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Homework answers / question archive / Chapter 8: Chemical Bonding 1)Which of the following compounds is likely to have covalent bonds? A) NaCl B) LiF C) CO D) CaBr2 E) MgO 2
Chapter 8: Chemical Bonding
1)Which of the following compounds is likely to have covalent bonds?
A) NaCl B) LiF C) CO D) CaBr2 E) MgO
2. Which of the following compounds is likely to have covalent bonds?
A) MgS B) KF C) SO2 D) SrCl2 E) RbF
3. Which of the following compounds is likely to have covalent bonds?
A) LiBr B) CsF C) BaCl2 D) Cr2O3 E) NO2
4. Which of the following compounds is likely to have covalent bonds?
A) CaBr2 B) OF2 C) NaF D) BaBr2 E) LiCl
5. Which of the following substances has bonding best described as ionic bonding?
A) SiO2 B) TiO2 C) SO2 D) CO2 E) O2
6. Which of the following substances has both ionic and covalent bonding?
A) NaCl B) Cl2 C) MgO D) MgCO3 E) None of these
7. Which image(s) in the figure represents an ionic compound?
A) I only B) II only C) III only D) IV only E) I and IV
8. Which image(s) in the figure represents a compound that contains covalent bonds?
A) I only B) II only C) II and III D) II, III, and V E) V only
9. Which image(s) in the figure represents an ionic compound?
A) I only B) II only C) III only D) IV only E) I and IV
10. Which image(s) in the figure represents a compound with covalent bonds?
A) II only B) III only C) IV only D) II and III E) II, III, and V
11. Which of the following compounds is likely to occur as a gas at room temperature?
A) CaF2 B) CH4 C) MgO D) FeCl3 E) LiF
12. Which of the following compounds is likely to occur as a gas at room temperature?
A) CaF2 B) MgS C) NO2 D) NaF E) CoCl2
13. Which of the following compounds is likely to occur as a solid at room temperature?
A) CH4 B) SO2 C) CaCl2 D) CO2 E) H2O2
14. Which of the following compounds is likely to occur as a solid at room temperature?
A) PH3 B) NO2 C) MgCl2 D) SO2 E) ClO2
15. Which of the following compounds is likely to have a relatively high boiling point?
A) CoCl3 B) NH3 C) CO D) NO2 E) CH4
16. Which of the following compounds is likely to have a relatively high boiling point?
A) PH3 B) FeCl3 C) NO D) SO2 E) C2H6
17. Which of the following elements is the most electronegative?
A) carbon B) silicon C) nitrogen D) oxygen E) lithium
18. Which of the following elements is the most electronegative?
A) H B) S C) F D) Cl E) P
19. In which of the following bonds does nitrogen have a partial negative charge (d–)?
A) N–C B) N–O C) N–F D) N–N E) None of these
20. In which of the following bonds does hydrogen have a partial negative charge (d–)?
A) H–F B) H–B C) H–C D) H–H E) None of these
21. In which of the following molecules does oxygen have a partial positive charge (d+)?
A) O2 B) OF2 C) H2O D) MgO E) None of these
22. Using periodic trends, arrange the following atoms in order of increasing electronegativity: Cl, Si, Ga, Sr
A) Cl < Si < Ga < Sr D) Sr < Ga < Si < Cl
B) Si < Ga < Sr < Cl E) Sr > Ga < Cl < Si
C) Si < Cl < Ga < Sr
23. Using periodic trends, arrange the following atoms in order of increasing electronegativity: F, O, S, As
A) F < O < S < As D) S < As < O < F
B) As < O < S < F E) S < As < F < O
