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Introductory Chemistry: Concepts and Critical Thinking
Chapter 4 Models of the Atom
Key Terms
1) What is the term for the weighted average mass of all the naturally occurring isotopes of an element?
A) atomic notation
B) atomic number
C) atomic mass
D) mass number
E) none of the above
Answer: C
Section: Key Terms
2) What is the term for a unit of mass exactly equal to 1/12 the mass of a carbon-12 atom?
A) atomic mass unit
B) hydrogen atom
C) neutron
D) proton
E) none of the above
Answer: A
Section: Key Terms
3) What is the term for a symbolic method of expressing the composition of an atomic nucleus?
A) atomic notation
B) atomic number
C) atomic mass
D) mass number
E) none of the above
Answer: A
Section: Key Terms
4) What is the term for the region of very high density in the center of the atom?
A) atomic center
B) atomic core
C) atomic kernel
D) atomic nucleus
E) none of the above
Answer: D
Section: Key Terms
5) What is the term for the value which indicates the number of protons for an atom of a given element?
A) atomic notation
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B) atomic number
C) atomic mass
D) mass number
E) none of the above
Answer: B
Section: Key Terms
6) What is the term for the atomic model that describes electrons circling the nucleus in an orbit of
specific energy?
A) Bohr atom
B) Rutherford atom
C) Thomson atom
D) quantum mechanical atom
E) none of the above
Answer: A
Section: Key Terms
7) What is the term for a broad uninterrupted band of radiant energy?
A) continuous spectrum
B) radiant energy spectrum
C) ultraviolet spectrum
D) visible spectrum
E) none of the above
Answer: A
Section: Key Terms
8) What is the negatively charged subatomic particle having a negligible mass?
A) electron
B) neutron
C) proton
D) quark
E) none of the above
Answer: A
Section: Key Terms
9) What is the term for the shorthand description of the arrangement of electrons by sublevels according
to increasing energy?
A) atomic notation
B) atomic number
C) continuous spectrum
D) electron configuration
E) none of the above
Answer: D
Section: Key Terms
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10) What is the term for the collection of narrow bands of light that results from excited atoms of a
given element releasing energy?
A) continuous spectrum
B) electromagnetic spectrum
C) emission line spectrum
D) radiant energy spectrum
E) none of the above
Answer: C
Section: Key Terms
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11) What is the term for an orbit that electrons occupy at a fixed distance from the nucleus; designated
1, 2, 3, 4 ...?
A) energy level
B) orbital
C) shell
D) subshell
E) none of the above
Answer: A
Section: Key Terms
12) What is the term for an electron energy level that results from splitting a main energy level?
A) energy sublevel
B) orbital
C) shell
D) subshell
E) none of the above
Answer: A
Section: Key Terms
13) What is the term for the number of times a light wave travels a complete cycle in one second?
A) energy
B) frequency
C) velocity
D) wavelength
E) none of the above
Answer: B
Section: Key Terms
14) What is the term for two atoms of the same element that differ by the number of neutrons in the
nucleus?
A) atomic mass units
B) isotopes
C) nucleons
D) photons
E) none of the above
Answer: B
Section: Key Terms
15) What is the general term that refers to either visible or invisible radiant energy?
A) continuous spectrum
B) emission spectrum
C) line spectrum
D) light
E) none of the above
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Answer: D
Section: Key Terms
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16) What is the term for the value which indicates the total number of protons and neutrons in an atom
of a given element?
A) atomic notation
B) atomic number
C) atomic mass
D) mass number
E) none of the above
Answer: D
Section: Key Terms
17) What is the neutral subatomic particle having an approximate mass of 1 amu?
A) electron
B) neutron
C) proton
D) quark
E) none of the above
Answer: B
Section: Key Terms
18) What is the term for the spatial region about the nucleus of an atom where there is a high probability
of finding an electron with a given energy?
A) electron shell
B) electron subshell
C) orbital
D) quantum level
E) none of the above
Answer: C
Section: Key Terms
19) What is the term for a particle of radiant energy?
A) electron
B) neutron
C) photon
D) proton
E) none of the above
Answer: C
Section: Key Terms
20) What is the positively charged subatomic particle having an approximate mass of 1 amu?
A) electron
B) neutron
C) proton
D) quark
E) none of the above
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Answer: C
Section: Key Terms
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21) What is the term for the atomic model that describes the energy of an electron in terms of its
probable location about the nucleus?
A) Bohr atom
B) nuclear atom
C) planetary atom
D) quantum mechanical atom
E) none of the above
Answer: D
Section: Key Terms
22) What is the term for the range of light energy extending from short wavelength gamma rays to long
wavelength microwaves?
A) gamma ray spectrum
B) microwave spectrum
C) radiant energy spectrum
D) visible spectrum
E) none of the above
Answer: C
Section: Key Terms
23) What is the term for the statement that it is impossible to precisely measure both the location and
energy of a particle at the same time?
