Chapter 7: Atomic Structure and Periodicity
Chapter 7: (2 points each)
1. In the following diagram of a wave
A)
B)
C)
(a) is amplitude and (b) is wavelength D)
(a) is frequency and (b) is amplitude E)
(a) is wavelength and (b) is frequency
(a) is amplitude and (b) is frequency
(a) is wavelength and (b) is amplitude
2. What is the wavelength of radiation that has a frequency of 5.39  1014 s–1? (c = 2.9979 
108 m/s)
A) 1.80  10–3 nm B) 556 nm C) 618 nm D) 6180 nm E) 1.61  1023 nm
3. Calculate the frequency of visible light having a wavelength of 686 nm.
A) 4.37  1014 /s
D) 2.29  10–15 /s
B) 4.37  105 /s
E) 2.29  10–6 /s
C) 6.17  1014 /s
4. Which one of the following sets of quantum numbers is not possible?
Chapter 7: Atomic Structure and Periodicity
5. Which one of the following sets of quantum numbers is not possible?
6. What is the maximum number of electrons in an atom that can have the following set of
quantum numbers?
n = 4 l = 3 ml = –2 ms = +1/2
A) 0 B) 1 C) 2 D) 6 E) 10
7. A possible set of quantum numbers for the last electron added to complete an atom of
gallium (Ga) in its ground state is
8. A possible set of quantum numbers for the last electron added to complete an atom of
germanium (Ge) in its ground state is
9. Electrons in an orbital with l = 3 are in a/an
A) d orbital. B) f orbital. C) g orbital. D) p orbital.
E) s orbital.
10. The number of orbitals in a d subshell is
A) 1 B) 2 C) 3 D) 5 E) 7
11. "No two electrons in an atom can have the same four quantum numbers" is a statement of
A) the Pauli exclusion principle.
D) de Broglie's relation.
B) Bohr's equation.
E) Dalton's atomic theory.
C) Hund's rule.
Chapter 7: Atomic Structure and Periodicity
12. The orbital diagram for a ground-state nitrogen atom is
13. The orbital diagram for a ground-state oxygen atom is
14. The orbital diagram for a ground state carbon atom is
15.Which ground-state atom has an electron configuration described by the following orbital
diagram?
A) phosphorus
B) germanium
C) selenium
D) tellurium
E) none of these
16. Which ground-state atom has an electron configuration described by the following orbital
diagram?
A) antimony B) germanium
C) indium
D) lead
E) tin
Chapter 7: Atomic Structure and Periodicity
17. Which ground-state atom has an electron configuration described by the following orbital
diagram?
A) phosphorus
B) nitrogen
C) arsenic D) vanadium
E) none of these
18. How many unpaired electrons does a ground-state atom of sulfur have?
A) 0 B) 1 C) 2 D) 3 E) 4
19. A ground-state atom of arsenic has
A) no unpaired electrons.
B) one unpaired electron.
C) two unpaired electrons.
D)
E)
three unpaired electrons.
four unpaired electrons.
20. Which element has the following ground-state electron configuration?
1s22s22p63s2
A) Na B) Mg C) Al D) Si E) Ne
21. Which element has the following ground-state electron configuration?
[Ar]4s23d104p5
A) aresnic B) bromine C) iodine D) selenium E) tellerium
22. Which element has the following ground-state electron configuration?
[Kr]5s14d5
A) Mn B) Mo C) Nb D) Re E) Tc
23. Which element has the following ground-state electron configuration?
[Kr]5s24d105p2
A) Sn B) Sb C) Pb D) Ge E) Te
24. The electron configuration of a ground-state Co atom is
A) [Ar]4s23d7
D) [Ar]4s13d5
2 2 6 2 9
B) 1s 2s 2p 3s 3d
E) [Ar]4s24d7
C) [Ne]3s23d7
25. The electron configuration of a ground-state vanadium atom is
A) [Ar]4s24d3 B) [Ar]4s24p3 C) [Ar]4s23d3 D) [Ar]3d5
26. The electron configuration of a ground-state copper atom is
A) [Ar]4s24d4 B) [Ar]4s24p63d3 C) [Ar]4s23d9 D) [Ar]3d9
27. The ground-state electron configuration for an atom of indium is
A) [Kr]5s24p64d5
D) [Kr]5s25p64d5
2 10 1
B) [Ar]4s 3d 4p
E) [Kr]5s24d105p1
C) [Ar]4s24p63d5
E) [Ar]4s13d10
Chapter 7: Atomic Structure and Periodicity
28. Which of the following is the ground-state electron configuration of a calcium atom?
A) [Ne]3s2 B) [Ne]3s23p6 C) [Ar]4s13d1 D) [Ar]4s2 E) [Ar]3d2
29. How many electrons are there in the 2nd principal energy level (n = 2) of a phosphorus
atom?
