chemistry with masteringchemistry®, 6/e john e mcmurry, robert c. fay, solutions manual and test bank
test bank for Chemistry, 6e (McMurry/Fay)
Chapter 2
Atoms, Molecules, and Ions
2.1 Multiple-Choice Questions
1) According to
history, the concept that all matter is composed of atoms was first proposed by
A) the Greek
philosopher Democritus, but not widely accepted until modern times.
B) Dalton, but
not widely accepted until the work of Mendeleev.
C) Dalton, but
not widely accepted until the work of Einstein.
D) Dalton, and
widely accepted within a few decades.
Answer: A
Topic: Section 2.1 The Conservation of Mass and the
Law of Definite Proportions
2) The observation that 15.0 g of hydrogen
reacts with 120.0 g of oxygen to form 135.0 g of water is evidence for the law
of
A)
definite proportions.
B)
energy conservation.
C)
mass conservation.
D)
multiple proportions.
Answer: C
Topic: Section 2.1 The Conservation of Mass and the
Law of Definite Proportions
3)
The observation that 4.0 g of hydrogen reacts with 32.0 g of oxygen to form a
product with
O:H
mass ratio = 8:1, and 6.0 g of hydrogen reacts with 48.0 g of oxygen to form
the same product
with
O/H mass ratio = 8:1 is evidence for the law of
A)
definite proportions.
B)
energy conservation.
C)
mass conservation.
D)
multiple proportions.
Answer: A
Topic: Section 2.1 The Conservation of Mass and the
Law of Definite Proportions
4) Methane and
oxygen react to form carbon dioxide and water. What mass of water is formed if
3.2 g of methane reacts with 12.8 g of oxygen to produce 8.8 g of carbon
dioxide?
A) 7.2 g
B) 8.8 g
C) 14.8 g
D) 16.0 g
Answer: A
Topic: Section 2.1 The Conservation of Mass and the
Law of Definite Proportions
5) Sodium metal
and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium
react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide,
what mass of water was consumed in the reaction?
A) 4.68 g
B) 5.98 g
C) 10.14 g
D) 10.66 g
Answer: A
Topic: Section 2.1 The Conservation of Mass and the
Law of Definite Proportions
6) A sample of
pure lithium carbonate contains 18.8% lithium by mass. What is the % lithium by
mass in a sample of pure lithium carbonate that has twice the mass of the first
sample?
A) 9.40%
B) 18.8%
C) 37.6%
D) 75.2%
Answer: B
Topic: Section 2.1 The Conservation of Mass and the
Law of Definite Proportions
7) A sample of
pure calcium fluoride with a mass of 15.0 g contains 7.70 g of calcium. How
much calcium is contained in 45.0 g of calcium fluoride?
A) 2.56 g
B) 7.70 g
C) 15.0 g
D) 23.1 g
Answer: D
Topic: Section 2.1 The Conservation of Mass and the
Law of Definite Proportions
8)
The observation that hydrogen and oxygen can react to form two compounds with
different chemical and physical properties, one having an O:H mass ratio = 8:1
and the other having an O:H mass ratio = 16:1 is consistent with the law of
A)
definite proportions.
B)
energy conservation.
C)
mass conservation.
D)
multiple proportions.
Answer: D
Topic: Section 2.2 The Law of Multiple Proportions
and Dalton's Atomic Theory
9) Which of the
following statements is not a postulate of Dalton's atomic theory?
A) Each element
is characterized by the mass of its atoms.
B) Atoms are
composed of protons, neutrons, and electrons.
C) Chemical
reactions only rearrange atomic combinations.
D) Elements are
composed of atoms.
Answer: B
Topic: Section 2.2 The Law of Multiple Proportions
and Dalton's Atomic Theory
10) Which of the
following is a part of Dalton's atomic theory?
A) Atoms are
rearranged but not changed during a chemical reaction.
B) Atoms break
down during radioactive decay.
C) Atoms contain
protons, neutrons, and electrons.
D) Isotopes of
the same element have different masses.
Answer: A
Topic: Section 2.2 The Law of Multiple Proportions
and Dalton's Atomic Theory
11) Which of the
following is not explained by Dalton's atomic theory?
