Chemistry Atoms First 3rd Edition by Julia Burdge – Test Bank
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Sample Test
Chapter 3
Quantum Theory and the Electronic Structure of Atoms
1. What
is the capacity to do work and transfer heat?
2. electricity
3. power
4. C. energy
5. temperature
6. work
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Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: System/Surroundings and Heat/Work
Topic: Thermochemistry
2. What
kind of energy results from the interaction of charged particles?
3. thermal
energy
4. kinetic
energy
5. chemical
energy
6. D. electrostatic
energy
7. charged
energy
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Units of Energy
Topic: Thermochemistry
3. What
kind of energy results from motion?
4. potential
energy
5. B. kinetic
energy
6. chemical
energy
7. electrostatic
energy
8. velocity
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Units of Energy
Topic: Thermochemistry
4. What
is the energy possessed by an object by virtue of its position?
5. A. potential
energy
6. kinetic
energy
7. work
8. thermal
energy
9. velocity
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Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Units of Energy
Topic: Thermochemistry
5. What
is defined as the distance between identical points on successive waves?
6. frequency
7. amplitude
8. magnitude
9. D. wavelength
10.
light
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Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
6. Visible
light, radio waves, microwave radiation, infrared, ultraviolet radiation,
X-rays, and gamma rays all constitute the electromagnetic spectrum. Which of
the following characteristics do all of these kinds of radiation share?
7. they
all have the ability to generate heat in objects.
8. they
all have the same frequencies.
9. C. they
are all the transmission of energy in the form of waves.
10.
they have equal energies.
11.
they have the same electron spin state.
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
7. According
to scientist James Clerk Maxwell in the year 1873, a(n) ______________ consists
of an electric field component and a magnetic field component.
8. electrostatic
wave
9. isoelectric
wave
10.
atom
11.
paramagnetic wave
12.
E. electromagnetic
wave
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
8. What
is defined as the number of waves that pass through a particular point in one
second?
9. light
10.
amplitude
11.
magnitude
12.
wavelength
13.
E. frequency
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
9. A(n)
_________ is a point at which a standing wave has zero amplitude.
10.
crevice
11.
B. node
12.
pit
13.
burrow
14.
orbital
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
10.
When a solid is heated, it emits electromagnetic radiation known
as ________________. An example of such radiation is the element of a stove
stop burning bright red.
11.
isoelectric radiation
12.
visible and ultraviolet radiation
13.
C. blackbody
radiation
14.
paramagnetic radiation
15.
whitebody radiation
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Topic: Quantum Theory and Atomic Structure
11.
In the ___________, electrons are ejected from the surface of a
metal exposed to light of a certain minimum frequency.
12.
aura effect
13.
photon effect
14.
ritzwald effect
15.
D. photoelectric
effect
16.
None of the answers is correct.
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
12.
What is defined as the vertical distance from the midline of a
wave to the top of the peak or the bottom of the trough?
13.
light
14.
B. amplitude
15.
magnitude
16.
wavelength
17.
frequency
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Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Topic: Quantum Theory and Atomic Structure
13.
What is the frequency of electromagnetic radiation with
wavelength 532 nm? (c =
3.00 × 108 m/s)
14.
A. 64 ×
1014 s–1
15.
6.48 × 1012 s–1
16.
4.18 × 1018 s–1
17.
6.23 × 1014 s–1
18.
3.75 × 1015 s–1
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
14.
What is the wavelength of light having a frequency of 4.8 × 1014 s–1? (c = 3.00 × 108 m/s)
15.
0.0016 nm
16.
1600 m
17.
C. 630
nm
18.
1600 nm
19.
6.3 × 10–7 nm
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
15.
What is the frequency of light having a wavelength of 360 nm? (c = 3.00 x 108 m/s)
16.
A. 3 ×
1014 s–1
17.
1.2 × 10–6 s–1
18.
8.3 × 105 s–1
19.
108 s–1
20.
1.2 × 10–15 s–1
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
16.
Select the arrangement of electromagnetic radiation which starts
with the shortest wavelength and increases to longest wavelength.
