C h ap te r 6 : C h e mi c al B on d smrbakerphysical.weebly.com/uploads/3/0/8/0/30809369/ch6_7_pack.pdfDescribing Molecular Compounds Group #_____ Main Idea ... 1. Describe a covalent

Chapter 6: Chemical Bonds Section 6.1: Ionic Bonding I. Stable Electron Configurations Group #_____

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Drawing_________________ A. Transfer of Electrons Group #_____

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Drawing_________________ A. Crystal Lattices Group #_____

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Section 6.2: Covalent Bonding I. Covalent Bonds Group #_____

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B. Molecules of Elements Group #_____ Main Idea:

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Drawing_________________ A. Polar Covalent Bonds Group #_____

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Drawing________________ B. Polar and Nonpolar Molecules Group #_____

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Drawing_________________ Section 6.3: Naming Compounds and Writing Formulas I. Describing Ionic Compounds Group #_____

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Drawing_________________ A. Binary Ionic Compounds Group #_____

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II. Describing Molecular Compounds Group #_____ Main Idea:

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A. Naming Molecular Compounds Group #_____ Main Idea:

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B. Writing Molecular Formulas Group #_____ Main Idea:

Drawing_________________ Section 6.4: The Structure of Metals I. Metallic Bonds Group #_____

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II. Explaining Properties of Metals Group #_____ Main Idea:

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III. Alloys Group #_____ Main Idea:

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A. Copper Alloys Group #_____ Main Idea:

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B. Steel Alloys Group #_____ Main Idea:

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C. Other Alloys Group #_____ Main Idea:

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Chapter 7: Chemical Reactions Section 7.1: Describing Reactions I. Chemical Equations Group #_____

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Drawing_______________ A. Using Equations to Represent Reactions Group #_____

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Drawing________________ B. Conservation of Mass Group #_____

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Drawing________________ A. Molar Mass Group #_____

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Drawing_________________ B. Mole-Mass Conversions Group #_____

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IV. Chemical Calculations Group #______ Main Idea:

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A. Converting Mass to Moles Group #_____ Main Idea:

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B. Using Mole Ratios Group #_____ Main Idea:

Drawing_______________ C. Converting Moles to Mass Group #_____

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Drawing_________________ Section 7.2: Types of Reactions I. Classifying Reactions Group #_____

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Drawing_______________ A. Synthesis Group #_____

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Drawing________________ B. Decomposition Group #_____

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II. Reactions as Electron Transfers Group #_____ Main Idea:

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B. Reduction Group #_____ Main Idea:

Drawing_________________ Section 7.3: Energy Changes in Reactions I. Chemical Bonds and Energy Group #_____

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Drawing_________________ A. Breaking Bonds Group #_____

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Drawing_________________ B. Forming Bonds Group #_____

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II. Exothermic and Endothermic Reactions Group #_____ Main Idea:

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Drawing_________________ B. Endothermic Reactions Group #_____

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Drawing_________________ Section 7.4: Reaction Rates I. Reactions Over Time Group #_____

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Drawing_________________ A. Temperature Group #_____

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Drawing_________________ Section 7.5: Equilibrium I. Types of Equilibria Group #_____

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B. Chemical Equilibrium Group #_____ Main Idea:

Drawing_________________ II. Factors Affecting Chemical Equilibrium Group #______

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Drawing_________________ A. Temperature Group #_____

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Drawing_________________ D. Catalysts Group #_____

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Chapter 6 Chemical Bonds

Section 6.1 Ionic Bonding (pages 158–164)This section describes the formation of ionic bonds and the properties of ioniccompounds.

Reading Strategy (page 158)

Sequencing As you read, complete the concept map to show whathappens to atoms during ionic bonding. For more information on thisReading Strategy, see the Reading and Study Skills in the Skills andReference Handbook at the end of your textbook.

Stable Electron Configurations (page 158)

1. Describe the type of electron configuration that makes an atom stable and not likely to react.

2. Describe an electron dot diagram.

Ionic Bonds (pages 159–161)

3. Some elements achieve stable electron configurations through thetransfer of between atoms.

4. By losing one valence electron, a sodium atom achieves the sameelectron arrangement as an atom of .

5. Circle the letter that states the result of a sodium atom transferringan electron to a chlorine atom. a. Each atom ends up with a more stable electron arrangement.b. The sodium atom becomes more stable, but the chlorine atom

becomes less stable.c. The chlorine atom becomes more stable, but the sodium atom

becomes less stable.d. Each atom ends up with a less stable electron arrangement.

