Interactive Media Contents in Mastering Chemistry
KEY CONCEPT VIDEOS (KCVs)
1.1 Atoms and Molecules
1.3 Classifying Matter
1.6 Units and Significant Figures
1.7 Significant Figures in Calculations
1.8 Solving Chemical Problems
2.3 Atomic Theory
2.6 Subatomic Particles and Isotope Symbols
2.7 The Periodic Law and the Periodic Table
2.9 The Mole Concept
3.5 Naming Ionic Compounds
3.6 Naming Molecular Compounds
4.2 Writing and Balancing Chemical Equations
4.3 Reaction Stoichiometry
4.4 Limiting Reactant, Theoretical Yield, and Percent Yield
5.2 Solution Concentration
5.5 Reactions in Solutions
6.3 Simple Gas Laws and Ideal Gas Law
6.6 Mixtures of Gases and Partial Pressures
6.8 Kinetic Molecular Theory
7.3 The First Law of Thermodynamics
7.4 Heat Capacity
7.6 The Change in Enthalpy for a Chemical Reaction
7.9 Determining the Enthalpy of Reaction from Standard Enthalpies of Formation
8.2 The Nature of Light
8.4 The Wave Nature of Matter
8.5A Quantum Mechanics and the Atom: Orbitals and Quantum Numbers
8.5B Atomic Spectroscopy
9.3 Electron Configurations
9.4 Writing an Electron Configuration Based on an Element’s Position on the Periodic Table
9.6 Periodic Trends in the Size of Atoms and Effective Nuclear Charge
10.5 The Lewis Model for Chemical Bonding
10.6 Electronegativity and Bond Polarity
10.7 Writing Lewis Structures for Molecular Compounds
10.8 Resonance and Formal Charge
10.9 Exceptions to the Octet Rule and Expanded Octets
11.2 VSEPR Theory
11.3 VSEPR Theory: The Effect of Lone Pairs
11.5 Molecular Shape and Polarity
11.6 Valence Bond Theory
11.7 Valence Bond Theory: Hybridization
12.3 Intermolecular Forces
12.5 Vaporization and Vapor Pressure
12.7 Heating Curve for Water
12.8 Phase Diagrams
13.3 Unit Cells: Simple Cubic, Body-Centered Cubic, and Face-Centered Cubic
14.4 Solution Equilibrium and the Factors Affecting Solubility
14.5 Solution Concentration: Molarity, Molality, Parts by Mass and Volume, Mole Fraction
14.6 Colligative Properties
15.2 The Rate of a Chemical Reaction
15.3 The Rate Law for a Chemical Reaction
15.4 The Integrated Rate Law
15.5 The Effect of Temperature on Reaction Rate
15.6 Reaction Mechanisms
16.3 The Equilibrium Constant
16.7 The Reaction Quotient
16.8 Finding Equilibrium Concentrations from Initial Concentrations
16.9 Le Châtelier’s Principle
17.3 Definitions of Acids and Bases
17.4 Acid Strength and the Acid Ionization Constant
17.5 The pH Scale
17.6 Finding the [H3O + ] and pH of Strong and Weak Acid Solutions
17.8 The Acid–Base Properties of Ions and Salts
18.2A Buffers
18.2B Finding pH and pH Changes in Buffer Solutions
18.4A The Titration of a Strong Acid with a Strong Base
18.4B The Titration of a Weak Acid and a Strong Base
19.3 Entropy and the Second Law of Thermodynamics
19.6 The Effect of ∆H, ∆S, and T on Reaction Spontaneity
19.7 Standard Molar Entropies
20.3 Voltaic Cells
20.4 Standard Electrode Potentials
20.5 Cell Potential, Free Energy, and the Equilibrium Constant
21.3 Types of Radioactivity
INTERACTIVE WORKED EXAMPLES (IWEs)
1.5 Determining the Number of Significant Figures in a Number
1.6 Significant Figures in Calculations
1.8 Unit Conversion
1.9 Unit Conversions Involving Units Raised to a Power
1.10 Density as a Conversion Factor
1.12 Problems with Equations
2.3 Atomic Numbers, Mass Numbers, and Isotope Symbols
2.5 Atomic Mass
2.8 The Mole Concept—Converting between Mass and Number of Atoms
2.9 The Mole Concept
3.3 Writing Formulas for Ionic Compounds
3.11 Using the Nomenclature Flowchart to Name Compounds
3.13 The Mole Concept—Converting between Mass and Number of Molecules
3.15 Using Mass Percent Composition as a Conversion Factor
3.16 Chemical Formulas as Conversion Factors
3.18 Obtaining an Empirical Formula from Experimental Data
3.21 Determining an Empirical Formula from Combustion Analysis
4.2 Balancing Chemical Equations
4.3 Balancing Chemical Equations Containing a Polyatomic Ion
4.4 Stoichiometry
4.6 Limiting Reactant and Theoretical Yield
5.1 Calculating Solution Concentration
5.2 Using Molarity in Calculations
5.3 Solution Dilution
5.4 Solution Stoichiometry
5.5 Predicting Whether an Ionic Compound Is Soluble
5.6 Writing Equations for Precipitation Reactions
5.9 Writing Equations for Acid–Base Reactions Involving a Strong Acid
5.11 Acid–Base Titration
5.13 Assigning Oxidation States
6.5 Ideal Gas Law I
6.7 Density
6.8 Molar Mass of a Gas
6.10 Partial Pressures and Mole Fractions
6.11 Collecting Gases over Water
6.12 Gases in Chemical Reactions
6.15 Graham’s Law of Effusion
7.2 Temperature Changes and Heat Capacity
7.3 Thermal Energy Transfer
7.5 Measuring ∆ Erxn in a Bomb Calorimeter
7.7 Stoichiometry Involving ∆H
7.8 Measuring ∆ Hrxn in a Coffee-Cup Calorimeter
7.9 Hess’s Law
7.11 ∆ H° rxn and Standard Enthalpies of Formation
8.2 Photon Energy
8.3 Wavelength, Energy, and Frequency
8.5 Quantum Numbers I
8.7 Wavelength of Light for a Transition in the Hydrogen Atom
9.2 Writing Orbital Diagrams
9.4 Writing Electron Configurations from the Periodic Table
9.5 Atomic Size
9.6 Electron Configurations and Magnetic Properties for Ions
9.8 First Ionization Energy
10.4 Writing Lewis Structures
10.6 Writing Lewis Structures for Polyatomic Ions
10.7 Writing Resonance Structures
10.8 Assigning Formal Charges
10.9 Drawing Resonance Structures and Assigning Formal Charge for Organic Compounds
10.10 Writing Lewis Structures for Compounds Having Expanded Octets
10.11 Calculating ∆ Hrxn from Bond Energies
11.1 VSEPR Theory and the Basic Shapes
