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Chapter 9 Chemical Names and Formulas 211
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 commonpolyatomic ions
• Identify the two common endings for the names of most polyatomic ions.
Vocabulary• monatomic ions
• polyatomic ions
Part A CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.
Ions that consist of a single atom are called ions. 1.
Metallic elements tend to electrons. Group 1A ions have a 2.
charge, whereas Group 2A metals form ions with a 3.
charge, and Group 3A metals form ions with a charge. 4.
The charge of a Group A nonmetal ion is determined by 5.
subtracting from the group number. For example, the 6.
Group 7A elements form ions with a charge of . 7.
Many of the have more than one common ionic 8.
charge. These ions are named using either the system 9.
or the naming system. 10.
Ions containing more than one atom are called ions. 11.
The names of most common polyatomic ions end in either 12.
or . 13.1312
11
10
9
8
7
6
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NAMING IONS9.1
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212 Core Teaching Resources
Part B True-FalseClassify 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 willalways 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 thegroup number from 8.
________ 18. The Group 6A ions have a charge of 2�.
Part C MatchingMatch each description in Column B to the correct term in Column A.
Part D Questions and ProblemsAnswer 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 thefollowing ions?
a. Ca2� c. I�
b. S2� d. Mn3�
Column B
a. negatively charged ions
b. ions formed from single atoms
c. a traditional way of naming transition metal cations
d. positively charged ions
e. ions formed from groups of atoms
Column A
monatomic ions
polyatomic ions
cations
anions
classical naming system
________ 19.
________ 20.
________ 21.
________ 22.
________ 23.
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05_CTR_ch09 7/9/04 3:29 PM Page 212
Chapter 9 Chemical Names and Formulas 213
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 CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.
Binary ionic compounds are named by writing the name of 1.
the followed by the name of the . Names of 2.
binary compounds end in . For example, NaI is . 3.
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 6.
or -ate contain a polyatomic that includes . 7.
In writing the formula of an ionic compound, the net ionic charge 8.
must be .
Part B True-FalseClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 9. The systematic name for baking soda (NaHCO3) is sodiumbicarbonate.
________ 10. In writing a formula for an ionic compound, the net ionic charge ofthe formula must be zero.
8
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5
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NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS
9.2
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214 Core Teaching Resources
________ 11. Anions that contain oxygen end in -ite or -ate.
________ 12. The cation name is placed first when naming ionic compounds.
Part C MatchingMatch each description in Column B to the correct term in Column A.
Part D Questions and ProblemsAnswer 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
c. Na2Cr2O7
18. Write the formulas for the following compounds.
a. sodium chlorate
b. lead(II) phosphate
c. magnesium hydrogen carbonate
Column B
a. ions that consist of a single atom
b. ionic compounds composed of two elements
c. Group B metals, many of which have more than onecommon ionic charge
d. ions that consist of more than one atom
Column A
binary compounds
monatomic ions
polyatomic ions
transition metals
________ 13.
________ 14.
________ 15.
________ 16.
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Chapter 9 Chemical Names and Formulas 215
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 CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.
Binary molecular compounds are composed of two 1.
elements. The name of this type of compound ends in . 2.
Prefixes are used to show how many of each element 3.
are present in a molecule of the compound. For example, 4.
the name of As2S5 is .
Part B True-FalseClassify 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 molecularcompounds.
________ 7. CO2 is named monocarbon dioxide.
4
3
2
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NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS
9.3
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216 Core Teaching Resources
Part C MatchingMatch each description in Column B to the correct term in Column A.
Part D Questions and ProblemsAnswer 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
b. dinitrogen tetroxide
Column B
a. used to indicate the relative number of atoms of anelement in a molecular compound
b. prefix indicating one atom of an element in a molecule
c. prefix indicating four atoms of an element in a molecule
d. nonionic compound containing atoms of two elements
Column A
binary molecularcompound
prefix
mono-
tetra-
________ 8.
________ 9.
________ 10.
________ 11.
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Chapter 9 Chemical Names and Formulas 217
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 CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.
