Download 2011-2012 ACAD REVIEW SHEET Chapter 8

Name:
Date:
Period:
ACADEMIC Chapter 8 Review
Vocabulary
Define each term in a complete sentence.
 valence-shell electron pair
repulsion theory
 bond angle
 hybrid orbital



dipole
polar
nonpolar
Section 8-1
1. What is the molecular shape of ammonia, NH3? What are the bond angles in this
molecule? Draw the LEWIS structure of this molecule.
2. What is the molecular shape of BF3? What are the bond angles in this molecule?
Draw the LEWIS structure of this molecule.
3. What is the molecular shape of oxygen dichloride, OCl2? What is the bond angle
in this molecule? Draw the LEWIS structure of this molecule.
4. What is the molecular shape of CCl2F2? What are the bond angles in this
molecule? Draw the LEWIS structure of this molecule.
5. A molecule of hydrogen cyanide contains 1 hydrogen atom, 1 carbon atom, and 1
nitrogen atom. The carbon is bonded to the hydrogen atom and to the nitrogen
atom. Predict the bond angle in this molecule. Draw the LEWIS structure of this
molecule.
Section 8-2
6. Identify the following as polar or nonpolar. Draw the LEWIS structure for each.
Identify the molecular geometry for each. Write the bond angle for each. Write
the hybridization for each. NOTE: Molecular geometry and molecular shape are
the same thing.
a. HCl
e. C2Cl2
i. CF2O
b. N2
f. C2H4
j. NH2F
c. H2O
g. C2H2
k. SF2
d. CO2
h. C2H6
7. Write the diatomic elements. There are 7 of them.
8. How is bond polarity determined? How is molecular polarity determined? What
is the difference between the two?
9. Identify the following as a polar bond or a non-polar bond.
a. HCl
c. CO2
b. H2O
d. O2
Name:
Date:
Period:
ACADEMIC Chapter 8 Review
Vocabulary
Define each term in a complete sentence.
 valence-shell electron pair
repulsion theory
 bond angle
 hybrid orbital



dipole
polar
nonpolar
Section 8-1
1. What is the molecular shape of ammonia, NH3? What are the bond angles in this
molecule? Draw the LEWIS structure of this molecule.
(ANS: trigonal pyramidal, 107 (~109.5), ask Mr. Lee to draw the Lewis
Structure on the board)
2. What is the molecular shape of BF3? What are the bond angles in this molecule?
Draw the LEWIS structure of this molecule.
(ANS: trigonal planar, 120, ask Mr. Lee to draw the Lewis Structure on the
board)
3. What is the molecular shape of water, OCl2? What is the bond angle in this
molecule? Draw the LEWIS structure of this molecule.
(ANS: bent, 105 (~109.5), ask Mr. Lee to draw the Lewis Structure on the
board)
4. What is the molecular shape of CCl2F2? What are the bond angles in this
molecule? Draw the LEWIS structure of this molecule.
(ANS: tetrahedral, 109.5, ask Mr. Lee to draw the Lewis Structure on the board)
5. A molecule of hydrogen cyanide contains 1 hydrogen atom, 1 carbon atom, and 1
nitrogen atom. The carbon is bonded to the hydrogen atom and to the nitrogen
atom. Predict the bond angle in this molecule. Draw the LEWIS structure of this
molecule.
(ANS: linear, 180, ask Mr. Lee to draw the Lewis Structure on the board)
Section 8-2
6. Identify the following as polar or nonpolar. Draw the LEWIS structure for each.
Identify the molecular geometry for each. Write the bond angle for each. Write
the hybridization for each. NOTE: Molecular geometry and molecular shape are
the same thing.
a. HCl
(ANS: polar, ask Mr. Lee for the Lewis structure, linear, 180, need at
least three particles to determine hybridization)
b. N2
(ANS: nonpolar, ask Mr. Lee for the Lewis structure, linear, 180, need at
least three particles to determine hybridization)
c. H2O
(ANS: polar, ask Mr. Lee for the Lewis structure, bent, 105 (~109.5),
sp3 hybridized)
d. CO2
(ANS: nonpolar, ask Mr. Lee for the Lewis structure, linear, 180, sp
hybridized)
e. C2Cl2
(ANS: nonpolar, ask Mr. Lee for the Lewis structure, for each carbon is
linear, for each carbon is 180, sp hybridized)
f. C2H4
(ANS: nonpolar, ask Mr. Lee for the Lewis structure, for each carbon is
trigonal planar, for each carbon is 120, sp2 hybridized)
g. C2H2
(ANS: nonpolar, ask Mr. Lee for the Lewis structure, for each carbon is
linear, for each carbon is 180, sp hybridized)
h. C2H6
(ANS: nonpolar, ask Mr. Lee for the Lewis structure, for each carbon is
tetrahedral, for each carbon is 109.5, sp3 hybridized)
i. CF2O
(ANS: polar, ask Mr. Lee for the Lewis structure, for the carbon is trigonal
planar, for the carbon is 120, sp2 hybridized)
j. NH2F
(ANS: polar, ask Mr. Lee for the Lewis structure, for the nitrogen is
trigonal pyramidal, for the nitrogen is 107 (~109.5), sp3 hybridized)
k. SF2
(ANS: polar, ask Mr. Lee for the Lewis structure, for the sulfur is bent, for
the sulfur is 105 (~109.5), sp3 hybridized)
7. Write the diatomic elements. There are 7 of them.
(ANS: hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine
8. How is bond polarity determined? How is molecular polarity determined? What
is the difference between the two?
(ANS: bond polarity is determined by electronegativity difference; molecular
polarity is primarily determined by symmetry; the difference between the two is
that bond polarity is only between two particles and molecular polarity is over the
whole molecule)
9. Identify the following as a polar bond or a non-polar bond.
a. HCl
c. CO2
(ANS: polar covalent
(ANS: polar covalent
bond)
bond)
b. H2O
d. O2
(ANS: polar covalent
(ANS: nonpolar covalent
bond)
bond)