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CHAPTER 5-6
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1)
What is the term for the weighted average mass of all the naturally occurring isotopes of an element?
1)
_______
atomic number
atomic notation
mass number
atomic mass
none of the above
2)
What is the term for a unit of mass exactly equal to 1/12 the mass of a carbon-12 atom?
2)
_______
neutron
hydrogen atom
atomic mass unit
proton
none of the above
3)
What is the term for a symbolic method of expressing the composition of an atomic nucleus?
3)
_______
mass number
atomic mass
atomic number
atomic notation
none of the above
4)
What is the term for the region of very high density in the center of the atom?
4)
_______
atomic kernel
atomic center
atomic core
atomic nucleus
none of the above
5)
What is the term for the value that indicates the number of protons for an atom of a given element?
5)
_______
mass number
atomic number
atomic notation
atomic mass
none of the above
6)
What is the term for the atomic model that describes electrons circling the nucleus in an orbit of specific energy?
6)
_______
Thomson atom
quantum mechanical atom
Rutherford atom
Bohr atom
none of the above
7)
What is the term for a broad uninterrupted band of radiant energy?
7)
_______
radiant energy spectrum
visible spectrum
continuous spectrum
ultraviolet spectrum
none of the above
8)
What is the negatively charged subatomic particle having a negligible mass?
8)
_______
quark
neutron
electron
proton
none of the above
9)
What is the term for the shorthand description of the arrangement of electrons by sublevels according to increasing energy?
9)
_______
atomic notation
electron configuration
atomic number
continuous spectrum
none of the above
10)
What is the term for the collection of narrow bands of light that results from excited atoms of a given element releasing energy?
10)
______
electromagnetic spectrum
continuous spectrum
emission line spectrum
radiant energy spectrum
none of the above
11)
What is the term for an orbit that electrons occupy at a fixed distance from the nucleus; designated 1, 2, 3, 4 ..?
11)
______
orbital
energy level
shell
subshell
none of the above
12)
What is the term for an electron energy level that results from splitting a main energy level?
12)
______
shell
subshell
energy sublevel
orbital
none of the above
13)
What is the term for the number of times a light wave travels a complete cycle in one second?
13)
______
wavelength
frequency
velocity
energy
none of the above
14)
What is the term for two atoms of the same element that differ by the number of neutrons in the nucleus?
14)
______
nucleons
photons
isotopes
atomic mass units
none of the above
15)
What is the general term that refers to either visible or invisible radiant energy?
15)
______
emission spectrum
continuous spectrum
line spectrum
light
none of the above
16)
What is the term for the value that indicates the total number of protons and neutrons in an atom of a given element?
16)
______
mass number
atomic notation
atomic number
atomic mass
none of the above
17)
What is the neutral subatomic particle having an approximate mass of 1 amu?
17)
______
proton
electron
quark
neutron
none of the above
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?
18)
______
quantum level
electron shell
orbital
electron subshell
none of the above
19)
What is the term for a particle of radiant energy?
19)
______
proton
electron
neutron
photon
none of the above
20)
What is the positively charged subatomic particle having an approximate mass of 1 amu?
20)
______
neutron
quark
proton
electron
none of the above
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?
21)
______
nuclear atom
quantum mechanical atom
Bohr atom
planetary atom
none of the above
22)
What is the term for the range of light energy extending from short wavelength gamma rays to long wavelength microwaves?
22)
______
visible spectrum
microwave spectrum
radiant energy spectrum
gamma ray spectrum
none of the above
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?
23)
______
uncertainty principle
spectrum rule
quantum principle
exclusion principle
none of the above
24)
What is the term for light energy that appears violet to red?
24)
______
radiant energy spectrum
infrared spectrum
visible spectrum
ultraviolet spectrum
none of the above
25)
What is the term for the distance a light wave travels to complete one cycle?
25)
______
frequency
energy
velocity
wavelength
none of the above
26)
Which of the following of Daltons proposals is still valid?
26)
______
An element is composed of tiny particles called atoms.
Compounds contain atoms in small whole number ratios.
Atoms of different elements combine to form compounds.
all of the above
none of the above
27)
Which of the following of Daltons proposals is still valid?
27)
______
Atoms can combine in more than one whole number ratio.
Atoms of different elements combine to form compounds.
Atoms can combine in small whole number ratios.
all of the above
none of the above
28)
Which of the following of Daltons proposals is still valid?