A) 3 B) 5 C) 6 D) 8 E) 10
30. How many electrons are there in the 3rd principal energy level (n = 3) of a phosphorus
atom?
A) 3 B) 5. C) 6 D) 8 E) 10
31. A ground-state atom of manganese has ___ unpaired electrons and is _____.
A) 0, diamagnetic
D) 5, paramagnetic
B) 2, diamagnetic
E) 7, paramagnetic
C) 3, paramagnetic
32. A ground-state atom of vanadium has ___ unpaired electrons and is _____.
A) 0, diamagnetic
D) 5, paramagnetic
B) 2, diamagnetic
E) 4, diamagnetic
C) 3, paramagnetic
33. A ground-state atom of iron has ___ unpaired electrons and is _____.
A) 0, diamagnetic
D) 5, paramagnetic
B) 6, diamagnetic
E) 4, paramagnetic
C) 3, paramagnetic
34. A ground-state chromium atom has how many unpaired electrons?
A) 1 B) 2 C) 4 D) 5 E) 6
35. An AM radio station broadcasts at a frequency of 1270 kHz. Calculate the wavelength of
the broadcast signal in meters. (c = 2.9979  108 m/s)
36. Write the ground state electron configuration for the selenium atom.
37. Write the ground state electron configuration for the phosphorus atom.
38. Write the ground state electron configuration for Ni.
39. Write the ground state electron configuration for Cr.
40. Calculate the energy of a photon of light with a wavelength of 360 nm.
41. What is the total number of electrons possible in the 2p orbitals?
Chapter 7: Atomic Structure and Periodicity
42. What is the total number of electrons possible in the 6s orbital?
43. What is the ground-state electron configuration for chlorine?
44. If one electron is added to the outer shell of chlorine, it would have the same electron
configuration as what element?
45. The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of
these colors, _______ has the most energy.
46. The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of
these colors, ______ has the least energy.
47. The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of
these colors, _______ has the longest wavelength.
48. The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of
these colors, ______ has the shortest wavelength.
49. A neon atom in its ground state will be diamagnetic (True or False).
50. For all atoms of the same element, the 2s orbital is larger than the 1s orbital (True or
False).
51. The elements in Group 7A are known by what name?
A) transition metals
D) alkaline earth metals
B) halogens
E) noble gases
C) alkali metals
52. The elements in Group 2A are known by what name?
A) transition metals
D) alkaline earth metals
B) halogens
E) noble gases
C) alkali metals
53. The alkali metal elements are found in _______ of the periodic table.
A) Group 1A B) Group 2A C) Group 3A D) Period 7 E) Period 1
54. Which one of the following elements is a transition element?
A) Sr B) Pb C) As D) Fe E) H
55. Which one of the following elements is a transition element?
A) antimony B) barium C) chromium D) potassium E) selenium
56. The general electron configuration for atoms of all elements in Group 5A is
A) ns2np6 B) ns2np5 C) ns2np4 D) ns2np3 E) ns2np1
Chapter 7: Atomic Structure and Periodicity
57. Which of the following is the general electron configuration for the outermost electrons
of elements in the alkaline earth group?
A) ns1 B) ns2 C) ns2np4 D) ns2np5 E) ns2np6(n -1)d6
58. The general electron configuration for atoms of the halogen group is
A) ns2np6 B) ns2np5 C) ns2np6(n -1)d7 D) ns1 E) ns2np7
59. The general electron configuration for noble gas atoms is
A) ns2np6 B) ns2np5 C) ns2np4 D) ns2np3 E) ns2
60. An element with the general electron configuration for its outermost electrons of ns2np1
would be in which element group?
A) 2A B) 3A C) 4A D) 5A E) 8A
61. How many valence electrons does an oxygen atom have?
A) 2 B) 4 C) 6 D) 7 E) 8
62. How many valence electrons does a tin (Sn) atom have?
A) 2 B) 4 C) 14 D) 36 E) 50
63. How many electrons are in the 4p orbitals of vanadium?
A) 0 B) 2 C) 4 D) 5 E) 6
64. What is the charge on the monatomic ion that calcium forms in its compounds?
A) +2 B) +1 C) –1 D) –2 E) –3
65. What is the charge on the monatomic ion of nitrogen, the nitride ion?
A) +2 B) +1 C) –1 D) –2 E) –3
66. Which two electron configurations represent elements that would have similar chemical
properties?