An acid is a compound that contains one or more 1.
atoms and produces when dissolved in water. There 2.
are rules for naming acids. For example, HBr is called 3.
acid, whereas HNO3 is called acid. 4.
A base is a(n) compound that produces when 5.
dissolved in water. Ionic compounds that are bases are named 6.
in the same way as other compounds, that is, the name 7.
of the is followed by the name of the . 8.
9.
Part B True-FalseClassify 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 whendissolved in water.
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NAMING AND WRITING FORMULAS FOR ACIDS AND BASES
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218 Core Teaching Resources
________ 11. An acid contains one or more hydroxide ions.
________ 12. Chemists have a special system for naming bases.
Part C MatchingMatch each description in Column B to the correct term in Column A.
Part D Questions and ProblemsAnswer the following in the space provided.
16. Write the formula for each acid or base.
a. magnesium hydroxide
b. hydrofluoric acid
c. phosphoric acid
d. lithium hydroxide
17. Name each acid or base.
a. KOH
b. HI
c. H2SO4
Column B
a. a compound containing hydrogen that ionizes to yieldhydrogen ions in solution
b. a solution in which the solvent is water
c. a compound that produces hydroxide ions in water
Column A
________ 13. acid
________ 14. base
________ 15. aqueous solution
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Chapter 9 Chemical Names and Formulas 219
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 CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number. [Use Figure 9.20 to complete this exercise.]
The law of states that in samples of any chemical 1.
compound, the masses of the elements are always in the same 2.
. 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.
element are in the ratio of numbers. 6.
H3PO4 is a(n) . It is called . 7.
CCl4 is not a(n) . It contains two elements, so it is a 8.
compound. It does not contain a metal, so it is a binary 9.
compound. The compound is called . 10.
Pb(C2H3O2)2 is not a(n) . It contains more than two 11.
. C2H3O2� is a polyatomic . Pb is a Group 12.
metal. The compound is called . 13.
14.
15.
15
141312
11
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THE LAWS GOVERNING FORMULAS AND NAMES
9.5
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220 Core Teaching Resources
Part B True-FalseClassify 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 ProblemsAnswer 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
c. nitric acid
d. potassium chloride
e. calcium nitrate
Name ___________________________ Date ___________________ Class __________________©
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Chapter 9 Chemical Names and Formulas 221
Practice ProblemsIn your notebook, solve the following problems.
SECTION 9.1 NAMING IONS1. What is the charge on the ion typically formed by each element?
a. oxygen c. sodium e. nickel, 2 electrons lost
b. iodine d. aluminum f. magnesium
2. How many electrons does the neutral atom gain or lose when each ionforms?
a. Cr3� c. Li� e. Cl�
b. P3� d. Ca2� f. O2�
3. Name each ion. Identify each as a cation or an anion.
a. Sn2� c. Br� e. H�
b. Co3� d. K� f. Mn2�
4. Write the formula (including charge) for each ion. Use Table 9.3 if necessary.
a. carbonate ion c. sulfate ion e. chromate ion
b. nitrite ion d. hydroxide ion f. ammonium ion
5. Name the following ions. Identify each as a cation or an anion.
a. CN� c. PO43� e. Ca2�
b. HCO3� d. Cl� f. SO3
2�
SECTION 9.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS
1. Write the formulas for these binary ionic compounds.
a. magnesium oxide c. potassium iodide e. sodium sulfide
b. tin(II) fluoride d. aluminum chloride f. ferric bromide
2. Write the formulas for the compounds formed from these pairs of ions.
a. Ba2�, Cl� c. Ca2�, S2� e. Al3�, O2�
b. Ag�, I� d. K�, Br� f. Fe2�, O2�
3. Name the following binary ionic compounds.
a. MnO2 c. CaCl2 e. NiCl2 g. CuCl2
b. Li3N d. SrBr2 f. K2S h. SnCl4
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CHEMICAL NAMES AND FORMULAS9
