Introduction to Chemistry

PrefaceIntroduction 1.1 General and Historical 1.2 Definitions of Some Chemical Terms 1.3 The Purity of Compounds 1.4 Chemical Symbols, Formulas, and Equations2 Electronic Structures of Atoms 2.1 Introduction 2.2 Quantization of Electricity 2.3 The Positive Ions (Positive Rays) 2.4 The Rutherford-Bohr Nuclear Theory of the Atom 2.5 The Nature of Light 2.6 Spectra of Elements 2.7 Quantization of the Energy of an Electron Associated with a Nucleus 2.8 Modification of the Bohr Theory 2.9 The Electron-How Shall We Think About It? 2.10 The Distribution of Electrons in Quantum Levels 2.11 The Energies of the Quantum Levels 2.12 Electron Spin 2.13 Aufbau 2.14 What Do The Quantum Numbers Represent? 2.15 Representations of the Shapes of Atomic Orbitals 2.16 Paramagnetism3 Chemical Periodicity 3.1 Formulas and Valence 3.2 Nomenclature 3.3 Chemical Periodicity before Mendeleev 3.4 Mendeleev; Meyer 3.5 The Periodic Law and the Periodic Table. Types of Elements 3.6 The Periodicity of Chemical Properties 3.7 Atomic Structure and Periodic Properties of Atoms4 Atomic and Molecular Weights. The Mole 4.1 The Law of Conservation of Matter 4.2 The Law of Definite Proportions 4.3 The Atomic Theory 4.4 The Law of Combining Volumes; The Avogadro Hypothesis 4.5 Approximate Molecular Weights of Gases. The Mole 4.6 Atomic Weights from Molecular Weights; The Cannizzaro Method 4.7 Molecular Formulas 4.8 Empirical Formulas; Ionic Solids 4.9 Mass Spectroscopy; Isotopes; Accurate Atomic Weights5 Stoichiometry-The Arithmetic of Chemistry 5.1 Chemical Equations 5.2 Quantitative information from Chemical Equations 5.3 Conversion and Selectivity (Yield)6 The First Law of Thermodynamics; Thermochemistry 6.1 Conservation of Energy 6.2 The First Law of Thermodynamics 6.3 Thermochemistry 6.4 Hess's Law 6.5 Bond Dissociation Energy 6.6 The Interconvertibility of Matter and Energy7 Types of Chemical Bonds 7.1 Introduction 7.2 What Type of Attractive Forces Hold Atoms Together in Chemical Bonds? 7.3 Lewis Symbols 7.4 The Ionic Bond 7.5 The Covalent Bond 7.6 The Multiple Bonds 7.7 Properties of Ionic and Covalent Compounds 7.8 Polar Covalent Bonds; Electronegativity 7.9 Exceptions to the Octet Rule 7.10 Formal Charge and Oxidation Number 7.11 Periodicity of Chemical Bonding8 The Covalent Bond 8.1 The Molecular Orbital 8.2 Sigma (s) Bonds and P1 (p) Bonds 8.3 Binary Covalent Molecules and Ions 8.4 Hybridization of Atomic Orbitals 8.5 Multiply Bonded Molecules 8.6 Hybrid Orbital Number 8.7 Relative Energy Levels of the s-p Type of Hybrid Orbital 8.8 Resonance and Delocalized p Electrons9 The Shapes and Symmetry of Molecules 9.1 Introduction 9.2 Hybridization of Orbitals of Atoms with more than an Octet of Valence Electrons 9.3 Principal Factors Determining Molecular Shape 9.4 Principal Effect of a Lone Pair of Electrons 9.5 Molecules whose Central Atoms use Unhybridized p Orbitals 9.6 Shapes of Multiple-Bonded Molecules 9.7 Molecular Symmetry 9.8 Molecular Dissymmetry10 Intermolecular Forces 10.1 Introduction 10.2 Dipole-Dipole Interaction 10.3 Ion-Dipole Attractions 10.4 Hydrogen Bonding 10.5 London Forces 10.6 London Forces and Molecular Shape11 Gases 11.1 The States of Aggregation of Molecules in Matter 11.2 The Properties of Gases 11.3 Boyle's Law 11.4 The Law of Charles and Gay-Lussac; Absolute Temperature 11.5 Avogadro's Law 11.6 The Gas Law; The Mole; Gas Densities 11.7 Dalton's Law of Partial Pressures 11.8 The Pressure of a Gas Confined by a Liquid 11.9 Gas Volume Corrections in Stoichiometry 11.10 Ideal Gases. The Kinetic Molecular Hypothesis 11.