Introductory Chemistry Essentials plus Pearson Mastering Chemistry with Pearson eText, Global Edition

Table of Contents:
1 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 2 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 3 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 4 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 5 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 6 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 7 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 8 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: