Test Bank Chapter 7 Chemical Bonding and Molecular Geometry

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Chapter 07: Chemical Bonding and Molecular Geometry

1. According to the octet rule, a magnesium atom has a tendency to (Outcome # 1,2,9) DOK 1
2. lose one electron.
3. lose two electrons.
4. gain one electron.
5. A molecule that has a single covalent bond is _____. (Outcome # 1,2,9) DOK 1
6. CO₂
7. CO
8. Cl₂
9. A diatomic molecule with a triple covalent bond is _____. (Outcome # 1,2,9) DOK 1
10. O₂
11. F₂
12. N₂
13. Which of the following diatomic molecules is joined by a double covalent bond? (Outcome # 1,2,9) DOK 1
14. Cl₂
15. O₂
16. N₂
17. Which of the following pairs of elements can be joined by a covalent bond? (Outcome # 1,2,9) DOK 1
18. N and C
19. Na and C
20. Mg and C
21. Which one of the following elements does not exist as a diatomic molecule in nature? (Outcome # 1,2,9) DOK 1
22. hydrogen
23. nitrogen
24. neon
25. Which of the following is an ionic compound? (Outcome # 1,2) DOK 1
26. CO
27. HCl
28. Na₂O
29. Which one of these compounds is an ionic compound? (Outcome # 1,2) DOK 1
30. Na₂O
31. CO₂
32. N₂
33. According to VSEPR theory, the shape of an ammonium ion, NH₄⁺, is most similar to __________. (Outcome # 1,2) DOK 2
34. CH₄
35. BH₃
36. N₂
37. According to periodic trends, which element is the most electronegative? (Outcome # 2) (DOK 1)
38. Ne
39. O
40. F
41. What is the electron group (EG) and molecular geometry (MG) of an ammonium ion? (Outcome # 2) (DOK 2)
42. (EG) tetrahedral and (MG) tetrahedral
43. (EG) tetrahedral and (MG) trigonal pyramidal
44. (EG) tetrahedral and (MG) bent
45. What is the electron group (EG) and molecular geometry (MG) of an ammonia molecule? (Outcome # 2) (DOK 2) (Paired item 1)
46. (EG) tetrahedral and (MG) tetrahedral
47. (EG) tetrahedral and (MG) trigonal pyramidal
48. (EG) tetrahedral and (MG) bent
49. According to the octet rule, which of elements will have a tendency to loss 2 electrons? (Outcome # 9) (DOK 1)
50. strontium
51. oxygen
52. cesium
53. Which of the following molecules has the greatest bond energy? (Outcome # 9) (DOK 2)
54. H₂
55. N₂
56. O₂
57. What type of bond will typically form between boron and hydrogen based on their electronegativity? (Outcome # 9) (DOK 2)
58. metallic
59. ionic
60. covalent
61. Based off periodic trends, which of the following has the strongest lattice energy? (Outcome # 9) (DOK 3)
62. aluminum chloride
63. calcium chloride
64. sodium chloride
65. Construct the molecule IF₅ using a molecular modeling software such as Spartan or 3D-ChemDraw. What are the bond angles of the equatorial fluorine’s in the structure? (Outcome # 12) (DOK 3)
66. 90°
67. 120°
68. 109.5°
69. Construct the molecule IF₅ and PF₅ using a molecular modeling software such as Spartan or 3D-ChemDraw. How do the molecular shapes differ? (Outcome # 12) (DOK 3)
70. In IF₅ there is a lone pair of electrons on iodine where as in PF₅ there are no lone pairs on phosphorus. As a result, the molecular shape of IF₅ is square pyramidal and PF₅ is trigonal bipyramidal.
71. In PF₅ there is a lone pair of electrons on phosphorus where as in IF₅ there are no lone pairs on iodine. As a result, the molecular shape of PF₅ is square pyramidal and IF₅ is trigonal bipyramidal.
72. In IF₅ there is a lone pair of electrons on iodine where as in PF₅ there are no lone pairs on phosphorus. As a result, the molecular shape of IF₅ is octahedral and PF₅ is trigonal bipyramidal.
