72) The 3p subshell in the ground state of atomic silicon contains ________ electrons.
A) 2
B) 6
C) 8
D) 10
E) 36
73) The second shell in the ground state of atomic argon contains ________ electrons.
A) 2
B) 6
C) 8
D) 18
E) 36
74) The 4d subshell in the ground state of atomic xenon contains ________ electrons.
A) 2
B) 6
C) 8
D) 10
E) 36
75) [Ar]4s23d104p3 is the electron configuration of a(n) ________ atom.
A) As
B) V
C) P
D) Sb
E) Sn
76) [Ne]3s23p3 is the electron configuration of a(n) ________ atom.
A) As
B) V
C) P
D) Sb
E) Sn
77) There are ________ unpaired electrons in a ground state fluorine atom.
A) 0
B) 1
C) 2
D) 3
E) 4
78) The electron configuration of a ground-state Ag atom is ________.
A) [Ar]4s24d9
B) [Kr]5s14d10
C) [Kr]5s23d9
D) [Ar]4s14d10
E) [Kr]5s24d10
79) The ground-state electron configuration for Zn is ________.
A) [Kr]4s23d10
B) [Ar]4s23d10
C) [Ar]4s13d10
D) [Ar]3s23d10
E) [Kr]3s23d10
80) The correct ground-state electron configuration for silver is ________.
A) [Kr]5s24d9
B) [Kr]5s14d10
C) [Kr]5s24d10
D) [Xe]5s24d9
E) [Xe]5s14d10
81) The correct ground-state electron configuration for molybdenum is ________.
A) [Kr]5s14d10
B) [Kr]5s24d4
C) [Kr] 5s14d5
D) [Kr]5s24d5
E) [Kr]5s24d9
82) All of the ________ have a valence shell electron configuration ns1.
A) noble gases
B) halogens
C) chalcogens
D) alkali metals
E) alkaline earth metals
83) The elements in the ________ period of the periodic table have a core-electron configuration that is the
same as the electron configuration of neon.
A) first
B) second
C) third
D) fourth
E) fifth
84) Elements in group ________ have a np6 electron configuration in the outer shell.
A) 4A
B) 6A
C) 7A
D) 8A
E) 5A
85) Which group in the periodic table contains elements with the valence electron configuration of
ns2np1?
A) 1A
B) 2A
C) 3A
D) 4A
E) 8A
1) Electromagnetic radiation with a wavelength of 640 nm appears as orange light to the human eye. The
frequency of this light is ________ s-1.
A) 4.688 × 1014
B) 4.688 × 105
C) 1.920 × 102
D) 1.920 × 1011
E) 2.133 × 10–15
2) The wavelength of light emitted from a traffic light having a frequency of 2.74 × 1014 Hz is ________
nm.
A) 1090
B) 109
C) 54.7
D) 36.5
E) 50.0
3) An FM radio station broadcasts electromagnetic radiation at a frequency of 89.7 MHz. The wavelength
of this radiation is ________ m.
A) 3.34 × 106
B) 3.34
C) 2.69 × 1016
D) 2.69 × 1010
E) 0.299
4) Electromagnetic radiation with a wavelength of 425 nm appears as violet light to the human eye. The
energy of one photon of this light is ________ J.
A) 8.45 × 10–32
B) 4.68 × 10–28
C) 4.68 × 10–19
D) 8.45 × 10–23
E) 2.14 × 1018
5) Electromagnetic radiation with a wavelength of 641 nm appears as orange light to the human eye. The
energy of one photon of this light is 3.10 × 10–19 J. Thus, a laser that emits 1.3 × 10–2 J of energy in a pulse
of light at this wavelength produces ________ photons in each pulse.
A) 2.4 × 10–17
B) 6.3 × 10–24
C) 2.7 × 1019
D) 4.2 × 1016
E) 6.5 × 1013
6) It takes 258 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of
light (nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect?
A) 464
B) 233
C) 165
D) 725
E) 552
7) A radio station broadcasts at 99.5 MHz. The wavelength of the signal is ________ m.
A) 3.10
B) 3.02
C) 2.90
D) 2.75
E) 4.71
8) When the electron in a hydrogen atom moves from n = 5 to n = 2, light with a wavelength of ________
nm is emitted.
A) 93.8
B) 410
C) 487
D) 657
E) 434
9) Of the following transitions in the Bohr hydrogen atom, the ________ transition results in the emission
of the highest-energy photon.
A) n = 6 → n = 4
B) n = 2 → n = 7
C) n = 4 → n = 6
D) n = 1 → n = 4
E) All transitions emit photons of equivalent energy.
10) Of the following transitions in the Bohr hydrogen atom, the ________ transition results in the
absorption of the highest-energy photon.
A) n = 2 → n = 5
B) n = 4 → n = 2
C) n = 3 → n = 2
D) n = 5 → n = 2
E) All transitions absorb photons of equivalent energy.
11) The de Broglie wavelength of an electron with a velocity of 7.90 × 106 m/s is ________ m. The mass of
the electron is 9.11 × 10–28 g.
A) 1.09 × 1010
B) 1.09 × 1013
C) 9.21 × 10–17
D) 9.21 × 10–14
E) 9.21 × 10–11
12) The de Broglie wavelength of a 84.32 gram bullet traveling at the speed of 308.6 m/s is ________ m.
A) 2.546 × 10–35
B) 2.546 × 10–36
C) 2.546 × 10–37
D) 2.546 × 10–38
E) 1.724 × 10–32
13) The de Broglie wavelength of a 0.02900 gram bullet traveling at the speed of 647.4 m/s is ________ m.
