Chapter 7

17. Which of the following statements concerning ground state electron configurations is/are CORRECT? 1. For a hydrogen atom with one electron, the 2s and 2p orbitals have identical energies. 2. For a lithium atom with three electrons, the 2s and 2p orbitals have different energies. 3.The effective nuclear charge felt by an electron in a 2p orbital is greater for a carbon atom than for a boron atom.

1, 2, and 3

41. If the ground state electron configuration of an element is [Ar]3d^10 4s^2 4p^5, what is the typical charge on the monatomic anion of the element?

1-

4. How many electrons can be described by the quantum numbers n= 3 and l= 2?

10

28. Which of the following electron configurations corresponds to the ground state of an atom of a transition element?

1s^2 2s^2 2p^6 3s^2 3p^6 3d^1 4s^2

29. The complete electron configuration of tin is _____.

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^2

9. Which of the following electron configurations is not allowed?

1s^2 2s^3

22. Which of the following orbital diagrams represents a paramagnetic atom?

2 and 3

3. How many electrons can be described by the following quantum numbers: n = 3, l = 2, ml = 1?

2

5. What is the maximum number of electrons that can occupy the n = 3 shell?

2

6. What is the maximum number of electrons that can occupy one s orbital?

2

11. The procedure by which electrons are assigned to (or built up into) orbitals is known as the ____ principle.

Aufbau

55. Rank the following atoms in order decreasing atomic radii: Be, Be, Be, B.

B > Be > Be^1+ > Be^2+

64. An atom of which of the following elements has the most negative electron affinity?

Cl

48. What 2+ ion has the following ground state electron configuration?

Co^2+

16. Which of the following statements is true?

Core electrons effectively shield outer electrons from nuclear charge.

83. Which of the following groups is a part of the s-block elements?

Group 2A

75. A metal halide forms when potassium reacts with elemental chlorine. What is the most likely formula of this metal halide?

KCl

61. For which one of the following elements is the second ionization energy over ten times larger than its first ionization energy?

Li

60. Which of the following equations corresponds to the second ionization of magnesium?

Mg(g) → Mg+(g) + e-

49. Which of the following ions has the given ground state electron configuration?

Sn^2+

52. Which of the following statements is true of atomic radii?

They increase down a group and decrease across a period.

12. Which of the following statements is true concerning the electron configuration [Xe]6p^2?

This configuration cannot be the ground-state electron configuration for a Ba atom because it violates the Aufbau principle.

54. Which of the following atoms of elements has the largest atomic radius?

Tl

39. For which of the following atoms is the 2+ ion diamagnetic in the ground state?

Zn

32. What noble gas core precedes the valence shell ground state electron configuration for potassium (K)?

[Ar]

35. Which element has the following ground state electron configuration?

[Ar] Sc

27. What is the ground-state electron configuration of sulfur (S)?

[Ne]3s^2 3p^4

63. The change in energy for the following reaction is referred to as the ____ for boron. B(g) + e- → B-(g)

electron affinity

19. An element that has the same ground state valence-shell electron configuration as thallium is

gallium.

10. Which of the following sets of quantum numbers is allowed?

n = 4, l = 1, ml = 0, ms = -1/2

84. In the context of magnetism, Cu2+ is _____.

paramagnetic

50. The ground-state electron configuration of a Ni^2+ ion is 1s^2 2s^2 2p^6 3s^2 3p^6 3d^8 . Therefore, Ni^2+ is

paramagnetic with two unpaired electrons.

47. What 2- ion has the following ground state electron configuration?

sulfide ion

23. Which of the following atoms is diamagnetic in its ground state?

mercury (Hg)

38. What is a possible set of quantum numbers for an unpaired electron in the orbital box diagram below?

n = 5, l = 1, ml = -1, ms = +1/2

72. What is the charge formed by alkaline earth metals when they react with nonmetals?

+2

21. How many unpaired electrons are found in the ground state electron configuration of barium (ba)?

0

2. How many electrons can be described by the following quantum numbers: n = 4, = 2, = 2, ms = -1/2?

1

1. Which of the following statements concerning the Pauli exclusion principle is/are CORRECT? 1. If two electrons occupy the same orbital they must have opposite spins. 2. No two electrons in an atom can have the same four quantum numbers. 3. Electrons with opposing spins are attracted to each other.