11.2 Predicting Molecular Geometries
11.4 Predicting the Shape of Larger Molecules
11.5 Determining Whether a Molecule Is Polar
11.8 Hybridization and Bonding Scheme
11.10 Molecular Orbital Theory
12.1 Dipole–Dipole Forces
12.2 Hydrogen Bonding
12.3 Using the Heat of Vaporization in Calculations
12.5 Using the Two-Point Form of the Clausius–Clapeyron Equation to Predict the Vapor Pressure at a Given Temperature
13.3 Relating Unit Cell Volume, Edge Length, and Atomic Radius
13.4 Relating Density to Crystal Structure
14.2 Henry’s Law
14.3 Using Parts by Mass in Calculations
14.4 Calculating Concentrations
14.5 Converting between Concentration Units
14.6 Calculating the Vapor Pressure of a Solution Containing a Nonelectrolyte and Nonvolatile Solute
14.9 Boiling Point Elevation
14.12 Calculating the Vapor Pressure of a Solution Containing an Ionic Solute
15.1 Expressing Reaction Rates
15.2 Determining the Order and Rate Constant of a Reaction
15.4 The First-Order Integrated Rate Law: Determining the Concentration of a Reactant at a Given Time
15.8 Using the Two-Point Form of the Arrhenius Equation
15.9 Reaction Mechanisms
16.1 Expressing Equilibrium Constants for Chemical Equations
16.3 Relating K p and K c
16.5 Finding Equilibrium Constants from Experimental Concentration Measurements
16.7 Predicting the Direction of a Reaction by Comparing Q and K
16.8 Finding Equilibrium Concentrations When You Know the Equilibrium Constant and All but One of the Equilibrium Concentrations of the Reactants and Products
16.9 Finding Equilibrium Concentrations from Initial Concentrations and the Equilibrium Constant
16.12 Finding Equilibrium Concentrations from Initial Concentrations in Cases with a Small Equilibrium Constant
16.14 The Effect of a Concentration Change on Equilibrium
17.1 Identifying Brønsted–Lowry Acids and Bases and Their Conjugates
17.3 Calculating pH from [H3O + ] or [OH - ]
17.5 Finding the [H3O + ] of a Weak Acid Solution
17.7 Finding the pH of a Weak Acid Solution in Cases Where the x is small Approximation Does Not Work
17.8 Finding the Equilibrium Constant from pH
17.9 Finding the Percent Ionization of a Weak Acid
17.12 Finding the [OH - ] and pH of a Weak Base Solution
17.14 Determining the pH of a Solution Containing an Anion Acting as a Base
17.16 Determining the Overall Acidity or Basicity of Salt Solutions
18.2 Calculating the pH of a Buffer Solution as an Equilibrium Problem and with the Henderson–Hasselbalch Equation
18.3 Calculating the pH Change in a Buffer Solution after the Addition of a Small Amount of Strong Acid or Base
18.4 Using the Henderson–Hasselbalch Equation to Calculate the pH of a Buffer Solution Composed of a Weak Base and Its Conjugate Acid
18.6 Strong Acid–Strong Base Titration pH Curve
18.7 Weak Acid–Strong Base Titration pH Curve
18.8 Calculating Molar Solubility from K sp
18.12 Predicting Precipitation Reactions by Comparing Q and Ksp
19.2 Calculating ∆S for a Change of State
19.3 Calculating Entropy Changes in the Surroundings
19.4 Calculating Gibbs Free Energy Changes and Predicting Spontaneity from ∆H and ∆S
19.5 Calculating Standard Entropy Changes ( ∆ S ° rxn)
19.6 Calculating the Standard Change in Free Energy for a Reaction Using ∆ G
19.10 Calculating ∆ Grxn under Nonstandard Conditions
19.11 The Equilibrium Constant and ∆ G ° rxn
20.2 Half-Reaction Method of Balancing Aqueous Redox Equations in Acidic Solution
20.3 Balancing Redox Reactions Occurring in Basic Solution
20.4 Calculating Standard Potentials for Electrochemical Cells from Standard Electrode Potentials of the Half-Reactions
20.6 Relating ∆ G° and E ° cell
21.1 Writing Nuclear Equations for Alpha Decay
21.2 Writing Nuclear Equations for Beta Decay, Positron Emission, and Electron Capture
21.4 Radioactive Decay Kinetics
21.5 Radiocarbon Dating
1 Matter, Measurement, and Problem Solving 42
1.1 Atoms and Molecules 43
1.2 The Scientific Approach to Knowledge 45
THE NATURE OF SCIENCE Thomas S. Kuhn and Scientific Revolutions 47
1.3 The Classification of Matter 47
The States of Matter: Solid, Liquid, and Gas 48
Classifying Matter by Composition: Elements, Compounds, and Mixtures 49 Separating Mixtures 50
1.4 Physical and Chemical Changes and Physical and Chemical Properties 51
1.5 Energy: A Fundamental Part of Physical and Chemical Change 54
1.6 The Units of Measurement 55
Standard Units 56 The Meter: A Measure of Length 56 The Kilogram: A Measure of Mass 56
The Second: A Measure of Time 56 The Kelvin: A Measure of Temperature 57 Prefix Multipliers 59
Derived Units: Volume and Density 59 Volume 60
Density 60 Calculating Density 61
CHEMISTRY AND MEDICINE Bone Density 62
1.7 The Reliability of a Measurement 62
Counting Significant Figures 64 Exact Numbers 64 Significant Figures in Calculations 65 Precision and Accuracy 67
CHEMISTRY IN YOUR DAY Integrity in Data Gathering 68
1.8 Solving Chemical Problems 68
Converting from One Unit to Another 68 General Problem-Solving Strategy 70 Units Raised to a Power 72 Order-of-Magnitude Estimations 73 Problems Involving an Equation 74
1.9 Analyzing and Interpreting Data 75
Identifying Patterns in Data 75 Interpreting Graphs 76
CHAPTER IN REVIEW Self-Assessment Quiz 78 Terms 79 Concepts 80 Equations and Relationships 80 Learning Outcomes 80
EXERCISES Review Questions 81 Problems by Topic 81
Cumulative Problems 85 Challenge Problems 87
Conceptual Problems 87 Questions for Group Work 88 Data Interpretation and Analysis 88 Answers to Conceptual Connections 89