6. Is the following sentence true or false? An ion is an atom that has anet positive or negative electric charge.

7. An ion with a negative charge is called a(n) .

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Physical Science Guided Reading and Study Workbook ■ Chapter 6 43

Atom

loseselectrons

to

gainselectrons

to

8. An ionic bond forms when are transferredfrom one atom to another.

9. Is the following sentence true or false? The lower the ionizationenergy, the easier it is to remove an electron from an atom.

Ionic Compounds (pages 161–164)

10. Circle the letter of each piece of information provided by thechemical formula of an ionic compound.a. which elements the compound containsb. the charge on each ion in the compoundc. how the ions are arranged in the compoundd. the ratio of ions in the compound

11. Circle the letter of the correct answer. The formula for magnesiumchloride is MgCl2. The charge on the magnesium ion is 2�. What isthe charge on each chloride ion?a. 2� b. 1�

c. 0 d. 1�

12. Look at the arrangement of ions in a sodium chloride crystal. How many sodium ions surround each chloride ion in this three-dimensional structure?a. 3 b. 4c. 6 d. 8

13. The shape of an ionic crystal depends on .14. Identify two factors that determine the arrangement of ions in an

ionic crystal. a. b.

15. Is the following sentence true or false? The attractions among ionswithin a crystal lattice are weak.

Name ___________________________ Class ___________________ Date _____________


44 Physical Science Guided Reading and Study Workbook ■ Chapter 6

Na� Cl�

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

Name ___________________________ Class ___________________ Date _____________


Section 6.2 Covalent Bonding(pages 165–169)This section discusses the formation of covalent bonds and the factors thatdetermine whether a molecule is polar or nonpolar. It also discussesattractions between molecules.


Relating Text and Visuals As you read the section, look closely atFigure 9. Complete the table by describing each type of model shown.For more information on this Reading Strategy, see the Reading andStudy Skills in the Skills and Reference Handbook at the end ofyour textbook.

Molecular Models

Model Description

Electron dot

Structural formula

Space-filling

Electron cloud

Covalent Bonds (pages 165–167)

1. Describe a covalent bond.

2. Circle the letters of molecular models that show orbitals of atomsoverlapping when a covalent bond forms. a. electron dot b. structural formulac. space-filling d. electron cloud

3. Describe a molecule.

4. Is the following sentence true or false? In a covalent bond, the atomsare held together by the attractions between the shared electronsand the protons in each nucleus.

5. Circle the correct answer. Nitrogen has five valence electrons. Howmany pairs of electrons must two nitrogen atoms share in order foreach atom to have eight valence electrons?

a. zero b. onec. two d. three

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Unequal Sharing of Electrons (pages 167–168)

6. In general, elements at the of a group have a greater attraction for electrons than elements at the

of a group have.7. In a hydrogen chloride molecule, the shared electrons spend

more time near the atom than near theatom.

8. Describe a polar covalent bond.

9. When atoms form a polar covalent bond, the atom with the greaterattraction for electrons has a partial charge.

10. Is the following sentence true or false? In a molecule of acompound, electrons are always shared equally by both atoms.

11. Circle the letter of each factor that determines whether a moleculeis polar or nonpolar.a. the number of atoms in the moleculeb. the type of atoms in the moleculec. the number of bonds in the moleculed. the shape of the molecule

12. Compare the shapes of carbon dioxide and water molecules. Circlethe letter of the polar molecule. a. carbon dioxide b. water

13. Is the following sentence true or false? In a water molecule, thehydrogen side of the molecule has a partial positive charge, andthe oxygen side has a partial negative charge.

Attraction Between Molecules (page 169)

14. Water has a higher boiling point than carbon dioxide becauseattractions between polar molecules are thanattractions between nonpolar molecules.

15. Is the following sentence true or false? Attractions amongnonpolar molecules explain why nitrogen can be stored as a liquidat low temperatures and high pressures.

Name ___________________________ Class ___________________ Date _____________



CO2 H2O

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

Name ___________________________ Class ___________________ Date _____________


Section 6.3 Naming Compounds and Writing Formulas(pages 170–175)This section explains how to name and write formulas for ionic and molecular compounds.


Predicting Before you read, predict the meaning of the termpolyatomic ion, and write your prediction in the table. After you read, if your prediction was incorrect, revise your definition. For more information on this Reading Strategy, see the Reading andStudy Skills in the Skills and Reference Handbook at the end of your textbook.