17.
radio, infrared, ultraviolet, gamma rays
18.
radio, ultraviolet, infrared, gamma rays
19.
gamma rays, radio, ultraviolet, infrared
20.
gamma rays, infrared, radio, ultraviolet
21.
E. gamma
rays, ultraviolet, infrared, radio
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
17.
Select the arrangement of electromagnetic radiation which starts
with the lowest energy and increases to the greatest energy.
18.
A. radio,
infrared, ultraviolet, gamma rays
19.
radio, ultraviolet, infrared, gamma rays
20.
gamma rays, infrared, radio, ultraviolet
21.
gamma rays, ultraviolet, infrared, radio
22.
infrared, ultraviolet, radio, gamma rays
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
18.
What is the wavelength of radiation that has a frequency of
6.912 × 1014 s–1? (c = 3.00 × 108 m/s)
19.
1.447 × 10–15 nm
20.
B. 337 ×
102 nm
21.
2.304 × 106 nm
22.
2.074 × 1023 nm
23.
4.337 × 10–7 nm
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
19.
Calculate the frequency of visible light having a wavelength of
686 nm. (c =
3.00 × 108 m/s)
20.
A. 37 ×
1014 s–1
21.
4.34 × 105 s–1
22.
6.17 × 1014 s–1
23.
2.29 × 10–15 s–1
24.
2.29 × 10–6 s–1
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
20.
The FM station KDUL broadcasts music at 99.1 MHz. Find the
wavelength of these waves. (c =
3.00 × 108 m/s)
21.
1.88 × 10–2 m
22.
0.330 m
23.
C. 03 m
24.
5.33 × 102 m
25.
> 103 m
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
21.
What is the energy in joules of a mole of photons associated
with visible light of wavelength 486 nm? (c =
3.00 × 108 m/s; h =
6.63 × 10–34 J • s; NA =
6.022 × 1023 moles–1)
22.
6.46 × 10–16 J
23.
6.46 × 10–25 J
24.
2.46 × 10–4 J
25.
12.4 kJ
26.
E. 246
kJ
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
Topic: Thermochemistry
22.
What is the energy in joules of a mole of photons associated
with red light of wavelength 7.00 × 102 nm? (c =
3.00 × 108 m/s; h =
6.63 × 10–34 J • s; NA =
6.022 × 1023 /mole)
23.
256 kJ
24.
B. 71 ×
105 J
25.
4.72 × 10–43J
26.
12.4 kJ
27.
2.12 × 1042J
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Subtopic: Units of Energy
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
Topic: Thermochemistry
23.
A radio wave has a frequency of 8.6 × 108 Hz.
What is the energy of one photon of this radiation? (h = 6.63 × 10–34 J
• s)
24.
7.7 × 10–43 J
25.
2.3 × 10–34 J
26.
C. 7 ×
10–25 J
27.
1.7 × 10–16 J
28.
> 10–15 J
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Subtopic: Units of Energy
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
Topic: Thermochemistry
24.
The solar radiation spectrum peaks at a wavelength of
approximately 500 nm. Calculate the energy of one photon of that radiation. (c = 3.00 × 108 m/s; h = 6.63 × 10–34 J
• s)
25.
4 × 10–10 J
26.
6 × 1014 J
27.
1 × 10–27 J
28.
2 × 10–25 J
29.
E. 4 ×
10–19 J
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Subtopic: Units of Energy
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
Topic: Thermochemistry
25.
If the energy of a photon is 1.32 × 10–18 J,
what is its wavelength in nm? (c =
3.00 × 108 m/s; h =
6.63 × 10–34 J • s)
26.
1.51 × 10–7 nm
27.
B. 151
nm
28.
1.99 × 1015 nm
29.
1.99 × 1024 nm
30.
None of these choices is correct.
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Bloom’s Level: 3. Apply
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Subtopic: Units of Energy
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
26.
A photon has an energy of 5.53 × 10–17 J.
What is its frequency in s–1? (h = 6.63 × 10–34 J
• s)
27.
3.66 × 10–50 s–1
28.
1.20 × 10–17 s–1
29.