2 Atoms and Elements 90
2.1 Brownian Motion: Atoms Confirmed 91
2.2 Early Ideas about the Building Blocks of Matter 93
2.3 Modern Atomic Theory and the Laws That Led to It 93
The Law of Conservation of Mass 93 The Law of Definite Proportions 94 The Law of Multiple Proportions 95 John Dalton and the Atomic Theory 96
CHEMISTRY IN YOUR DAY Atoms and Humans 96
2.4 The Discovery of the Electron 97 Cathode Rays 97 Millikan’s Oil Drop Experiment: The Charge of the Electron 98
2.5 The Structure of the Atom 99
2.6 Subatomic Particles: Protons, Neutrons, and Electrons in Atoms 101
Elements: Defined by Their Numbers of Protons 102 Isotopes: When the Number of Neutrons Varies 103 Ions: Losing and Gaining Electrons 105
CHEMISTRY IN YOUR DAY Where Did Elements Come From? 106
2.7 Finding Patterns: The Periodic Law and the Periodic Table 107
Modern Periodic Table Organization 108 Ions and the Periodic Table 110
CHEMISTRY AND MEDICINE The Elements of Life 111
2.8 Atomic Mass: The Average Mass of an Element’s Atoms 111
Mass Spectrometry: Measuring the Mass of Atoms and Molecules 112
CHEMISTRY IN YOUR DAY Evolving Atomic Masses 114
2.9 Molar Mass: Counting Atoms by Weighing Them 115
The Mole: A Chemist’s “Dozen” 115 Converting between Number of Moles and Number of Atoms 116 Converting between Mass and Amount (Number of Moles) 117
CHAPTER IN REVIEW Self-Assessment Quiz 120 Terms 121 Concepts 122 Equations and Relationships 122 Learning Outcomes 123
EXERCISES Review Questions 123 Problems by Topic 124
Cumulative Problems 127 Challenge Problems 128 Conceptual Problems 129 Questions for Group Work 130 Data Interpretation and Analysis 130 Answers to Conceptual Connections 131
3 Molecules and Compounds 132
3.1 Hydrogen, Oxygen, and Water 133
3.2 Chemical Bonds 135 Ionic Bonds 135 Covalent Bonds 136
3.3 Representing Compounds: Chemical Formulas and Molecular Models 136 Types of Chemical Formulas 136 Molecular Models 138
3.4 An Atomic-Level View of Elements and Compounds 138
3.5 Ionic Compounds: Formulas and Names 142 Writing Formulas for Ionic Compounds 142 Naming Ionic Compounds 143 Naming Binary Ionic Compounds Containing a Metal That Forms Only One Type of Cation 144 Naming Binary Ionic Compounds Containing a Metal That Forms More Than One Kind of Cation 145 Naming Ionic Compounds Containing Polyatomic Ions 146 Hydrated Ionic Compounds 147
3.6 Molecular Compounds: Formulas and Names 148 Naming Molecular Compounds 148 Naming Acids 149 Naming Binary Acids 150 Naming Oxyacids 150 CHEMISTRY IN THE ENVIRONMENT Acid Rain 150
3.7 Summary of Inorganic Nomenclature 151
3.8 Formula Mass and the Mole Concept for Compounds 153 Molar Mass of a Compound 153 Using Molar Mass to Count Molecules by Weighing 153
3.9 Composition of Compounds 155
Mass Percent Composition as a Conversion Factor 156
Conversion Factors from Chemical Formulas 158
CHEMISTRY AND MEDICINE Methylmercury in Fish 160
3.10 Determining a Chemical Formula from Experimental Data 160
Determining Molecular Formulas for Compounds 162 Combustion Analysis 163
3.11 Organic Compounds 165
Hydrocarbons 166 Functionalized Hydrocarbons 167
CHAPTER IN REVIEW Self-Assessment Quiz 169 Terms 170 Concepts 170 Equations and Relationships 171 Learning Outcomes 171
EXERCISES Review Questions 171 Problems by Topic 172 Cumulative Problems 176 Challenge Problems 177 Conceptual Problems 177 Questions for Group Work 178 Data Interpretation and Analysis 178 Answers to Conceptual Connections 178
4 Chemical Reactions and
Chemical Quantities 180
4.1 Climate Change and the Combustion of Fossil Fuels 181
4.2 Writing and Balancing Chemical Equations 183
4.3 Reaction Stoichiometry: How Much Carbon Dioxide? 187
Making Pizza: The Relationships among Ingredients 187 Making Molecules: Mole-to-Mole Conversions 188 Making Molecules: Mass-to-Mass Conversions 188
4.4 Stoichiometric Relationships: Limiting Reactant, Theoretical Yield, Percent Yield, and Reactant in Excess 191
Calculating Limiting Reactant, Theoretical Yield, and Percent Yield 193 Calculating Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Reactant Masses 194
4.5 Three Examples of Chemical Reactions: Combustion, Alkali Metals, and Halogens 197 Combustion Reactions 197 Alkali Metal Reactions 198 Halogen Reactions 198
CHAPTER IN REVIEW Self-Assessment Quiz 200 Terms 201 Concepts 201 Equations and Relationships 201 Learning Outcomes 201
EXERCISES Review Questions 202 Problems by Topic 202 Cumulative Problems 205 Challenge Problems 206 Conceptual Problems 206 Questions for Group Work 207 Data Interpretation and Analysis 207 Answers to Conceptual Connections 207
5 Introduction to Solutions
and Aqueous Reactions 208
5.1 Molecular Gastronomy and the Spherified Cherry 209
5.2 Solution Concentration 210
Solution Concentration 210 Using Molarity in Calculations 212 Solution Dilution 213
5.3 Solution Stoichiometry 215
5.4 Types of Aqueous Solutions and Solubility 217 Electrolyte and Nonelectrolyte Solutions 217 The Solubility of Ionic Compounds 219
5.5 Precipitation Reactions 221
5.6 Representing Aqueous Reactions: Molecular, Ionic, and Net Ionic Equations 225
5.7 Acid–Base Reactions 227 Acid–Base Reactions 227 Acid–Base Titrations 231
5.8 Gas-Evolution Reactions 233
5.9 Oxidation–Reduction Reactions 235 Oxidation States 236 Identifying Redox Reactions 238 The Activity Series: Predicting Whether a Redox Reaction Is Spontaneous 240
CHEMISTRY IN YOUR DAY Bleached Blonde 241
CHAPTER IN REVIEW Self-Assessment Quiz 243 Terms 244 Concepts 244 Equations and Relationships 245 Learning Outcomes 245
