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Table of Contents
- The Chemical World
- 1.1 Sand and Water
- 1.2 Chemicals Compose Ordinary Things
- 1.3 The Scientific Method: How Chemists Think
- 1.4 Analyzing and Interpreting Data
- 1.5 A Beginning Chemist: How to Succeed
- Measurement and Problem Solving
- 2.1 The Metric Mix-up: A $125 Million Unit Error
- 2.2 Scientific Notation: Writing Large and Small Numbers
- 2.3 Significant Figures: Writing Numbers to Reflect Precision
- 2.4 Significant Figures in Calculations
- 2.5 The Basic Units of Measurement
- 2.6 Problem Solving and Unit Conversion
- 2.7 Solving Multistep Unit Conversion Problems
- 2.8 Unit Conversion in Both the Numerator and Denominator
- 2.9 Units Raised to a Power
- 2.10 Density
- 2.11 Numerical Problem-Solving Strategies and the Solution Map
- Matter and Energy
- 3.1 In Your Room
- 3.2 What Is Matter?
- 3.3 Classifying Matter According to Its State: Solid, Liquid, and Gas
- 3.4 Classifying Matter According to Its Composition: Elements, Compounds, and Mixtures
- 3.5 Differences in Matter: Physical and Chemical Properties
- 3.6 Changes in Matter: Physical and Chemical Changes
- 3.7 Conservation of Mass: There Is No New Matter
- 3.8 Energy
- 3.9 Energy and Chemical and Physical Change
- 3.10 Temperature: Random Motion of Molecules and Atoms
- 3.11 Temperature Changes: Heat Capacity
- 3.12 Energy and Heat Capacity Calculations
- Atoms and Elements
- 4.1 Experiencing Atoms at Tiburon
- 4.2 Indivisible: The Atomic Theory
- 4.3 The Nuclear Atom
- 4.4 The Properties of Protons, Neutrons, and Electrons
- 4.5 Elements: Defined by Their Numbers of Protons
- 4.6 Looking for Patterns: The Periodic Law and the Periodic Table
- 4.7 Ions: Losing and Gaining Electrons
- 4.8 Isotopes: When the Number of Neutrons Varies
- 4.9 Atomic Mass: The Average Mass of an Element’s Atoms
- Molecules and Compounds
- 5.1 Sugar and Salt
- 5.2 Compounds Display Constant Composition
- 5.3 Chemical Formulas: How to Represent Compounds
- 5.4 A Molecular View of Elements and Compounds
- 5.5 Writing Formulas for Ionic Compounds
- 5.6 Nomenclature: Naming Compounds
- 5.7 Naming Ionic Compounds
- 5.8 Naming Molecular Compounds
- 5.9 Naming Acids
- 5.10 Nomenclature Summary
- 5.11 Formula Mass: The Mass of a Molecule or Formula Unit
- Chemical Composition
- 6.1 How Much Sodium?
- 6.2 Counting Nails by the Pound
- 6.3 Counting Atoms by the Gram
- 6.4 Counting Molecules by the Gram
- 6.5 Chemical Formulas as Conversion Factors
- 6.6 Mass Percent Composition of Compounds
- 6.7 Mass Percent Composition from a Chemical Formula
- 6.8 Calculating Empirical Formulas for Compounds
- 6.9 Calculating Molecular Formulas for Compounds
- Chemical Reactions
- 7.1 Grade School Volcanoes, Automobiles, and Laundry Detergents
- 7.2 Evidence of a Chemical Reaction
- 7.3 The Chemical Equation
- 7.4 How to Write Balanced Chemical Equations
- 7.5 Aqueous Solutions and Solubility: Compounds Dissolved in Water
- 7.6 Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid
- 7.7 Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations
- 7.8 Acid—Base and Gas Evolution Reactions
- 7.9 Oxidation—Reduction Reactions
- 7.10 Classifying Chemical Reactions
- Quantities in Chemical Reactions
- 8.1 Climate Change: Too Much Carbon Dioxide
- 8.2 Making Pancakes: Relationships between Ingredients
- 8.3 Making Molecules: Mole-to-Mole Conversions
- 8.4 Making Molecules: Mass-to-Mass Conversions
- 8.5 More Pancakes: Limiting Reactant, Theoretical Yield, and Percent Yield
- 8.6 Limiting Reactant[JJ2] , Theoretical Yield, and Percent Yield from Initial Masses of Reactants
- 8.7 Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction
- Electrons in Atoms and the Periodic Table
- 9.1 Blimps, Balloons, and Models of the Atom
- 9.2 Light: Electromagnetic Radiation
- 9.3 The Electromagnetic Spectrum
- 9.4 The Bohr Model: Atoms with Orbits
- 9.5 The Quantum-Mechanical Model: Atoms with Orbitals
- 9.6 Quantum-Mechanical Orbitals and Electron Configurations
- 9.7 Electron Configurations and the Periodic Table
- 9.8 The Explanatory Power of the Quantum-Mechanical Model
- 9.9 Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
- Chemical Bonding
- 10.1 Bonding Models and AIDS Drugs
- 10.2 Representing Valence Electrons with Dots
- 10.3 Lewis Structures of Ionic Compounds: Electrons Transferred
- 10.4 Covalent Lewis Structures: Electrons Shared
- 10.5 Writing Lewis Structures for Covalent Compounds
- 10.6 Resonance: Equivalent Lewis Structures for the Same Molecule
