67) Niels Bohr promoted the connection between the periodic table and quantum theory. Which of the
following statements is INCORRECT?
A) The link between the table arrangement and quantum theory is electron configuration.
B) Elements in the same group have similar electron configurations.
C) Elements in the same group have the same number of electrons in the outer orbit.
D) Elements in the same group have the same principle quantum number.
E) Elements in the same group have the same number of valence electrons.
68) The fact that the valence orbital configuration of nitrogen in the ground state is 2s2, 2px12py12pz1 is
an illustration of:
A) the Bohr Theory
B) Hund’s Rule
C) the Aufbau Principle
D) the Pauli Exclusion Principle
E) the Heisenberg Uncertainty Principle
69) The quantum numbers of the last electron of arsenic could be:
A) n = 4, ℓ = 2, mℓ = 1, ms = +1/2
B) n = 4, ℓ = 1, mℓ = 1, ms = +1/2
C) n = 3, ℓ = 1, mℓ = 1, ms = +1/2
D) n = 4, ℓ = 3, mℓ = 1, ms = +1/2
E) n = 4, ℓ = 1, mℓ = 1/2, ms = 0
70) The quantum numbers of the last electron of nickel could be:
A) n = 3, ℓ = 2, mℓ = 0, ms = -1/2
B) n = 4, ℓ = 2, mℓ = 0, ms = +1/2
C) n = 3, ℓ = 1, mℓ = 0, ms = +1/2
D) n = 3, ℓ = 2, mℓ = 0, ms = 0
E) n = 3, ℓ = 2, mℓ = 1/2, ms = +1/2
71) Arrange the following in order of increasing ENERGY:
UV radiation, visible radiation, X-rays, and microwaves.
A) X-rays < microwave < UV < visible
B) X-ray < microwave < visible < UV
C) microwave < visible < UV < X-rays
D) visible < UV < X-rays < microwave
E) UV < X-rays < microwave < visible
72) A television signal has a wavelength of 10.0 km. What is its frequency in kilohertz?
A) 30.0 kHz
B) 3.00 × 104 kHz
C) 3.00 × 107 kHz
D) 3.33 × 10-7 kHz
E) 3.33 × 10-2 kHz
73) Use the Balmer equation to determine n for the spectral line of wavelength 656 nm. The constant for
Balmer’s equation is 3.2881 × 1015 s-1.
A) 3
B) 4
C) 5
D) 6
E) 7
74) Use the Balmer equation to determine n for the spectral line of wavelength 434 nm. The constant for
Balmer’s equation is 3.2881 × 1015 s-1.
A) 3
B) 4
C) 5
D) 6
E) 7
75) Use the Balmer equation to determine the wavelength, in nm, of the line in the Balmer series
corresponding to n = 4. The constant for Balmer’s equation is 3.2881 × 1015 s-1.
A) 365 nm
B) 45.6 nm
C) 205 nm
D) 486 nm
E) 1459 nm
76) What is the wavelength, in nm, of the spectral line resulting from the transition of an electron from n =
3 to n = 2 in a Bohr hydrogen atom? The constant for Balmer‘s equation is 3.2881 × 1015 s-1.
A) 18.3 nm
B) 656 nm
C) 547 nm
D) 152 nm
E) 252 nm
77) What is the wavelength of the line in the Balmer series of hydrogen corresponding to the transition
from n = 5 to n = 2? The constant for Balmer’s equation is 3.2881 × 1015 s-1.
A) 304 nm
B) 30.4 nm
C) 329 nm
D) 535 nm
E) 434 nm
78) Calculate the wavelength, in nm, of the first line of the Balmer series. The constant for Balmer’s
equation is 3.2881 × 1015 s-1.
A) 18.3 nm
B) 656 nm
C) 547 nm
D) 152 nm
E) 252 nm
79) What is the wavelength, in nm, of light with an energy content of 550 kJ/mol?
A) 0.218 nm
B) 0.419 nm
C) 157 nm
D) 218 nm
E) 6579 nm
80) Use Planck’s equation to determine the wavelength, in nm, of radiation with 200.0 kJ/mol of energy.
A) 167 nm
B) 598 nm
C) 5.98 × 105 nm
D) 1.67 × 105 nm
E) 242 nm
81) What is the energy in joules of a mole of photons with the energy of the 656 nm spectral line of
hydrogen?
A) 2.62 × 10–7 J
B) 78.3 J
C) 3.03 J
D) 8.73 × 10-25 J
E) 1.82 × 105 J
82) To what uncertainty, in pm, can the position of an electron traveling at 1.89 × 105 m/s be measured if
the uncertainty of the speed is 2.00%?
