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• Periodic Table of the Elements
• List of Elements with Their Symbols and Atomic Weights
• Half Title
• Title Page
• Copyright
• Dedication
• Brief Contents
• Contents
• Chemical Applications and Essays
• Interactive Media
• Preface
• About The Authors
• Visual Walkthrough
  • New Levels of Student Interaction for Improved Conceptual Understanding
  • Visually Revised to Better Help Students Build General Chemistry
  • Knowledge and Understanding
  • Continuous Learning Before, During, and After Class with Pearson Mastering Chemistry (I)
  • Continuous Learning Before, During, and After Class with Pearson Mastering Chemistry (II)
  • Continuous Learning Before, During, and After Class with Pearson Mastering Chemistry (III)
  • Continuous Learning Before, During, and After Class with Pearson Mastering Chemistry (IV)
  • Instructor and Student Resources
• Chapter 1: Introduction: Matter, Energy, and Measurement
  • 1.1 The Study of Chemistry
    • The Atomic and Molecular Perspective of Chemistry
    • Why Study Chemistry?
  • 1.2 Classifications of Matter
    • States of Matter
    • Pure Substances
    • Elements
    • Compounds
    • Mixtures
  • 1.3 Properties of Matter
    • Physical and Chemical Changes
    • Separation of Mixtures
  • 1.4 The Nature of Energy
    • Kinetic Energy and Potential Energy
  • 1.5 Units of Measurement
    • SI Units
    • Length and Mass
    • Temperature
    • Derived SI Units
    • Volume
    • Density
    • Units of Energy
  • 1.6 Uncertainty in Measurement
    • Precision and Accuracy
    • Significant Figures
    • Significant Figures in Calculations
  • 1.7 Dimensional Analysis
    • Conversion Factors
    • Using Two or More Conversion Factors
    • Conversions Involving Volume
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Chemistry Put to Work Chemistry and the Chemical Industry
  • A Closer Look The Scientific Method
  • Chemistry Put to Work Chemistry in the News
  • Strategies for Success Estimating Answers
  • Strategies for Success The Importance of Practice
  • Strategies for Success The Features of This Book
• Chapter 2: Atoms, Molecules, and Ions
  • 2.1 The Atomic Theory of Matter
  • 2.2 The Discovery of Atomic Structure
    • Cathode Rays and Electrons
    • Radioactivity
    • The Nuclear Model of the Atom
  • 2.3 The Modern View of Atomic Structure
    • Atomic Numbers, Mass Numbers, and Isotopes
  • 2.4 Atomic Weights
    • The Atomic Mass Scale
    • Atomic Weight
  • 2.5 The Periodic Table
  • 2.6 Molecules and Molecular Compounds
    • Molecules and Chemical Formulas
    • Molecular and Empirical Formulas
    • Picturing Molecules
  • 2.7 Ions and Ionic Compounds
    • Predicting Ionic Charges
    • Ionic Compounds
  • 2.8 Naming Inorganic Compounds
    • Names and Formulas of Ionic Compounds
    • Names and Formulas of Acids
    • Names and Formulas of Binary Molecular Compounds
  • 2.9 Some Simple Organic Compounds
    • Alkanes
    • Some Derivatives of Alkanes
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • A Closer Look Basic Forces
  • A Closer Look The Mass Spectrometer
  • Chemistry and Life Elements Required by Living Organisms
  • Strategies for Success How to Take a Test
• Chapter 3: Chemical Reactions and Stoichiometry
  • 3.1 The Conservation of Mass, Chemical Equations, and Stoichiometry
    • How to Balance Chemical Equations
    • A Step-by-Step Example of Balancing a Chemical Equation
  • 3.2 Simple Patterns of Chemical Reactivity: Combination, Decomposition, and Combustion
    • Combination and Decomposition Reactions
    • Combustion Reactions
  • 3.3 Formula Weights and Elemental Compositions of Substances
