Name ___________________________
Date ___________________
Class __________________
IONS
7.1
Section Review
Objectives
• Determine the number of valence electrons in an atom of a representative
element
• Explain the octet rule
• Describe how cations form
• Explain how anions form
Vocabulary
• valence electrons
• electron dot structures
• octet rule
• halide ions
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
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Elements within the same group of the periodic table behave
1
similarly because they have the same number of
2
1.
2.
. The
number of a representative element indicates how many
3.
valence electrons that element has. Diagrams that show valence
4.
3
5.
electrons as dots are called
. Gilbert Lewis’s
4
states
that in forming compounds, atoms tend to achieve the electron
6.
configuration of a noble gas.
7.
The transfer of valence electrons produces positively charged
5
ions, or
, and negatively charged ions called
cations of Group 1A elements always have a charge of
6
7
. The
9.
.
10.
8
are produced when atoms of the elements in Group 7A
9
an electron. For transition metals, the
10
8.
of cations
may vary.
Chapter 7 Ionic and Metallic Bonding
155
Name ___________________________
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. The chlorine atom gains seven electrons when it becomes an ion.
________ 12. The chemical properties of an element are largely determined by the
number of valence electrons the element has.
________ 13. Atoms acquire the stable electron structure of a noble gas by losing
electrons.
________ 14. An atom of an element in Group 1A has seven valence electrons.
________ 15. Among the Group 1A and 2A elements, the group number of each
element is equal to the number of valence electrons in an atom of
that element.
________ 16. Sulfur and magnesium both have two valence electrons.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. ions that are produced when halogens gain electrons
________ 18. valence electron
b. a depiction of valence electrons around the symbol
of an element
________ 19. octet rule
c. has the electron configuration of argon
________ 20. cations
d. an electron in the highest occupied energy level of
an element’s atom
________ 21. anions
e. Atoms in compounds tend to have the electron
configuration of a noble gas.
________ 22. halide ions
f. atoms or groups of atoms with a negative charge
________ 23. chloride ion
g. atoms or groups of atoms with a positive charge
Part D Questions and Problems
Answer the following in the space provided.
24. Write the electron dot structures for the following atoms.
a. silicon
b. rubidium
c. barium
156
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________ 17. electron dot structure
Name ___________________________
Date ___________________
Class __________________
25. State the number of electrons lost or gained in forming each of these ions.
Name the ions and tell whether it is an anion or a cation.
a. Mg2!
c. Br"
b. Ca2!
d. Ag!
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26. Describe the formation of an ion from a metal and a nonmetal in terms of the octet rule.
Chapter 7 Ionic and Metallic Bonding
157
Name ___________________________
9.1
Date ___________________
Class __________________
NAMING IONS
Section Review
Objectives
• Determine the charges of monatomic ions by using the periodic table and write
the names of the ions
• Define a polyatomic ion and write the names and formulas of the most common
polyatomic ions
• Identify the two common endings for the names of most polyatomic ions.
Vocabulary
• monatomic ions
• polyatomic ions
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
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Ions that consist of a single atom are called
Metallic elements tend to
3
2
1.
ions.
electrons. Group 1A ions have a
4
charge, whereas Group 2A metals form ions with a
charge, and Group 3A metals form ions with a
5
charge.
6
from the group number. For example, the
Group 7A elements form ions with a charge of
8
Many of the
10
9
system
11
The names of most common polyatomic ions end in either
12
or
13
.
6.
8.
9.
10.
naming system.
Ions containing more than one atom are called
4.
7.
.
have more than one common ionic
charge. These ions are named using either the
or the
7
3.
5.
The charge of a Group A nonmetal ion is determined by
subtracting
2.
ions.
11.
12.
13.
Chapter 9 Chemical Names and Formulas
211
Name ___________________________
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 14. The names of polyatomic ions end in -ite or -ate.
________ 15. In polyatomic ions for which there is an -ite/-ate pair, the -ite ending will
always indicate one less oxygen atom than the -ate ending.
________ 16. Polyatomic ions are anions.
________ 17. The charge on Group A metal ions is determined by subtracting the
group number from 8.
________ 18. The Group 6A ions have a charge of 2!.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. negatively charged ions
________ 20. polyatomic ions
b. ions formed from single atoms
________ 21. cations
c. a traditional way of naming transition metal cations
________ 22. anions
d. positively charged ions
________ 23. classical naming system
e. ions formed from groups of atoms
Part D Questions and Problems
Answer the following in the space provided.
24. What is the charge on a typical ion for each of the following groups?
a. 1A
c. 7A
b. 6A
d. 2A
25. Write the name of each of the following polyatomic ions.
a. HCO3!
c. MnO4!
b. NH4"
d. OH!
26. How many electrons does the neutral atom gain or lose to form each of the
following ions?
212
a. Ca2"
c. I!
b. S2!
d. Mn3"
Core Teaching Resources
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________ 19. monatomic ions
Name ___________________________
7.2
Date ___________________
Class __________________
IONIC BONDS AND IONIC COMPOUNDS
Section Review
Objectives
• Explain the electrical charge of an ionic compound
• Describe three properties of ionic compounds
Vocabulary
• ionic compounds
• ionic bonds
• chemical formula
• formula unit
• coordination number
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
Anions and cations attract one another by means of
The forces of attraction that hold
3
1.
charged ions together in
2.
. Although they are composed
3.
of ions, ionic compounds are electrically
4
. The lowest whole-
4.
