1 naming first name, last name score /...

9 NAMING

Positive Ions (cations)

Aluminum Al 3+

Ammonium NH4 +

Antimony (III) Sb3+

Antimony (V) Sb5+

Arsenic (III) As3+

Arsenic (V) As5+

Barium Ba2+

Beryllium Be2+

Bismuth (III) Bi3+

Bismuth (V) Bi5+

Cadmium Cd2+

Calcium Ca 2+

Chromium (II) Cr 2+

Chromium (III) Cr 3+

Cobalt (II) Co 2+

Cobalt (III) Co 3+

Copper (I) Cu +

Copper (II) Cu 2+

Hydrogen, hydronium ** H + , H

3O+

Iron (II) Fe 2+

Iron (III) Fe 3+

Lead (II) Pb 2+

Lead (IV) Pb 4+

Lithium Li +

Magnesium Mg 2+

Manganese (II) Mn 2+

Manganese (IV) Mn 4+

Mercury (I)* Hg2 2+

Mercury (II) Hg 2+

Nickel Ni 2+

Oxonium ** H3O +

Potassium K +

Scandium Sc 2+

Silver Ag +

Sodium Na +

Strontium Sr 2+

Tin (II) Sn 2+

Tin (IV) Sn 4+

Zinc Zn 2+

First Name, Last Name_____ ____Score _____/______ Period

Negative Ions (anions) ACIDS Acetic Acid

Acetate CH3COO- HCH3COO

Borate BO33-

Bromate BrO3 -

Bromide Br -

Carbonate CO3 2- H2 CO3 Carbonic A.

Chlorate ClO3 - HClO3 Chloric A.

Chloride Cl - HCl Hyrdrochloric A.

Chlorite ClO2- HClO2 Hypochlorous A

Chromate CrO42-

Cyanide CN-

Dichromate Cr2O72-

Dihydrogen phosphate H2PO4

- H3PO4 Phosphoric A.

Fluoride F - HF Hydrofluoric A.

Hydrogen carbonate HCO3

-

Hydrogen phosphate HPO42-

Hydrogen sulfate HSO4-

Hydrogen sulfide HS- Hydrosulfuric A

Hydrogen sulfite HSO3- Sulfurous A.

Hydride H-

Hydroxide OH-

Hypochlorite ClO- HClO Hypochlorous A

Iodate IO3 -

Iodide I -

Nitrate NO3- HNO3 Nitric Acid

Nitride N3-

Nitrite NO2- HNO2

Oxalate C2O42- H2C2O4

Oxide O2-

Perchlorate ClO4- HClO4 Perchloric A.

Permanganate MnO4-

Peroxide O22-

Phosphate PO43-

Phosphide P3-

Phosphite PO33-

Silicate SiO44-

Sulfate SO42-

Sulfide S2-

Sulfite SO32-

Polyatomic Questions Directions: Look at the table to answer the below: 1. If an ion ending in “ate” is a “O4“, then what is it called if it ends in “O3 “?__

In ions with much oxygen O3 or O4 end in ate like Chlorate When Hydrogen is placed in front, the name changes in 3 ways. What are they? 2. The _____ is dropped off. 3. The letters ___ are added. 4. The word ____ follows. In polyatomics with one less Oxygen (O2 or O3) like Sulfite When Hydrogen is placed in front, the name changes in 3 ways. What are they? 5. The _____ is dropped off. 6. The letters ___ are added. 7. The word ____ follows

Based on the rules for changing polyatomics with –ate and -ite to acids that become –ic Acids and –ous Acids, please fill in the boxes w/ names of Acids 8. 9. 10.

11. For extra find any others (2pts).

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9 NAMING COMPOUNDS __ /__ pts First Last Name___Per__

Anticipatory Response 1 Cornell Question & Ans 1.Li+ is called Lithium ion? Y N 2 Directions:Make 5 questions2. O2‐ is called Oxygen ion? Y N 3 & answers that are different3. Molecular for. are the same 4 than the Anticipatory Responseas structural formulas? Y N 5 1. 4. Diatomic molecules are like 6 Siamese twins (ex. O2)? Y N 7 5. Formula Units are reduced 8 ratios/empirical formulas? Y N 9 Type 4 10

He

H‐ 2.