C) As < S < O < F
24. Using periodic trends, arrange the following atoms in order of increasing electronegativity: Se, Cl, Mg, Na
A) Se < Cl < Mg < Na D) Se < Mg < Na < Cl
B) Na < Mg < Cl < Se E) Na < Mg < Se < Cl
C) Mg < Na < Se < Cl
25. Using periodic trends, arrange the following atoms in order of increasing electronegativity: S, Sr, P, Cs
A) S < Sr < P < Cs D) Cs < Sr < S < P
B) S < P < Sr < Cs E) Cs < Sr < P < S
C) P < Cs < Sr < S
26. Which of the following molecules contains the most polar bonds?
A) F2 B) OF2 C) NF3 D) BF3 E) CF4
27. Arrange the following bonds in order of increasing polarity: C-O, C-C, C-N, C-F
A) C-O < C-C < C-N < C-F D) C-C < C-N < C-O < C-F
B) C-N < C-O < C-F < C-C E) C-C < C-O < C-N < C-F
C) C-F < C-O < C-N < C-C
28. Arrange the following bonds in order of increasing polarity: F-F, F-C, F-O, F-N
A) F-F < F-C < F-O < F-N D) F-N < F-O < F-F < F-C
B) F-F < F-O < F-N < F-C E) F-N < F-C < F-O < F-F
C) F-O < F-N < F-F < F-C
29. Arrange the following bonds in order of increasing polarity: Cl-S, Cl-P, Cl-Si, Cl-Cl
A) Cl-S < Cl-P < Cl-Si < Cl-Cl D) Cl-Cl < Cl-S < Cl-P < Cl-Si
B) Cl-S < Cl-Si < Cl-P < Cl-Cl E) Cl-Cl < Cl-P < Cl-Si < Cl-S
C) Cl-Si < Cl-S < Cl-Cl < Cl-P
30. Arrange the following bonds in order of increasing polarity: O-H, C-H, F-H, H-H
A) O-H < C-H < F-H < H-H D) C-H < H-H < O-H < F-H
B) C-H < O-H < F-H < H-H E) H-H < C-H < F-H < O-H
C) H-H < C-H < O-H < F-H
31. Arrange the following bonds in order of increasing polarity: H-Cl, H-I, H-Br, H-F
A) H-Cl < H-I < H-Br < H-F D) H-I < H-Br < H-Cl < H-F
B) H-Cl < H-Br < H-I < H-F E) H-I < H-Cl < H-Br < H-F
C) H-F < H-Cl < H-Br < H-I
32. The Lewis symbol for F is:
A) A B) B C) C D) D E) E
33. The Lewis symbol for Mg is:
A) A B) B C) C D) D E) E
34. The Lewis symbol for S is:
A) A B) B C) C D) D E) E
35. The Lewis symbol for C is:
A) A B) B C) C D) D E) E
36. The Lewis symbol for N is:
A) A B) B C) C D) D E) E
37. The Lewis symbol for O2- is:
A) A B) B C) C D) D E) E
38. The Lewis symbol for P3- is:
A) A B) B C) C D) D E) E
39. The Lewis symbol for Ba2+ is:
A) A B) B C) C D) D E) E
40. The Lewis symbol for Al3+ is:
A) A B) B C) C D) D E) E
41. The formula for calcium sulfide is:
A) Ca2S B) CaS2 C) CaS D) Ca2S2 E) Ca2S3
42. The formula for aluminum chloride is:
A) AlCl B) AlCl2 C) Al2Cl3 D) AlCl3 E) AlCl4
43. The formula for aluminum oxide is:
A) AlO B) Al2O C) AlO2 D) Al3O2 E) Al2O3
44. The formula for calcium nitride is:
A) CaN B) Ca2N C) CaN2 D) Ca3N2 E) Ca2N3
45. Which of the following statements regarding ionic compounds is incorrect?
A) Ions are held together in an ionic lattice by electrostatic attractions.
B) The crystal structure of a given compound will depend on the sizes and number of ions in a formula unit of the compound.
C) Ionic compounds tend to have low melting points.
D) Ionic compounds are formed when a metal and a nonmetal react.
E) In forming an ionic compound, one element transfers one or more electrons to another element.
46. Which of the following statements regarding ionic compounds is incorrect?
A) In many ionic compounds, a metal accepts electron(s) from a nonmetal.
B) Ionic compounds tend to have high melting points.