EXERCISES Review Questions 246 Problems by Topic 246
Cumulative Problems 248 Challenge Problems 249 Conceptual Problems 249 Questions for Group Work 250 Data Interpretation and Analysis 250 Answers to Conceptual Connections 251
Gases 252
6.1 Supersonic Skydiving and the Risk of Decompression 253
6.2 Pressure: The Result of Molecular Collisions 254 Pressure Units 255 The Manometer: A Way to Measure Pressure in the Laboratory 256
CHEMISTRY AND MEDICINE Blood Pressure 257
6.3 The Simple Gas Laws: Boyle’s Law, Charles’s Law, and Avogadro’s Law 257 Boyle’s Law: Volume and Pressure 258 Charles’s Law: Volume and Temperature 260
CHEMISTRY IN YOUR DAY Extra-Long Snorkels 261 Avogadro’s Law: Volume and Amount (in Moles) 263
6.4 The Ideal Gas Law 264
6.5 Applications of the Ideal Gas Law: Molar Volume, Density, and Molar Mass of a Gas 267 Molar Volume at Standard Temperature and Pressure 267 Density of a Gas 268 Molar Mass of a Gas 269
6.6 Mixtures of Gases and Partial Pressures 270 Deep-Sea Diving and Partial Pressures 273 Collecting Gases over Water 275
6.7 Gases in Chemical Reactions: Stoichiometry Revisited 277 Molar Volume and Stoichiometry 278
ANALYZING AND INTERPRETING DATA Good News about Our Nation’s Air Quality 280
6.8 Kinetic Molecular Theory: A Model for Gases 280 How Kinetic Molecular Theory Explains Pressure and the Simple Gas Laws 281 Kinetic Molecular Theory and the Ideal Gas Law 282 Temperature and Molecular Velocities 284
6.9 Mean Free Path, Diffusion, and Effusion of Gases 287
6.10 Real Gases: The Effects of Size and Intermolecular Forces 288
The Effect of the Finite Volume of Gas Particles 289 The Effect of Intermolecular Forces 290 Van der Waals Equation 291 Real Gases 291
CHAPTER IN REVIEW Self-Assessment Quiz 292 Terms 293 Concepts 293 Equations and Relationships 294 Learning Outcomes 294
EXERCISES Review Questions 295 Problems by Topic 295 Cumulative Problems 299 Challenge Problems 301 Conceptual Problems 302 Questions for Group Work 302 Data Interpretation and Analysis 302 Answers to Conceptual Connections 303
7 Thermochemistry 304
7.1 Chemical Hand Warmers 305
7.2 The Nature of Energy: Key Definitions 306 Types of Energy 306 Energy Conservation and Energy Transfer 307 Units of Energy 307
7.3 The First Law of Thermodynamics: There Is No Free Lunch 309 Internal Energy 309
CHEMISTRY IN YOUR DAY Redheffer’s Perpetual Motion Machine 309 Heat and Work 312
7.4 Quantifying Heat and Work 314
Heat 314 Temperature Changes and Heat Capacity 314 Thermal Energy Transfer 316 Work: Pressure–Volume Work 318
7.5 Measuring ∆E for Chemical Reactions: Constant-Volume Calorimetry 320
7.6 Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure 323 Exothermic and Endothermic Processes: A Molecular View 325 Stoichiometry Involving ∆H: Thermochemical Equations 325
7.7 Constant-Pressure Calorimetry: Measuring ∆ Hrxn 327
7.8 Relationships Involving ∆ Hrxn 328
7.9 Determining Enthalpies of Reaction from Standard Enthalpies of Formation 331 Standard States and Standard Enthalpy Changes 331 Calculating the Standard Enthalpy Change for a Reaction 333
7.10 Energy Use and the Environment 336 Energy Consumption 336 Environmental Problems Associated with Fossil Fuel Use 337 Air Pollution 337 Global Climate Change 338 CHEMISTRY IN THE ENVIRONMENT Renewable Energy 340
CHAPTER IN REVIEW Self-Assessment Quiz 341 Terms 342 Concepts 342 Equations and Relationships 343 Learning Outcomes 343
EXERCISES Review Questions 344 Problems by Topic 344 Cumulative Problems 348 Challenge Problems 349 Conceptual Problems 350 Questions for Group Work 350 Data Interpretation and Analysis 351 Answers to Conceptual Connections 351
8 The Quantum-Mechanical Model of the Atom 352
8.1 Schrödinger’s Cat 353
8.2 The Nature of Light 354
The Wave Nature of Light 355 The Electromagnetic Spectrum 357
CHEMISTRY AND MEDICINE Radiation Treatment for Cancer 359 Interference and Diffraction 359 The Particle Nature of Light 360
8.3 Atomic Spectroscopy and the Bohr Model 364
CHEMISTRY IN YOUR DAY Atomic Spectroscopy, a Bar Code for Atoms 366
8.4 The Wave Nature of Matter: The de Broglie Wavelength, the Uncertainty Principle, and Indeterminacy 367
The de Broglie Wavelength 369 The Uncertainty Principle 370 Indeterminacy and Probability Distribution Maps 371
8.5 Quantum Mechanics and the Atom 373 Solutions to the Schrödinger Equation for the Hydrogen Atom 373 Atomic Spectroscopy Explained 376
8.6 The Shapes of Atomic Orbitals 379
s Orbitals (l = 0) 379 p Orbitals (I = 1) 382
d Orbitals (I = 2) 382 f Orbitals (I = 3) 382
The Phase of Orbitals 383 The Shape of Atoms 384
CHAPTER IN REVIEW Self-Assessment Quiz 384 Terms 385 Concepts 385 Equations and Relationships 386 Learning Outcomes 386
EXERCISES Review Questions 386 Problems by Topic 387 Cumulative Problems 388 Challenge Problems 389 Conceptual Problems 390 Questions for Group Work 390 Data Interpretation and Analysis 391 Answers to Conceptual Connections 391
9 Periodic Properties of the Elements 392
9.1 Nerve Signal Transmission 393
9.2 The Development of the Periodic Table 394
9.3 Electron Configurations: How Electrons Occupy Orbitals 395
Electron Spin and the Pauli Exclusion Principle 396 Sublevel Energy Splitting in Multielectron Atoms 396 Coulomb’s Law 397 Shielding 398 Penetration 398 Electron Spatial Distributions and Sublevel Splitting 398 Electron Configurations for Multielectron Atoms 400
9.4 Electron Configurations, Valence Electrons, and the Periodic Table 403
