TY - BOOK AU - Silberberg,Martin S. TI - Chemistry: the molecular nature of matter and change SN - 9780697395979 U1 - 540 21 PY - 2000/// CY - Boston PB - McGraw-Hill KW - Chemistry N1 - Contents; Chapter 1. Keys to the study of chemistry 1.1 Some fundamental definitions 1.2 Chemical arts and the origins of modern chemistry 1.3 The scientific approach: Developing a model 1.4 Chemistry problem solving 1.5 Measurement in scientific study etc. Chapter 2. The components of matter 2.1 Elements, compounds and mixtures: An atomic overview 2.2 The observation that led to an atomic view of matter 2.3 Dalton's Atomic theory 2.4 The observations that led to the nuclear Atom model 2.5 The Atomic theory today etc. Chapter 3. Stoichiometry: Mole-mass-number relationships in chemical systems 3.1 The mole 3.2 Determining the formula of the unknown compound 3.3 Writing and balancing chemical equations 3.4 Calculating amounts of reactant and product 3.5 Fundamentals of solution stoichiometry Chapter 4. The major classes of chemical reactions 4.1 The role of water as a solvent 4.2 Writing equations for aqueous ionic reactions 4.3 Precipitation reactions 4.4 Acid-base reactions 4.5 Oxidation-reduction ( redox) reactions Chapter 5. Gases and the kinetic-molecular theory 5.1 An overview of th physical states of matter 5.2 Gas pressure and its measurement 5.3 The gas laws and their experimental foundations 5.4 Further applications of the ideal gas law 5.5 The ideal gas law and reactions stoichiometry etc. Chapter 6. Thermochemistry: Energy flow and chemical change 6.1 Forms of energy and their interconversion 6.2 Enthalpy: Heats of reaction and chemical change 6.3 Calorimetry:Laboratory measurement of heats of reactions 6.4 Stoichiometry of thermochemical equations 6.5 Hess's law of heat summation etc. Chapter 7. Quantum theory and atomic structure 7.1 The nature of light 7.2 Atomic spectra 7.3 The wave-particle duality of matter and energy 7.4 The quantum-mechanical model of the atom Chapter 8. Electron configuration and chemical periodicity 8.1 Development of the periodic table 8.2 Characteristics of many-electron atoms 8.3 The quantum-mechanical model and the periodic table 8.4 Trends in some key periodic atomic properties 8.5 The connection between atomic structure and chemical reactivity Chapter 9. Models of chemical bonding 9.1 Atomic properties and chemical bonds 9.2 The ionic bonding model 9.3 The covalent bonding model 9.4 Between the extremes: Electronegativity and bond polarity 9.5 An introduction to metallic bonding Chapter 10. The shapes of molecules 10.1 Depicting molecules and ions with Lewis structure 10.2 Using Lewis structures and bond energies to calculate heats of reaction 10.3 Valence-shell electron-pair repulsion (VSEPR) theory and molecular shape 10.4 Molecular shape and molecular polarity etc. Chapter 11. Theories of covalent bonding 11.1 Valence bond (VB) theory and orbital hybridization 11.2 The mode of orbital overlap and the types of covalent bonds 11.3 Molecular orbital (MO) theory and electron delocalization Chapter 12 Intermolecular forces:Liquids,solids and phase changes 12.1 An overview of physical states and phase changes 12.2 Quantitative aspects of phase changes 12.3 Types of intermolecular forces 12.4 Properties of the liquid state etc. Chapter 13. The properties of mixtures: solutions and colloids 13.1 Types of solutions: intermolecular forces and predicting solubility 13.2 Energy changes in the solution process 13.3 Solubility as an equilibrium process 13.4 Quantitative ways of expressing concentration etc. Chapter 14. Periodic patterns in the main- group elements:Bonding,structure, and reactivity 14.1 Hydrogen, the simplest atom 14.2 Trends across the periodic table: The period elements 14.3 Group 1A (1): The alkali metals 14.4 Group 1A (2):The alkaline earth metals etc. Chapter 15. Organic compounds and the atomic properties of carbon 15.1 The special nature of carbon and the characteristics of organic molecules 15.2 The structures and classes of hydrocarbons 15.3 Some important classes of organic reactions 15.4 Properties and reactivities of common functional groups Chapter 16. Kinetics: Rates and Mechanisms of Chemical Reactions 16.1 Factors That Influence Reaction Rate 16.2 Expressing the Reaction Rate 16.3 The Rate Law and Its Components Tools of the Laboratory: Measuring Reaction Rates Determining the Initial Rate Reaction Order Terminology Determining Reaction Orders Determining the Rate Constant 16.4 Integrated Rate Laws: Concentration Changes over Time Integrated Rate Laws for First-, Second-, and Zero-Order Reactions Determining the Reaction Order from the Integrated Rate Law Reaction Half-Life etc. Chapter 17. Equilibrium: The Extent of Chemical Reactions 17.1 The Dynamic Nature of the Equilibrium State 17.2 The Reaction Quotient and the Equilibrium Constant Writing the Reaction Quotient Variations in the Form of the Reaction Quotient 17.3 Expressing Equilibria with Pressure Terms: Relation Between Kc and Kp 17.4 Reaction Direction: Comparing Q and K etc. Chapter 18. Acid-Base Equilibria 18.1 Acids and Bases in Water Release of H+ or OH- and the Classical Acid-Base Definition Variation in Acid Strength: The Acid-Dissociation Constant (Ka) Classifying the Relative Strengths of Acids and Bases 18.2 Autoionization of Water and the pH Scale The Equilibrium Nature of Autoionization: The Ion-Product Constant for Water (Kw) Expressing the Hydronium Ion Concentration: The pH Scale 18.3 Proton Transfer and the Bronsted-Lowry Acid-Base Definition The Conjugate Acid-Base PairRelative Acid-Base Strength and the Net Direction of Reaction 18.4 Solving Problems Involving Weak-Acid Equilibria Finding Ka Given a Concentration Finding Concentration Given Ka The Effect of Concentration on the Extent of Acid Dissociation The Behavior of Polyprotic Acids etc Chapter 19. Ionic Equilibria in Aqueous Systems 19.1 Equilibria of Acid-Base Buffer Systems How a Buffer Works: The Common-Ion Effect The Henderson-Hasselbalch Equation Buffer Capacity and Buffer Range Preparing a Buffer 19.2 Acid-Base Titration Curves Monitoring pH with Acid-Base Indicators Strong Acid-Strong Base Titration Curves Weak Acid-Strong Base Titration Curves Weak Base-Strong Acid Titration Curves Titration Curves for Polyprotic Acids Amino Acids as Biological Polyprotic Acids 19.3 Equilibria of Slightly Soluble Ionic Compounds The Ion-Product Expression (Qsp) and the Solubility-Product Constant (Ksp) Calculations Involving the Solubility-Product Constant The Effect of a Common Ion on Soubility The Effect of pH on Solubility Chemical Connections to Geology: Creation of a Limestone Cave Predicting the Formation of a Precipitate: Qsp vs. Ksp Chemical Connections to Environmental Science: The Acid-Rain Problem 19.4 Equilibria Involving Complex Ions Formation of Complex Ions Complex Ions and the Solubility of Precipitates Complex Ions of Amphoteric Hydroxides etc. Chapter 20. Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions Chapter 21. Eletrochemistry : Chemical Change and Electrical Work Chapter 22.The Elements in Nature and Industry Chapter 23. The Transition Elements and their Coordination Compounds Chapter 24. Nuclear Reactions and their Applications ; Includes bibliographical references and index ER -