4) 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
5) Of the following, which has the shortest de Broglie wavelength?
A) an airplane moving at a velocity of 350 mph
B) a helium nucleus moving at a velocity of 800 mph
C) a nitrogen molecule moving at a velocity of 900 mph
D) a nitrogen molecule moving at a velocity of 5000 mph
6) What is the de Broglie wavelength of a 300. g object moving at a velocity of 25.0 m/s (about 100 mph)?
A) 8.84 × 10–41 m
B) 8.84 × 10–35 m
C) 8.84 × 106 m
D) 8.84 × 1012 m
7) What are the possible values of n and ml for an electron in a 3d orbital?
A) n = 1, 2, or 3 and ml = 2
B) n = 1, 2, or 3 and ml = -2, -1, 0, +1, or +2
C) n = 3 and ml = 2
D) n = 3 and ml = -2, -1, 0, +1, or +2
8) How many subshells are there in the shell with n = 4?
A) 3
B) 4
C) 6
D) 18
9) What are the possible values of l if n = 3?
A) 3
B) 0, 1, or 2
C) -4, -3, -2, -1, 0, +1, +2, +3, or +4
D) -5, -4, –3, -2, -1, 0, +1, +2, +3, +4, or +5
10) How many orbitals are there in the sixth shell?
A) 5
B) 6
C) 15
D) 36
11) 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
12) For a hydrogen atom, which electronic transition would result in the emission of a photon with the
highest energy?
A) 2s → 5p
B) 3p → 5d
C) 4p → 2s
D) 5f → 4d
13) Which orbitals do not have a node at the nucleus?
A) all beyond the second shell
B) s and d
C) d
D) s
14) What is the number of spherical nodes in a 6s orbital?
A) zero
B) six
C) five
D) seven
15) For a particular orbital, as one goes away from the nucleus along the z-axis, the probability density
decreases to zero, then increases, and finally decreases without increasing a second time. This is
consistent with a
A) 2s orbital.
B) 4px orbital.
C) 3f orbital.
D) 4s orbital.
16) Which of the following is not a valid set of quantum numbers?
A) n = 2, l = 1, ml = 0, and ms = +1/2
B) n = 2, l = 1, ml = -1, and ms = +1/2
C) n = 3, l = 0, ml = 0, and ms = +1/2
D) n = 3, l = 2, ml = 3, and ms = +1/2
17) An electron in a 4p orbital can have a wave function with which of the following set of quantum
numbers, (n, l, ml, ms)?
A) (4, 3, -1, 1/2)
B) (4, 1, -1, –1/2)
C) (5, 0, 1, -1/2)
D) (5, 1, 4, 1/2)
18) Which of the following represent electron configurations that violate the Pauli exclusion principle?
(A) [Ne]3s13p5 (B) [Kr]4d125s25p6 (C) [Ar]3d104s24p2
A) only (A)
B) only (B)
C) (A) and (B)
D) (B) and (C)
19) How many unpaired electrons are there in the ground state of element N?
A) 1
B) 2
C) 3
D) 4
40
20) Which has the highest Zeff for its valence electrons?
A) Cs
B) W
C) Pb
D) At
21) Which of the following represent electron configurations that are allowed but do not represent
ground-state configurations?
(A) [Ne]3s13p5 (B) [Kr]4d125s25p5 (C) [Ar]3d104s24p2
A) only (A)
B) only (B)
C) (A) and (B)
D) (B) and (C)
22) Which of the following elements would you predict to have an anomalous electron configuration?
A) W
B) Mg
C) Al
D) Sb
23) What is the ground-state electron configuration of V?
A) [Ar]3d5
B) [Ar]4s13d4
C) [Ar]4s23d3
D) [Ar]4s24p64d1
24) How many unpaired electrons are in an atom of Mt in its ground state?
A) 1
B) 2
C) 3
D) 5
25) Which have the largest number of unpaired electrons in p orbitals in their ground-state electron
configurations?
A) N, As, Bi
B) F, At, Br
C) Ne, Ar, Xe
D) B, Ga, Tl
26) Which of the following does not have their valence electrons in the same shell?
A) S
B) Ga
C) Br
D) As
27) Which of the following does not have the same number of valence electrons?
A) O
B) S
C) Ca
D) Po
28) The element Bh has how many valence electrons?
A) 2
B) 5
C) 7
D) 1
29) The element Ga has how many valence electrons?
A) 1
B) 2
C) 3
D) 4
30) Which of the following have their valence electrons in the same shell?
