Chapter 1. Keys to the Study of Chemistry
Chapter 2. The Components of Matter
Chapter 3. Stoichiometry of Formulas and Equations
Chapter 4. Three Major Classes of Chemical Reactions
Chapter 5. Gases and the Kinetic-Molecular Theory
Chapter 6. Thermochemistry: Energy Flow and Chemical Change
Chapter 7. Quantum Theory and Atomic Structure
Chapter 8. Electron Configuration and Chemical Periodicity
Chapter 9. Models of Chemical Bonding
Chapter 10. The Shapes of Molecules
Chapter 11. Theories of Covalent Bonding
Chapter 12. Intermolecular Forces: Liquids, Solids, and Phase Changes
Chapter 13. The Properties of Mixtures: Solutions and Colloids
Chapter 14. Periodic Patterns in the Main-Group Elements
Chapter 15. Organic Compounds and the Atomic Properties of Carbon
Chapter 16. Kinetics: Rates and Mechanisms of Chemical Reactions
Chapter 17. Equilibrium: The Extent of Chemical Reactions
Chapter 18. Acid-Base Equilibria
Chapter 19. Ionic Equilibria in Aqueous Systems
Chapter 20. Thermodynamics: Entropy, Free Energy, and the Direction of Chemical
Reactions
Chapter 21. Electrochemistry: Chemical Change and Electrical Work
Chapter 22. The Elements in Nature and Industry
Chapter 23. Transition Elements and Their Coordination Compounds
Chapter 24. Nuclear Reactions and Their Applications


1.1
Some Fundamental Definitions o States of Matter o Properties of Matter and Its Changes o Central Theme in Chemistry o Importance of Energy

1.2
Chemical Arts and the Origins of Modern Chemistry o Prechemical Traditions o Impact of Lavoisier

1.3
The Scientific Approach: Developing a Model

1.4
Measurement and Chemical Problem Solving o Features of SI Units o SI Units in Chemistry o Units and Conversion Factors o Systematic Problem-Solving Approach o Temperature Scales o Extensive and Intensive Properties

1.5
Uncertainty in Measurement: Significant Figures o Determining Significant Digits o Calculations and Rounding Off o Precision, Accuracy, and Instrument Calibration
Concepts and Skills to Review Before You Study This Chapter
1. exponential (scientific) notation (Appendix A)

2.1
Elements, Compounds, and Mixtures: An Atomic Overview

2.2
The Observations That Led to an Atomic View of Matter o Mass Conservation o Definite Composition o Multiple Proportions

2.3
Dalton's Atomic Theory o Postulates of the Theory o Explanation of the Mass Laws

2.4
The Observations That Led to the Nuclear Atom Model o Discovery of the Electron o Discovery of the Nucleus

2.5
The Atomic Theory Today o Structure of the Atom o Atomic Number, Mass Number, and Atomic Symbol o Isotopes o Atomic Masses

2.6
Elements: A First Look at the Periodic Table

2.7
Compounds: Introduction to Bonding o Formation of Ionic Compounds o Formation of Covalent Substances

2.8
Compounds: Formulas, Names, and Masses o Binary Ionic Compounds o Compounds with Polyatomic Ions o Acid Names from Anion Names o Binary Covalent Compounds o Straight-Chain Alkanes o Molecular Masses o Formulas and Models

2.9
Mixtures: Classification and Separation o An Overview of the Components of Matter
Concepts and Skills to Review Before You Study This Chapter
1. physical and chemical change (Section 1.1)
2.
3. states of matter (Section 1.1) attraction and repulsion between charged particles (Section 1.1)

4. meaning of a scientific model (Section 1.3)
5.
6.
SI units and conversion factors (Section 1.4) significant figures in calculations (Section 1.5)
1.