Orbital Blocks in the Periodic Table 404 Writing an Electron Configuration for an Element from Its Position in the Periodic Table 405 The Transition and Inner Transition Elements 406
9.5 The Explanatory Power of the Quantum-Mechanical Model 407
9.6 Periodic Trends in the Size of Atoms and Effective Nuclear Charge 408 Effective Nuclear Charge 410 Atomic Radii and the Transition Elements 411
9.7 Ions: Electron Configurations, Magnetic Properties, Ionic Radii, and Ionization Energy 413
Electron Configurations and Magnetic Properties of Ions 413 Ionic Radii 415 Ionization Energy 417 Trends in First Ionization Energy 417 Exceptions to Trends in First Ionization Energy 419 Trends in Second and Successive Ionization Energies 420
9.8 Electron Affinities and Metallic Character 421 Electron Affinity 421 Metallic Character 422
9.9 Periodic Trends Summary 425
CHAPTER IN REVIEW Self-Assessment Quiz 425 Terms 426 Concepts 426 Equations and Relationships 427 Learning Outcomes 427
EXERCISES Review Questions 428 Problems by Topic 429 Cumulative Problems 430 Challenge Problems 431 Conceptual Problems 432 Questions for Group Work 432 Data Interpretation and Analysis 433 Answers to Conceptual Connections 433
10 Chemical Bonding I: The Lewis Model
434
10.1 Bonding Models and AIDS Drugs 435
10.2 Types of Chemical Bonds 436
10.3 Representing Valence Electrons with Dots 438
10.4 Ionic Bonding: Lewis Symbols and Lattice Energies 439
Ionic Bonding and Electron Transfer 439 Lattice Energy: The Rest of the Story 440 The Born–Haber Cycle 440 Trends in Lattice Energies: Ion Size 443 Trends in Lattice Energies: Ion Charge 443 Ionic Bonding: Models and Reality 444
CHEMISTRY AND MEDICINE Ionic Compounds in Medicine 445
10.5 Covalent Bonding: Lewis Structures 446
Single Covalent Bonds 446 Double and Triple Covalent Bonds 446 Covalent Bonding: Models and Reality 447
10.6 Electronegativity and Bond Polarity 448
Electronegativity 449 Bond Polarity, Dipole Moment, and Percent Ionic Character 450
10.7 Lewis Structures of Molecular Compounds and Polyatomic Ions 452
Writing Lewis Structures for Molecular Compounds 452
Writing Lewis Structures for Polyatomic Ions 454
10.8 Resonance and Formal Charge 454
Resonance 454 Formal Charge 456
10.9 Exceptions to the Octet Rule: Odd-Electron Species, Incomplete Octets, and Expanded Octets 459
Odd-Electron Species 460 Incomplete Octets 460
CHEMISTRY IN THE ENVIRONMENT Free Radicals and the Atmospheric Vacuum Cleaner 461
Expanded Octets 462
10.10 Bond Energies and Bond Lengths 464
Bond Energy 464 Using Average Bond Energies to Estimate Enthalpy Changes for Reactions 465 Bond Lengths 466
10.11 Bonding in Metals: The Electron Sea Model 467
CHEMISTRY IN THE ENVIRONMENT The Lewis Structure of Ozone 468
CHAPTER IN REVIEW Self-Assessment Quiz 469 Terms 470 Concepts 470 Equations and Relationships 471 Learning Outcomes 471
EXERCISES Review Questions 472 Problems by Topic 472 Cumulative Problems 474 Challenge Problems 476 Conceptual Problems 476 Questions for Group Work 476 Data Interpretation and Analysis 477 Answers to Conceptual Connections 477
11 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 478
11.1 Morphine: A Molecular Imposter 479
11.2 VSEPR Theory: The Five Basic Shapes 480
Two Electron Groups: Linear Geometry 481
Three Electron Groups: Trigonal Planar Geometry 481
Four Electron Groups: Tetrahedral Geometry 481
Five Electron Groups: Trigonal Bipyramidal Geometry 483
Six Electron Groups: Octahedral Geometry 483
11.3 VSEPR Theory: The Effect of Lone Pairs 484
Four Electron Groups with Lone Pairs 484 Five Electron Groups with Lone Pairs 486 Six Electron Groups with Lone Pairs 487
11.4 VSEPR Theory: Predicting Molecular Geometries 489
Representing Molecular Geometries on Paper 491 Predicting the Shapes of Larger Molecules 491
11.5 Molecular Shape and Polarity 492 Vector Addition 494
CHEMISTRY IN YOUR DAY How Soap Works 496
11.6 Valence Bond Theory: Orbital Overlap as a Chemical Bond 497
11.7 Valence Bond Theory: Hybridization of Atomic Orbitals 499 sp3 Hybridization 500 sp2 Hybridization and Double Bonds 502
CHEMISTRY IN YOUR DAY The Chemistry of Vision 506 sp Hybridization and Triple Bonds 506 sp3d and sp3d 2 Hybridization 508 Writing Hybridization and Bonding Schemes 509
11.8 Molecular Orbital Theory: Electron Delocalization 512 Linear Combination of Atomic Orbitals (LCAOs) 513 Period Two Homonuclear Diatomic Molecules 517 Second-Period Heteronuclear Diatomic Molecules 522 Polyatomic Molecules 524
CHAPTER IN REVIEW Self-Assessment Quiz 525 Terms 526 Concepts 526 Equations and Relationships 526 Learning Outcomes 527
EXERCISES Review Questions 527 Problems by Topic 528 Cumulative Problems 530 Challenge Problems 532 Conceptual Problems 533 Questions for Group Work 533 Data Interpretation and Analysis 534 Answers to Conceptual Connections 534
12 Liquids, Solids, and Intermolecular Forces 536
12.1 Water, No Gravity 537
12.2 Solids, Liquids, and Gases: A Molecular Comparison 538
Differences between States of Matter 538
Changes between States 540
12.3 Intermolecular Forces: The Forces That Hold Condensed States Together 541
Dispersion Force 542 Dipole–Dipole Force 544
Hydrogen Bonding 547 Ion–Dipole Force 549
CHEMISTRY AND MEDICINE Hydrogen Bonding in DNA 550
12.4 Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action 551
Surface Tension 551 Viscosity 553
CHEMISTRY IN YOUR DAY Viscosity and Motor Oil 553 Capillary Action 553
12.5 Vaporization and Vapor Pressure 554