- 10.7 Predicting the Shapes of Molecules
- 10.8 Electronegativity and Polarity: Why Oil and Water Don’t Mix
- Gases
- 11.1 Extra-Long Straws
- 11.2 Kinetic Molecular Theory: A Model for Gases
- 11.3 Pressure: The Result of Constant Molecular Collisions
- 11.4 Boyle’s Law: Pressure and Volume
- 11.5 Charles’s Law: Volume and Temperature
- 11.6 The Combined Gas Law: Pressure, Volume, and Temperature
- 11.7 Avogadro’s Law: Volume and Moles
- 11.8 The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
- 11.9 Mixtures of Gases
- 11.10 Gases in Chemical Reactions
- Liquids, Solids, and Intermolecular Forces
- 12.1 Spherical Water
- 12.2 Properties of Liquids and Solids
- 12.3 Intermolecular Forces in Action: Surface Tension and Viscosity
- 12.4 Evaporation and Condensation
- 12.5 Melting, Freezing, and Sublimation
- 12.6 Types of Intermolecular Forces: Dispersion, Dipole—Dipole, Hydrogen Bonding, and Ion—Dipole
- 12.7 Types of Crystalline Solids: Molecular, Ionic, and Atomic
- 12.8 Water: A Remarkable Molecule
- Solutions
- 13.1 Tragedy in Cameroon
- 13.2 Solutions: Homogeneous Mixtures
- 13.3 Solutions of Solids Dissolved in Water: How to Make Rock Candy
- 13.4 Solutions of Gases in Water: How Soda Pop Gets Its Fizz
- 13.5 Specifying Solution Concentration: Mass Percent
- 13.6 Specifying Solution Concentration: Molarity
- 13.7 Solution Dilution
- 13.8 Solution Stoichiometry
- 13.9 Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter
- 13.10 Osmosis: Why Drinking Saltwater Causes Dehydration
- Acids and Bases
- 14.1 Sour Patch Kids and International Spy Movies
- 14.2 Acids: Properties and Examples
- 14.3 Bases: Properties and Examples
- 14.4 Molecular Definitions of Acids and Bases
- 14.5 Reactions of Acids and Bases
- 14.6 Acid—Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution
- 14.7 Strong and Weak Acids and Bases
- 14.8 Water: Acid and Base in One
- 14.9 The pH and pOH Scales: Ways to Express Acidity and Basicity
- 14.10 Buffers: Solutions That Resist pH Change
- Chemical Equilibrium
- 15.1 Life: Controlled Disequilibrium
- 15.2 The Rate of a Chemical Reaction
- 15.3 The Idea of Dynamic Chemical Equilibrium
- 15.4 The Equilibrium Constant: A Measure of How Far a Reaction Goes
- 15.5 Heterogeneous Equilibria: The Equilibrium Expression for Reactions Involving a Solid or a Liquid
- 15.6 Calculating and Using Equilibrium Constants
- 15.7 Disturbing a Reaction at Equilibrium: Le Châtelier’s Principle
- 15.8 The Effect of a Concentration Change on Equilibrium
- 15.9 The Effect of a Volume Change on Equilibrium
- 15.10 The Effect of a Temperature Change on Equilibrium
- 15.11 The Solubility-Product Constant
- 15.12 The Path of a Reaction and the Effect of a Catalyst
- Oxidation and Reduction
- 16.1 The End of the Internal Combustion Engine?
- 16.2 Oxidation and Reduction: Some Definitions
- 16.3 Oxidation States: Electron Bookkeeping
- 16.4 Balancing Redox Equations
- 16.5 The Activity Series: Predicting Spontaneous Redox Reactions[JJ3]
- 16.6 Batteries: Using Chemistry to Generate Electricity
- 16.7 Electrolysis: Using Electricity to Do Chemistry
- 16.8 Corrosion: Undesirable Redox Reactions
- Radioactivity and Nuclear Chemistry
- 17.1 Diagnosing Appendicitis
- 17.2 The Discovery of Radioactivity
- 17.3 Types of Radioactivity: Alpha, Beta, and Gamma Decay
- 17.4 Detecting Radioactivity
- 17.5 Natural Radioactivity and Half-Life
- 17.6 Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Other Artifacts
- 17.7 The Discovery of Fission and the Atomic Bomb
- 17.8 Nuclear Power: Using Fission to Generate Electricity
- 17.9 Nuclear Fusion: The Power of the Sun
- 17.10 The Effects of Radiation on Life
- 17.11 Radioactivity in Medicine
- Organic Chemistry
- 18.1 What Do I Smell?
- 18.2 Vitalism: The Difference between Organic and Inorganic
- 18.3 Carbon: A Versatile Atom
- 18.4 Hydrocarbons: Compounds Containing Only Carbon and Hydrogen
- 18.5 Alkanes: Saturated Hydrocarbons
- 18.6 Isomers: Same Formula, Different Structure
- 18.7 Naming Alkanes
- 18.8 Alkenes and Alkynes
- 18.9 Hydrocarbon Reactions
- 18.10 Aromatic Hydrocarbons
- 18.11 Functional Groups
- 18.12 Alcohols
- 18.13 Ethers
- 18.14 Aldehydes and Ketones
- 18.15 Carboxylic Acids and Esters
- 18.16 Amines
- 18.17 Polymers
- Biochemistry
- 19.1 The Human Genome Project
- 19.2 The Cell and Its Main Chemical Components
- 19.3 Carbohydrates: Sugar, Starch, and Fiber
- 19.4 Lipids
- 19.5 Proteins
- 19.6 Protein Structure
- 19.7 Nucleic Acids: Molecular Blueprints
- 19.8 DNA Structure, DNA Replication, and Protein Synthesis
