Chemical reactions occur as a result of __________
A. the attraction between opposite charges.
B. the nucleus–nucleus interactions.
C. the motion of electrons.
D. like atoms interacting.
E. combining two chemicals.
Answer: C
Learning Objective: 1.1 Compare and contrast organic and inorganic compounds
Difficulty: Easy
2. From the following, identify the item which does not contain organic compounds.
A. medicine
B. socks
C. a plant
D. a coin
E. a plastic cup
Answer: D
Learning Objective: 1.1 Compare and contrast organic and inorganic compounds
Difficulty: Easy
3. What is the difference between inorganic and organic compounds?
A. organic compounds do not contain carbon
B. organic compounds contain carbon
C. organic compounds are without pesticides
D. inorganic compounds contain carbon
E. inorganic compounds are composed exclusively of transition metal elements
Answer: B
Learning Objective: 1.1 Compare and contrast organic and inorganic compounds
Difficulty: Easy
4. Constitutional isomers do not differ in ____________.
A. physical properties
B. atomic connectivity
C. molecular formula
D. name
E. constitution
Answer: C
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Easy
5. What is the relationship between the following compounds?
A. isotopes
B. constitutional isomers
C. the same structure
D. composed of different elements
E. no relationship
Answer: B
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Easy
6. What is the relationship between the following compounds?
A. resonance isomers
B. constitutional isomers
C. empirical isomers
D. There is no relationship
Answer: B
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Easy
7. Carbon is considered to be _______.
A. tetravalent
B. divalent
C. trivalent
D. monovalent
E. pentavalent
Answer: A
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Easy
8. Which of the following compounds are constitutional isomers of each other?
A. I and II
B. III and IV
C. I, II and IV
D. II, III and IV
E. I, II, and III
Answer: E
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Medium
9. Which of the following compounds are constitutional isomers of each other?
A. I and II
B. III and IV
C. II and III
D. I and IV
E. All of these
Answer: D
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Medium
10. Draw three constitutional isomers that have molecular formula C4H8BrCl
Answer:
There are additional correct answers.
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Medium
11. Draw three constitutional isomers that have molecular formula C4H8O.
Answer:
There are additional correct answers
Learning Objective: 1.2 Describe structural theory of matter, molecular formula and structural formula
Difficulty: Hard
12. What force is NOTtaken into account in the formation of a covalent bond?
A. repulsion between two positively charged nuclei
B. force of attraction between positively charged nuclei and negatively charged electrons
C. repulsion between two negatively charged nuclei
D. repulsion between positively charged nuclei and negatively charged electrons
Answer: D
Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair
Difficulty: Easy
13. What is the correct Lewis dot structure for S?
A. I
B. II
C. III
D. IV
E. V
Answer: C
Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair
Difficulty: Easy
14. What is the correct Lewis dot structure for C?
A. I
B. II
C. III
D. IV
E. V
Answer: E
Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair
Difficulty: Easy
15. What is the correct Lewis structure for PH3?
A. I
B. II
C. III
D. IV
E. V
Answer: A
Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair
Difficulty: Easy
16. What is the correct Lewis structure for COCl2?
A. I
B. II
C. III
D. IV
E. V
Answer: B
Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair
Difficulty: Hard
17. What is the correct Lewis structure for CH3CO2H?
A. I
B. II
C. III
D. IV
E. V
Answer: D
Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair
Difficulty: Hard
18. Which of the following compounds has two lone pairs on the central atom?
A. CO2
B. SCl2
C. NF3
D. CS2
E. SO3
Answer: B
Learning Objective: 1.3 Define covalent bond, valence electrons, octet rule, and lone pair