    • Formula and Molecular Weights
    • Elemental Compositions of Substances
  • 3.4 Avogadro’s Number and the Mole; Molar Mass
    • The Mole and Avogadro’s Number
    • Molar Mass
    • Converting Between Masses, Moles, and Atoms/Molecules/Ions
  • 3.5 Formula Weights and Elemental Compositions of Substances
    • Molecular Formulas from Empirical Formulas
    • Combustion Analysis
  • 3.6 Reaction Stoichiometry
  • 3.7 Limiting Reactants
    • Theoretical and Percent Yields
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Strategies for Success Problem Solving
  • Chemistry and Life Glucose Monitoring
  • Strategies for Success Design an Experiment
• Chapter 4: Reactions in Aqueous Solution
  • 4.1 General Properties of Aqueous Solutions
    • Electrolytes and Nonelectrolytes
    • How Compounds Dissolve in Water
    • Strong and Weak Electrolytes
  • 4.2 Precipitation Reactions
    • Solubility Guidelines for Ionic Compounds
    • Exchange (Metathesis) Reactions
    • Ionic Equations and Spectator Ions
  • 4.3 Acids, Bases, and Neutralization Reactions
    • Acids
    • Bases
    • Strong and Weak Acids and Bases
    • Identifying Strong and Weak Electrolytes
    • Neutralization Reactions and Salts
    • Neutralization Reactions with Gas Formation
  • 4.4 Oxidation–Reduction Reactions
    • Oxidation and Reduction
    • Oxidation Numbers
    • Oxidation of Metals by Acids and Salts
    • The Activity Series
  • 4.5 Concentrations of Solutions
    • Molarity
    • Expressing the Concentration of an Electrolyte
    • Interconverting Molarity, Moles, and Volume
    • Dilution
  • 4.6 Solution Stoichiometry and Chemical Analysis
    • Titrations
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry Put to Work Antacids
  • Strategies for Success Analyzing Chemical Reactions
• Chapter 5: Thermochemistry
  • 5.1 The Nature of Chemical Energy
  • 5.2 The First Law of Thermodynamics
    • System and Surroundings
    • Internal Energy
    • Relating ΔE to Heat and Work
    • Endothermic and Exothermic Processes
    • State Functions
  • 5.3 Enthalpy
    • Pressure–Volume Work
    • Enthalpy Change
  • 5.4 Enthalpies of Reaction
  • 5.5 Calorimetry
    • Heat Capacity and Specific Heat
    • Constant-Pressure Calorimetry
    • Bomb Calorimetry (Constant-Volume Calorimetry)
  • 5.6 Hess’s Law
  • 5.7 Enthalpies of Formation
    • Using Enthalpies of Formation to Calculate Enthalpies of Reaction
  • 5.8 Bond Enthalpies
    • Bond Enthalpies and the Enthalpies of Reactions
  • 5.9 Foods and Fuels
    • Foods
    • Fuels
    • Other Energy Sources
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Energy, Enthalpy, and P-V Work
  • A Closer Look Using Enthalpy as a Guide
  • Chemistry and Life The Regulation of Body Temperature
  • Chemistry Put to Work The Scientific and Political Challenges of Biofuels
• Chapter 6: Electronic Structure of Atoms
  • 6.1 The Wave Nature of Light
  • 6.2 Quantized Energy and Photons
    • Hot Objects and the Quantization of Energy
    • The Photoelectric Effect and Photons
  • 6.3 Line Spectra and the Bohr Model
    • Line Spectra
    • Bohr’s Model
    • The Energy States of the Hydrogen Atom
    • Limitations of the Bohr Model
  • 6.4 The Wave Behavior of Matter
    • The Uncertainty Principle
  • 6.5 Quantum Mechanics and Atomic Orbitals
    • Orbitals and Quantum Numbers
  • 6.6 Representations of Orbitals
    • The s Orbitals
    • The p Orbitals
    • The d and f Orbitals
  • 6.7 Many-Electron Atoms
    • Orbitals and Their Energies
    • Electron Spin and the Pauli Exclusion Principle
  • 6.8 Electron Configurations
    • Hund’s Rule
    • Condensed Electron Configurations
    • Transition Metals
    • The Lanthanides and Actinides