3.59 × 10–9 s–1
30.
2.78 × 108 s–1
31.
E. 34 ×
1016 s–1
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
27.
Calculate the energy, in joules, required to excite a hydrogen
atom by causing an electronic transition from the n = 1 to the n = 4 principal
energy level. Recall that the energy levels of the H atom are given by En =
–2.18 × 10–18 J(1/n2 ).
28.
2.07 × 10–29 J
29.
2.19 × 105 J
30.
C. 04 ×
10–18 J
31.
3.27 × 10–17 J
32.
2.25 × 10–18 J
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
Topic: Thermochemistry
28.
Calculate the wavelength, in nanometers, of the light emitted by
a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal
energy level. Recall that the energy levels of the H atom are given by En =
–2.18 × 10–18 J (1/n2). (c = 3.00 × 108 m/s; h = 6.63 × 10–34 J
• s)
29.
4.45 × 10–20 nm
30.
2.16 × 10–6 nm
31.
9.18 × 10–20 nm
32.
1.38 × 1014 nm
33.
E. 17 ×
103 nm
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Subtopic: Units of Energy
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
Topic: Thermochemistry
29.
Calculate the frequency of the light emitted by a hydrogen atom
during a transition of its electron from the n = 4 to the n = 1 principal
energy level. Recall that for hydrogen En =
–2.18 × 10–18 J(1/n2 ).
(h = 6.63
× 10–34 J • s)
30.
A. 08
×1015 s–1
31.
1.03 × 108 s–1
32.
2.06 × 1014 s–1
33.
1.35 × 10–51 s–1
34.
8.22 × 1014 s–1
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Bloom’s Level: 3. Apply
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
30.
Use the Rydberg equation to calculate the frequency of a photon
absorbed when the hydrogen atom undergoes a transition from n1 = 2 to n2 = 4.
(R =
1.096776 × 107 m–1; c = 3.00 × 108 m/s)
31.
2.06 × 106 s–1
32.
2.74 × 106 s–1
33.
C. 17 ×
1014 s–1
34.
8.23 × 1014 s–1
35.
> 1015 s–1
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
31.
Line spectra from all regions of the electromagnetic spectrum,
including the Paschen series of infrared lines for hydrogen, are used by
astronomers to identify elements present in the atmospheres of stars. Calculate
the wavelength of the photon emitted when the hydrogen atom undergoes a
transition from n =
5 to n =
3. (R =
1.096776 × 107 m–1)
32.
205.1 nm
33.
384.6 nm
34.
683.8 nm
35.
D. 1282
nm
36.
>1500 nm
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
32.
Calculate the wavelength associated with a 20Ne+ ion
moving at a velocity of 2.0 × 105 m/s.
The atomic mass of Ne-20 is 19.992 amu. (1 amu = 1.66 × 10–24 g
and h =
6.63 × 10–34 J • s)
33.
A. 0 ×
10–13 m
34.
1.0 × 10–16 m
35.
1.0 × 10–18 m
36.
9.7 × 1012 m
37.
2.0 × 10–13 cm
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
33.
Calculate the wavelength of a neutron that has a velocity of
200. cm/s. (mass of a neutron = 1.675 × 10–27 kg
and h =
6.63 × 10–34 J • s)
34.
1.98 × 10–9 m
35.
216 nm
36.
1.8 × 1050 m
37.
D. 198
nm
38.
5.05 mm
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
34.
A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s.
What is his wavelength at this speed if his mass is 84.5 kg ? (h = 6.63 × 10–34 J
• s)
35.
A. 31 ×
10–37 m
36.
3.26 × 10–37 m
37.
5.08 × 10–30 m
38.
1.34 × 10–30 m
39.
None of these choices is correct.
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Bloom’s Level: 3. Apply
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Quantum Mechanics (Wave-Particle Duality and the
Heisenberg Uncertainty Principle)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
35.
The de Broglie equation predicts that the wavelength (in m) of a
proton moving at 1000. m/s is ________________.
