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• Periodic Table of the Elements
• Title Page
• Copyright Page
• Brief Contents
• Content
• Preface
• For Instructors
• 1 Chemical Tools: Experimentation and Measurement
• 1.1 The Scientific Method: Nanoparticle Catalysts for Fuel Cells
• 1.2 Measurements: SI Units and Scientific Notation
• 1.3 Mass and Its Measurement
• 1.4 Length and Its Measurement
• 1.5 Temperature and Its Measurement
• 1.6 Derived Units: Volume and Its Measurement
• 1.7 Derived Units: Density and Its Measurement
• 1.8 Derived Units: Energy and Its Measurement
• 1.9 Accuracy, Precision, and Significant Figures in Measurement
• 1.10 Significant Figures in Calculations
• 1.11 Converting from One Unit to Another
• INQUIRY? What are the unique properties of nanoscale materials?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 2 Atoms, Molecules, and Ions
• 2.1 Chemistry and the Elements
• 2.2 Elements and the Periodic Table
• 2.3 Some Common Groups of Elements and Their Properties
• 2.4 Observations Supporting Atomic Theory: The Conservation of Mass and the Law of Definite Proporti
• 2.5 The Law of Multiple Proportions and Dalton’s Atomic Theory
• 2.6 Atomic Structure: Electrons
• 2.7 Atomic Structure: Protons and Neutrons
• 2.8 Atomic Numbers
• 2.9 Atomic Weights and the Mole
• 2.10 Measuring Atomic Weight: Mass Spectrometry
• 2.11 Mixtures and Chemical Compounds; Molecules and Covalent Bonds
• 2.12 Ions and Ionic Bonds
• 2.13 Naming Chemical Compounds
• INQUIRY? How can measurements of oxygen and hydrogen isotopes in ice cores determine past climates?
• Study Guide
• Key Terms
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 3 Mass Relationships in Chemical Reactions
• 3.1 Representing Chemistry on Different Levels
• 3.2 Balancing Chemical Equations
• 3.3 Molecular Weight and Molar Mass
• 3.4 Stoichiometry: Relating Amounts of Reactants and Products
• 3.5 Yields of Chemical Reactions
• 3.6 Reactions with Limiting Amounts of Reactants
• 3.7 Percent Composition and Empirical Formulas
• 3.8 Determining Empirical Formulas: Elemental Analysis
• 3.9 Determining Molecular Weights: Mass Spectrometry
• INQUIRY? How is the principle of atom economy used to minimize waste in a chemical synthesis?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 4 Reactions in Aqueous Solution
• 4.1 Solution Concentration: Molarity
• 4.2 Diluting Concentrated Solutions
• 4.3 Electrolytes in Aqueous Solution
• 4.4 Types of Chemical Reactions in Aqueous Solution
• 4.5 Aqueous Reactions and Net Ionic Equations
• 4.6 Precipitation Reactions and Solubility Guidelines
• 4.7 Acids, Bases, and Neutralization Reactions
• 4.8 Solution Stoichiometry
• 4.9 Measuring the Concentration of a Solution: Titration
• 4.10 Oxidation–Reduction (Redox) Reactions
• 4.11 Identifying Redox Reactions
• 4.12 The Activity Series of the Elements
• 4.13 Redox Titrations
• 4.14 Some Applications of Redox Reactions
• INQUIRY? How do sports drinks replenish the substances lost in sweat?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 5 Periodicity and the Electronic Structure of Atoms
• 5.1 Wave Properties of Radiant Energy and the Electromagnetic Spectrum
• 5.2 Particlelike Properties of Radiant Energy: The Photoelectric Effect and Planck’s Postulate
• 5.3 Atomic Line Spectra and Quantized Energy
• 5.4 Wavelike Properties of Matter: de Broglie’s Hypothesis
• 5.5 The Quantum Mechanical Model of the Atom: Heisenberg’s Uncertainty Principle
• 5.6 The Quantum Mechanical Model of the Atom: Orbitals and Quantum Numbers
• 5.7 The Shapes of Orbitals
• 5.8 Electron Spin and the Pauli Exclusion Principle
• 5.9 Orbital Energy Levels in Multielectron Atoms
• 5.10 Electron Configurations of Multielectron Atoms
• 5.11 Anomalous Electron Configurations
• 5.12 Electron Configurations and the Periodic Table
• 5.13 Electron Configurations and Periodic Properties: Atomic Radii