  • 6.9 Electron Configurations and the Periodic Table
    • Anomalous Electron Configurations
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Measurement and the Uncertainty Principle
  • A Closer Look Thought Experiments and Schrödinger’s Cat
  • A Closer Look Probability Density and Radial Probability Functions
  • Chemistry and Life Nuclear Spin and Magnetic Resonance Imaging
• Chapter 7: Periodic Properties of the Elements
  • 7.1 Development of the Periodic Table
  • 7.2 Effective Nuclear Charge
  • 7.3 Sizes of Atoms and Ions
    • Periodic Trends in Atomic Radii
    • Periodic Trends in Ionic Radii
  • 7.4 Ionization Energy
    • Variations in Successive Ionization Energies
    • Periodic Trends in First Ionization Energies
    • Electron Configurations of Ions
  • 7.5 Electron Affinity
    • Periodic Trends in Electron Affinity
  • 7.6 Metals, Nonmetals, and Metalloids
    • Metals
    • Nonmetals
    • Metalloids
  • 7.7 Trends for Group 1 and Group 2 Metals
    • Group 1: The Alkali Metals
    • Group 2: The Alkaline Earth Metals
  • 7.8 Trends for Selected Nonmetals
    • Hydrogen
    • Group 16: The Oxygen Group
    • Group 17: The Halogens
    • Group 18: The Noble Gases
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Effective Nuclear Charge
  • Chemistry Put to Work Ionic Size and Lithium-Ion Batteries
  • Chemistry and Life The Improbable Development of Lithium Drugs
• Chapter 8: Basic Concepts of Chemical Bonding
  • 8.1 Lewis Symbols and the Octet Rule
    • Lewis Symbols
    • The Octet Rule
  • 8.2 Ionic Bonding
    • Energetics of Ionic Bond Formation
    • Electron Configurations of Ions of the s- and p-Block Elements
    • Transition Metal Ions
  • 8.3 Covalent Bonding
    • Lewis Structures
    • Multiple Bonds
  • 8.4 Bond Polarity and Electronegativity
    • Electronegativity
    • Electronegativity and Bond Polarity
    • Dipole Moments
    • Comparing Ionic and Covalent Bonding
  • 8.5 Drawing Lewis Structures
    • Formal Charge and Alternative Lewis Structures
  • 8.6 Resonance Structures
    • Resonance in Benzene
  • 8.7 Exceptions to the Octet Rule
    • Odd Number of Electrons
    • Less Than an Octet of Valence Electrons
    • More Than an Octet of Valence Electrons
  • 8.8 Strengths and Lengths of Covalent Bonds
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Calculation of Lattice Energies: The Born–Haber Cycle
  • A Closer Look Oxidation Numbers, Formal Charges, and Actual Partial Charges
• Chapter 9: Molecular Geometry and Bonding Theories
  • 9.1 Molecular Shapes
  • 9.2 The VSEPR Model
    • Applying the VSEPR Model to Determine Molecular Shapes
    • Effect of Nonbonding Electrons and Multiple Bonds on Bond Angles
    • Molecules with Expanded Valence Shells
    • Shapes of Larger Molecules
  • 9.3 Molecular Shape and Molecular Polarity
  • 9.4 Covalent Bonding and Orbital Overlap
  • 9.5 Hybrid Orbitals
    • sp Hybrid Orbitals
    • sp2 and sp3 Hybrid Orbitals
    • Hypervalent Molecules
    • Hybrid Orbital Summary
  • 9.6 Multiple Bonds
    • Resonance Structures, Delocalization, and π Bonding
    • General Conclusions about σ and π Bonding
  • 9.7 Molecular Orbitals
    • Molecular Orbitals of the Hydrogen Molecule
    • Bond Order
  • 9.8 Bonding in Period 2 Diatomic Molecules
    • Molecular Orbitals for Li2 and Be2
    • Molecular Orbitals from 2p Atomic Orbitals
    • Electron Configurations for B2 through Ne2
    • Electron Configurations and Molecular Properties
    • Heteronuclear Diatomic Molecules
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Phases in Atomic and Molecular Orbitals
  • Chemistry Put to Work Orbitals and Energy
• Chapter 10: Gases
  • 10.1 Characteristics of Gases
  • 10.2 Pressure
