine
343
1/09-39
• Which process is exothermic?
(1) boiling water
(2) melting copper
(3) condensing of ethanol vapor
(4) sublimation of iodine
correct
344
1/09-40
• Which sample, when dissolved in 1.0 liter of water, produces a solution
with the lowest freezing point?
(1) 0.1 mol of C2H5OH
(2) 0.1 mol of LiBr
(3) 0.2 mol of C6H12O6
(4) 0.2 mol of CaCl2
345
1/09-40
• Which sample, when dissolved in 1.0 liter of water, produces a solution
with the lowest freezing point?
(1) 0.1 mol of C2H5OH
(2) 0.1 mol of LiBr
(3) 0.2 mol of C6H12O6
(4) 0.2 mol of CaCl2
correct
346
1/09-43
• Which compound is an alkyne?
(1) C2H2
(2) C2H4
(3) C4H8
(4) C4H10
347
1/09-43
• Which compound is an alkyne?
(1) C2H2
(3) C4H8
correct
(2) C2H4
(4) C4H10
348
1/09-44
• What is the oxidation state of sulfur in Na2S2O3?
(1) -1
(2) +2
(3) +6
(4) +4
349
1/09-44
• What is the oxidation state of sulfur in Na2S2O3?
(1) -1
(2) +2
(3) +6
(4) +4
correct
350
1/09-47
• A 25.0-milliliter sample of HNO3(aq) is neutralized by 32.1 milliliters of
0.150 M KOH(aq). What is the molarity of the HNO3(aq)?
(1) 0.117 M
(2) 0.150 M
(3) 0.193 M
(4) 0.300 M
351
1/09-47
• A 25.0-milliliter sample of HNO3(aq) is neutralized by 32.1 milliliters of
0.150 M KOH(aq). What is the molarity of the HNO3(aq)?
(1) 0.117 M
(3) 0.193 M
(2) 0.150 M
correct
(4) 0.300 M
352
1/09-48
• Which nuclide has a half-life that is less than one minute?
(1) cesium-137
(2) francium-220
(3) phosphorous-32
(4) strontium-90
353
1/09-48
• Which nuclide has a half-life that is less than one minute?
(1) cesium-137
(2) francium-220
(3) phosphorous-32
(4) strontium-90
correct
354
1/09-50
• Cobalt-60 and iodine-131 are radioactive isotopes that are used in
(1) dating geologic formations
(2) industrial measurements
(3) medical procedures
(4) nuclear power
355
1/09-50
• Cobalt-60 and iodine-131 are radioactive isotopes that are used in
(1) dating geologic formations
(2) industrial measurements
(3) medical procedures
(4) nuclear power
correct
356
1/08-1
• Which quantity indentifies an element?
(1) atomic number
(2) mass number
(3) total number of neutrons in an atom
of an element
(4) total number of valence electrons in
an atom of an element
357
1/08-1
• Which quantity indentifies an element?
(1) atomic number
correct
(3) total number of neutrons in an atom
of an element
(2) mass number
(4) total number of valence electrons in
an atom of an element
358
1/08-2
• Which atom in the ground state has a partially filled second electron
shell?
(1) hydrogen atom
(2) lithium atom
(3) potassium atom
(4) sodium atom
359
1/08-2
• Which atom in the ground state has a partially filled second electron
shell?
(1) hydrogen atom
(2) lithium atom
(3) potassium atom
(4) sodium atom
correct
360
1/08-3
• What is the total charge of the nucleus of a nitrogen atom?
(1) +5
(2) +2
(3) +7
(4) +14
361
1/08-3
• What is the total charge of the nucleus of a nitrogen atom?
(1) +5
(3) +7
(2) +2
correct
(4) +14
362
1/08-4
• Which value of an element is calculated using both the mass and the
relative abundance of each of the naturally occurring isotopes of this
element?
(1) atomic number
(2) atomic mass
(3) half-life
(4) molar volume
363
1/08-4
• Which value of an element is calculated using both the mass and the
relative abundance of each of the naturally occurring isotopes of this
element?
(1) atomic number
(2) atomic mass
(3) half-life
(4) molar volume
correct
364
1/08-5
• The mass of 12 protons is approximately equal to
(1) 1 atomic mass unit
(2) 12 atomic mass units
(3) the mass of 1 electron
(4) the mass of 12 electrons
365
1/08-5
• The mass of 12 protons is approximately equal to
(1) 1 atomic mass unit
(2) 12 atomic mass units
(3) the mass of 1 electron
(4) the mass of 12 electrons
correct
366
1/08-6
• Sodium atoms, potassium atoms, and cesium atoms have the same
(1) atomic radius
(2) first ionization energy
(3) total number of protons
(4) oxidation state
367
1/08-6
• Sodium atoms, potassium atoms, and cesium atoms have the same
(1) atomic radius
(2) first ionization energy
(3) total number of protons
(4) oxidation state
correct
368
1/08-7
• Which statement describes a chemical property of hydrogen gas?
(1) hydrogen burns in air
(2) hydrogen gas is colorless
(3) hydrogen gas has a density of 0.00009
g/cm3
(4) hydrogen gas has a boiling point of 20.
K at standard pressure.
369
1/08-7
• Which statement describes a chemical property of hydrogen gas?
(1) hydrogen burns in air
(2) hydrogen gas is colorless
(3) hydrogen gas has a density of 0.00009
g/cm3
(4) hydrogen gas has a boiling point of 20.
K at standard pressure.
correct
370
1/08-8
• Which element has the greatest density at STP?
(1) calcium
(2) carbon
(3) chlorine
(4) copper
371
1/08-8
• Which element has the greatest density at STP?
(1) calcium
(2) carbon
(3) chlorine
(4) copper
correct
372
1/08-9
• Which equation shows conservation of atoms?
(1) H2 + O2 -> H2O
(2) H2 + O2 -> 2H2O
(3) 2H2 + O2 -> 2H2O
(4) 2H2 + 2O2 -> 2H2O
373
1/08-9
• Which equation shows conservation of atoms?
(1) H2 + O2 -> H2O
(3) 2H2 + O2 -> 2H2O
(2) H2 + O2 -> 2H2O
correct
(4) 2H2 + 2O2 -> 2H2O
374
1/08-10
• Which term indicates how strongly an atom attracts the electrons in a
chemical bond?
(1) alkalinity
(2) atomic mass
(3) electronegativity
(4) activation energy
375
1/08-10
• Which term indicates how strongly an atom attracts the electrons in a
chemical bond?
(1) alkalinity
(3) electronegativity
(2) atomic mass
correct
(4) activation energy
376
1/08-11
• A solid substance is an excellent conductor of electricity. The chemical
bonds in this substance are most likely
(1) ionic, because the valence electrons
are shared between atoms
(2) ionic, because the valence electrons
are mobile
(3) electronegativity
(4) activation energy
377
1/08-11
• A solid substance is an excellent conductor of electricity. The chemical
bonds in this substance are most likely
(1) ionic, because the valence electrons
are shared between atoms
(2) ionic, because the valence electrons
are mobile
(3) electronegativity
(4) activation energy
correct
378
1/08-12
• Magnesium nitrate contains chemical bonds that are
(1) covalent, only
(2) ionic, only
(3) both covalent and ionic
(4) neither covalent nor ionic
379
1/08-12
• Magnesium nitrate contains chemical bonds that are
(1) covalent, only
(3) both covalent and ionic
(2) ionic, only
correct
(4) neither covalent nor ionic
380
1/08-13
• Which substance can be broken down by a chemical change?
(1) antimony
(2) carbon
(3) hexane
(4) sulfur
381
1/08-13
• Which substance can be broken down by a chemical change?
(1) antimony
(3) hexane
(2) carbon
correct
(4) sulfur
382
1/08-14
• Which barium salt is insoluble in water?
(1) BaCO3
(2) BaCl2
(3) Ba(ClO4)2
(4) Ba(NO3)2
383
1/08-14
• Which barium salt is insoluble in water?
(1) BaCO3
(3) Ba(ClO4)2
correct
(2) BaCl2
(4) Ba(NO3)2
384
1/08-16
• Under which conditions of temperature and pressure is a gas most
soluble in water?
(1) high temperature and low pressure
(2) high temperature and high pressure
(3) low temperature and low pressure
(4) low temperature and high pressure
385
1/08-16
• Under which conditions of temperature and pressure is a gas most
soluble in water?