• INQUIRY? How does knowledge of atomic emission spectra help us build more efficient light bulbs?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 6 Ionic Compounds: Periodic Trends and Bonding Theory
• 6.1 Electron Configurations of Ions
• 6.2 Ionic Radii
• 6.3 Ionization Energy
• 6.4 Higher Ionization Energies
• 6.5 Electron Affinity
• 6.6 The Octet Rule
• 6.7 Ionic Bonds and the Formation of Ionic Solids
• 6.8 Lattice Energies in Ionic Solids
• INQUIRY? How do ionic liquids lead to more environmentally friendly processes?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 7 Covalent Bonding and Electron-Dot Structures
• 7.1 Covalent Bonding in Molecules
• 7.2 Strengths of Covalent Bonds
• 7.3 Polar Covalent Bonds: Electronegativity
• 7.4 A Comparison of Ionic and Covalent Compounds
• 7.5 Electron-Dot Structures: The Octet Rule
• 7.6 Procedure for Drawing Electron-Dot Structures
• 7.7 Drawing Electron-Dot Structures for Radicals
• 7.8 Electron-Dot Structures of Compounds Containing Only Hydrogen and Second-Row Elements
• 7.9 Electron-Dot Structures and Resonance
• 7.10 Formal Charges
• INQUIRY? How does bond polarity affect the toxicity of organophosphate insecticides?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 8 Covalent Compounds: Bonding Theories and Molecular Structure
• 8.1 Molecular Shapes: The VSEPR Model
• 8.2 Valence Bond Theory
• 8.3 Hybridization and sp3 Hybrid Orbitals
• 8.4 Other Kinds of Hybrid Orbitals
• 8.5 Polar Covalent Bonds and Dipole Moments
• 8.6 Intermolecular Forces
• 8.7 Molecular Orbital Theory: The Hydrogen Molecule
• 8.8 Molecular Orbital Theory: Other Diatomic Molecules
• 8.9 Combining Valence Bond Theory and Molecular Orbital Theory
• INQUIRY? Which is better for human health, natural or synthetic vitamins?
• Study Guide
• Key Terms
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 9 Thermochemistry: Chemical Energy
• 9.1 Energy and Its Conservation
• 9.2 Internal Energy and State Functions
• 9.3 Expansion Work
• 9.4 Energy and Enthalpy
• 9.5 Thermochemical Equations and the Thermodynamic Standard State
• 9.6 Enthalpies of Chemical and Physical Changes
• 9.7 Calorimetry and Heat Capacity
• 9.8 Hess’s Law
• 9.9 Standard Heats of Formation
• 9.10 Bond Dissociation Energies
• 9.11 An Introduction to Entropy
• 9.12 An Introduction to Free Energy
• INQUIRY? How do we determine the energy content of biofuels?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 10 Gases: Their Properties and Behavior
• 10.1 Gases and Gas Pressure
• 10.2 The Gas Laws
• 10.3 The Ideal Gas Law
• 10.4 Stoichiometric Relationships with Gases
• 10.5 Mixtures of Gases: Partial Pressure and Dalton’s Law
• 10.6 The Kinetic–Molecular Theory of Gases
• 10.7 Gas Diffusion and Effusion: Graham’s Law
• 10.8 The Behavior of Real Gases
• 10.9 The Earth’s Atmosphere and the Greenhouse Effect
• 10.10 Greenhouse Gases
• 10.11 Climate Change
• INQUIRY? How do inhaled anesthetics work?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 11 Liquids and Phase Changes
• 11.1 Properties of Liquids
• 11.2 Vapor Pressure and Boiling Point
• 11.3 Phase Changes between Solids, Liquids, and Gases
• 11.4 Energy Changes during Phase Transitions
• 11.5 Phase Diagrams
• 11.6 Liquid Crystals
• INQUIRY? How is caffeine removed from coffee?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 12 Solids and Solid-State Materials
• 12.1 Types of Solids
• 12.2 Probing the Structure of Solids: X-Ray Crystallography
• 12.3 The Packing of Spheres in Crystalline Solids: Unit Cells
• 12.4 Structures of Some Ionic Solids
• 12.5 Structures of Some Covalent Network Solids
• 12.6 Bonding in Metals
• 12.7 Semiconductors
• 12.8 Semiconductor Applications
• 12.9 Superconductors
• 12.10 Ceramics and Composites
• INQUIRY? What are quantum dots, and what controls their color?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 13 Solutions and Their Properties
• 13.1 Solutions