    • Atmospheric Pressure and the Barometer
  • 10.3 The Gas Laws
    • The Pressure–Volume Relationship: Boyle’s Law
    • The Temperature–Volume Relationship: Charles’s Law
    • The Quantity–Volume Relationship: Avogadro’s Law
  • 10.4 The Ideal Gas Equation
    • Relating the Ideal Gas Equation and the Gas Laws
    • Gas Densities and Molar Mass
    • Volumes of Gases in Chemical Reactions
  • 10.5 Gas Mixtures and Partial Pressures
    • Partial Pressures and Mole Fractions
  • 10.6 The Kinetic-Molecular Theory of Gases
    • Distributions of Molecular Speed
    • Application of Kinetic-Molecular Theory to the Gas Laws
  • 10.7 Molecular Effusion and Diffusion
    • Graham’s Law of Effusion
    • Diffusion and Mean Free Path
  • 10.8 Real Gases: Deviations from Ideal Behavior
    • The van der Waals Equation
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry and Life Blood Pressure
  • Strategies for Success Calculations Involving Many Variables
  • A Closer Look The Ideal Gas Equation
  • Chemistry Put to Work Gas Separations
• Chapter 11: Liquids and Intermolecular Forces
  • 11.1 A Molecular Comparison of Gases, Liquids, and Solids
  • 11.2 Intermolecular Forces
    • Dispersion Forces
    • Dipole–Dipole Interactions
    • Hydrogen Bonding
    • Ion–Dipole Forces
    • Comparing Intermolecular Forces
  • 11.3 Select Properties of Liquids
    • Viscosity
    • Surface Tension
    • Capillary Action
  • 11.4 Phase Changes
    • Energy Changes Accompany Phase Changes
    • Heating Curves
    • Critical Temperature and Pressure
  • 11.5 Vapor Pressure
    • Volatility, Vapor Pressure, and Temperature
    • Vapor Pressure and Boiling Point
  • 11.6 Phase Diagrams
    • The Phase Diagrams of H2O and CO2
  • 11.7 Liquid Crystals
    • Types of Liquid Crystals
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry Put to Work Ionic Liquids
  • A Closer Look The Clausius–Clapeyron Equation
  • Chemistry and Life Liquid Crystal Displays
• Chapter 12: Solids and Modern Materials
  • 12.1 Classification of Solids
    • Crystalline and Amorphous Solids
    • Unit Cells and Crystal Lattices
    • Filling the Unit Cell
  • 12.2 Metallic Solids
    • The Structures of Metallic Solids
    • Close Packing
    • Alloys
    • Metallic Bonding
    • Electron-Sea Model
    • Molecular Orbital Model
  • 12.3 Ionic Solids
    • Structures of Ionic Solids
  • 12.4 Covalent Solids
    • Molecular Solids
    • Covalent-Network Solids
    • Semiconductors
    • Semiconductor Doping
  • 12.5 Polymers
    • Making Polymers
    • Structure and Physical Properties of Polymers
  • 12.6 Nanomaterials
    • Semiconductors on the Nanoscale
    • Metals on the Nanoscale
    • Carbon on the Nanoscale
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look X-ray Diffraction
  • Chemistry Put to Work Alloys of Gold
  • Chemistry Put to Work Solid-State Lighting
  • Chemistry Put to Work Modern Materials in the Automobile
  • Chemistry Put to Work Microporous and Mesoporous Materials
• Chapter 13: Properties of Solutions
  • 13.1 The Solution Process
    • The Natural Tendency toward Mixing
    • The Effect of Intermolecular Forces on Solution Formation
    • Energetics of Solution Formation
    • Solution Formation and Chemical Reactions
  • 13.2 Saturated Solutions and Solubility
  • 13.3 Factors Affecting Solubility
    • Solute–Solvent Interactions
    • Pressure Effects
    • Temperature Effects
  • 13.4 Expressing Solution Concentration
    • Mass Percentage, ppm, and ppb
    • Mole Fraction, Molarity, and Molality
    • Converting Concentration Units
  • 13.5 Colligative Properties
    • Vapor–Pressure Lowering
    • Boiling-Point Elevation
    • Freezing-Point Depression
    • Osmosis