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222 Core Teaching Resources
4. Write formulas for the following ionic compounds.
a. sodium phosphate c. sodium hydroxide e. ammonium chloride
b. magnesium sulfate d. potassium cyanide f. potassium dichromate
5. Write formulas for compounds formed from these pairs of ions.
a. NH4�, SO4
2� c. barium ion and hydroxide ion
b. K�, NO3� d. lithium ion and carbonate ion
6. Name the following compounds.
a. NaCN c. Na2SO4 e. Cu(OH)2
b. FeCl3 d. K2CO3 f. LiNO3
7. Name and give the charge of the metal cation in each of the following ionic compounds.
a. Na3PO4 c. CaS e. FeCl3
b. NiCl2 d. K2S f. CuI
SECTION 9.3 NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS
1. Name the following molecular compounds.
a. PCl5 c. NO2 e. P4O6 g. SiO2
b. CCl4 d. N2F2 f. XeF2 h. Cl2O7
2. Write the formulas for the following binary molecular compounds.
a. nitrogen tribromide c. sulfur dioxide
b. dichlorine monoxide d. dinitrogen tetrafluoride
SECTION 9.4 NAMING AND WRITING FORMULAS FOR ACIDS AND BASES
1. Name the following compounds as acids.
a. HNO2 b. H2SO4 c. HF d. H2CO3
2. Write the formulas for the following bases.
a. calcium hydroxide c. aluminum hydroxide
b. ammonium hydroxide d. lithium hydroxide
SECTION 9.5 THE LAWS GOVERNING FORMULAS AND NAMES1. Write the formulas for these compounds.
a. potassium sulfide e. hydrobromic acid i. sulfur hexafluoride
b. tin(IV) chloride f. aluminum fluoride j. magnesium chloride
c. hydrosulfuric acid g. dinitrogen pentoxide k. phosphoric acid
d. calcium oxide h. iron(III) carbonate l. nitric acid
Name ___________________________ Date ___________________ Class __________________©
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Chapter 9 Chemical Names and Formulas 223
2. Complete this table by writing correct formulas for the compounds formed bycombining positive and negative ions.
3. Name the following compounds.
a. K3PO4 c. NaHSO4 e. N2O5 g. PI3
b. Al(OH)3 d. HgO f. NBr3 h. (NH4)2SO4
4. Explain the difference between the law of definite proportions and the law ofmultiple proportions.
SO42� NO3
� OH� PO43�
Ca2�
Al3�
Na�
Pb4�
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224 Core Teaching Resources
Use the abbreviated periodic table above to answer the following questions.
1. Which group on the periodic table contains magnesium (Mg)?
2. How many electrons does a magnesium atom lose to form a magnesium cation?
3. How many electrons does a neutral magnesium atom contain?
4. How many electrons does a magnesium cation contain?
5. Which group on the periodic table contains fluorine (F)?
6. How many electrons does a fluorine atom gain to form a fluoride anion?
7. How many electrons does a neutral fluorine atom contain?
Group1A
2A 3A 4A 5A 6A 7A
8A
H1
Hydrogen
Li3
Lithium
Na11
Sodium
K19
Potassium
Ca20
Calcium
Be4
Beryllium
Mg12
Magnesium
B5
Boron
Al13
Aluminum
C6
Carbon
Si14
Silicon
N7
Nitrogen
P15
Phosphorus
O8
Oxygen
S16
Sulfur
F9
Fluorine
Cl17
Hydrogen
He2
Helium
Ne10
Neon
Ar18
Argon
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INTERPRETING GRAPHICSUse with Section 9.1
9
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Chapter 9 Chemical Names and Formulas 225
8. How many electrons does a fluoride anion contain?
9. How many electrons does a sodium cation contain?
10. How many electrons does an oxide anion contain?
11. How many electrons does each of the following ions contain?
a. S2�
b. Ca2�
c. K�
d. Cl�
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Name ___________________________ Date ___________________ Class __________________
Vocabulary ReviewMatch the correct vocabulary term to each numbered statement. Write the letter of thecorrect term on the line.
