Table of Contents vii

Student Guide

Reading for Information . . . . . . . . . . xviiiScavenger Hunt. . . . . . . . . . . . . . . . . . . .xxi

Chapter 1Introduction to Chemistry . . . . . . . . . . . . 21.1 A Story of Two Substances. . . . . . . . . . . . . . . . . . . . .41.2 Chemistry and Matter . . . . . . . . . . . . . . . . . . . . . . . .91.3 Scientific Methods . . . . . . . . . . . . . . . . . . . . . . . . . .121.4 Scientific Research. . . . . . . . . . . . . . . . . . . . . . . . . .17

Chapter 2Analyzing Data . . . . . . . . . . . . . . . . . . . . 302.1 Units and Measurements. . . . . . . . . . . . . . . . . . . . .322.2 Scientific Notation and Dimensional Analysis . . . . .402.3 Uncertainty in Data . . . . . . . . . . . . . . . . . . . . . . . . .472.4 Representing Data. . . . . . . . . . . . . . . . . . . . . . . . . .55

Chapter 3Matter—Properties and Changes . . . . . 683.1 Properties of Matter . . . . . . . . . . . . . . . . . . . . . . . .703.2 Changes in Matter. . . . . . . . . . . . . . . . . . . . . . . . . .763.3 Mixtures of Matter . . . . . . . . . . . . . . . . . . . . . . . . .803.4 Elements and Compounds. . . . . . . . . . . . . . . . . . . .84

Chapter 4The Structure of the Atom. . . . . . . . . . 1004.1 Early Ideas About Matter. . . . . . . . . . . . . . . . . . . .1024.2 Defining the Atom . . . . . . . . . . . . . . . . . . . . . . . . .1064.3 How Atoms Differ . . . . . . . . . . . . . . . . . . . . . . . . .1154.4 Unstable Nuclei and Radioactive Decay . . . . . . . .122

Chapter 5Electrons in Atoms . . . . . . . . . . . . . . . . 1345.1 Light and Quantized Energy . . . . . . . . . . . . . . . . .1365.2 Quantum Theory and the Atom . . . . . . . . . . . . . . .1465.3 Electron Configuration. . . . . . . . . . . . . . . . . . . . . .156

Chapter 6The Periodic Table and Periodic Law. . 1726.1 Development of the Modern Periodic Table . . . . . .1746.2 Classification of the Elements . . . . . . . . . . . . . . . .1826.3 Periodic Trends. . . . . . . . . . . . . . . . . . . . . . . . . . . .187

THEMES are overarching concepts used throughout the entire book that help you tie what you learn together. They help you see the connec-tions among major ideas and concepts.

BIG Idea appear in each chapter and help you focus on topics within the themes. The Big Ideas are broken down even further into Main Ideas.

MAIN Idea draw you into more specific details about chemistry. All the Main Ideas of a chapter add up to the chapter’s Big Idea.

Your book is divided into chapters that are organized around Themes, Big Ideas, and Main Ideas of chemistry.

BIG Idea

One per chapter

MAIN Idea

One per section

THEMESMatter

Physical and Chemical ChangesBondingEnergy

Equilibrium

viii Table of Contents

Contents

Chapter 7Ionic Compounds and Metals . . . . . . . 2047.1 Ion Formation . . . . . . . . . . . . . . . . . . . . . . . . . . . .2067.2 Ionic Bonds and Ionic Compounds . . . . . . . . . . . .2107.3 Names and Formulas for Ionic Compounds . . . . . .2187.4 Metallic Bonds and the Properties of Metals. . . . .225

Chapter 8Covalent Bonding . . . . . . . . . . . . . . . . . 2388.1 The Covalent Bond . . . . . . . . . . . . . . . . . . . . . . . .2408.2 Naming Molecules. . . . . . . . . . . . . . . . . . . . . . . . .2488.3 Molecular Structures . . . . . . . . . . . . . . . . . . . . . . .2538.4 Molecular Shapes . . . . . . . . . . . . . . . . . . . . . . . . .2618.5 Electronegativity and Polarity . . . . . . . . . . . . . . . .265

Chapter 9 Chemical Reactions . . . . . . . . . . . . . . . 2809.1 Reactions and Equations . . . . . . . . . . . . . . . . . . . .2829.2 Classifying Chemical Reactions . . . . . . . . . . . . . . .2899.3 Reactions in Aqueous Solutions. . . . . . . . . . . . . . .299

Chapter 10 The Mole . . . . . . . . . . . . . . . . . . . . . . . . 31810.1 Measuring Matter . . . . . . . . . . . . . . . . . . . . . . . .32010.2 Mass and the Mole . . . . . . . . . . . . . . . . . . . . . . .32510.3 Moles of Compounds . . . . . . . . . . . . . . . . . . . . .33310.4 Empirical and Molecular Formulas . . . . . . . . . . .34110.5 Formulas of Hydrates. . . . . . . . . . . . . . . . . . . . . .351

Chapter 11Stoichiometry . . . . . . . . . . . . . . . . . . . . 36611.1 Defining Stoichiometry . . . . . . . . . . . . . . . . . . . .36811.2 Stoichiometric Calculations . . . . . . . . . . . . . . . . .37311.3 Limiting Reactants. . . . . . . . . . . . . . . . . . . . . . . .37911.4 Percent Yield . . . . . . . . . . . . . . . . . . . . . . . . . . . .385

Chapter 12States of Matter . . . . . . . . . . . . . . . . . . 40012.1 Gases . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .40212.2 Forces of Attraction . . . . . . . . . . . . . . . . . . . . . . .41112.3 Liquids and Solids . . . . . . . . . . . . . . . . . . . . . . . .41512.4 Phase Changes . . . . . . . . . . . . . . . . . . . . . . . . . .425

Chapter 13Gases . . . . . . . . . . . . . . . . . . . . . . . . . . . 44013.1 The Gas Laws . . . . . . . . . . . . . . . . . . . . . . . . . . .44213.2 The Ideal Gas Law . . . . . . . . . . . . . . . . . . . . . . . .45213.3 Gas Stoichiometry . . . . . . . . . . . . . . . . . . . . . . . .460

Chapter 14Mixtures and Solutions . . . . . . . . . . . . 47414.1 Types of Mixtures . . . . . . . . . . . . . . . . . . . . . . . .47614.2 Solution Concentration . . . . . . . . . . . . . . . . . . . .48014.3 Factors Affecting Solvation . . . . . . . . . . . . . . . . .48914.4 Colligative Properties of Solutions. . . . . . . . . . . .498

