Chapter 9 Chemical Bonding: General Concepts


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Chapter 9 Chemical Bonding: General Concepts
Multiple Choice
Section 9.1 1. Sodium tends to form ions which have the electronic configuration of a noble gas. What is the
electronic configuration of the noble gas which the sodium ion mimics?
a. 1s2 b. 1s2 2p6 ! c. 1s2 2s2 2p6 d. 1s2 2s2 2p6 3s2 e. 1s2 2s2 2p6 3s2 3p6
Section 9.1 2. Bromine tends to form simple ions which have the electronic configuration of a noble gas. What
is the electronic configuration of the noble gas which the bromide ion mimics?
a. 1s2 2s2 2p6 3s2 3p6 3d10 4p6 b. 1s2 2s2 2p6 3s2 3p6 4p6 4d10 c. 1s2 2s2 2p6 3s2 3p6 4s2 4p6 ! d. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 e. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10
Section 9.3 16. The atoms in the nitrogen molecule, N2, are held together by
a. a single covalent bond b. a double covalent bond ! c. a triple covalent bond d. an ionic bond e. a magnetic dipole bond
Section 9.3 17. The atoms in the oxygen molecule, O2, are held together by
a. a single covalent bond ! b. a double covalent bond
c. a triple covalent bond d. an ionic bond e. a magnetic dipole bond
Section 9.3 18. The atoms in the hydrogen fluoride molecule are held together by
! a. a single covalent bond b. a double covalent bond c. a triple covalent bond d. an ionic bond
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e. a magnetic dipole bond
Section 9.3 19. The Lewis symbol for the carbon atom shows __ valence electrons. The number of bonds which
carbon usually forms in order to complete its valence shell and obey the octet rule is ___
a. 4, 1 b. 4, 2 c. 2, 4 d. 4, 3 ! e. 4, 4 Section 9.3 20. The Lewis symbol for the nitrogen atom shows __ valence electrons. The number of bonds which nitrogen usually forms in order to complete its valence shell and obey the octet rule is ___.
a. 5, 1 b. 5, 2 c. 3, 4 ! d. 5, 3 e. 5, 4

Section 9.3 23. Complete the Lewis structure for HClO3 from the skeletal template presented below by filling in the
bonds and the remaining valence electrons (those which are not in the bonds). If the valence shells are filled to the usual limit (maximum of 8), what is the sum of the absolute values of all the formal charges in the molecule?
O
H O Cl O
a. 0 b. 1 c. 2 d. 3 ! e. 4

Section 9.4 29. The compound shown immediately below is an example of

H OH

│ ║│

H—C—C—C—H





H

H

a. an alcohol
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! b. a ketone c. an acid d. a hydrocarbon e. an amine

Section 9.4 30. The compound shown immediately below is an example of

HOH H

│ ║││

H—C—C—C—C—H



│ │

H

H H

a. an alcohol b. an acid c. an amine ! d. a ketone e. a hydrocarbon

Section 9.4 31. The compound shown immediately below is an example of

HH O │ │║ H—C—C—C—H │ │ H H

a. an alcohol b. a ketone ! c. an aldehyde d. an acid e. an amine

Section 9.4 33. The compound shown immediately below is an example of

HH H │ ││ H—C—C—N—H │ │ H H

a. an alcohol b. a ketone c. an aldehyde d. an acid ! e. an amine
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Section 9.4 34. The compound shown immediately below is an example of
HHH H │ ││ │ H—C—C—C—N—H │ ││ H HH
a. an acid b. an alcohol c. an aldehyde ! d. an amine e. a ketone
Section 9.4 35. The compound shown immediately below is an example of
H H │ │ H—C—C—O—H │ │ H H
! a. an alcohol b. a ketone c. an aldehyde d. an acid e. an amine
Section 9.4 37. The compound shown immediately below is an example of
HH O │ │║ H—C—C—C—O—H │ │ H H
a. an alcohol b. a ketone c. an aldehyde ! d. an acid e. an amine
Section 9.5 39. Which one of the following bonds is the most polar one of the set?
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a. H—Br b. H—Cl ! c. H—F d. H—I e. H—N
Section 9.5 44. Which one of the following is the least electronegative element of the set presented?
a. F b. N c. C d. O ! e. H
Section 9.5 46. Which one of the following is the least electronegative element of the set presented?
a. N b. O c. Cl d. Br ! e. I
Section 9.6 47. Based on electronegativity considerations, which one of the following listed species should be the
strongest oxidizing agent?
a. Ne b. Kr c. Br2 ! d. Cl2 e. S
Section 9.8 53. The formal charge on the oxygen atom in the carbon monoxide molecule is
a. -2 b. -1 c. 0 ! d. +1 e. +2 55. The formal charge on the carbon atom in the carbonate ion is
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a. -2 ! b. 0
c. +1 d. +2 e. +4
Section 9.8 60. Complete the Lewis structure for HClO3 from the skeletal template presented below by filling in the
bonds and the remaining valence electrons (those which are not in the bonds). If the valence shells are filled to the usual limit (maximum of 8), what is the formal charge on the chlorine atom?
O H O Cl O a. -1 b. 0 c. +1 ! d. +2 e. +3
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Section 9.8 62. A student drew four possible Lewis structures for HBrO4

A. O │
H—O—Br═O │ O

B.

O



H—O—Br═O



O

C. O ║
H—O—Br═O ║ O

D. O │
H—O—Br—O │ O

Complete these Lewis structures presented above by filling in the remaining valence electrons (those which are not in the bonds). Based on these structures, the preferred structure would be the structure shown as ____ in which the sum of the absolute values of the formal charges on all the atoms is ____, _____

a. A, 4 b. B, 2 ! c. C, 0 d. D, 6 e. D, 0 Section 9.8 63. Draw a correct Lewis structure for CH2Cl2. the formal charge on the carbon atom is

Based on this Lewis structure, the calculated value for

! a. 0 b. +4 c. +2 d. -2 e. -4

Section 9.8 64. Draw a correct Lewis structure for H3C—NH2. Based on this Lewis structure, the calculated value
for the formal charge on the nitrogen atom is

a. -2 b. +3 c. -3 d. +2 ! e. 0

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Section 9.9 68. How many resonance structures, if any, can be drawn for the O3 molecule?
a. 1 (no resonance) ! b. 2
c. 3 d. 4 e. 5 Section 9.9 69. How many resonance structures, if any, can be drawn for the nitrate ion? a. 1 (no resonance) b. 2 ! c. 3 d. 4 e. 5
Section 9.9 71. How many resonance structures, if any, can be drawn for the BF3 molecule?
! a. 1 (no resonance) b. 2 c. 3 d. 4 e. 5
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Chapter 9 Chemical Bonding: General Concepts