Preface for Teachers
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1. Student Audience and Preparedness
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2. Our Emphasis on Mastery, Integration, and Wonder
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3. Recommendations for Teaching With This Text
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4. Laboratory Work and Lab Reports
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Preface for Students
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Introduction: What is Chemistry All About?
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I.1 A Few Major Themes
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I.1.1 Chemistry Is All About Electrons
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I.1.2 Chemistry Is All About Electrical Forces
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| Hmm… Interesting. Why water forms beads |
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I.1.3 Chemistry Is All About Minimizing Energy
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I.1.4 Chemistry Is All About Whole Number Ratios of Atoms
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I.1.5 Chemistry Is All About Modeling
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I.2 Conclusion
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Chapter 1: Measurements
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1.1 Science and Measurements
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1.1.1 No Measurements, No Science
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1.1.2 Matter, Volume, and Mass
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1.1.3 The US Customary System
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1.1.4 The SI Unit System
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1.1.5 Metric Prefixes
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1.2 Converting Units of Measure
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1.2.1 Basic Principles of Unit Conversion Factors
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1.2.2 Tips for Converting Units of Measure
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1.2.3 Converting Temperature Units
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1.3 Accuracy and Precision
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1.3.1 Distinguishing Between Accuracy and Precision
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1.3.2 Significant Digits
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1.4 Other Important Math Skills
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1.4.1 Scientific Notation
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1.4.2 Calculating Percent Difference
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Chapter 2: Atoms and Substances
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2.1 Atoms and Molecules
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2.1.1 Atomic Facts
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2.1.2 The History of Atomic Models
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2.2 Types of Substances
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2.2.1 Pure Substances: Elements and Compounds
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2.2.2 Mixtures
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| Hmm… Interesting. Bownian motion |
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2.2.3 Physical and Chemical Properties
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2.3 Isotopes and Atomic Masses
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2.3.1 Isotopes
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2.3.2 The Unifies Atomic Mass Unit
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2.3.3 Atomic Masses
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2.3 Density and Quantity of Substances
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2.4.1 Density
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2.4.2 The Mole and the Avogadro Constant
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2.4.3 Molar Mass and Formula Mass
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2.4.4 Gram Masses of Atoms and Molecules
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Chapter 3: Atomic Structure
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3.1 Atomic Spectra
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3.1.1 The Electromagnetic Spectrum
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3.1.2 Energy in Atoms
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| Hmm… Interesting. Neon Signs and Photons |
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3.1.3 The Hydrogen Atom
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3.2 The Bohr Model of the Atom
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3.3 The Quantum Model of the Atom
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3.3.1 Schrödinger and Pauli
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3.3.2 Shells, Subshells, and Orbitals
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3.3.3 The Aufbau Priciple, the Madelung Rule, and Hund’s Rule
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3.4 Electron Configurations
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3.4.1 Electron Configurations and Orbital Diagrams
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3.4.2 Condensed Electron Configurations
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3.5 Empirical Formulas
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3.5.1 Percent Composition and Empirical Formulas
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3.5.2 Determining a Molecular Formula from an Empirical Formula
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Chapter 4: The Periodic Law
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4.1 The Periodic Table of The Elements
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4.2 Periodic Table Nomenclature
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4.3 Periodic Physical Properties
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4.3.1 Atomic Radius and Bonding Atomic Radius
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4.3.2 Ionic Radius
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4.4 Periodic Chemical properties
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4.4.1 Core and Valence Electrons
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4.4.2 Ionization Energy
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4.4.3 Electron Affinity
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4.4.4 Electronegativity
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4.5 A Few Notes About Hydrogen
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| Hmm… Interesting. Hydrogen in space |
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Chapter 5: Chemical Bonding
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5.1 Preliminaries
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5.1.1 Chemical Possibilities
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5.1.2 The Octet Rule
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5.2 Ionic Bonding
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5.2.1 Ionic Bonds and Crystals
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5.2.2 Naming Ionic Compounds
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5.2.3 Energy in Ionic Bonds
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5.2.4 Hydrates
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5.2.5 Intensive and Extensive Properties
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5.2.6 Physical Properties of Ionically Bonded Substances
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5.3 Covalent Bonding
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5.3.1 Covalent Bonds and Molecules
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5.3.2 Polyatomic Ions
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5.3.3 Ionic Compounds With Polyatomic Ions
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5.3.4 Polyatomic Ion Names
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5.3.5 Naming Acids
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5.3.6 Lewis Structures
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5.3.7 Exceptions to The Octet Rule
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5.3.8 Resonance Structures
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5.3.9 Naming Binary Covalent Compounds
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5.3.10 Energy in Covalent Bonds
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5.3.11 Physical Properties of Covalently Bonded Substances
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5.4 Electronegativity, Polarity, and Bond Character
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5.4.1 Polarity and Dipoles
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5.4.2 The Nature of The Bond
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| Hmm… Interesting. The molecular structure of glass and quartz |
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Chapter 6: Molecular Theory and Metallic Bonding
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6.1 Molecular Structure
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6.1.1 Covalent Bond Theory
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6.1.2 Valence Shell Electron Pair Repulsion (VSEPR) Theory
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6.1.3 The Effect of Nonbonding Domains on Bond Angle
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6.2 Metallic Bonding
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6.2.1 Metallic Lattices
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6.2.2 Physical Properties of Metals
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6.3 Intermolecular Forces
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6.3.1 Bonding Forces
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6.3.2 Intermolecular Forces
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6.3.3 Hydrogen Bonding
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| Hmm… Interesting. Tin pest |