(1) high temperature and low pressure
(2) high temperature and high pressure
(3) low temperature and low pressure
(4) low temperature and high pressure
correct
386
1/08-15
• Which unit can be used to express solution concentration?
(1) J/mol
(2) L/mol
(3) mol/L
(4) mol/s
387
1/08-15
• Which unit can be used to express solution concentration?
(1) J/mol
(3) mol/L
(2) L/mol
correct
(4) mol/s
388
1/08-17
• Given the equation representing a system at equilibrium:
H2O(s) = H2O(l)
At which temperature does the equilibrium exist at 101.3 kPa?
(1) 0 K
(2) 0°C
(3) 32 K
(4) 273°C
389
1/08-17
• Given the equation representing a system at equilibrium:
H2O(s) = H2O(l)
At which temperature does the equilibrium exist at 101.3 kPa?
(1) 0 K
(2) 0°C
(3) 32 K
(4) 273°C
correct
390
1/08-18
• In a redox reaction, the total number of electrons lost is
(1) less than the total number of electrons (2) greater than the total number of
gained
electrons gained
(3) equal to the total number of electrons
gained
(4) equal to the total number of protons
gained
391
1/08-18
• In a redox reaction, the total number of electrons lost is
(1) less than the total number of electrons (2) greater than the total number of
gained
electrons gained
(3) equal to the total number of electrons
correct
gained
(4) equal to the total number of protons
gained
392
1/08-19
• Which formula represents and alkene?
(1) C2H6
(2) C3H6
(3) C4H10
(4) C5H12
393
1/08-19
• Which formula represents and alkene?
(1) C2H6
(2) C3H6
(3) C4H10
(4) C5H12
correct
394
1/08-20
• Which term refers to the difference between the potential energy of the
products and the potential energy of the reactants for any chemical
change?
(1) heat of decomposition
(2) heat of fusion
(3) heat of reaction
(4) heat of vaporization
395
1/08-20
• Which term refers to the difference between the potential energy of the
products and the potential energy of the reactants for any chemical
change?
(1) heat of decomposition
(3) heat of reaction
(2) heat of fusion
correct
(4) heat of vaporization
396
1/08-21
• Which energy conversion occurs in a voltaic cell?
(1) chemical energy to electrical energy
(2) chemical energy to nuclear energy
(3) electrical energy to chemical energy
(4) nuclear energy to electrical energy
397
1/08-21
• Which energy conversion occurs in a voltaic cell?
(1) chemical energy to electrical energy
(2) chemical energy to nuclear energy
(3) electrical energy to chemical energy
(4) nuclear energy to electrical energy
correct
398
1/08-22
• Which metal is more active than Ni and less active than Zn?
(1) Cu
(2) Cr
(3) Mg
(4) Pb
399
1/08-22
• Which metal is more active than Ni and less active than Zn?
(1) Cu
(2) Cr
(3) Mg
(4) Pb
correct
400
1/08-23
• As water is added to a 0.10 M NaCl aqueous solution, the conductivity of
the resulting solution
(1) decreases because the concentration
of the ions decreases
(2) decreases, but the concentration of
ions remains the same
(3) increases because the concentration
of ions decreases
(4) increases, but the concentration of
ions remains the same
401
1/08-23
• As water is added to a 0.10 M NaCl aqueous solution, the conductivity of
the resulting solution
(1) decreases because the concentration
correct
of the ions decreases
(2) decreases, but the concentration of
ions remains the same
(3) increases because the concentration
of ions decreases
(4) increases, but the concentration of
ions remains the same
402
1/08-24
• Which substance is an Arrhenius acid?
(1) Ba(OH)2
(2) CH3COOCH3
(3) H3PO4
(4) NaCl
403
1/08-24
• Which substance is an Arrhenius acid?
(1) Ba(OH)2
(3) H3PO4
(2) CH3COOCH3
correct
(4) NaCl
404
1/08-25
• Which compound releases hydroxide ions in an aqueous solution?
(1) CH3COOH
(2) CH3OH
(3) HCl
(4) KOH
405
1/08-25
• Which compound releases hydroxide ions in an aqueous solution?
(1) CH3COOH
(2) CH3OH
(3) HCl
(4) KOH
correct
406
1/08-26
• Which reaction converts an atom of one element to an atom of another
element?
(1) combustion
(2) polymerization
(3) saponification
(4) transmutation
407
1/08-26
• Which reaction converts an atom of one element to an atom of another
element?
(1) combustion
(2) polymerization
(3) saponification
(4) transmutation
correct
408
1/08-27
• Which nuclear emission has the greatest mass?
(1) alpha particle
(2) beta particle
(3) gamma ray
(4) positron
409
1/08-27
• Which nuclear emission has the greatest mass?
(1) alpha particle
(3) gamma ray
correct
(2) beta particle
(4) positron
410
1/08-28
• Which two isotopes have the same decay mode?
(1) 37Ca and 53Fe
(2) 220Fr and 60Co
(3) 37K and 42K
(4) 99Tc and 19Ne
411
1/08-28
• Which two isotopes have the same decay mode?
(1) 37Ca and 53Fe
(3) 37K and 42K
correct
(2) 220Fr and 60Co
(4) 99Tc and 19Ne
412
1/08-29
• Which list of nuclear emissions is arranged in order from the least
penetrating power to the greatest penetrating power?
(1) alpha particle, beta particle, gamma
ray
(2) alpha particle, gamma ray, beta
particle
(3) gamma ray, beta particle, alpha
particle
(4) beta particle, alpha particle, gamma
ray
413
1/08-29
• Which list of nuclear emissions is arranged in order from the least
penetrating power to the greatest penetrating power?
(1) alpha particle, beta particle, gamma
correct
ray
(2) alpha particle, gamma ray, beta
particle
(3) gamma ray, beta particle, alpha
particle
(4) beta particle, alpha particle, gamma
ray
414
1/08-30
• One benefit of nuclear fission reactions is
(1) nuclear reactor meltdowns
(2) storage of waste materials
(3) biological exposure
(4) production of energy
415
1/08-30
• One benefit of nuclear fission reactions is
(1) nuclear reactor meltdowns
(2) storage of waste materials
(3) biological exposure
(4) production of energy
correct
416
1/08-31
• Which list of elements consists of metalloids only?
(1) B, Al, Ga
(2) C, N, P
(3) O, S, Se
(4) Si, Ge, As
417
1/08-31
• Which list of elements consists of metalloids only?
(1) B, Al, Ga
(2) C, N, P
(3) O, S, Se
(4) Si, Ge, As
correct
418
1/08-32
• Which two notations represent different isotopes of the same element?
(1) 4Be6 and 4Be9
(2) 3Li7 and 3Li7
(3) 7N14 and 6C14
(4) 15P32 and 16S32
419
1/08-32
• Which two notations represent different isotopes of the same element?
(1) 4Be6 and 4Be9
(3) 7N14 and 6C14
correct
(2) 3Li7 and 3Li7
(4) 15P32 and 16S32
420
1/08-33
• Which general trend is found in Period 2 on the Periodic Table as the
elements are considered in order of increasing atomic number?
(1) decreasing atomic mass
(2) decreasing electronegativity
(3) increasing atomic radius
(4) increasing first ionization energy
421
1/08-33
• Which general trend is found in Period 2 on the Periodic Table as the
elements are considered in order of increasing atomic number?
(1) decreasing atomic mass
(2) decreasing electronegativity
(3) increasing atomic radius
(4) increasing first ionization energy
correct
422
1/08-34
• What is the gram-formula mass of Ca3(PO4)2?
(1) 248 g/mol
(2) 263 g/mol
(3) 279 g/mol
(4) 310. g/mol
423
1/08-34
• What is the gram-formula mass of Ca3(PO4)2?
(1) 248 g/mol
(2) 263 g/mol
(3) 279 g/mol
(4) 310. g/mol
correct
424
1/08-36
• When sodium and fluorine combine to produce the compound NaF, the
ions formed have the same electron configuration as atoms of
(1) argon, only
(2) neon, only
(3) both argon and neon
(4) neither argon nor neon
425
1/08-36
• When sodium and fluorine combine to produce the compound NaF, the
ions formed have the same electron configuration as atoms of
(1) argon, only
(2) neon, only
(3) both argon and neon
(4) neither argon nor neon
correct
426
1/08-35
• What is the total number of pairs of electrons shared between the carbon
atom and the oxygen atom in a molecule of methanal?