The Process of Vaporization 554 The Energetics of Vaporization 556 Vapor Pressure and Dynamic Equilibrium 557 Temperature Dependence of Vapor Pressure and Boiling Point 559 The Clausius–Clapeyron Equation 560 The Critical Point: The Transition to an Unusual State of Matter 563
12.6 Sublimation and Fusion 564
Sublimation 564 Fusion 565 Energetics of Melting and Freezing 565
12.7 Heating Curve for Water 566
12.8 Phase Diagrams 569
The Major Features of a Phase Diagram 569 Navigation within a Phase Diagram 570 The Phase Diagrams of Other Substances 571
12.9 Water: An Extraordinary Substance 571
CHEMISTRY IN THE ENVIRONMENT Water Pollution 573
CHAPTER IN REVIEW Self-Assessment Quiz 573 Terms 574 Concepts 574 Equations and Relationships 575 Learning Outcomes 575
EXERCISES Review Questions 576 Problems by Topic 576 Cumulative Problems 579 Challenge Problems 579 Conceptual Problems 580 Questions for Group Work 580 Data Interpretation and Analysis 581 Answers to Conceptual Connections 581
Solids and Modern Materials
582
13.1 Friday Night Experiments: The Discovery of Graphene 583
13.2 X-Ray Crystallography 584
13.3 Unit Cells and Basic Structures 587
Cubic Unit Cells 587 Closest-Packed Structures 593
13.4 The Fundamental Types of Crystalline Solids 594
Molecular Solids 595
CHEMISTRY IN YOUR DAY Chocolate, An Edible Material 596
Ionic Solids 597 Atomic Solids 597
13.5 The Structures of Ionic Solids 598
13.6 Network Covalent Atomic Solids: Carbon and Silicates 600
Carbon 600 Silicates 603
13.7 Ceramics, Cement, and Glass 603
Ceramics 603 Cement 604 Glass 605
13.8 Semiconductors and Band Theory 605
Molecular Orbitals and Energy Bands 605 Doping: Controlling the Conductivity of Semiconductors 607
13.9 Polymers and Plastics 607
CHEMISTRY IN YOUR DAY Kevlar 610
CHAPTER IN REVIEW Self-Assessment Quiz 611 Terms 612 Concepts 612 Equations and Relationships 613 Learning Outcomes 613
EXERCISES Review Questions 613 Problems by Topic 614 Cumulative Problems 617 Challenge Problems 618 Conceptual Problems 618 Questions for Group Work 618 Data Interpretation and Analysis 619 Answers to Conceptual Connections 619
14 Solutions 620
14.1 Thirsty Solutions: Why You Shouldn’t Drink Seawater 621
14.2 Types of Solutions and Solubility 623
Nature’s Tendency toward Mixing: Entropy 624 The Effect of Intermolecular Forces 624
14.3 Energetics of Solution Formation 628
Energy Changes in Solution Formation 628 Aqueous Solutions and Heats of Hydration 630
14.4 Solution Equilibrium and Factors Affecting Solubility 631
The Temperature Dependence of the Solubility of Solids 633 Factors Affecting the Solubility of Gases in Water 633
14.5 Expressing Solution Concentration 636
CHEMISTRY IN THE ENVIRONMENT Lake Nyos 636 Molarity 637 Molality 638 Parts by Mass and Parts by Volume 638 Using Parts by Mass (or Parts by Volume) in Calculations 639 Mole Fraction and Mole Percent 640
CHEMISTRY IN THE ENVIRONMENT The Dirty Dozen 640
14.6 Colligative Properties: Vapor Pressure
Lowering, Freezing Point Depression, Boiling Point Elevation, and Osmotic Pressure 643
Vapor Pressure Lowering 644 Vapor Pressures of Solutions Containing a Volatile (Nonelectrolyte) Solute 647 Freezing Point Depression and Boiling Point Elevation 650
CHEMISTRY IN YOUR DAY Antifreeze in Frogs 653
Osmotic Pressure 653
14.7 Colligative Properties of Strong Electrolyte
Solutions 655 Strong Electrolytes and Vapor Pressure 656
Colligative Properties and Medical Solutions 657
14.8 Colloids 658
CHAPTER IN REVIEW Self-Assessment Quiz 661 Terms 662 Concepts 662 Equations and Relationships 663 Learning Outcomes 663
EXERCISES Review Questions 664 Problems by Topic 665 Cumulative Problems 668 Challenge Problems 669 Conceptual Problems 670 Questions for Group Work 670 Data Interpretation and Analysis 671 Answers to Conceptual Connections 671
15 Chemical Kinetics 672
15.1 Catching Lizards 673
15.2 The Rate of a Chemical Reaction 674 Definition of Reaction Rate 674 Measuring Reaction Rates 678
15.3 The Rate Law: The Effect of Concentration on Reaction Rate 679
The Three Common Reaction Orders (n = 0, 1, and 2) 679
Determining the Order of a Reaction 680 Reaction Order for Multiple Reactants 682
15.4 The Integrated Rate Law: The Dependence of Concentration on Time 684
The Integrated Rate Law 684 The Half-Life of a Reaction 688
15.5 The Effect of Temperature on Reaction Rate 692
The Arrhenius Equation 692 The Activation Energy, Frequency Factor, and Exponential Factor 693 Arrhenius Plots: Experimental Measurements of the Frequency Factor and the Activation Energy 694 The Collision Model: A Closer Look at the Frequency Factor 697
15.6 Reaction Mechanisms 698 Rate Laws for Elementary Steps 699 Rate-Determining Steps and Overall Reaction Rate Laws 700 Mechanisms with a Fast Initial Step 701
15.7 Catalysis 703
Homogeneous and Heterogeneous Catalysis 705 Enzymes: Biological Catalysts 706
CHEMISTRY AND MEDICINE Enzyme Catalysis and the Role of Chymotrypsin in Digestion 708
CHAPTER IN REVIEW Self-Assessment Quiz 709 Terms 711 Concepts 711 Equations and Relationships 712 Learning Outcomes 712
EXERCISES Review Questions 712 Problems by Topic 713
Cumulative Problems 718 Challenge Problems 720 Conceptual Problems 721 Questions for Group Work 722 Data Interpretation and Analysis 722 Answers to Conceptual Connections 723
16 Chemical Equilibrium
724
16.1 Fetal Hemoglobin and Equilibrium 725
16.2 The Concept of Dynamic Equilibrium 727
16.3 The Equilibrium Constant (K) 730
Expressing Equilibrium Constants for Chemical Reactions 730
