1. The electron configuration of Cl^- is (the Periodic Table should help you):
   1. 1s2s²2p⁶3s²3p⁵
   2. 1s²2s²2p⁶3s²3p⁶
   3. 1s²2s²2p⁶3d¹⁰
   4. 1s²2s²2p⁶
   5. 1s²2s²2p⁶3s²3p⁶3d¹⁰

2. How many unpaired electrons are present in ground-state atomic nitrogen?
   1. 0
   2. 2
   3. 4
   4. 3
   5. 5

3. Which orbital is being filled in the lanthanide series?
   1. 4f
   2. 4d
   3. 5f
   4. 5d
   5. 3p

4. Which of the following elements is not a metal?
   1. Na
   2. Cu
   3. Pb
   4. Mg
   5. C

5. Which of the following pairs is isoelectronic?
   1. Li, Be²⁺
   2. F^-, Na⁺
   3. O, F^-
   4. Li⁺, Na⁺

6. Which of the following has the largest radius?
   1. Na⁺
   2. Li⁺
   3. Cl^-
   4. Cl
   5. H

7. Which of the following has the largest first electron affinity (ignore sign, just magnitude)?
   1. F
   2. Li
   3. Na
   4. Br
   5. Ne

8. The electron configuration of S^2- is (the Periodic Table should help you):
   1. 1s²2s²2p⁶3s²3p⁵
   2. 1s²2s²2p⁶3s²3p⁶
   3. 1s²2s²2p⁶3d¹⁰
   4. 1s²2s²2p⁶
   5. 1s²2s²2p⁶3s²3p⁶3d¹⁰

9. How many unpaired electrons are present in ground-state atomic oxygen?
   1. 0
   2. 2
   3. 4
   4. 3
   5. 5

10. Which of the following has the largest radius?
    1. K
    2. K⁺
    3. Cl^-
    4. Cl
    5. Ne

11. Which of the following has the most favorable first electron affinity?
    1. F
    2. Li
    3. Na
    4. Br
    5. Ne

12. Which of the following has the lowest ionization energy?
    1. Li
    2. K⁺
    3. K
    4. Ne
    5. O

13. How many unpaired electrons are there in Arsenic (As)?
    1. 0
    2. 1
    3. 2
    4. 3
    5. 4

14. An element has an electron configuration of 1s²2s²2p⁶3s². Which electrons experience the greatest effective nuclear charge, and which experience the most shielding, respectively?

    	greatest effective nuclear charge	most shielding
    (a)	1s2 electrons	2s2 electrons
    (b)	1s2 electrons	3s2 electrons
    (c)	2s2 electrons	3s2 electrons
    (d)	3s2 electrons	1s2 electrons
    (e)	3s2 electrons	2p6 electrons

15. Choose the electron configuration that results when the outermost electron is ionized from the Se atom.
    1. [Ar]4s²3d¹⁰4p⁴
    2. [Ar]4s²3d¹⁰4p³
    3. [Ar]4s²3d¹⁰4p⁵
    4. [Ar]4s¹3d¹⁰4p³
    5. none of the above are correct

16. Which of the following has the highest electron affinity?
    1. Cs
    2. Na
    3. Si
    4. Ne
    5. F

17. Which of the following has the largest first ionization energy?
    1. Cs
    2. Na
    3. Si
    4. Ne
    5. F

18. Which of the following elements has the most nonmetallic character?
    1. F
    2. Ge
    3. Hg
    4. In
    5. S

19. What is the electron configuration of Fe³⁺?
    1. [Ar]4s²3d⁹
    2. [Ar]4s¹3d⁵
    3. [Ar]4s²3d³
    4. [Ar]3d⁵
    5. [Ar]3d⁶

20. Which of the following elements is the least electronegative?
    1. F
    2. Ga
    3. Os
    4. P
    5. Ra

21. Which of the following has the largest size?
    1. O
    2. F
    3. Al³⁺
    4. K⁺
    5. Rb

22. Which of the following is the correct electron configuration for Ge atoms in the ground state?
    1. [Ne]4s²3d¹⁰
    2. [Ne]4s²3d¹⁰4p¹
    3. [Kr]4s²3d¹⁰4p³
    4. [Ar]4s²3d¹⁰4p²
    5. [Ar]4s²3d¹⁰4p⁴

23. Which of the following sets is isoelectronic with Xe?
    1. I^-, Cs⁺, Ba²⁺, La³⁺
    2. Br^-, I^-, Cs, Cs⁺
    3. He, Ne, Ar, Kr
    4. Sn²⁺, Sb³⁺, Te^2-, I^-
    5. Sn⁴⁺, Sb⁵⁺, Te^2- , I