(h =
6.63 × 10–34 J • s; mass of a proton = 1.673 × 10–24 g)
3. A. 96 ×
10–10 m
4. 3.96
× 10–7 m
5. 2.52
× 106 m
6. 2.52
× 109 m
7. >
1010 m
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Quantum Mechanics (Wave-Particle Duality and the
Heisenberg Uncertainty Principle)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
36.
According to the Heisenberg uncertainty principle, if the
uncertainty in the speed of an electron is 3.5 × 103 m/s,
the uncertainty in its position (in m) is at least ___________. (mass of an electron
= 9.11 × 10–28 g)
37.
A. 7 ×
10–8 m
38.
6.6 × 10–8 m
39.
17 m
40.
66 m
41.
None of these choices is correct.
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Dimensional Analysis
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Quantum Mechanics (Wave-Particle Duality and the
Heisenberg Uncertainty Principle)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
Topic: Study of Chemistry
37.
What is the emission of light at only specific wavelengths?
38.
emission spectra
39.
hydrogen spectrum
40.
wave spectra
41.
limited spectra
42.
E. line
spectra
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Measurement (SI Units)
Subtopic: Scientific Notation and Significant Figures
Topic: Quantum Theory and Atomic Structure
38.
The word _________ is used as an acronym for the amplification
of light which is stimulated by the emission of radiation.
39.
beam
40.
B. laser
41.
emit
42.
brighten
43.
light
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Electromagnetic Radiation (Wave Properties)
Topic: Quantum Theory and Atomic Structure
39.
Which scientist proposed that energy of radiation is composed of
extremely small indivisible packages called quanta? (“Quanta” is the plural of
“quantum.”)
40.
A. Max
Planck
41.
Louis de Broglie
42.
Clinton Davisson
43.
Sir Isaac Newton
44.
Lothan Meyer
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Electromagnetic Radiation (Wave Properties)
Subtopic: Plank’s Quantum Theory and Einstein’s Photoelectric
Effect
Topic: Quantum Theory and Atomic Structure
40.
The size of an atomic orbital is associated with
41.
A. the
principal quantum number (n).
42.
the angular momentum quantum number (l).
43.
the magnetic quantum number (ml).
44.
the spin quantum number (ms).
45.
the angular momentum and magnetic quantum numbers, together.
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Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Atomic Theories
Subtopic: Quantum Numbers
Topic: Components of Matter
Topic: Quantum Theory and Atomic Structure
41.
The shape of an atomic orbital is associated with
42.
the principal quantum number (n).
43.
B. the
angular momentum quantum number (l).
44.
the magnetic quantum number (ml).
45.
the spin quantum number (ms).
46.
the magnetic and spin quantum numbers, together.
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Bloom’s Level: 3. Apply
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Theories
Subtopic: Quantum Numbers
Topic: Components of Matter
Topic: Quantum Theory and Atomic Structure
42.
The orientation in space of an atomic orbital is associated with
43.
the principal quantum number (n).
44.
the angular momentum quantum number (l).
45.
C. the
magnetic quantum number (ml).
46.
the spin quantum number (ms)
47.
None of these choices is correct.
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Bloom’s Level: 3. Apply
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Theories
Subtopic: Quantum Numbers
Topic: Components of Matter
Topic: Quantum Theory and Atomic Structure
43.
Atomic orbitals developed using quantum mechanics
44.
A. describe
regions of space in which one is most likely to find an electron.
45.
describe exact paths for electron motion.
46.
give a description of the atomic structure which is essentially
the same as the Bohr model.
47.
allow scientists to calculate an exact volume for the hydrogen
atom.
48.
are in conflict with the Heisenberg uncertainty principle.
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Bloom’s Level: 3. Apply
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Theories
Subtopic: Quantum Numbers
Topic: Components of Matter
Topic: Quantum Theory and Atomic Structure
44.
The energy of an electron in the hydrogen atom is determined by
45.
A. the
principal quantum number (n)
only.
46.
the angular momentum quantum number (l) only.
47.
the principal and angular momentum quantum numbers (n & l).
48.
the principal and magnetic quantum numbers (n & ml).
49.
the principal, angular momentum, and magnetic quantum numbers.
