Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
80 Chemistry: Matter and Change
Solving Problems: A Chemistry Handbook
SOLVING PROBLEMS:
A CHEMISTRY HANDBOOK
CHAPTER 8
such as oxygen, the intermolecular force can be quite strong and is
called hydrogen bonding. Such covalent substances have relatively
high boiling points for their molecular size. In some covalent substances, the atoms are connected in large networks of bonds. Such
substances, called covalent network solids, are very hard and have
very high melting points.
Practice Problems
13. Use the electronegativity values in Figure 9-15 in your textbook
to determine whether the following molecules have polar or
nonpolar bonds. Apply the VSEPR model to determine the
shape of each molecule. Then state whether the molecule as a
whole is polar or nonpolar.
a. SiF 4
c. H 2 S
b. PCl 3
d. CH 3 Cl
Chapter 8 Review
14. Why do atoms tend to bond?
15. Define covalent bond.
16. What is the difference between a sigma bond and a pi bond?
How many of each type of bond are found in a triple bond?
17. What is bond dissociation energy?
18. What kind of reaction occurs when a greater amount of energy
is required to break the existing bonds in the reactants than is
released when the new bonds form in the products?
19. State the rules for naming binary molecular compounds.
20. State the steps used to draw a Lewis structure.
21. Explain when the condition called resonance occurs.
22. What is the VSEPR model used to determine?
23. Define hybridization.
24. When is a bond polar? When is a molecule polar?
80 Chemistry: Matter and Change
Solving Problems: A Chemistry Handbook
SOLVING PROBLEMS:
A CHEMISTRY HANDBOOK
CHAPTER 8
such as oxygen, the intermolecular force can be quite strong and is
called hydrogen bonding. Such covalent substances have relatively
high boiling points for their molecular size. In some covalent substances, the atoms are connected in large networks of bonds. Such
substances, called covalent network solids, are very hard and have
very high melting points.
Practice Problems
13. Use the electronegativity values in Figure 9-15 in your textbook
to determine whether the following molecules have polar or
nonpolar bonds. Apply the VSEPR model to determine the
shape of each molecule. Then state whether the molecule as a
whole is polar or nonpolar.
a. SiF 4
c. H 2 S
b. PCl 3
d. CH 3 Cl
Chapter 8 Review
14. Why do atoms tend to bond?
15. Define covalent bond.
16. What is the difference between a sigma bond and a pi bond?
How many of each type of bond are found in a triple bond?
17. What is bond dissociation energy?
18. What kind of reaction occurs when a greater amount of energy
is required to break the existing bonds in the reactants than is
released when the new bonds form in the products?
19. State the rules for naming binary molecular compounds.
20. State the steps used to draw a Lewis structure.
21. Explain when the condition called resonance occurs.
22. What is the VSEPR model used to determine?
23. Define hybridization.
24. When is a bond polar? When is a molecule polar?