Chapter 15Energy and Chemical Change . . . . . . . 51415.1 Energy . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .51615.2 Heat . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .52315.3 Thermochemical Equations . . . . . . . . . . . . . . . . .52915.4 Calculating Enthalpy Change . . . . . . . . . . . . . . .53415.5 Reaction Spontaneity . . . . . . . . . . . . . . . . . . . . .542

Chapter 16Reaction Rates . . . . . . . . . . . . . . . . . . . 55816.1 A Model for Reaction Rates. . . . . . . . . . . . . . . . .56016.2 Factors Affecting Reaction Rates . . . . . . . . . . . . .56816.3 Reaction Rate Laws. . . . . . . . . . . . . . . . . . . . . . .57416.4 Instantaneous Reaction Rates and

Reaction Mechanisms . . . . . . . . . . . . . . . . . . . . .578

Chapter 17Chemical Equilibrium . . . . . . . . . . . . . . 59217.1 A State of Dynamic Balance . . . . . . . . . . . . . . . .59417.2 Factors Affecting Chemical Equilibrium . . . . . . . .60617.3 Using Equilibrium Constants . . . . . . . . . . . . . . . .612

Chapter 18Acids and Bases . . . . . . . . . . . . . . . . . . 63218.1 Introduction to Acids and Bases . . . . . . . . . . . . .63418.2 Strengths of Acids and Bases. . . . . . . . . . . . . . . .64418.3 Hydrogen Ions and pH. . . . . . . . . . . . . . . . . . . . .65018.4 Neutralization . . . . . . . . . . . . . . . . . . . . . . . . . . .659

Chapter 19Redox Reactions . . . . . . . . . . . . . . . . . . 67819.1 Oxidation and Reduction. . . . . . . . . . . . . . . . . . .68019.2 Balancing Redox Equations . . . . . . . . . . . . . . . . .689

Table of Contents ix

Contents

Chapter 20Electrochemistry. . . . . . . . . . . . . . . . . . 70620.1 Voltaic Cells. . . . . . . . . . . . . . . . . . . . . . . . . . . . .70820.2 Batteries . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .71820.3 Electrolysis . . . . . . . . . . . . . . . . . . . . . . . . . . . . .728

Chapter 21Hydrocarbons . . . . . . . . . . . . . . . . . . . . 74221.1 Introduction to Hydrocarbons . . . . . . . . . . . . . . .74421.2 Alkanes . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .75021.3 Alkenes and Alkynes . . . . . . . . . . . . . . . . . . . . . .75921.4 Hydrocarbon Isomers. . . . . . . . . . . . . . . . . . . . . .76521.5 Aromatic Hydrocarbons. . . . . . . . . . . . . . . . . . . .770

Chapter 22Substituted Hydrocarbons and

Their Reactions . . . . . . . . . . . . . . . . . 78422.1 Alkyl Halides and Aryl Halides . . . . . . . . . . . . . . .78622.2 Alcohols, Ethers, and Amines. . . . . . . . . . . . . . . .79222.3 Carbonyl Compounds . . . . . . . . . . . . . . . . . . . . .79622.4 Other Reactions of Organic Compounds . . . . . . .80222.5 Polymers . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .809

Chapter 23The Chemistry of Life . . . . . . . . . . . . . . 82423.1 Proteins . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .82623.2 Carbohydrates . . . . . . . . . . . . . . . . . . . . . . . . . . .83223.3 Lipids. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .83523.4 Nucleic Acids . . . . . . . . . . . . . . . . . . . . . . . . . . . .84023.5 Metabolism . . . . . . . . . . . . . . . . . . . . . . . . . . . . .844

Chapter 24Nuclear Chemistry . . . . . . . . . . . . . . . . 85824.1 Nuclear Radiation . . . . . . . . . . . . . . . . . . . . . . . .86024.2 Radioactive Decay . . . . . . . . . . . . . . . . . . . . . . . .86524.3 Nuclear Reactions . . . . . . . . . . . . . . . . . . . . . . . .87524.4 Applications and Effects of Nuclear

Reactions. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .885

Student Resources

Elements Handbook . . . . . . . . . . . . . . . 901Math Handbook . . . . . . . . . . . . . . . . . . 946

Scientific Notation . . . . . . . . . . . . . . . . . . . . . . . . . . .946Operations with Scientific Notation . . . . . . . . . . . . . .948Square and Cube Root . . . . . . . . . . . . . . . . . . . . . . . .949Significant Figures. . . . . . . . . . . . . . . . . . . . . . . . . . . .949Solving Algebraic Equations . . . . . . . . . . . . . . . . . . . .954Dimensional Analysis . . . . . . . . . . . . . . . . . . . . . . . . .956Unit Conversion . . . . . . . . . . . . . . . . . . . . . . . . . . . . .957Drawing Line Graphs . . . . . . . . . . . . . . . . . . . . . . . . .959Using Line Graphs. . . . . . . . . . . . . . . . . . . . . . . . . . . .961Ratios, Fractions, and Percents . . . . . . . . . . . . . . . . . .964Operations Involving Fractions . . . . . . . . . . . . . . . . . .965Logarithms and Antilogarithms. . . . . . . . . . . . . . . . . .966

Reference Tables. . . . . . . . . . . . . . . . . . 968R-1 Color Key . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .968R-2 Symbols and Abbreviations. . . . . . . . . . . . . . . . . .968R-3 Solubility Product Constants . . . . . . . . . . . . . . . . .969R-4 Physical Constants . . . . . . . . . . . . . . . . . . . . . . . .969R-5 Names and Charges of Polyatomic Ions . . . . . . . .970R-6 Ionization Constants . . . . . . . . . . . . . . . . . . . . . . .970R-7 Properties of Elements . . . . . . . . . . . . . . . . . . . . .971R-8 Solubility Guidelines . . . . . . . . . . . . . . . . . . . . . . .974R-9 Specific Heat Values . . . . . . . . . . . . . . . . . . . . . . .975R-10 Molal Freezing-Point Depression and

Boiling-Point Elevation Constants. . . . . . . . . . . .975R-11 Heat of Formation Values . . . . . . . . . . . . . . . . . .975

Supplemental Practice Problems . . . . 976Solutions to Selected Practice

Problems . . . . . . . . . . . . . . . . . . . . . . 992Glossary/Glosario . . . . . . . . . . . . . . . . 1005Index . . . . . . . . . . . . . . . . . . . . . . . . . . 1031Credits . . . . . . . . . . . . . . . . . . . . . . . . . 1051

x Launch Lab

LAUNCH LAUNCH LabLabChapter Chapter

Begin each chapter with a hands-on introduction to the subject matter.

