,Chapter 01 - Structure and Bonding
1. How many total valence electrons are represented in the following electron configuration?
2 2 2 2 1 2 2 5
1s 2s 2px 2py 2pz or 1s 2s 2p
a. 1
b. 3
c. 5
d. 7
e. 9
ANSWER: d
POINTS: 1
Instructions: Write valid Lewis (electron-dot) structures for each formula below. Show all electrons as dots and show all
nonbonding electrons.
2. Write:
CH3CH2OH ethanol
ANSWER:
POINTS: 1
3. The structure of urea is shown below. Fill in any nonbonding valence electrons that are missing from the line-bond
structure.
ANSWER:
POINTS: 1
Instructions: Determine the hybridization for the indicated atoms in each structure below.
4. Refer to instructions. The hybridization of carbon atom A is _____.
ANSWER: sp2
POINTS: 1
5. Refer to instructions. The hybridization of carbon atom B is _____.
ANSWER: sp
POINTS: 1
6. How many nonbonding electron pairs are in the structure shown below?
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,Chapter 01 - Structure and Bonding
a. 2
b. 4
c. 6
d. 8
e. none of these
ANSWER: b
POINTS: 1
7. The molecular formula C2H4O can be converted into three-line bond (Kekulé) structures that are consistent with
valence rules. Which one of the following Kekulé structures is not consistent with valence rules?
a.
b.
c.
d.
ANSWER: d
POINTS: 1
Instructions: Propose a structure for a molecule that meets the following description.
8. Refer to instructions. Contains only two sp3 hybridized carbons and two sp hybridized carbons.
ANSWER:
POINTS: 1
3 2
9. Refer to instructions. Contains only one sp hybridized carbon and two sp hybridized carbons.
ANSWER:
POINTS: 1
2
10. Consider the formation of an sp hybrid orbital. Which of the following is true?
a. Four equivalent hybrid orbitals are produced.
b. One s and one p atomic orbital are involved.
c. One p atomic orbital remains unhybridized.
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, Chapter 01 - Structure and Bonding
d. The hybrid orbitals produced can form π bonds.
e. none of these
ANSWER: c
POINTS: 1
11. According to atomic theory:
a. the nucleus is positively charged.
b. the nucleus contains both charged and uncharged particles.
c. the electrons contribute very little to the total mass of the atom.
d. the electrons are located in the atomic space outside the nucleus.
e. all of these
ANSWER: e
POINTS: 1
12. In drawing the Lewis structure for an organic compound, the carbon atoms should always be shown with
a. lone pairs of electrons.
b. four single bonds.
c. eight total electrons.
d. a positive charge.
e. none of these
ANSWER: c
POINTS: 1
13. Covalent bonding
a. involves a transfer of electrons from one atom to another.
b. occurs when atoms share all their valence electrons.
c. occurs when unpaired valence electrons are shared between atoms.
d. occurs when nonvalence electrons are shared between atoms.
e. none of these
ANSWER: c
POINTS: 1
14. Which of the following best represents the shape of a 2p atomic orbital of carbon?
A
B
C
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1. How many total valence electrons are represented in the following electron configuration?
2 2 2 2 1 2 2 5
1s 2s 2px 2py 2pz or 1s 2s 2p
a. 1
b. 3
c. 5
d. 7
e. 9
ANSWER: d
POINTS: 1
Instructions: Write valid Lewis (electron-dot) structures for each formula below. Show all electrons as dots and show all
nonbonding electrons.
2. Write:
CH3CH2OH ethanol
ANSWER:
POINTS: 1
3. The structure of urea is shown below. Fill in any nonbonding valence electrons that are missing from the line-bond
structure.
ANSWER:
POINTS: 1
Instructions: Determine the hybridization for the indicated atoms in each structure below.
4. Refer to instructions. The hybridization of carbon atom A is _____.
ANSWER: sp2
POINTS: 1
5. Refer to instructions. The hybridization of carbon atom B is _____.
ANSWER: sp
POINTS: 1
6. How many nonbonding electron pairs are in the structure shown below?
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,Chapter 01 - Structure and Bonding
a. 2
b. 4
c. 6
d. 8
e. none of these
ANSWER: b
POINTS: 1
7. The molecular formula C2H4O can be converted into three-line bond (Kekulé) structures that are consistent with
valence rules. Which one of the following Kekulé structures is not consistent with valence rules?
a.
b.
c.
d.
ANSWER: d
POINTS: 1
Instructions: Propose a structure for a molecule that meets the following description.
8. Refer to instructions. Contains only two sp3 hybridized carbons and two sp hybridized carbons.
ANSWER:
POINTS: 1
3 2
9. Refer to instructions. Contains only one sp hybridized carbon and two sp hybridized carbons.
ANSWER:
POINTS: 1
2
10. Consider the formation of an sp hybrid orbital. Which of the following is true?
a. Four equivalent hybrid orbitals are produced.
b. One s and one p atomic orbital are involved.
c. One p atomic orbital remains unhybridized.
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, Chapter 01 - Structure and Bonding
d. The hybrid orbitals produced can form π bonds.
e. none of these
ANSWER: c
POINTS: 1
11. According to atomic theory:
a. the nucleus is positively charged.
b. the nucleus contains both charged and uncharged particles.
c. the electrons contribute very little to the total mass of the atom.
d. the electrons are located in the atomic space outside the nucleus.
e. all of these
ANSWER: e
POINTS: 1
12. In drawing the Lewis structure for an organic compound, the carbon atoms should always be shown with
a. lone pairs of electrons.
b. four single bonds.
c. eight total electrons.
d. a positive charge.
e. none of these
ANSWER: c
POINTS: 1
13. Covalent bonding
a. involves a transfer of electrons from one atom to another.
b. occurs when atoms share all their valence electrons.
c. occurs when unpaired valence electrons are shared between atoms.
d. occurs when nonvalence electrons are shared between atoms.
e. none of these
ANSWER: c
POINTS: 1
14. Which of the following best represents the shape of a 2p atomic orbital of carbon?
A
B
C
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