Column B
a. anion
b. law of multipleproportions
c. base
d. ionic compounds
e. binary compound
f. monatomic ion
g. cation
h. polyatomic ion
i. acids
j. law of definiteproportions
Column A
compounds that contain one or more hydrogen atomsand produce hydrogen ions in solution
an ionic compound that produces hydroxide ionswhen dissolved in water
any atom or group of atoms that has a positive charge
compounds composed of metal cations and nonmetalanions
composed of two elements and can be either ionic ormolecular
an ion consisting of a single atom with a positive ornegative charge
Whenever two elements form more than onecompound, the different masses of one element thatcombine with the same mass of the other element arein the ratio of small whole numbers.
a tightly bound group of atoms that behaves as a unitand carries a charge
In samples of any chemical compound, the masses ofthe elements are always in the same proportions.
any atom or group of atoms that has a negative charge
________ 1.
________ 2.
________ 3.
________ 4.
________ 5.
________ 6.
________ 7.
________ 8.
________ 9.
________ 10.
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CHEMICAL NAMES AND FORMULAS9
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Chapter 9 Chemical Names and Formulas 227
Chapter QuizFill in the word(s) that will make each statement true.
1. tend to lose electrons when they react to form 1.compounds.
2. The formula for phosphorus pentachloride is . 2.
3. A(n) is any atom or group of atoms with a 3.negative charge.
4. The law of states that in any chemical compound, 4.the elements are always combined in the same proportion by mass.
5. The charge on an ion of a Group A nonmetal is determined 5.by subtracting 8 from .
6. The metals in Groups 1A, 2A, and 3A electrons 6.when they form ions.
7. The two common polyatomic ions whose names end in -ide 7.are the cyanide ion and the ion.
8. The formula for the dihydrogen phosphate ion is . 8.
9. The systematic name for laughing gas (N2O) is . 9.
Write your answer in the space provided.
10. What is the formula for iron(II) chloride? 10.
11. Name the compound whose formula is SnS2. 11.
12. Name the compound N2O5. 12.
13. Name the compound NaHCO3. 13.
14. Write the formula for copper(II) hydroxide. 14.
15. Name the compound HNO3 as an acid. 15. 9.4
9.2
9.2
9.3
9.2
9.2
9.3 9
9.18
79.1
9.16
59.1
9.54
9.13
9.32
9.11
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CHEMICAL NAMES AND FORMULAS9
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228 Core Teaching Resources
Chapter Test A
A. MatchingMatch each description in Column B to the correct term in Column A. Write theletter of the correct description in the blank.
B. Multiple ChoiceChoose the best answer and write its letter on the line.
________ 10. The correct name for the N3� ion is the:a. nitrate ion. c. nitride ion.b. nitric ion. d. nitrite ion.
Column B
a. any atom or group of atoms with a negative charge
b. When two elements combine to form more than onecompound, the different masses of one element thatcombine with the same mass of the other element are inthe ratio of small whole numbers.
c. tightly bound group of atoms that behaves as a unit andcarries a charge
d. a compound that produces hydroxide ions when dissolvedin water
e. a compound composed of two different elements
f. any atom or group of atoms with a positive charge
g. In all samples of the same chemical compound, theelements are always combined in the same proportion by mass.
h. a compound that produces hydrogen ions when dissolvedin water
i. consists of a single atom with a positive or negative charge
Column A
cation
anion
law of definiteproportions
acid
base
law of multipleproportions
polyatomic ion
monatomic ion
binary compound
________ 1.
________ 2.
________ 3.
________ 4.
________ 5.
________ 6.
________ 7.
________ 8.
________ 9.
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CHEMICAL NAMES AND FORMULAS9
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Chapter 9 Chemical Names and Formulas 229
________ 11. Elements of Group 4A:a. generally form positive ions.b. generally form negative ions.c. do not commonly form ions.d. do not combine with other elements.