1 Where did the mass go? . . . . . . . . . . . . . . . . . . . 3

2 How can you form layers of liquids? . . . . . . . . . 31

3 How can you observe chemical change? . . . . . . 69

4 How can the effects of electric charges be observed? . . . . . . . . . . . . . . . . . . . . . . . . . . 101

5 How do you know what is inside an atom? . . . 135

6 How can you recognize trends? . . . . . . . . . . . . 173

7 What compounds conduct electricityin solution? . . . . . . . . . . . . . . . . . . . . . . . . . . . 205

8 What type of compound is used to make a Super Ball? . . . . . . . . . . . . . . . . . . . . . . . . . . 239

9 How do you know when a chemical change has occurred?. . . . . . . . . . . . . . . . . . . . . . . . . . 281

10 How much is a mole?. . . . . . . . . . . . . . . . . . . . 319

11 What evidence can you observe that a reaction is taking place? . . . . . . . . . . . . . . . . . 367

12 How do different liquids affect the speed of a sinking ball bearing?. . . . . . . . . . . . . . . . . 401

13 How does temperature affect the volume of a gas? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 441

14 How does energy change when solutions form? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 475

15 How can you make a cold pack? . . . . . . . . . . . 515

16 How can you accelerate a reaction? . . . . . . . . 559

17 What is equal about equilibrium? . . . . . . . . . . 593

18 What is in your cupboards? . . . . . . . . . . . . . . . 633

19 What happens when iron and copper(II) sulfate react? . . . . . . . . . . . . . . . . . . . . . . . . . . 679

20 How can you make a battery from a lemon? . . 707

21 How can you model simple hydrocarbons? . . . 743

22 How do you make slime? . . . . . . . . . . . . . . . . . 785

23 How do you test for simple sugars?. . . . . . . . . 825

24 How do chain reactions occur? . . . . . . . . . . . . 859

Problem-Solving and Data Analysis Labs xi

Labs

PRoblem-solving labPRoblem-solving lab

DATA ANALYSIS labDATA ANALYSIS lab

Chapter Chapter

Build your analytical skills using real-world applications of chemistry concepts.

Build your analytical skills using actual data from real scientific sources.

2 Identify an Unknown: How can mass and volume data for an unknown sample be used to identify the unknown?. . . . . . . . . . . . . . . . . . 50

3 Recognize Cause and Effect: How is compressed gas released? . . . . . . . . . . . . . . . . . 72

5 Interpret Scientific Illustrations: What electron transitions account for the Balmer series? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 150

6 Analyze Trends: Francium—solid, liquid, or gas? . . . . . . . . . . . . . . . . . . . . . . . . . 180

9 Analyze Trends: How can you explain the reactivities of halogens? . . . . . . . . . . . . . . 294

10 Formulate a Model: How are molar mass, Avogadro’s number, and the atomic nucleus related? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 326

13 Apply Scientific Explanations: What does Boyle’s law have to do with breathing?. . . . . . 444

15 Make and Use Graphs: How can you derive the heating curve for water? . . . . . . . . . 531

16 Interpret Data: How does the rate of decomposition vary over time? . . . . . . . . . . . . 566

17 Apply Scientific Explanations: How does the fluoride ion prevent tooth decay? . . . . . . . 622

18 Apply Scientific Explanations: How does your blood maintain its pH?. . . . . . . . . . . . . . . 668

23 Formulate a Model: How does DNA replicate? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 842

24 Interpret Graphs: How does distance affect radiation exposure? . . . . . . . . . . . . . . . . 890

1 Interpret Graphs: How do ozone levels vary throughout the year in Antarctica?. . . . . . . 21

4 Interpret Scientific Illustrations: What are the apparent atomic distances of carbon atoms in a well-defined crystalline material?. . 113

7 Interpret Data: Can embedding nanoparticles of silver into a polymer give the polymer antimicrobial properties? . . . . . . . 216

8 Interpret Data: How does the polarity of the mobile phase affect chromatograms? . . . . 269

11 Analyze and Conclude: Can rocks on the Moon provide an effective oxygen source for future lunar missions? . . . . . . . . . . . . . . . . 387

12 Make and Use Graphs: How are the depth of a dive and altitude related? . . . . . . . . . . . . . 408

14 Design an Experiment: How can you measure turbidity? . . . . . . . . . . . . . . . . . . . . . . 478

19 Analyze and Conclude: How does redox lift a space shuttle? . . . . . . . . . . . . . . . . . . . . . 691

20 Interpret Graphs: How can you get electric current from microbes? . . . . . . . . . . . . . . . . . . 724

21 Interpret Data: What are the rates of oxidation of dichloroethene isomers? . . . . . . . 768

22 Interpret Data: What are the optimal conditions to hydrogenate canola oil? . . . . . . . 805

Chapter Chapter

xii Mini Labs

Labs

Chapter Chapter

13 Model a Fire Extinguisher: Why is carbon dioxide used in fire extinguishers?. . . . . . . . . . 457

14 Examine Freezing Point Depression: How do you measure freezing point depression? . . . . . . . . . . . . . . . . . . . . . . . . . . . 502

15 Determine Specific Heat: How can you determine the specific heat of a metal?. . . . . . 526

16 Examine Reaction Rate and Temperature: What is the effect of temperature on a common chemical reaction? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 571

17 Observe Shifts in Equilibrium: If a stress is placed on a reaction at equilibrium, how will the system shift to relieve the stress? . . . . . . . 611

18 Compare Acid Strengths: How can you determine the relative strengths of acid solutions? . . . . . . . . . . . . . . . . . . . . . . . . . . . . 648

19 Observe a Redox Reaction: How can tarnish be removed from silver?. . . . . . . . . . . . 683

20 Observe Corrosion: Which metal will corrode?. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 726

21 Synthesize and Observe Ethyne: Why is ethyne used in welding torches? . . . . . . . . . . . 763

22 Make an Ester: How can you recognize an ester? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 800

23 Observe A Saponification Reaction: How is soap made? . . . . . . . . . . . . . . . . . . . . . 837

24 Model Radioactive Decay: How do radioactive isotopes decay? . . . . . . . . . . . . . . . 873

1 Develop Observation Skills: Why are observation skills important in chemistry?. . . . . 13

2 Determine Density: What is the density of an unknown and irregularly shaped solid? . . 39

3 Observe Dye Separation: How does paper chromatography allow you to separate substances? . . . . . . . . . . . . . . . . . . . . . . . . . . . . 82

