, Chapter 01 Test Bank: Structure and Bonding
Student: ___________________________________________________________________________
1. What is the ground-state electronic configuration of a carbon atom?
A. 1s2, 2s2, 2p5
B. 1s2, 2s2, 2p2
C. 1s2, 2s2, 2p6
D. 1s2, 2s2, 2p4
2. What is the ground-state electronic configuration of a fluorine atom?
A. 1s2, 2s2, 2p2
B. 1s2, 2s2, 2p3
C. 1s2, 2s2, 2p4
D. 1s2, 2s2, 2p5
3. What is the ground-state electronic configuration of a magnesium cation (Mg 2+)?
A. 1s2, 2s2, 2p6
B. 1s2, 2s2, 2p6, 3s1
C. C. 1s2, 2s2, 2p6, 3s2
D. D. 1s2, 2s2, 2p6, 3s2, 3p2
4. What is the ground-state electronic configuration of a chlorine anion (Cl —)?
A. 1s2, 2s2, 2p6
B. 1s2, 2s2, 2p6, 3s2, 3p6
C. C. 1s2, 2s2, 2p6, 3s2, 3p5
D. D. 1s2, 2s2, 2p6, 3s2, 3p4
01-1
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
,5. Which of the following statements about valence electrons is true?
A. They are the most tightly held electrons.
B. They do not participate in chemical reactions.
C. They are the outermost electrons.
D. They reveal the period number of a second-row element.
6. Which of the following statements about bonding is true?
A. Covalent bonds result from the transfer of electrons from one element to another.
B. Ionic bonds result from the transfer of electrons from a metal to a non-metal.
C. Ionic bonds result from the sharing of electrons between two non-metals.
D. Covalent bonds result from the sharing of electrons between two metals.
7. Which of the following would you expect to have ionic bonds?
A. CO
B. FBr
C. NF3
D. NaCl
8. Which of the following molecules has nonpolar covalent bonds?
A. HCl
B. N2
C. CHCl3
D. NO
9. Which of the following molecules contain both covalent and ionic bonds?
A. I, II
B. I, IV
C. II, III
D. II, IV
01-2
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
, 10. Arrange the following bonds in decreasing order of ionic character, putting the most ionic first.
A. I > II > III > IV
B. IV > II > I > III
C. IV > III > II > I
D. IV > II > III > I
11. Which of the following statements correctly describes the typical number of bonds for carbon, nitrogen, and oxygen in
most neutral organic molecules?
A. Carbon forms 4 covalent bonds, nitrogen forms 2 covalent bonds, and oxygen forms 3 covalent bonds.
B. Carbon forms 4 covalent bonds, nitrogen forms 3 covalent bonds, and oxygen forms 2 covalent bonds.
C. Carbon forms 4 covalent bonds, nitrogen forms 5 covalent bonds, and oxygen forms 2 covalent bonds.
D. Carbon forms 4 covalent bonds, nitrogen forms 5 covalent bonds, and oxygen forms 4 covalent bonds.
12. Which is not an acceptable Lewis structure for the anion CH2NCO—?
A. I
B. II
C. III
D. IV
13. Which of the following Lewis structures is correct?
A. I
B. II
C. III
D. IV
01-3
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
Student: ___________________________________________________________________________
1. What is the ground-state electronic configuration of a carbon atom?
A. 1s2, 2s2, 2p5
B. 1s2, 2s2, 2p2
C. 1s2, 2s2, 2p6
D. 1s2, 2s2, 2p4
2. What is the ground-state electronic configuration of a fluorine atom?
A. 1s2, 2s2, 2p2
B. 1s2, 2s2, 2p3
C. 1s2, 2s2, 2p4
D. 1s2, 2s2, 2p5
3. What is the ground-state electronic configuration of a magnesium cation (Mg 2+)?
A. 1s2, 2s2, 2p6
B. 1s2, 2s2, 2p6, 3s1
C. C. 1s2, 2s2, 2p6, 3s2
D. D. 1s2, 2s2, 2p6, 3s2, 3p2
4. What is the ground-state electronic configuration of a chlorine anion (Cl —)?
A. 1s2, 2s2, 2p6
B. 1s2, 2s2, 2p6, 3s2, 3p6
C. C. 1s2, 2s2, 2p6, 3s2, 3p5
D. D. 1s2, 2s2, 2p6, 3s2, 3p4
01-1
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
,5. Which of the following statements about valence electrons is true?
A. They are the most tightly held electrons.
B. They do not participate in chemical reactions.
C. They are the outermost electrons.
D. They reveal the period number of a second-row element.
6. Which of the following statements about bonding is true?
A. Covalent bonds result from the transfer of electrons from one element to another.
B. Ionic bonds result from the transfer of electrons from a metal to a non-metal.
C. Ionic bonds result from the sharing of electrons between two non-metals.
D. Covalent bonds result from the sharing of electrons between two metals.
7. Which of the following would you expect to have ionic bonds?
A. CO
B. FBr
C. NF3
D. NaCl
8. Which of the following molecules has nonpolar covalent bonds?
A. HCl
B. N2
C. CHCl3
D. NO
9. Which of the following molecules contain both covalent and ionic bonds?
A. I, II
B. I, IV
C. II, III
D. II, IV
01-2
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
, 10. Arrange the following bonds in decreasing order of ionic character, putting the most ionic first.
A. I > II > III > IV
B. IV > II > I > III
C. IV > III > II > I
D. IV > II > III > I
11. Which of the following statements correctly describes the typical number of bonds for carbon, nitrogen, and oxygen in
most neutral organic molecules?
A. Carbon forms 4 covalent bonds, nitrogen forms 2 covalent bonds, and oxygen forms 3 covalent bonds.
B. Carbon forms 4 covalent bonds, nitrogen forms 3 covalent bonds, and oxygen forms 2 covalent bonds.
C. Carbon forms 4 covalent bonds, nitrogen forms 5 covalent bonds, and oxygen forms 2 covalent bonds.
D. Carbon forms 4 covalent bonds, nitrogen forms 5 covalent bonds, and oxygen forms 4 covalent bonds.
12. Which is not an acceptable Lewis structure for the anion CH2NCO—?
A. I
B. II
C. III
D. IV
13. Which of the following Lewis structures is correct?
A. I
B. II
C. III
D. IV
01-3
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