• 13.2 Enthalpy Changes and the Solution Process
• 13.3 Predicting Solubility
• 13.4 Concentration Units for Solutions
• 13.5 Some Factors That Affect Solubility
• 13.6 Physical Behavior of Solutions: Colligative Properties
• 13.7 Vapor-Pressure Lowering of Solutions: Raoult’s Law
• 13.8 Boiling-Point Elevation and Freezing-Point Depression of Solutions
• 13.9 Osmosis and Osmotic Pressure
• INQUIRY? How does hemodialysis cleanse the blood of patients with kidney failure?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 14 Chemical Kinetics
• 14.1 Reaction Rates
• 14.2 Rate Laws and Reaction Order
• 14.3 Method of Initial Rates: Experimental Determination of a Rate Law
• 14.4 Integrated Rate Law: Zeroth-Order Reactions
• 14.5 Integrated Rate Law: First-Order Reactions
• 14.6 Integrated Rate Law: Second-Order Reactions
• 14.7 Reaction Rates and Temperature: The Arrhenius Equation
• 14.8 Using the Arrhenius Equation
• 14.9 Reaction Mechanisms
• 14.10 Rate Laws for Elementary Reactions
• 14.11 Rate Laws for Overall Reactions
• 14.12 Catalysis
• 14.13 Homogeneous and Heterogeneous Catalysts
• INQUIRY? How do enzymes work?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 15 Chemical Equilibrium
• 15.1 The Equilibrium State
• 15.2 The Equilibrium Constant Kc
• 15.3 The Equilibrium Constant Kp
• 15.4 Heterogeneous Equilibria
• 15.5 Using the Equilibrium Constant
• 15.6 Factors That Alter the Composition of an Equilibrium Mixture: Le Châtelier’s Principle
• 15.7 Altering an Equilibrium Mixture: Changes in Concentration
• 15.8 Altering an Equilibrium Mixture: Changes in Pressure and Volume
• 15.9 Altering an Equilibrium Mixture: Changes in Temperature
• 15.10 The Link between Chemical Equilibrium and Chemical Kinetics
• INQUIRY? How does high altitude affect oxygen transport in the body?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 16 Aqueous Equilibria: Acids and Bases
• 16.1 Acid–Base Concepts: The Brønsted–Lowry Theory
• 16.2 Acid Strength and Base Strength
• 16.3 Factors That Affect Acid Strength
• 16.4 Dissociation of Water
• 16.5 The pH Scale
• 16.6 Measuring pH
• 16.7 The pH in Solutions of Strong Acids and Strong Bases
• 16.8 Equilibria in Solutions of Weak Acids
• 16.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids
• 16.10 Percent Dissociation in Solutions of Weak Acids
• 16.11 Polyprotic Acids
• 16.12 Equilibria in Solutions of Weak Bases
• 16.13 Relation Between Ka and Kb
• 16.14 Acid–Base Properties of Salts
• 16.15 Lewis Acids and Bases
• INQUIRY? Has the problem of acid rain been solved?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 17 Applications of Aqueous Equilibria
• 17.1 Neutralization Reactions
• 17.2 The Common-Ion Effect
• 17.3 Buffer Solutions
• 17.4 The Henderson–Hasselbalch Equation
• 17.5 pH Titration Curves
• 17.6 Strong Acid–Strong Base Titrations
• 17.7 Weak Acid–Strong Base Titrations
• 17.8 Weak Base–Strong Acid Titrations
• 17.9 Polyprotic Acid–Strong Base Titrations
• 17.10 Solubility Equilibria for Ionic Compounds
• 17.11 Measuring Ksp and Calculating Solubility from Ksp
• 17.12 Factors That Affect Solubility
• 17.13 Precipitation of Ionic Compounds
• 17.14 Separation of Ions by Selective Precipitation
• 17.15 Qualitative Analysis
• INQUIRY? What is causing ocean acidification?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 18 Thermodynamics: Entropy, Free Energy, and Spontaneity
• 18.1 Spontaneous Processes
• 18.2 Enthalpy, Entropy, and Spontaneous Processes
• 18.3 Entropy and Probability
• 18.4 Entropy and Temperature
• 18.5 Standard Molar Entropies and Standard Entropies of Reaction
• 18.6 Entropy and the Second Law of Thermodynamics
• 18.7 Free Energy and the Spontaneity of Chemical Reactions
• 18.8 Standard Free-Energy Changes for Reactions
• 18.9 Standard Free Energies of Formation
• 18.10 Free-Energy Changes for Reactions under Nonstandard-State Conditions
• 18.11 Free Energy and Chemical Equilibrium
