Chapter 01 - Structure and Bonding
1. Give the ground-state electron configuration for carbon (atomic number 6).
1s22s22px12py1 or 1s22s22p2
2. Give the ground-state electron configuration for fluorine (atomic number 9).
ANSWER:
POINTS: 1
1s22s22px2 2py2 2pz1 or 1s22s22p5
3. Give the ground-...
,Chapter 01 - Structure and Bonding
1. Give the ground-state electron configuration for carbon (atomic number 6).
ANSWER: 1s22s22px12py1 or 1s22s22p2
POINTS: 1
2. Give the ground-state electron configuration for fluorine (atomic number 9).
ANSWER: 1s22s22px2 2py2 2pz1 or 1s22s22p5
POINTS: 1
3. Give the ground-state electron configuration for magnesium (atomic number 12).
ANSWER: 1s22s22p63s2
POINTS: 1
4. How many electrons does silicon have in its valence shell?
ANSWER: four
POINTS: 1
Exhibit 1-1
Write valid Lewis (electron-dot) structures for each formula below. Show all electrons as dots and show all non-bonding
electrons.
5. C2Cl4 tetrachloroethylene
ANSWER:
POINTS: 1
6. CO2 carbon dioxide
ANSWER:
POINTS: 1
7. CH4O methanol
ANSWER:
POINTS: 1
Exhibit 1-2
Consider the structure of urea, shown below, to answer the following question(s).
8. Refer to Exhibit 1-2. Fill in any non-bonding valence electrons that are missing from the line-bond structure.
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,Chapter 01 - Structure and Bonding
ANSWER:
POINTS: 1
9. Refer to Exhibit 1-2. The carbon atom in urea is:
3
a. sp hybridized
2
b. sp hybridized
c. sp hybridized
d. not hybridized
ANSWER: b
POINTS: 1
10. Refer to Exhibit 1-2. The predicted NH2−C=O bond angle in urea is:
a. 109.5°
b. 120°
c. 180°
d. not predictable
ANSWER: b
POINTS: 1
Exhibit 1-3
Determine the hybridization for the indicated atoms in each structure below.
11. Refer to Exhibit 1-3. The hybridization of this oxygen atom (A) is ______.
ANSWER: 2
sp
POINTS: 1
12. Refer to Exhibit 1-3. The hybridization of this oxygen atom (B) is ______.
ANSWER: sp3
POINTS: 1
13. Refer to Exhibit 1-3. The hybridization of this carbon atom (C) is ______.
ANSWER: sp3
POINTS: 1
14. Refer to Exhibit 1-3. The hybridization of this carbon atom (D) is ______.
ANSWER: sp
POINTS: 1
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, Chapter 01 - Structure and Bonding
15. The molecular formula C2H4O can be converted into three-line bond (Kekulé) structures that are consistent with
valence rules.
a. b. c. d.
a. Which one of the Kekulé structures is not consistent with valence rules?
b. Explain why the structure you chose in part a is not consistent with valence rules.
ANSWER: a. d
The carbon bonded to the oxygen atom in structure d is pentavalent; it has 10 valence
b. electrons. Carbon can only have eight valence electrons. In addition, the other carbon
has only six valence electrons when it would prefer to have eight.
POINTS: 1
16. The original question was combined with #15. This placeholder question is here to maintain the integrity of the
numbering system between the printed copy and ExamView. Therefore, it has been marked "do not use on test" in
ExamView's question information dialog. As a result, this placeholder question is automatically prevented from being
chosen as a test question.
ANSWER: Answer not provided.
POINTS: 1
17. Convert the following structure to a skeletal drawing and give its molecular formula.
ANSWER:
Molecular formula: C5H7Br
POINTS: 1
18. Draw an orbital picture for acetylene, C 2H2. Clearly label each bond type and indicate the type of orbitals involved in
each bond.
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