11) What is the wavelength of light (nm) that has a frequency of 6.44 × 1013 s-1?
A) 4660 nm
B) 6490 nm
C) 4.66 × 10-8 nm
D) 6.49 × 10-8 nm
E) 932 nm
12) What is the wavelength of light (nm) that has a frequency 4.62 × 1014 s-1?
A) 932 nm
B) 649 nm
C) 1.39 × 1023 nm
D) 1.54 × 10-3 nm
E) 1.07 × 106 nm
13) The wavelength of a photon that has an energy of 6.33 × 10–18 J is ________ m.
A) 3.79 × 10-7
B) 3.10 × 10-8
C) 2.38 × 1023
D) 4.21 × 10–24
E) 9.55 × 1015
14) The energy of a photon of light is ________ proportional to its frequency and ________ proportional to
its wavelength.
A) directly, directly
B) inversely, inversely
C) inversely, directly
D) directly, inversely
E) indirectly, not
15) The wavelength of a photon that has an energy of 5.25 × 10–19 J is ________ m.
A) 3.79 × 10-7
B) 2.64 × 106
C) 2.38 × 1023
D) 4.21 × 10–24
E) 3.79 × 107
16) The energy of a photon that has a wavelength of 9.0 m is ________ J.
A) 2.2 × 10–26
B) 4.5 × 1025
C) 6.0 × 10–23
D) 2.7 × 109
E) 4.5 × 10–25
17) The energy of a photon that has a wavelength of 8.33 × 10-6 m is ________ J.
A) 2.20 × 10–26
B) 3.60 × 1013
C) 2.39 × 10–20
D) 2.7 × 109
E) 4.5 × 10-25
18) The frequency of a photon that has an energy of 3.7 × 10–18 J is ________ s-1.
A) 5.6 × 1015
B) 1.8 × 10–16
C) 2.5 × 10–15
D) 5.4 × 10-8
E) 2.5 × 1015
19) The frequency of a photon that has an energy of 8.5 × 10–12 J is ________ s-1.
A) 1.3 × 1022
B) 1.8 × 10–16
C) 2.5 × 10–15
D) 5.4 × 10-8
E) 2.5 × 1015
20) The energy of a photon that has a wavelength of 12.3 nm is ________ J.
A) 1.51 × 10–17
B) 4.42 × 10–23
C) 1.99 × 10–25
D) 2.72 × 10–50
E) 1.62 × 10–17
21) The energy of a photon that has a wavelength of 13.2 nm is ________ J.
A) 9.55 × 10–25
B) 1.62 × 10–17
C) 1.99 × 10–25
D) 4.42 × 10–23
E) 1.51 × 10–17
22) The energy of a photon that has a frequency of 8.21 × 1015 s-1 is ________ J.
A) 8.08 × 10–50
B) 1.99 × 10–25
C) 5.44 × 10–18
D) 1.24 × 1049
E) 1.26 × 10–19
23) The energy of a photon that has a frequency of 1.821 × 1016 s-1 is ________ J.
A) 5.44 × 10–18
B) 1.99 × 10–25
C) 3.49 × 10–48
D) 1.21 × 10–17
E) 5.46 × 10–24
24) What is the frequency (s-1) of a photon that has an energy of 4.38 × 10–18 J?
A) 436 s-1
B) 6.61 × 1015 s-1
C) 1.45 × 10–16 s-1
D) 2.30 ×107 s-1
E) 1.31 × 10-9 s-1
25) What is the wavelength (angstroms) of a photon that has an energy of 4.38 × 10–18 J?
A) 45.4 angstroms
B) 2.30 × 107 angstroms
C) 6.89 × 1015 angstroms
D) 1.45 × 10–16 angstroms
E) 1.31 × 10-9 angstroms
26) What is the wavelength (angstroms) of a photon that has an energy of 5.69 × 10–17 J?
A) 454 angstroms
B) 34.9 angstroms
C) 6.89 × 1015 angstroms
D) 3.66 × 109 angstroms
E) 3.50 × 10-9 angstroms
25
27) A mole of red photons of wavelength 725 nm has ________ kJ of energy.
A) 2.74 × 10–19
B) 4.56 × 10–46
C) 6.05 × 10-3
D) 165
E) 227
28) A mole of yellow photons of wavelength 527 nm has ________ kJ of energy.