1 and 2

58. Which of the following statements is/are CORRECT? 1. For any element, the second ionization energy is larger than the first ionization energy. 2. Ionization energy is a positive value for all elements. 3. Ionization energy increases down a group of the periodic table.

1 and 2

14. Which of the following statements is/are CORRECT for an oxygen atom? 1. The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s electron. 2. The effective nuclear charges felt by 2s and 2p electrons are identical. 3. The effective nuclear charge felt by a 2p electron is less than that felt by a 2s electron.

3 only

13. According to the Aufbau principle, which of the following subshells is typically filled next after the 4s subshell?

3d

7. Which of the following orbital occupancy designations is incorrect?

3d^12

20. How many valence electrons does an arsenic atom have?

5

8. The maximum number of electrons that can be accommodated in a p subshell is

6

40. Which of the following elements in its 1+ ionic state has the ground state electron configuration [Kr]4d^10?

Ag

69. Place the following ions in order from smallest to largest ionic radii: K+, Na+, Mg2+, and Al3+.

Al3+ < Mg2+ < Na+ < K+

68. Rank the following ions in order of decreasing ionic radii: Al3+, Mg2+, Al3+, Al3+.

Al3+ > Al3+ > Mg2+ > Al3+

59. The change in energy for which of the following processes corresponds to the first ionization energy of beryllium?

Be(g) → Be+(g) + e-

62. Arrange F, Cl, and Br in order of their increasing first ionization energies.

Br < Cl < F

56. Place the following atoms in order of increasing atomic radii: Se, Sb, Br, and Te.

Br < Se < Te < Sb

70. Which of the following species has the largest radius?

Br-

45. Which of the following has the same (total) number of electrons as Ar?

Ca^2+

51. Which of the following cations has the same number of unpaired electrons as Fe^2+?

Cr^2+

57. An atom of which of the following elements has the smallest ionization energy?

Cs

26. Which of the following elements has the ground state electron configuration [Ar]3d^10 4s^1?

Cu

53. An atom of which of the following elements has the smallest atomic radius?

F

71. Which of the following elements would be expected to have chemical and physical properties most similar to Iodine (I)?

Fluorine (F)

66. According to the general trend in electron affinities, which group (or family) of elements tends to form the most stable anions in the gas phase?

Halogens

36. Which element has the following ground state electron configuration?

In

18. Which of the following elements is found in the d-block of the periodic table?

Ir

73. A metal oxide forms when potassium reacts with oxygen. What is the most likely formula of this metal oxide?

K2O

74. A metal phosphide forms when potassium reacts with elemental phosphorus. What is the most likely formula of this metal phosphide?

K3P

34. Which element has the following ground state electron configuration?

N

44. Which of the given ions have the same ground state electron configuration: S^2-, N^3-, Mg^2+, and Br^-?

N^3- and Mg^2+

33. Which ground-state electron configuration is incorrect?

Ni: [Ar]3d^5

65. _____ have no affinity for electrons.

Noble gases

25. Which atom has the ground state electronic configuration 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3?

V

31. All of the following ground-state electron configurations are correct except

V: [Ar]4s^2 4d^3

42. What is the ground state electron configuration for Cr^3+?

[Ar]3d^3

43. What is the ground state electron configuration for Sn^2+?

[Kr]4d^10 5s^2

67. Which group of the periodic table of elements forms only 2+ ions?

group 2A

30. Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)

has the maximum number of unpaired electrons, all with the same spin.

15. The small, but important, energy differences between 3s, 3p, and 3d electrons is a consequence of

their effective nuclear charge