(1) 1
(2) 2
(3) 3
(4) 4
427
1/08-35
• What is the total number of pairs of electrons shared between the carbon
atom and the oxygen atom in a molecule of methanal?
(1) 1
(2) 2
(3) 3
(4) 4
correct
428
1/08-37
• In which compound is the ratio of metal ions to nonmetal ions 1 to 2?
(1) calcium bromide
(2) calcium oxide
(3) calcium phosphide
(4) calcium sulfide
429
1/08-37
• In which compound is the ratio of metal ions to nonmetal ions 1 to 2?
(1) calcium bromide
(3) calcium phosphide
correct
(2) calcium oxide
(4) calcium sulfide
430
1/08-38
• What is the concentration of O2(g), in parts per million, in a solution that
contains 0.008 gram of O2(g) dissolved in 1000. grams of H2O(l)?
(1) 0.8 ppm
(2) 8 ppm
(3) 80 ppm
(4) 800 ppm
431
1/08-38
• What is the concentration of O2(g), in parts per million, in a solution that
contains 0.008 gram of O2(g) dissolved in 1000. grams of H2O(l)?
(1) 0.8 ppm
(2) 8 ppm
(3) 80 ppm
(4) 800 ppm
correct
432
1/08-40
• At which temperature is the vapor pressure of ethanol equal to the vapor
pressure of propanone at 35°C?
(1) 35°C
(2) 60.°C
(3) 82°C
(4) 95°C
correct
433
1/08-41
• A rigid cylinder with a moveable piston contains a 2.0-Liter sample of
neon gas at STP. What is the volume of this sample of neon gas when its
temperature is increased to 30.°C while its pressure is decreased to 90.
kilopascals?
(1) 2.5 L
(2) 2.0 L
(3) 1.6 L
(4) 0.22 L
434
1/08-41
• A rigid cylinder with a moveable piston contains a 2.0-Liter sample of
neon gas at STP. What is the volume of this sample of neon gas when its
temperature is increased to 30.°C while its pressure is decreased to 90.
kilopascals?
(1) 2.5 L
(3) 1.6 L
correct
(2) 2.0 L
(4) 0.22 L
435
1/08-42
• Which compound is a saturated hydrocarbon?
(1) CH2CH2
(2) CH3CHO
(3) CH3CH3
(4) CH3CH2OH
436
1/08-42
• Which compound is a saturated hydrocarbon?
(1) CH2CH2
(3) CH3CH3
(2) CH3CHO
correct
(4) CH3CH2OH
437
1/08-43
• A molecule of a compound contains a total of 10 hydrogen atoms and has
the general formula CnH2n+2. Which prefix is used in the name of this
compound?
(1) but-
(2) dec-
(3) oct-
(4) pent-
438
1/08-43
• A molecule of a compound contains a total of 10 hydrogen atoms and has
the general formula CnH2n+2. Which prefix is used in the name of this
compound?
(1) but(3) oct-
correct
(2) dec(4) pent-
439
1/08-44
• Reduction occurs at the cathode in
(1) electrolytic cells, only
(2) voltaic cells, only
(3) both electrolytic cells and voltaic cells
(4) neither electrolytic cells nor voltaic
cells
440
1/08-44
• Reduction occurs at the cathode in
(1) electrolytic cells, only
(2) voltaic cells, only
(3) both electrolytic cells and voltaic cells
(4) neither electrolytic cells nor voltaic
cells
correct
441
1/08-45
• Which are the products of a reaction between KOH(aq) and HCl(aq)?
(1) H2 and KClO3
(2) H2O and KCl
(3) KH and HClO
(4) KOH and HCl
442
1/08-45
• Which are the products of a reaction between KOH(aq) and HCl(aq)?
(1) H2 and KClO3
(2) H2O and KCl
(3) KH and HClO
(4) KOH and HCl
correct
443
1/08-46
• Which volume of 0.10 M NaOH(aq) exactly neutralizes 15.0 millimliters of
0.20 M HNO3(aq)?
(1) 1.5 mL
(2) 7.5 mL
(3) 3.0 mL
(4) 30. mL
444
1/08-47
• Which indicator, when added to a solution, changes color from yellow to
blue as the pH of the solution in changed from 5.5 to 8.0?
(1) bromcresol green
(2) bromthymol blue
(3) litmus
(4) methyl orange
445
1/08-47
• Which indicator, when added to a solution, changes color from yellow to
blue as the pH of the solution in changed from 5.5 to 8.0?
(1) bromcresol green
(2) bromthymol blue
(3) litmus
(4) methyl orange
correct
446
1/08-48
• The pH of an aqueous solution changes from 4 to 3 when hydrogen ion
concentration in the solution is
(1) decreased by a factor of 3/4
(2) decreased by a factor of 10
(3) increased by a factor of 4/3
(4) increased by a factor of 10
447
1/08-48
• The pH of an aqueous solution changes from 4 to 3 when hydrogen ion
concentration in the solution is
(1) decreased by a factor of 3/4
(2) decreased by a factor of 10
(3) increased by a factor of 4/3
(4) increased by a factor of 10
correct
448
1/08-49
• Which fraction of an original 20.00-gram sample of nitrogen-16 remains
unchanged after 36.0 seconds?
(1) 1/5
(2) 1/8
(3) 1/16
(4) 1/32
449
1/08-49
• Which fraction of an original 20.00-gram sample of nitrogen-16 remains
unchanged after 36.0 seconds?
(1) 1/5
(2) 1/8
(3) 1/16
(4) 1/32
correct
450
1/08-50
• Which radioactive isotope is used in treating cancer?
(1) carbon-14
(2) cobalt-60
(3) lead-206
(4) uranium-238
451
1/08-50
• Which radioactive isotope is used in treating cancer?
(1) carbon-14
(3) lead-206
(2) cobalt-60
correct
(4) uranium-238
452
6/08-1
• An atom in the ground state has seven valence electrons. This atom
could be an atom of which element?
(1) calcium
(2) fluorine
(3) oxygen
(4) sodium
453
6/08-1
• An atom in the ground state has seven valence electrons. This atom
could be an atom of which element?
(1) calcium
(2) fluorine
(3) oxygen
(4) sodium
correct
454
6/08-2
• What is the total number of electrons in an atom of potassium??
(1) 18
(2) 19
(3) 20
(4) 39
455
6/08-2
• What is the total number of electrons in an atom of potassium??
(1) 18
(2) 19
(3) 20
(4) 39
correct
456
6/08-3
• A proton has a charge that is opposite the charge of
(1) an alpha particle
(2) a neutron
(3) an electron
(4) a positron
457
6/08-3
• A proton has a charge that is opposite the charge of
(1) an alpha particle
(3) an electron
(2) a neutron
correct
(4) a positron
458
6/08-4
• Which conclusion was a direct result of the gold foil experiment?
(1) An atom is mostly empty space with a
dense, positively charged nucleus.
(2) An atom is composed of at least three
types of subatomic particles.
(3) An electron has a positive charge and
is located inside the nucleus.
(4) An electron has properties of both
waves and particles.
459
6/08-4
• Which conclusion was a direct result of the gold foil experiment?
(1) An atom is mostly empty space with a
dense, positively charged nucleus.
(2) An atom is composed of at least three
types of subatomic particles.
(3) An electron has a positive charge and
is located inside the nucleus.
(4) An electron has properties of both
waves and particles.
correct
460
6/08-5
• Which statement identifies the element arsenic?
(1) Arsenic has an atomic number of 33.
(2) Arsenic has a melting point of 84 K.
(3) An atom of arsenic in the ground state
has eight valence electrons.
(4) An atom of arsenic in the ground state
has a radius of 146 pm.
461
6/08-5
• Which statement identifies the element arsenic?
(1) Arsenic has an atomic number of 33.
(2) Arsenic has a melting point of 84 K.
correct
(3) An atom of arsenic in the ground state
has eight valence electrons.
(4) An atom of arsenic in the ground state
has a radius of 146 pm.
462
6/08-6
• Which element has an atom with the greatest attraction for electrons in a
chemical bond?