A) 165
B) 227
C) 4.56 × 10–46
D) 6.05 × 10-3
E) 2.74 × 10–19
29) Of the following, ________ radiation has the longest wavelength and ________ radiation has the
greatest energy.
gamma ultraviolet visible
A) ultraviolet, gamma
B) visible, ultraviolet
C) gamma, gamma
D) visible, gamma
E) gamma, visible
30) What color of visible light has the longest wavelength?
A) blue
B) violet
C) red
D) yellow
E) green
31) Of the following, ________ radiation has the shortest wavelength and ________ radiation has the
greatest energy.
gamma ultraviolet visible
A) gamma, visible
B) visible, gamma
C) visible, ultraviolet
D) ultraviolet, gamma
E) gamma, gamma
32) What color of visible light has the highest energy?
A) violet
B) blue
C) red
D) green
E) yellow
33) Using Bohr’s equation for the energy levels of the electron in the hydrogen atom, determine the
energy (J) of an electron in the n = 4 level.
A) -1.36 × 10–19
B) -5.45 × 10–19
C) -7.34 × 1018
D) -1.84 × 10–29
E) +1.84 × 10–29
34) An electron in a Bohr hydrogen atom has an energy of -1.362 × 10–19 J. The value of n for this electron
is ________.
A) 1
B) 2
C) 3
D) 4
E) 5
35) The energy (J) required for an electronic transition in a Bohr hydrogen atom from n = 2 to n = 3 is
________ J.
A) 4.00 × 10–19
B) 3.00 × 10–19
C) -3.00 × 10–19
D) -7.90 × 10–19
E) 4.60 × 1014
36) The energy (J) required for an electronic transition in a Bohr hydrogen atom from n = 1 to n = 3 is
________ J.
A) -8.90 × 10-1
B) 3.00 × 10–19
C) -3.00 × 10–19
D) 1.94 × 10–18
E) 8.90 × 10-1
28
37) Calculate the energy (J) change associated with an electron transition from n = 2 to n = 5 in a Bohr
hydrogen atom.
A) 6.5 × 10–19 J
B) 5.5 × 10–19 J
C) 8.7 × 10–20 J
D) 4.9 × 10–19 J
E) 5.8 × 10–53 J
38) The frequency of electromagnetic radiation required to promote an electron from n = 2 to n = 4 in a
Bohr hydrogen atom is ________ Hz.
A) 4.13 × 10–19
B) 6.17 × 1014
C) 5.46 × 10–19
D) 8.22 × 1014
E) 4.13 × 1019
39) A spectrum containing only specific wavelengths is called a(n) ________ spectrum.
A) line
B) continuous
C) visible
D) Rydberg
E) invariant
40) When the electron in a hydrogen atom moves from n = 6 to n = 1, light with a wavelength of ________
nm is emitted.
A) 487
B) 411
C) 434
D) 93.8
E) 657
41) When the electron in a hydrogen atom moves from n = 8 to n = 2 light with a wavelength of ________
29
nm is emitted.
A) 657
B) 93.8
C) 411
D) 487
E) 389
42) The n = 2 to n = 6 transition in the Bohr hydrogen atom corresponds to the ________ of a photon with
a wavelength of ________ nm.
A) emission, 410
B) absorption, 410
C) absorption, 660
D) emission, 94
E) emission, 390
43) The n = 5 to n = 3 transition in the Bohr hydrogen atom corresponds to the ________ of a photon with
a wavelength of ________ nm.
A) absorption, 657
B) absorption, 1280
C) emission, 657
D) emission, 1280
E) emission, 389
44) The n = 8 to n = 4 transition in the Bohr hydrogen atom occurs in the ________ region of the
electromagnetic spectrum.
A) infrared
B) visible
C) ultraviolet
D) microwave
E) X-ray
45) The n = 8 to n = 2 transition in the Bohr hydrogen atom occurs in the ________ region of the
electromagnetic spectrum.
A) radio
B) X-ray
C) infrared
D) microwave
E) ultraviolet
46) The de Broglie wavelength of a particle is given by ________.
A) h + mv
B) hmv
C) h/mv
D) mv/c
E) mv
47) What is the de Broglie wavelength (m) of a 2.0-kg object moving at a speed of 50 m/s?
A) 6.6 × 10–36 m
B) 1.5 × 1035 m
C) 5.3 × 10–33 m
D) 2.6 × 10–35 m
E) 3.8 × 1034 m
48) What is the de Broglie wavelength (m) of a 25-g object moving at a speed of 5.0 m/s?
