Efnisyfirlit

• 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
  • 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
• Photo/Text Credits
• Back Cover

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