Chemistry: The Central Science, 12e (Brown et al.)
Chapter 6 Electronic Structure of Atoms
6.1 Multiple–Choice Questions
1) Which one of the following is correct?
A) ν + λ = c
B) ν ÷ λ = c
C) ν = cλ
D) λ = c ν
E) νλ = c
2) The wavelength of light emitted from a traffic light having a frequency of 5.75 × 1014 Hz is
__________.
A) 702 nm
B) 641 nm
C) 674 nm
D) 522 nm
E) 583 nm
3) Of the following, __________ radiation has the shortest wavelength.
A) X-ray
B) radio
C) microwave
D) ultraviolet
E) infrared
4) The photoelectric effect is __________.
A) the total reflection of light by metals giving them their typical luster
B) the production of current by silicon solar cells when exposed to sunlight
C) the ejection of electrons by a metal when struck with light of sufficient energy
D) the darkening of photographic film when exposed to an electric field
E) a relativistic effect
5) Which one of the following is considered to be ionizing radiation?
A) visible light
B) radio waves
C) X-rays
D) microwaves
E) infrared radiation
6) Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the
emission of the highest-energy photon.
A) n = 1 → n = 6
B) n = 6 → n = 1
C) n = 6 → n = 3
D) n = 3 → n = 6
E) n = 1 → n = 4
7) Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the
emission of the lowest-energy photon.
A) n = 1 → n = 6
B) n = 6 → n = 1
C) n = 6 → n = 3
D) n = 3 → n = 6
E) n = 1 → n = 4
8) In the Bohr model of the atom, __________.
A) electrons travel in circular paths called orbitals
B) electrons can have any energy
C) electron energies are quantized
D) electron paths are controlled by probability
E) both A and C
9) The de Broglie wavelength of a 6.0 gram bullet traveling at the speed of sound is __________. The
speed of sound is 331 m/sec.
A) 2.7 × 10-34 m
B) 3.3 × 10-34 m
C) 3.35 × 10-33 m
D) 2.7 × 10-37 m
E) 6.6 × 10-31 m
10) According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the
position and the __________ of an electron.
A) mass
B) color
C) momentum
D) shape
E) charge
11) All of the orbitals in a given electron shell have the same value of the __________ quantum number.
A) principal
B) angular momentum
C) magnetic
D) spin
E) psi
12) The de Broglie wavelength of a __________ will have the shortest wavelength when traveling at 30
cm/s.
A) marble
B) car
C) planet
D) uranium atom
E) hydrogen atom
13) The uncertainty principle states that __________.
A) matter and energy are really the same thing
B) it is impossible to know anything with certainty
C) it is impossible to know the exact position and momentum of an electron
D) there can only be one uncertain digit in a reported number
E) it is impossible to know how many electrons there are in an atom
14) All of the orbitals in a given subshell have the same value of the __________ quantum number.
A) principal
B) angular momentum
C) magnetic
D) A and B
E) B and C
15) Which one of the following is not a valid value for the magnetic quantum number of an electron in a
5d subshell?
A) 2
B) 3
C) 0
D) 1
E) -1
16) Which of the subshells below do not exist due to the constraints upon the angular momentum
quantum number?
A) 2d
B) 2s
C) 2p
D) all of the above
E) none of the above
17) Which of the subshells below do not exist due to the constraints upon the angular momentum
quantum number?
A) 4f
B) 4d
C) 4p
D) 4s
E) none of the above
18) An electron cannot have the quantum numbers n = __________, l = __________, ml = __________.
A) 2, 0, 0
B) 2, 1, -1
C) 3, 1, -1
D) 1, 1, 1
E) 3, 2, 1
19) An electron cannot have the quantum numbers n = __________, l = __________, ml = __________.
A) 6, 1, 0
B) 3, 2, 3
C) 3, 2, -2
D) 1, 0, 0
E) 3, 2, 1
20) Which one of the following is an incorrect subshell notation?
A) 4f
B) 2d
C) 3s
D) 2p
E) 3d
21) Which one of the following is an incorrect orbital notation?
A) 2s
B) 3py
C) 3f
D) 4dxy
E) 4s
22) Which quantum number determines the energy of an electron in a hydrogen atom?
A) n
B) E
C) ml
D) l
E) n and l
23) Which one of the quantum numbers does not result from the solution of the Schrodinger equation?
A) principal
B) azimuthal
C) magnetic
D) spin
E) angular momentum
24) Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a
one-electron system (such as hydrogen)?