    • Determination of Molar Mass from Colligative Properties
  • 13.6 Colloids
    • Hydrophilic and Hydrophobic Colloids
    • Colloidal Motion in Liquids
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry and Life Fat-Soluble and Water-Soluble Vitamins
  • Chemistry and Life Blood Gases and Deep-Sea Diving
  • A Closer Look Ideal Solutions with Two or More Volatile Components
  • A Closer Look The van’t Hoff Factor
  • Chemistry and Life Sickle-Cell Anemia
• Chapter 14: Chemical Kinetics
  • 14.1 Factors That Affect Reaction Rates
  • 14.2 Reaction Rates
    • Change of Rate with Time
    • Instantaneous Rate
    • Reaction Rates and Stoichiometry
  • 14.3 Concentration and Rate Laws
    • Reaction Orders: The Exponents in the Rate Law
    • Magnitudes and Units of Rate Constants
    • Using Initial Rates to Determine Rate Laws
  • 14.4 The Change of Concentration with Time
    • First-Order Reactions
    • Second-Order Reactions
    • Zero-Order Reactions
    • Half-Life
  • 14.5 Temperature and Rate
    • The Collision Model
    • The Orientation Factor
    • Activation Energy
    • The Arrhenius Equation
    • Determining the Activation Energy
  • 14.6 Reaction Mechanisms
    • Elementary Reactions
    • Multistep Mechanisms
    • Rate Laws for Elementary Reactions
    • The Rate-Determining Step for a Multistep Mechanism
    • Mechanisms with a Slow Initial Step
    • Mechanisms with a Fast Initial Step
  • 14.7 Catalysis
    • Homogeneous Catalysis
    • Heterogeneous Catalysis
    • Enzymes
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Using Spectroscopic Methods to Measure Reaction Rates: Beer’s Law
  • Chemistry Put to Work Bromomethane in the Atmosphere
  • Chemistry Put to Work Catalytic Converters
  • Chemistry and Life Nitrogen Fixation and Nitrogenase
• Chapter 15: Chemical Equilibrium
  • 15.1 The Concept of Equilibrium
  • 15.2 The Equilibrium Constant
    • Evaluating Kc
    • Equilibrium Constants in Terms of Pressure, Kp
    • Equilibrium Constants and Units
  • 15.3 Understanding and Working with Equilibrium Constants
    • The Magnitude of Equilibrium Constants
    • The Direction of the Chemical Equation and K
    • Relating Chemical Equation Stoichiometry and Equilibrium Constants
    • Heterogeneous Equilibria
  • 15.4 Calculating Equilibrium Constants
    • Applications of Equilibrium Constants
    • Predicting the Direction of Reaction
    • Calculating Equilibrium Concentrations
  • 15.5 Le Châtelier’s Principle
    • Change in Reactant or Product Concentration
    • Effects of Volume and Pressure Changes
    • Effect of Temperature Changes
    • The Effect of Catalysts
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry Put to Work The Haber Process
  • A Closer Look Temperature Changes and Le Châtelier’s Principle
  • Chemistry Put to Work Controlling Nitric Oxide Emissions
• Chapter 16: Acid–Base Equilibria
  • 16.1 Acid–Base Equilibria
    • Arrhenius Acids and Bases
    • Brønsted–Lowry Acids and Bases
    • The H+ Ion in Water
    • Proton-Transfer Reactions
    • Conjugate Acid–Base Pairs
    • Relative Strengths of Acids and Bases
  • 16.2 The Autoionization of Water
    • The Ion Product of Water
  • 16.3 The pH Scale
    • pOH and Other “p” Scales
    • Measuring pH
  • 16.4 Strong Acids and Bases
    • Strong Acids
    • Strong Bases
  • 16.5 Weak Acids
    • Calculating Ka from pH
    • Percent Ionization
    • Using Ka to Calculate pH
    • Polyprotic Acids
  • 16.6 Weak Bases
    • Types of Weak Bases
    • Relationship Between Ka and Kb
  • 16.7 Acid–Base Properties of Salt Solutions
    • An Anion’s Ability to React with Water
    • A Cation’s Ability to React with Water
    • Combined Effect of Cation and Anion in Solution