73. Construct the molecule PF₅ using a molecular modeling software such as Spartan or 3D-ChemDraw. What are the bond angles of the equatorial fluorine’s in the structure? (Outcome # 12) (DOK 3)
74. 90°
75. 120°
76. 109.5°
77. Construct the molecule PF₅ using a molecular modeling software such as Spartan or 3D-ChemDraw. What are the bond angles of the axial fluorine’s in the structure? (Outcome # 12) (DOK 3)
78. 90°
79. 120°
80. 109.5°
81. Using VSEPR theory, predict the molecule shape of a molecule that contains 2 electron groups. (Outcome # 12) (DOK 1)
82. trigonal planar
83. linear
84. bent
85. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 4 electron groups (3 bonds and 1 lone pair electrons). (Outcome # 12) (DOK 2)
86. tetrahedral, trigonal pyramidal, >109.5°
87. tetrahedral, trigonal pyramidal, <109.5°
88. tetrahedral, trigonal pyramidal, 109.5°
89. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 5 electron groups (2 bonds and 3 lone pair electrons). (Outcome # 12) (DOK 2) (Paired item 1)
90. trigonal bipyramidal, linear, 180°
91. trigonal bipyramidal, trigonal bipyramidal, 90° and 120°
92. trigonal bipyramidal, trigonal bipyramidal, 180°
93. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 6 electron groups (5 bonds and 1 lone pair electrons). (Outcome # 12) (DOK 2) (Paired item 2)
94. octahedral, octahedral, 90°
95. octahedral, square planar, 90°
96. octahedral, square pyramidal, 90°
97. Using VSEPR theory, predict the molecular shape and bond angles in BCl₃. (Outcome # 12) (DOK 2)
98. trigonal planer, 120°
99. trigonal pyramidal, 120°
100. trigonal bent, 120°
101. Construct the molecule H₂O using a molecular modeling software such as Spartan or 3D-ChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2)
102. 104.5°
103. 107°
104. 109.5°
105. Construct the molecule NH₃ using a molecular modeling software such as Spartan or 3D-ChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2)
106. 104.5°
107. 107°
108. 109.5°
109. Construct the molecule CH₄ using a molecular modeling software such as Spartan or 3D-ChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2)
110. 104.5°
111. 107°
112. 109.5°
113. The bond angles in CH₄, NH₃, and H₂O are 109.5°, 107°, and 104.5°, respectfully. Which of the statements best describes the variance in bond angles? (Outcome # 12) (DOK 3)
114. CH₄ has no lone pairs of electrons on the central atom so the optimal molecular shape would be tetrahedral with bond angles of 109.5°. In NH₃ and H₂O there are 1 and 2 lone pairs, respectfully, so more repulsion exists between the bonds and lone pairs, as a result, the bond angles are less than 109.5°.
115. NH₃ and H₂O have a trigonal pyramidal and bent molecular shape, respectfully, which is the reason why the bond angles are less than 109.5°.
116. CH₄ only has nonpolar bonds while NH₃ and H₂O have polar bonds which results in the difference in bond angels.
117. Based off the following data, what is the lattice energy of sodium chloride? (Outcome # 11) (DOK 2)

ΔH_sub of Na = 108 kJ/mol
D_o of Cl₂ = 243 kJ/mol
IE of Na(g) = 496 kJ/mol
EA of Cl(g) = -349 kJ/mol
ΔH_f of NaCl = -411 kJ/mol

1. -1490 kJ/mol
2. -909 kJ/mol
3. -788 kJ/mol
4. In an ionic bond, the charge on the cation (i.e. the metal) is (Outcome # 1,7,9) (DOK 1)
5. always positive.
6. always negative.
7. either positive or negative.
8. According to the octet rule, a magnesium atom has a tendency to (Outcome # 1,9) (Dok 2)
9. lose one electron.
10. lose two electrons.
11. gain one electron.
12. A covalent bond is formed when two atoms (Outcome # 1,9) (DOK 2)
13. share an electron with each other.
14. share one or more pairs of electrons with each other.
15. gain electrons.
16. According to the octet rule, a bromine atom has a tendency to (Outcome # 1,9) (DOK 2)
17. lose one electron.
18. lose two electrons.
19. gain one electron.