24. All the following diagrams represent an atom in the ground state EXCEPT:
    

25. Which of the following neutral atoms would be the smallest?
    1. Cs
    2. Li
    3. Rb
    4. K
    5. Na

26. Identify the element in the second period (row) whose first six successive ionization energies in units of electron volts are listed below:

    IE1	IE2	IE3	IE4	IE5	IE6
    11	24	48	64	392	490

    1. Boron
    2. Carbon
    3. Nitrogen
    4. Oxygen
    5. Fluorine

27. For the following atoms the order of increasing electron affinity is:
    1. Br < Rb < Cl < I
    2. I < Rb < Cl < Br
    3. Rb < I < Br < Cl
    4. Cl < Br < Rb < I
    5. Br < Cl < I < Rb

28. Which of the following atoms will have the highest second ionization energy?
    1. Na
    2. Mg
    3. Al
    4. Ca
    5. Y

29. Which pair of elements react to form an ionic compound?
    1. calcium and copper
    2. calcium and chlorine
    3. nitrogen and chlorine
    4. argon and oxygen
    5. fluorine and iodine

30. The smallest atom in the following list is:
    1. B
    2. C
    3. N
    4. P
    5. As

31. Which of the following elements would be expected to lose electrons and form positive ions when it reacts?
    1. phosphorus
    2. nitrogen
    3. iron
    4. iodine
    5. fluorine

32. The ion correctly matched with its grounded state electron configuration is:
    1. Al³⁺: [Ne]3s²3p⁶
    2. Cr³⁺: [Ar]4s²3d¹
    3. Fe³⁺: [Ar]3d⁶
    4. Zn²⁺: [Ar]4s²3d⁸
    5. Ni²⁺: [Ar]3d⁸

33. Arrange the following elements in order of increasing metallic character: As, P, Bi, Sb, N.
    1. As, P, Bi, Sb, N
    2. N, Sb, Bi, P, As
    3. As, Bi, N, P, Sb
    4. Bi, Sb, As, P, N
    5. N, P, As, Sb, Bi

34. The number of valence electrons in an oxalate ion, C₂O₄^2-, is:
    1. 2
    2. 10
    3. 32
    4. 34
    5. 44

35. Which of the following oxides is most acidic?
    1. Cl₂O₇
    2. Al₂O₃
    3. Ga₂O₃
    4. CaO
    5. K₂O

36. Which of the following dissolves in water to form a basic solution?
    1. CaO
    2. HCl
    3. N₂O₅
    4. CaO and HCl
    5. HCl and N₂O₅

37. Which of the ions is unlikely to be formed?
    1. O^2-
    2. Al³⁺
    3. Na⁺
    4. S^3-
    5. Mg²⁺

38. The oxidation number of Cr in dichromate ion, Cr₂O₇^2-, is:
    1. +3
    2. +6
    3. +7
    4. +12
    5. +14

39. Which equation represents an oxidation-reduction reaction?
    1. 2HCl(aq) + Mg(s) --> MgCl₂(aq) + H₂(g)
    2. Na₂O(s) + H₂O(l) --> 2NaOH(aq)
    3. CO₂(g) + H₂O(l) --> H₂CO₃(aq)
    4. CaO(s) + SO₃(g) --> CaSO₄(s)
    5. NH₃(g) + HCl(g) --> NH₄Cl(s)

40. Which electron configuration for nitrogen would satisfy Hund's Rule?
    1. 1s²2s²2p_x¹2p_y¹2p_z¹
    2. 1s¹2s¹2p_x¹2p_y¹2p_z¹
    3. 1s²2s¹2p_x¹2p_y¹2p_z¹
    4. 1s²2s²2p_x³2p_y⁰2p_z⁰
    5. 1s²2s²2p_x²2p_y¹2p_z⁰

41. The electron configuration of a certain element is [X]4s²3d¹⁰4p², where X stands for a noble gas. The element in question and the noble gas X are, respectively:
    1. Ga and Ar
    2. Ge and Ar
    3. Sn and Kr
    4. Ge and Kr
    5. Si and Ar

42. Which of the species below has the electronic configuration 1s²2s²2p⁶?
    1. Na⁺
    2. O^2-
    3. Ne
    4. N^3-
    5. All of the above

43. Which of the following species has the largest size?
    1. S
    2. Se
    3. Se^2-
    4. O^2-
    5. F

44. The successive ionization energies of a certain element in units of kJ/mol are: I₁ = 578; I₂ = 1820; I₃ = 2750; I₄ = 11,600. [I₁ is the first ionization energy; I₂, the second, etc.] This element most likely is:
    1. Na
    2. Mg
    3. Al
    4. Si
    5. P

