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
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]4d24d9
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 nsl.
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 ns2npl?
A) 1A
B) 2A
C) 3A
D) 4A
E) 8A
6.3 Algorithmic Questions
1) Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The
frequency of this light is __________ sl.
A) 5.71 × 1014
B) 5.71 × 105
C) 1.58 × 102
D) 1.58 × 1011
E) 1.75 × 10-15
2) An FM radio station broadcasts electromagnetic radiation at a frequency of 100.6 MHz. The
wavelength of this radiation is __________ m.
A) 2.982 × 106
B) 2.982
C) 3.018 × 1016
D) 3.018 × 1010
E) 0.3353
3) 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 × 10-28
C) 3.79 × 10-19
D) 1.04 × 10-22
E) 2.64 × 1018
4) 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 × 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) 2.9 × 10-17
B) 9.2 × 10-24
C) 1.8 × 1019
D) 3.5 × 1016
E) 6.5 × 1013
5) It takes 261 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) 458
B) 233
C) 165
D) 725
E) 552
6) A radio station broadcasts at 105.2 MHz. The wavelength of the signal is __________ m.
A) 3.10
B) 2.85
C) 2.90
D) 3.02
E) 3.84
7) When the electron in a hydrogen atom moves from n = 4 to n = 2, light with a wavelength of
__________ nm is emitted.
A) 93.8
B) 434
C) 410
D) 657
E) 486
8) The de Broglie wavelength of an electron with a velocity of 6.00 × 106 m/s is __________ m. The
mass of the electron is 9.11 × 10-28 g.
A) 8.25 × 109
B) 8.25 × 1012
C) 1.21 × 10-16
D) 1.21 × 10-13
E) 1.21 × 10-10
9) Which set of three quantum numbers (n, l, ml) corresponds to a 3p orbital?
A) 3,0,1
B) 3,0,0
C) 3,1,0
D) 3,2,0
E) 3,3,1
10) How many p-orbitals are occupied in a B atom?
A) 5
B) 6
C) 0
D) 1
E) 3
11) The element that corresponds to the electron configuration 1s22s22p6 is __________.
A) sodium
B) magnesium
C) lithium
D) beryllium
E) neon
12) There are __________ unpaired electrons in a ground state nitrogen atom.
A) 0
B) 1
C) 2
D) 3
E) 4
13) The complete electron configuration of argon, element 18, is __________.
A) 1s22s22p63s23p6
B) 1s22s2p103s23p2
C) 1s42s42p63s4
D) 1s42s42p10
E) 1s62s62p23s4
14) The complete electron configuration of gallium, element 31, is __________.
A) 1s22s22p103s23p104s23d3
B) 1s22s22p63s23p63d104s24p1
C) 1s42s42p63s43p64s43d3
D) 1s42s42p103s43p9
E) 1s42s42p83s43p84s3
15) In a ground-state silver atoms, the __________ subshell is partially filled.
A) 3d
B) 3s
C) 4s
D) 4d
E) 4p
16) The principal quantum number for the outermost electrons in a Ca atom in the ground state is
__________.
A) 2
B) 3
C) 4
D) 5
E) 6
17) The angular momentum quantum number for the outermost electrons in a boron atom in the ground
state is __________.
A) 0
B) 1
C) 2
D) 3
E) -1
18) The condensed electron configuration of silicon, element 14, is __________.
A) [He]2s42p6
B) [Ne]2p10
C) [Ne]3s23p2
D) [He]2s4
E) [He]2s62p2
19) The condensed electron configuration of krypton, element 36, is __________.
A) [Kr]4s23d8
B) [Ar]4s4
C) [Kr]4s43d8
D) [Ar]3d104s24p6
E) [Ar]4s43d4
20) The largest principal quantum number in the ground state electron configuration of cobalt is
__________.
A) 2
B) 3
C) 4
D) 7
E) 9
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 __________.
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 a 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) Black body 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.