The Significance of the Equilibrium Constant 731
CHEMISTRY AND MEDICINE Life and Equilibrium 732 Relationships between the Equilibrium Constant and the Chemical Equation 733
16.4 Expressing the Equilibrium Constant in Terms of Pressure 734
Relationship Between Kp and Kc 735 Units of K 736
16.5 Heterogeneous Equilibria: Reactions Involving Solids and Liquids 737
16.6 Calculating the Equilibrium Constant from Measured Equilibrium Concentrations 738
16.7 The Reaction Quotient: Predicting the Direction of Change 741
16.8 Finding Equilibrium Concentrations 743
Finding Equilibrium Concentrations from the Equilibrium Constant and All but One of the Equilibrium Concentrations of the Reactants and Products 744 Finding Equilibrium Concentrations from the Equilibrium Constant and Initial Concentrations or Pressures 745 Simplifying Approximations in Working Equilibrium Problems 749
16.9 Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances 753
The Effect of a Concentration Change on Equilibrium 754 The Effect of a Volume (or Pressure) Change on Equilibrium 756 The Effect of a Temperature Change on Equilibrium 758
CHAPTER IN REVIEW Self-Assessment Quiz 760 Terms 761 Concepts 761 Equations and Relationships 762 Learning Outcomes 762
EXERCISES Review Questions 763 Problems by Topic 764
Cumulative Problems 767 Challenge Problems 769 Conceptual Problems 769 Questions for Group Work 770 Data Interpretation and Analysis 770 Answers to Conceptual Connections 771
17 Acids and Bases 772
17.1 Heartburn 773
17.2 The Nature of Acids and Bases 774
17.3 Definitions of Acids and Bases 776 The Arrhenius Definition 776 The Brønsted–Lowry Definition 777
17.4 Acid Strength and the Acid Ionization Constant (Ka) 779
Strong Acids 779 Weak Acids 780 The Acid Ionization Constant (Ka) 781
17.5 Autoionization of Water and pH 782
The pH Scale: A Way to Quantify Acidity and Basicity 784 pOH and Other p Scales 785
CHEMISTRY AND MEDICINE Ulcers 786
17.6 Finding the [H3O + ] and pH of Strong and Weak Acid Solutions 787
Strong Acids 787 Weak Acids 787 Percent Ionization of a Weak Acid 792 Mixtures of Acids 793
17.7 Base Solutions 796
Strong Bases 796 Weak Bases 796
Finding the [OH - ] and pH of Basic Solutions 798
CHEMISTRY AND MEDICINE What’s in My Antacid? 800
17.8 The Acid–Base Properties of Ions and Salts 800 Anions as Weak Bases 801 Cations as Weak Acids 804
Classifying Salt Solutions as Acidic, Basic, or Neutral 805
17.9 Polyprotic Acids 807
Finding the pH of Polyprotic Acid Solutions 808 Finding the Concentration of the Anions for a Weak Diprotic Acid Solution 810
17.10 Acid Strength and Molecular Structure 812 Binary Acids 812 Oxyacids 813
17.11 Lewis Acids and Bases 814
Molecules That Act as Lewis Acids 814 Cations That Act as Lewis Acids 815
17.12 Acid Rain 815
Effects of Acid Rain 816 Acid Rain Legislation 817
CHAPTER IN REVIEW Self-Assessment Quiz 817 Terms 818 Concepts 818 Equations and Relationships 819 Learning Outcomes 820
EXERCISES Review Questions 820 Problems by Topic 821
Cumulative Problems 824 Challenge Problems 826 Conceptual Problems 826 Questions for Group Work 826 Data Interpretation and Analysis 826 Answers to Conceptual Connections 827
18 Aqueous Ionic Equilibrium 828
18.1 The Danger of Antifreeze 829
18.2 Buffers: Solutions That Resist pH Change 830
Calculating the pH of a Buffer Solution 832 The Henderson–Hasselbalch Equation 833 Calculating pH Changes in a Buffer Solution 836 The Stoichiometry
Calculation 836 The Equilibrium Calculation 836
Buffers Containing a Base and Its Conjugate Acid 840
18.3 Buffer Effectiveness: Buffer Range and Buffer Capacity 841
Relative Amounts of Acid and Base 841 Absolute Concentrations of the Acid and Conjugate Base 842
Buffer Range 843
CHEMISTRY AND MEDICINE Buffer Effectiveness in Human Blood 844
Buffer Capacity 844
18.4 Titrations and pH Curves 845
The Titration of a Strong Acid with a Strong Base 846
The Titration of a Weak Acid with a Strong Base 850
The Titration of a Weak Base with a Strong Acid 855
The Titration of a Polyprotic Acid 856
Indicators: pH-Dependent Colors 856
18.5 Solubility Equilibria and the Solubility
Product Constant 859
Ksp and Molar Solubility 859
CHEMISTRY IN YOUR DAY Hard Water 861
Ksp and Relative Solubility 862 The Effect of a Common Ion on Solubility 862 The Effect of pH on Solubility 864
18.6 Precipitation 865
Selective Precipitation 866
18.7 Qualitative Chemical Analysis 868
Group 1: Insoluble Chlorides 869 Group 2: AcidInsoluble Sulfides 869 Group 3: Base-Insoluble Sulfides and Hydroxides 870 Group 4: Insoluble
Phosphates 870 Group 5: Alkali Metals and NH4 + 870
18.8 Complex Ion Equilibria 871
The Effect of Complex Ion Equilibria on Solubility 873
The Solubility of Amphoteric Metal Hydroxides 874
CHAPTER IN REVIEW Self-Assessment Quiz 875 Terms 876 Concepts 876 Equations and Relationships 877 Learning Outcomes 877
EXERCISES Review Questions 878 Problems by Topic 879
Cumulative Problems 884 Challenge Problems 885 Conceptual Problems 885 Questions for Group Work 886
Data Interpretation and Analysis 886 Answers to Conceptual Connections 887
19 Free Energy and Thermodynamics 888
19.1 Cold Coffee and Dead Universes 889
19.2 Spontaneous and Nonspontaneous Processes 890
19.3 Entropy and the Second Law of Thermodynamics 892
Entropy 894 The Entropy Change upon the Expansion of an Ideal Gas 896
19.4 Entropy Changes Associated with State Changes 898
Entropy and State Change: The Concept 899 Entropy and State Changes: The Calculation 900