Type 1 TYPE 3 Group 1, 2, Al, Zn, Ag, Ni, Cd TYPE II Nonmetals & Metalloids only Transition Metals 3. 4. Anticipatory Response TYPE 4 – 5. 1. HF is Hydrogen Fluoride?Y N Acids (H‐X) 2.H2S is Hydrogen Sulfide? Y N 3. PbO2 is Lead Dioxide? Y N 4. Fe2O3 is Iron II Oxide? Y N 5. SO3 & SCl4 are Sulfur Triox‐ ide & Sulfur TetraChloride?Y N Summary Section:

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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

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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 __________________©

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

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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.

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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.

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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.

Name ___________________________ Date ___________________ Class __________________©


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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.

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9 NAMING COMPOUNDS

Write the formula for each of the following compounds:

calcium chloride sodium flouride sodium cyanide aluminum nitrate magnesium oxide zinc iodide barium oxide cobalt (II) carbonate potassium hydride mercury (II) cyanide zinc tartrate cadmium silicate ammonium dichromate lead (II) nitrate copper (II) perchlorate sodium tetraborate

Write the formula for the compound made from each of the following pairs:

silver and fluorine Ammonium and oxalate ions nickel (II) and sulfur strontium and iodine chromium (III) and bromine lithium and oxygen lead (II) and phosphate

Name the following compounds:

BaS Mg3N2 ZnF2 BiI3 PbBr2 CaH2 Na3P CaS TlI CoBr2 BaCl2 AlF3 KCl Zn(No3)2 NaBr Li2CO3 HgI2 Ba(OH)2

Use inorganic numerical prefixes to name each of the following:

P2O5 PCl5 SF6 PCl3 CO SO2 SO3 CCl4 NCl3 S4N4

Write the formulas for each of the following:

Carbon tetrabromide Xenon diflouride Sulfur hexaflouride Bromine trioxide Iodine trichloride Sulfur tetraiodide For the below use the following 3 words to fill in: Metallic, Ionic & Covalent ____ Substances _______ Substances Substances High melting points Atoms same electronegativity high conductivity conduct when melted shared electrons malleable soluble in H2O non-metals luster crystallize form molecules mix to form alloys from electron transfer poor conductors form ionic compounds

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9 NAMING COMPOUNDS

Type I (Group 1 & 2 Alkalis +) Type II (Transition Metals) Directions: Write the formula for each of the following compounds: Sodium cyanide Cobalt (I) Carbonate Magnesium oxide Cobalt (II) Carbonate Aluminum hydride Mercury (II) Cyanide Cadmium silicate Mercury (I) Cyanide Silver dichromate Lead (II) Nitrate Zinc Chloride Lead (IV) Nitrate Nickel Chloride Copper (II) Perchlorate

Type I Type II Directions: Remember to balance charges when you write the formula for the compound made. Silver and Fluorine Iron (II) and Oxygen Nickel and Sulfur Iron (III) and Oxygen Lithium and Oxygen Chromium (III) and bromine Ammonium and Oxalate Lead (II) and phosphate Directions: Name the following compounds: BaS PbBr ZnF2 PbBr2 CaH2 PbBr4 Na3P CoBr AlF3 CoBr2 BaCl2 HgI2 KCl HgI4 Na3PO4 FeO Ba(OH)2 Fe2O3

Type III Directions: Use inorganic numerical prefixes to name each of the following: P2O5 PCl5 SF6 PCl3 CO SO2 SO3 CCl4 NCl3 S4N4 Directions: Write the formulas for each of the following: Carbon tetrabromide Xenon diflouride Sulfur hexaflouride Bromine trioxide Iodine trichloride Sulfur tetraiodide sodium tetraborate Dichromate Heptoxide For the below use the following 3 words to fill in: Metallic, Ionic & Covalent ____ Substances _______ Substances Substances High melting points Atoms same electronegativity high conductivity conduct when melted shared electrons malleable soluble in H2O non-metals luster crystallize form molecules mix to form alloys from electron transfer poor conductors high ductility form ionic compounds weak bonds strong bonds

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Name the following compounds:

1. Li3PO4

2. RbMnO4

3. CaCO3

4. Fe(OH)3

5. Fe(OH)2

6. CuO

7. Cu2O

Write the formula for each of the following compounds:

8. Iron (II) carbonate

9. Copper (I) chromate

10. Ferric oxide

11. Ferrous oxide

12. Iron (II) oxide

13. Calcium chloride

14. Calcium chlorate

Correct the following incorrectly written compounds:

15. NaCl2

16. Al(OH)2

17. ZnPO4

18. LiSO4

19. K(MnO4)2

20. LiO

Answer the following using complete sentences. Use diagrams where helpful:

21. What is meant by “Crystalline structure?”

22. What holds the atoms of a salt together?

23. Why do atoms tend to become ionized?

24 Explain why crystalline structures, like sodium chloride, easily shatter

when hit by a hammer?