4 Model Isotopes: How can you calculate the atomic mass of an element using the percentage abundance of its isotopes? . . . . . . 120

5 Identify Compounds: How do flame colors vary for different elements? . . . . . . . . . . . . . . . 144

6 Organize Elements: Can you find the pattern? . . . . . . . . . . . . . . . . . . . . . . . . . . . 193

7 Observe Properties: How do the properties of steel change when it is subjected to different types of heat treatment? . . . . . . . . . . 227

8 Compare Melting Points: How can you determine the relationship between bond type and melting point?. . . . . . . . . . . . . . . . . . 242

9 Observe a Precipitate-Forming Reaction: How do two liquids form a solid? . . . . . . . . . . 301

10 Analyze Chewing Gum: Are sweetening and flavoring added as a coating or mixed throughout chewing gum?. . . . . . . . . . . . . . . . 342

11 Apply Stoichiometry: How much sodium carbonate ( Na 2 C O 3 ) is produced when baking soda decomposes?. . . . . . . . . . . . . . . . . . . . . . 378

12 Model Crystal Unit Cells: How can you make physical models that illustrate the structures of crystals? . . . . . . . . . . . . . . . . . . . 423

Practice scientific methods and hone your lab skills with these quick activities.

Chem Labs xiii

Labs

Chapter Chapter

1 Forensics: Identify the Water Source CBL . . . 24

2 Forensics: Use Density to Date a Coin . . . . . . 60

3 Identify the Products of a Chemical Reaction. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 92

4 Model Atomic Mass . . . . . . . . . . . . . . . . . . . . . 126

5 Analyze Line Spectra . . . . . . . . . . . . . . . . . . . . 164

6 Investigate Descriptive Chemistry . . . . . . . . . . 196

7 Synthesize an Ionic Compound . . . . . . . . . . . . 230

8 Model Molecular Shapes . . . . . . . . . . . . . . . . . 272

9 Small Scale: Develop an Activity Series. . . . . 310

10 Determine the Formula of a Hydrate CBL . . . . 356

11 Determine the Mole Ratio CBL . . . . . . . . . . . 390

12 Small Scale Internet: Compare Rates of Evaporation . . . . . . . . . . . . . . . . . . . . . . . . . 432

13 Internet: Determine Pressure in Popcorn Kernels . . . . . . . . . . . . . . . . . . . . . . . . 466

14 Investigate Factors Affecting Solubility . . . . . . 506

15 Internet: Measure Calories CBL . . . . . . . . . . 550

16 Observe How Concentration Affects Reaction Rate CBL . . . . . . . . . . . . . . . . . . . . . 584

17 Small Scale: Compare Two Solubility Product Constants . . . . . . . . . . . . . . . . . . . . . . 624

18 Standardize a Base CBL . . . . . . . . . . . . . . . . . 670

19 Small Scale Forensics: Identify the Damaging Dumper. . . . . . . . . . . . . . . . . . . . . . 698

20 Small Scale: Measure Voltaic Cell Potentials CBL . . . . . . . . . . . . . . . . . . . . . . . . 734

21 Forensics: Analyze Hydrocarbon Burner Gases . . . . . . . . . . . . . . . . . . . . . . . . . . 776

22 Small Scale Internet: Observe Properties of Alcohols . . . . . . . . . . . . . . . . . . . . . . . . . . . . 816

23 Observe Temperature and Enzyme Action CBL . . . . . . . . . . . . . . . . . . . . . . . . . . . 850

24 Investigate Radiation Dosage CBL . . . . . . . . . 892

2 Recognizing Significant Figures . . . . . . . . . . . . . 51

Rounding Numbers . . . . . . . . . . . . . . . . . . . . . . 52

5 Filling Atomic Orbitals. . . . . . . . . . . . . . . . . . . . 160

7 Naming Ionic Compounds . . . . . . . . . . . . . . . . 224

8 Drawing Lewis Structures. . . . . . . . . . . . . . . . . 254

11 Mastering Stoichiometry . . . . . . . . . . . . . . . . . 374

13 Deriving Gas Laws . . . . . . . . . . . . . . . . . . . . . . 458

17 Using Assumptions. . . . . . . . . . . . . . . . . . . . . . 621

18 Calculating Molarity. . . . . . . . . . . . . . . . . . . . . 663

19 Balancing Redox Equations . . . . . . . . . . . . . . . 696

20 Determining Cell Potentials . . . . . . . . . . . . . . . 717

24 Calculating Mass Defect . . . . . . . . . . . . . . . . . 878

Chapter Chapter

Problem-Solving Strategies Learn strategies you can apply to chemistry problems.

Apply the skills you developed in Launch Labs, MiniLabs, Problem-Solving Labs, and Data Analysis Labs in these chapter-culminating, hands-on labs.

CBL Alternate CBL instructions can be found at glencoe.com.

xiv Real-World Chemistry Features

Explore today’s world of chemistry. Learn how things work, discover chemistry in everyday experiences, uncover the links between chemistry and health, and investigate careers in chemistry.

Examine how chemistry helps make familiar things work.

Chapter 4 Mass Spectrometer: Chemical Detective . . 125

Chapter 8 Sticky Feet: How Geckos Grip . . . . . . . . . 271

Chapter 9 Lighting up the Night: Bioluminescence . . 309

Chapter 15 Driving the Future: Flexible Fuel Vehicles . 549

Chapter 20 The Pacemaker: Helping a Broken Heart. . . . . . . . . . . . . . . . . . . . . . . . . . . 733

Chapter 21 Pooch to Power: How a Methane Digester Works . . . . . . . . . . . . . . . . . . . . 775

Discover chemistry in everyday experiences.

Chapter 7 Killer Fashion . . . . . . . . . . . . . . . . . . . . . 229

Chapter 10 History in a Glass of Water . . . . . . . . . . . 355

Chapter 12 Cocoa Chemistry . . . . . . . . . . . . . . . . . . 431

Chapter 18 Acid-Base Reactions on the Rise . . . . . . . 669

Chapter 22 Garlic: Pleasure and Pain. . . . . . . . . . . . . 815

Investigate how chemistry and health are interrelated.