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Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Atomic Theories
Subtopic: Quantum Numbers
Topic: Components of Matter
Topic: Quantum Theory and Atomic Structure
45.
Which of the following is a correct set of quantum numbers for
an electron in a 3d orbital?
46.
n =
3, l =
0, ml = –1
47.
n =
3, l =
1, ml = +3
48.
n =
3, l =
2, ml = 3
49.
n =
3, l =
3, ml = +2
50.
E. n =
3, l =
2, ml = –2
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Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
46.
Which of the following is a correct set of quantum numbers for
an electron in a 5f orbital?
47.
A. n =
5, l =
3, ml = +1
48.
n =
5, l =
2, ml = +3
49.
n =
4, l =
3, ml = 0
50.
n =
4, l =
2, ml = +1
51.
n =
5, l =
4, ml = 3.
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Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
47.
In the quantum mechanical treatment of the hydrogen atom, which
one of the following combinations of quantum numbers is not allowed?
|
|
n |
l |
ml |
|
A |
3 |
0 |
0 |
|
B |
3 |
1 |
–1 |
|
C |
3 |
2 |
2 |
|
D |
3 |
2 |
–1 |
|
E |
3 |
3 |
2 |
1. A
2. B
3. C
4. D
5. E. E
Bloom’s Level: 5. Evaluate
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
48.
Which one of the following sets of quantum numbers can correctly
represent a 3p orbital?
|
A |
B |
C |
D |
E |
|
n = 3 |
n = 1 |
n = 3 |
n = 3 |
n = 3 |
|
l = 1 |
l = 3 |
l = 2 |
l = 1 |
l = 0 |
|
ml = 2 |
ml = 3 |
ml = 1 |
ml = –1 |
ml = 1 |
1. A
2. B
3. C
4. D. D
5. E
Bloom’s Level: 5. Evaluate
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
49.
Which one of the following sets of quantum numbers is not
possible?
|
n |
l |
ml |
ms |
|
|
A |
4 |
3 |
–2 |
+1/2 |
|
B |
3 |
0 |
1 |
–1/2 |
|
C |
3 |
0 |
0 |
+1/2 |
|
D |
2 |
1 |
1 |
–1/2 |
|
E |
2 |
0 |
0 |
+1/2 |
1. A
2. B. B
3. C
4. D
5. E
Bloom’s Level: 5. Evaluate
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
50.
Which one of the following sets of quantum numbers is not
possible?
|
n |
l |
ml |
ms |
|
|
A |
4 |
3 |
–2 |
+1/2 |
|
B |
3 |
2 |
–3 |
–1/2 |
|
C |
3 |
0 |
0 |
+1/2 |
|
D |
4 |
1 |
1 |
–1/2 |
|
E |
2 |
0 |
0 |
+1/2 |
1. A
2. B. B
3. C
4. D
5. E
Bloom’s Level: 5. Evaluate
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
51.
What is the maximum number of electrons in an atom that can have
the following set of quantum numbers? n =
4, l =
3, ml =
–2, ms =
+1/2
52.
o
53.
B. 1
54.
2
55.
6
56.
10
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Bloom’s Level: 5. Evaluate
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
52.
A possible set of quantum numbers for the last electron added to
complete an atom of gallium (Ga) in its ground state is
|
|
n |
l |
ml |
ms |
|
A |
4 |
0 |
0 |
–1/2 |
|
B |
3 |
1 |
0 |
–1/2 |
|
C |
4 |
1 |
0 |
+1/2 |
|
D |
3 |
1 |
1 |
+1/2 |
|
E |
4 |
2 |
1 |
+1/2 |
1. A
2. B
3. C. C
4. D
5. E
Accessibility: Keyboard Navigation
Bloom’s Level: 5. Evaluate
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
53.
A possible set of quantum numbers for the last electron added to
complete an atom of germanium in its ground state is n l
|
|
n |
l |
ml |
ms |
|
A |
4 |
0 |
0 |
+1/2 |
|
B |
3 |
0 |
+1 |
–1/2 |
|
C |
4 |
1 |
–1 |
+1/2 |
|
D |
3 |
1 |
+1 |
–1/2 |
|
E |
4 |
2 |
+2 |
–1/2 |
1. A
2. B
3. C. C
4. D
5. E
Accessibility: Keyboard Navigation
Bloom’s Level: 5. Evaluate
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
54.