45. Which of the following elements has the most negative electron affinity?
    1. K
    2. He
    3. Co
    4. S
    5. Cl

46. From its position in the Periodic Table, the most stable ion of the Z=88 element radium is likely to be:
    1. Ra⁺
    2. Ra²⁺
    3. Ra³⁺
    4. Ra^2-
    5. Ra^-

47. Lithium is a reactive metal. Which of the following is not a common reaction of Li?
    1. 3Li + Al --> Li₃Al
    2. 4Li + O₂ --> 2Li₂O
    3. 2Li + Cl₂ --> 2LiCl
    4. 2Li + 2H₂O --> 2LiOH + H₂
    5. All of the reactions (a)-(d) are common reactions.

48. Which of the following are not all isoelectronic?
    1. Se^2-, Sr²⁺, Br^-, Rb⁺
    2. S^2-, Cl^-, Li⁺, Be²⁺
    3. N^3-, O^2-, F^-, Ne
    4. Ar, K⁺, Ca²⁺, Sc³⁺
    5. Te^2-, I^-, Cs⁺, Ba²⁺

49. What are the changes in oxidation numbers in the reaction:
    MnO₂(s) + 4HCl(aq) --> MnCl₂(aq) + Cl₂(aq) + 2H₂O(l)
    1. Cl increases from -1 to 0; Mn decreases from +4 to +2.
    2. H increases from -1 to +1; Mn decreases from +4 to +2.
    3. H increases from -1 to +1; O decreases from -1 to -2.
    4. Mn increases from +2 to +4; O decreases from -1 to -2.
    5. There are no changes in oxidation number.

50. Which of the following reactions is not an oxidation-reduction reaction?
    1. 2Cs + Cl₂ --> 2CsCl
    2. N₂ + 3H₂ --> 2NH₃
    3. SO₃ + H₂O --> H₂SO₄
    4. Cu + 2Ag⁺ --> Cu²⁺ + 2Ag
    5. 2K + 2H₂O --> 2KOH + H₂

51. What is the correct electron configuration for C?
    1. 1s²2s²
    2. 1s²2s²3p⁴
    3. 1s¹2s²
    4. 1s²2s²2p²
    5. 1s²2s²2p⁶3s²

52. The second row transition-metal period involves filling which sub-shell?
    1. 4d
    2. 3f
    3. 3d
    4. 2d
    5. 3p

53. Which one of the following elements is not a metal?
    1. Sn
    2. Na
    3. Fe
    4. S
    5. Be

54. Which one of the following statements is incorrect?
    1. The radius of Na is larger than Na⁺
    2. The radius of Mg is larger than Na
    3. The ionization energy of Na is smaller than Na⁺
    4. The electron affinity of Cl is more negative than C (carbon)

55. Which of the following atoms has the smallest radius?
    1. Na
    2. K
    3. Al
    4. Kr
    5. Ar

56. Which of the elements below has the smallest first ionization energy?
    1. F
    2. Mg
    3. Kr
    4. K
    5. Li

57. Identify the element having the first three ionization energies as follows: I₁ = 900 kJ/mol; I₂ = 1760 kJ/mol; I₃ = 14,900 kJ/mol
    1. H
    2. He
    3. Li
    4. Be
    5. B

58. Which of the following elements is X in the compound LiXO₃?
    1. Mg
    2. Al
    3. C
    4. N
    5. Ne

59. Which of the following is least metallic?
    1. As
    2. Ge
    3. Ga
    4. In
    5. Tl

60. Cr has the electronic configuration [Ar]4s²3d^x. How many d electrons are in a Cr atom?
    1. 2
    2. 4
    3. 5
    4. 6
    5. 8

61. The electron affinity of F is, in effect, the energy required for which of the following reactions?
    1. F₂(g) --> 2F(g)
    2. F(g) --> F⁺(g) + e^-
    3. F⁺(g) --> F₂⁺(g) + e^-
    4. F^-(g) --> F(g) + e^-
    5. F₂(g) + e^- --> F^-(g) + F(g)

62. Which of the following compounds is LEAST likely to exist?
    1. BaF₂
    2. LaF₃
    3. SrF₃
    4. PbS
    5. Ca(OH)₂

63. Which of the following atoms can form an oxide involving the highest oxidation state?
    1. Li
    2. N
    3. K
    4. Ga
    5. Ba

64. The oxidation number of iodine in KIO₄ is:
    1. +7
    2. +5
    3. +3
    4. +1
    5. -1

65. The vertical columns in the Periodic Table are commonly referred to as:
    1. groups.
    2. families.
    3. periods.
    4. verticals.
    5. categories.