Chapter 2 Toxicology: Assessing Health Risk . . . . . . . 59

Chapter 5 Micro Scissors and Tiny Tweezers . . . . . . . 163

Chapter 6 Elements of the Body . . . . . . . . . . . . . . . 195

Chapter 11 Battling Resistant Strains . . . . . . . . . . . . 389

Chapter 13 Health Under Pressure . . . . . . . . . . . . . . 465

Chapter 16 Reaction Rate and Body Temperature. . . . . . . . . . . . . . . . . . . . . . 583

Chapter 17 Hemoglobin Rises to the Challenge . . . . . 623

Investigate a day in the life of people working in the field of chemistry.

Chapter 1 Career: Art Restorer . . . . . . . . . . . . . . . . . 23

Chapter 3 Career: Arson Investigator . . . . . . . . . . . . . 91

Chapter 14 Career: Environmental Chemist . . . . . . . . 505

Chapter 19 Career: Crime Scene Investigator . . . . . . . 697

Chapter 23 Career: Molecular Paleontologist . . . . . . . 849

Chapter 24 Career: Archaeologist . . . . . . . . . . . . . . . 891

Careers and Concepts in Motion xv

Careers in Chemistry

4 Development of Modern Atomic Theory . . . . . . . . . . . . . . . . . . . . . . . . . 110

6 History of the Periodic Table. . . . . . . . . . . . . . . 184

7 Milestones in Ionic and Metallic Bonding . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 212

9 Real-World Chemical Reactions . . . . . . . . . . . . 290

12 Studying States of Matter . . . . . . . . . . . . . . . . 416

14 Milestones in Solution Chemistry. . . . . . . . . . . 490

18 History of Acids and Bases . . . . . . . . . . . . . . . . 636

22 The Age of Polymers. . . . . . . . . . . . . . . . . . . . . 810

24 The Nuclear Age. . . . . . . . . . . . . . . . . . . . . . . . 882

Chapter Chapter

Chapter 1 Environmental Chemist . . . . . . . . . . . . . . . . 7

Chapter 2 Calibration Technician . . . . . . . . . . . . . . . . 56

Chapter 3 Materials Scientist . . . . . . . . . . . . . . . . . . 81

Chapter 4 Chemistry Teacher . . . . . . . . . . . . . . . . . 123

Chapter 5 Spectroscopist . . . . . . . . . . . . . . . . . . . . 139

Chapter 6 Research Chemist . . . . . . . . . . . . . . . . . . 185

Chapter 7 Food Scientist. . . . . . . . . . . . . . . . . . . . . 219

Chapter 8 Flavor Chemist . . . . . . . . . . . . . . . . . . . . 267

Chapter 9 Biochemist. . . . . . . . . . . . . . . . . . . . . . . 308

Chapter 10 Medicinal Chemist . . . . . . . . . . . . . . . . . 342

Chapter 11 Pharmacist. . . . . . . . . . . . . . . . . . . . . . . 381

Chapter 12 Metallurgist . . . . . . . . . . . . . . . . . . . . . . 423

Chapter 13 Meteorologist . . . . . . . . . . . . . . . . . . . . 447

Chapter 14 Pharmacy Technician. . . . . . . . . . . . . . . . 483

Chapter 15 Heating and Cooling Specialist . . . . . . . . 527

Chapter 16 Chemical Engineer . . . . . . . . . . . . . . . . . 580

Chapter 17 Science Writer . . . . . . . . . . . . . . . . . . . . 604

Chapter 18 Nursery Worker . . . . . . . . . . . . . . . . . . . 646

Chapter 19 Potter . . . . . . . . . . . . . . . . . . . . . . . . . . 682

Chapter 20 Alternative Energy Specialist . . . . . . . . . . 729

Chapter 21 Petroleum Technician . . . . . . . . . . . . . . . 748

Chapter 22 Polymer Chemist . . . . . . . . . . . . . . . . . . 813

Chapter 23 Baker. . . . . . . . . . . . . . . . . . . . . . . . . . . 847

Chapter 24 Radiation Therapist. . . . . . . . . . . . . . . . . 887

Get an inside look at careers in chemistry.

Interactive Time LineExplore science and history through milestones in chemistry.

xvi Concepts in Motion

Chapter Chapter

1 Table 1.1 Some Branches of Chemistry . . . . . . 11

2 Table 2.2 SI Prefixes . . . . . . . . . . . . . . . . . . . . 33

3 Table 3.3 Types of Solution Systems . . . . . . . . 81

4 Table 4.3 Properties of Subatomic Particles . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 114

5 Table 5.4 Electron Configurations and Orbital Diagrams for Elements 1–10 . . . . . . . . 158

Table 5.6 Electron Configurations andDot Structures . . . . . . . . . . . . . . . . . . . . . . . . . 161

6 Table 6.4 Noble Gas Electron Configuration. . . . . . . . . . . . . . . . . . . . . . . . . . 184

7 Table 7.1 Electron-Dot Structures . . . . . . . . . 207

8 Table 8.3 Prefixes in Covalent Compounds . . . . . . . . . . . . . . . . . . . . . . . . . . . 248

Table 8.5 Formulas and Names of Some Covalent Compounds . . . . . . . . . . . . . . . 251

Table 8.6 Molecular Shapes . . . . . . . . . . . . . 263

9 Table 9.2 Steps for Balancing Equations . . . . 286

Table 9.4 Predicting Products of Chemical Reactions . . . . . . . . . . . . . . . . . . . . . 298

10 Table 10.1 Formulas of Hydrates. . . . . . . . . . 351

11 Table 11.1 Relationships Derived from a Balanced Chemical Equation . . . . . . . . . . . . . . 369

12 Table 12.4 Unit Cells. . . . . . . . . . . . . . . . . . . 421

Table 12.5 Types of Crystalline Solids . . . . . . 422

13 Table 13.1 The Gas Laws . . . . . . . . . . . . . . . 451

14 Table 14.2 Types and Examples of Solutions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 479

15 Table 15.6 Reaction Spontaneity . . . . . . . . . 547

18 Table 18.2 Three Models for Acids and Bases . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 642

Table 18.3 Ionization Equations . . . . . . . . . . 645

19 Table 19.1 Summary of Redox Reactions . . . 683

21 Table 21.5 Examples of Alkenes . . . . . . . . . . 759

Table 21.6 Examples of Alkynes . . . . . . . . . . 763

22 Table 22.1 Organic Compounds andTheir Functional Groups . . . . . . . . . . . . . . . . . . 787

Table 22.14 Common Polymers . . . . . . . . . . 812

23 Table 23.1 Amino Acid Examples . . . . . . . . . 827

24 Table 24.3 Summary of Radioactive Decay Processes. . . . . . . . . . . . . . . . . . . . . . . . 868

Interactive Tables Check your understanding by viewing interactive versions of some of the tables in your text.