Electrons in an orbital with l = 3 are in a/an
55.
d orbital.
56.
B. f
57.
g orbital.
58.
p orbital.
59.
s orbital.
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Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
55.
The number of orbitals in a d subshell is
56.
1.
57.
2.
58.
3.
59.
D.
60.
7.
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Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
56.
The maximum number of electrons that can occupy an energy level
described by the principal quantum number, n, is
57.
n
58.
n + 1
59.
2n
60.
D. 2n2
61.
n2
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Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
57.
How many orbitals are allowed in a subshell if the angular
momentum quantum number for electrons in that subshell is 3?
58.
1
59.
3
60.
5
61.
D. 7
62.
9
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Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
58.
The Pauli exclusion principle states that no ____ electrons
within an atom can have the same ____ quantum numbers.
59.
4; 6
60.
B. 2; 4
61.
3; 6
62.
6; 10
63.
3; 8
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Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
59.
Hund’s rule states that the most stable arrangement of electrons
in orbitals of equal energy is the one in which the number of electrons with
parallel spin is ______________.
60.
minimized
61.
nullified
62.
neutral
63.
D. maximized
64.
not relevant
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Bloom’s Level: 1. Remember
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Hund’s Rule
Topic: Electron Configuration
60.
___________________ is the wavelength associated with a moving
particle.
61.
A. The
de Broglie wavelength
62.
The Heisenburg wavelength
63.
The Hund wavelength
64.
The Aufbau wavelength
65.
None of these choices is correct.
Accessibility: Keyboard Navigation
Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Quantum Mechanics (Wave-Particle Duality and the
Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure
61.
Atomic orbitals that have the same amount of energy are
______________.
62.
regenerative
63.
negatively charged
64.
C. degenerate
65.
positively charged
66.
zwitterionic
Accessibility: Keyboard Navigation
Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
62.
What type of configuration specifies the arrangement of
electrons in the orbitals of an atom?
63.
heisenberg configuration
64.
nuclear configuration
65.
atomic configuration
66.
proton configuration
67.
E. electron
configuration
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Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
63.
“No two electrons in an atom can have the same four quantum
numbers” is a statement of
64.
A. the
Pauli exclusion principle.
65.
Bohr’s equation.
66.
Hund’s rule.
67.
de Broglie’s relation.
68.
Dalton’s atomic theory.
Accessibility: Keyboard Navigation
Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
64.
The most stable arrangement of electrons in orbitals of equal
energy is the one in which the number of electrons with the same spin is maximized
65.
the Pauli exclusion principle.
66.
Bohr’s equation.
67.
C. Hund’s
rule.
68.
de Broglie’s relation.
69.
Dalton’s atomic theory.
Accessibility: Keyboard Navigation
Bloom’s Level: 2. Understand
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Hund’s Rule
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure
65.
How many orbitals are there in the n = 4 level of the
H-atom?
66.
4
67.
6
68.
8
69.
D. 16
70.
18
Accessibility: Keyboard Navigation
Bloom’s Level: 3. Apply
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Hard
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
66.
The orbital diagram for a ground-state nitrogen atom is
|
|
1s |
2s |
2p |
|
|
|
A |
↿⇂ |
↿⇂ |
↿ |
↿ |
↿ |
|
B |
↿⇂ |
↿ |
↿⇂ |
↿ |
— |
|
C |
↿⇂ |
↿⇂ |
↿⇂ |
↿ |
— |
|
D |
↿⇂ |
↿⇂ |
↿⇂ |
↿ |
↿ |
|
E |
↿⇂ |
↿⇂ |
↿⇂ |
↿⇂ |
↿ |
1. A. A
2. B
3. C
4. D
5. E
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
67.
