Chemistry

Chemistry: The Molecular Nature of Matter, 8th Edition bridges the invisible molecular world with observable chemical phenomena, making the abstract tangible for students at every level. This edition transforms how students understand chemistry by revealing the intimate relationship between atomic structure and the macroscopic properties they can see, touch, and measure in their daily lives. What distinguishes this text is its revolutionary integration of real-world relevance with rigorous scientific thinking. Updated examples connect student experiences directly to chemical principles while aligning with contemporary career paths in environmental science, engineering, biology, pharmaceuticals, and medicine. The result is a learning experience where chemistry becomes not just understandable, but personally meaningful and professionally relevant. The 8th edition's strategic focus on problem-solving mastery ensures students don't just memorize—they develop the analytical thinking skills that define scientific success. Problems progress systematically from confidence-building basics to complex applications, creating a scaffold for deep understanding and long-term retention.

0 A Very Brief History of Chemistry 1 0.1 Chemistry's Important Concepts 2 0.2 Stars, Supernovas, and the Elements 3 0.3 Elements and the Earth 6 0.4 Dalton's Atomic Theory 8 0.5 Internal Structure of the Atom 9 1 Scientific Measurements 27 1.1 Laws and Theories: The Scientific Method 28 1.2 Matter and Its Classifications 30 1.3 Physical and Chemical Properties 34 1.4 Measurement of Physical and Chemical Properties 36 1.5 Making Measurements in the Laboratory 46 1.6 Dimensional Analysis 51 1.7 Density and Specific Gravity 55 2 Elements, Compounds, and the Periodic Table 70 2.1 The Periodic Table 71 2.2 Metals, Nonmetals, and Metalloids 74 2.3 Molecules and Chemical Formulas 77 2.4 Chemical Reactions and Chemical Equations 84 2.5 Ionic Compounds 87 2.6 Nomenclature of Ionic Compounds 94 2.7 Molecular Compounds 98 2.8 Nomenclature of Molecular Compounds 102 3 The Mole and Stoichiometry 115 3.1 The Mole and Avogadro's Constant 116 3.2 The Mole, Formula Mass, and Stoichiometry 122 3.3 Chemical Formula and Percentage Composition 126 3.4 Determining Empirical and Molecular Formulas 128 3.5 Stoichiometry and Chemical Equations 136 3.6 Limiting Reactants 144 3.7 Theoretical Yield and Percentage Yield 148 4 Molecular View of Reactions in Aqueous Solutions 163 4.1 Describing Aqueous Solutions 164 4.2 Electrolytes and Nonelectrolytes 166 4.3 Balanced Equations for Ionic Reactions 168 4.4 Introducing Acids and Bases 172 4.5 Naming Acids and Bases 180 4.6 Double Replacement (Metathesis) Reactions 181 4.7 Molarity 192 4.8 Solution Stoichiometry 198 4.9 Titrations and Chemical Analysis 203 5 Oxidation–Reduction Reactions 219 5.1 Oxidation–Reduction Reactions 220 5.2 Balancing Redox Equations 227 5.3 Acids as Oxidizing Agents 233 5.4 Redox Reactions of Metals 236 5.5 Molecular Oxygen as an Oxidizing Agent 241 5.6 Stoichiometry of Redox Reactions 245 6 Energy and Chemical Change 259 6.1 Energy: The Ability to Do Work 260 6.2 Heat, Temperature, and Internal Energy 263 6.3 Measuring Heat 267 6.4 Energy of Chemical Reactions 272 6.5 Heat, Work, and the First Law of Thermodynamics 274\ 6.6 Heats of Reaction 278 6.7 Thermochemical Equations 284 6.8 Hess's Law 286 6.9 Standard Heats of Reaction 291 7 The Quantum Mechanical Atom 309 7.1 Electromagnetic Radiation 311 7.2 Line Spectra and the Rydberg Equation 319 7.3 The Bohr Theory 322 7.4 The Wave Mechanical Model 324 7.5 Quantum Numbers of Electrons in Atoms 330 7.6 Electron Spin 333 7.7 Energy Levels and Ground State Electron Configurations 334 7.8 Periodic Table and Ground State Electron Configurations 337 7.9 Atomic Orbitals: Shapes and Orientations 343 7.10 Periodic Table and Properties of the Elements 347 8 The Basics of Chemical Bonding 365 8.1 Energy Requirements for Bond Formation 366 8.2 Ionic Bonding 367 8.3 Octet Rule and Electron Configurations of Ions 371 8.4 Lewis Symbols: Keeping Track of Valence Electrons 375 8.5 Covalent Bonds 377 8.6 Bond Polarity and Electronegativity 382 8.7 Lewis Structures 387 8.8 Resonance Structures 398 8.9 Covalent Compounds of Carbon 402 9 Theories of Bonding and Structure 418 9.1 Five Basic Molecular Geometries 420 9.2 Molecular Shapes and the Valence Shell Electron Pair Repulsion (VSEPR) Model 423 9.3 Molecular Structure and Dipole Moments 432 9.4 Valence Bond Theory 436 9.5 Hybrid Orbitals and Molecular Geometry 439 9.6 Hybrid Orbitals and Multiple Bonds 451 9.7 Molecular Orbital Theory Basics 457 9.8 Delocalized Molecular Orbitals 464 9.9 Bonding in Solids 465 9.10 Bonding of the Allotropes of the Elements 467 10 Properties of Gases 483 10.1 A Molecular Look at Gases 484 