A) 1.9 × 1032 m
B) 5.3 × 10–33 m
C) 6.6 × 10–36 m
D) 3.32 × 10–36 m
E) 3.02 × 1045 m
49) What is the de Broglie wavelength (m) of a 15-g object moving at a speed of 3.0 m/s?
A) 1.9 × 1032 m
B) 5.3 × 10–33 m
C) 1.9 × 10–36 m
D) 1.5 × 10–32 m
E) 3.0 × 1045 m
50) At what speed (m/s) must a 10.0-mg object be moving to have a de Broglie wavelength of
3.3 × 10–41 m?
A) 4.1 m/s
B) 1.9 × 10–11 m/s
C) 2.0 × 1012 m/s
D) 3.3 × 10–42 m/s
E) 1.9 × 1013 m/s
51) At what speed (m/s) must a 3.0-mg object be moving in order to have a de Broglie wavelength of
5.4 × 10–29 m?
A) 1.6 × 10–28 m/s
B) 3.9 × 10-4 m/s
C) 2.0 × 1012 m/s
D) 4.1 m/s
E) 6.3 m/s
52) The de Broglie wavelength of an electron is 8.7 × 10–11 m. The mass of an electron is 9.1 × 10–31 kg.
The velocity of this electron is ________ m/s.
A) 8.4 × 103
B) 1.2 × 10-7
C) 6.9 × 10–5
D) 8.4 × 106
E) 8.4 × 10-3
53) The de Broglie wavelength of a bullet (7.5 g) traveling at 700 m/s is ________ m.
A) 7.7 × 1033
B) 1.3 × 10–34
C) 6.2 × 10–29
D) 1.3 × 10–27
E) 1.3 × 10–23
54) The de Broglie wavelength of a car (1.0 × 103 kg) traveling at 75 km/hr is ________ m.
A) 3.2 × 10–38
B) 8.8 × 10–39
C) 3.2 × 10–35
D) 1.4 × 10–35
E) 1.4 × 1035
55) The wavelength of an electron whose velocity is 1.7 × 104 m/s and whose mass is 9.1 × 10–28 g is
________ m.
A) 4.3 × 10–11
B) 12
C) 4.3 × 10–8
D) 2.3 × 107
E) 2.3 × 10-7
56) The ________ quantum number defines the shape of an orbital.
A) spin
B) magnetic
C) principal
D) angular momentum
E) psi
57) There are ________ orbitals in the third shell.
A) 25
B) 4
C) 9
D) 16
E) 1
58) The ________ subshell contains only one orbital.
A) 5d
B) 6f
C) 4s
D) 3d
E) 1p
59) There are ________ orbitals in the second shell.
A) 1
B) 2
C) 4
D) 8
E) 9
60) The angular momentum quantum number is 3 in ________ orbitals.
A) s
B) p
C) d
D) f
E) a
61) The n = 1 shell contains ________ p orbitals. All the other shells contain ________ p orbitals.
A) 3, 6
B) 0, 3
C) 6, 2
D) 3, 3
E) 0, 6
62) The lowest energy shell that contains f orbitals is the shell with n = ________.
A) 3
B) 2
C) 4
D) 1
E) 5
63) The principal quantum number of the first d subshell is ________.
A) 1
B) 2
C) 3
D) 4
E) 0
64) The total number of orbitals in a shell is given by ________.
A) I2
B) n2
C) 2n
D) 2n + 1
E) 2l + 1
65) In a hydrogen atom, an electron in a ________ orbital can absorb a photon, but cannot emit a photon.
A) 3s
B) 2s
C) 3p
D) 1s
E) 3f
66) ________-orbitals are spherically symmetrical.
A) s
B) p
C) d
D) f
E) g
67) Each p-subshell can accommodate a maximum of ________ electrons.
A) 6
B) 2
C) 10
D) 3
E) 5
68) Each d-subshell can accommodate a maximum of ________ electrons.
A) 6
B) 2
C) 10
D) 3
E) 5
69) How many quantum numbers are necessary to designate a particular electron in an atom?
A) 3
B) 4
C) 2
D) 1
E) 5
70) A ________ orbital is degenerate with a 5dz2 in a many-electron atom.
A) 5pz
B) 4dz2
C) 5s
D) 5dxy
E) 4dzz
71) The 3p subshell in the ground state of atomic xenon contains ________ electrons.
A) 2
B) 6
C) 8
D) 10
E) 36