Name ___________________________
Chapter 6
Class ___________________
Date _____________
Chemical Bonds
Section 6.1 Ionic Bonding
(pages 158–164)
This section describes the formation of ionic bonds and the properties of ionic
compounds.
Reading Strategy
(page 158)
Sequencing As you read, complete the concept map to show what
happens to atoms during ionic bonding. For more information on this
Reading Strategy, see the Reading and Study Skills in the Skills and
Reference Handbook at the end of your textbook.
loses
electrons
to
Atom
gains
electrons
to
Stable Electron Configurations (page 158)
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1. Describe the type of electron configuration that makes an atom
stable and not likely to react.
2. Describe an electron dot diagram.
Ionic Bonds
(pages 159–161)
3. Some elements achieve stable electron configurations through the
transfer of
between atoms.
4. By losing one valence electron, a sodium atom achieves the same
electron arrangement as an atom of
.
5. Circle the letter that states the result of a sodium atom transferring
an electron to a chlorine atom.
a. Each atom ends up with a more stable electron arrangement.
b. The sodium atom becomes more stable, but the chlorine atom
becomes less stable.
c. The chlorine atom becomes more stable, but the sodium atom
becomes less stable.
d. Each atom ends up with a less stable electron arrangement.
6. Is the following sentence true or false? An ion is an atom that has a
net positive or negative electric charge.
7. An ion with a negative charge is called a(n)
.
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Name ___________________________
Chapter 6
Class ___________________
Date _____________
Chemical Bonds
8. An ionic bond forms when
are transferred
from one atom to another.
9. Is the following sentence true or false? The lower the ionization
energy, the easier it is to remove an electron from an atom.
Ionic Compounds (pages 161–164)
10. Circle the letter of each piece of information provided by the
chemical formula of an ionic compound.
a. which elements the compound contains
b. the charge on each ion in the compound
c. how the ions are arranged in the compound
d. the ratio of ions in the compound
11. Circle the letter of the correct answer. The formula for magnesium
chloride is MgCl2. The charge on the magnesium ion is 2⫹. What is
the charge on each chloride ion?
a. 2⫺
b. 1⫺
c. 0
d. 1⫹
Clⴚ
Naⴙ
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.
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12. Look at the arrangement of ions in a sodium chloride crystal.
How many sodium ions surround each chloride ion in this
three-dimensional structure?
a. 3
b. 4
c. 6
d. 8
13. The shape of an ionic crystal depends on
14. Identify two factors that determine the arrangement of ions in an
ionic crystal.
a.
b.
15. Is the following sentence true or false? The attractions among ions
within a crystal lattice are weak.
Name ___________________________
Chapter 6
Class ___________________
Date _____________
Chemical Bonds
Section 6.2 Covalent Bonding
(pages 165–169)
This section discusses the formation of covalent bonds and the factors that
determine whether a molecule is polar or nonpolar. It also discusses
attractions between molecules.
Reading Strategy (page 165)
Relating Text and Visuals As you read the section, look closely at
Figure 9. Complete the table by describing each type of model shown.
For more information on this Reading Strategy, see the Reading and
Study Skills in the Skills and Reference Handbook at the end of
your textbook.
Molecular Models
Model
Description
Electron dot
Structural formula
Space-filling
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
Electron cloud
Covalent Bonds
(pages 165–167)
1. Describe a covalent bond.
2. Circle the letters of molecular models that show orbitals of atoms
overlapping when a covalent bond forms.
a. electron dot
b. structural formula
c. space-filling
d. electron cloud
3. Describe a molecule.
4. Is the following sentence true or false? In a covalent bond, the atoms
are held together by the attractions between the shared electrons
and the protons in each nucleus.
5. Circle the correct answer. Nitrogen has five valence electrons. How
many pairs of electrons must two nitrogen atoms share in order for
each atom to have eight valence electrons?
a. zero
b. one
c. two
d. three
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Name ___________________________
Chapter 6
Class ___________________
Date _____________
Chemical Bonds
Unequal Sharing of Electrons
(pages 167–168)
6. In general, elements at the
of a group
have a greater attraction for electrons than elements at the
of a group have.
7. In a hydrogen chloride molecule, the shared electrons spend
more time near the
atom than near the
atom.
8. Describe a polar covalent bond.
9. When atoms form a polar covalent bond, the atom with the greater
attraction for electrons has a partial
charge.
10. Is the following sentence true or false? In a molecule of a
compound, electrons are always shared equally by both atoms.
11. Circle the letter of each factor that determines whether a molecule
is polar or nonpolar.
a. the number of atoms in the molecule
b. the type of atoms in the molecule
c. the number of bonds in the molecule
d. the shape of the molecule
H2O
12. Compare the shapes of carbon dioxide and water molecules. Circle
the letter of the polar molecule.
a. carbon dioxide
b. water
13. Is the following sentence true or false? In a water molecule, the
hydrogen side of the molecule has a partial positive charge, and
the oxygen side has a partial negative charge.
Attraction Between Molecules
(page 169)
14. Water has a higher boiling point than carbon dioxide because
attractions between polar molecules are
than
attractions between nonpolar molecules.
15. Is the following sentence true or false? Attractions among
nonpolar molecules explain why nitrogen can be stored as a liquid
at low temperatures and high pressures.
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CO2