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6.3.4 Van Der Waals Forces
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Chapter 7: Chemical Reactions and Stoichiometry
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7.1 Introduction to Chemical Equations
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7.1.1 Fascinating Chemistry
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7.1.2 The Law of Conservation of Mass in Chemical Reactions
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7.1.3 Reaction Notation
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7.1.4 Balancing Chemical Equations
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7.1.5 Oxidation States
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| Hmm… Interesting. Why nitrates and nitros blow up |
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7.2 General Types of Chemical Reactions
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7.2.1 Synthesis Reactions
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7.2.2 Decomposition Reactions
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7.2.3 The Activity Series of Metals
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7.2.4 Single Replacement Reactions
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7.2.5 Double Replacement Reactions
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| Hmm… Interesting. A story about aqua regia |
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7.2.6 Combustion Reactions
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7.2.7 Acid-Base Reactions
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7.2.8 Oxidation-Reduction Reactions
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7.3 Stoichiometry
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7.3.1 Stoichiometric Calculations
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7.3.2 Limiting Reactant
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7.3.3 Theoretical Yield and Percent Yield
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Chapter 8: Kinetic Theory and States of Matter
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8.1 Temperature, Kinetic-Molecular Theory, and Pressure
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8.1.1 Temperature and Molecular Energy
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8.1.2 Velocity Distribution of Gases
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8.1.3 The Kinetic-Molecular Theory of Gases
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8.1.4 Gas Pressure
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8.2 States of Matter
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8.2.1 The Four Basic States of Matter
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| Hmm… Interesting. How barometers work |
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8.2.2 Solids
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8.2.3 Liquids
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8.2.4 Gases
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| Hmm… Interesting. Gas diffusion |
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8.2.5 Plasmas
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8.2.6 Phase Transitions and Phase Diagrams
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8.2.7 Heat Capacity, Heat of Fusion, and Heat of Vaporization
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8.2.8 Evaporation
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8.2.9 Vapor Pressure
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Chapter 9: The Gas Laws
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9.1 Early Formulations of The Gas Laws
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9.1.1 Boyle’s Law
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9.1.3 Avogadro’s Law
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9.2 The Ideal Gas Law
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9.2.1 Standard Temperature and Pressure
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9.2.2 The Ideal Gas Law
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| Hmm… Interesting. The gas laws as models |
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9.2.3 Using The Ideal Gas Law to Find Molar Mass and Density
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9.3 The Law of Partial Pressures
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9.3.1 Dalton’s Law of Partial Pressures
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9.3.2 Collecting A Gas Over Water
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9.4 Stoichiometry of Gases and Effusion
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9.4.1 Stoichiometry of Gases
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9.4.2 Gas Diffusion and Effusion
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| Hmm… Interesting. Uranium enrichment |
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Chapter 10: Solution Chemistry
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10.1 Dissolution
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10.1.1 The Process of Dissolving
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10.1.2 Enthalpy of Solution
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10.1.3 Entropy and Free Energy
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10.1.4 Electrolytes
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10.2 Solubility
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10.2.1 Ionic Solids in Water
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10.2.2 Ionic Solids in Nonpolar Solvents
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10.2.3 Polar Liquids
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10.2.4 Nonpolar Liquids
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10.2.5 Solutions of Solids
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10.2.6 Gases in Liquid Solutions
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10.2.7 The Effect of Temperature on Solubility
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10.3 Quantifying Solution Concentration
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10.3.1 Molarity
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| Hmm… Interesting. How soap works |
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10.3.2 Molality
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10.4 Compounds in Aqueous Solution
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10.4.1 Ionic Equations and Precipitates
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10.4.2 Net Ionic Equations and Spectator Ions
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10.5 Colligative Properties of Solutions
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10.5.1 Vapor Pressure Lowering
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10.5.2 Freezing Point Depression and Boiling Point Elevation
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Chapter 11 Acids and Bases
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11.1 Properties and Nomenclature of Acids and Bases
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11.2 Acid-Base Theories
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11.2.1 Arrhenius Acids and Bases
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11.2.2 Brønsted-Lowry Acids and Bases
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| Hmm… Interesting. What is an alkali? |
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11.2.3 Lewis Acids and Bases
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11.2.4 Strength of Acids and Bases
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11.3 Aqueous Solutions and pH
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11.3.1 The Self-ionization of Water
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11.3.2 Calculating [H3O+] and [OH–]
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11.3.3 pH as a Measure of Ion Concentration and Acidity
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11.3.4 pH Measurement, pH Indicators, and Titration
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11.3.5 Titration Procedure
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11.3.6 Determining [H3O+] or [OH–] from Titration Data
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Chapter 12: Redox Chemistry
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12.1 Oxidation and Reduction
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12.1.1 Introduction to Redox Reactions
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12.1.2 Oxidation States
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12.1.3 Strengths of Oxidizing and Reducing Agents
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12.2 Redox Reaction Equations
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12.2.1 Redox Half-Reactions
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12.2.2 Balancing Redox Equations
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12.3 Electrochemistry
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12.3.1 Copper and Zinc Redox
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12.3.2 Electricity Instead of Heat
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12.3.3 Electrochemical Cells
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| Hmm… Interesting. How are salt bridges made? |
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12.3.4 Electrode Potentials
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12.3.5 Electrochemical Applications
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Glossary
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Answers to Selected Exercises
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Appendix A: Reference Data
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Appendix B: Scientists to Know About
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References and Citations
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Image Credits
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Index
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Principles of Chemistry is a mastery-learning, integrated, and wonder-inspiring textbook for high school. Rigor and elegance have met.