Difficulty: Medium
19. What is the formal charge on oxygen in the following structure?
A. 2-
B. 1-
C. 2+
D. 1+
E. 0
Answer: D
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Easy
20. What is the formal charge on nitrogen in the following structure?
A. 2-
B. 1-
C. 2+
D. 1+
E. 0
Answer: D
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Easy
21. What is the formal charge on oxygen in the following structure?
A. 0
B. 1+
C. 2+
D. 1-
E. 2-
Answer: B
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Easy
22. What is the formal charge on oxygen in the following structure?
A. 2+
B. 2-
C. 1+
D. 1-
E. 0
Answer: E
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Easy
23. Which of the following structures have a zero formal charge on the carbon atom?
A. I and III
B. II and III
C. III and IV
D. I and IV
E. II and IV
Answer: C
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
24. Which of the following structures have a 1- formal charge on the sulfur atom?
A. I
B. II
C. III
D. IV
E. V
Answer: A
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Easy
25. Which of the following structures have a 1+ formal charge on the sulfur atom?
A. I
B. II
C. III
D. IV
E. V
Answer: C
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Easy
26. What are the formal charges on boron and fluorine in the following structure?
A. B = 1+, N = 1+
B. B = 1+, N = 1-
C. B = 1-, N = 1-
D. B = 1-, N = 1+
E. B = 1-, N = 0
Answer: D
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
27. What are the formal charges on boron and oxygen in the following structure?
A. B = 1-, O = 1-
B. B = 1-, O = 1+
C. B = 1+, O = 1+
D. B = 1+, O = 1-
E. B = 1-, O = 0
Answer: B
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
28. Which of the following structures have 1+ formal charge on the central atom?
A. I
B. II
C. III
D. III and V
E. IV and V
Answer: E
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
29. Which of the following structures have a formal charge on at least one atom?
A. I
B. II
C. III
D. IV
E. None of these
Answer: A
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
30. Which of the following structures have a 1- formal charge on the nitrogen atom?
A. I
B. II
C. III
D. IV
E. V
Answer: B
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
31. The bonding pattern of oxygen with a formal charge of –1 could be described as _____.
A. one lone pair of electrons and three single bonds
B. two lone pairs of electrons and two single bonds
C. three lone pairs of electrons, and one single bond
D. one lone pair of electrons, one single, and one double bond
E. zero lone pairs, and two single and one double bond
Answer: C
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
32. In an ammonium ion, nitrogen has a valence of 4, and zero nonbonding electrons. What is the correct formal charge of nitrogen with 4 covalent bonds?
A. 2-
B. 2+
C. 1-
D. 1+
E. 0
Answer: D
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
33. What is the correct Lewis structure for nitric acid, HNO3, including the formal charges?
A. I
B. II
C. III
D. IV
E. None of these
Answer: D
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
34. What is the correct Lewis structure for hydrocyanic acid, HCN, including the formal charges, if any?
A. I
B. II
C. III
D. IV
E. V
Answer: B
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Hard
35. What is the correct Lewis structure for SCN— including the formal charges, if any?
A. I
B. II
C. III
D. IV
E. V
Answer: A
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Hard
36. What is the correct Lewis structure for N2O including the formal charges, if any?
A. I
B. II
C. III
D. IV
E. V
Answer: B
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Hard
37. What is the correct Lewis structure for hydrazoic acid, HN3, including the formal charges, if any?
A. I
B. II
C. III
D. IV
E. V
Answer: A
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Hard
38. Draw the Lewis structure for NH2CN including formal charges, if any?
Answer:
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
39. Draw the Lewis structure for –CH2CN including formal charges?
Answer:
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
40. Draw the Lewis structure for ozone, O3, including formal charges, if any?
Answer:
Learning Objective: 1.4 Define formal charge and describe how formal charge is calculated
Difficulty: Medium
41. The electronegativity of elements on the periodic table tends to increase_______.
A. from left to right, top to bottom
B. from right to left, bottom to top
C. from left to right, bottom to top
D. from right to left, top to bottom
E. from upper right to lower left
Answer: C
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
42. Which of the following is the least electronegative element?
A. B
B. C
C. N
D. O
E. F
Answer: A
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
43. Which of the following is the most electronegative element?
A. B
B. C
C. N
D. O
E. H
Answer: D
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
44. Which of the following is the least electronegative element?
A. P
B. N
C. Mg
D. Si
E. K
Answer: E
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
45. Which of the following is the most electronegative element?
A. P
B. N
C. S
D. O
E. F
Answer: E
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
46. What is the correct order of increasing electronegativity for Rb, F and O?
A. Rb < F < O
B. Rb < O < F
C. O < F < Rb
D. F < Rb < O
E. None of these
Answer: B
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
47. Which of the following series has the correct order of elements in increasing electronegativity?
A. C < N < B < Br
B. P < N < As < F
C. Li < B < N < F
D. Cl < Cs < C < Co
E. Be < B < Ba < Br
Answer: C
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
48. The Cl—Cl bond is best described as___________.
A. nonpolar covalent
B. polar covalent
C. ionic
D. coordinate covalent
E. None of these.
Answer: A
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
49. The C—Cl bond is best described as___________.
A. nonpolar covalent
B. polar covalent
C. ionic
D. coordinate covalent
E. None of these.
Answer: B
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
50. The bond between potassium and oxygen is best described as___________.
A. nonpolar covalent
B. polar covalent
C. ionic
D. coordinate covalent
E. None of these.
Answer: C
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
51. The bond between carbon and hydrogen is best described as ___________.
A. nonpolar covalent
B. polar covalent
C. ionic
D. coordinate covalent
E. None of these.
Answer: A
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
52. Which of the following is the correct depiction of induction for a C—F bond?
A. I
B. II
C. III
D. IV
E. None of these.
Answer: A
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
53. Which of the following is the correct representation of the dipole for a P—Cl bond?
A. I
B. II
C. III
D. IV
E. V
Answer: C
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Easy
54. Which of the following is the correct representation of partial charges at the indicated atoms?
A. I = d+; II = d+; III = d+
B. I = d–; II = d–; III = d–
C. I = d+; II = d+; III = d–
D. I = d–; II = d–; III = d+
E. I = d+; II = d–; III = d+
Answer: D
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
55. Which atom has the most d+ in the following compound?
A. N
B. O
C. Br
D. H
E. C
Answer: E
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
56. Which of the following statements best describes the C—Cl bond in the following compound?
A. nonpolar; no dipole
B. polar; d+ at carbon and d– at chlorine
C. polar; d– at carbon and d+ at chlorine
D. ionic
E. None of these.
Answer: B
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
57. Which of the following compounds have both polar covalent and ionic bonds?
A. NH4Br
B. H2O2
C. HCN
D. H2S
E. None of these.
Answer: A
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
58. For the following compound identify the polar covalent bonds and indicate the partial charges by using d+ and d-.
Answer:
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
59. For the following compound identify the polar covalent bonds and indicate the partial charges by using d+ and d-.
Answer:
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
60. For NaSCH3, identify each bond as polar covalent, nonpolar covalent or ionic.
Answer:
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
61. For the following compound, identify each bond as polar covalent, nonpolar covalent or ionic and place a d+ on the most electropositive carbon.
Answer:
Learning Objective: 1.5 Describe the relationship between electronegativity and covalent, polar covalent, and ionic bonds
Difficulty: Medium
62. Orbitals with the same energy are called ___________.
A. quantum orbitals
B. atomic orbitals
C. antibonding orbitals
D. bonding orbitals
E. degenerate orbitals
Answer: E
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
63. What is the letter designation for the following atomic orbital?
A. s
B. p
C. d
D. f
E. g
Answer: B
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
64. What is the letter designation for the following atomic orbital?
A. s
B. p
C. d
D. f
E. g
Answer: C
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
65. In quantum mechanics a node (nodal surface or plane) is ________ .
A. location where y is negative
B. location where y is positive
C. location where y2 is positive
D. location where y2is negative
E. location where y is zero
Answer: E
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
66. Which of the following principle states that “Each orbital can accommodate a maximum of two electrons with opposite spin”?
A. Aufbau principle
B. Pauli exclusion principle
C. Hund’s Rule
D. Heizenberg Uncertainty principle
E. Le Chatelier’s principle
Answer: B
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
67. Which of the following principle states “When orbitals of equal energy are available, every orbital gets one electron before any gets two electrons”?
A. Aufbau principle
B. Pauli exclusion principle
C. Hund’s Rule
D. Heizenberg Uncertainty principle
E. Le Chatelier’s principle
Answer: C
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
68. Which of the following represents the ground state electron configuration for phosphorous?
A. 1s2 2s2 2p6 3s1 3p4
B. 1s2 2s2 2p6 3s2 3p4
C. 1s2 2s2 2p6 3s2 3p3
D. 1s2 2s2 2p6 3s2 3p2
E. 1s2 2s2 2p6 3s2 3p5
Answer: C
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
69. The atomic number for nitrogen is 7. Which of the following represents the ground state electron configuration for nitrogen?
A. 1s2 2s1 2p4
B. 1s2 2p5
C. 2s2 2p5
D. 1s2 2s2 2p3
E. 1s2 2s2 3s3
Answer: D
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
70. Which element has the electron configuration 1s2 2s2 2p6 3s2 3p5?
A. oxygen
B. fluorine
C. sulfur
D. chlorine
E. bromine
Answer: D
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
71. Which element has the electron configuration 1s2 2s2 2p6 3s2 3p3?
A. Cl
B. S
C. P
D. Al
E. N
Answer: C
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
72. What is the electronic configuration for the nitride ion?
A. 1s2 2s2 2p0
B. 1s2 2s2 2p2
C. 1s2 2s22p3
D. 1s2 2s22p4
E. 1s2 2s2 2p6
Answer: E
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
73. What is the electronic configuration for the magnesium ion?
A. 1s2 2s2 2p63s2
B. 1s2 2s2 2p6
C. 1s2 2s22p4
D. 1s2 2s22p63s1
E. 1s2 2s2 2p63s22p2
Answer: B
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
74. What is the electronic configuration for the oxide ion?
A. 1s2 2s2 2p6
B. 1s2 2s2 2p2
C. 1s2 2s22p4
D. 1s2 2s02p6
E. 1s2 2s2 2p63s22p2
Answer: A
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
75. Which element has the following electronic configuration?
A. boron
B. carbon
C. silicon
D. nitrogen
E. fluorine
Answer: D
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
76. Which element has the following electronic configuration?
A. boron
B. carbon
C. silicon
D. nitrogen
E. fluorine
Answer: E
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
77. The following ground state electron configuration violates ___.
A. the Aufbau principle
B. the Pauli Exclusion principle
C. Hund’s Rule
D. Heisenberg’s Uncertainty principle
E. None of these.
Answer: C
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
78. The following ground state electron configuration violates ____.
A. the Aufbau principle
B. the Pauli Exclusion principle
C. Hund’s Rule
D. Heisenberg’s Uncertainty principle
E. None of these.
Answer: A
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
79. The following ground state electron configuration violates ____.
A. the Aufbau principle
B. the Pauli Exclusion principle
C. Hund’s Rule
D. Heisenberg’s Uncertainty principle
E. None of these.
Answer: B
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Easy
80. Ar, K+, and Cl– have equal numbers of electrons, and are considered isoelectronic. Provide the ground state electron configuration for them.