C) Electrostatic attractions hold the ions together in an ionic lattice.
D) Ionic compounds must be electrically neutral.
E) The formula of an ionic compound will have the simplest possible whole-number ratio of the ions to each other.
47. Which of the following statements regarding covalent bonding is incorrect?
A) In covalent bonding, electrons are shared between two atoms.
B) Most elements try to acquire an octet of electrons in their valence shell when bonding.
C) Hydrogen only requires two electrons in its valence shell when bonding.
D) Covalent bonds occur between a metal and a nonmetal.
E) It is possible for two atoms to share more than one pair of electrons.
48. Which of the following statements regarding covalent bonding is incorrect?
A) All atoms in a Lewis structure will have eight electrons around their element symbol.
B) Covalent bonds occur between two nonmetals.
C) Two atoms may share up to three pairs of electrons.
D) Carbon typically forms four bonds.
E) The elements which exist as diatomic molecules do so in order to achieve a stable electron configuration.
49. Draw the Lewis symbol for NaBr.
A)
B) Na-Br C) Na-Br: D) :Na-Br: E)
50. Draw the Lewis symbol for MgCl2.
A) Cl-Mg-Cl D) :Cl-Mg-Cl:
B)
E)
C) Mg-Cl-Cl
51. Draw the Lewis symbol for CaO.
A) A B) B C) C D) D E) E
52. Draw the Lewis symbol for K2O.
A) A B) B C) C D) D E) E
53. How many single bonds are typically formed by the element C?
A) 1 B) 2 C) 3 D) 4 E) the number of bonds varies
54. How many single bonds are typically formed by the element N?
A) 1 B) 2 C) 3 D) 4 E) the number of bonds varies
55. How many single bonds are typically formed by the element O?
A) 1 B) 2 C) 3 D) 4 E) the number of bonds varies
56. Identify the main-group element X that could form the compound
A) C B) O C) N D) F E) P
57. Identify the main-group element X that could form the compound
A) C B) O C) N D) F E) P
58. Identify the main-group element X that could form the compound
A) P B) B C) C D) F E) )
59. An unknown molecular compound has the following Lewis structure. Which of the following elements could be the identity of X?
A) S B) H C) C D) Cl E) N
60. An unknown molecular compound has the following Lewis structure. Which of the following elements could be the identity of X?
A) Si B) P C) S D) Cl E) Ne
61. An unknown molecular compound has the following Lewis structure. Which of the following elements could be the identity of X?
A) C B) N C) O D) Cl E) Ne
62. The correctly drawn Lewis formula for CBr4 will have __________.
A) 4 single bonds
B) 5 single bonds
C) 4 single bonds and 1 pair of nonbonding electrons on the carbon atom
D) 4 single bonds and 2 pairs of nonbonding electrons on the carbon atom
E) 4 single bonds and 3 pairs of nonbonding electrons on the carbon atom
63. The correctly drawn Lewis formula for C2H2 will have __________.
A) 4 single bonds D) 4 single bonds and 1 triple bond
B) 5 single bonds E) 5 double bonds
C) 4 single bonds and 1 double bond
64. The correctly drawn Lewis formula for SiH4 will have __________.
A) 4 single bonds and 1 pair of nonbonding electrons on the Si atom
B) 4 double bonds to the Si atom
C) 2 single and 2 double bonds on the Si atom
D) 2 single bonds to Si and 2 single bonds to terminal H atoms
E) 4 single bonds to Si
65. The correctly drawn Lewis formula for NH2OH will have __________.
A) 3 single bonds and 3 pairs of nonbonding electrons
B) 4 single bonds and 3 pairs of nonbonding electrons
C) 3 single bonds, 1 double bond, and 2 pairs of nonbonding electrons
D) 2 single bonds, 2 double bonds, and 2 pairs of nonbonding electrons
E) 4 single bonds and 2 pairs of nonbonding electrons
66. The correctly drawn Lewis formula for HCN will have __________.
A) 2 single bonds and 5 pairs of nonbonding electrons
B) 1 single bond, 1 double bond, and 3 pairs of nonbonding electrons
C) 2 double bonds and 2 pairs of nonbonding electrons
D) 1 single bond, 1 triple bond, and 1 pair of nonbonding electrons
E) 2 double bonds and 1 pair of nonbonding electrons
67. Which of the following contains a triple bond?
A) H2 B) N2 C) O2 D) F2 E) Cl2
68. Which of the following contains a double bond?
A) CH4 B) C2H6 C) C2H4 D) C2H2 E) H2
69. Which of the following contains a triple bond?
A) C2H6 B) HCN C) NO3- D) NH3 E) O3
70. Draw the Lewis structure for the NO2– ion. What is the total number of electrons shared between nitrogen and the two oxygen atoms?
A) 2 B) 3 C) 5 D) 6 E) 8
71. Which of the following molecules would exhibit resonance?
A) H2O B) N2 C) NO2 D) CO2 E) CCl4
72. Which of the following molecules would exhibit resonance?
A) H2S B) Cl2 C) SO2 D) O2 E) CH4
73. Which of the following molecules or ions would exhibit resonance?
A) C2H2 B) Br2 C) CO32‾ D) CO E) SiH4
74. How many equivalent resonance structures best represent(s) the NO2– ion?
A) 1 B) 2 C) 3 D) 4 E) It does not exhibit resonance.
75. Which of the following is best represented by two equivalent resonance structures?
A) O3 B) CO2 C) NO3– D) N2 E) none of these
76. Which of these molecules or ions has a violation of the octet rule (other than H)?
A) CO2 B) H2S C) SF4 D) CH4 E) PCl3
77. Which of these molecules or ions has a violation of the octet rule (other than H)?
A) CO B) H2O C) PCl5 D) Br2 E) NH3
78. Which of these molecules or ions has a violation of the octet rule (other than H)?
A) BCl3 B) F2 C) PH3 D) NO3‾ E) SF2
79. Which of these molecules or ions has a violation of the octet rule (other than H)?
A) C2H2 B) NH4+ C) SO2 D) BeF2 E) I2
80. In which of the following does the central atom NOT obey the octet rule?
A) BH3 B) NH3 C) PH3 D) H2S E) All of these obey the octet rule.
81. Identify the class of organic substance for the molecule CH3CH2-OH.
A) alkane B) alkene C) alcohol D) amine E) ester
82. Identify the class of organic substance for the molecule CH3CH2-NH2.
A) alkane B) alkene C) alcohol D) amine E) ester
83. Identify the class of organic substance for the molecule CH3CH=CH2.
A) alkane B) alkene C) alcohol D) amine E) ester
84. Identify the class of organic substance for the molecule H3C-CH3.
A) alkane B) alkene C) alcohol D) amine E) ester
85. Which of the following statements regarding VSEPR theory is correct?
A) The name of the molecular shape which has three atoms and one unshared pair of electrons on the central atom is tetrahedral.
B) Nonbonding electron pairs have no influence on molecular shape.
C) It is not necessary to draw the Lewis structure of a molecule before predicting its shape.
D) VSEPR theory can be used to predict the shape of a molecule.
E) The molecular shape called “bent” always has only one pair of unshared electrons on the central atom.
86. Which of the following statements regarding VSEPR theory is correct?
A) When counting the number of electron groups on the central atom, a double bond counts as two groups.
B) The trigonal pyramidal shape has three atoms and one unshared pair of electrons on the central atom.
C) The unshared pairs of electrons are unimportant in both the Lewis structure and in VSEPR theory.
D) A trigonal planar molecular shape has four atoms attached to the central atom.
E) It is not necessary to calculate the number of valence electrons available in a given molecule before using VSEPR to predict the shape of that molecule.
87. Which of the following has a parent structure that is tetrahedral?
A) H2S B) SiCl4 C) NF3 D) SO42– E) all of these
88. Which of the following has a parent structure that is trigonal planar?
A) NH3 B) H2O C) SO2 D) CO2 E) all of these
89. Predict the molecular shape and give the approximate bond angles of the PCl3 molecule.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 120°
C) tetrahedral, 109.5°
90. Predict the molecular shape and give the approximate bond angles of the SO2 molecule.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 120°
C) tetrahedral, 109.5°
91. Predict the molecular shape and give the approximate bond angles of the CO2 molecule.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 120°
C) tetrahedral, 109.5°
92. Predict the molecular shape and give the approximate bond angles of the SiH4 molecule.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 120°
C) tetrahedral, 109.5°
93. Predict the molecular shape and give the approximate bond angles of the SO3 molecule.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 120°
C) tetrahedral, 109.5°
94. Predict the molecular shape and give the approximate bond angles of the SO32–polyatomic ion.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 120°
C) tetrahedral, 109.5°
95. Predict the molecular shape and give the approximate bond angles of the CO32–polyatomic ion.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 120°
C) tetrahedral, 109.5°
96. Predict the molecular shape and give the approximate bond angles of the OF2 molecule.
A) linear, 180° D) trigonal pyramidal, 109.5°
B) trigonal planar, 120° E) bent, 109.5°
C) tetrahedral, 109.5°
97. Which of the following has bond angles closest to 120°?
A) CO2 B) H2O C) O3 D) CH4 E) NH3
98. Which of the molecules in the figure are polar? (Assume that the bonds are all polar.)
A) I, II, and III D) I, II, and IV
B) I, II, III, and IV E) I, III, and IV
C) II, III, and IV
99. Which of the molecules in the figure are polar? (Assume that the bonds are all polar.)
A) I, II, and III B) I and II C) I, III, and IV D) II only E) II and IV
100. Which of the molecules in the figure has unshared electron pairs on the central atom?
A) I, II, and III D) II only
B) I and II E) not enough information
C) I, III, and IV
101. Which of the molecules in the figure has unshared electron pairs on the central atom?
A) II and III D) I, II, III, and IV
B) I and III E) not enough information
C) I, II, and III
102. Which of the following molecules is polar?
A) CCl4 B) H2S C) SO3 D) CO2 E) BeF2
103. Which of the following molecules is polar?
A) BCl3 B) NH3 C) SiCl4 D) CBr4 E) BeBr2
104. Which of the following molecules is polar?
A) BF3 B) CH4 C) CS2 D) PCl3 E) BeCl2
105. Which of the following molecules is a nonpolar molecule with polar bonds?
A) NF3 B) CH2Cl2 C) CF4 D) O3 E) CO
106. The K2+ ion forms commonly because it is isoelectronic with chlorine.
107. When there are extra electrons available in a Lewis structure, they are used to make double or triple bonds in the molecule.
108. Resonance is a representation of how electrons shift rapidly from one atom to another in a molecule or ion.
109. If a molecule has polar bonds, the overall molecule must be polar.
110. Electronegativity is a measure of the amount of energy needed to remove an electron from an atom.
111. Electrons pairs on molecules maximize the distance between themselves in order to minimize repulsions.
112. Molecular compounds are more likely to be gases at room temperature than ionic compounds.
113. Metallic elements are more electronegative than nonmetallic elements.
114. Diatomic elements such as F2 and Cl2 are polar because these elements are very electronegative.
115. A trigonal planar molecule will have an unshared pair of electrons on the central atom.
116. Draw a Lewis structure for CCl4.
117. Draw a Lewis structure for H2S.
118. Draw a Lewis structure for PH3.
119. Draw a Lewis structure for SO2.
120. Write the Lewis structure for CO32-, including resonance forms, if necessary.
121. Write the Lewis structure for NO3-, including resonance forms, if necessary.
122. One of these molecules is SF2, and one is BeF2. Label them appropriately and tell if either or both of the molecules are polar.
123. Give an example of a nonpolar molecule which has polar bonds.
124. Write the Lewis structure for PCl3, draw a VSEPR sketch of the molecule, name the shape of the molecule, and indicate if it is polar or nonpolar.
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