(1) As
(2) Bi
(3) N
(4) P
463
6/08-6
• Which element has an atom with the greatest attraction for electrons in a
chemical bond?
(1) As
(3) N
(2) Bi
correct
(4) P
464
6/08-7
• Given the balanced equation representing a reaction:
H+(aq) + OH-(aq) -> H2O(l) + energy
In this reaction there is a conservation of
(1) mass, only
(2) mass and charge, only
(3) charge and energy, only
(4) charge , energy, and mass
465
6/08-7
• Given the balanced equation representing a reaction:
H+(aq) + OH-(aq) -> H2O(l) + energy
In this reaction there is a conservation of
(1) mass, only
(2) mass and charge, only
(3) charge and energy, only
(4) charge , energy, and mass
correct
466
6/08-8
• Which statement describes the composition of potassium chlorate,
KClO3?
(1) The proportion by mass of elements
combined in potassium chlorate is
fixed.
(2) The proportion by mass of elements
combined in potassium chlorate varies.
(3) Potassium chlorate is composed of
four elements.
(4) Potassium chlorate is composed of five
elements.
467
6/08-8
• Which statement describes the composition of potassium chlorate,
KClO3?
(1) The proportion by mass of elements
combined in potassium chlorate is
correct
fixed.
(2) The proportion by mass of elements
combined in potassium chlorate varies.
(3) Potassium chlorate is composed of
four elements.
(4) Potassium chlorate is composed of five
elements.
468
6/08-9
• As a bond between a hydrogen atom and a sulfur atom is formed,
electrons are
(1) shared to form an ionic bond
(2) shared to form a covalent bond
(3) transferred to form an ionic bond
(4) transferred to form a covalent bond
469
6/08-9
• As a bond between a hydrogen atom and a sulfur atom is formed,
electrons are
(1) shared to form an ionic bond
(2) shared to form a covalent bond
correct
(3) transferred to form an ionic bond
(4) transferred to form a covalent bond
470
6/08-10
• Atoms of which element can bond to each other to form chains, rings, and
networks?
(1) carbon
(2) fluorine
(3) hydrogen
(4) oxygen
471
6/08-10
• Atoms of which element can bond to each other to form chains, rings, and
networks?
(1) carbon
(3) hydrogen
correct
(2) fluorine
(4) oxygen
472
6/08-11
• Which formula represents a polar molecule?
(1) Br2
(2) CO2
(3) CH4
(4) NH3
473
6/08-11
• Which formula represents a polar molecule?
(1) Br2
(2) CO2
(3) CH4
(4) NH3
correct
474
6/08-12
• Two solid sample each contain sulfur, oxygen, and sodium atoms, only.
These samples have the same color, melting point, density, and reaction
with an aqueous solution of barium chloride solution. It can be concluded
that the two samples are the same
(1) compound
(2) element
(3) mixture
(4) solution
475
6/08-12
• Two solid sample each contain sulfur, oxygen, and sodium atoms, only.
These samples have the same color, melting point, density, and reaction
with an aqueous solution of barium chloride solution. It can be concluded
that the two samples are the same
(1) compound
(3) mixture
correct
(2) element
(4) solution
476
6/08-13
• Which equation represents a physical change?
(1) 1
(2) 2
(3) 3
(4) 4
477
6/08-13
• Which equation represents a physical change?
(1) 1
(3) 3
correct
(2) 2
(4) 4
478
6/08-14
• Which liquid has the lowest vapor pressure at 65°C?
(1) ethanoic acid
(2) propanone
(3) ethanol
(4) water
479
6/08-14
• Which liquid has the lowest vapor pressure at 65°C?
(1) ethanoic acid
(3) ethanol
correct
(2) propanone
(4) water
480
6/08-15
• Which substance cannot be broken down by a chemical reaction?
(1) ammonia
(2) argon
(3) methane
(4) water
481
6/08-15
• Which substance cannot be broken down by a chemical reaction?
(1) ammonia
(2) argon
(3) methane
(4) water
correct
482
6/08-16
• In which sample is the average kinetic energy of the particles greatest?
(1) 10. mL of HCl(aq) at 25°C
(2) 15 mL of HCl(aq) at 20.°C
(3) 10. mL of H2O at 35°C
(4) 15 mL of H2O at 30.°C
483
6/08-16
• In which sample is the average kinetic energy of the particles greatest?
(1) 10. mL of HCl(aq) at 25°C
(2) 15 mL of HCl(aq) at 20.°C
(3) 10. mL of H2O at 35°C
(4) 15 mL of H2O at 30.°C
correct
484
6/08-17
• A thermometer is in a beaker of water. Which statement best explains
why the thermometer reading initially increases when LiBr(s) is dissolved
in the water.
(1) The entropy of the LiBr(aq) is greater
than the entropy of the water.
(2) The entropy of the LiBr(aq) is less than
the entropy of the water.
(3) The dissolving of the LiBr(s) in water is
an endothermic process.
(4) The dissolving of LiBr(s) in water is an
exothermic process.
485
6/08-17
• A thermometer is in a beaker of water. Which statement best explains
why the thermometer reading initially increases when LiBr(s) is dissolved
in the water.
(1) The entropy of the LiBr(aq) is greater
than the entropy of the water.
(2) The entropy of the LiBr(aq) is less than
the entropy of the water.
(3) The dissolving of the LiBr(s) in water is
an endothermic process.
(4) The dissolving of LiBr(s) in water is an
exothermic process.
correct
486
6/08-18
• Which process increases the potential energy of the particles in a
sample?
(1) condensation
(2) deposition
(3) solidification
(4) vaporization
487
6/08-18
• Which process increases the potential energy of the particles in a
sample?
(1) condensation
(2) deposition
(3) solidification
(4) vaporization
correct
488
6/08-19
• Which sample at STP has the same number of molecules as 5 Liters of
NO2(g) at STP?
(1) 5 grams of H2(g)
(2) 5 liters of CH4(g)
(3) 5 moles of O2(g)
(4) 5 x 1023 molecules of CO2(g)
489
6/08-19
• Which sample at STP has the same number of molecules as 5 Liters of
NO2(g) at STP?
(1) 5 grams of H2(g)
(2) 5 liters of CH4(g)
(3) 5 moles of O2(g)
(4) 5 x 1023 molecules of CO2(g)
correct
490
6/08-20
• Under which conditions of temperature and pressure does oxygen gas
behave least like an ideal gas?
(1) low temperature and low pressure
(2) low temperature and high pressure
(3) high temperature and low pressure
(4) high temperature and high pressure
491
6/08-20
• Under which conditions of temperature and pressure does oxygen gas
behave least like an ideal gas?
(1) low temperature and low pressure
(2) low temperature and high pressure
(3) high temperature and low pressure
(4) high temperature and high pressure
correct
492
6/08-21
• How is a chemical reaction affected by the addition of a catalyst?
(1) The activation energy decreases.
(2) The heat of reaction increases.
(3) The number of collisions between
particles increases.
(4) The potential energy of the reactants
increases.
493
6/08-21
• How is a chemical reaction affected by the addition of a catalyst?
(1) The activation energy decreases.
(2) The heat of reaction increases.
(3) The number of collisions between
particles increases.
(4) The potential energy of the reactants
increases.
correct
494
6/08-22
• Systems in nature tend to undergo changes toward
(1) lower energy and lower disorder
(2) lower energy and more disorder
(3) higher energy and less disorder
(4) higher energy and more disorder
495
6/08-22
• Systems in nature tend to undergo changes toward
(1) lower energy and lower disorder
(2) lower energy and more disorder
(3) higher energy and less disorder
(4) higher energy and more disorder
correct
496
6/08-23
• What can be concluded if an ion of an element is smaller than an atom of
the same element?
(1) The ion is negatively charged because
it has fewer electrons than the atom.
(2) The ion is negatively charged because
it has more electrons than the atom.
(3) The ion is positively charged because it (4) The ion is positively charged because it
has fewer electrons than the atom.
has more electrons than the atom.
497
6/08-23
• What can be concluded if an ion of an element is smaller than an atom of
the same element?
(1) The ion is negatively charged because
it has fewer electrons than the atom.
(2) The ion is negatively charged because
it has more electrons than the atom.
(3) The ion is positively charged because it (4) The ion is positively charged because it
has fewer electrons than the atom.correct
has more electrons than the atom.