19.5 Heat Transfer and Changes in the Entropy of the Surroundings 902
The Temperature Dependence of ∆ Ssurr 903
Quantifying Entropy Changes in the Surroundings 903
19.6 Gibbs Free Energy 905
The Effect of ∆H, ∆S, and T on Spontaneity 906
19.7 Entropy Changes in Chemical Reactions:
Calculating ∆ S° rxn 909
Defining Standard States and Standard Entropy Changes 909 Standard Molar Entropies (S°) and the Third Law of Thermodynamics 909 Calculating the Standard Entropy Change ( ∆ S° rxn) for a Reaction 913
19.8 Free Energy Changes in Chemical Reactions:
Calculating ∆ G° rxn 913
Calculating Standard Free Energy Changes with ∆ G° rxn = ∆ H° rxn - T ∆ S° rxn 914
Calculating ∆ G° rxn with Tabulated Values of Free Energies of Formation 915
CHEMISTRY IN YOUR DAY Making a Nonspontaneous Process Spontaneous 917
Calculating ∆ G° rxn for a Stepwise Reaction from the Changes in Free Energy for Each of the Steps 917 Why Free Energy Is “Free” 918
19.9 Free Energy Changes for Nonstandard States:
The Relationship between ∆ G° rxn and ∆ Grxn 920
Standard versus Nonstandard States 920 The Free Energy Change of a Reaction under Nonstandard Conditions 920 Standard Conditions 920 Equilibrium Conditions 921 Other Nonstandard Conditions 922
19.10 Free Energy and Equilibrium: Relating ∆ G° rxn to the Equilibrium Constant (K) 923
The Relationship between ∆ G° rxn and K 923 The Temperature Dependence of the Equilibrium Constant 925
CHAPTER IN REVIEW Self-Assessment Quiz 926 Terms 927
Concepts 927 Equations and Relationships 928
Learning Outcomes 928
EXERCISES Review Questions 929 Problems by Topic 930
Cumulative Problems 933 Challenge Problems 934 Conceptual Problems 935 Questions for Group Work 935 Data
Interpretation and Analysis 936 Answers to Conceptual Connections 936
20 Electrochemistry 938
20.1 Lightning and Batteries 939
20.2 Balancing Oxidation–Reduction Equations 940
20.3 Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions 943
The Voltaic Cell 944 Current and Potential Difference 945 Anode, Cathode, and Salt Bridge 946 Electrochemical Cell Notation 947
20.4 Standard Electrode Potentials 947
Predicting the Spontaneous Direction of an Oxidation–Reduction Reaction 952 Predicting Whether a Metal Will Dissolve in Acid 955
20.5 Cell Potential, Free Energy, and the Equilibrium Constant 955
The Relationship between ∆G° and E ° cell 956
The Relationship between E ° cell and K 958
20.6 Cell Potential and Concentration 959
Cell Potential under Nonstandard Conditions: The Nernst Equation 959 Concentration Cells 962
CHEMISTRY AND MEDICINE Concentration Cells in Human Nerve Cells 964
20.7 Batteries: Using Chemistry to Generate Electricity 964
Dry-Cell Batteries 964 Lead–Acid Storage Batteries 965 Other Rechargeable Batteries 966 Fuel Cells 967
CHEMISTRY IN YOUR DAY The Fuel-Cell Breathalyzer 968
20.8 Electrolysis: Driving Nonspontaneous Chemical Reactions with Electricity 968
Predicting the Products of Electrolysis 971 Stoichiometry of Electrolysis 974
20.9 Corrosion: Undesirable Redox Reactions 975 Corrosion of Iron 976 Preventing the Corrosion of Iron 977
CHAPTER IN REVIEW Self-Assessment Quiz 978 Terms 979 Concepts 979 Equations and Relationships 980 Learning Outcomes 980
EXERCISES Review Questions 981 Problems by Topic 981 Cumulative Problems 985 Challenge Problems 986 Conceptual Problems 986 Questions for Group Work 986 Data
Interpretation and Analysis 987 Answers to Conceptual Connections 987
21 Radioactivity and Nuclear Chemistry 988
21.1 Diagnosing Appendicitis 989
21.2 The Discovery of Radioactivity 990
21.3 Types of Radioactivity 991
Alpha (a) Decay 992 Beta (b) Decay 993 Gamma (g) Ray Emission 994 Positron Emission 994 Electron Capture 995
21.4 The Valley of Stability: Predicting the Type of Radioactivity 996
Magic Numbers 998 Radioactive Decay Series 998
21.5 Detecting Radioactivity 999
21.6 The Kinetics of Radioactive Decay and Radiometric Dating 1000
The Integrated Rate Law 1002 Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Artifacts 1003
CHEMISTRY IN YOUR DAY Radiocarbon Dating and the Shroud of Turin 1005
Uranium/Lead Dating 1005 The Age of Earth 1006
21.7 The Discovery of Fission: The Atomic Bomb and Nuclear Power 1007
The Manhattan Project 1007 Nuclear Power: Using Fission to Generate Electricity 1009 Problems with Nuclear Power 1010
21.8 Converting Mass to Energy: Mass Defect and Nuclear Binding Energy 1011
Mass Defect and Nuclear Binding Energy 1011 The Nuclear Binding Energy Curve 1013
21.9 Nuclear Fusion: The Power of the Sun 1013
21.10 Nuclear Transmutation and Transuranium Elements 1014
21.11 The Effects of Radiation on Life 1016
Acute Radiation Damage 1016 Increased Cancer Risk 1016
Genetic Defects 1016 Measuring Radiation Exposure and Dose 1017
21.12 Radioactivity in Medicine and Other Applications 1018
Diagnosis in Medicine 1019 Radiotherapy in Medicine 1020 Other Applications 1020
CHAPTER IN REVIEW Self-Assessment Quiz 1021 Terms 1022 Concepts 1022 Equations and Relationships 1023
Learning Outcomes 1023
EXERCISES Review Questions 1024 Problems by Topic 1024
Cumulative Problems 1026 Challenge Problems 1027 Conceptual Problems 1028 Questions for Group Work 1028 Data Interpretation and Analysis 1029 Answers to Conceptual Connections 1029
Appendix I Common Mathematical Operations in Chemistry A-1
Appendix II Useful Data A-5
Appendix III Answers to Selected Exercises A-15
Appendix IV Answers to In-Chapter Practice Problems A-45
Glossary G-1
Photo and Text Credits C-1
Index I-1