  • 16.8 Acid–Base Behavior and Chemical Structure
    • Factors That Affect Acid Strength
    • Binary Acids
    • Oxyacids
    • Carboxylic Acids
    • Lewis Acids and Bases
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Polyprotic Acids
  • Chemistry Put to Work Amines and Amine Hydrochlorides
  • Chemistry and Life The Amphiprotic Behavior of Amino Acids
• Chapter 17: Additional Aspects of Aqueous Equilibria
  • 17.1 The Common-Ion Effect
  • 17.2 Buffers
    • Composition and Action of Buffers
    • Calculating the pH of a Buffer
    • Buffer Capacity and pH Range
    • Addition of Strong Acids or Bases to Buffers
  • 17.3 Acid–Base Titrations
    • Strong Acid–Strong Base Titrations
    • Weak Acid–Strong Base Titrations
    • Titrating with an Acid–Base Indicator
    • Titrations of Polyprotic Acids
  • 17.4 Solubility Equilibria
    • The Solubility-Product Constant, Ksp
    • Solubility and Ksp
  • 17.5 Factors That Affect Solubility
    • The Common-Ion Effect
    • Solubility and pH
    • Formation of Complex Ions
    • Amphoterism
  • 17.6 Precipitation and Separation of Ions
    • Selective Precipitation of Ions
    • Qualitative Analysis for Metallic Elements
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry and Life Blood as a Buffered Solution
  • A Closer Look Limitations of Solubility Products
  • Chemistry and Life Tooth Decay and Fluoridation
  • A Closer Look Lead Contamination in Drinking Water
• Chapter 18: Chemistry of the Environment
  • 18.1 Earth’s Atmosphere
    • Composition of the Atmosphere
    • Photochemical Reactions in the Atmosphere
    • Ozone in the Stratosphere
  • 18.2 Human Activities and Earth’s Atmosphere
    • The Ozone Layer and Its Depletion
    • Sulfur Compounds and Acid Rain
    • Nitrogen Oxides and Photochemical Smog
    • Greenhouse Gases: Water Vapor, Carbon Dioxide, and Climate
  • 18.3 Earth’s Water
    • The Global Water Cycle
    • Salt Water: Earth’s Oceans and Seas
    • Freshwater and Groundwater
  • 18.4 Human Activities and Water Quality
    • Dissolved Oxygen and Water Quality
    • Water Purification: Desalination
    • Water Purification: Municipal Treatment
  • 18.5 Green Chemistry
    • Supercritical Solvents
    • Greener Reagents and Processes
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Other Greenhouse Gases
  • A Closer Look Fracking and Water Quality
  • Chemistry and Life Ocean Acidification
• Chapter 19: Chemical Thermodynamics
  • 19.1 Spontaneous Processes
    • Seeking a Criterion for Spontaneity
    • Reversible and Irreversible Processes
  • 19.2 Entropy and the Second Law of Thermodynamics
    • The Relationship between Entropy and Heat
    • ΔS for Phase Changes
    • The Second Law of Thermodynamics
  • 19.3 The Molecular Interpretation of Entropy and the Third Law of Thermodynamics
    • Expansion of a Gas at the Molecular Level
    • Boltzmann’s Equation and Microstates
    • Molecular Motions and Energy
    • Making Qualitative Predictions about ΔS
    • The Third Law of Thermodynamics
  • 19.4 Entropy Changes in Chemical Reactions
    • Temperature Variation of Entropy
    • Standard Molar Entropies
    • Calculating the Standard Entropy Change for a Reaction
    • Entropy Changes in the Surroundings
  • 19.5 Gibbs Free Energy
    • Standard Free Energy of Formation
  • 19.6 Free Energy and Temperature
  • 19.7 Free Energy and the Equilibrium Constant
    • Free Energy under Nonstandard Conditions
    • Relationship between ΔG° and K
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look The Entropy Change When a Gas Expands Isothermally
  • Chemistry and Life Entropy and Human Society
  • A Closer Look What’s “Free” About Free Energy?