A) 3.529 × 10–32
B) 3.529 × 10-33
C) 3.529 × 10–34
D) 3.529 × 10–35
E) 1.244 × 10–35
14) The symbol for the spin magnetic quantum number is ________.
A) ms
B) n
C) l
D) ml
E) sm
15) The angular momentum quantum number (l) value of 2 indicates the ________ subshell.
A) d
B) f
C) s
D) p
E) +1/2
16) At maximum, an d-subshell can hold ________ electrons.
A) 10
B) 6
C) 2
D) 8
E) 14
45
17) If an electron has a principal quantum number (n) of 7 and an angular momentum quantum number
(l) of 3, the subshell designation is ________.
A) 7f
B) 7s
C) 7p
D) 3f
E) 3d
18) 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) 3, 2, –2, -1/2
B) 3, 3, –4, 1/2
C) 3, 4, 6, –1/2
D) 3, 2, 0, 0
E) 3, 3, 3, –1/2
19) 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) 3, 0, 0, –1/2
B) 3, -1, -4, 1/2
C) 3, -3, 1, -1/2
D) 0, 2, 1, 0
E) 3, 3, 4, 3
20) 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) 4, 3, 0, 0
B) 4, 3, –3, 1/2
C) 4, 3, 3, –1/2
D) 4, 3, 0, +1/2
E) 4, 2, –2, -1/2
21) Which set of three quantum numbers (n, l, ml) corresponds to a 4s orbital?
A) 4,0,1
B) 4,0,2
C) 4,0,0
D) 4,1,0
E) 4,1,1
22) How many p-orbitals are occupied in a O atom?
A) 5
B) 6
C) 0
D) 3
E) 1
23) The element that corresponds to the electron configuration 1s22s22p2 is ________.
A) lithium
B) beryllium
C) boron
D) nitrogen
E) carbon
24) There are ________ unpaired electrons in a ground state chlorine atom.
A) 4
B) 3
C) 2
D) 1
E) 0
25) The ground-state electron configuration of V is ________.
A) 1s22s22p63s23p64s23d3
B) 1s22s22p63s23p63d5
C) 1s22s22p63s23p11
D) 1s22s22p63s23p64s23d4
E) None of the above
26) The complete electron configuration of sulfur, element 16, is ________.
A) 1s22s22p63s23p4
B) 1s22s22p103s2
C) 1s42s42p63s2
D) 1s42s42p8
E) 1s62s62p23s2
27) The complete electron configuration of vanadium, element 23, is ________.
A) 1s22s22p103s23p7
B) 1s22s22p63s23p63d34s2
C) 1s42s42p63s43p5
D) 1s42s42p103s43p1
E) 1s42s42p83s43p3
28) In a ground-state copper atom, the ________ subshell is partially filled.
A) 3s
B) 4s
C) 4p
D) 3d
E) 4d
29) The principal quantum number for the outermost electrons in a Te atom in the ground state is
________.
A) 3
B) 4
C) 5
D) 6
E) 7
30) The angular momentum quantum number for the outermost electrons in a manganese atom in the
ground state is ________.
A) 1
B) 2
C) 3
D) -1
E) 0
31) The condensed electron configuration of argon, element 18, is ________.
A) [Ne]3s4
B) [Ar]3s23p2
C) [Ne]3s23p6
D) [He]2s42p10
E) [He]3s4
32) The condensed electron configuration of titanium, element 22, is ________.
A) [Ar]3s23p6
B) [Ne]3s4
C) [Ar]3s43p4
D) [Ar]3d24s2
E) [Ne]3s43p2
33) The element that has a valence configuration of 2s2 is ________.
A) Be
B) Mg
C) Ca
D) Sr
E) Ba
34) The element that has a valence configuration of 5s25p6 is ________.
A) Xe
B) Rn
C) Ne
D) Ar
E) Kr
35) The element that has a valence configuration of 2s1 is ________.
A) Li
B) Na
C) K
D) Rb
E) Cs
36) The largest principal quantum number in the ground state electron configuration of barium is
________.
A) 1
B) 2
C) 6
D) 4
E) 5
6.4 Short Answer Questions
1) What wavelengths correspond to the visible region of the electromagnetic spectrum?
2) In the de Broglie formula describing the movement of an electron about the nucleus, the quantity “mv”
is called its ________.
3) A spectrum containing radiation of specific wavelengths is called a(n) ________.
4) The shape of an orbital is defined by the angular momentum quantum number which is represented as
letter ________.
5) All of the subshells in a given shell have the same energy in the hydrogen atom. In a many-electron
atom, the subshells in a given shell do not have the same energy. Why?
6) The largest principal quantum number in the ground state electron configuration of francium is
________.
7) The ground state electron configuration of scandium is ________.
8) The electron configuration of the valence electrons of an atom in its ground state is ns2np3. This atom
is a group ________ element.
9) Elements in group ________ have an np5 electron configuration in the outer shell.
10) The ground state electron configuration of copper is ________.
6.5 True/False Questions
1) The wavelength of radio waves can be longer than a football field.
2) Blackbody radiation is the emission of light from metal surfaces.
3) If a hydrogen atom electron jumps from the n=6 orbit to the n=2 orbit, energy is released.
4) The square of Schrodinger’s wave equation is called an orbital.
5) The electron density of the 2s orbital is asymmetric.
6) The larger the principal quantum number of an orbital, the lower is the energy of the electrons in that
orbital.
7) When the value of n is greater than or equal to 3, electrons can reside in d orbitals.
8) An NMR spectrum results from photon irradiation in which the nuclear spin alignment is flipped.