Name

Date Period______ 9 Ionic Compounds & Crystalline Structure

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Naming Covalent Compounds

Name each of the following:

1. P3O4 Triphosphosphur tretraoxide___________________

2. S3F6

3. NH3

4. H2S

5. SeCl3

6. CCl4

7. PCl5

8. S4N9

9. NO2

10. CO

Write the formulas for each of the following:

11. Carbon tetraiodide C IIII4______________________________________________

12. Sulfur diflouride

13. Sulfur tetraiodide

14. Xenon hexaflouride

15. Bromine trioxide

16. Dihydrogen monoxide

17. Carbon tetrahydride

18. Tricarbon octahydride

19. Tetracarbon decahydride

20. Dicabon hexahydride

Name

Date Period _________

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9 9 9 9 NAMING NAMING NAMING NAMING & & & &

WRITINGWRITINGWRITINGWRITING SALTSSALTSSALTSSALTS COMPLETE THE FOLLOWING TABLE:

Cation Name

Cation Symbol

Anion Name

Anion Symbol

Ionic Compoud Formed Compound Formula

Strontium Sr 2+ Nitride N3-

Strontium nitride Sr3N2

Strontium nitrate

Strontium nitrite

Potassium chloride

Potassium chlorate

Potassium perchlorate

Potassium chlorite

Potassium hypochlorite

Ferric carbonate

Ferrous carbonate

Iron (II) bisulfate

Iron (III) bisulfate

Copper (I) iodide

Copper (II) iodide

Sodium sulfite

Calcium nitrate

Ammonium hydroxide

Ammonium oxide

Ammonium peroxide

Lithium hydroxide

Lithium oxide

Lithium perioxide

Zinc oxide

Hydrogen peroxide

Ammonium nitrate

Ammonium dihydrogen phosphate

Calcium hydrogen phosphate

Name Date Per

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9 NAMING & WRITING SALTS

Directions: COMPLETE THE FOLLOWING TABLE. Don’t forget to balance the charges in the compound below.

Cation Name

Cation Symbol

Anion Name

Anion Symbol

Ionic Compound Formed

Compound Formula

Strontium Sr 2+ Nitride N3- Strontium nitride Sr2+N3- Sr3N2

Strontium Strontium nitrate

Sr2+NO3- Sr(NO3)2

Nitrite Strontium nitrite

Potassium Potassium chloride

Chlorate Potassium chlorate

Potassium Potassium perchlorate

Chlorite Potassium chlorite

Potassium Potassium hypochlorite

Carbonate Ferric carbonate

Iron II Ferrous carbonate

Sulfate Iron (II) sulfate

Iron III Iron (III) sulfite

Iodide Copper (I) iodide

Cuprous Copper (II) iodide

Sulfite Sodium sulfite

Calcium Calcium nitrate

Hydroxide Ammonium hydroxide

Ammonium Ammonium oxide

Peroxide Ammonium peroxide

Lithium Lithium hydroxide

Oxide Lithium oxide

Cesium Cesium perioxide

Oxide Zinc oxide

Hydrogen Hydrogen peroxide

Nitrate Ammonium nitrate

Ammonium Ammonium dihydrogen phosphate

Hydrogen Phosphate

Calcium hydrogen phosphate

Name Date Per

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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.

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15.

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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 __________________

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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

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 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

Name ___________________________ Date ___________________ Class __________________©

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9 CHEMISTRY NAME SEARCH

Chemical

Name

Formula Lewis Structure Angle Shape Polarity

Hi Lo

Substance

& Use CCl4

O2

Example Ethanol

C2H5OH

H H

H – C – C – OH

H H

109tetrahedral

104 bent

Cyclohexane

Water

Methane

Hydrogen

Peroxide

BaCl2

HCl

NH3

Ethene

Sodium

Chloride

CFC or CCl2F2

21

21 ↑

user

Highlight

user

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9 IONIC COMPOUND NAMING CHART

Directions: Write the formala name of each compound.

F- Cl- SO42- CO3

2- NO3- PO4

3- CrO42- CH3CO2

3-

NH4+

Ammonium Flouride

Ammonium Acetate (vinegar)

K+

Na+

Ag

Ca 2+

Mg 2+

Ba 2+

Al 3+

Fe 2+

Fe 3+

Iron III Flouride Iron III

Phosphate

9 IONIC COMPOUND FORMULA CHART

Directions: Write the chemical formula of each compound. Make sure the oxidation number add up to zero.