  • Chemistry and Life Driving Nonspontaneous Reactions: Coupling Reactions
• Chapter 20: Electrochemistry
  • 20.1 Oxidation States and Oxidation–Reduction Reactions
  • 20.2 Balancing Redox Equations
    • Half-Reactions
    • Balancing Equations by the Method of Half-Reactions
    • Balancing Equations for Reactions Occurring in Basic Solution
  • 20.3 Voltaic Cells
  • 20.4 Cell Potentials under Standard Conditions
    • Standard Reduction Potentials
    • Strengths of Oxidizing and Reducing Agents
  • 20.5 Free Energy and Redox Reactions
    • Emf, Free Energy, and the Equilibrium Constant
  • 20.6 Cell Potentials under Nonstandard Conditions
    • The Nernst Equation
    • Concentration Cells
  • 20.7 Batteries and Fuel Cells
    • Lead–Acid Battery
    • Alkaline Battery
    • Nickel–Cadmium and Nickel–Metal Hydride Batteries
    • Lithium-Ion Batteries
    • Hydrogen Fuel Cells
  • 20.8 Corrosion
    • Corrosion of Iron (Rusting)
    • Preventing Corrosion of Iron
  • 20.9 Electrolysis
    • Quantitative Aspects of Electrolysis
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Electrical Work
  • Chemistry and Life Heartbeats and Electrocardiography
  • Chemistry Put to Work Batteries for Hybrid and Electric Vehicles
  • Chemistry Put to Work Electrometallurgy of Aluminum
• Chapter 21: Nuclear Chemistry
  • 21.1 Radioactivity and Nuclear Equations
    • Nuclear Equations
    • Types of Radioactive Decay
  • 21.2 Patterns of Nuclear Stability
    • Neutron-to-Proton Ratio
    • Radioactive Decay Chains
    • Further Observations
    • Nuclear Transmutations
    • Accelerating Charged Particles
    • Reactions Involving Neutrons
    • Transuranium Elements
  • 21.3 Rates of Radioactive Decay
    • Radiometric Dating
    • Calculations Based on Half-Life
  • 21.4 Detection of Radioactivity
    • Radiotracers
  • 21.5 Energy Changes in Nuclear Reactions
    • Nuclear Binding Energies
    • Nuclear Power: Fission
    • Nuclear Reactors
    • Nuclear Waste
    • Nuclear Power: Fusion
  • 21.6 Radiation in the Environment and Living Systems
    • Radiation Doses
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Key Equations
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry and Life Medical Applications of Radiotracers
  • A Closer Look The Dawning of the Nuclear Age
  • A Closer Look Nuclear Synthesis of the Elements
  • Chemistry and Life Radiation Therapy
• Chapter 22: Chemistry of the Nonmetals
  • 22.1 Periodic Trends and Chemical Reactions
    • Chemical Reactions
  • 22.2 Hydrogen
    • Isotopes of Hydrogen
    • Properties of Hydrogen
    • Production of Hydrogen
    • Uses of Hydrogen
    • Binary Hydrogen Compounds
  • 22.3 Group 18: The Noble Gases
    • Noble Gas Compounds
  • 22.4 Group 17: The Halogens
    • Properties and Production of the Halogens
    • Uses of the Halogens
    • The Hydrogen Halides
    • Interhalogen Compounds
    • Oxyacids and Oxyanions
  • 22.5 Oxygen
    • Properties of Oxygen
    • Production of Oxygen
    • Uses of Oxygen
    • Ozone
    • Oxides
    • Peroxides and Superoxides
  • 22.6 The Other Group 16 Elements: S, Se, Te, and Po
    • Occurrence and Production of S, Se, and Te
    • Properties and Uses of Sulfur, Selenium, and Tellurium
    • Sulfides
    • Oxides, Oxyacids, and Oxyanions of Sulfur
  • 22.7 Nitrogen
    • Properties of Nitrogen
    • Production and Uses of Nitrogen
    • Hydrogen Compounds of Nitrogen
    • Oxides and Oxyacids of Nitrogen
  • 22.8 The Other Group 15 Elements: P, As, Sb, and Bi
    • Occurrence, Isolation, and Properties of Phosphorus
    • Phosphorus Halides
    • Oxy Compounds of Phosphorus
  • 22.9 Carbon
    • Elemental Forms of Carbon
    • Oxides of Carbon
