05 CTR ch09 7/9/04 3:29 PM Page 211 NAMING IONS...

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

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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.

Name ___________________________ Date ___________________ Class __________________©

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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


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 .


________ 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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NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS

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________ 11. Anions that contain oxygen end in -ite or -ate.

________ 12. The cation name is placed first when naming ionic compounds.



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.

Name ___________________________ Date ___________________ Class __________________©


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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


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 .


________ 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

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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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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


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.


________ 10. A compound that contains hydrogen atoms will be an acid whendissolved in water.

98

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NAMING AND WRITING FORMULAS FOR ACIDS AND BASES

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________ 11. An acid contains one or more hydroxide ions.

________ 12. Chemists have a special system for naming bases.



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

Name ___________________________ Date ___________________ Class __________________©


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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

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THE LAWS GOVERNING FORMULAS AND NAMES

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________ 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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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

Name ___________________________ Date ___________________ Class __________________

CHEMICAL NAMES AND FORMULAS9

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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


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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2. Complete this table by writing correct formulas for the compounds formed bycombining positive and negative ions.


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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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

Name ___________________________ Date ___________________ Class __________________©


INTERPRETING GRAPHICSUse with Section 9.1

9

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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.

© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.


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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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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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________ 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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________ 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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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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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.

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________ 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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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�

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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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05_CTR_ch09 7/9/04 3:29 PM Page 235

05 CTR ch09 7/9/04 3:29 PM Page 211 NAMING IONS...

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