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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
ions.
1.
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.
The charge of a Group A nonmetal ion is determined by
subtracting
6
8
Many of the
10
.
9
system
naming system.
Ions containing more than one atom are called
or
13
.
6.
8.
9.
10.
11
The names of most common polyatomic ions end in either
12
4.
7.
have more than one common ionic
charge. These ions are named using either the
or the
7
3.
5.
from the group number. For example, the
Group 7A elements form ions with a charge of
2.
ions.
11.
12.
13.
Chapter 9 Chemical Names and Formulas
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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
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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.
Binary ionic compounds are named by writing the name of
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
the
1
followed by the name of the
binary compounds end in
3
2
1.
. Names of
4
. For example, NaI is
2.
.
5
When a cation has more than one ionic charge, a
4.
is used in the name.
5.
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
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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
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Name ___________________________
9.3
Date ___________________
Class __________________
NAMING AND WRITING FORMULAS
FOR MOLECULAR COMPOUNDS
Section Review
Objectives
• Interpret the prefixes in the names of molecular compounds in terms of their
chemical formulas
• Apply the rules for naming and writing formulas for binary molecular compounds
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 molecular compounds are composed of two
2
elements. The name of this type of compound ends in
Prefixes are used to show how many
3
of each element
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are present in a molecule of the compound. For example,
the name of As2S5 is
4
1.
.
2.
3.
4.
.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 5. Binary molecular compounds contain carbon.
________ 6. Charges must be balanced when writing formulas for molecular
compounds.
________ 7. CO2 is named monocarbon dioxide.
Chapter 9 Chemical Names and Formulas
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Date ___________________
Class __________________
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 8. binary molecular
compound
a. used to indicate the relative number of atoms of an
element in a molecular compound
________ 9. prefix
b. prefix indicating one atom of an element in a molecule
________ 10. mono-
c. prefix indicating four atoms of an element in a molecule
________ 11. tetra-
d. nonionic compound containing atoms of two elements
Part D Questions and Problems
Answer the following in the space provided.
12. Name each of the following compounds.
a. PCl5
b. SO2
c. P4S10
13. Write formulas for the following compounds.
a. carbon tetrabromide
216
Core Teaching Resources
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b. dinitrogen tetroxide
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Name ___________________________
9.4
Date ___________________
Class __________________
NAMING AND WRITING FORMULAS
FOR ACIDS AND BASES
Section Review
Objectives
• Apply three rules for naming acids
• Apply the rules in reverse to write formulas of acids
• Apply the rules for naming bases
Vocabulary
• acid
• base
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
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
An acid is a compound that contains one or more
2
atoms and produces
1.
when dissolved in water. There
2.
are rules for naming acids. For example, HBr is called
3
acid, whereas HNO3 is called
A base is a(n)
5
4
3.
acid.
4.
6
compound that produces
when
dissolved in water. Ionic compounds that are bases are named
in the same way as other
of the
8
7
compounds, that is, the name
is followed by the name of the
9
.
5.
6.
7.
8.
9.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 10. A compound that contains hydrogen atoms will be an acid when
dissolved in water.
Chapter 9 Chemical Names and Formulas
217
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Name ___________________________
Date ___________________
Class __________________
________ 11. An acid contains one or more hydroxide ions.
________ 12. Chemists have a special system for naming bases.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 13. acid
a. a compound containing hydrogen that ionizes to yield
hydrogen ions in solution
________ 14. base
b. a solution in which the solvent is water
________ 15. aqueous solution
c. a compound that produces hydroxide ions in water
Part D Questions and Problems
Answer the following in the space provided.
16. Write the formula for each acid or base.
a. magnesium hydroxide
b. hydrofluoric acid
d. lithium hydroxide
17. Name each acid or base.
a. KOH
b. HI
c. H2SO4
218
Core Teaching Resources
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c. phosphoric acid
05_CTR_ch09 7/9/04 3:29 PM Page 219
Name ___________________________
9.5
Date ___________________
Class __________________
THE LAWS GOVERNING FORMULAS
AND NAMES
Section Review
Objectives
• Define the laws of definite proportions and multiple proportions
• Apply the rules for writing chemical formulas by using a flowchart
• Apply the rules for naming chemical compounds by using a flowchart
Vocabulary
• law of definite proportions
• law of multiple proportions
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. [Use Figure 9.20 to complete this exercise.]
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
The law of
1
states that in samples of any chemical
1.
compound, the masses of the elements are always in the same
2.
2
3
. The law of
states that whenever the same two
3.
elements form more than one compound, the different masses
4.
of one element that combine with the same mass of the other
5.
4
6.
element are in the ratio of
H3PO4 is a(n)
CCl4 is not a(n)
5
numbers.
6
. It is called
7
.
7.
. It contains two elements, so it is a
8.
8
compound. It does not contain a metal, so it is a binary
9.
9
compound. The compound is called
Pb(C2H3O2)2 is not a(n)
12
11
.
10.
. It contains more than two
. C2H3O2 is a polyatomic
metal. The compound is called
10
13
15
.
. Pb is a Group
14
11.
12.
13.
14.
15.
Chapter 9 Chemical Names and Formulas
219
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Name ___________________________
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 16. Roman numerals are used when naming Group B metal cations.
________ 17. Names of compounds containing polyatomic anions end in -ide.
________ 18. Prefixes are used when naming binary ionic compounds.
________ 19. Compounds containing two elements are called binary compounds.
Part C Questions and Problems
Answer the following in the space provided.
20. Name the following compounds.
a. Pb(C2H3O2)4
b. HF
c. P2O5
d. LiBr
21. Write formulas for the following compounds.
a. phosphorus pentachloride
b. iron(II) oxide
d. potassium chloride
e. calcium nitrate
220
Core Teaching Resources
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c. nitric acid