A) conservation
of mass during a chemical reaction
B) the existence
of more than one isotope of an element
C) the law of
definite proportions
D) the law of
multiple proportions
Answer: B
Topic: Section 2.2 The Law of Multiple Proportions
and Dalton's Atomic Theory
12) Elements A
and Q form two compounds, AQ and A2Q3. The mass ratio (mass Q)/(mass A) for AQ is
0.574. What is the mass ratio (mass Q)/(mass A) for A2Q3?
A) 0.383
B) 0.861
C) 1.16
D) 2.61
Answer: B
Topic: Section 2.2 The Law of Multiple Proportions
and Dalton's Atomic Theory
13) Elements A
and Q form two compounds, AQ and A2Q. Which of the following must be true?
A) (mass
Q)/(mass A) is one for AQ, and 1/2 for A2Q.
B) (mass
Q)/(mass A) for AQ must equal (mass Q)/(mass A) for A2Q.
C) (mass
Q)/(mass A) for AQ must be 2 times (mass Q)/(mass A) for A2Q.
D) (mass
Q)/(mass A) for AQ must be 1/2 (mass Q)/(mass A) for A2Q.
Answer: C
Topic: Section 2.2 The Law of Multiple Proportions
and Dalton's Atomic Theory
14) Elements A
and Q form two compounds. The ratio (mass Q)/(mass A) for compound one is 0.271
and ratio (mass Q)/(mass A) for compound two is 0.362. If compound one has the
chemical formula AQ, what is the chemical formula for compound two?
A) A3Q4
B) A2Q3
C) AQ2
D) AQ3
Answer: A
Topic: Section 2.2 The Law of Multiple Proportions
and Dalton's Atomic Theory
15)
The existence of electrons in atoms of all elements was demonstrated by
A)
Millikan's oil drop experiment.
B)
Rutherford's gold foil experiment.
C)
Thomson's cathode ray tube experiment.
D)
None of these
Answer: C
Topic: Section 2.3 Atomic Structure: Electrons
16)
The charge-to-mass ratio of an electron was established by
A)
Millikan's oil drop experiment.
B)
Rutherford's gold foil experiment.
C)
Thomson's cathode ray tube experiment.
D)
None of these
Answer: C
Topic: Section 2.3 Atomic Structure: Electrons
17)
The current model of the atom in which essentially all of an atom's mass is
contained in a very small nucleus, whereas most of an atom's volume is due to
the space in which the atom's electrons move was established by
A)
Millikan's oil drop experiment.
B)
Rutherford's gold foil experiment.
C)
Thomson's cathode ray tube experiment.
D)
None of these
Answer: B
Topic: Section 2.4 Atomic Structure: Protons and
Neutrons
18)
The existence of neutrons in the nucleus of an atom was demonstrated by
A)
Millikan's oil drop experiment.
B)
Rutherford's gold foil experiment.
C)
Thomson's cathode ray tube experiment.
D)
None of these
Answer: D
Topic: Section 2.4 Atomic Structure: Protons and
Neutrons
19) Most of the
alpha particles directed at a thin gold foil in Rutherford's experiment
A) bounced
directly back from the foil.
B) passed
directly through the foil undeflected.
C) passed
through the foil but were deflected at an angle.
D) were absorbed
by the foil.
Answer: B
Topic: Section 2.4 Atomic Structure: Protons and
Neutrons
20) Which
subatomic particle has the smallest mass?
A) a proton
B) a neutron
C) an electron
D) an alpha
particle
Answer: C
Topic: Section 2.4 Atomic Structure: Protons and
Neutrons
21)
A proton is approximately
A)
200 times larger than an electron.
B)
2000 times larger than an electron.
C)
200 times smaller than an electron.
D)
2000 times smaller than an electron.
Answer: B
Topic: Section 2.4 Atomic Structure: Protons and
Neutrons
22)
The symbol that is usually used to represent atomic number is ________.
A)
A
B)
N
C)
X
D)
Z
Answer: D
Topic: Section 2.5 Atomic Numbers
23)
The mass number of an atom is equal to the number of
A)
electrons.
B)
neutrons.
C)
protons.
D)
protons plus neutrons.
Answer: D
Topic: Section 2.5 Atomic Numbers
24) Which of the
following two atoms are isotopes?
A)
and
B)
and
C)
and
D)
and
Answer: B
Topic: Section 2.5 Atomic Numbers
25) Which are
isotopes? An atom that has an atomic number of 34 and a mass number of 76 is an
isotope of an atom that has
A) an atomic
number of 32 and a mass number of 76.
B) an atomic
number of 34 and a mass number of 80.
C) 42 neutrons
and 34 protons.
D) 42 protons
and 34 neutrons.
Answer: B
Topic: Section 2.5 Atomic Numbers
26)
Which of the following represent isotopes?
A:
[ ] B:
[ ] C:
[ ] D:
[ ]
A) A and B
B) A and C
C) A and D
D) C and D
Answer: B
Topic: Section 2.5 Atomic Numbers
27) The isotope
represented by
is named
A)
carbon-6
B)
carbon-7
C)
carbon-13
D)
carbon-19
Answer: C
Topic: Section 2.5 Atomic Numbers
28) Boron-9 can
be represented as
A)
.
B)
.
C)
.
D)
.
Answer: B
Topic: Section 2.5 Atomic Numbers
29)
How many protons (p) and neutrons (n) are in an atom of
?
A)
38 p, 52 n
B)
38 p, 90 n
C)
52 p, 38 n
D)
90 p, 38 n
Answer: A
Topic: Section 2.5 Atomic Numbers
30) How many
protons (p) and neutrons (n) are in an atom of calcium-46?
A) 20 p, 26 n
B) 20 p, 46 n
C) 26 p, 20 n
D) 46 p, 60 n
Answer: A
Topic: Section 2.5 Atomic Numbers
31) What is the
chemical symbol for an atom that has 29 protons and 36 neutrons?
A) Cu
B) Kr
C) N
D) Tb
Answer: A
Topic: Section 2.5 Atomic Numbers
32) How many
electrons are in a neutral atom of iodine-131?
A) 1
B) 53
C) 54
D) 131
Answer: B
Topic: Section 2.5 Atomic Numbers
33) How many
protons (p), neutrons (n), and electrons (e) are in one atom of
?
A) 12 p, 12 n,
12 e
B) 12 p, 11 n,
12 e
C) 12 p, 11 n,
10 e
D) 12 p, 11 n,
14 e
Answer: B
Topic: Section 2.5 Atomic Numbers
34) Identify the chemical symbol
of element Q in
.
A) Br
B) Hg
C) Pd
D) Se
Answer: D
Topic: Section 2.5 Atomic Numbers
35) The atoms of
a particular element all have the same number of protons as neutrons. Which of
the following must be true?
A) The atomic
weight must be a whole number.
B) The mass
number for each atom must equal the atomic weight of the element.
C) The mass
number must be exactly twice the atomic number for each atom.
D) All of these
are true.
Answer: C
Topic: Section 2.5 Atomic Numbers
36) The smallest
sample of carbon atoms that can be observed with the naked eye has a mass of
approximately 2 × 10-8 g. Given that 1 g = 6.02
× 1023 amu, and that carbon has an atomic weight of
12.01 amu, determine the number of carbon atoms present in the sample.
A) 1 × 1015
B) 1 × 1016
C) 1 × 1017
D) 6 × 1023
Answer: A
Topic: Section 2.6 Atomic Masses and the Mole
37) An element
has two naturally occurring isotopes. One has an abundance of 37.4% and an
isotopic mass of 184.953 amu, and the other has an abundance of 62.6% and a
mass of 186.956 amu. What is the atomic weight of the element?
A) 185.702 amu
B) 185.954 amu
C) 186.207 amu
D) 186.956 amu
Answer: C
Topic: Section 2.6 Atomic Masses and the Mole
38) The element
antimony has an atomic weight of 121.757 amu and only two naturally-occurring
isotopes. One isotope has an abundance of 57.3% and an isotopic mass of 120.904
amu. Based on these data, what is the mass of the other isotope?