A) exclusion principle
B) quantum principle
C) spectrum rule
D) uncertainty principle
E) none of the above
Answer: D
Section: Key Terms
24) What is the term for light energy that appears violet to red?
A) infrared spectrum
B) radiant energy spectrum
C) ultraviolet spectrum
D) visible spectrum
E) none of the above
Answer: D
Section: Key Terms
25) What is the term for the distance a light wave travels to complete one cycle?
A) energy
B) frequency
C) velocity
D) wavelength
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E) none of the above
Answer: D
Section: Key Terms
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Questions for Chapter 4
1) Which of the following of Dalton's proposals is still valid?
A) An element is composed of tiny particles called atoms.
B) Atoms of different elements combine to form compounds.
C) Compounds contain atoms in small whole number ratios.
D) all of the above
E) none of the above
Answer: D
Section: 4.1 Dalton Model of the Atom
2) Which of the following of Dalton's proposals is still valid?
A) Atoms of different elements combine to form compounds.
B) Atoms can combine in small whole number ratios.
C) Atoms can combine in more than one whole number ratio.
D) all of the above
E) none of the above
Answer: D
Section: 4.1 Dalton Model of the Atom
3) Which of the following of Dalton's proposals is still valid?
A) Atoms are indivisible.
B) Atoms are indestructible.
C) All atoms of an element are identical.
D) all of the above
E) none of the above
Answer: E
Section: 4.1 Dalton Model of the Atom
4) According to the Thomson model of the atom, what is the simplest negative particle in an atom?
A) alpha
B) electron
C) neutron
D) proton
E) none of the above
Answer: B
Section: 4.2 Thomson Model of the Atom
5) According to the Thomson model, what is the simplest positive particle in an atom?
A) alpha
B) electron
C) neutron
D) proton
E) none of the above
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Answer: D
Section: 4.2 Thomson Model of the Atom
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6) According to the Thomson model, what is the relative charge on an electron?
A) -1
B) +1
C) -2
D) +2
E) none of the above
Answer: A
Section: 4.2 Thomson Model of the Atom
7) According to the Thomson model, what is the relative charge on a proton?
A) -1
B) +1
C) -2
D) +2
E) none of the above
Answer: B
Section: 4.2 Thomson Model of the Atom
8) What do the raisins represent in the raisin pudding model of the atom?
A) electrons
B) neutrons
C) protons
D) nuclei
E) none of the above
Answer: A
Section: 4.2 Thomson Model of the Atom
9) What does the pudding represent in the plum pudding model of the atom?
A) homogeneous negative charge
B) homogeneous positive charge
C) heterogeneous negative charge
D) heterogeneous positive charge
E) none of the above
Answer: B
Section: 4.2 Thomson Model of the Atom
10) Which of the following subatomic particles is found outside the nucleus?
A) electron
B) neutron
C) proton
D) all of the above
E) none of the above
Answer: A
Section: 4.3 Rutherford Model of the Atom
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11) Which of the following subatomic particles are found inside the nucleus?
A) electron and neutron
B) neutron and proton
C) proton and electron
D) all of the above
E) none of the above
Answer: B
Section: 4.3 Rutherford Model of the Atom
12) Which of the following subatomic particles are found outside the nucleus?
A) electron and neutron
B) neutron and proton
C) proton and electron
D) all of the above
E) none of the above
Answer: E
Section: 4.3 Rutherford Model of the Atom
13) Which subatomic particle has a relative charge of -1 and a mass of ~0 amu?
A) alpha
B) electron
C) neutron
D) proton
E) none of the above
Answer: B
Section: 4.3 Rutherford Model of the Atom
14) Which subatomic particle has a relative charge of +1 and a mass of ~1 amu?
A) alpha
B) electron
C) neutron
D) proton
E) none of the above
Answer: D
Section: 4.3 Rutherford Model of the Atom
15) Which subatomic particle has a relative charge of 0 and a mass of ~1 amu?
A) alpha
B) electron
C) neutron
D) proton
E) none of the above
Answer: C
Section: 4.3 Rutherford Model of the Atom
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16) Using atomic notation, indicate the isotope having 11 p+, 12 n0, and 11 e-.
A)
Na
B)
Na
C)
Na
D)
Mg
E)
Mg
Answer: B
Section: 4.4 Atomic Notation
17) Using atomic notation, indicate the isotope having 26 p+, 32 n0, and 26 e-.
A)
Fe
B)
Fe
C)
Fe
D)
S
E)
S
Answer: B
Section: 4.4 Atomic Notation
18) Using atomic notation, indicate the isotope having 30 p+, 35 n0, and 30 e-.
A)
Zn
B)
Zn
C)
Zn
D)
Br
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E)
Br
Answer: B
Section: 4.4 Atomic Notation
19) How many neutrons are in the nucleus of an atom of
O?
A) 8
B) 10
C) 18
D) 26
E) none of the above
Answer: B
Section: 4.4 Atomic Notation
20) How many neutrons are in the nucleus of an atom of
Co?
A) 27
B) 33
C) 60
D) 87
E) none of the above
Answer: B
Section: 4.4 Atomic Notation
21) How many neutrons are in the nucleus of an atom of
Sn?
A) 50
B) 68
C) 118
D) 168
E) none of the above
Answer: B
Section: 4.4 Atomic Notation
22) How many neutrons are in the nucleus of an atom of iron-56?
A) 26
B) 30
C) 56
D) 82
E) none of the above
Answer: B
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Section:
4.4 Atomic Notation
23) How many neutrons are in the nucleus of an atom of copper-65?
A) 29
B) 36
C) 65
D) 94
E) none of the above
Answer: B
Section: 4.4 Atomic Notation
24) How many neutrons are in the nucleus of an atom of silver-107?
A) 47
B) 60
C) 107
D) 154
E) none of the above
Answer: B
Section: 4.4 Atomic Notation
25) How many neutrons are in the nucleus of an atom of 195Pt?
A) 78
B) 117
C) 195
D) 273
E) none of the above
Answer: B
Section: 4.4 Atomic Notation
26) How many neutrons are in the nucleus of an atom of 200Hg?
A) 80
B) 120
C) 200
D) 280
E) none of the above
Answer: B
Section: 4.4 Atomic Notation
27) What is the current reference isotope for the atomic mass scale?
A) hydrogen-1
B) helium-4
C) carbon-12
D) oxygen-16
E) none of the above
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Answer: C
Section: 4.5 Atomic Mass
28) What is the assigned mass of the reference isotope for the atomic mass scale?
A) 1.01 amu
B) 4.00 amu
C) 12.01 amu
D) 16.00 amu
E) 12 amu exactly
Answer: E
Section: 4.5 Atomic Mass
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29) Why are atomic masses expressed on a relative atomic mass scale?
A) Atoms are electrically positive.
B) Atoms are electrically neutral.
C) Atoms are too reactive to weigh directly.
D) Atoms are too small to weigh directly.
E) none of the above
Answer: D
Section: 4.5 Atomic Mass
30) Given that the only naturally occurring isotope of sodium is 23Na, what is its isotopic mass? (Hint:
Refer to the Periodic Table.)
A) 11.00 amu
B) 11.99 amu
C) 12.00 amu
D) 22.99 amu
E) 34.99 amu
Answer: D
Section: 4.5 Atomic Mass
31) Given that the only naturally occurring isotope of aluminum is 27Al, what is its isotopic mass?
(Hint: Refer to the Periodic Table.)
A) 13.00 amu
B) 13.98 amu
C) 14.00 amu
D) 26.98 amu
E) 39.98 amu
Answer: D
Section: 4.5 Atomic Mass
32) Given that the only naturally occurring isotope of gold is 197Au, what is its isotopic mass? (Hint:
Refer to the Periodic Table.)
A) 79.00 amu
B) 117.97 amu
C) 118.00 amu
D) 196.97 amu
E) 275.97 amu
Answer: D
Section: 4.5 Atomic Mass
33) Element X has two natural isotopes: X-6 (6.015 amu) and X-7 (7.016 amu). Calculate the atomic
mass of element X given the abundance of X-7 is 92.5%.
A) 6.09 amu
B) 6.50 amu
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C) 6.52 amu
D) 6.94 amu
E) 12.5 amu
Answer: D
Section: 4.5 Atomic Mass
34) Element Y has two natural isotopes: Y-63 (62.940 amu) and Y-65 (64.928 amu). Calculate the
atomic mass of element Y given the abundance of Y-63 is 69.17%.
A) 63.55 amu
B) 64.00 amu
C) 64.32 amu
D) 107.85 amu
E) 108.46 amu
Answer: A
Section: 4.5 Atomic Mass
35) Element Z has two natural isotopes: Z-79 (78.918 amu) and Z-81 (80.916 amu). Calculate the
atomic mass of element Z given the abundance of Z-81 is 49.31%.
A) 79.00 amu
B) 79.90 amu
C) 80.00 amu
D) 119.93 amu
E) 120.92 amu
Answer: B
Section: 4.5 Atomic Mass
36) Lithium occurs naturally as 6Li and 7Li . Which isotope is more abundant? (Hint: Refer to the
Periodic Table.)
A) lithium-3
B) lithium-4
C) lithium-6
D) lithium-7
E) none of the above
Answer: D
Section: 4.5 Atomic Mass
37) Boron occurs naturally as 10B and 11B. Which isotope is more abundant?
(Hint: Refer to the Periodic Table.)
A) boron-5
B) boron-6
C) boron-10
D) boron-11
E) none of the above
Answer: D
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Section:
4.5 Atomic Mass
38) Copper occurs naturally as
Periodic Table.)
A) copper-34
B) copper-36
C) copper-63
D) copper-65
E) none of the above
Answer: C
Section: 4.5 Atomic Mass
63Cu and 65Cu. Which isotope is more abundant? (Hint: Refer to the
39) Which of the following colors of light has the longest wavelength?
A) violet
B) blue
C) orange
D) red
E) All colors have the same wavelength.
Answer: D
Section: 4.6 The Wave Nature of Light
40) Which of the following colors of light has the shortest wavelength?
A) violet
B) green
C) yellow
D) red
E) All colors have the same wavelength.
Answer: A
Section: 4.6 The Wave Nature of Light
41) Which of the following types of radiation has the longest wavelength?
A) X rays
B) ultraviolet
C) visible
D) infrared
E) All radiation has the same wavelength.
Answer: D
Section: 4.6 The Wave Nature of Light
42) Which of the following colors of light has the highest frequency?
A) violet
B) green
C) yellow
D) red
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E) All colors have the same frequency.
Answer: A
Section: 4.6 The Wave Nature of Light
43) Which of the following wavelengths of light has the lowest frequency?
A) 440 nm
B) 470 nm
C) 540 nm
D) 650 nm
E) All wavelengths have the same frequency.
Answer: D
Section: 4.6 The Wave Nature of Light
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44) Which of the following types of radiation has the highest frequency?
A) X rays
B) ultraviolet
C) visible
D) infrared
E) All radiation has the same frequency.
Answer: A
Section: 4.6 The Wave Nature of Light
45) Which of the following colors of light has the highest energy?
A) violet
B) blue
C) green
D) red
E) All colors have the same energy.
Answer: A
Section: 4.6 The Wave Nature of Light
46) Which of the following wavelengths of light has the lowest energy?
A) 440 nm
B) 470 nm
C) 540 nm
D) 650 nm
E) All wavelengths have the same energy.
Answer: D
Section: 4.6 The Wave Nature of Light
47) Which of the following types of radiation has the highest energy?
A) X rays
B) ultraviolet
C) visible
D) infrared
E) All radiation has the same energy.
Answer: A
Section: 4.6 The Wave Nature of Light
48) Which of the following colors of light has the highest velocity?
A) red
B) orange
C) yellow
D) green
E) All colors have the same velocity.
Answer: E
Section: 4.6 The Wave Nature of Light
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49) Which of the following wavelengths has the lowest velocity?
A) 440 nm
B) 470 nm
C) 540 nm
D) 650 nm
E) All wavelengths have the same velocity.
Answer: E
Section: 4.6 The Wave Nature of Light
50) Which of the following types of radiation has the highest velocity?
A) X rays
B) ultraviolet
C) visible
D) infrared
E) All radiation has the same velocity.
Answer: E
Section: 4.6 The Wave Nature of Light
51) Which of the following wavelengths of light is in the visible region of the radiant energy spectrum?
A) 250 nm
B) 550 nm
C) 850 nm
D) all of the above
E) none of the above
Answer: B
Section: 4.6 The Wave Nature of Light
52) Which of the following wavelengths of light is in the infrared region of the radiant energy spectrum?
A) 180 nm
B) 380 nm
C) 580 nm
D) 780 nm
E) all of the above
Answer: D
Section: 4.6 The Wave Nature of Light
53) Which of the following wavelengths of light is in the ultraviolet region of the radiant energy
spectrum?
A) 380 nm
B) 580 nm
C) 780 nm
D) 980 nm
E) all of the above
Answer: A
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Section:
4.6 The Wave Nature of Light
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54) Which of the following is an example of a quantized change in energy?
A) a ball rolling up a ramp
B) a ball rolling down a ramp
C) a ball rolling down a flight of stairs
D) a ball rolling across a playground
E) none of the above
Answer: C
Section: 4.7 The Quantum Concept
55) Which of the following instruments produces quantized musical notes?
A) cello
B) guitar
C) piano
D) violin
E) all of the above
Answer: C
Section: 4.7 The Quantum Concept
56) Which of the following instruments produces quantized musical notes?
A) banjo
B) harp
C) keyboard
D) ukulele
E) all of the above
Answer: C
Section: 4.7 The Quantum Concept
57) Which of the following instruments provides a quantized measurement?
A) meter stick
B) beam balance
C) 100-mL beaker
D) digital clock
E) none of the above
Answer: D
Section: 4.7 The Quantum Concept
58) Which of the following instruments provides a quantized measurement?
A) metric ruler
B) electronic balance
C) graduated cylinder
D) sweep-second watch
E) none of the above
Answer: B
Section: 4.7 The Quantum Concept
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59) Which of the following is evidence for an electron quantum jump?
A) infrared spectrum
B) line spectrum
C) ultraviolet spectrum
D) visible spectrum
E) none of the above
Answer: B
Section: 4.7 The Quantum Concept
60) How many photons of light are emitted when the electron in a hydrogen atom drops from energy
level 3 to 1?
A) 1
B) 2
C) 3
D) 4
E) none of the above
Answer: A
Section: 4.8 Bohr Model of the Atom
61) How many photons of light are emitted when the electron in a hydrogen atom drops from energy
level 4 to 2?
A) 1
B) 2
C) 3
D) 4
E) none of the above
Answer: A
Section: 4.8 Bohr Model of the Atom
62) How many photons of light are emitted when the electron in a hydrogen atom drops from energy
level 5 to 3?
A) 1
B) 2
C) 3
D) 5
E) none of the above
Answer: A
Section: 4.8 Bohr Model of the Atom
63) How many photons of light are emitted when the electrons in 10 hydrogen atoms drop from energy
level 3 to 1?
A) 1
B) 10
C) 20
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D) 30
E) none of the above
Answer: B
Section: 4.8 Bohr Model of the Atom
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64) How many photons of light are emitted when the electrons in 10 hydrogen atoms drop from energy
level 4 to 2?
A) 1
B) 10
C) 20
D) 40
E) none of the above
Answer: B
Section: 4.8 Bohr Model of the Atom
65) How many photons of light are emitted when the electrons in 10 hydrogen atoms drop from energy
level 5 to 3?
A) 1
B) 10
C) 30
D) 50
E) none of the above
Answer: B
Section: 4.8 Bohr Model of the Atom
66) Which of the following produces the "atomic fingerprint" of an element?
A) excited electrons jumping to a higher energy level
B) excited electrons dropping to a lower energy level
C) excited protons jumping to a higher energy level
D) excited protons dropping to a lower energy level
E) none of the above
Answer: B
Section: 4.8 Bohr Model of the Atom
67) In 1895 lines were observed in the spectrum of uranium ore identical to those of helium in the
spectrum of the Sun. Which of the following produced the lines in the helium spectrum?
A) excited electrons jumping to a higher energy level
B) excited electrons dropping to a lower energy level
C) excited protons jumping to a higher energy level
D) excited protons dropping to a lower energy level
E) none of the above
Answer: B
Section: 4.8 Bohr Model of the Atom
68) In 1861 a green line was observed in the spectrum of selenium ore that led to the discovery of the
element thallium. Which of the following was responsible for the green line in the spectrum?
A) excited electrons jumping to a higher energy level
B) excited electrons dropping to a lower energy level
C) excited protons jumping to a higher energy level
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D) excited protons dropping to a lower energy level
E) none of the above
Answer: B
Section: 4.8 Bohr Model of the Atom
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69) Which of the following energy-level changes for an electron is most energetic?
A) 3 → 1
B) 4 → 1
C) 5 → 1
D) 6 → 1
E) All changes have the same energy.
Answer: D
Section: 4.8 Bohr Model of the Atom
70) Which of the following energy-level changes for an electron is most energetic?
A) 2 → 1
B) 3 → 2
C) 4 → 3
D) 5 → 4
E) All changes have the same energy.
Answer: A
Section: 4.8 Bohr Model of the Atom
71) Which of the following energy-level changes for an electron is least energetic?
A) 2 → 1
B) 3 → 2
C) 4 → 3
D) 5 → 4
E) All changes have the same energy.
Answer: D
Section: 4.8 Bohr Model of the Atom
72) Which of the following energy level changes in a hydrogen atom produces a visible spectral line?
A) 3 → 2
B) 4 → 2
C) 5 → 2
D) all of the above
E) none of the above
Answer: D
Section: 4.8 Bohr Model of the Atom
73) Which of the following energy level changes in a hydrogen atom produces a visible spectral line?
A) 3 → 1
B) 4 → 2
C) 5 → 3
D) all of the above
E) none of the above
Answer: B
Section: 4.8 Bohr Model of the Atom
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74) Which of the following energy level changes in a hydrogen atom produces a visible spectral line?
A) 2 → 1
B) 3 → 1
C) 4 → 1
D) all of the above
E) none of the above
Answer: E
Section: 4.8 Bohr Model of the Atom
75) What type of radiation is emitted when an electron in a hydrogen atom drops from energy level 5 to
2?
A) infrared
B) visible
C) ultraviolet
D) X ray
E) gamma ray
Answer: B
Section: 4.8 Bohr Model of the Atom
76) What type of radiation is emitted when an electron in a hydrogen atom drops from energy level 5 to
1?
A) infrared
B) visible
C) ultraviolet
D) X ray
E) gamma ray
Answer: C
Section: 4.8 Bohr Model of the Atom
77) What type of radiation is emitted when an electron in a hydrogen atom drops from energy level 5 to
4?
A) infrared
B) visible
C) ultraviolet
D) X ray
E) gamma ray
Answer: A
Section: 4.8 Bohr Model of the Atom
78) How many energy sublevels exist within the 1st principal energy level?
A) 1
B) 2
C) 3
D) 4
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E) none of the above
Answer: A
Section: 4.9 Energy Levels and Sublevels
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79) How many energy sublevels exist within in the 2nd principal energy level?
A) 1
B) 2
C) 3
D) 4
E) none of the above
Answer: B
Section: 4.9 Energy Levels and Sublevels
80) How many energy sublevels exist within the 3rd principal energy level?
A) 1
B) 2
C) 3
D) 4
E) none of the above
Answer: C
Section: 4.9 Energy Levels and Sublevels
81) How many energy sublevels exist within the 4th principal energy level?