________ 12. What is the ionic charge on the chromium ion in the ionic compoundthat has the formula Cr2O3?a. 3� c. 5�
b. 2� d. 5�
________ 13. Which element when combined with chlorine would most likely forman ionic compound?a. lithium c. phosphorusb. carbon d. bromine
________ 14. What is the formula for calcium hydrogen phosphate?a. CaHPO4 c. Ca(H2PO4)2
b. Ca2HPO4 d. Ca(HPO4)2
________ 15. A cation is any atom or group of atoms with:a. a positive charge.b. no charge.c. a negative charge.d. more electrons than the corresponding atoms.
________ 16. The cation Fe3� is formed when:a. an atom of iron loses two electrons.b. an atom of zinc loses two electrons.c. an atom of iron loses three electrons.d. an atom of iron gains three electrons.
________ 17. A molecular formula:a. gives information about molecular geometry.b. can be written for ionic compounds.c. shows the number and kinds of atoms in a molecule of a
compound.d. uses superscripts to show the number of atoms of each kind.
________ 18. The metals in Groups 1A, 2A, and 3A:a. gain electrons when they form ions.b. form ions with a charge found by subtracting 8 from the
group number.c. all form ions with a 1� charge.d. lose electrons when they form ions.
________ 19. When naming an ion of a transition metal that has more than onecommon ionic charge, the numerical value of the charge is indicatedby a:a. prefix.b. suffix.c. Roman numeral following the name.d. superscript after the name.
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230 Core Teaching Resources
________ 20. In naming a binary molecular compound, the number of atoms ofeach element present in the molecule is indicated by:a. Roman numerals. c. prefixes.b. superscripts. d. suffixes.
________ 21. An -ite or -ate ending on the name of a compound indicates that thecompound:a. is a binary ionic compound.b. is a binary molecular compound.c. contains a polyatomic anion.d. contains a polyatomic cation.
________ 22. What is the formula for sulfuric acid?a. H2S2 c. H2SO3
b. H2SO4 d. H2S
C. CompletionFill in the word(s) that will make each statement true.
23. The ionic charge of lead, Pb, in the compound PbS2 is . 23. _______________________
24. The typical ionic charge of an ion formed by an element in 24. _______________________Group 7A is .
25. Atoms that have a positive or negative charge are called . 25. _______________________
26. The name of a monatomic anion ends in . 26. _______________________
27. The ionic charge of chlorine, Cl, in the compound MgCl2 is 27. _______________________.
28. In a polyatomic ion, the -ite ending indicates one fewer 28. _______________________atom than the -ate ending.
29. Binary molecular compounds are composed of two 29. _______________________elements.
30. Acids are compounds that produce ions when dissolved 30. _______________________in water.
D. ProblemsWrite the answers in the space provided.
31. Write the formulas for these compounds.
a. magnesium cyanide a.
b. mercury(II) bromide b.
c. sulfur hexafluoride c.
30
29
28
27
26
25
24
23
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Chapter 9 Chemical Names and Formulas 231
32. Name these compounds.
a. CuCl a.
b. N2O3 b.
c. KC2H3O2 c.
E. EssayWrite a short essay for the following.
33. Why was it necessary for chemists to develop a system for naming chemical compounds?
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232 Core Teaching Resources
Chapter Test B
A. MatchingMatch each term in Column B to the correct description in Column A. Write the letterof the correct description on the line.