498
6/08-24
• Which class of compounds has molecules that contain nitrogen atoms?
(1) alcohol
(2) amine
(3) ether
(4) ketone
499
6/08-24
• Which class of compounds has molecules that contain nitrogen atoms?
(1) alcohol
(2) amine
(3) ether
(4) ketone
correct
500
6/08-25
• Which two compounds have the same molecular formula but different
chemical and physical properties?
(1) CH3CH2Cl and CH3CH2Br
(2) CH3CHCH2 and CH3CH2CH3
(3) CH3CHO and CH3COCH3
(4) CH3CH2OH and CH3OCH3
501
6/08-25
• Which two compounds have the same molecular formula but different
chemical and physical properties?
(1) CH3CH2Cl and CH3CH2Br
(2) CH3CHCH2 and CH3CH2CH3
(3) CH3CHO and CH3COCH3
(4) CH3CH2OH and CH3OCH3
correct
502
6/08-26
• Which half reaction equation represents the reduction of a potassium
ion?
(1) K+ + e- -> K
(2) K + e- -> K+
(3) K+ -> K + e-
(4) K -> K+ + e-
503
6/08-26
• Which half reaction equation represents the reduction of a potassium
ion?
(1) K+ + e- -> K
(3) K+ -> K + e-
correct
(2) K + e- -> K+
(4) K -> K+ + e-
504
6/08-27
• According to the Arrhenius theory, an acid is a substance that
(1) changes litmus from red to blue
(2) changes phenolphthalein from
colorless to pink
(3) produces hydronium ions as the only
positive ions in an aqueous solution
(4) produces hydroxide ions as the only
negative ion in an aqueous solution
505
6/08-27
• According to the Arrhenius theory, an acid is a substance that
(1) changes litmus from red to blue
(2) changes phenolphthalein from
colorless to pink
(3) produces hydronium ions as the only
correct
positive ions in an aqueous solution
(4) produces hydroxide ions as the only
negative ion in an aqueous solution
506
6/08-28
• Which type of reaction occurs when a high-energy particle collides with
the nucleus of an atom, converting that atom to an atom of a different
element?
(1) addition
(2) neutralization
(3) substitution
(4) transmutation
507
6/08-28
• Which type of reaction occurs when a high-energy particle collides with
the nucleus of an atom, converting that atom to an atom of a different
element?
(1) addition
(2) neutralization
(3) substitution
(4) transmutation
correct
508
6/08-29
• Which particle is emitted when an atom of 85Kr spontaneously decays?
(1) an alpha particle
(2) a beta particle
(3) a neutron
(4) a proton
509
6/08-29
• Which particle is emitted when an atom of 85Kr spontaneously decays?
(1) an alpha particle
(2) a beta particle
(3) a neutron
(4) a proton
correct
510
6/08-30
• What is a problem commonly associated with nuclear power facilities?
(1) A small quantity of energy is
produced.
(2) Reaction products contribute to acid
rain.
(3) It is impossible to control nuclear
fission.
(4) It is difficult to dispose of waste.
511
6/08-30
• What is a problem commonly associated with nuclear power facilities?
(1) A small quantity of energy is
produced.
(2) Reaction products contribute to acid
rain.
(3) It is impossible to control nuclear
fission.
(4) It is difficult to dispose of waste.
correct
512
6/08-31
• The wave-mechanical model of the atom is required to explain the
(1) mass number and atomic number of
an atom
(2) organization of atoms in crystals
(3) radioactive nature of some atoms
(4) spectra of elements in multielectron
atoms
513
6/08-31
• The wave-mechanical model of the atom is required to explain the
(1) mass number and atomic number of
an atom
(2) organization of atoms in crystals
(3) radioactive nature of some atoms
(4) spectra of elements in multielectron
correct
atoms
514
6/08-32
• Magnesium and calcium have similar chemical properties because an
atom of each element has the same total number of
(1) electron shells
(2) valence electrons
(3) neutrons
(4) protons
515
6/08-32
• Magnesium and calcium have similar chemical properties because an
atom of each element has the same total number of
(1) electron shells
(2) valence electrons
(3) neutrons
(4) protons
correct
516
6/08-34
• A barium atom attains a stable electron configuration when it bonds with
(1) one chlorine atom
(2) two chlorine atoms
(3) one sodium atom
(4) two sodium atoms
517
6/08-34
• A barium atom attains a stable electron configuration when it bonds with
(1) one chlorine atom
(2) two chlorine atoms
(3) one sodium atom
(4) two sodium atoms
correct
518
6/08-35
• A student measures the mass and volume of a piece of aluminum. The
measurements are 25.6 grams and 9.1 cubic centimeters. The student
calculates the density of the aluminum. What is the percent error of the
student’s calculated density of aluminum?
(1) 1%
(2) 2%
(3) 3%
(4) 4%
519
6/08-35
• A student measures the mass and volume of a piece of aluminum. The
measurements are 25.6 grams and 9.1 cubic centimeters. The student
calculates the density of the aluminum. What is the percent error of the
student’s calculated density of aluminum?
(1) 1%
(2) 2%
(3) 3%
(4) 4%
correct
520
6/08-36
• Given the balanced equation representing a reaction:
2H2 + O2 -> 2H2O
What is the total mass of water formed when 8 grams of hydrogen reacts
completely with 64 grams of oxygen?
(1) 18 g
(2) 36 g
(3) 56 g
(4) 72 g
521
6/08-36
• Given the balanced equation representing a reaction:
2H2 + O2 -> 2H2O
What is the total mass of water formed when 8 grams of hydrogen reacts
completely with 64 grams of oxygen?
(1) 18 g
(2) 36 g
(3) 56 g
(4) 72 g
correct
522
6/08-37
• Which compound contains both ionic and covalent bonds?
(1) ammonia
(2) methane
(3) sodium nitrate
(4) potassium chloride
523
6/08-37
• Which compound contains both ionic and covalent bonds?
(1) ammonia
(3) sodium nitrate
(2) methane
correct
(4) potassium chloride
524
6/08-38
• An iron bar at 325 K is placed in a sample of water. The iron bar gains
energy from the water if the temperature of the water is
(1) 65 K
(2) 45 K
(3) 65°C
(4) 45°C
525
6/08-38
• An iron bar at 325 K is placed in a sample of water. The iron bar gains
energy from the water if the temperature of the water is
(1) 65 K
(3) 65°C
(2) 45 K
correct
(4) 45°C
526
6/08-40
• Given the balanced equation representing a reaction:
Cu + S -> CuS + energy
Which statement explains why the energy term is written to the right of the
arrow?
(1) The compound CuS is composed of
two metals.
(2) The compound CuS is composed of
two nonmetals.
(3) Energy is absorbed as the bonds in CuS (4) Energy is released as the bonds in CuS
form.
form.
527
6/08-40
• Given the balanced equation representing a reaction:
Cu + S -> CuS + energy
Which statement explains why the energy term is written to the right of the
arrow?
(1) The compound CuS is composed of
two metals.
(2) The compound CuS is composed of
two nonmetals.
(3) Energy is absorbed as the bonds in CuS (4) Energy is released as the bonds in CuS
correct
form.
form.
528
6/08-41
• A 1.0-liter sample of which element will uniformly fill a closed 2.0-liter
container at STP?
(1) Antimony
(2) sulfur
(3) tellurium
(4) xenon
529
6/08-41
• A 1.0-liter sample of which element will uniformly fill a closed 2.0-liter
container at STP?
(1) Antimony
(2) sulfur
(3) tellurium
(4) xenon
correct
530
6/08-42
• Given the balanced equation representing a reaction:
C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g)
What is the total number of moles of O2(g) required for the complete
combustion of 1.5 moles of C3H8(g)?
(1) 0.30 mol
(2) 1.5 mol
(3) 4.5 mol
(4) 7.5 mol
531
6/08-42
• Given the balanced equation representing a reaction:
C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g)
What is the total number of moles of O2(g) required for the complete
combustion of 1.5 moles of C3H8(g)?
(1) 0.30 mol
(2) 1.5 mol
(3) 4.5 mol
(4) 7.5 mol
correct
532
6/08-43
• A sample of gas occupies a volume of 50.0 milliliters in a cylinder with a
movable piston. The pressure of the sample is 0.90 atmosphere and the
temperature is 298 K. What is the volume of the sample at STP?