A) 1
B) 2
C) 3
D) 4
E) none of the above
Answer: D
Section: 4.9 Energy Levels and Sublevels
82) What is the maximum number of electrons that can occupy an s energy sublevel?
A) 2
B) 6
C) 10
D) 14
E) none of the above
Answer: A
Section: 4.9 Energy Levels and Sublevels
83) What is the maximum number of electrons that can occupy a p energy sublevel?
A) 2
B) 6
C) 10
D) 14
E) none of the above
Answer: B
Section: 4.9 Energy Levels and Sublevels
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84) What is the maximum number of electrons that can occupy a d energy sublevel?
A) 2
B) 6
C) 10
D) 14
E) none of the above
Answer: C
Section: 4.9 Energy Levels and Sublevels
85) What is the maximum number of electrons that can occupy an f energy sublevel?
A) 2
B) 6
C) 10
D) 14
E) none of the above
Answer: D
Section: 4.9 Energy Levels and Sublevels
86) What is the maximum number of electrons that can occupy the 1st principal energy level?
A) 1
B) 2
C) 4
D) 8
E) none of the above
Answer: B
Section: 4.9 Energy Levels and Sublevels
87) What is the maximum number of electrons that can occupy the 2nd principal energy level?
A) 1
B) 2
C) 4
D) 8
E) none of the above
Answer: D
Section: 4.9 Energy Levels and Sublevels
88) What is the maximum number of electrons that can occupy the 3rd principal energy level?
A) 1
B) 2
C) 4
D) 8
E) none of the above
Answer: E
Section: 4.9 Energy Levels and Sublevels
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89) What is the maximum number of electrons that can occupy the 4th principal energy level?
A) 1
B) 2
C) 4
D) 8
E) none of the above
Answer: E
Section: 4.9 Energy Levels and Sublevels
90) Which electron sublevel follows the 4s sublevel according to increasing energy?
A) 3p
B) 3d
C) 4p
D) 4d
E) 5s
Answer: B
Section: 4.10 Electroni Configuration
91) Which electron sublevel follows the 3d sublevel according to increasing energy?
A) 3s
B) 3p
C) 4s
D) 4p
E) 4d
Answer: D
Section: 4.10 Electroni Configuration
92) Which electron sublevel follows the 4p sublevel according to increasing energy?
A) 3d
B) 4d
C) 4s
D) 5s
E) 5p
Answer: D
Section: 4.10 Electroni Configuration
93) Which electron sublevel follows the 5s sublevel according to increasing energy?
A) 4p
B) 4d
C) 5p
D) 5d
E) 6s
Answer: B
Section: 4.10 Electroni Configuration
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94) Which electron sublevel follows the 4d sublevel according to increasing energy?
A) 4s
B) 4p
C) 5s
D) 5p
E) 5d
Answer: D
Section: 4.10 Electroni Configuration
95) Which electron sublevel follows the 5p sublevel according to increasing energy?
A) 4d
B) 5d
C) 5s
D) 6s
E) 6p
Answer: D
Section: 4.10 Electroni Configuration
96) What is the electron configuration for an atom of fluorine?
A) 1s2 2s2 2p3
B) 1s2 2s2 2p5
C) 1s2 2s2 2p6 3s1
D) 1s2 2s2 2p6 3s2 3p5
E) none of the above
Answer: B
Section: 4.10 Electroni Configuration
97) What is the electron configuration for an atom of silicon?
A) 1s2 2s2 2p4
B) 1s2 2s2 2p6 3s2
C) 1s2 2s2 2p6 3s2 3p2
D) 1s2 2s2 2p6 3s2 3p4
E) none of the above
Answer: C
Section: 4.10 Electroni Configuration
98) What is the electron configuration for an atom of nickel?
A) 1s2 2s2 2p6 3s2 3p6 3d8
B) 1s2 2s2 2p6 3s2 3p6 4s2 3d8
C) 1s2 2s2 2p6 3s2 3p6 4s2 4p8
D) 1s2 2s2 2p6 3s2 3p6 4s2 4d8
E) none of the above
Answer: B
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Section:
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99) Which element has the following electron configuration: 1s2 2s2 2p6 3s2?
A) Ca
B) Mg
C) Na
D) Si
E) none of the above
Answer: B
Section: 4.10 Electroni Configuration
100) Which element has the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s1?
A) Al
B) Ca
C) K
D) Na
E) none of the above
Answer: C
Section: 4.10 Electroni Configuration
101) Which element has the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10?
A) Ca
B) Cd
C) Kr
D) Zn
E) none of the above
Answer: D
Section: 4.10 Electroni Configuration
102) Which element has the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2
3d10 4p6 5s2?
A) Ca
B) Rb
C) Sn
D) Sr
E) none of the above
Answer: D
Section: 4.10 Electroni Configuration
103) Which element has the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
4d5?