F- Cl- SO42- CO3

2- NO3- PO4

3- CrO42- CH3CO2

3-

NH4+

NH4 F

K+

Na+

Ag+

Ca2+

Mg2+

Ba2+

Al3+

Fe2+

Fe3 (PO4)2

Fe3+

FeCl3

22

22 ↑

9 IONIC REACTION LAB CHART

Directions:

1) Write the entire chemical formula of each anion & cation below to be used (look at NaCl/AgNO3).

2) Put one drop of each chemical on the plastic grid sheet. Record your observations below.

Anions��

Cations !

F- Cl-

NaCl

SO42- CO3

2- NO3-

CaNO3

PO43- CrO4

2

-

CH3CO23

-

A AgNO3

White

ppt

No (NR) Reaction

B

C

D

E

F

G

H

I

J

1 2 3 4 5 6 7 8 9 10 11

Directions: 1) Pick one reaction which made a Precipitate from each column and write the ionic reaction. 2) Use the solubility rule to determine which product formed the precipitate & which was soluble. 3) Cross out the products which were soluble because they’re spectators as reactants & products.

column Reactants Products

AgNO3 + NaCl � AgCl + NaNO3 Rule # states that Chlorides are soluble

A 2 Ag++NO3- + Na++Cl- �� AgCl +Na++NO3

- except with Ag, Pb & Hg.

Ag++ Cl- �� AgCl Total ionic equation B C D E F G H I J

23

23 ↑

First Last Name Per Score ___/20

4 – 9, 25 Cumulative & Reteaching 4 Atomic Structure Problem Number

Symbol

Isotope Name

Avg Atomic Mass

Mass Number

Atomic Number =

Neutrons

Electrons

Protons

1. 45 ? 21

Scandium‐? 44.9 =

2. From the above chart, Isotopes of the same element the same number of: protons, neutrons, mass 3. Elements are always Identified by the same: protons, neutrons, atomic mass 4. Ions are formed because of a losing or gaining protons, neutrons, electrons

25 Nuclear Chemistry 5. Proton 6. __________ 7. BetaMass Letter P He Charge

Fill missing numbers

Reaction type Radioisotope Name ‐ #

Reactants Reacts To Form

Products

Fission Or Fusion

8. Beta Decay Polonium ‐ # 209Po ‐1 e +

9. Which results in a decrease in the atomic number and atomic mass? (Alpha decay, beta decay, Alpha Capture) 10. From the above, Beta decay results in a loss of (0,1, or 2 )a.m.u’s and a(n) (increase or decrease) in nuclear charge.

5&6 Electron Configuration Element Electron Configuration Noble Gas Shorthand Highest Energy Level

with Electrons # electrons in highest level Lewis Dot

11. 1s2 2s2 2p6 3s2 3p4 12. In “3s2 “, the 3 represents which 3 (column, group, family, period, row or energy level). 13. In “3s2 “, the p4 represents which 3 (column, group, family, period, row or energy level).

7 Ions and Bonding 14. Which 2 have 2 valence electron? (sodium, magnesium, Group 1A, Group 2A) 16. Magnesium’s charge after reacting would be (1‐, 0, 1+, 2+) 18. Which formula is correct? (MgCl, MgCl2, MgCl3)

8 Covalent Bonding 19. What type of bond is MgCl2? (covalent, ionic, metallic) 20. What type of bond is in CO2? (covalent, ionic, metallic) 21. Why is CH4 non‐polar? (C & H share e‐ evenly, they share unevenly, they don’t share)

9 Naming Type 1 Type II Type III 22. What is the name of BaCl2? Barium Chloride Barium Dichloride Barium II Chloride 23. What is the name of CuCl2? Copper Chloride Copper II Chloride Copper Dichloride 24. What is the name of OCl2? Oxygen Chlorided Oxygen II Chloride Oxygen Dichloride 25. From the above, Type I is (alkalis, transitions), Type II is (transitions, non‐metals) & Type III is (alkalis, nonmetals)

corrected by:________

24

24 ↑

___________________________ First Name, Last ________

Period

SCORE: ___/10 pts

3 Chemical Naming Formative Assessment 3

Directions – You can use your Periodic & Polyatomic tables and help sheet. Circle the answers below to best name the below chemicals. Type I, II & III 1. Li2SO4 Lithium Disulfide Lithium Sulfite Lithium Sulfate 2. MgPO3 Magnesium Phosphite Magnesium Phosphate 3. Copper (II) Phosphide Cu2P Cu3P2 4. Cobalt (III) Nitrite Co (NO2)3 Co3NO2 5. Sulfur Trioxide SO3 SO3

2- 6. P4O10 Phosphorus Decoxide Tetraphosphorus Decoxide All Types 7. CoCl2 Cobalt (II) Chloride or Carboxy - Chloride 8. COCl2 Carbonyl Chloride Cobalt (II) Chloride 9. Pb(OH)2 Lead Hydroxide or Lead(II) hydroxide Lead Dihydroxide 10. OF2 Oxygen Fluoride Oxygen difluoride Fluoroxide

25

25 ↑

___________________________ First Name, Last ________

Period

SCORE: ___/10 pts


Directions - Circle the answers below to best name the below chemicals. Type I – Regular Metals 1. Li2S Lithium Disulfide or Lithium Sulfide 2. Mgl2 Magnesium Di-iodide or Magnesium Iodide Type II – Transition Metals (hint: what is the charge on the metal?) 3. Cul2 Copper (I) Iodide or Copper (II) Iodide 4. CoF3 Cobalt (III) Fluoride or Cobalt (I) Fluoride Type III 5. Carbon Dioxide CO2 or C2O 6. Tetraphosphorus Decoxide 4P10O or P4O10 All Types 7. CoCl2 Cobalt (II) Chloride or Cobalt (I) Chloride or Cobalt Chloride 8. CoCl Cobalt (II) Chloride or Cobalt (I) Chloride or Cobalt Chloride 9. Ba(OH)2 Barium Hydroxide or Barium Dihydroxide 10. SiO2 Silicon Dioxide or Silicon (IV) Oxide

26

26 ↑

___________________________ First Name, Last ________

Period

SCORE: ___/10 pts


Directions - Circle the answers below to best name the below chemicals. Type I – Regular Metals 1. Li2O Lithium Dioxide or Lithium Oxide 2. BaCl2 Barium Chloride or Barium Dichloride 3. Al2S3 Aluminum Sulfide or Dialuminum Trisulfide Type II – Transition Metals (hint: what is the charge on the metal?) 4. CuCl2 Copper (I) Chloride or Copper (II) Chloride 5. FeF3 Iron (III) Flouride or Iron (I) Flouride 6. PbO Lead (II) Oxide or Lead (IV) Oxide Type I & II (hint: some answers are above). 7. Iron (III) Flouride Fe3F or FeF3 8. Lead (II) Oxide Pb2O or PbO 9. Barium Chloride BaCl or BaCl2 10. Lead (IV) Chloride Pb4Cl or or PbCl4

27

27 ↑

Na

Cl

Coun

ting Atom

s In Crystals

Ch

emical Nam

e

Ions Present

Chem

ical

Form

ula

Chem

ical Structure

How

man

y

atom

s?

Total

Atom

s Ad

d & Total

Charge

Ch

arge

Ex:1

Sodium

Chloride

Na+

Cl‐

(Cross charges)

NaCl

Na: 1

Cl: 1

2

+1‐1 = 0

Ex:2

Iro

n III Nitrate

Fe3+ N

O31‐

(Cross charges)

Fe(NO

3)3

Fe

N

N

N

O O

O O O

O O

O O

Fe:1

N: 3

O: 9

13

1(3+) +

3(‐1) =

3 ‐ 3 = 0

1

Cu

2+Cl

1‐

2

Chromium II______

CrSO

4

Cr:

S:

O:

3

Cr3+SO

42‐

4

Sr

S S S

O O O O O O O O O

17

5 Am

mon

ium Sulfid

e

N

H4+

N:

H:

S:

2(+1) +

1(2‐) =

=

6 Alum

inum

Nitrite

(NO

2)3

7

Al:2

O:3

Que

stions: 1. What d

o all the

total charges all add up

to?_____

4. A

re crystals ion

ic or m

olecular?

2. W

hy do all of the

charges always a

dd up to th

e above answ

er?

5. W

hy (for #4)?

3. W

hat w

ould be the form

ula if we had 2 form

ula un

its of C

hrom

ium II Su lfate? ____________

How

abo

ut

6. Two form

. U. of A

luminum

Nitrate?___

28

28 ↑

1 naming first name, last name score /...

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