(1) 1s22s22p4
(2) 1s22s22p5
(3) [Ar]4s23d5
(4) [Ar]4s23d104p5
A) (1) and (2) B) (1) and (3) C) (2) and (3) D) (2) and (4) E) (3) and (4)
67. Which one of the following pairs are isoelectronic?
A) Mn2+ and Ar
D) Cl– and S
2+
2+
B) Zn and Cu
E) K+ and Cl–
C) Na+ and K+
68. Which ion is isoelectronic with Ar?
A) Fe2+ B) F– C) Br– D) Ga3+
E) Ca2+
69. Which of the following is the electron configuration of the iron(III) ion?
A) [Ar]3d5 B) [Ar]4s13d5 C) [Ar]4s23d3 D) [Ar]3d6 E) [Ar]4s23d9
Chapter 7: Atomic Structure and Periodicity
70. The electron configuration of a copper(I) ion is
A) [Ar]4s23d8 B) [Ar]4s13d9 C) [Ar]3d10 D) [Ar]4s23d64p2
E) [Kr]
71. The sulfide ion, S2–, is isoelectronic with which one of the following?
A) O2– B) F– C) Na+ D) Al3+ E) K+
72. The cobalt(III) ion, Co3+, has how many 3d electrons?
A) 0 B) 7 C) 6 D) 5 E) 4
73. How many 3d electrons does the manganese(II) ion, Mn2+, have?
A) 3 B) 4 C) 5 D) 6 E) 7
74. How many 3d electrons does an Fe3+ ion have?
A) 9 B) 6 C) 5 D) 4 E) 3
75. Which of the following ground-state ions has the largest number of unpaired electrons?
A) Cr2+ B) Mn2+ C) Ni2+ D) Cu+ E) Co2+
76. Which of the following ground-state ions has unpaired electrons?
A) P3– B) V5+ C) Mg2+ D) Sc2+ E) S2+
77. Which of the atoms listed below has the smallest radius?
A) Al B) P C) As D) Te E) Na
78. Which of the elements listed below has the greatest atomic radius?
A) B B) Al C) S D) P E) Si
79. Which one of the following ions has the largest radius?
A) Cl– B) K+ C) S2– D) Na+ E) O2–
80. Arrange the following ions in order of increasing ionic radius: K+, P3– , S2–, Cl–.
increasing radius 
A) K+ < Cl– < S2– < P3–
D) Cl– < S2– < P3– < K+
+
3–
2–
–
B) K < P < S < Cl
E) Cl– < S2– < K+ < P3–
C) P3– < S2– < Cl– < K+
81. Arrange the following ions in order of decreasing ionic radius: Al3+, Mg2+, Na+, O2–.
decreasing radius 
A) Al3+ > Mg2+ > O2– > Na+
D) O2– > Al3+ > Mg2+ > Na+
3+
2+
+
2–
B) Al > Mg > Na > O
E) O2– > Na+ > Mg2+ > Al3+
C) Na+ > Mg2+ > Al3+ > O2–
82. Which of the elements listed below has the highest first ionization energy?
A) He B) Ne C) Ar D) Kr E) Xe
Chapter 7: Atomic Structure and Periodicity
83. Which of the elements listed below has the highest first ionization energy?
A) C B) Ge C) P D) O E) Se
84. Which of the following elements has the smallest first ionization energy?
A) Cl B) Na C) Be D) K E) As
85. Which of the following elements has the smallest ionization energy?
A) Li B) Na C) Be D) K E) Rb
86. Which of the following elements has the greatest electron affinity (largest positive
value)?
A) Mg B) Al C) Si D) P E) S
87. Which of the following is an amphoteric oxide?
A) Na2O B) MgO C) Al2O3 D) SO2 E) Cl2O7
88. Which of the following is an acidic oxide?
A) P4O10 B) MgO C) Fe2O3 D) K2O
89. Which of the following is a basic oxide?
A) NO2 B) H2O C) Na2O D) SnO
E) Cr2O3
E) SO2
90. Consider the following reaction: 3Li + Z  Li3Z. What is the formula for the compound
if we substitute sodium for lithium?
A) NaZ B) Na2Z C) NaZ2 D) Na3Z E) NaZ3
91. Consider the following reaction: 3Li + Z  Li3Z. What is the formula for the compound
if we substitute magnesium for lithium?
A) MgZ B) Mg2Z C) MgZ2 D) Mg3Z E) Mg3Z2
92. Write the ground-state electron configuration for S2–.
93. Write the ground-state electron configuration for Cr3+.
94. Write the ground-state electron configuration for Ni2+.
95. Write the ground-state electron configuration for Br–.
96. Write the ground-state electron configuration for K+.
97. Why is the Mg2+ ion smaller than F–, even though they are isoelectronic?
98. The radii of ions are always smaller than the radii of the corresponding atoms of the same
element. (True or False)
Chapter 7: Atomic Structure and Periodicity
99. The electron configuration of the outermost electrons of atoms of the halogen group is
ns2np7. (True or False)
100. Amphoteric oxides exhibit both acidic and basic properties. (True or False)