Answer: 1s2 2s2 2p6 3s2 3p6
Learning Objective: 1.6 Describe the shape and phase of s and p atomic orbitals and the process of filling orbitals with electrons
Difficulty: Medium
81. Constructive interference of waves results in_______.
A. a wave with smaller amplitude
B. a wave with larger amplitude
C. cancellation of both waves
D. formation of a node
E. Both C and D
Answer: B
Learning Objective: 1.7 Define a bond in terms of valence bond theory
Difficulty: Easy
82. Destructive interference of waves results in_______.
A. a wave with smaller amplitude
B. a wave with larger amplitude
C. cancellation of both waves
D. formation of a node
E. Both C and D
Answer: E
Learning Objective: 1.7 Define a bond in terms of valence bond theory
Difficulty: Easy
83. All single bonds can be classified as _______.
A. nonpolar covalent
B. polar covalent
C. ionic
D. sigma bonds
E. pi bonds
Answer: D
Learning Objective: 1.7 Define a bond in terms of valence bond theory
Difficulty: Easy
84. Which of the bonding type has circular symmetry with respect to the bond axis?
A. sigma bond
B. pi bond
C. delta bond
D. covalent bond
E. ionic bond
Answer: A
Learning Objective: 1.7 Define a bond in terms of valence bond theory
Difficulty: Medium
85. The difference between valence bond theory and molecular orbital (MO) theory is _____.
A. valence bond theory requires the linear combination of atomic orbitals
B. MO theory requires the linear combination of atomic orbitals
C. valence bond theory considers only individual atomic orbitals
D. Both A and B
E. Both B and C
Answer: E
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Medium
86. How many molecular orbitals are formed, when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?
A. 1
B. 2
C. 3
D. 4
E. 5
Answer: B
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Medium
87. Which molecular orbitals are formed, when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?
A. two bonding molecular orbitals
B. only one bonding molecular orbital
C. one bonding and one antibonding molecular orbital
D. two antibonding molecular orbitals
E. only one antibonding orbital
Answer: C
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Medium
88. How are electrons distributed in the molecular orbitals, when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?
A. two electrons in the bonding molecular orbital
B. one electron in the bonding molecular orbital, one electron in the non–bonding molecular orbital
C. one electron in the bonding molecular orbital, one electron in the antibonding molecular orbital
D. two electrons in the antibonding molecular orbital
E. two electrons in the non–bonding molecular orbital
Answer: A
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Medium
89. According to molecular orbital theory, the constructive interference of two atomic orbitals results in a(n) _______.
Answer: bonding molecular orbital
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Medium
90. According to molecular orbital theory, the destructive interference of two atomic orbitals results in a(n) _______.
Answer: antibonding molecular orbital
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Medium
91. According to molecular orbital theory the highest energy molecular orbital that is occupied with an electron is referred to as _____.
A. degenerate
B. antibonding
C. the LCAO
D. the LUMO
E. the HOMO
Answer: E
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Easy
92. According to molecular orbital theory the lowest energy molecular orbital that is unoccupied with an electron is referred to as _______.
A. degenerate
B. antibonding
C. the LCAO
D. the LUMO
E. the HOMO
Answer: D
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Easy
93. Which of the following statement is incorrect, when the 1s atomic orbitals of two hydrogen atoms results in constructive interference?
A. a sigma bonding molecular orbital is formed
B. the bonding molecular orbital formed is lower in energy than the 1s atomic orbital
C. the bonding molecular orbital formed has a node between the atoms
D. the bonding molecular orbital formed has circular symmetry
E. a maximum of two electrons may occupy the bonding molecular orbital
Answer: C
Learning Objective: 1.8 Compare and contrast molecular orbital theory and valence bond theory, molecular orbitals and atomic orbitals, and bonding MOs and antibonding MOs
Difficulty: Hard
94. Describe what happens to create a sp3 hybridized orbital.
A. two s electrons are promoted to a p orbital
B. three p electrons are promoted to a s orbital
C. two p electrons are promoted to a s orbital
D. an s electron is promoted to a p orbital
E. a p electron is promoted to a s orbital
Answer: D
Answer: sigma bonding molecular orbital
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
95. Interaction of the following two atomic orbitals results in what kind of molecular orbital, in the orientation shown?
Answer: sigma bonding molecular orbital
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
96. Interaction of the following two atomic orbitals results in what kind of molecular orbital, in the orientation shown?
Answer: pi bonding molecular orbital
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
97. Interaction of the following two atomic orbitals results in what kind of molecular orbital, in the orientation shown?
Answer: pi antibonding molecular orbital
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
98. What is the hybridization state of the oxygen atom in the following compound?
A. sp
B. sp2
C. sp3
D. sp3d
E. s2p
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
99. What is the hybridization state of the carbon in CO2?
A. sp
B. sp2
C. sp3
D. sp3d
E. s2p
Answer: A
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
100. What is the hybridization state of the nitrogen atom in the following compound?
A. sp
B. sp2
C. sp3
D. sp3d
E. s2p
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
101. What is the hybridization state of the boron atom in the following compound?
A. sp
B. sp2
C. sp3
D. sp3d
E. s2p
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
102. What is the hybridization state of the carbon (I) atom in the following compound?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
103. What is the hybridization state of the nitrogen atom in the following compound?
A. sp
B. sp2
C. sp3
D. sp4
E. s2p
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
104. The lone pairs of electrons of the nitrogen atom are located in which orbitals?
A. sp2
B. sp3
C. sp
D. s
E. p
Answer: A
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
105. Which of the following structures have carbon with sp2 hybridization state?
A. I and II
B. III and IV
C. I and III
D. II and IV
E. I and IV
Answer: E
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
106. Which of the indicated carbon atoms have sp2 hybridization state in the following compound?
A. I and II
B. III and IV
C. II and III
D. I and III
E. II and IV
Answer: D
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
107. What is the correct order of hybridization state for the numbered carbon atoms in the following compound?
A. I = sp3, II = sp2, III = sp
B. I = sp2, II = sp, III = sp2
C. I = sp, II = sp2, III = sp3
D. I = sp, II = sp2, III = sp
E. I = sp2, II = sp3, III = sp2
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
108. How many s—sp2 sigma bonds are in the following compound?
A. 2
B. 3
C. 4
D. 5
E. 6
Answer: D
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
109. The C2—C3 bond in the following compound results from the overlap of which orbitals?
A. sp–sp2
B. sp–sp3
C. sp2–sp2
D. sp2–sp3
E. sp3–sp2
Answer: D
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
110. The sigma bond that is part of C=C in the following compound results from the overlap of which orbitals?
A. sp–sp2
B. sp–sp3
C. sp2–sp2
D. sp2–sp3
E. sp3–sp2
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
111. The C—C sigma bond in ethyne (H—CºC—H) results from the overlap of which orbitals?
A. sp–sp
B. sp–sp3
C. sp2–sp2
D. sp–s
E. p–p
Answer: A
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
112. How many pi bonds are present in the following compound?
A. one
B. two
C. three
D. four
E. five
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
113. How many pi bonds are present in the following compound?
A. two
B. three
C. four
D. five
E. six
Answer: E
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
114. How many sigma bonds are present in the following compound?
A. 20
B. 22
C. 24
D. 25
E. 27
Answer: E
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
115. The sigma bond that is part of C=N in the following compound results from the overlap of which orbitals?
A. sp2–sp2
B. sp–sp
C. sp2–sp3
D. sp3–sp3
E. sp3–sp2
Answer: A
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
116. The bonds indicated by the arrow in the following compound results from the overlap of which orbitals?
A. sp2–sp2
B. sp3–sp3
C. p–p
D. Both A and B
E. Both A and C
Answer: E
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
117. Which orbitals are involved in the C—O, sigma bond in acetone, shown below?
A. Csp2—Osp2
B. Csp3—Osp3
C. Csp—Osp
D. Cp—Op
E. Csp—Op
Answer: A
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
118. Which of the following best describes the orbitals involved in the formation of the C=O bond in acetone, shown below?
A.
B.
C.
D.
E.
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
119. The C—H bond in the methyl cation, CH3+, results from the overlap of which orbitals?
A. sp3–sp2
B. sp3–sp3
C. sp2–s
D. sp3–p
E. p–s
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
120. The lone pair of electrons in the methyl anion, CH3—, resides in which orbital?
A. s2
B. p
C. sp
D. sp3
E. sp2
Answer: D
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: medium
121. What is the hybridization state of the indicated atoms in the following compound?
A. I – sp ; II – sp2 ; III – sp3 ; IV – sp2
B. I – sp2 ; II – sp ; III – sp2 ; IV – sp3
C. I – sp3 ; II – sp2 ; III – sp ; IV – sp2
D. I – sp2 ; II – sp3 ; III – sp2 ; IV – sp
E. I – sp2 ; II – sp2 ; III – sp2 ; IV – sp3
Answer: B
Learning Objective: 1.9 Explain how pi bonds an sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Hard
122. The carbon and oxygen atoms in carbon monoxide are connected by which type of bond(s)?
A. a sigma (s) bond
B. two sigma (s) bonds
C. a pi (p) bond
D. two pi (p) bonds
E. both A and D
Answer: E
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
123. The N—H bond in the following compound is a _____ and is formed from the _____.
A. σ bond; sp2 – s orbital overlap
B. σ bond; sp3 – s orbital overlap
C. π bond; sp3 – s orbital overlap
D. π bond; sp2 – p orbital overlap
E. π bond; p – p orbital overlap
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
124. Which is the shortest bond in the following compound?
A. I
B. II
C. III
D. IV
E. I and III have the same length
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
125. Which of the following compounds contains the shortest carbon–carbon bond?
A. I
B. II
C. III
D. IV
E. All of these
Answer: D
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
126. Compare the bond length and strength for the following compounds.
A. the shortest and strongest bond is found in compound I
B. the shortest and strongest bond is found in compound II
C. the shortest and weakest bond is found in compound I
D. the shortest and weakest bond is found in compound II
E. the bonds are of identical length and strength
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
127. Which is the longest C—C bond in the following compound?
A. I
B. II
C. III
D. I and III
E. All of these
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
128. Rank the indicated C—C bonds in increasing order of bond length.
A. I < II < III
B. II < III < I
C. III < I< II
D. II < I< III
E. I < III< II
Answer: D
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Medium
129. Identify the compound with the strongest carbon – nitrogen bond.
A. CH3CH2CH=NH
B. CH3CH2NH2
C. CH3CH2C≡N
D. The length of the carbon-nitrogen bonds are the same
Answer: C
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
130. Identify the compound with the longest carbon – nitrogen bond.
A. CH3CH2CH=NH
B. CH3CH2NH2
C. CH3CH2C≡N
D. The length of the carbon-nitrogen bonds are the same
Answer: B
Learning Objective: 1.9 Explain how pi bonds and sp3, sp2, and sp hybrid orbital sets are formed