(1) 41 mL
(2) 49 mL
(3) 51 mL
(4) 55 mL
533
6/08-43
• A sample of gas occupies a volume of 50.0 milliliters in a cylinder with a
movable piston. The pressure of the sample is 0.90 atmosphere and the
temperature is 298 K. What is the volume of the sample at STP?
(1) 41 mL
(3) 51 mL
correct
(2) 49 mL
(4) 55 mL
534
6/08-44
• Which solution has the lowest freezing point?
(1) 10. g of KI dissolved in 100. g of water
(2) 20. g of KI dissolved in 200 g of water
(3) 30. g of KI dissolved in 100. g of water
(4) 40. g of KI dissolved in 200. g of water
535
6/08-44
• Which solution has the lowest freezing point?
(1) 10. g of KI dissolved in 100. g of water
(2) 20. g of KI dissolved in 200 g of water
(3) 30. g of KI dissolved in 100. g of water
(4) 40. g of KI dissolved in 200. g of water
correct
536
6/08-45
• Which 1-mole sample has the lowest entropy?
(1) Br2(s) at 266 K
(2) Br2(l) at 266 K
(3) Br2(l) at 332 K
(4) Br2(g) at 332 K
537
6/08-45
• Which 1-mole sample has the least entropy?
(1) Br2(s) at 266 K
(2) Br2(l) at 266 K
(3) Br2(l) at 332 K
(4) Br2(g) at 332 K
538
6/08-46
• At 20.°C, a 1.2-gram sample of Mg ribbon reacts rapidly with 10.0
milliliters of 1.0 M HCl(aq). Which change in conditions would have
caused the reaction to proceed more slowly?
(1) increasing the initial temperature to
25°C
(2) decreasing the concentration of
HCl(aq) to 0.1 M
(3) using 1.2 g of powdered Mg
(4) using 2.4 g of Mg ribbon
539
6/08-46
• At 20.°C, a 1.2-gram sample of Mg ribbon reacts rapidly with 10.0
milliliters of 1.0 M HCl(aq). Which change in conditions would have
caused the reaction to proceed more slowly?
(1) increasing the initial temperature to
25°C
(2) decreasing the concentration of
correct
HCl(aq) to 0.1 M
(3) using 1.2 g of powdered Mg
(4) using 2.4 g of Mg ribbon
540
6/08-47
• Which general formula represents the compound CH3CH2CCH?
(1) CnHn
(2) CnH2n
(3) CnH2n-2
(4) CnH2n+2
541
6/08-47
• Which general formula represents the compound CH3CH2CCH?
(1) CnHn
(3) CnH2n-2
(2) CnH2n
correct
(4) CnH2n+2
542
6/08-48
• Which compound dissolves in water to form an aqueous solution that can
conduct an electric current?
(1) CCl4
(2) C2H5OH
(3) CH3COOH
(4) CH4
543
6/08-48
• Which compound dissolves in water to form an aqueous solution that can
conduct an electric current?
(1) CCl4
(3) CH3COOH
(2) C2H5OH
correct
(4) CH4
544
6/08-50
• An original sample of K-40 has a mass 0f 25.00 grams. After 3.9 x 109
years, 3.125 grams of the original sample remains unchanged. What is
the half-life of K-40?
(1) 1.3 x 109 y
(2) 2.6 x 109 y
(3) 3.9 x 109 y
(4) 1.2 x 1010 y
545
6/08-50
• An original sample of K-40 has a mass 0f 25.00 grams. After 3.9 x 109
years, 3.125 grams of the original sample remains unchanged. What is
the half-life of K-40?
(1) 1.3 x 109 y
(3) 3.9 x 109 y
correct
(2) 2.6 x 109 y
(4) 1.2 x 1010 y
546
6/08-49
• Given the equation representing a reaction at equilibrium:
NH3(g) + H2O(l) = NH4+(aq) + OH-(aq)
The H+ acceptor for the forward reaction is
(1) H2O(l)
(2) NH3(g)
(3) NH4+(aq)
(4) OH-(aq)
547
6/08-49
• Given the equation representing a reaction at equilibrium:
NH3(g) + H2O(l) = NH4+(aq) + OH-(aq)
The H+ acceptor for the forward reaction is
(1) H2O(l)
(2) NH3(g)
(3) NH4+(aq)
(4) OH-(aq)
correct
548
8/08-1
• In the wave-mechanical model of the atom, orbitals are regions of the
most probable locations of
(1) protons
(2) positrons
(3) neutrons
(4) electrons
549
8/08-1
• In the wave-mechanical model of the atom, orbitals are regions of the
most probable locations of
(1) protons
(2) positrons
(3) neutrons
(4) electrons
correct
550
8/08-2
• Which phrase describes an atom?
(1) a positively charged electron cloud
surrounding a positively charged
nucleus
(2) a positively charged electron cloud
surrounding a negative charged nucleus
(3) a negative charged electron cloud
surrounding a positively charged nucleus
(4) a negatively charged electron cloud
surrounding a negatively charged nucleus
551
8/08-2
• Which phrase describes an atom?
(1) a positively charged electron cloud
surrounding a positively charged
nucleus
(2) a positively charged electron cloud
surrounding a negative charged nucleus
(3) a negative charged electron cloud
surrounding a positively charged nucleus
(4) a negatively charged electron cloud
surrounding a negatively charged nucleus
correct
552
8/08-3
• Which total mass is the smallest?
(1) the mass of two electrons
(2) the mass of two neutrons
(3) the mass of one electron plus the
mass of one proton
(4) the mass of one neutron plus the mass
of one proton
553
8/08-3
• Which total mass is the smallest?
(1) the mass of two electrons
(2) the mass of two neutrons
(3) the mass of one electron plus the
mass of one proton
(4) the mass of one neutron plus the mass
of one proton
correct
554
8/08-4
• Elements on the modern Periodic Table are arranged in order of
increasing
(1) atomic mass
(2) atomic number
(3) number of neutrons
(4) number of valence electrons
555
8/08-4
• Elements on the modern Periodic Table are arranged in order of
increasing
(1) atomic mass
(2) atomic number
(3) number of neutrons
(4) number of valence electrons
correct
556
8/08-5
• As the elements of Group 17 are considered in order of increasing atomic
number, there is an increase in
(1) atomic radius
(2) electronegativity
(3) first ionization energy
(4) number of electrons in the first shell
557
8/08-5
• As the elements of Group 17 are considered in order of increasing atomic
number, there is an increase in
(1) atomic radius
(3) first ionization energy
correct
(2) electronegativity
(4) number of electrons in the first shell
558
8/08-6
• Chlorine-37 can be represented as
(1) 35Cl17
(2) 37Cl20
(3) 20Cl35
(4) 17Cl37
559
8/08-6
• Chlorine-37 can be represented as
(1) 35Cl17
(2) 37Cl20
(3) 20Cl35
(4) 17Cl37
correct
560
8/08-7
• Which element is a metal that is in the liquid phase at STP?
(1) bromine
(2) cobalt
(3) hydrogen
(4) mercury
561
8/08-7
• Which element is a metal that is in the liquid phase at STP?
(1) bromine
(2) cobalt
(3) hydrogen
(4) mercury
correct
562
8/08-8
• Which list of formulas represents compounds, only?
(1) CO2, H2O, NH3
(2) H2, N2, O2
(3) H2, Ne, NaCl
(4) MgO, NaCl, O2
563
8/08-8
• Which list of formulas represents compounds, only?
(1) CO2, H2O, NH3
(3) H2, Ne, NaCl
correct
(2) H2, N2, O2
(4) MgO, NaCl, O2
564
8/08-9
• What is the chemical formula for iron(III) oxide?
(1) FeO
(2) Fe2O3
(3) Fe3O
(4) Fe3O2
565
8/08-9
• What is the chemical formula for iron(III) oxide?
(1) FeO
(2) Fe2O3
(3) Fe3O
(4) Fe3O2
correct
566
8/08-10
• An atom of which element has the greatest attraction for the electrons in
a bond with the hydrogen atom?
(1) chlorine
(2) phosphorous
(3) silicon
(4) sulfur
567
8/08-10
• An atom of which element has the greatest attraction for the electrons in
a bond with the hydrogen atom?