    • Carbonic Acid and Carbonates
    • Carbides
  • 22.10 The Other Group 14 Elements: Si, Ge, Sn, and Pb
    • General Characteristics of the Group 14 Elements
    • Occurrence and Preparation of Silicon
    • Silicates
    • Glass
    • Silicones
  • 22.11 Boron
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look The Hydrogen Economy
  • Chemistry and Life Nitroglycerin, Nitric Oxide, and Heart Disease
  • Chemistry and Life Arsenic in Drinking Water
  • Chemistry Put to Work Carbon Fibers and Composites
• Chapter 23: Transition Metals and Coordination Chemistry
  • 23.1 The Transition Metals
    • Physical Properties
    • Electron Configurations and Oxidation States
    • Magnetism
  • 23.2 Transition-Metal Complexes
    • The Development of Coordination Chemistry: Werner’s Theory
    • The Metal–Ligand Bond
    • Charges, Coordination Numbers, and Geometries
  • 23.3 Common Ligands in Coordination Chemistry
    • Metals and Chelates in Living Systems
  • 23.4 Nomenclature and Isomerism in Coordination Chemistry
    • Isomerism
    • Constitutional Isomerism
    • Stereoisomerism
  • 23.5 Color and Magnetism in Coordination Chemistry
    • Color
    • Magnetism of Coordination Compounds
  • 23.6 Crystal-Field Theory
    • Electron Configurations in Octahedral Complexes
    • Tetrahedral and Square-Planar Complexes
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • A Closer Look Entropy and the Chelate Effect
  • Chemistry and Life The Battle for Iron in Living Systems
  • A Closer Look Charge-Transfer Color
• Chapter 24: The Chemistry of Life: Organic and Biological Chemistry
  • 24.1 General Characteristics of Organic Molecules
    • The Structures of Organic Molecules
    • The Stability of Organic Compounds
    • Solubility and Acid–Base Properties of Organic Compounds
  • 24.2 Introduction to Hydrocarbons
    • Structures of Alkanes
    • Constitutional Isomers
    • Nomenclature of Alkanes
    • Cycloalkanes
    • Reactions of Alkanes
  • 24.3 Alkenes, Alkynes, and Aromatic Hydrocarbons
    • Alkenes
    • Alkynes
    • Addition Reactions of Alkenes and Alkynes
    • Aromatic Hydrocarbons
    • Stabilization of π Electrons by Delocalization
    • Substitution Reactions of Aromatic Hydrocarbons
  • 24.4 Organic Functional Groups
    • Alcohols
    • Ethers
    • Aldehydes and Ketones
    • Carboxylic Acids and Esters
    • Amines and Amides
  • 24.5 Chirality in Organic Chemistry
  • 24.6 Introduction to Biochemistry
  • 24.7 Proteins
    • Amino Acids
    • Polypeptides and Proteins
    • Protein Structure
  • 24.8 Carbohydrates
    • Disaccharides
    • Polysaccharides
  • 24.9 Lipids
    • Fats
    • Phospholipids
  • 24.10 Nucleic Acids
  • Chapter Summary and Key Terms
  • Learning Outcomes
  • Exercises
  • Additional Exercises
  • Integrative Exercises
  • Design an Experiment
  • Chemistry Put to Work Petroleum
  • A Closer Look Mechanism of Addition Reactions
  • Strategies for Success What Now?
• Appendices
  • Appendix A: Mathematical Operations
  • Appendix B: Properties of Water
  • Appendix C: Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C)
  • Appendix D: Aqueous Equilibrium Constants
  • Appendix E: Standard Reduction Potentials at 25 °C
• Answers to Selected Exercises
• Answers to Go Figure
• Answers to Selected Practice Exercises
• Glossary
• Photo and Art Credits
• Index
  • A
  • B
  • C
  • D
  • E
  • F
  • G
  • H
  • I
  • J
  • K
  • L
  • M
  • N
  • O
  • P
  • Q
  • R
  • S
  • T
  • U
  • V
  • W
  • X
  • Y
  • Z
• Common Ions
• Fundamental Constants
• Useful Conversion Factors and Relationships
• Color Chart for Common Elements

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