66. Given that the electronic structure of the nitrogen atom is 1s²2s²2p³, how many unpaired electrons are present in atomic oxygen?
    1. 2
    2. 4
    3. 3
    4. 8
    5. 1

67. Which of the following is an alkali metal?
    1. H
    2. Ca
    3. Zn
    4. Fe
    5. Rb

68. The electron configuration of ₁₃Al³⁺ is:
    1. 1s²2s²2p⁶3s²3p¹
    2. 1s²2s²2p⁶3s²
    3. 1s²2s²2p⁶
    4. 1s²2s²2p³3s²3p¹
    5. 1s²2s²2p⁶3d³

69. Which of the following ions does not have the electronic configuration of argon, ₁₈Ar?
    1. ₁₇Cl^-
    2. ₁₉K⁺
    3. ₂₀Ca²⁺
    4. ₂₁Sc³⁺
    5. ₉F^-

70. Which of the following statements are incorrect?
    1. Atoms tend to get larger as one goes across the Periodic Table from left to right in a given period.
    2. Atoms get larger as one proceeds down a given group.
    3. For a given pair of isoelectronic ions, cations are smaller than anions.
    4. The first ionization energy for a given element tends to be smaller than the second ionization energy.
    5. Less electronegative elements tend to have smaller ionization energies.

71. The ability of an element to act as an oxidizing agent tends to:
    1. increase as the ionization energy decreases.
    2. increase as the electronegativity increases.
    3. increase as the atom becomes larger.
    4. increase as the element becomes more metallic.
    5. decrease as the electronegativity increases.

72. The electron configuration of phosphorus is:
    1. [He]2s²3p³
    2. [Ne]3s²3p³
    3. [Ne]3s²3p⁴
    4. [Ne]3s²3d¹⁰3p³
    5. none of these

73. Which of the following pairs is isoelectronic?
    1. F, Cl
    2. K, Cl
    3. Li⁺, H
    4. H^-, He
    5. Ne, Ar

74. Given that the electronic structure of oxygen is [He]2s²2p⁴, how many unpaired electrons are there in O^2-?
    1. 8
    2. 2
    3. 4
    4. 10
    5. 0

75. Which of the following statements is incorrect?
    1. Atoms get larger as one moves down a group in the Periodic Table.
    2. Atoms get larger as one moves to the right across a period in the Periodic Table.
    3. Atoms get smaller when electrons are removed.
    4. Ne atoms are smaller than Na atoms.

76. Which of the following statements is correct?
    1. Ionization energies get smaller as more electrons are removed from an atom.
    2. The ionization energy increases as one moves down a group.
    3. The ionization energy increases as one moves to the right across a period.
    4. Electron affinities are always larger than ionization energies.
    5. None of the above.

77. Which of the following salts has the largest lattice energy?
    1. MgO
    2. CH₄
    3. Na₂O
    4. NaI
    5. CO₂

78. Which one of the following sets are all metals?
    1. Mg, Li, C
    2. H, Li, Na
    3. He, Be, Mg
    4. Al, Si, P
    5. Ca, Cr, Co

79. Which of the following is covalent?
    1. Li₂S
    2. MgO
    3. Fe₂O₃
    4. Bi₂O₃
    5. P₂O₅

80. What is the oxidation number of phosphorus in H₂PO₄^-?
    1. +3
    2. +4
    3. +5
    4. +6
    5. +7

81. Which of the following increase as you proceed down a group on the periodic table?
    1. atomic radius
    2. ionization energy
    3. electron affinity
    4. electronegativity
    5. all of the above

82. The first-row transition metal period involves filling which subshell?
    1. 3d
    2. 4d
    3. 3p
    4. 4f
    5. 3s

Answers

1. B
2. D
3. A
4. E
5. B
6. C
7. A
8. B
9. B
10. A
11. A
12. C
13. D
14. B
15. B
16. E
17. D
18. A
19. D
20. E
21. E
22. D
23. A
24. B
25. B
26. B
27. C
28. A
29. B
30. C
31. C
32. E
33. E
34. D
35. A
36. A
37. D
38. B
39. A
40. A
41. B
42. E
43. C
44. C
45. E
46. B
47. A
48. B
49. A
50. C
51. D
52. A
53. D
54. B
55. E
56. D
57. D
58. D
59. A
60. B
61. E
62. C
63. B
64. A
65. A
66. A
67. E
68. C
69. E
70. A
71. B
72. B
73. D
74. E
75. B
76. C
77. A
78. E
79. E
80. C
81. A
82. A