(1) chlorine
(3) silicon
correct
(2) phosphorous
(4) sulfur
568
8/08-11
• Which property could be used to identify a compound in the laboratory?
(1) mass
(2) melting point
(3) temperature
(4) volume
569
8/08-11
• Which property could be used to identify a compound in the laboratory?
(1) mass
(2) melting point
(3) temperature
(4) volume
correct
570
8/08-12
• Which statement describes what occurs as two atoms of bromine
combine to form a molecule of bromine?
(1) Energy is absorbed as a bond is
formed.
(2) Energy is absorbed as a bond is
broken.
(3) Energy is released as a bond is formed. (4) Energy is absorbed as a bond is
broken.
571
8/08-12
• Which statement describes what occurs as two atoms of bromine
combine to form a molecule of bromine?
(1) Energy is absorbed as a bond is
formed.
(2) Energy is absorbed as a bond is
broken.
(3) Energy is released as a bond is formed. (4) Energy is absorbed as a bond is
correct
broken.
572
8/08-14
• Solid ZnCl2 and liquid ZnCl2 have different
(1) empirical formulas
(2) formula masses
(3) ion ratios
(4) physical properties
573
8/08-14
• Solid ZnCl2 and liquid ZnCl2 have different
(1) empirical formulas
(2) formula masses
(3) ion ratios
(4) physical properties
correct
574
8/08-15
• Which phrase describes the molarity of a solution?
(1) liters of solute per mole of solution
(2) liters of solution per mole of solution
(3) moles of solute per liter of solution
(4) moles of solution per liter of solution
575
8/08-15
• Which phrase describes the molarity of a solution?
(1) liters of solute per mole of solution
(2) liters of solution per mole of solution
(3) moles of solute per liter of solution
(4) moles of solution per liter of solution
correct
576
8/08-16
• Which substance cannot be decomposed by a chemical change?
(1) AlCl3
(2) H2O
(3) HI
(4) Cu
577
8/08-16
• Which substance cannot be decomposed by a chemical change?
(1) AlCl3
(2) H2O
(3) HI
(4) Cu
correct
578
8/08-17
• Tetrachloromethane, CCl4, is classified as a
(1) compound because the atoms of the
elements are combined in a fixed
proportion
(2) compound because the atoms of the
elements are combined in a proportion
that varies
(3) mixture because the atoms of the
elements are combined in a fixed
proportion
(4) mixture because the atoms of the
elements are combined in a proportion
that varies
579
8/08-17
• Tetrachloromethane, CCl4, is classified as a
(1) compound because the atoms of the
elements are combined in a fixed
correct
proportion
(2) compound because the atoms of the
elements are combined in a proportion
that varies
(3) mixture because the atoms of the
elements are combined in a fixed
proportion
(4) mixture because the atoms of the
elements are combined in a proportion
that varies
580
8/08-18
• Which formulas represent two polar molecules?
(1) CO2 and HCl
(2) CO2 and CH4
(3) H2O and HCl
(4) H2O and CH4
581
8/08-18
• Which formulas represent two polar molecules?
(1) CO2 and HCl
(3) H2O and HCl
(2) CO2 and CH4
correct
(4) H2O and CH4
582
8/08-19
• Hydrocarbons are compounds that contain
(1) carbon, only
(2) carbon and hydrogen, only
(3) carbon, hydrogen, and oxygen, only
(4) carbon, hydrogen, oxygen, and
nitrogen, only
583
8/08-19
• Hydrocarbons are compounds that contain
(1) carbon, only
(2) carbon and hydrogen, only
correct
(3) carbon, hydrogen, and oxygen, only
(4) carbon, hydrogen, oxygen, and
nitrogen, only
584
8/08-20
• The reaction that joins thousands of small, identical molecules to form
one very long molecule is called
(1) esterification
(2) fermentation
(3) polymerization
(4) substitution
585
8/08-20
• The reaction that joins thousands of small, identical molecules to form
one very long molecule is called
(1) esterification
(3) polymerization
(2) fermentation
correct
(4) substitution
586
8/08-22
• A voltaic cell spontaneously converts chemical energy to
(1) electrical energy
(2) geothermal energy
(3) mechanical energy
(4) nuclear energy
587
8/08-22
• A voltaic cell spontaneously converts chemical energy to
(1) electrical energy
(3) mechanical energy
correct
(2) geothermal energy
(4) nuclear energy
588
8/08-23
• Given the balanced equation representing a reaction:
Mg(s) + Ni+2(aq) -> Mg+2(aq) + Ni(s)
What is the total number of moles of electrons lost by Mg(s) when 2.0
moles of electrons are gained by Ni+2(aq)?
(1) 1.0 mol
(2) 2.0 mol
(3) 3.0 mol
(4) 4.0 mol
589
8/08-23
• Given the balanced equation representing a reaction:
Mg(s) + Ni+2(aq) -> Mg+2(aq) + Ni(s)
What is the total number of moles of electrons lost by Mg(s) when 2.0
moles of electrons are gained by Ni+2(aq)?
(1) 1.0 mol
(2) 2.0 mol
(3) 3.0 mol
(4) 4.0 mol
correct
590
8/08-24
• Which half reaction correctly represents reduction?
(1) Mn4+-> Mn3++ e-
(2) Mn4+-> Mn7++ 3e-
(3) Mn4++ e- -> Mn3+
(4) Mn4+ + 3e- -> Mn7+
591
8/08-24
• Which half reaction correctly represents reduction?
(1) Mn4+-> Mn3++ e-
(2) Mn4+-> Mn7++ 3e-
(3) Mn4++ e- -> Mn3+
(4) Mn4+ + 3e- -> Mn7+
correct
592
8/08-25
• Which indicator is blue in a solution that has a pH of 5.6?
(1) bromcresol green
(2) bromthymol blue
(3) methyl orange
(4) thymol blue
593
8/08-25
• Which indicator is blue in a solution that has a pH of 5.6?
(1) bromcresol green
(3) methyl orange
correct
(2) bromthymol blue
(4) thymol blue
594
8/08-26
• The Arrhenius theory explains the behavior of
(1) acids and bases
(2) alcohols and amines
(3) isomers and isotopes
(4) metals and nonmetals
595
8/08-26
• The Arrhenius theory explains the behavior of
(1) acids and bases
(3) isomers and isotopes
correct
(2) alcohols and amines
(4) metals and nonmetals
596
8/08-27
• In which laboratory process could a student use 0.10 M NaOH(aq) to
determine the concentration of an aqueous solution of HBr?
(1) chromatography
(2) decomposition of the solute
(3) evaporation of the solvent
(4) titration
597
8/08-27
• In which laboratory process could a student use 0.10 M NaOH(aq) to
determine the concentration of an aqueous solution of HBr?
(1) chromatography
(2) decomposition of the solute
(3) evaporation of the solvent
(4) titration
correct
598
8/08-28
• A nuclear reaction in which two light nuclei combine to form a more
massive nucleus is called
(1) addition
(2) fission
(3) fusion
(4) substitution
599
8/08-28
• A nuclear reaction in which two light nuclei combine to form a more
massive nucleus is called
(1) addition
(3) fusion
(2) fission
correct
(4) substitution
600
8/08-29
• The nucleus of a radium-226 atom is unstable, which causes the nucleus
to spontaneously
(1) absorb electrons
(2) absorb protons
(3) decay
(4) oxidize
601
8/08-29
• The nucleus of a radium-226 atom is unstable, which causes the nucleus
to spontaneously
(1) absorb electrons
(3) decay
(2) absorb protons
correct
(4) oxidize
602
8/08-30
• A serious risk factor associated with the operation of a nuclear power
plant is the production of
(1) acid rain
(2) helium gas
(3) greenhouse gases, such as CO2
(4) radioisotopes with long half-lives
603
8/08-30
• A serious risk factor associated with the operation of a nuclear power
plant is the production of
(1) acid rain
(2) helium gas
(3) greenhouse gases, such as CO2
(4) radioisotopes with long half-lives
correct
604
8/08-31
• What is the total number of protons in an atom with the electron
configuration 2-8-28-32-18-1?
(1) 69
(2) 79
(3) 118
(4) 197
605
8/08-31
• What is the total number of protons in an atom with the electron
configuration 2-8-28-32-18-1?