A) Br
B) Mn
C) Nb
D) Tc
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E) none of the above
Answer: D
Section: 4.10 Electroni Configuration
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104) Which element has the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2
3d10 4p6 5s2 4d10 5p2?
A) Sr
B) Zr
C) Sn
D) Hf
E) none of the above
Answer: C
Section: 4.10 Electroni Configuration
105) Which of the following is true of an electron orbit?
A) An electron orbit is a fixed energy state.
B) An electron orbit represents an energy level.
C) An electron orbit may contain eight electrons.
D) An electron orbit increases in size with greater energy.
E) all of the above
Answer: E
Section: 4.11 Quantum Mechanical Model of the Atom
106) Which of the following is true of an electron orbital?
A) An orbital may not gain or lose energy.
B) An orbital represents a probability boundary.
C) An orbital represents an energy state of an electron.
D) An orbital may contain no more than two electrons.
E) all of the above
Answer: E
Section: 4.11 Quantum Mechanical Model of the Atom
107) Which of the following is true for both an orbit and an orbital?
A) An orbit and an orbital always contain two electrons.
B) An orbit and an orbital can be described as elliptical.
C) An orbit and an orbital represent a fixed energy state.
D) An orbit and an orbital represent an electron boundary.
E) all of the above
Answer: C
Section: 4.11 Quantum Mechanical Model of the Atom
108) What term best describes the shape of an s orbital?
A) sphere
B) dumbbell
C) clover
D) ellipse
E) wave
Answer: A
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Section:
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109) What term best describes the shape of a p orbital?
A) sphere
B) dumbbell
C) clover
D) ellipse
E) wave
Answer: B
Section: 4.11 Quantum Mechanical Model of the Atom
110) Which of the following orbitals has a spherical shape?
A) 4s
B) 4px
C) 4dxy
D) all of the above
E) none of the above
Answer: A
Section: 4.11 Quantum Mechanical Model of the Atom
111) Which of the following orbitals has a "dumbbell" shape?
A) 4s
B) 4px
C) 4dxy
D) all of the above
E) none of the above
Answer: B
Section: 4.11 Quantum Mechanical Model of the Atom
112) Which of the following orbitals is the largest in size?
A) 1s
B) 2s
C) 3s
D) 4s
E) all s orbitals are the same size
Answer: D
Section: 4.11 Quantum Mechanical Model of the Atom
113) Which of the following orbitals is the lowest energy?
A) 1s
B) 2s
C) 3s
D) 4s
E) all s orbitals are the same energy
Answer: A
Section: 4.11 Quantum Mechanical Model of the Atom
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114) Which of the following orbitals is the highest energy?
A) 2px
B) 3px
C) 4px
D) 5px
E) all px orbitals are the same energy
Answer: D
Section: 4.11 Quantum Mechanical Model of the Atom
115) What is the maximum number of electrons in a 4s orbital?
A) 1
B) 2
C) 4
D) 6
E) none of the above
Answer: B
Section: 4.11 Quantum Mechanical Model of the Atom
116) What is the maximum number of electrons in a 4p orbital?
A) 1
B) 2
C) 3
D) 6
E) none of the above
Answer: B
Section: 4.11 Quantum Mechanical Model of the Atom
117) What is the maximum number of electrons in a 4d orbital?
A) 1
B) 2
C) 5
D) 10
E) none of the above
Answer: B
Section: 4.11 Quantum Mechanical Model of the Atom
118) How many orbitals are in the 4s subshell?
A) 1
B) 3
C) 4
D) 5
E) none of the above
Answer: A
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Section:
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119) How many orbitals are in the 4p subshell?
A) 1
B) 3
C) 4
D) 5
E) none of the above
Answer: B
Section: 4.11 Quantum Mechanical Model of the Atom
120) How many orbitals are in the 4d subshell?
A) 1
B) 3
C) 4
D) 5
E) none of the above
Answer: D
Section: 4.11 Quantum Mechanical Model of the Atom
121) What is the approximate diameter of an atom?
A) 10-13 cm
B) 10-8 cm
C) 1 cm
D) 108 cm
E) 1013 cm
Answer: B
Section: General Exercises
122) What is the approximate diameter of an atomic nucleus?
A) 10-13 cm
B) 10-8 cm
C) 1 cm
D) 108 cm
E) 1013 cm
Answer: A
Section: General Exercises
123) Which of the following statements is true?
A) Dalton proposed a "particle model" of matter.
B) Thomson proposed a "plum pudding model" of the atom.
C) Rutherford proposed a "nuclear model" of the atom.
D) Bohr proposed a "planetary model" of the atom.
E) all of the above.
Answer: E
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Section:
General Exercises
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124) Which of the following elements does not have a stable isotope? (Hint: Refer to the Periodic
Table.)
A) Ta
B) Tc
C) Te
D) Ti
E) none of the above
Answer: B
Section: General Exercises
125) Which of the following elements does not have a stable isotope? (Hint: Refer to the Periodic
Table.)