A) 121.757 amu
B) 122.393 amu
C) 122.610 amu
D) 122.902 amu
Answer: D
Topic: Section 2.6 Atomic Masses and the Mole
39) What is the
standard isotope that is used to define the number of atoms in a mole?
A) 1H
B) 12C
C) 16O
D) 20Ne
Answer: B
Topic: Section 2.6 Atomic Masses and the Mole
40)
The number of atoms of carbon in 12 g of carbon is closest to .
A)
12
B)
1022
C)
1023
D)
1024
Answer: D
Topic: Section 2.6 Atomic Masses and the Mole
41)
What is the mass of one atom of the element hydrogen?
A)
2.0 g
B)
1.0 g
C) 3.4 × 10-24 g
D) 1.7 × 10-24 g
Answer: D
Topic: Section 2.6 Atomic Masses and the Mole
42)
One mole of which element has the smallest mass?
A)
Co
B)
Cu
C)
Ni
D)
Zn
Answer: C
Topic: Section 2.6 Atomic Masses and the Mole
43)
24.0 g of which element contains the greatest number of atoms?
A)
B
B)
C
C)
N
D)
O
Answer: A
Topic: Section 2.6 Atomic Masses and the Mole
44)
How many moles and how many atoms of zinc are in a sample weighing 34.9 g?
A)
0.533 mol, 8.85 ×10-25 atoms
B)
0.533 mol, 3.21 ×1023 atoms
C)
1.87 mol, 3.10 × 10-24 atoms
D)
1.87 mol, 1.13 × 1024 atoms
Answer: B
Topic: Section 2.6 Atomic Masses and the Mole
45) Which
statement about nuclear reactions is true?
A) New elements
are never produced in a nuclear reaction.
B) Nuclear
reactions involve valence electrons.
C) The rate of a
nuclear reaction is affected by catalysts.
D) Tremendous
amounts of energy are involved in nuclear reactions.
Answer: D
Topic: Section 2.7 Nuclear Chemistry: The Change of
One Element Into Another
46) The term
"nucleons" refers to the number of ________ in the atom.
A) neutrons
B) protons
C) protons and
neutrons
D) protons,
neutrons, and electrons
Answer: C
Topic: Section 2.7 Nuclear Chemistry: The Change of
One Element Into Another
47) The number
of nucleons in an atom or ion is the same as the
A) atomic
number.
B) charge on the
atom or ion.
C) mass number.
D) none of these
Answer: C
Topic: Section 2.7 Nuclear Chemistry: The Change of
One Element Into Another
48) The number
of nucleons in a
nucleus is
A) 92.
B) 144.
C) 236.
D) 328.
Answer: C
Topic: Section 2.7 Nuclear Chemistry: The Change of
One Element Into Another
49) The number
of neutrons in
is
A) 26.
B) 29.
C) 53.
D) 55.
Answer: B
Topic: Section 2.7 Nuclear Chemistry: The Change of
One Element Into Another
50)
"Isotopes" are atoms with the same number of ________ but different
number of ________.
A) electrons,
protons
B) neutrons,
protons
C) protons,
electrons
D) protons,
neutrons
Answer: D
Topic: Section 2.7 Nuclear Chemistry: The Change of
One Element Into Another
51) The rate of
a nuclear reaction can be changed by
A) adding a
catalyst.
B) decreasing
the pressure.
C) increasing
the temperature.
D) None of these
Answer: D
Topic: Section 2.7 Nuclear Chemistry: The Change of
One Element Into Another
52) Which of the
following statements is not correct when balancing a nuclear equation?
I. The
mass numbers must be conserved on both sides of the reaction arrow.
II. The
ionic charges must be conserved on both sides of the reaction arrow.
III. The
atomic numbers must be conserved on both sides of the reaction arrow.
IV. The
elements must be the same on both sides of the reaction arrow.
A) II only
B) II and III
C) I and III
D) II and IV
Answer: D
Topic: Section 2.8 Radioactivity
53) An alpha
particle is
A)
.
B)
.
C)
.
D)
.
Answer: D
Topic: Section 2.8 Radioactivity
54) When a
substance decays by alpha radiation, the mass number of the nucleus ________
and the atomic number ________.