B. Multiple ChoiceChoose the best answer and write its letter on the line.
________ 10. Which of the following is a nonmetal?a. iron c. oxygenb. silver d. copper
________ 11. Which of the following is an anion?a. O2� c. Al3�
b. Mg2� d. H
Column B
a. law of definiteproportions
b. acid
c. law of multipleproportions
d. base
e. polyatomic ion
f. cation
g. monatomic ion
h. anion
i. binary compound
Column A
a compound composed of two elements
a compound that produces hydrogen ions when dissolvedin water
When two elements combine to form more than onecompound, the different masses of one element thatcombine with the same mass of the other element are inthe ratio of small whole numbers.
an atom or group of atoms with a negative charge
consists of a single atom with a positive or negative charge
In any sample of a chemical compound, the elements arealways combined in the same proportions by mass.
any atom or group of atoms with a positive charge
tightly bound group of atoms that behaves as a unit andcarries a charge
compound that produces hydroxide ions when dissolved inwater
________ 1.
________ 2.
________ 3.
________ 4.
________ 5.
________ 6.
________ 7.
________ 8.
________ 9.
Name ___________________________ Date ___________________ Class __________________©
Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
CHEMICAL NAMES AND FORMULAS9
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Chapter 9 Chemical Names and Formulas 233
________ 12. Nitrogen reacts with oxygen to form two compounds. Compound Acontains 2.8 g of nitrogen for each 1.6 g of oxygen. Compound Bcontains 5.6 g of nitrogen for each 9.6 g of oxygen. What is the lowestwhole-number mass ratio of nitrogen that combines with a given massof oxygen?a. 3:1 c. 4:7b. 2:1 d. 1:6
________ 13. The nonmetals in Groups 5A, 6A, and 7A:a. lose electrons when they form ions.b. form positively charged ions.c. form ions with charges of 3�, 2�, and 1�, respectively.d. form ions with a numerical charge equal to their group number.
________ 14. Among the following, which atom is most likely to form an ion with acharge of 2�?a. O c. Alb. Na d. Ca
________ 15. The correct name for the ion Fe2� is:a. ferric. c. ferrous.b. iron(II). d. both b and c.
________ 16. Among these element groups, which is least likely to form ions?a. 1A c. 4Ab. 3A d. 7A
________ 17. The sulfate ion is written in which of the following ways?a. S2� c. SO4
2�
b. SO32� d. none of the above
________ 18. What is the formula for aluminum oxide?a. AlO3 c. Al3O2
b. Al2O3 d. Al2O
________ 19. Among the following, which is a binary molecular compound?a. CO2 c. FeOb. NaCl d. MgS
________ 20. What is the formula for carbon tetrachloride?a. CCl c. CCl3
b. CCl2 d. CCl4
________ 21. The compound H3PO4 is named:a. nitric acid. c. phosphoric acid.b. sulfuric acid. d. ethanoic acid.
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234 Core Teaching Resources
C. CompletionFill in the word(s) that will make each statement true.
22. The atoms of Group 7A elements electrons whenthey form ions.
23. The atoms of Group B elements electrons whenthey form ions.
24. An atom or group of atoms with a positive charge is a(n) .
25. The law of states that in all samples of the samechemical compound, the masses of the elements are always in the sameproportions.
26. The ionic charge of an element in Group 6A is .
27. The symbol for the ammonium ion is .
28. The name of the compound Mg(NO3)2 is .
29. The names of all binary compounds, both ionic and molecular, end in the
letters .
30. The formula for calcium phosphate is .
31. In a polyatomic ion, the -ate ending indicates one oxygen than the -ite ending.
D. QuestionsAnswer the following questions in the space provided.
32. For each pair of ions listed, write the correct formula and then name thecompound formed by combining the two ions.
Formula Name
a. Ca2� and NO3�
b. Na� and SO42�
c. Fe3� and O2�
d. Al3� and CO32�
Name ___________________________ Date ___________________ Class __________________©
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Chapter 9 Chemical Names and Formulas 235
33. Write the formulas for the following compounds.
a. silicon dioxide e. nitric acid
b. carbon tetrafluoride f. silver nitrate
c. zinc hydroxide g. ferric sulfate
d. phosphorus tribromide h. mercury(II) chloride
34. Name the following compounds:
a. CS2 e. Sn(OH)4
b. (NH4)2CO3 f. H2SO4
c. As2O5 g. PI5
d. CO h. KMnO4
E. EssayWrite a short essay for the following.
35. Distinguish between ionic and molecular compounds, both in terms ofcomposition and method of naming.
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