A) Na
B) Ne
C) Ni
D) No
E) none of the above
Answer: D
Section: General Exercises
126) Which of the following elements has at least one stable isotope? (Hint: Refer to the Periodic
Table.)
A) Ra
B) Rf
C) Rh
D) Rn
E) none of the above
Answer: C
Section: General Exercises
127) Which of the following is the best description of the Bohr atom?
A) an indivisible, indestructible particle
B) a homogeneous sphere of "plum pudding"
C) a sphere with a heavy, dense nucleus surrounded by electrons
D) a sphere with a heavy, dense nucleus circled by electrons in orbits
E) a sphere with a heavy, dense nucleus surrounded by electron orbitals
Answer: D
Section: General Exercises
128) An atom can be described by the analogy "like a marble in the Dallas Cowboys Stadium." If the
stadium represents an atom, what does the marble represent?
A) marble
B) electron
C) neutron
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D) nucleus
E) proton
Answer: D
Section: General Exercises
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129) The scattering of alpha particles by a thin metal foil can be described by the analogy "like a missile
shot through our solar system." If the missile represents an alpha particle, what do planets in our solar
system represent?
A) atoms
B) electrons
C) neutrons
D) nuclei
E) protons
Answer: D
Section: General Exercises
130) If an atom is enlarged to the size of a marble, and a marble is enlarged similarly, what would be the
approximate size of the marble?
A) a marble, ~1 cm
B) a baseball, ~10 cm
C) a beach ball, ~100 cm
D) Dallas Cowboys Stadium, ~10,000 cm
E) the Moon, ~100,000,000 cm
Answer: E
Section: General Exercises
131) Which of the following represents the quantum nature of matter?
A) atom
B) electron
C) neutron
D) photon
E) proton
Answer: A
Section: General Exercises
132) Which of the following represents the quantum nature of electricity?
A) atom
B) electron
C) ion
D) photon
E) proton
Answer: B
Section: General Exercises
133) Which of the following represents the quantum nature of light?
A) atom
B) electron
C) ion
D) photon
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E) proton
Answer: D
Section: General Exercises
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134) How many energy sublevels theoretically exist in the 5th energy level?
A) 1
B) 2
C) 3
D) 4
E) none of the above
Answer: E
Section: General Exercises
135) How many energy sublevels theoretically exist in the 6th energy level?
A) 1
B) 2
C) 3
D) 4
E) none of the above
Answer: E
Section: General Exercises
Chemistry Conncection - John Dalton
1) Which of the following was established by John Dalton?
A) atomic theory
B) quantum theory
C) law of conservation of mass
D) law of conservation of energy
E) law of conservation of mass and energy
Answer: A
2) Which of the following was responsible for Dalton's scientific success?
A) Dalton inherited great family wealth.
B) Dalton taught at a prestigious university.
C) Dalton had an excellent scientific education.
D) Dalton had meticulous work habits.
E) Dalton had political influence.
Answer: D
3) How was Dalton able to accept a degree from Oxford dressed in a scarlet robe, when wearing scarlet
was forbidden by his Quaker faith?
A) Dalton was color-blind and the robe appeared gray.
B) Dalton had to refuse the honor.
C) Dalton received special permission.
D) Dalton was given a private ceremony.
E) Dalton ignored his Quaker faith.
Answer: A
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Chemistry Connection - Heavy Water
1) Which of the following refers to a molecule of water in which the hydrogen atoms contain a neutron?
A) D2O
B) deuterium oxide
C) heavy water
D) all of the above
E) none of the above
Answer: D
2) What is the systematic name for heavy water?
A) deuterium oxide
B) deuterium water
C) tritium oxide
D) tritium water
E) none of the above
Answer: A
3) Which of the following physical properties has a higher value for heavy water than for ordinary
water?
A) molar mass
B) melting point
C) heat of fusion
D) all of the above
E) none of the above
Answer: D
4) Which of the following physical properties has a lower value for heavy water than for ordinary water?
A) density
B) boiling point
C) heat of vaporization
D) all of the above
E) none of the above
Answer: E
5) Which of the following physical properties is different for ordinary water and heavy water?
A) density
B) melting point
C) molar mass
D) all of the above
E) none of the above
Answer: D
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6) Which of the following physiological properties is different for ordinary water and heavy water?
A) odor
B) taste
C) toxicity
D) all of the above
E) none of the above
Answer: C
Critical Thinking - Neon Lights
1) Which of the following gaseous elements produces a reddish-purple light in an advertising display?
A) helium
B) hydrogen
C) mercury
D) neon
E) all of the above
Answer: B
2) Which of the following gaseous elements produces pink light in an advertising display?
A) helium
B) hydrogen
C) mercury
D) neon
E) all of the above
Answer: A
3) Which of the following gaseous elements produces blue light in an advertising display?
A) helium
B) hydrogen
C) mercury
D) neon
E) all of the above
Answer: C
4) Which of the following gaseous elements produces a reddish-orange light in an advertising display?
A) helium
B) hydrogen
C) mercury
D) neon
E) all of the above
Answer: D
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