Concepts in Motion xvii

Chapter Chapter

1 Figure 1.13 Ozone Depletion . . . . . . . . . . . . . 15

2 Figure 2.10 Precision and Accuracy . . . . . . . . 47

3 Figure 3.4 States of Matter. . . . . . . . . . . . . . . 72

Figure 3.10 Conservation of Mass . . . . . . . . . 79

4 Figure 4.12 Gold Foil Experiment . . . . . . . . . 112

Figure 4.14 Structure of the Atom . . . . . . . . 114

Figure 4.21 Radiation Deflection . . . . . . . . . 123

5 Figure 5.11 Balmer Series. . . . . . . . . . . . . . . 147

Figure 5.12 Electron Transitions . . . . . . . . . . 148

Table 5.5 Electron Configurations . . . . . . . . . 159

6 Figure 6.5 The Periodic Table . . . . . . . . . . . . 178

Figure 6.11 Atomic Radii . . . . . . . . . . . . . . . 188

Figure 6.18 Electronegativity . . . . . . . . . . . . 194

7 Table 7.4 Sodium Chloride Ionic Bond . . . . . 211

8 Figure 8.9 Sigma and Pi Bonding . . . . . . . . . 246

Figure 8.19 Molecular Shapes . . . . . . . . . . . 262

Figure 8.22 Bond Types . . . . . . . . . . . . . . . . 267

9 Figure 9.15 Precipitate Formation . . . . . . . . 296

10 Figure 10.6 Molar Mass . . . . . . . . . . . . . . . . 326

11 Figure 11.5 Limiting Reactants. . . . . . . . . . . 380

12 Figure 12.30 Phase Diagram . . . . . . . . . . . . 430

13 Figure 13.3 The Gas Laws. . . . . . . . . . . . . . . 447

14 Figure 14.10 Dissolution of Compounds . . . 490

Figure 14.19 Strong, Weak, and Nonelectrolytes . . . . . . . . . . . . . . . . . . . . . . . . 498

Figure 14.23 Osmosis. . . . . . . . . . . . . . . . . . 504

15 Figure 15.5 Calorimetry . . . . . . . . . . . . . . . . 523

Figure 15.10 Heat Flow in Endothermic and Exothermic Reactions. . . . . . . . . . . . . . . . . . . . 530

16 Figure 16.4 Molecular Orientation and Collision Effectiveness . . . . . . . . . . . . . . . . . . . 564

17 Figure 17.14 Equilibrium Shifts . . . . . . . . . . 610

Figure 17.19 Precipitation Reaction . . . . . . . 618

18 Figure 18.20 Neutralization Reaction. . . . . . 660

Figure 18.21 Titration. . . . . . . . . . . . . . . . . . 660

Figure 18.22 Neutralization Reactions . . . . . 661

19 Figure 19.2 Redox Reaction . . . . . . . . . . . . . 681

20 Figure 20.2 Voltaic Cell . . . . . . . . . . . . . . . . 709

21 Figure 21.17 Isomers of Pentane . . . . . . . . . 765

Figure 21.25 Sigma- and Pi-Bonding in Benzene . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 771

23 Figure 23.21 Structure of DNA . . . . . . . . . . . 841

24 Figure 24.16 Nuclear Chain Reaction . . . . . . 879

Figure 24.17 Critical Mass . . . . . . . . . . . . . . 880

Figure 24.20 Nuclear Power . . . . . . . . . . . . . 881

Interactive Figures Enhance and enrich your knowledge of chemistry concepts through animations of visuals.

Combined

Gas Laws

BoyleCharles

Gay-Lussac

Ideal

Chapter 13 • Gases 441

Start-Up ActivitiesStart-Up Activities

STEP 1 Stack three sheets of paper with the top edges about 2 cm apart vertically.

STEP 2 Fold up the bottom edges of the paper to form five equal tabs. Crease the fold to hold the tabs in place.

STEP 3 Staple along the fold. Label from top to bottom as follows: Gas Laws, Boyle, Charles, Gay-Lussac, Combined, and Ideal.

Use this Foldable with Sections 13.1 and 13.2. As you read the sections, summarize the gas laws in your own words.

LLAAUUNCH NCH LabLabHow does temperature affect the volume of a gas?In the hot-air balloon at left, the burners raise the temper-ature of the air inside the balloon to keep it aloft.

Procedure 1. Read and complete the lab safety form.2. Inflate a round balloon, and tie it closed.3. Pour cold water into a bucket until it is half full, then

add ice. Use paper towels to wipe up any spilled water.

4. Use string to measure the circumference of the balloon.

5. Use a stirring rod to stir the water in the bucket to equalize the temperature. Submerge the balloon in the ice water for 15 min.

6. Remove the balloon from the water. Measure the cir-cumference again.

Analysis1. Describe what happened to the size of the balloon

when its temperature decreased.2. Predict what might happen to the balloon’s size if

the bucket contained warm water.

Inquiry What do you think would happen if you filled the balloon with helium instead of air and repeated the experiment?

The Gas Laws Make the following Foldable to help you organize your study of the gas laws.

Visit glencoe.com to: study the entire chapter online

explore

take Self-Check Quizzes

use the Personal Tutor to work Example Problems step-by-step

access Web Links for more information, projects, and activities

find the Try at Home Lab, Under Pressure

C13_CO_874637.indd 441 1/29/07 4:02:09 PM

440

ChemFacts

• The air inside a hot-air balloon is hot enough to boil water.

• In the nineteenth century, scientist Joseph Gay-Lussac used hot air balloon flights for research and experimentation, while scientist Jacques Charles experimented with hydrogen balloons.

• The average hot-air balloon holds 2.5 million liters of gas.

BIG Idea Gases respond in predictable ways to pressure, temperature, volume, and changes in number of particles.

13.1 The Gas LawsMAIN Idea For a fixed amount of gas, a change in one variable—pressure, temperature, or volume—affects the other two.

13.2 The Ideal Gas LawMAIN Idea The ideal gas law relates the number of particles to pressure, temperature, and volume.

13.3 Gas StoichiometryMAIN Idea When gases react, the coefficients in the balanced chemical equation represent both molar amounts and relative volumes.

Balloon basket

Propane burner

Gases

C13_CO_874637.indd 440 1/29/07 4:01:20 PM

xviii Reading for Information

When you read Chemistry: Matter and Change, you need to read for information. Science is nonfiction writing; it describes real-life events, people, ideas, and technology. Here are some tools that Chemistry: Matter and Change has to help you read.