Difficulty: Easy
131. The molecular geometry of carbon tetrachloride, CCl4, is _________ .
A. tetrahedral
B. trigonal planar
C. trigonal pyramidal
D. square planar
E. linear
Answer: A
Learning Objective: 1.10 Describe VSEPR theory
Difficulty: Easy
132. Which of the following compounds have trigonal planar molecular geometry?
A. I
B. II
C. III
D. IV
E. I and IV
Answer: A
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Easy
133. Which of the following compounds have trigonal pyramidal molecular geometry?
A. I
B. II
C. III
D. IV
E. I and IV
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Easy
134. Which of the following compounds have bent molecular geometry?
A. I
B. II
C. III
D. IV
E. I and IV
Answer: B
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
135. Which of the following compounds have trigonal planar molecular geometry?
A. I, II and III
B. II and III
C. III and V
D. V only
E. All of these
Answer: C
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
136. Which of the following compounds have tetrahedral electron geometry?
A. I, II and III
B. I, II, IV and V
C. III and IV and V
D. IV and V
E. All of these
Answer: B
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
137. Which of the following compounds have trigonal planar electron geometry?
A. I, II and III
B. I, II, IV and V
C. III and IV and V
D. II and III
E. All of these
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
138. What is the molecular geometry at the central atom in CH2Br2?
A. trigonal planar
B. trigonal pyramidal
C. square planar
D. tetrahedral
E. None of these
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
139. What is the molecular geometry at the central atom in Cl2CO?
A. trigonal planar
B. trigonal pyramidal
C. square planar
D. tetrahedral
E. bent
Answer: A
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
140. What is the molecular geometry at the nitrogen atom in the following compound?
A. trigonal planar
B. trigonal pyramidal
C. linear
D. tetrahedral
E. bent
Answer: E
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
141. Which compound does not have a linear molecular geometry?
A. CO2
B. H2O
C. BeCl2
D. HCN
E. C2H2
Answer: B
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
142. What is the approximate bond angle around the indicated carbon atom?
A. 600
B. 900
C. 109.50
D. 1200
E. 1800
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Easy
143. What is the approximate bond angle around the indicated carbon atom?
A. 600
B. 900
C. 109.50
D. 1200
E. 1800
Answer: E
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Easy
144. What is the approximate bond angle around the nitrogen atom?
A. 900
B. 109.50
C. 1200
D. 1800
E. 1000
Answer: C
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
145. What is the approximate bond angle around sulfur atom in Cl2CO?
A. 900
B. 109.50
C. 1050
D. 1200
E. 1800
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
146. What is the hybridization state and approximate bond angle around the carbon atom in HCN?
A. sp2, 1200
B. sp, 1800
C. sp3, 109.50
D. sp3, 1200
E. sp, 1200
Answer: B
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
147. What is the hybridization state and approximate bond angle around nitrogen in the following compound?
A. sp2, 109.5°
B. sp2, 107°
C. sp3, 109.5°
D. sp3, 1070
E. sp2, 1200
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
148. What is the hybridization state and approximate bond angle around sulfur in the following compound?
A. sp2, 109.5°
B. sp3, 109.5°
C. sp3, 107°
D. sp3, 1050
E. sp2, 1050
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Hard
149. What is the hybridization state and molecular geometry around the sulfur atom in SO3?
A. sp2, tetrahedral
B. sp2, trigonal planar
C. sp3, tetrahedral
D. sp3, trigonal pyramidal
E. sp2, trigonal pyramidal
Answer: B
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Hard
150. What is the hybridization state and molecular geometry around the carbon atom in CO2?
A. sp, linear
B. sp2, trigonal planar
C. sp3, tetrahedral
D. sp3, trigonal pyramidal
E. sp2, trigonal pyramidal
Answer: A
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
151. What are the hybridization state, molecular geometry and approximate bond angle for the methyl cation, CH3+?
A. sp2, tetrahedral, 1090
B. sp2, trigonal planar, 1200
C. sp3, tetrahedral, 109.50
D. sp3, trigonal pyramidal, 1200
E. sp2, trigonal pyramidal, 1800
Answer: B
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
152. What are the hybridization state, molecular geometry and approximate bond angle for the methyl anion, CH3—?
A. sp2, tetrahedral, 1090
B. sp2, trigonal planar, 1200
C. sp3, tetrahedral, 109.50
D. sp3, trigonal pyramidal, <109.50
E. sp2, trigonal pyramidal, 1800
Answer: D
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Medium
153. Draw the Lewis structure for SOCl2 and predict the hybridization state, molecular geometry and approximate bond angle around the central atom.
Answer:
sp3, trigonal pyramidal, 1070
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Hard
154. Draw the Lewis structure for HCOOH and predict the hybridization state, molecular geometry and approximate bond angle around the central atom.
Answer:
sp2, trigonal planar, 1200
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Hard
155. Following is the structure for Propranolol, and antihypertensive drug. What are the hybridization state, molecular geometry and approximate bond angle at the indicated nitrogen and oxygen atom in Propranolol?
Answer:
N: sp3, trigonal pyramidal, 1070
O: sp3, bent, 1050
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Hard
156. What are the hybridization state, molecular geometry and approximate bond angle at each nitrogen atom in the following compound?
Answer:
N(I): sp2, bent, 1200
N(II): sp2, trigonal planar, 1200
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Hard
157. Tryptophan is an essential amino acid important in the synthesis of the neurotransmitter serotonin in the body. What are the hybridization state, molecular geometry and approximate bond angle at the indicated carbon and nitrogen atoms?
Answer:
C(I): sp2, trigonal planar, 1200
C(II): sp3, tetrahedral, 109.50
C(III): sp2, trigonal planar, 1200
N(IV): sp3, trigonal pyramidal, 1070
Learning Objective: 1.10 Describe VSEPR Theory
Difficulty: Hard
158. Which of the following covalent bonds has the largest dipole moment?
A. C—C
B. C—H
C. C—O
D. N—H
E. H—F
Answer: E
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Easy
159. Which of the following compounds has no dipole moment?
A. CH4
B. NH3
C. HF
D. HCl
E. HBr
Answer: A
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Easy
160. Which of the following compounds has polar covalent bonds?
A. NH3
B. Na2O
C. H2
D. KF
E. Both A and C
Answer: A
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Easy
161. Which of the following compounds have a net dipole moment?
A. CBr4
B. CO2
C. CH4
D. H2O
E. C2H4
Answer: D
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Medium
162. Which of the following compounds does not have dipole moment?
A. HCl
B. NCl3
C. CO
D. BF3
E. All have dipole moment
Answer: D
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Medium
163. Which of the following compounds has a net dipole moment of zero?
A. I
B. II
C. III
D. IV
E. V
Answer: A
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Medium
164. Which of the following compounds have a dipole moment?
A. II
B. III
C. II and III
D. I, II and III
E. II, III and IV
Answer: E
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Medium
165. Rank the following compounds in order of decreasing dipole moment.
A. I > II > III
B. II > III > I
C. I > III > II
D. III > II > I
E. II > I > III
Answer: D
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Hard
166. Rank the following compounds in order of decreasing dipole moment.
A. I > II > III
B. II >III > I
C. I > III > II
D. III > I > II
E. II > I > III
Answer: D
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Medium
167. Which of the following compounds has a dipole moment? Indicate the direction of the dipole moment.
Answer: Compound I has no dipole moment. Compound II has a dipole moment.
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Medium
168. Which of the following compounds has a dipole moment? Indicate the direction of the dipole moment.
Answer: Compound II has no dipole moment. Compound I has a dipole moment.
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Medium
169. BF3 has a no dipole moment. Draw the Lewis structure for BF3, showing all nonbonding electrons. Indicate the polarity of every atom in the structure using δ+ and δ– notation. Explain why the molecule has no net dipole.
Answer:
The trigonal planar geometry of BF3 results in the cancellation of individual bond dipoles, producing a net molecular dipole of zero.