A) n, l, and ml
B) n and l only
C) l and ml
D) ml only
E) n only
25) In a px orbital, the subscript x denotes the __________ of the electron.
A) energy
B) spin of the electrons
C) probability of the shell
D) size of the orbital
E) axis along which the orbital is aligned
26) The __________ orbital is degenerate with 5py in a many-electron atom.
A) 5s
B) 5px
C) 4py
D) 5dxy
E) 5d2
27) At maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________
electrons, and a p-subshell can hold __________ electrons.
A) 14, 10, 6
B) 2, 8, 18
C) 14, 8, 2
D) 2, 12, 21
E) 2, 6, 10
28) If an electron has a principal quantum number (n) of 3 and an angular momentum quantum number
(l) of 2, the subshell designation is __________.
A) 3p
B) 3d
C) 4s
D) 4p
E) 4d
29) Which one of the following represents an acceptable set of quantum numbers for an electron in an
atom? (arranged as n, l, ml, and ms)
A) 2, 2, -1, -1/2
B) 1, 0, 0, 1/2
C) 3, 3, 3, 1/2
D) 5, 4,- 5, 1/2
E) 3, 3, 3, -1/2
30) Which one of the following represents an acceptable possible set of quantum numbers (in the order
n, l, ml, ms) for an electron in an atom?
A) 2, 1, -1, 1/2
B) 2, 1, 0, 0
C) 2, 2, 0, 1/2
D) 2, 0, 1, -1/2
E) 2, 0, 2, +1/2
31) Which one of the following orbitals can hold two electrons?
A) 2px
B) 3s
C) 4dxy
D) all of the above
E) none of the above
32) Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a
many-electron system?
A) n, l, and ml
B) n only
C) n, l, ml, and ms
D) ms only
E) n and l only
33) Which one of the following represents an impossible set of quantum numbers for an electron in an
atom? (arranged as n, l, ml, and ms)
A) 2, 1, -1, -1/2
B) 1, 0, 0, 1/2
C) 3, 3, 3, 1/2
D) 5, 4, – 3, 1/2
E) 5, 4, -3, -1/2
34) Which of the following is not a valid set of four quantum numbers? (n, l, ml, ms)
A) 2, 0, 0, +1/2
B) 2, 1, 0, -1/2
C) 3, 1, -1, -1/2
D) 1, 0, 0, +1/2
E) 1, 1, 0, +1/2
35) Which of the following is a valid set of four quantum numbers? (n, l, ml, ms)
A) 2, 1, 0, +1/2
B) 2, 2, 1, -1/2
C) 1, 0, 1, +1/2
D) 2, 1, +2, +1/2
E) 1, 1, 0, -1/2
36) Which electron configuration represents a violation of the Pauli exclusion principle?
A)
B)
C)
D)
E)
37) Which electron configuration represents a violation of the Pauli exclusion principle?
A)
B)
C)
D)
E)
38) Which electron configuration represents a violation of the Pauli exclusion principle?
A)
B)
C)
D)
E)
39) Which one of the following is the correct electron configuration for a ground-state nitrogen atom?
A)
B)
C)
D)
E) None of the above is correct.
40) Which electron configuration denotes an atom in its ground state?
A)
B)
C)
D)
E)
41) The ground state electron configuration of Fe is __________.
A) 1s22s23s23p63d6
B) 1s22s22p63s23p64s23d6
C) 1s22s22p63s23p64s2
D) 1a22s22p63s23p64s24d6
E) 1s22s23s23p10
42) The ground state electron configuration of Ga is __________.
A) 1s22s23s23p64s23d104p1
B) 1s22s22p63s23p64s24d104p1
C) 1s22s22p63s23p64s23d104p1
D) 1s22s22p63s23p64s23d104d1
E) [Ar]4s23d11
43) The ground-state electron configuration of the element __________ is [Kr]5s14d5.
A) Nb
B) Mo
C) Cr
D) Mn
E) Tc
44) The ground-state electron configuration of __________ is [Ar]4s13d5.
A) V
B) Mn
C) Fe
D) Cr
E) K
45) Which one of the following configurations depicts an excited oxygen atom?
A) 1s22s22p2
B) 1s22s22p23s2
C) 1s22s22p1
D) 1s22s22p4
E) [He]2s22p4
46) Which one of the following configurations depicts an excited carbon atom?
A) 1s22s22p13s1
B) 1s22s22p3
C) 1s22s22p1
D) 1s22s23s1
E) 1s22s22p2
47) Which electron configuration represents a violation of Hund’s rule for an atom in its ground state?