Vocabulary Term Before You Read After You Read

Polyatomic ion

Describing Ionic Compounds (pages 171–173)

1. Is the following sentence true or false? The name of an ioniccompound must distinguish the compound from other ioniccompounds containing the same elements.

2. What information is provided by the formula for an ionic compound?

3. Circle the letter of the word that describes a compound made fromonly two elements.a. ionic b. binary c. diatomic d. polar

4. Is the following sentence true or false? Names of anions are formedby placing the suffix -ide after part of the name of the nonmetal.

5. When a metal forms more than one ion, the name of the ion contains a Roman numeral to indicate the on the ion.

6. What is a polyatomic ion?

7. Is the following sentence true or false? Because all compounds areneutral, the total charges on the cations and anions in the formula ofan ionic compound must add up to zero.


charge

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8. Circle the letter of the correct answer. The formula for sodiumsulfide is Na2S. The sodium ion has a charge of 1�. What must thecharge on the sulfide ion be?a. 1� b. 0c. 1� d. 2�

9. Circle the letter that identifies the number of ammonium ionsneeded to form a compound with one phosphate ion.a. one b. twoc. three d. four

Describing Molecular Compounds (pages 174–175)

10. What information is provided by the name and formula of a molecular compound?

11. Describe the general rule for naming molecular compounds.

12. Is the following sentence true or false? The formula for a molecularcompound is written with the symbols for the elements in thesame order as the elements appear in the name of the compound.

13. Circle the letter that identifies the method of naming the numberof atoms in molecular compounds.a. prefix b. suffixc. number d. symbol

14. In the formula of a molecular compound, the number of atoms ofan element in the molecule is represented by a(n)

.

Name ___________________________ Class ___________________ Date _____________

Chapter 6 Chemical Bonds©

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


Name Formula FormulaName

Some Polyatomic Ions

Ammonium

Hydroxide

Nitrate

Sulfate

Carbonate

Phosphate

Acetate

Peroxide

Permanganate

Hydrogen sulfate

Hydrogen carbonate

Hydrogen phosphate

C2H3O2�

O22�

MnO4�

HSO4�

HCO3�

HPO42�

NH4�

OH�

NO3�

SO42�

CO32�

PO43�

Name ___________________________ Class ___________________ Date _____________


Section 6.4 The Structure of Metals(pages 176–181)This section discusses metallic bonds and the properties of metals. It alsoexplains how the properties of an alloy are controlled.


Relating Cause and Effect As you read, complete the concept map torelate the structure of metals to their properties. For more informationon this Reading Strategy, see the Reading and Study Skills in theSkills and Reference Handbook at the end of your textbook.

1. Circle the letter of the metal with the highest melting point.a. gold b. vanadiumc. titanium d. tungsten

2. Is the following sentence true or false? The properties of a metal arerelated to bonds within the metal.

Metallic Bonds (pages 176–177)

3. Describe a metallic bond.

4. The cations in a metal form a lattice. What holds the lattice in place?

5. Is the following sentence true or false? The more valence electrons a metal has, the stronger its metallic bonds will be.

Explaining Properties of Metals (page 177)

6. Some of the properties of metals can be explained by theof the electrons within a metal lattice.

7. Name two important properties of metals that can be explained bymetallic bonding.a. b.

Alloys (pages 178–181)

8. Circle the letter of the percentage of gold in jewelry that is labeled18-karat gold.a. 18 percent b. 50 percentc. 75 percent d. 100 percent

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Mobileelectrons produce

9. Is the following sentence true or false? When a metal such ascopper is mixed with gold, the gold becomes softer.

10. Describe an alloy.

11. How do the hardness and strength of bronze compare to the hardness andstrength of copper alone and tin alone?

12. Name two factors that scientists can vary to design alloys withspecific properties.a.b.

13. Complete the following table.

Comparing Bronze and Brass

Alloy Component Metals Comparative Hardness Comparative Speedof Bronze and Brass of Weathering

Bronze Copper, tin Weathers more slowly

Brass Softer

14. When carbon is added to iron, the lattice becomesthan a lattice that contains only iron.

15. Circle the letters of the elements that all types of steel contain.a. carbon b. chromiumc. iron d. manganese

16. Circle the letters of each correct description of stainless steel.a. Stainless steel contains more carbon than chromium.b. Chromium forms an oxide that protects stainless steel

from rusting.c. Stainless steel is more brittle than steels that contain

more carbon.d. Stainless steel contains more than 3 percent carbon by mass.