A) Rb, Sb, I
B) Ga, Sn, Bi
C) As, Sb, Bi
D) Ar, Kr, Br
31) Which of the following have the same number of valence electrons?
A) Cs, Bi, At
B) In, Pb, Bi
C) N, P, As
D) Xe, Rn, At
32) What is the general valence-electron ground-state electron configuration for neutral alkaline earth
metals?
A) ns1
B) ns2
C) 1s22s22p4
D) 1s22s2
33) Which element has the ground-state electron configuration [Xe]6s2 4?
A) Re
B) Ir
C) Eu
D) Gd
34) How many valence electrons does a neutral polonium atom have?
A) 2
B) 4
C) 6
D) 84
35) A neutral N atom has how many valence electrons?
A) 1
B) 3
C) 6
D) 14
36) Of the following, which atom has the largest atomic radius?
A) Na
B) Cl
C) K
D) Br
37) Of the following, which atom has the largest atomic radius?
A) V
B) Ni
C) Sc
D) Br
38) Of the following, which atom has the smallest atomic radius?
A) K
B) As
C) Rb
D) Sb
39) Of the following, which atom has the smallest atomic radius?
A) Ca
B) As
C) Mn
D) Ni
40) Which atom in each group (I and II) has the smallest atomic radius?
(I) K, Zn, Br (II) Al, Ga, In
A) K; Al
B) K; In
C) Br; Al
D) Br; In
41) Which atom in each group (I and II) has the smallest atomic radius?
(I)Rb, Zr, I (II)Sb, N, As
A) Rb; Sb
B) Rb; As
C) Te; Sb
D) Te; As
5.3 Short Answer Questions
1) Compared to ultraviolet radiation, infrared radiation occurs at ________ wavelengths, ________
frequencies, and ________ energies.
2) The visible region of the electromagnetic radiation spectrum extends from ________ nm to ________
nm.
3) The highest note on a piano has a frequency of 4186 Hz. In a vacuum 4186 Hz has a corresponding
wavelength of ________ m.
4) The property of a wave that is associated with brightness or intensity is ________.
5) A radio station that broadcasts at 99.1 MHz is broadcasting at a frequency of ________ s–1.
6) The amount of data that can be stored in an optical disc storage medium is related to the wavelength of
the laser employed. Blu-Ray discs that are read by a laser having a wavelength of 405 nm have a much
greater storage capacity than a DVD that is read by a 650 nm laser. The color of the 405 nm laser beam is
________, whereas the color of the 650 nm laser is ________.
7) Light behaves as if it were a stream of small particles, called ________, each having an amount of
energy called a ________.
8) The average bond dissociation energy of a carbon-carbon bond is 410 kJ/mol. What wavelength in
nanometers of ultraviolet radiation has an energy of 410 kJ/mol?
9) The laser used to read Blu-Ray discs have a wavelength of 405 nm. 405 nm photons have of an energy
of ________ J, and a mole of 405 nm photons has an energy of ________ kJ/mol.
10) The smallest number that can be used for m or n in the Balmer-Rydberg equation is ________ and the
largest number is ________.
11) According to the Balmer-Rydberg equation, transitions from n = 5 to m = 2 result in a photons of light
that give rise to a spectral line with what color?
12) What is the deBroglie wavelength in meters of a 1-ton (907 kg) vehicle having a velocity of 95 km/hr?
13) A solution to the Schrödinger wave equation is a ________, or orbital, represented by the symbol Ψ,
and the probability of finding an electron defined by Ψ within a given volume of space around the
nucleus is ________.
14) The energy of an electron in a multielectron atom depends on the quantum numbers ________ and
________.
48
15) An orbital with n = 5 and l = 2 is a ________ orbital.
16) The number of orbitals having the quantum numbers, n = 5 and l = 3 is ________.
17) The number of orbitals in the n = 3 shell is ________.
18) According to the Bohr model of the atom, when an electron goes from a higher–energy orbit to a
lower-energy orbit, it ________ electromagnetic energy with an energy that is equal to the ________
between the two orbits.
19) In a representation of an orbital, a region having zero probability of finding an electron is called a
________.
20) The algebraic signs (+ and -) sometimes written within the lobes of orbitals are analogous to different
________ of a wave.
21) An orbital that as the appearance of a three-dimensional clover leaf has a quantum number l =
________.
22) Copper has the anomalous electron configuration ________.
23) Using shorthand notation, the electron configuration of Ni is ________.
24) The ground-state electron configuration of the C4-, is the same as which noble gas?
25) Compared to Si , Cl has a ________ effective nuclear charge, Zeff, and a ________ atomic radius.