A)
B)
C)
D)
E)
48) Which electron configuration represents a violation of Hund’s rule for an atom in its ground state?
A)
B)
C)
D)
E)
49) Which electron configuration represents a violation of Hund’s rule for an atom in its ground state?
A)
B)
C)
D)
E)
50) The ground state configuration of fluorine is __________.
A) [He]2s22p2
B) [He]2s22p3
C) [He]2s22p4
D) [He]2s22p5
E) [He]2s22p6
51) The ground state configuration of tungsten is __________.
A) [Ar]4s23d3
B) [Xe]6s24f145d4
C) [Ne]3s1
D) [Xe]6s24f7
E) [Kr]5s24d105p5
52) The lowest orbital energy is reached when the number of electrons with the same spin is maximized.
This statement describes __________.
A) Pauli Exclusion Principle
B) Planck’s constant
C) deBroglie hypothesis
D) Heisenberg Uncertainty Principle
E) Hund’s rule
53) The element that has a valence configuration of 4s1 is __________.
A) Li
B) Na
C) K
D) Rb
E) Cs
54) Which of the following elements has a ground-state electron configuration different from the
predicted one?
A) Cu
B) Ca
C) Xe
D) Cl
E) Ti
55) Which two elements have the same ground-state electron configuration?
A) Pd and Pt
B) Cu and Ag
C) Fe and Cu
D) Cl and Ar
E) No two elements have the same ground-state electron configuration.
56) How many different principal quantum numbers can be found in the ground state electron
configuration of nickel?
A) 2
B) 3
C) 4
D) 5
E) 6
57) The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X
has a partially filled 4d subshell. What type of element is X?
A) main group element
B) chalcogen
C) halogen
D) transition metal
E) alkali metal
6.2 Bimodal Questions
1) Electromagnetic radiation travels through vacuum at a speed of __________ m/s.
A) 186,000
B) 125
C) 3.00 × 108
D) 10,000
E) It depends on wavelength.
2) The wavelength of light that has a frequency of 1.20 ×1013s-1 is __________ m.
A) 25.0
B) 2.50 × 10-5
C) 0.0400
D) 12.0
E) 2.5
3) The wavelength of light that has a frequency of 1.66 × 109s-1 is __________ m.
A) 0.181
B) 5.53
C) 2.00 x 10-9
D) 5.53 x 108
E) none of the above
4) Ham radio operators often broadcast on the 6-meter band. The frequency of this electromagnetic
radiation is __________ MHz.
A) 500
B) 200
C) 50
D) 20
E) 2.0
5) What is the frequency (s-1) of electromagnetic radiation that has a wavelength of 0.53 m?
A) 5.7 × 108
B) 1.8 × 10-9
C) 1.6 × 108
D) 1.3 × 10-33
E) 1.3 × 1033
6) What is the frequency (s-1) of electromagnetic radiation that has a wavelength of 2.3 m?
A) 1.3 × 108
B) 1.8 × 10-9
C) 1.6 × 108
D) 1.3 × 10-33
E) 1.3 × 1033
7) What is the frequency of light (s-1) that has a wavelength of 1.23 × 10-6 cm?
A) 3.69
B) 2.44 × 1016
C) 4.10 × 10-17
D) 9.62 × 1012
E) 1.04 × 10-13
8) What is the frequency of light (s-1) that has a wavelength of 3.86 × 10-5 cm?
A) 7.77 × 1014
B) 6.32 × 10-12
C) 1.04 × 10-13
D) 9.62 × 1012
E) 2.14 × 10-16
9) What is the frequency of light (s-1) that has a wavelength of 3.12 × 10-3 cm?
A) 3.69
B) 2.44 × 1016
C) 9.62 × 1012
D) 4.10 × 10-17
E) 1.04 × 10-13
10) What is the wavelength of light (nm) that has a frequency of 3.22 × 1014 s-1?
A) 932
B) 649
C) 9.66 × 1022
D) 9.32 × 10-7
E) 1.07 × 106
11) What is the wavelength of light (nm) that has a frequency of 6.44 × 1013 s-1?
A) 4660
B) 6490
C) 4.66 × 10-8
D) 6.49 × 10-8
E) 932
12) What is the wavelength of light (nm) that has a frequency 4.62 × 1014 s-1?
A) 932
B) 649
C) 1.39 × 1023
D) 1.54 × 10-3
E) 1.07 × 106
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