Learning Objective: 1.11 Describe how dipole moment is used in calculating the ionic character of a bond
Difficulty: Easy
170. Which of the intermolecular forces listed below is generally considered the strongest?
A. London dispersion forces
B. fleeting dipole-dipole interactions
C. dipole-dipole interactions
D. hydrogen bonding
E. the vital force
Answer: D
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
171. Which intermolecular force is generally considered the weakest?
A. ion-dipole interactions
B. London dispersion forces
C. dipole-dipole interactions
D. hydrogen bonding
E. covalent bonding
Answer: B
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
172. Which intermolecular force is primarily responsible for base pairing, and stability, of the double helix in DNA?
A. ion-dipole interactions
B. London dispersion forces
C. dipole-dipole interactions
D. hydrogen bonding
E. covalent bonding
Answer: D
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
173. What is the strongest intermolecular force present in the following compound?
A. ion-dipole interactions
B. London dispersion forces
C. dipole-dipole interactions
D. hydrogen bonding
E. covalent bonding
Answer: D
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
174. What is the strongest intermolecular force present in the following compound?
A. ion-dipole interactions
B. London dispersion forces
C. dipole-dipole interactions
D. hydrogen bonding
E. covalent bonding
Answer: C
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Medium
175. Which of the following statements best explains the observation that hydrogen fluoride has the highest boiling point of all the hydrogen halides?
A. The fluorine in HF is the smallest atom for all of the halogens
B. Fluorine is the most electronegative of the atoms
C. Hydrogen fluoride can participate in hydrogen bonding
D. HF is very reactive and can react and dissolve glass
E. HF is a weak acid, and doesn’t completely dissociate
Answer: C
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Medium
176. Which of the following compounds have the greatest fleeting dipole interactions between like molecules?
A. I
B. II
C. III
D. IV
E. I, III and IV
Answer: D
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
177. Which of the following compounds have the highest boiling point?
A. I
B. II
C. III
D. IV
E. II and IV
Answer: B
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
178. Which of the following compounds have the lowest boiling point?
A. I
B. II
C. III
D. IV
E. II and IV
Answer: C
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
179. Which of the following compounds have the lowest boiling point?
A. CH3Cl
B. CH2Cl2
C. CH4
D. CHCl3
E. CCl4
Answer: C
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
180. Which of the following compounds have the lowest boiling point?
A. I
B. II
C. III
D. IV
E. I and III
Answer: C
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Medium
181. Rank the following compounds in decreasing order of boiling point.
A. III > I > IV > II
B. II > I > IV > III
C. III > I > II > IV
D. IV > II > I > III
E. I > III > II > IV
Answer: D
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Medium
182. Rank the following compounds in decreasing order of boiling point.
A. III > I > IV > II
B. II > IV > I > III
C. III > I > II > IV
D. IV > II > I > III
E. I > III > II > IV
Answer: B
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Hard
183. Rank the following compounds in decreasing order of boiling point.
A. III > I > IV > II
B. II > IV > III > I
C. III > I > II > IV
D. IV > II > I > III
E. I > III > II > IV
Answer: A
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Medium
184. Which of the following compounds has a higher boiling point? Explain why.
Answer: Compound II has a higher boiling point than compound I. Compound II has larger surface area that allows for stronger fleeting dipole-dipole interactions between molecules.
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Medium
185. Which of the following compounds has a higher boiling point? Explain why.
Answer: Compound I has a higher boiling point than compound II. Compound I has hydrogen bonding interactions between molecules. Compound II has dipole-dipole interactions that are weaker than hydrogen bonding interactions.
Learning Objective: 1.12 Describe the basic nature of all intermolecular forces
Difficulty: Easy
186. Which of the following compounds is most soluble in water?
A. I
B. II
C. III
D. IV
E. II and III
Answer: B
Learning Objective: 1.13 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility
Difficulty: Easy
187. Which of the following compounds is most soluble in butane, CH3CH2CH2CH3?
A. I
B. II
C. III
D. IV
E. II and III
Answer: A
Learning Objective: 1.13 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility
Difficulty: Medium
188. For soap to remove and dissolve oil in water, what molecular features are needed?
A. one end of the molecule must be polar
B. the compound must contain oxygen atoms
C. one end of the molecule must be nonpolar
D. Both A and C
E. All A, B and C
Answer: D
Learning Objective: 1.13 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility
Difficulty: Medium
189. Amino acids are the building blocks of proteins. Which statement best describes the physical properties of the following amino acid?
A. high melting points and low solubility in water
B. large dipole moments and no hydrogen bonding
C. high melting points and large dipole moments
D. low solubility in water and small dipole moments
E. small dipole moments and are hydrophobic
Answer: C
Learning Objective: 1.13 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility
Difficulty: Medium
190. Sugars, an example of which is shown below, tend to be very soluble in water. Explain why.
Answer: Favorable hydrogen bonding between the sugar and water readily occurs as both contain O–H groups capable of hydrogen bonding.
Learning Objective: 1.13 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility
Difficulty: Medium
191. Describe how soaps function as cleaning agents.
Answer: Soaps form clusters called micelles. The polar groups of the soaps form the surface of the micelle and hydrogen bond to the surrounding water. The interior of the micelle is composed of the nonpolar, hydrophobic portions of the soap molecules. Grease and dirt are nonpolar and have limited solubility in water. In soapy water however, grease and dirt will dissolve in the nonpolar interior of the soap micelles, which in turn are soluble in the water.
Learning Objective: 1.13 Compare the actions of soap and dry cleaning in removing oil or grease from clothing, including a statement of the basic principle involved in solubility
Difficulty: Medium