10.2 Measurement of Pressure 485 10.3 Gas Laws 490 10.4 Stoichiometry Using Gas Volumes 496 10.5 Ideal Gas Law 501 10.6 Dalton's Law of Partial Pressures 509 10.7 Kinetic Molecular Theory of Gases 519 10.8 Real Gases 522 11 Intermolecular Attractions and the Properties of Liquids and Solids 533 11.1 Intermolecular Forces 535 11.2 Intermolecular Forces and Physical Properties 543 11.3 Changes of State and Dynamic Equilibria 549 11.4 Vapor Pressures of Liquids and Solids 551 11.5 Boiling Points of Liquids 553 11.6 Energy and Changes of State 555 11.7 Phase Diagrams 559 11.8 Le Chatelier's Principle and Changes of State 563 11.9 Determining Heats of Vaporization 565 11.10 Structures of Crystalline Solids 567 11.11 Determining the Structure of Solids 575 11.12 Crystal Types and Physical Properties 577 12 Mixtures at the Molecular Level: Properties of Solutions 595 12.1 Intermolecular Forces and the Formation of Solutions 597 12.2 Heats of Solution 600 12.3 Solubility as a Function of Temperature 604 12.4 Henry's Law 606 12.5 Concentration Units 608 12.6 Colligative Properties 615 12.7 Heterogeneous Mixtures 633 13 Chemical Kinetics 647 13.1 Factors that Affect the Rate of Chemical Change 648 13.2 Measuring Reaction Rates 650 13.3 Rate Laws 656 13.4 Integrated Rate Laws 665 13.5 Molecular Basis of Collision Theory 676 13.6 Molecular Basis of Transition State Theory 679 13.7 Activation Energies 682 13.8 Mechanisms of Reactions 687 13.9 Catalysts 694 14 Chemical Equilibrium 713 14.1 Dynamic Equilibrium in Chemical Systems 714 14.2 Equilibrium Laws 717 14.3 Equilibrium Laws Based on Pressures or Concentrations 721 14.4 Equilibrium Laws for Heterogeneous Reactions 725 14.5 Position of Equilibrium and the Equilibrium Constant 726 14.6 Equilibrium and Le Chatelier's Principle 728 14.7 Calculating Equilibrium Constants 733 14.8 Using Equilibrium Constants to Calculate Concentrations 736 15 Acids and Bases: A Molecular Look 759 15.1 Bronsted–Lowry Acids and Bases 760 15.2 Strengths of Bronsted–Lowry Acids and Bases 765 15.3 Periodic Trends in the Strengths of Acids 768 15.4 Lewis Acids and Bases 774 15.5 Acid–Base Properties of Elements and Their Oxides 778 15.6 Advanced Ceramics and Acid–Base Chemistry 781 16 Acid–Base Equilibria in Aqueous Solutions 792 16.1 Water, pH, and "p" Notation 793 16.2 pH of Strong Acid and Base Solutions 798 16.3 Ionization Constants, Ka and Kb 799 16.4 Determining Ka and Kb Values 804 16.5 pH of Weak Acid and Weak Base Solutions 807 16.6 Acid–Base Properties of Salt Solutions 812 16.7 Buffer Solutions 816 16.8 Polyprotic Acids 823 16.9 Acid–Base Titrations 829 17 Solubility and Simultaneous Equilibria 847 17.1 Equilibria in Solutions of Slightly Soluble Salts 848 17.2 Solubility of Basic Salts 860 17.3 Equilibria in Solutions of Metal Oxides and Sulfides 863 17.4 Selective Precipitation 866 17.5 Equilibria Involving Complex Ions 873 17.6 Complexation and Solubility 877 18 Thermodynamics 889 18.1 First Law of Thermodynamics 890 18.2 Spontaneous Change 894 18.3 Entropy 896 18.4 Second Law of Thermodynamics 901 18.5 Third Law of Thermodynamics 905 18.6 Standard Free Energy Change, ΔG° 908 18.7 Maximum Work and ΔG 910 18.8 Free Energy and Equilibrium 914 18.9 Equilibrium Constants and ΔG° 920 18.10 Bond Energies 923 19 Electrochemistry 938 19.1 Galvanic (Voltaic) Cells 939 19.2 Cell Potentials 944 19.3 Utilizing Standard Reduction Potentials 951 19.4 E°cell and ΔG° 956 19.5 Cell Potentials and Concentrations 959 19.6 Electricity 965 19.7 Electrolytic Cells 971 19.8 Electrolysis Stoichiometry 977 19.9 Practical Applications of Electrolysis 981 20 Nuclear Reactions and Their Role in Chemistry 994 20.1 Law of Conservation of Mass–Energy 995 20.2 Nuclear Binding Energy 997 20.3 Radioactivity 999 20.4 Band of Stability 1006 20.5 Transmutation 1009 20.6 Measuring Radioactivity 1012 20.7 Medical and Analytical Applications of Radionuclides 1016 20.8 Nuclear Fission and Fusion 1021 21 Metal Complexes 1037 21.1 Complex Ions 1038 21.2 Metal Complex Nomenclature 1044 21.3 Coordination Number and Structure 1046 21.4 Isomers of Metal Complexes 1049 21.5 Bonding in Metal Complexes 1053 21.6 Biological Functions of Metal Ions 1060 22 Organic Compounds, Polymers, and Biochemicals 1070 22.1 Organic Structures and Functional Groups 1071 22.2 Hydrocarbons: Structure, Nomenclature, and Reactions 1076 22.3 Organic Compounds Containing Oxygen 1084 22.4 Organic Derivatives of Ammonia 1091 22.5 Organic Polymers 1093 22.6 Carbohydrates, Lipids, and Proteins 1100 22.7 Nucleic Acids, DNA and RNA 1109 Tools for Problem Solving 1115 Review Questions and Problems 1117 Appendices Appendix A Review of Mathematics A–1 Appendix B Answers to Practice Exercises and Selected Problems A–6 Appendix C Tables of Selected Data A–30 Glossary G–1 Index I–1