20. The halogens have how many valence electrons? (Outcome # 1,9) (DOK 1)
21. 4
22. 6
23. 7
24. How many electrons are shared in a single covalent bond? (Outcome # 1,9) (DOK 1)
25. 2
26. 3
27. 1
28. How many electrons are shared in a double covalent bond? (Outcome # 1,9) (DOK 1)
29. 3
30. 4
31. 2
32. A molecule that has a single covalent bond is _____. (Outcome # 1,9) (DOK 1)
33. CO₂
34. CO
35. Cl₂
36. A diatomic molecule with a triple covalent bond is _____. (Outcome # 1,9) (DOK 2)
37. O₂
38. F₂
39. N₂
40. Which of the following diatomic molecules is joined by a double covalent bond? (Outcome # 1,9) (DOK 2)
41. Cl₂
42. O₂
43. N₂
44. Which of the following pairs of elements can be joined by a covalent bond? (Outcome # 1,9) (DOK 2)
45. N and C
46. Na and C
47. Mg and C
48. _____ is a diatomic molecule that has a double covalent bond. (Outcome # 9) (DOK 2)
49. Br₂
50. I₂
51. O₂
52. Which element contains triple covalent bonds? (Outcome # 9) (DOK 1)
53. oxygen
54. nitrogen
55. iodine
56. What is the molecular shape of CO₂? (Outcome # 9) (DOK 1)
57. linear
58. bent
59. trigonal planar
60. How many polar bonds does CH₄ contain? (Outcome # 9) (DOK 1)
61. 0
62. 2
63. 4
64. Which molecule has only covalent bonds? (Outcome # 9) (DOK 1)
65. CO₂
66. Al₂O₃
67. Mg₃N₂
68. Which compound has only ionic bonds? (Outcome # 9) (DOK 1) (Paired item 1)
69. CO₂
70. Al₂O₃
71. H₂O₂
72. The octet rule states that main group elements in the periodic table react to achieve a filled valence shell which consists of how many electrons? (Outcome # 9) (DOK 1)
73. 2
74. 4
75. 8
76. What is the molecular shape and polarity for xenon tetrafluoride? (Outcome # 9) (DOK 3)
77. square-planar and polar
78. square-planar and non-polar
79. tetrahedral and non-polar
80. Which of the following elements are found in the p-block and can form an octet? (Outcome # 7) (DOK 1)
81. He, P, S, As
82. P, S, O, C
83. He, Ar, Kr, Ne
84. Based off molecular polarity determined by VSEPR theory, which of the following would be soluble in methanol? (Outcome # 8) (DOK 3)
85. heptane
86. ethanol
87. pentane
88. Based off molecular polarity determined by VSEPR theory, which of the following would be insoluble in CCl₄? (Outcome # 8) (DOK 3)
89. methanol
90. octane
91. hexane
92. Based off molecular polarity determined by VSEPR theory, in which solvent would NaCl be the most soluble? (Outcome # 8) (DOK 3)
93. CH₃OH
94. CH₃CH₂OH
95. H₂O
96. Based off molecular polarity determined by VSEPR theory, in which solvent would glucose be the least soluble? (Outcome # 8) (DOK 3)
97. CH₃CH₂OCH₂CH₃
98. CH₃OH
99. H₂O
100. Which statement best describes a bond forming between fluorine and iodine? (Outcome # 8) (DOK 3)
101. fluorine and iodine are in the same group so the electron density in the bond is equaling shared giving rise to a non-polar bond
102. fluorine is more electronegative than iodine so it will attract the electron density in the bond giving rise to a polar bond
103. fluorine is less electronegative than iodine so it will attract the electron density in the bond giving rise to a polar bond
104. Why are detergents and soaps good at cleaning up oily stains from dishes or clothing? (Outcome # 8) (DOK 3)
105. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (polar) and hydrophobic (non-polar) ends. The hydrophobic end attaches to oils via hydrogen bonds creating micelles which leave the hydrophilic part exposed and can be washed away by water.
106. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (non-polar) and hydrophobic (polar) ends. The hydrophobic end attaches to oils via London forces creating micelles which leave the hydrophilic part exposed and can be washed away by water.
107. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (polar) and hydrophobic (non-polar) ends. The hydrophobic end attaches to oils via London forces creating micelles which leave the hydrophilic part exposed and can be washed away by water.
108. Is it true that a molecule with polar bonds will always be polar? (Outcome # 8) (DOK 2)
109. that is false, molecular polarity is determined by molecular shape
110. that is true, molecular polarity is determined by bond polarity only
111. that is false, molecular polarity is determined by electron group geometry
112. An _____ reaction results when the energy required to break bonds in the reactants is greater than the energy released by the formation of products. (Outcome # 3) (DOK 1)
113. exergonic
114. endothermic
115. exothermic
116. An _____ reaction results when the energy released by the formation of products is greater than the energy required to break the bonds in the reactants. (Outcome # 3) (DOK 1)
117. exergonic
118. endothermic
119. exothermic
120. How many non-polar bonds does CH₃OH contain? (Outcome # 9) (DOK 1)
121. 2
122. 3
123. 4
124. How many polar bonds does CCl₄ have in its structure? (Outcome # 9) (DOK 1)
125. 0
126. 2
127. 4