The orbital diagram for a ground-state oxygen atom is
|
|
1s |
2s |
2p |
|
|
|
A |
↿⇂ |
↿⇂ |
↿ |
↿ |
↿ |
|
B |
↿⇂ |
↿⇂ |
↿⇂ |
↿⇂ |
— |
|
C |
↿⇂ |
↿⇂ |
↿⇂ |
↿ |
— |
|
D |
↿⇂ |
↿⇂ |
↿⇂ |
↿ |
↿ |
|
E |
↿⇂ |
↿⇂ |
↿⇂ |
↿⇂ |
↿ |
1. A
2. B
3. C
4. D. D
5. E
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
68.
The orbital diagram for a ground-state carbon atom is
|
|
1s |
2s |
2p |
|
|
|
|
A |
↿⇂ |
↿⇂ |
↿⇂ |
— |
— |
|
|
B |
↿⇂ |
↿ |
↿ |
↿ |
↿ |
|
|
C |
↿⇂ |
↿⇂ |
↿ |
↿ |
↿ |
|
|
D |
↿⇂ |
↿⇂ |
↿ |
↿ |
— |
|
|
E |
↿⇂ |
↿⇂ |
↿⇂ |
↿⇂ |
↿ |
|
1. A
2. B
3. C
4. D. D
5. E
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
69.
Which ground-state atom has an electron configuration described
by the following orbital
diagram?
|
[Ar] |
↿⇂ |
|
↿⇂ |
↿⇂ |
↿⇂ |
↿⇂ |
↿⇂ |
|
↿⇂ |
↿ |
↿ |
|
|
4s |
|
|
|
3d |
|
|
|
|
4p |
1. phosphorus
2. germanium
3. C. selenium
4. tellurium
5. potassium
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
70.
Which ground-state atom has an electron configuration described
by the following orbital
diagram?
|
[Ne] |
↿⇂ |
|
↿ |
↿ |
↿ |
|
|
3s |
|
|
3p |
|
1. A. phosphorus
2. nitrogen
3. arsenic
4. vanadium
5. sulfur
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
71.
How many unpaired electrons does a ground-state atom of sulfur
have?
72.
0
73.
1
74.
C. 2
75.
3
76.
4
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
72.
Which element has the following ground-state electron
configuration?
1s2 2s2 2p6 3s2
1. Na
2. B. Mg
3. Al
4. Si
5. Ne
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Hund’s Rule
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
73.
Which element has the following ground-state electron
configuration?
[Kr]5s24d105p3
1. Sn
2. B. Sb
3. Pb
4. Bi
5. Te
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
74.
Which element has the following ground-state electron
configuration?
[Kr]5s24d105p2
1. A. Sn
2. Sb
3. Pb
4. Ge
5. Te
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
75.
The electron configuration of a ground-state Co atom is
76.
A. [Ar]4s23d7
77.
1s22s22p63s23d9
78.
[Ne]3s23d7
79.
[Ar]4s13d5
80.
[Ar]4s24d7
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
76.
The electron configuration of a ground-state vanadium atom is
77.
[Ar]4s24d3
78.
[Ar]4s24p3
79.
C. [Ar]4s23d3
80.
[Ar]3d5
81.
[Ar]4s23d7
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
77.
The electron configuration of a ground-state copper atom is
78.
[Ar]4s24d4
79.
[Ar]4s24p63d3
80.
[Ar]4s23d9
81.
[Ar]3d9
82.
E. [Ar]4s13d10
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
78.
The ground-state electron configuration for an atom of indium is
79.
[Kr]5s24p64d5
80.
[Ar]4s23d104p1
81.
[Ar]4s24p63d5
82.
[Kr]5s25p64d5
83.
E. [Kr]5s24d105p1
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Medium
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau
Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
79.
The ground-state electron configuration of a calcium atom is
80.
[Ne]3s2
81.
[Ne]3s23p6
82.
[Ar]4s13d1
83.
D. [Ar]4s2
84.
[Ar]3d2
Accessibility: Keyboard Navigation
Bloom’s Level: 4. Analyze
Chapter: 03 Quantum Theory and the Electronic Structure of Atoms
Difficulty: Easy
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Energy-Level Splitting (Zeff and Shielding)
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure
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