28)
______
Atoms of the same element are identical.
Atoms are indestructible.
Atoms are indivisible.
all of the above
none of the above
29)
According to the Thomson model of the atom, what is the simplest negative particle in an atom?
29)
______
alpha
electron
proton
neutron
none of the above
30)
According to the Thomson model, what is the simplest positive particle in an atom?
30)
______
proton
neutron
alpha
electron
none of the above
31)
According to the Thomson model, what is the relative charge on an electron?
31)
______
-1
+2
+1
-2
none of the above
32)
According to the Thomson model, what is the relative charge on a proton?
32)
______
+2
-2
-1
+1
none of the above
33)
What do the raisins represent in the plum-pudding analogy of the atom?
33)
______
electrons
alpha particles
neutrons
protons
none of the above
34)
Where is the mass of an atom according to the plum-pudding model?
34)
______
The mass is found in the electrons.
The mass is found in the nucleus.
The mass is distributed homogeneously.
The mass is found in the protons.
none of the above
35)
Which subatomic particle has a relative charge of -1 and a mass of ~0 amu?
35)
______
neutron
electron
proton
alpha
none of the above
36)
Which subatomic particle has a relative charge of +1 and a mass of ~1 amu?
36)
______
electron
proton
alpha
neutron
none of the above
37)
Which subatomic particle has a relative charge of 0 and a mass of ~1 amu?
37)
______
alpha
electron
proton
neutron
none of the above
38)
Which of the following subatomic particles is found outside the nucleus?
38)
______
neutron
proton
electron
all of the above
none of the above
39)
Which of the following subatomic particles are found inside the nucleus?
39)
______
neutron and proton
proton and electron
electron and neutron
all of the above
none of the above
40)
Which of the following subatomic particles are found outside the nucleus?
40)
______
proton and electron
electron and neutron
neutron and proton
all of the above
none of the above
41)
Using atomic notation, indicate the isotope having 11 p+, 12 n0, and 11 e-.
41)
______
Mg
Na
Na
Mg
Na
42)
Using atomic notation, indicate the isotope having 26 p+, 32 n0, and 26 e-.
42)
______
Fe
Fe
Fe
S
S
43)
Using atomic notation, indicate the isotope having 25 p+, 30 n0, and 25 e-.
43)
______
Mn
Zn
Mn
Mn
Zn
44)
How many neutrons are in the nucleus of an atom of O?
44)
______
10
26
18
8
none of the above
45)
How many neutrons are in the nucleus of an atom of Co?
45)
______
87
60
33
27
none of the above
46)
How many neutrons are in the nucleus of an atom of Sn?
46)
______
168
50
118
68
none of the above
47)
How many neutrons are in the nucleus of an atom of copper-65?
47)
______
65
94
36
29
none of the above
48)
How many neutrons are in the nucleus of an atom of bromine-79?
48)
______
114
44
79
35
none of the above
49)
How many neutrons are in the nucleus of an atom of silver-107?
49)
______
107
154
60
47
none of the above
50)
How many neutrons are in the nucleus of an atom of platinum-195?
50)
______
195
273
117
78
none of the above
51)
How many neutrons are in the nucleus of an atom of gold-197?
51)
______
197
79
276
118
none of the above
52)
What is the current reference isotope for the atomic mass scale?
52)
______
hydrogen-1
carbon-12
oxygen-16
helium-4
none of the above
53)
What is the assigned mass of the reference isotope for the atomic mass scale?
53)
______
1.01 amu
12 amu exactly
4.00 amu
16.00 amu
12.01 amu
54)
Why are atomic masses expressed on a relative atomic mass scale?
54)
______
Atoms are electrically neutral.
Atoms are too small to weigh directly.
Atoms are electrically positive.
Atoms are too reactive to weigh directly.
none of the above
55)
Given that the only naturally occurring isotope of sodium is 23Na,what is its isotopic mass? (Hint: Refer to the Periodic Table.)
55)
______
12.00 amu
11.99 amu
22.99 amu
11.00 amu
34.99 amu
56)
Given that the only naturally occurring isotope of aluminum is 27Al, what is its isotopic mass? (Hint: Refer to the Periodic Table.)
56)
______
26.98 amu
39.98 amu
13.98 amu
13.00 amu
14.00 amu
57)
Given that the only naturally occurring isotope of gold is 197Au,what is its isotopic mass? (Hint: Refer to the Periodic Table.)