• INQUIRY? Does the formation of highly ordered molecules violate the second law of thermodynamics?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 19 Electrochemistry
• 19.1 Balancing Redox Reactions by the Half-Reaction Method
• 19.2 Galvanic Cells
• 19.3 Shorthand Notation for Galvanic Cells
• 19.4 Cell Potentials and Free-Energy Changes for Cell Reactions
• 19.5 Standard Reduction Potentials
• 19.6 Using Standard Reduction Potentials
• 19.7 Cell Potentials under Nonstandard-State Conditions: The Nernst Equation
• 19.8 Electrochemical Determination of pH
• 19.9 Standard Cell Potentials and Equilibrium Constants
• 19.10 Batteries
• 19.11 Corrosion
• 19.12 Electrolysis and Electrolytic Cells
• 19.13 Commercial Applications of Electrolysis
• 19.14 Quantitative Aspects of Electrolysis
• INQUIRY? How do hydrogen fuel cells work?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 20 Nuclear Chemistry
• 20.1 Nuclear Reactions and Their Characteristics
• 20.2 Radioactivity
• 20.3 Nuclear Stability
• 20.4 Radioactive Decay Rates
• 20.5 Dating with Radioisotopes
• 20.6 Energy Changes during Nuclear Reactions
• 20.7 Nuclear Fission and Fusion
• 20.8 Nuclear Transmutation
• 20.9 Detecting and Measuring Radioactivity
• INQUIRY? How are radioisotopes used in medicine?
• Study Guide
• Key Terms
• Key Equations
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 21 Transition Elements and Coordination Chemistry
• 21.1 Electron Configurations
• 21.2 Properties of Transition Elements
• 21.3 Oxidation States of Transition Elements
• 21.4 Coordination Compounds
• 21.5 Ligands
• 21.6 Naming Coordination Compounds
• 21.7 Isomers
• 21.8 Enantiomers and Molecular Handedness
• 21.9 Color of Transition Metal Complexes
• 21.10 Crystal Field Theory
• 21.11 Bonding in Complexes: Valence Bond Theory
• INQUIRY? How does cisplatin kill cancer cells?
• Study Guide
• Key Terms
• Key Equation
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 22 The Main-Group Elements
• 22.1 A Review of General Properties and Periodic Trends
• 22.2 Distinctive Properties of the Second-Row Elements
• 22.3 Group 1A: Hydrogen
• 22.4 Group 1A: Alkali Metals and Group 2A: Alkaline Earth Metals
• 22.5 Group 3A Elements
• 22.6 Group 4A Elements
• 22.7 Group 5A Elements
• 22.8 Group 6A Elements
• 22.9 Group 7A: The Halogens
• 22.10 Group 8A: Noble Gases
• INQUIRY? What are the barriers to a hydrogen economy?
• Study Guide
• Key Terms
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• 23 Organic and Biological Chemistry
• 23.1 Organic Molecules and Their Structures: Consitutional Isomers
• 23.2 Stereoisomers: Chiral Molecules
• 23.3 Families of Organic Compounds: Functional Groups
• 23.4 Carbohydrates: A Biological Example of Isomers
• 23.5 Valence Bond Theory and Orbital Overlap Pictures
• 23.6 Lipids: A Biological Example of Cis–Trans Isomerism
• 23.7 Formal Charge and Resonance in Organic Compounds
• 23.8 Conjugated Systems
• 23.9 Proteins: A Biological Example of Conjugation
• 23.10 Aromatic Compounds and Molecular Orbital Theory
• 23.11 Nucleic Acids: A Biological Example of Aromaticity
• INQUIRY? Why do enantiomers have different biological responses?
• Study Guide
• Key Terms
• Practice Test
• Conceptual Problems
• Section Problems
• Multiconcept Problems
• Appendix A: Mathematical Operations
• A.1 Scientific Notation
• A.2 Logarithms
• A.3 Straight-Line Graphs and Linear Equations
• A.4 Quadratic Equations
• A.5 Calculus Derivations of Integrated Rate Laws
• Appendix B: Thermodynamic Properties at 25 °C
• Appendix C: Equilibrium Constants at 25 °C
• Appendix D: Standard Reduction Potentials at 25 °C
• Appendix E: Properties of Water
• Answers to Selected Problems
• Glossary
• Index
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• B
• C
• D
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• F
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• Photo/Text Credits
• Back Cover