5
5.
number ratio of ions in an ionic compound is called a
6
Nearly all ionic compounds are solid
at room
temperature. Ionic compounds in general have very
8
melting temperatures. This is because the
9
7
attractive
.
6.
7.
8.
structure.
9.
Ionic compounds conduct an electric current when in the
10.
forces between the ions result in a very
10
state or dissolved in water.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. During the formation of the compound NaCl, one electron is
transferred from a sodium atom to a chlorine atom.
158
Core Teaching Resources
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ionic compounds are called
2
.
Name ___________________________
Date ___________________
Class __________________
________ 12. The coordination number of an ion is the number of ions of positive
charge that surround the ion in a crystal.
________ 13. The coordination number of the ion Na! in NaCl is 6.
________ 14. In forming an ionic compound, an atom of an element gains electrons.
________ 15. Ionic compounds cannot conduct electricity if they are dissolved in water.
Part C Matching
Match each description in Column B to the correct term in Column A.
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Column A
Column B
________ 16. ionic compounds
a. the number of ions of opposite charge surrounding
each ion in a crystal
________ 17. ionic bonds
b. compounds composed of cations and anions
________ 18. chemical formula
c. shows the kinds and numbers of atoms in the
smallest representative unit of a substance
________ 19. formula unit
d. lowest whole-number ratio of ions in an ionic
compound
________ 20. coordination number
e. the electrostatic forces of attraction binding
oppositely charged ions together
Part D Questions and Problems
Answer the following in the space provided.
21. List the characteristics of an ionic bond.
22. Explain the electrical conductivity of melted and of aqueous solutions of ionic
compounds using the characteristics of ionic compounds.
Chapter 7 Ionic and Metallic Bonding
159
Name ___________________________
Date ___________________
Class __________________
NAMING AND WRITING FORMULAS
FOR IONIC COMPOUNDS
9.2
Section Review
Objectives
• Apply the rules for naming and writing formulas for binary ionic compounds
• Apply the rules for naming and writing formulas for compounds with
polyatomic ions
Vocabulary
• binary compound
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1.
Binary ionic compounds are named by writing the name of
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the
1
followed by the name of the
binary compounds end in
3
2
2.
. Names of
4
. For example, NaI is
.
5
When a cation has more than one ionic charge, a
4.
5.
is used in the name.
Compounds with polyatomic ions whose names end in -ite
or -ate contain a polyatomic
6
that includes
7
.
In writing the formula of an ionic compound, the net ionic charge
must be
8
3.
6.
7.
8.
.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 9. The systematic name for baking soda (NaHCO3) is sodium
bicarbonate.
________ 10. In writing a formula for an ionic compound, the net ionic charge of
the formula must be zero.
Chapter 9 Chemical Names and Formulas
213
Name ___________________________
Date ___________________
Class __________________
________ 11. Anions that contain oxygen end in -ite or -ate.
________ 12. The cation name is placed first when naming ionic compounds.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 13. binary compounds
a. ions that consist of a single atom
________ 14. monatomic ions
b. ionic compounds composed of two elements
________ 15. polyatomic ions
c. Group B metals, many of which have more than one
common ionic charge
________ 16. transition metals
d. ions that consist of more than one atom
Part D Questions and Problems
Answer the following in the space provided.
17. Name the following compounds and tell what type of compound they are
(binary ionic or ionic with a polyatomic ion).
a. FeBr3
b. KOH
18. Write the formulas for the following compounds.
a. sodium chlorate
b. lead(II) phosphate
c. magnesium hydrogen carbonate
214
Core Teaching Resources
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c. Na2Cr2O7
Name ___________________________
Date ___________________
Class __________________
BONDING IN METALS
7.3
Section Review
Objectives
• Model the valence electrons of metal ions
• Describe the arrangement of atoms in a metal
• Explain the importance of alloys
Vocabulary
• metallic bonds
• alloys
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
Metals consist of closely packed
2
by a sea of
1
that are surrounded
. This arrangement constitutes the
3
4
conductivity of metals and helps explain why
5
metals are
packed in a
7
and
6
cubic, a
2.
3.
4.
. Metal atoms are commonly
5.
8
6.
cubic, or a
9
arrangement. When two or more elements, at least one of which
7.
is a metal, are mixed together, the resulting mixture is called
8.
an
10
.
9.
10.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. In a body-centered cubic structure, each atom has 12 neighbors.
________ 12. Metallic objects are formed from pure metals.
160
Core Teaching Resources
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bond. The electron mobility accounts for the excellent
1.
Name ___________________________
Date ___________________
Class __________________
________ 13. Metals that are good conductors of electricity are said to be ductile.
________ 14. Drifting valence electrons insulate cations from one another and
contribute to the malleability of a metal.
________ 15. Metals are good conductors of electricity because electrons can flow
freely in them.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 16. ductile
a. an alloy whose component atoms are different sizes
________ 17. metallic bonds
b. a mixture of two or more elements, at least one of which
is a metal
________ 18. alloy
c. can be hammered or forced into shapes
________ 19. malleable
d. can be drawn into wires
________ 20. interstitial alloy
e. the attraction of valence electrons for positive metal ions
Part D Questions and Problems
Answer the following in the space provided.
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21. Explain the physical properties of metals, using the theory of metallic bonding.
22. Explain why the properties of alloys are generally superior to their constituent
components.
Chapter 7 Ionic and Metallic Bonding
161