57)
______
275.97 amu
117.97 amu
196.97 amu
118.00 amu
79.00 amu
58)
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%.
58)
______
6.50 amu
12.5 amu
6.94 amu
6.52 amu
6.09 amu
59)
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%.
59)
______
64.00 amu
107.85 amu
108.46 amu
64.32 amu
63.55 amu
60)
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%.
60)
______
120.92 amu
79.90 amu
80.00 amu
79.00 amu
119.93 amu
61)
Lithium occurs naturally as 6Li and 7Li. Which isotope is more abundant? (Hint: Refer to the Periodic Table.)
61)
______
lithium-4
lithium-6
lithium-3
lithium-7
none of the above
62)
Boron occurs naturally as 10B and 11B. Which isotope is more abundant? (Hint: Refer to the Periodic Table.)
62)
______
boron-6
boron-11
boron-5
boron-10
none of the above
63)
Copper occurs naturally as 63Cu and 65Cu. Which isotope is more abundant? (Hint: Refer to the Periodic Table.)
63)
______
copper-34
copper-65
copper-63
copper-36
none of the above
64)
Which of the following colors of light has the longest wavelength?
64)
______
orange
red
blue
violet
All colors have the same wavelength.
65)
Which of the following colors of light has the shortest wavelength?
65)
______
yellow
violet
red
green
All colors have the same wavelength.
66)
Which of the following types of radiation has the longest wavelength?
66)
______
visible
infrared
ultraviolet
X rays
All radiation has the same wavelength.
67)
Which of the following colors of light has the highest frequency?
67)
______
violet
yellow
red
green
All colors have the same frequency.
68)
Which of the following wavelengths has the lowest frequency?
68)
______
540 nm
440 nm
650 nm
470 nm
All wavelengths have the same frequency.
69)
Which of the following types of radiation has the highest frequency?
69)
______
infrared
X rays
ultraviolet
visible
All radiation has the same frequency.
70)
Which of the following colors of light has the highest energy?
70)
______
red
blue
violet
green
All colors have the same energy.
71)
Which of the following wavelengths has the lowest energy?
71)
______
470 nm
650 nm
440 nm
540 nm
All wavelengths have the same energy.
72)
Which of the following types of radiation has the highest energy?
72)
______
X rays
ultraviolet
infrared
visible
All radiation has the same energy.
73)
Which of the following colors of light has the highest velocity?
73)
______
green
orange
red
yellow
All colors have the same velocity.
74)
Which of the following wavelengths has the lowest velocity?
74)
______
470 nm
440 nm
650 nm
540 nm
All wavelengths have the same velocity.
75)
Which of the following types of radiation has the highest velocity?
75)
______
ultraviolet
X rays
visible
infrared
All radiation has the same velocity.
76)
Which of the following wavelengths of light is in the visible region of the radiant energy spectrum?
76)
______
550 nm
250 nm
950 nm
all of the above
none of the above
77)
Which of the following wavelengths of light is in the infrared region of the radiant energy spectrum?
77)
______
980 nm
180 nm
480 nm
all of the above
none of the above
78)
Which of the following wavelengths of light is in the ultraviolet region of the radiant energy spectrum?
78)
______
920 nm
520 nm
220 nm
all of the above
none of the above
79)
Which of the following is an example of a quantized change in energy?
79)
______
a ball rolling up a ramp
a ball rolling down a flight of stairs
a ball rolling down a ramp
a ball rolling across a playground
none of the above
80)
Which of the following instruments produces quantized musical notes?
80)
______
violin
cello
piano
guitar
all of the above
81)
Which of the following instruments produces quantized musical notes?
81)
______
banjo
ukulele
keyboard
harp
all of the above
82)
Which of the following instruments provides a quantized measurement?
82)
______
100-mL beaker
beam balance
digital clock
meter stick
none of the above
83)
Which of the following instruments provides a quantized measurement?
83)
______
metric ruler
sweep-second watch
graduated cylinder
electronic balance
none of the above
84)
Which of the following spectra is evidence for a quantized change?
84)
______
ultraviolet spectrum
line spectrum
visible spectrum
infrared spectrum
none of the above
85)
How many photons of light are emitted when the electron in a hydrogen atom drops from energy level 3 to 1?
85)
______
1
2
3
4
none of the above
86)
How many photons of light are emitted when the electron in a hydrogen atom drops from energy level 4 to 2?