17. Explain why pure aluminum is not the best material for the body of a plane.

18. What type of alloy is used to make airplane parts that need to beextremely lightweight?

Name ___________________________ Class ___________________ Date _____________

Chapter 6 Chemical Bonds©



Name ___________________________ Class ___________________ Date _____________

Chapter 7 Chemical Reactions

Section 7.1 Describing Reactions (pages 192–198)This section discusses the use of chemical equations and how to balance them.It also demonstrates the use of calculations in chemistry.


Monitoring Your Understanding Preview the Key Concepts, topicheadings, vocabulary, and figures in this section. List two things you expect to learn. After reading, state what you learned about each item you listed. For more information on this Reading Strategy,see the Reading and Study Skills in the Skills and ReferenceHandbook at the end of your textbook.

What I Expect to Learn What I Learned

Chemical Equations (pages 192–193)

1. Is the following sentence true or false? The new substances formedas a result of a chemical reaction are called products.

2. Circle the letter of each sentence that is a correct interpretation ofthe chemical equation C � O2 h CO2.a. Carbon and oxygen react and form carbon monoxide.b. Carbon and oxygen react and form carbon dioxide.c. Carbon dioxide yields carbon and oxygen.d. The reaction of carbon and oxygen yields carbon dioxide.

3. Is the following sentence true or false? The law of conservation of mass states that mass is neither created nor destroyed in achemical reaction.

4. Circle the letter of the correct answer. According to the equation C � O2 h CO2, how many carbon atoms react with 14 moleculesof oxygen to form 14 molecules of carbon dioxide?a. 1 b. 7c. 14 d. 28

5. In the reaction represented by the equation C � O2 h CO2, the mass of carbon dioxide produced equals

.

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Balancing Equations (pages 194–195)

6. Is the following sentence true or false? A chemical equation mustbe balanced in order to show that mass is conserved during areaction.

7. Circle the letter of the name given to the numbers that appearbefore the formulas in a chemical equation.a. subscripts b. mass numbersc. atomic numbers d. coefficients

8. Is the following sentence true or false? Because the equationN2H4 � O2 h N2 � H2O has two nitrogen atoms on each side,the equation is balanced.

Counting With Moles (pages 195–196)

9. Chemists use a counting unit called a(n) tomeasure amounts of a substance because chemical reactions ofteninvolve large numbers of small particles.

10. Circle the letter of the correct answer. If one carbon atom has anatomic mass of 12.0 amu and one oxygen atom has an atomic massof 16.0 amu, what is the molar mass of carbon dioxide?a. 28.0 amu b. 44.0 amuc. 28.0 g d. 44.0 g

11. Circle the letter of the correct answer. To convert grams of carbondioxide to moles of carbon dioxide, you must multiply by whichconversion factor?

a. b.

c. d.

Chemical Calculations (pages 197–198)

12. Complete the table.

Formation of Water

Equation 2H2 + O2 h 2H2O

Amount 2 mol 1 mol

Molar Mass 2.0 g/mol 18.0 g/mol

Mass (Moles � Molar Mass) 32.0 g 36.0 g

13. Circle the letter of the correct answer. One mole of oxygen has amass of 32 grams. What is the mass of four moles of oxygen?a. 128 g b. 144 gc. 128 amu d. 144 amu

1 mol CO2

28.0 g CO2

28.0 g CO2

1 mol CO2

1 mol CO2

44.0 g CO2

44.0 g CO2

1 mol CO2

Name ___________________________ Class ___________________ Date _____________

Chapter 7 Chemical Reactions©



Name ___________________________ Class ___________________ Date _____________


Section 7.2 Types of Reactions(pages 199–205)This section discusses how chemical reactions are classified into different types.


Previewing Skim the section and begin a concept map like the one below that identifies types of reactions with a general form. As you read, add the general form of each type of reaction. For moreinformation on this Reading Strategy, see the Reading and Study Skillsin the Skills and Reference Handbook at the end of your textbook.

Classifying Reactions (pages 199–204)

1. Name five general types of chemical reactions.

2. Circle the letter of each equation that represents a synthesis reaction.a. 2Na � Cl2 h 2NaClb. 2NaCl h 2Na � Cl2

c. 2H2O h 2H2 � O2

d. 2H2 � O2 h 2H2O3. Is the following sentence true or false? A decomposition reaction is

the opposite of a synthesis reaction. 4. Write the equation for the decomposition of calcium carbonate into calcium oxide

and carbon dioxide.