By reading the BIG Idea , MAIN Idea , and Launch Lab prior to reading the chapter or section, you will get a preview of the coming material.

The BIG Idea describes what you will learn in the chapter. The MAIN Ideas within a chapter support the Big Idea of the chapter. Each section of the chapter has a Main Idea that describes the focus of the section.

❯

Before You Read

Each chapter starts with a hands-on introduction to the material being covered. Read and perform the Launch Lab to discover concepts covered in the chapter.

❮

Source: Chapter 13, p. 440

• Read the chapter title to find out what the topic will be.

• Skim the photos, illustrations, captions, graphs, and tables.

• Look for key terms that are boldfaced and highlighted.

• Create an outline using section titles and heads.

OTHER WAYS TO PREVIEW

Source: Chapter 13, p. 441

452 Chapter 13 • Gases

Section 13.213.2

The Ideal Gas LawMAIN Idea The ideal gas law relates the number of particles to pressure, temperature, and volume.

Real-World Reading Link You know that adding air to a tire causes the pressure in the tire to increase. But did you know that the recommended pressure for car tires is specified for cold tires? As tires roll over the road, friction causes their temperatures to increase. This also causes the pressure to increase.

Avogadro’s PrincipleThe particles that make up different gases can vary greatly in size. However, kinetic-molecular theory assumes that the particles in a gas sample are far enough apart that size has very little influence on the vol-ume occupied by a gas. For example, 1000 relatively large krypton gas particles occupy the same volume as 1000 smaller helium gas particles at the same temperature and pressure. It was Avogadro who first pro-posed this idea in 1811. Avogadro’s principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. Figure 13.5 shows equal volumes of carbon dioxide, helium, and oxygen.

Volume and moles Recall from Chapter 10 that 1 mol contains 6.02 × 1 0 23 particles. The molar volume of a gas is the volume that1 mol occupies at 0.00°C and 1.00 atm pressure. The conditions of 0.00°C and 1.00 atm are known as standard temperature and pressure (STP). Avogadro showed experimentally that 1 mol of any gas occupies a volume of 22.4 L at STP. Because the volume of 1 mol of a gas at STP is 22.4 L, you can use 22.4 L/mol as a conversion factor whenever a gas is at STP.

For example, suppose you want to find the number of moles in a sample of gas that has a volume of 3.72 L at STP. Use the molar volume to convert from volume to moles.

3.72 L × 1 mol

_ 22.4 L

= 0.166 mol

Objectives

◗ Relate number of particles and volume using Avogadro’s principle.

◗ Relate the amount of gas present to its pressure, temperature, and volume using the ideal gas law.

◗ Compare the properties of real and ideal gases.

Review Vocabularymole: an SI base unit used to measure the amount of a substance; the amount of a pure substance that contains 6.02 × 1 0 23 representative particles

New VocabularyAvogadro’s principlemolar volumeideal gas constant (R)ideal gas law

■ Figure 13.5 Gas tanks of equal volume that are at the same pressure and temperature contain equal numbers of gas particles, regardless of which gas they contain.Infer Why doesn’t Avogadro’s principle apply to liquids and solids?

C13_S2_874637.indd 452 1/29/07 4:04:10 PM

Section 13.2 • The Ideal Gas Law 453

EXAMPLE Problem 13.5

Molar Volume The main component of natural gas used for home heating and cooking is methane (C H 4 ). Calculate the volume that 2.00 kg of methane gas will occupy at STP.

1 Analyze the ProblemThe number of moles can be calculated by dividing the mass of the sample, m, by its molar mass, M. The gas is at STP (0.00°C and 1.00 atm pressure), so you can use the molar volume to convert from the number of moles to the volume.

Known Unknownm = 2.00 kg V = ? LT = 0.00ºCP = 1.00 atm

2 Solve for the UnknownDetermine the molar mass for methane.

M = 1 C atom (12.01 amu_1 C atom ) + 4 H atoms (1.01 amu_

1 H atom) Determine the molecular mass.

= 12.01 amu + 4.04 amu = 16.05 amu= 16.05 g/mol Express the molecular mass as g/mol

to arrive at the molar mass.

Determine the number of moles of methane.

2.00 kg (1000 g_1 kg ) = 2.00 × 1 03 g Convert the mass from kg to g.

m_M=

2.00 × 1 03 g_16.05 g/mol

= 125 mol Divide mass by molar mass to determine the number of moles.

Use the molar volume to determine the volume of methane at STP.

V = 125 mol = 22.4 L_1 mol

= 2.80 × 103 L Use the molar volume, 22.4 L/mol, to convert from moles to the volume.

3 Evaluate the AnswerThe amount of methane present is much more than 1 mol, so you should expecta large volume, which is in agreement with the answer. The unit is liters, a volumeunit, and there are three significant figures.

PRACTICE Problems Extra Practice Page 984 and glencoe.com

20. What size container do you need to hold 0.0459 mol of N2 gas at STP?

21. How much carbon dioxide gas, in grams, is in a 1.0-L balloon at STP?

22. What volume in milliliters will 0.00922 g of H2 gas occupy at STP?

23. What volume will 0.416 g of krypton gas occupy at STP?

24. Calculate the volume that 4.5 kg of ethylene gas ( C2H4) will occupy at STP.

25. Challenge A flexible plastic container contains 0.860 g of helium gas in a volume of 19.2 L. If 0.205 g of helium is removed at constant pressure and temperature, what will be the new volume?

Unit Conversionpage 957

Math Handbook

C13_S2_874637.indd 453 1/29/07 4:04:43 PM

Reading for Information xix

Reading for Information

As You ReadWithin each section you will find a tool to deepen your understanding and tools to check your understanding.

Source: Section 13.2, p. 452

Example Problems take you step-by-step to solve problems in chemistry. Reinforce the skills you’ve learned by working through the Practice Problems.

❯

• Ask yourself what is the BIG Idea ?

What is the MAIN Idea ?

• Relate the information in Chemistry: Matter and Change to other areas you have studied.

• Predict events or outcomes by using clues and information that you already know.

• Change your predictions as you read and gather new information.

OTHER READING SKILLS

Source: Section 13.2, p. 453

The Real-World Reading Link describes how the section’s content may relate to you. ❮

xx Reading for Information

Reading for Information

Follow up your reading with a summary and assessment of the material to evaluate if you understood the text.