A) 765
B) 654
C) 8.33 × 104
D) 1.53 × 105
E) 1.53 × 104
83) What is the total number of orbitals possible for n = 3?
A) 9
B) 6
C) 5
D) 3
E) 11
84) Chlorine (atomic number = 17) has the electronic configuration: ________.
A) 1s22s22p63s23d5
B) 1s22s22p62d53s2
C) 1s22s22p63s23p5
D) 1s22s22d103s2
E) 1s22s22p62d63s1
85) The ground state electron configuration of Sc is ________.
A) 1s22s22p62d103s1
B) 1s21p62s22p63d5
C) 1s22s22p63s23p63d3
D) 1s22s22p63s23p64s23d1
E) 1s22s22p63s23p64s24p1
86) The ground state electron configuration of phosphorus is ________.
A) 1s22s22p43p63d1
B) [Ar] 3s23p3
C) 1s22s22p63s23p3
D) 1s22s22p63s43p1
E) 1s22s22p63s22d3
87) 1s22s22p63s23p64s23d3 is the ground state electronic configuration of ________.
A) scandium
B) niobium
C) chromium
D) vanadium
E) molybdenum
88) [Kr]5s24d105p5 is the ground state electronic configuration of ________.
A) Te
B) I
C) Br
D) At
E) S
89) Use the basic rules for electron configuration to indicate the number of unpaired electrons in
phosphorus.
A) 0
B) 1
C) 3
D) 5
E) 2
90) How many unpaired electrons are in the ground state electron configuration of chromium?
A) 5
B) 6
C) 4
D) 2
E) 0
91) How many unpaired electrons are in the ground state electron configuration of calcium?
A) 5
B) 2
C) 0
D) 1
E) 3
92) The correct electron configuration for is ________.
A) [Br] 3d104s24p6
B) [Ar] 3d104s24p6
C) [Br] 4s23d104p5
D) [Ar] 3d104s24p5
E) [Ne] 3d104s24p6
93) The ground state electron configuration for antimony is ________.
A) [Kr] 5s25d105p3
B) [Kr] 4s24d105p3
C) [Xe] 5s24d105p2
D) [Kr] 4d105s25p3
E) [Xe] 5s25d105p3
94) Use the spdf notation to write out the complete electron configuration of Br.
A) [Ar] 3d104s24p5
B) [Kr] 3d104s24p4
C) [Ar] 3d94s24p6
D) [Ar] 3d104p65s2
E) [Ar] 4s24p24d9
95) The four quantum numbers of the LAST electron to be placed into a Ca atom are ________.
A) n = 4, ℓ = 1, mℓ = 0, ms = -1/2
B) n = 3, ℓ = 0, mℓ = 1, ms = -1/2
C) n = 4, ℓ = 1, mℓ = 0, ms = +1/2
D) n = 4, ℓ = 0, mℓ = 0, ms = -1/2
E) n = 4, ℓ = 2, mℓ = 0, ms = +1/2
96) The quantum numbers of the last electron of cerium are ________.
A) n = 6, ℓ = 3, mℓ = -2, ms = +1/2
B) n = 5, ℓ = 3, mℓ = -2, ms = +1/2
C) n = 4, ℓ = 3, mℓ = -2, ms = +1/2
D) n = 4, ℓ = 2, mℓ = -2, ms = +1/2
E) n = 4, ℓ = 4, mℓ = -2, ms = +1/2
97) The quantum numbers of the last electron of cesium are ________.
A) n = 5, ℓ = 0, mℓ = 0, ms = +1/2
B) n = 6, ℓ = 1, mℓ = 0, ms = +1/2
C) n = 6, ℓ = 1, mℓ = 1, ms = +1/2
D) n = 6, ℓ = 0, mℓ = 0, ms = +1/2
E) n = 6, ℓ = 2, mℓ = 2, ms = +1/2
98) The quantum numbers of the last electron of silicon are ________.
A) n = 3, ℓ = 1, mℓ = 1, ms = 1
B) n = 2, ℓ = 1, mℓ = 1, ms = +1/2
C) n = 4, ℓ = 1, mℓ = 1, ms = +1/2
D) n = 3, ℓ = 1, mℓ = 0, ms = +1/2
E) n = 2, ℓ = 0, mℓ = 0, ms = +1/2
99) The quantum numbers of the last electron of barium are ________.
A) n = 6, ℓ = 0, mℓ = 1, ms = 1
B) n = 5, ℓ = 0, mℓ = 0, ms = +1/2
C) n = 6, ℓ = 0, mℓ = 1, ms = +1/2
D) n = 6, ℓ = 1, mℓ = 0, ms = +1/2
E) n = 6, ℓ = 0, mℓ = 0, ms = -1/2
100) Electromagnetic radiation with a wavelength of 640 nm appears as orange light to the human eye.