5. Circle the letter of the correct answer. Copper reacts with silvernitrate in a single-replacement reaction. What are the products ofthis reaction?a. copper(II) nitride and silver oxideb. copper(II) nitrate and silverc. copper(II) oxide and silver nitrated. copper, nitrogen, and silver oxide

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Types of Reactions

A � B h AB

SynthesisSingle

Replacement

6. What is a double-replacement reaction?

7. Complete the chart by filling in the general forms of the reactions shown.

General Forms

Single-Replacement Reaction Double-Replacement Reaction

8. Lead(II) nitrate reacts with potassium iodide to form lead(II) iodide and potassium nitrate. Write the balanced equation for this double-replacement reaction.

9. Circle the letter of the correct answer. Calcium carbonate, CaCO3,reacts with hydrochloric acid, HCl, in a double-replacementreaction. What are the products of this reaction?a. calcium chloride, CaCl2, and carbonic acid, H2CO3

b. calcium hydride, CaH2, chlorine, Cl2, and carbon dioxide, CO2

c. calcium hydrogen carbonate, Ca(HCO3)2, and chlorine, Cl2

d. calcium perchlorate, Ca(ClO4)2, and methane, CH4

10. Is the following sentence true or false? A combustion reaction is areaction in which a substance reacts with carbon dioxide, oftenproducing heat and light.

11. Methane, CH4, burns in oxygen to form carbon dioxide and water. Write the balanced equation for this reaction.

12. Is the following sentence true or false? The reaction that formswater can be classified as either a synthesis reaction or acombustion reaction.

Reactions as Electron Transfers (pages 204–205)

13. What is an oxidation-reduction reaction?

14. Calcium reacts with oxygen to form calcium oxide. Which reactantis oxidized in this reaction?

15. Is the following sentence true or false? When calcium reacts withoxygen, each calcium atom gains two electrons and becomes acalcium ion with a charge of 2–.

16. Is the following sentence true or false? Oxygen must be present inorder for an oxidation-reduction reaction to take place.

17. The process in which an element gains electrons during a chemicalreaction is called .

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Section 7.3 Energy Changes in Reactions(pages 206–209)This section discusses how chemical bonds and energy relate to chemical reactions.


Comparing and Contrasting As you read, complete the Venndiagram below to show the differences between exothermic andendothermic reactions. For more information on this Reading Strategy,see the Reading and Study Skills in the Skills and ReferenceHandbook at the end of your textbook.

Exothermic Reaction Endothermic Reaction

Chemical Bonds and Energy (pages 206–207)

1. What is chemical energy?

2. Chemical reactions involve the breaking of chemical bonds in the reactants and the formation of chemical bonds in the .

3. Is the following sentence true or false? The formation of chemicalbonds absorbs energy.

4. What role does the spark from the igniter play in the reaction that takes place when propane is burned in a gas grill?

5. Is the following sentence true or false? The heat and light given off by a propane stove result from the formation of new chemicalbonds.

6. The combustion of one molecule of propane (C3H8) results in theformation of C�O double bonds and

O�H single bonds.© Pe

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Chemicalbonds are

broken andformed.

Exothermic and Endothermic Reactions (pages 208–209)

7. During a chemical reaction, energy is either released or.

8. Is the following sentence true or false? Physical and chemicalchanges can be either exothermic or endothermic changes.

9. What is an exothermic reaction?

10. Is the following sentence true or false? In exothermic reactions, theenergy required to break the bonds in the reactants is greater thanthe energy released as the products form.

11. Circle the letter of each sentence that is correct for the graph above.a. The energy required to break the bonds in the reactants is

greater than the energy released as the products form.b. The energy released as the products form is greater than the

energy required to break the bonds in the reactants.c. The chemical energy of the reactants is greater than the

chemical energy of the products.d. The chemical energy of the products is greater than the

chemical energy of the reactants.12. In an exothermic reaction, the difference between the chemical energy

of the reactants and the chemical energy of the products equals .

13. Where does the energy term appear in the equation for an endothermic reaction?

Conservation of Energy (page 209)

14. In an endothermic reaction, heat from the surroundings plus thechemical energy of the reactants is converted into the

.

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Reaction Progress

Ch

emic

al E

ner

gy

Reaction Energy—Exothermic

Reactants

Products

Energyreleased

by reaction

Name ___________________________ Class ___________________ Date _____________


Section 7.4 Reaction Rates(pages 212–215)This section discusses the factors that affect reaction rates.


Building Vocabulary As you read, complete the web diagram belowwith key terms from this section. For more information on thisReading Strategy, see the Reading and Study Skills in the Skills andReference Handbook at the end of your textbook.

