Chemistry : the molecular nature of matter and change / Martin Silberberg ; consultants, Randy Duran . . . [et al.].

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