,Chapter 1-Structure and Bonding:Acids and Bases
1. How many total valence electrons are represented in the following electron configuration?
1s22s22px2 2py2 2pz1 or 1s22s22p5
a. 1
b. 3
c. 5
d. 7
e. 9
ANS: D
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
ANS:
3. The structure of urea is shown below. Fill in any nonbonding valence electrons that are missing from
the line-bond structure.
ANS:
Instructions: Determine the hybridization for the indicated atoms in each structure below.
4. Refer to instructions. The hybridization of carbon atom A is _____.
ANS: sp2
,5. Refer to instructions. The hybridization of carbon atom B is _____.
ANS:
sp
6. How many nonbonding electron pairs are in the structure shown below?
a. 2
b. 4
c. 6
d. 8
e. none of these
ANS: B
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.
ANS: D
, 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.
ANS:
9. Refer to instructions. Contains only one sp3 hybridized carbon and two sp2 hybridized carbons.
ANS:
10. Consider the formation of an sp2 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.
d. The hybrid orbitals produced can form bonds.
e. none of these
ANS: C
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
ANS: E
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
ANS: C
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
ANS: C
1. How many total valence electrons are represented in the following electron configuration?
1s22s22px2 2py2 2pz1 or 1s22s22p5
a. 1
b. 3
c. 5
d. 7
e. 9
ANS: D
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
ANS:
3. The structure of urea is shown below. Fill in any nonbonding valence electrons that are missing from
the line-bond structure.
ANS:
Instructions: Determine the hybridization for the indicated atoms in each structure below.
4. Refer to instructions. The hybridization of carbon atom A is _____.
ANS: sp2
,5. Refer to instructions. The hybridization of carbon atom B is _____.
ANS:
sp
6. How many nonbonding electron pairs are in the structure shown below?
a. 2
b. 4
c. 6
d. 8
e. none of these
ANS: B
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.
ANS: D
, 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.
ANS:
9. Refer to instructions. Contains only one sp3 hybridized carbon and two sp2 hybridized carbons.
ANS:
10. Consider the formation of an sp2 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.
d. The hybrid orbitals produced can form bonds.
e. none of these
ANS: C
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
ANS: E
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
ANS: C
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
ANS: C