86)
______
1
2
3
4
none of the above
87)
How many photons of light are emitted when the electron in a hydrogen atom drops from energy level 5 to 3?
87)
______
1
2
3
5
none of the above
88)
How many photons of light are emitted when the electrons in 10 hydrogen atoms drop from energy level 3 to 1?
88)
______
1
10
20
30
none of the above
89)
How many photons of light are emitted when the electrons in 10 hydrogen atoms drop from energy level 4 to 2?
89)
______
1
10
20
40
none of the above
90)
How many photons of light are emitted when the electrons in 10 hydrogen atoms drop from energy level 5 to 3?
90)
______
1
10
30
50
none of the above
91)
Which of the following produces the atomic fingerprint of an element?
91)
______
protons jumping to a higher energy level
electrons dropping to a lower energy level
protons dropping to a lower energy level
electrons jumping to a higher energy level
none of the above
92)
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?
92)
______
protons jumping to a higher energy level
electrons jumping to a higher energy level
protons dropping to a lower energy level
electrons dropping to a lower energy level
none of the above
93)
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?
93)
______
electrons dropping to a lower energy level
electrons jumping to a higher energy level
protons jumping to a higher energy level
protons dropping to a lower energy level
none of the above
94)
Which of the following energy-level changes for an electron is most energetic?
94)
______
5 1
3 1
4 1
6 1
All changes have the same energy.
95)
Which of the following energy-level changes for an electron is most energetic?
95)
______
4 3
2 1
5 4
3 2
All changes have the same energy.
96)
Which of the following energy-level changes for an electron is least energetic?
96)
______
3 2
5 4
4 3
2 1
All changes have the same energy.
97)
Which of the following energy level changes in a hydrogen atom produces a visible spectral line?
97)
______
4 2
3 2
5 2
all of the above
none of the above
98)
Which of the following energy level changes in a hydrogen atom produces a visible spectral line?
98)
______
4 2
3 1
5 3
all of the above
none of the above
99)
Which of the following energy level changes in a hydrogen atom produces a visible spectral line?
99)
______
3 1
4 1
2 1
all of the above
none of the above
100)
What type of radiation is emitted when an electron in a hydrogen atom drops from energy level 5 to 2?
100)
_____
X ray
gamma ray
infrared
visible
ultraviolet
101)
What type of radiation is emitted when an electron in a hydrogen atom drops from energy level 5 to 1?
101)
_____
X ray
visible
infrared
gamma ray
ultraviolet
102)
What type of radiation is emitted when an electron in a hydrogen atom drops from energy level 5 to 4?
102)
_____
visible
infrared
ultraviolet
gamma ray
X ray
103)
How many energy sublevels exist within the 1st principal energy level?
103)
_____
1
2
3
4
none of the above
104)
How many energy sublevels exist within in the 2nd principal energy level?
104)
_____
1
2
3
4
none of the above
105)
How many energy sublevels exist within the 3rd principal energy level?
105)
_____
1
2
3
4
none of the above
106)
How many energy sublevels exist within the 4th principal energy level?
106)
_____
1
2
3
4
none of the above
107)
What is the maximum number of electrons that can occupy an s energy sublevel?
107)
_____
2
6
10
14
none of the above
108)
What is the maximum number of electrons that can occupy a p energy sublevel?
108)
_____
2
6
10
14
none of the above
109)
What is the maximum number of electrons that can occupy a d energy sublevel?
109)
_____
2
6
10
14
none of the above
110)
What is the maximum number of electrons that can occupy an f energy sublevel?
110)
_____
2
6
10
14
none of the above
111)
What is the maximum number of electrons that can occupy the 1st principal energy level?
111)
_____
1
2
4
8
none of the above
112)
What is the maximum number of electrons that can occupy the 2nd principal energy level?
112)
_____
1
2
4
8
none of the above
113)
What is the maximum number of electrons that can occupy the 3rd principal energy level?
113)
_____
1
2
4
8
none of the above
114)
What is the maximum number of electrons that can occupy the 4th principal energy level?
114)
_____
1
2
4
8
none of the above
115)
Which electron sublevel follows the 4s sublevel according to increasing energy?
115)
_____
3p
3d
4p
4d
5s
116)
Which electron sublevel follows the 3d sublevel according to increasing energy?
116)
_____
3s
3p
4s
4p
4d
117)
Which electron sublevel follows the 4p sublevel
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