Chapter 6
Standardized Test Preparation
Preview
• Multiple Choice
• Short Answer
• Extended Response
Chapter 6
Standardized Test Preparation
Multiple Choice
1. A chemical bond results from the mutual attraction of
the nuclei for
A. electrons.
B. neutrons.
C. protons.
D. dipoles.
Chapter 6
Standardized Test Preparation
Multiple Choice
1. A chemical bond results from the mutual attraction of
the nuclei for
A. electrons.
B. neutrons.
C. protons.
D. dipoles.
Chapter 6
Standardized Test Preparation
Multiple Choice
2. A polar covalent bond is likely to form between two
atoms that
A. are similar in electronegativity.
B. are of similar size.
C. differ in electronegativity.
D. have the same number of electrons.
Chapter 6
Standardized Test Preparation
Multiple Choice
2. A polar covalent bond is likely to form between two
atoms that
A. are similar in electronegativity.
B. are of similar size.
C. differ in electronegativity.
D. have the same number of electrons.
Chapter 6
Standardized Test Preparation
Multiple Choice
3. The Lewis structure of HCN contains
A. one double bond and one single bond.
B. one triple bond and one single bond.
C. two single bonds.
D. two double bonds.
Chapter 6
Standardized Test Preparation
Multiple Choice
3. The Lewis structure of HCN contains
A. one double bond and one single bond.
B. one triple bond and one single bond.
C. two single bonds.
D. two double bonds.
Chapter 6
Standardized Test Preparation
Multiple Choice
4. According to VSEPR theory, the molecular geometry
for CH+3 is
A. tetrahedral.
B. trigonal-pyramidal.
C. bent or angular.
D. None of the above
Chapter 6
Standardized Test Preparation
Multiple Choice
4. According to VSEPR theory, the molecular geometry
for CH+3 is
A. tetrahedral.
B. trigonal-pyramidal.
C. bent or angular.
D. None of the above
Chapter 6
Standardized Test Preparation
Multiple Choice
5. Which molecule contains a double bond?
A. COCl2
B. C2H6
C. CF4
D. SF2
Chapter 6
Standardized Test Preparation
Multiple Choice
5. Which molecule contains a double bond?
A. COCl2
B. C2H6
C. CF4
D. SF2
Chapter 6
Standardized Test Preparation
Multiple Choice
6. Which molecule is polar?
A. CCl4
B. CO2
C. SO3
D. none of these
Chapter 6
Standardized Test Preparation
Multiple Choice
6. Which molecule is polar?
A. CCl4
B. CO2
C. SO3
D. none of these
Chapter 6
Standardized Test Preparation
Multiple Choice
7. What is the hybridization of the carbon atoms in C2H2?
A. sp
B. sp2
C. sp3
D. The carbon atoms do not hybridize in C2H2.
Chapter 6
Standardized Test Preparation
Multiple Choice
7. What is the hybridization of the carbon atoms in C2H2?
A. sp
B. sp2
C. sp3
D. The carbon atoms do not hybridize in C2H2.
Chapter 6
Standardized Test Preparation
Multiple Choice
8. Which of the following compounds is predicted to have
the highest boiling point?
A. HCl
B. CH3COOH (Note: the two oxygen atoms bond to
the carbon)
C. Cl2
D. SO2
Chapter 6
Standardized Test Preparation
Multiple Choice
8. Which of the following compounds is predicted to have
the highest boiling point?
A. HCl
B. CH3COOH (Note: the two oxygen atoms bond to
the carbon)
C. Cl2
D. SO2
Chapter 6
Standardized Test Preparation
Multiple Choice
9. An unknown substance is an excellent electrical
conductor in the solid state and is malleable. What type
of chemical bonding does this substance exhibit?
A. ionic bonding
B. molecular bonding
C. metallic bonding
D. cannot determine from the information given
Chapter 6
Standardized Test Preparation
Multiple Choice
9. An unknown substance is an excellent electrical
conductor in the solid state and is malleable. What type
of chemical bonding does this substance exhibit?
A. ionic bonding
B. molecular bonding
C. metallic bonding
D. cannot determine from the information given
Chapter 6
Standardized Test Preparation
Short Answer
10. What does the hybridization model help explain?
Chapter 6
Standardized Test Preparation
Short Answer
10. What does the hybridization model help explain?
Answer: Hybridization explains how the orbitals of an
atom become rearranged when the atom forms
covalent bonds.
Chapter 6
Standardized Test Preparation
Short Answer
11. Explain why ionic crystals are brittle.
Chapter 6
Standardized Test Preparation
Short Answer
11. Explain why ionic crystals are brittle.
Answer: Ionic crystals are brittle because shifting of the
layers of ions results in large repulsive forces that
cause the layers to part completely.
Chapter 6
Standardized Test Preparation
Extended Response
12. Naphthalene, C10H8, is a nonpolar molecule and has a boiling
point of 218°C. Acetic acid, CH3CO2H, is a polar molecule and
has a boiling point of 118°C. Which substance has the stronger
intermolecular forces? Briefly explain your answer.
Chapter 6
Standardized Test Preparation
Extended Response
12. Naphthalene, C10H8, is a nonpolar molecule and has a boiling
point of 218°C. Acetic acid, CH3CO2H, is a polar molecule and
has a boiling point of 118°C. Which substance has the stronger
intermolecular forces? Briefly explain your answer.
Answer: Naphthalene has the stronger intermolecular forces even
though it is nonpolar, because its boiling point is higher than that
of acetic acid. Boiling point is directly correlated to strength of
intermolecular forces; the stronger the intermolecular forces, the
more energy needed to break all the intermolecular forces, and
therefore the higher the boiling point. Naphthalene is so large
that its dispersion forces are greater than the sum of the
dispersion forces and hydrogen bonding in acetic acid.
Chapter 6
Standardized Test Preparation
Extended Response
13. Describe and explain the potential energy changes
that occur during the formation of a covalent bond.
Chapter 6
Standardized Test Preparation
Extended Response
13. Describe and explain the potential energy changes
that occur during the formation of a covalent bond.
Answer: There is a repulsive region at small bond distances, a
minimum well at an intermediate bond distance, and an
asymptotic region at large bond distances. The repulsive region
is due to the repulsion between the two positive nuclei at
distances where the nuclei are close to each other. The
asymptotic region is where the atoms are far apart and therefore
do not interact with each other. The potential energy decreases
as the atoms come closer together and are attracted to each
other. The minimum well is the region where the attractive forces
are balanced by the repulsive forces. This distance is the
equilibrium bond length.