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Modern Chemistry • CHAPTER 6
HOMEWORK 6-5
(pp. 172–175)
VOCABULARY
Define.
1. double bond ________________________________________________________________________
__________________________________________________________________________________
2. a. triple bond ______________________________________________________________________
b. How is a triple bond shown? _______________________________________________________
3. resonance _________________________________________________________________________
__________________________________________________________________________________
4. resonance structures _________________________________________________________________
__________________________________________________________________________________
GRAPHIC ORGANIZER
On a separate sheet of paper, use Table 6-2 on page 173 to create a graph comparing bond length to
bond energy. Plot bond length on the x-axis (in pm) and bond energy on the y-axis (in kJ/mol).
Depict all the bonds shown in the table on your graph.
y
x
What does your graph show about the relationship between bond length and bond energy? Which bonds
are stronger—single, double, or triple?
STANDARDIZED TEST PREP
Circle the letter of the best answer.
H
H
C
C
H
H . This Lewis structure shows that
1. The Lewis structure for C2H4 is
a. the bonds between carbon and hydrogen are double bonds.
b. each hydrogen atom has two valence electrons.
c. the bond between the carbon atoms is a double bond.
d. the bond energies of the carbon-hydrogen bonds are higher than the bond energy of the
carbon-carbon bond.
2. Which is the correct Lewis structure for HCl?
a. H Cl
b. H
Cl
c. H
Cl
d. H Cl
Modern Chemistry
Copyright © by Holt, Rinehart and Winston. All rights reserved.
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CHAPTER 6
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• HOMEWORK 6-5
VOCABULARY
1. a covalent bond produced by the sharing of two pairs of electrons between two atoms; by two
side-by-side pairs of dots or by two parallel dashes
2. a. a covalent bond produced by the sharing of three pairs of electrons between two atoms
b. by three pairs of dots or three parallel dashes
3. bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
4. the “average” of two or more structures that represent the same molecule
GRAPHIC ORGANIZER
The graph should show that as bond length decreases, bond energy increases. Triple bonds are generally
stronger than single or double. Double bonds are stronger than single bonds.
STANDARDIZED TEST PREP
1. c
2. a
CHAPTER 6
• HOMEWORK 6-6
VOCABULARY
1. a compound composed of positive and negative ions that are combined so that the numbers of positive
and negative charges are equal
2. the simplest ratio of the compound’s combined ions that gives electrical neutrality
3. the simplest collection of atoms from which an ionic compound’s formula can be established
4. the ions in the crystal minimize their potential energy
5. one mole of an ionic crystalline compound is formed from gaseous ions
SKILL BUILDER
Sample response: The forces of attraction between molecules are weaker than the forces of ionic bonding.
Molecular compounds melt at lower temperatures than ionic compounds because of these weak bonds.
Ionic compounds have higher boiling points than molecular compounds because of their stronger bonds.
Molecular compounds vaporize at room temperature more easily than ionic compounds. Ionic compounds
are hard, but they are brittle. Many ionic compounds are soluble in water. When they are dissolved in
water, they are electrical conductors.
STANDARDIZED TEST PREP
1. d
2. c