Reactions Over Time (page 212)

1. Any change that happens over time can be expressed as a(n).

2. What is a reaction rate?

Factors Affecting Reaction Rates (pages 213–215)

3. Is the following sentence true or false? One way to observe the rateof a reaction is to observe how fast products are being formed.

4. Is the following sentence true or false? The rate of any reaction is aconstant that does not change when the reaction conditions change.

5. Generally, an increase in temperature will the reaction rate.

6. Is the following sentence true or false? Storing milk in a refrigeratorstops the reactions that would cause the milk to spoil.

7. How does an increase in surface area affect the exposure of reactants to oneanother?

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Factors affecting reaction rates

8. Why does increasing the surface area of a reactant tend to increase the reaction rate?

9. Stirring the reactants in a reaction mixture will generallythe reaction rate.

10. Is the following sentence true or false? Increasing theconcentration of the reactants will generally slow down a chemicalreaction.

11. Is the following sentence true or false? A piece of material dippedin a concentrated dye solution will change color more quickly thanin a dilute dye solution.

12. Why does an increase in pressure speed up the rate of a reaction involving gases?

13. What is a catalyst?

14. Circle the letters of the sentences that correctly identify whychemists use catalysts. a. to speed up a reactionb. to enable a reaction to occur at a higher temperaturec. to slow down a reactiond. to enable a reaction to occur at a lower temperature

15. Is the following sentence true or false? Because a catalyst is quicklyconsumed in a reaction, it must be added to the reaction mixtureover and over again to keep the reaction going.

16. Identify where the catalyst V2O5 should go in the formula shownand write it in the correct location.

2SO2 � O2 h 2SO3

17. Circle the letter of the correct answer. In the reaction representedby the equation 2H2O2 h 2H2O + O2, which substance acts as acatalyst?a. H2O2 b. Ptc. H2O d. O2

18. One way that a catalyst can lower the energy barrier of a reaction is by providing a surface on which the can come together.

Name ___________________________ Class ___________________ Date _____________




Pt

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Section 7.5 Equilibrium(pages 216–219)This section explains physical and chemical equilibria, and describes thefactors that affect chemical equilibrium.


Outlining As you read, make an outline of the most important ideasfrom this section. For more information on this Reading Strategy, seethe Reading and Study Skills in the Skills and Reference Handbookat the end of your textbook.

I. Equilibrium

A. Types of Equilibria

1.

2.

B.

1. Temperature

2. Pressure

3.

Types of Equilibria (pages 216–217)

1. What is equilibrium?

2. Circle the letter of the correct answer. In the system described by theequation H2O(l) m H2O(g), at room temperature, which of thefollowing two physical changes are in equilibrium?a. sublimation and condensationb. evaporation and meltingc. sublimation and depositiond. evaporation and condensation

3. What happens when a physical change does not go to completion?

4. What does the single arrow imply about the reaction described in the following equation?

CH4(g) + 2O2(g) h CO2(g) + 2H2O(g) © Pe

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5. Circle the letter of the correct answer. In the system described bythe equation 2SO2(g) � O2(g) m 2SO3(g), what two reactiontypes are in equilibrium?a. synthesis and decomposition b. single replacement and decompositionc. synthesis and combustion d. synthesis and double replacement

6. What happens when a chemical change does not go to completion?

Factors Affecting Chemical Equilibrium (pages 218–219)

7. Is the following sentence true or false? A change in reactionconditions does not affect a chemical equilibrium.

8. Circle the letter of each correct answer. The synthesis of ammoniais described by the equation N2(g) � 3H2(g) m 2NH3(g) � heat.Which reaction is favored when the temperature is lowered?a. the forward reactionb. the reverse reactionc. the reaction that removes heat from the systemd. the reaction that adds heat to the system

9. Circle the letter of each correct answer. During the synthesis of ammonia, which reaction is favored when hydrogen is added to the system?a. the forward reactionb. the reverse reactionc. the reaction that removes hydrogen from the systemd. the reaction that adds hydrogen to the system

10. According to Le Châtelier’s principle, how does lowering the concentration of areaction product affect a chemical equilibrium?

11. Use the equation C(s) + H2O(g) + heat m CO(g) + H2(g) tocomplete the table below.

An Example of Le Châtelier’s Principle

An increase in Shifts the equilibrium so as to Favoring the

Remove heat Forward reaction

Pressure Produce fewer gas molecules

Concentration of H2 Reverse reaction

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