A) increases by
4, increases by 2
B) reduces by 4,
reduces by 2
C) increases by
2, increases by 4
D) reduces by 2,
reduces by 4
Answer: B
Topic: Section 2.8 Radioactivity
55)
The nuclear decay process that involves the particle having the greatest mass
is ________ emission.
A)
alpha
B)
beta
C)
gamma
D)
positron
Answer: A
Topic: Section 2.8 Radioactivity
56) A beta
particle is
A)
.
B)
.
C)
.
D)
.
Answer: A
Topic: Section 2.8 Radioactivity
57) When a
substance decays by beta emission, the mass number of the nucleus ________ and
the atomic number ________.
A) decreases by
1, remains the same
B) increases by
1, remains the same
C) remains the
same, decreases by 1
D) remains the
same, increases by 1
Answer: D
Topic: Section 2.8 Radioactivity
58) Beta decay
of 24Na
produces a beta particle and
A) 20F.
B) 23Na.
C) 24Ne.
D) 24Mg.
Answer: D
Topic: Section 2.8 Radioactivity
59) Which of the
following statements about gamma radiation is false?
A) It almost
always accompanies alpha or beta emission.
B) It is a
mechanism to release excess energy in the nucleus.
C) Gamma rays
are high energy photons.
D) The mass
number decreases by one with each gamma emitted.
Answer: D
Topic: Section 2.8 Radioactivity
60) Gamma
radiation can be described as
A) a helium
nucleus.
B) a negatively
charged free electron.
C) high energy
electromagnetic radiation.
D) a positively
charged free electron.
Answer: C
Topic: Section 2.8 Radioactivity
61) A positron
is
A)
.
B)
.
C)
.
D)
.
Answer: C
Topic: Section 2.8 Radioactivity
62) Positron
emission changes the atomic number of an element by
A) -2.
B) -1.
C) +1.
D) +2.
Answer: B
Topic: Section 2.8 Radioactivity
63) Which of the
following statements about positrons is false?
A) The positron
has same mass as an electron.
B) A positron is
ejected from the nucleus during the conversion of a proton into a neutron.
C) A positron is
a positive electron.
D) When positron
emission occurs, the atomic number of the nucleus increases.
Answer: D
Topic: Section 2.8 Radioactivity
64)
The nuclear transformation potassium-40 argon-40 + ? is classified as
A)
alpha emission.
B)
beta emission.
C)
electron capture.
D)
positron emission.
Answer: D
Topic: Section 2.8 Radioactivity
65) Which of the
following statements about electron capture is false?
A) The electron
is used to convert a proton to a neutron.
B) The electron
involved is most likely an outer shell valence electron.
C) In electron
capture decay, the atomic number decreases by one.
D) In electron
capture decay, the mass number remains unchanged.
Answer: B
Topic: Section 2.8 Radioactivity
66) Which one of
the following processes does not result in transmutation to another
element?
A) alpha
emission
B) beta emission
C) electron
capture
D) gamma
emission
Answer: D
Topic: Section 2.8 Radioactivity
67) Which of the
following decay processes give a product nuclide whose atomic number is one
less than the starting nuclide?
A) alpha decay
B) beta decay
and positron decay
C) gamma decay
and beta decay
D) positron
decay and electron capture
Answer: D
Topic: Section 2.8 Radioactivity
68) Which
reaction below represents
decay by positron
emission?
A)
→
+
B)
→
+
C)
→
+
D)
→
+
Answer: B
Topic: Section 2.8 Radioactivity
69) Which reaction below represents
decay by alpha
emission?
A)
→
+
B)
→
+
C)
→
p +
D)
→
n +
Answer: A
Topic: Section 2.8 Radioactivity
Experiment 8
Reactions in Aqueous Solutions: Strong Acids and Bases
Instructor Notes and Lab Preparation:
Chemicals and Equipment:
0.5 M HCl 1 liter, dyed red
0.5 M NaOH 1 liter, dyed blue
1 mL graduated pipette (plastic)
3-way rubber bulb
25 mL volumetric flasks
50 mL beaker as needed
hot plates
pH meter
power supply
calibration instructions
buffer solutions
Setup:
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