(1) 69
(2) 79
(3) 118
(4) 197
correct
606
8/08-32
• Which two elements have the most similar chemical properties?
(1) Be and Mg
(2) Ca and Br
(3) Cl and Ar
(4) Na and P
607
8/08-32
• Which two elements have the most similar chemical properties?
(1) Be and Mg
(3) Cl and Ar
correct
(2) Ca and Br
(4) Na and P
608
8/08-33
• In the ground state, each atom of an element has two valence electrons.
The element has a lower first ionization energy than calcium. Where is this
element located on the Periodic Table?
(1) Group 1, Period 4
(2) Group 2, Period 5
(3) Group 2, Period 3
(4) Group 3, Period 4
609
8/08-33
• In the ground state, each atom of an element has two valence electrons.
The element has a lower first ionization energy than calcium. Where is this
element located on the Periodic Table?
(1) Group 1, Period 4
(2) Group 2, Period 5
(3) Group 2, Period 3
(4) Group 3, Period 4
correct
610
8/08-34
• Which equation shows conservation of mass and charge?
(1) 1
(2) 2
(3) 3
(4) 4
611
8/08-34
• Which equation shows conservation of mass and charge?
(1) 1
(2) 2
(3) 3
(4) 4
correct
612
8/08-35
• What is the percent composition by mass of hydrogen in NH4HCO3 (gram
formula mass = 79 grams/mole)?
(1) 5.1%
(2) 6.3%
(3) 10.%
(4) 50.%
613
8/08-35
• What is the percent composition by mass of hydrogen in NH4HCO3 (gram
formula mass = 79 grams/mole)?
(1) 5.1%
(2) 6.3%
correct
(3) 10.%
(4) 50.%
614
8/08-36
• What is the total number of valence electrons in a sulfide ion in the
ground state?
(1) 8
(2) 2
(3) 16
(4) 18
615
8/08-36
• What is the total number of valence electrons in a sulfide ion in the
ground state?
(1) 8
(2) 2
correct
(3) 16
(4) 18
616
8/08-37
• A temperature of 37°C is equivalent to a temperature of
(1) 98.6 K
(2) 236 K
(3) 310. K
(4) 371 K
617
8/08-37
• A temperature of 37°C is equivalent to a temperature of
(1) 98.6 K
(3) 310. K
(2) 236 K
correct
(4) 371 K
618
8/08-38
• Which balanced equation represents a chemical change?
(1) 1
(2) 2
(3) 3
(4) 4
619
8/08-38
• Which balanced equation represents a chemical change?
(1) 1
(2) 2
(3) 3
(4) 4
correct
620
8/08-39
• When 5 grams of KCl are dissolved in 50. grams of water at 25°C, the
resulting mixture can be described as
(1) heterogeneous and unsaturated
(2) heterogeneous and supersaturated
(3) homogeneous and unsaturated
(4) homogeneous and supersaturated
621
8/08-39
• When 5 grams of KCl are dissolved in 50. grams of water at 25°C, the
resulting mixture can be described as
(1) heterogeneous and unsaturated
(2) heterogeneous and supersaturated
(3) homogeneous and unsaturated
(4) homogeneous and supersaturated
correct
622
8/08-40
• Which aqueous solution of KI freezes at the lowest temperature?
(1) 1 mol of KI in 500. grams of water
(2) 2 mol of KI in 500. grams of water
(3) 1 mol of KI in 1000. grams of water
(4) 2 mol of KI in 1000. grams of water
623
8/08-40
• Which aqueous solution of KI freezes at the lowest temperature?
(1) 1 mol of KI in 500. grams of water
(2) 2 mol of KI in 500. grams of water
correct
(3) 1 mol of KI in 1000. grams of water
(4) 2 mol of KI in 1000. grams of water
624
8/08-41
• Which compound is a member of the same homologous series as C3H8?
(1) CH4
(2) C4H8
(3) C5H8
(4) C5H10
625
8/08-41
• Which compound is a member of the same homologous series as C3H8?
(1) CH4
(3) C5H8
correct
(2) C4H8
(4) C5H10
626
8/08-42
• Which equation represents an oxidation-reduction reaction?
(1) 1
(2) 2
(3) 3
(4) 4
627
8/08-42
• Which equation represents an oxidation-reduction reaction?
(1) 1
(3) 3
correct
(2) 2
(4) 4
628
8/08-43
• Given the balanced equation representing a reaction:
2KClO3(s) -> 2KCl(s) + 3O2(g)
The oxidation state of chlorine in this reaction changes from
(1) -1 to +1
(2) -1 to +5
(3) +1 to -1
(4) +5 to -1
629
8/08-43
• Given the balanced equation representing a reaction:
2KClO3(s) -> 2KCl(s) + 3O2(g)
The oxidation state of chlorine in this reaction changes from
(1) -1 to +1
(2) -1 to +5
(3) +1 to -1
(4) +5 to -1
correct
630
8/08-45
• Given the balanced equation representing a reaction occuring in an
electrolytic cell:
2NaCl(l) -> 2Na(l) + Cl2(g)
Where is Na(l) produced in the cell?
(1) at the anode, where oxidation occurs
(2) at the anode, where reduction occurs
(3) at the cathode, where oxidation occurs (4) at the cathode, where reduction
occurs
631
8/08-45
• Given the balanced equation representing a reaction occuring in an
electrolytic cell:
2NaCl(l) -> 2Na(l) + Cl2(g)
Where is Na(l) produced in the cell?
(1) at the anode, where oxidation occurs
(2) at the anode, where reduction occurs
(3) at the cathode, where oxidation occurs (4) at the cathode, where reduction
correct
occurs
632
8/08-46
• Given the balanced equation representing a reaction:
NH3(g) + H2O(l) -> NH4+(aq) + OH-(aq)
According to one acid-base theory, the NH3(g) molecules act as
(1) an acid because they accept H+ ions
(2) an acid because they donate H+ ions
(3) a base because they accept H+ ions
(4) a base because the donate H+ ions
633
8/08-46
• Given the balanced equation representing a reaction:
NH3(g) + H2O(l) -> NH4+(aq) + OH-(aq)
According to one acid-base theory, the NH3(g) molecules act as
(1) an acid because they accept H+ ions
(2) an acid because they donate H+ ions
(3) a base because they accept H+ ions
(4) a base because the donate H+ ions
correct
634
8/08-47
• What volume of 0.120 M HNO3(aq) is needed to completely neutralize
150.0 milliliters of 0.100 M NaOH(aq)?
(1) 62.5 mL
(2) 125 mL
(3) 180.mL
(4) 360. mL
635
8/08-47
• What volume of 0.120 M HNO3(aq) is needed to completely neutralize
150.0 milliliters of 0.100 M NaOH(aq)?
(1) 62.5 mL
(2) 125 mL
(3) 180.mL
(4) 360. mL
correct
636
8/08-49
• An original sample of a radioisotope fluorine-21 had a mass of 80.0
milligrams. Only 20.0 milligrams of this original sample remain unchanged
after 8.32 seconds. What is the half-life of fluorine-21
(1) 1.04 s
(2) 2.08 s
(3) 4.16 s
(4) 8.32 s
637
8/08-49
• An original sample of a radioisotope fluorine-21 had a mass of 80.0
milligrams. Only 20.0 milligrams of this original sample remain unchanged
after 8.32 seconds. What is the half-life of fluorine-21
(1) 1.04 s
(2) 2.08 s
(3) 4.16 s
(4) 8.32 s
638
8/08-48
• Given the balanced equation representing a reaction:
Which particle is represented by X?
(1) electron
(2) proton
(3) alpha particle
(4) neutron
639
8/08-48
• Given the balanced equation representing a reaction:
Which particle is represented by X?
(1) electron
(2) proton
(3) alpha particle
(4) neutron
correct
640
8/08-50
• Which nuclide is paired with a specific use of that nuclide?
(1) carbon-14, treatment of cancer
(2) cobalt-60, dating of rock formations
(3) iodine-131, treatment of thyroid
disorders
(4) uranium-238, dating of once-living
organisms
641
8/08-50
• Which nuclide is paired with a specific use of that nuclide?
(1) carbon-14, treatment of cancer
(2) cobalt-60, dating of rock formations
(3) iodine-131, treatment of thyroid
correct
disorders
(4) uranium-238, dating of once-living
organisms
642