The frequency of this light is ________ .
A) 4.69 ×
B) 4.69 ×
C) 1.92 ×
D) 1.92 ×
E) 2.13 ×
101) An FM radio station broadcasts electromagnetic radiation at a frequency of 100.6 MHz. The
wavelength of this radiation is ________ m.
A) 2.982 ×
B) 2.982
C) 3.018 ×
D) 3.018 ×
E) 0.3353
102) Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The
energy of one photon of this light is ________ J.
A) 1.04 × 10–31
B) 3.79 ×
C) 3.79 ×
D) 1.04 × 10–22
E) 2.64 ×
103) Electromagnetic radiation with a wavelength of 531 nm appears as green light to the human eye. The
energy of one photon of this light is 3.74 × J. Thus, a laser that emits of energy in a pulse
of light at this wavelength produces ________ photons in each pulse.
A) 2.9 ×
B) 9.2 × 10–24
C) 1.8 ×
D) 3.5 ×
E) 6.5 ×
104) The de Broglie wavelength of an electron with a velocity of 6.00 × 106 m s-1 is ________ m. The mass
of the electron is 9.11 × g.
A) 8.25 × 109
B) 8.25 × 1012
C) 1.21 × 10–16
D) 1.21 × 10–13
E) 1.21 × 10–10
105) What are the possible values of n and ml for an electron in a 4p orbital?
A) n = 1, 2, 3, or 4 and ml = 1
B) n = 1, 2, 3, or 4 and ml = -2, -1, 0, +1, or +2
C) n = 4 and ml = 1
D) n = 4 and ml = –1, 0, +1
106) How many subshells are there in the shell with n = 4?
A) 3
B) 4
C) 6
D) 18
107) What are the possible values of l if n = 6?
A) 6
B) 0, 1, 2, 3, 4, or 5
C) -4, -3, -2, -1, 0, +1, +2, +3, or +4
D) -5, -4, -3, -2, -1, 0, +1, +2, +3, +4, or +5
108) How many orbitals are there in the fourth shell?
A) 3
B) 4
C) 6
D) 16
109) For a hydrogen atom, which electronic transition would result in the emission of a photon with the
highest energy?
A) 2s → 3p
B) 2p → 6d
C) 6p → 4s
D) 7f → 5d
110) For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d
orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1.
A) 656.3 nm
B) 486.2 nm
C) 364.6 nm
D) 2.057 × 10-3 nm
111) Which ion does not have a noble gas configuration in its ground electronic state?
A) Sc3+
B) Al3+
C) Ga3+
D) As3-
112) The element that corresponds to the electron configuration 1s22s22p3 is:
A) carbon
B) lithium
C) beryllium
D) boron
E) nitrogen
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113) The complete electron configuration of phosphorous, element 15, is:
A) 1s22s22p63s23p3
B) 2p103s1
C) 2p63s1
D) 2s42p7
E) 2s62p23s1
114) The complete electron configuration of nickel, element 28, is:
A) 3p12
B) 3d84s2
C) 3p84s2
D) 3s43p6
E) 3p8
115) The condensed electron configuration of sulfur, element 16, is:
A) [Ne]3s2
B) [Ar]3s2
C) [Ne]3s23p4
D) [He]2s42p8
E) [He]3s2
116) The condensed electron configuration of krypton, element 36, is:
A) [Kr]4s23d8
B) [Ar]4s4
C) [Kr]4s43d8
D) [Ar]3d104s24p6
E) [Ar]4s43d4
117) How many electrons are in the outermost shell of the Ga3+ ion in its ground state?
A) 2
B) 3
C) 6
D) 18
118) How many valence shell electrons does an atom of boron have?
A) 1
B) 2
C) 3
D) 5
E) 13
119) Which of the following have their valence electrons in the same shell?
A) Li, N, F
B) B, Si, As
C) N, As, Bi
D) He, Ne, F
120) Which of the following have the same number of valence electrons?
A) Rb, Sb, I
B) Ga, Sn, Bi
C) As, Sb, Bi
D) Ar, Kr, Br
121) What is the general valence-electron ground-state electron configuration for neutral alkaline earth
metals?
A) ns1
B) ns2
C) 1s22s1
D) 1s22s2
122) Which element has the ground-state electron configuration [Rn]7s2 6d 2?
A) Rf
B) Sg
C) Th
D) Pa
29
123) How many valence electrons does a neutral tellurium atom have?
A) 2
B) 4
C) 6
D) 52