After You ReadNonpolar gas

Polar gas Force of attraction

Section 13.213.2 Assessment

Section 13.2 • The Ideal Gas Law 459Self-Check Quiz glencoe.com

Polarity and size of particles The nature of the particles making up a gas also affects how ideally the gas behaves. For example, polar gas molecules, such as water vapor, generally have larger attractive forces between their particles than nonpolar gases, such as helium. The oppo-sitely charged ends of polar molecules are pulled together through electrostatic forces, as shown in Figure 13.9. Therefore, polar gases do not behave as ideal gases. Also, the particles of gases composed of larger nonpolar molecules, such as butane ( C 4 H 10 ), occupy more actual vol-ume than an equal number of smaller gas particles in gases such as helium (He). Therefore, larger gas particles tend to exhibit a greater departure from ideal behavior than do smaller gas particles.

Section Summary◗ ◗ Avogadro’s principle states that equal

volumes of gases at the same pres-sure and temperature contain equal numbers of particles.

◗ ◗ The ideal gas law relates the amount of a gas present to its pressure, tem-perature, and volume.

◗ ◗ The ideal gas law can be used to find molar mass if the mass of the gas is known, or the density of the gas if its molar mass is known.

◗ ◗ At very high pressures and very low temperatures, real gases behave differently than ideal gases.

31. MAIN Idea Explain why Avogadro’s principle holds true for gases that have small particles and for gases that have large particles.

32. State the equation for the ideal gas law.

33. Analyze how the ideal gas law applies to real gases using the kinetic-molecular theory.

34. Predict the conditions under which a real gas might deviate from ideal behavior.

35. List common units for each variable in the ideal gas law.

36. Calculate A 2.00-L flask is filled with propane gas ( C 3 H 8 ) at a pressure of 1.00 atm and a temperature of -15.0°C. What is the mass of the propane in the flask?

37. Make and Use Graphs For every 6°C drop in temperature, the air pressure in a car’s tires goes down by about 1 psi (14.7 psi = 1.00 atm). Make a graph illustrating the change in tire pressure from 20°C to -20°C (assume 30.0 psi at 20°C).

Helium Water vapor

■ Figure 13.9 In a nonpolar gas, there is minimal attraction between particles. However, polar gases, such as water vapor, experi-ence forces of attraction between particles.Infer Assuming the volume of the particles is negligible, how will the measured pressure for a sample of gas that experiences significant intermolecular attractive forces compare to the pressure predicted by the ideal gas law?

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Source: Chapter 13, p. 459

At the end of each chapter you will find a Study Guide. The chapter’s vocabulary terms as well as key concepts are listed here. Use this guide for review and to check your comprehension.

❮

Chapter 13 • Study Guide 467Vocabulary PuzzleMaker glencoe.com

Download quizzes, key terms, and flash cards from glencoe.com.

BIG Idea Gases respond in predictable ways to pressure, temperature, volume, and changes in number of particles.

Section 13.1Section 13.1 The Gas Laws

MAIN Idea For a fixed amount of gas, a change in one variable—pressure, temperature, or volume—affects the other two.

Vocabulary• absolute zero (p. 445)• Boyle’s law (p. 442)• Charles’s law (p. 445)• combined gas law (p. 449)• Gay-Lussac’s law (p. 447)

Key Concepts• Boyle’s law states that the volume of a fixed amount of gas is inversely proportional

to its pressure at constant temperature.

P 1 V 1 = P 2 V 2

• Charles’s law states that the volume of a fixed amount of gas is directly proportional to its kelvin temperature at constant pressure.

V 1

_ T 1

= V 2

_ T 2

• Gay-Lussac’s law states that the pressure of a fixed amount of gas is directly proportional to its kelvin temperature at constant volume.

P 1

_ T 1

= P 2

_ T 2

• The combined gas law relates pressure, temperature, and volume in a single statement.

P 1 V 1

_ T 1

= P 2 V 2

_ T 2

Section 13.2Section 13.2 The Ideal Gas Law

MAIN Idea The ideal gas law relates the number of particles to pressure, temperature, and volume.

Vocabulary• Avogadro’s principle (p. 452)• ideal gas constant (p. 454)• ideal gas law (R) (p. 454)• molar volume (p. 452)

Key Concepts• Avogadro’s principle states that equal volumes of gases at the same pressure and

temperature contain equal numbers of particles.

• The ideal gas law relates the amount of a gas present to its pressure, temperature, and volume.

PV = nRT

• The ideal gas law can be used to find molar mass if the mass of the gas is known, or the density of the gas if its molar mass is known.

M = mRT

_ PV

D = MP _

RT

• At very high pressures and very low temperatures, real gases behave differently than ideal gases.

Section 13.3Section 13.3 Gas Stoichiometry

MAIN Idea When gases react, the coefficients in the balanced chemical equation represent both molar amounts and relative volumes.

Key Concepts• The coefficients in a balanced chemical equation specify volume ratios for gaseous

reactants and products.

• The gas laws can be used along with balanced chemical equations to calculate the amount of a gaseous reactant or product in a reaction.

C13_CA_874637.indd 467 1/29/07 4:06:02 PM

• State the BIG Idea .

• Relate the MAIN Idea to the BIG Idea .

• Use your own words to explain what you read.

• Apply this information in other school subjects or at home.

• Identify sources you could use to find out more information about this topic.

OTHER WAYS TO REVIEW

Source: Chapter 13, p. 467

Each section concludes with an assessment. The assessment contains a summary and questions. The summary reviews the section’s key concepts while the questions test your understanding.

❯

Scavenger Hunt xxi

Chemistry: Matter and Change contains a wealth of information. Complete this fun activity so you will know where to look to learn as much as you can.

As you complete this scavenger hunt, either alone, with your teacher, or with others, you will quickly learn how Chemistry: Matter and Change is organized and how to get the most out of your reading and study time.

How many chapters are in this book?

On what page does the glossary begin? What glossary is online?

In what two areas can you find a listing of Laboratory

Safety Symbols?

If you want to find all the MiniLabs, Problem-Solving Labs, Data

Analysis Labs, and ChemLabs, where in the front do you look?

How can you quickly find the pages that have information about an

arson investigator?

What is the name of the table that summarizes the Key Concepts

of a chapter?

Where can you find reference tables? What are the page numbers?

On what page can you find the BIG Idea for Chapter 1? On what

pages can you find the MAIN Ideas for Chapter 2?

Where can you find information on hydrogen?

Name four activities that are found at .

What study tool shown at the beginning of a chapter can

you make from notebook paper?

Where do you go to view the ?

and

are two types of chapter features. What are the other two types?