3.1
The Mole o Defining the Mole o Molar Mass o Amount-Mass-Number Conversions o Mass Percent

3.2
Determining the Formula of an Unknown Compound o Empirical Formulas o Molecular Formulas o Formulas and Structures

3.3
Writing and Balancing Chemical Equations

3.4
Calculating Quantities of Reactant and Product o Molar Ratios from Balanced Equations o Reaction Sequences o Limiting Reactants o Reaction Yields
Concepts and Skills to Review Before You Study This Chapter atomic mass (Section 2.5)
2. names and formulas of compounds (Section 2.8)
3. molecular (or formula) mass (Section 2.8)
4. molecular and structural formulas, & ball-and-stick and space-filling models (Section 2.8)

4.1
Solution Concentration and the Role of Water as a Solvent o Polar Nature of Water o Ionic Compounds in Water o Covalent Compounds in Water o Expressing Concentration in Terms of Molarity o Amount-Mass-Number Conversions Involving Solutions o Preparing and Diluting Molar Solutions

4.2
Writing Equations for Aqueous Ionic Reactions

4.3
Precipitation Reactions o The Key Event: Formation of a Solid o Predicting Whether a Precipitate Will Form o Stoichiometry of Precipitation Reactions

4.4
Acid-Base Reactions o The Key Event: Formation of Water o Proton Transfer in Acid-Base Reactions o Stoichiometry of Acid-Base Reactions: Acid-Base Titrations

4.5
Oxidation-Reduction (Redox) Reactions o The Key Event: Movement of Electrons o Redox Terminology o Oxidation Numbers o Stoichiometry of Redox Reactions: Redox Titrations

4.6
Elements in Redox Reactions o Combination Reactions o Decomposition Reactions o Displacement Reactions and Activity Series o Combustion Reactions

4.7
The Reversibility of Reactions and the Equilibrium State
Concepts and Skills to Review Before You Study This Chapter
1. names and formulas of compounds (Section 2.8)

2.
3.
4.
5. nature of ionic and covalent bonding (Section 2.7) amount-mass-number conversions (Section 3.1) balancing chemical equations (Section 3.3) calculating quantities of reactants and products (Section 3.4)

5.1
An Overview of the Physical States of Matter

5.2
Gas Pressure and Its Measurement o Measuring Pressure o Units of Pressure

5.3
The Gas Laws and Their Experimental Foundations o Relationship Between Volume and Pressure: Boyle's Law o Relationship Between Volume and Temperature: Charles's Law o Relationship Between Volume and Amount: Avogadro's Law o Gas Behavior at Standard Conditions o The Ideal Gas Law o Solving Gas Law Problems

5.4
Rearrangements of the Ideal Gas Law o Density of a Gas o Molar Mass of a Gas o Partial Pressure of a Gas o Reaction Stoichiometry

5.5
The Kinetic-Molecular Theory: A Model for Gas Behavior o How the Theory Explains the Gas Laws o Effusion and Diffusion o Mean Free Path and Collision Frequency

5.6
Real Gases: Deviations from Ideal Behavior o Effects of Extreme Conditions o The van der Waals Equation: Adjusting the Ideal Gas Law
Concepts and Skills to Review Before You Study This Chapter
1. physical states of matter (Section 1.1)
2. SI unit conversions (Section 1.4)
3. amount-mass-number conversions (Section 3.1)

6.1
Forms of Energy and Their Interconversion o Defining System and Surroundings o Energy Change (∆ E ) o Heat and Work o Law of Energy Conservation o Units of Energy o State Functions

6.2
Enthalpy: Changes at Constant Pressure o PV Work and the Meaning of Enthalpy o Comparing ∆ E and ∆ H o Exothermic and Endothermic Processes

6.3
Calorimetry: Measuring the Heat of a Chemical or Physical Change o Specific Heat Capacity o The Two Major Types of Calorimetry

6.4
Stoichiometry of Thermochemical Equations

6.5
Hess's Law: Finding ∆ H of Any Reaction

6.6
Standard Enthalpies of Reaction o Formation Equations o Determining from Values
Concepts and Skills to Review Before You Study This Chapter
1.
2. interconverting potential and kinetic energy (Section 1.1) distinction between heat and temperature (Section 1.4)

3.
4.
5.
6. nature of chemical bonding (Section 2.7) calculations of reaction stoichiometry (Section 3.4) properties of the gaseous state (Section 5.1) relation between kinetic energy and temperature (Section 5.5)
2.
3.
4.
5.

7.1
The Nature of Light o Wave Nature of Light o Particle Nature of Light

7.2
Atomic Spectra o Line Spectra and the Rydberg Equation o Bohr Model of the Hydrogen Atom o Energy Levels of the Hydrogen Atom

7.3
The Wave-Particle Duality of Matter and Energy o Wave Nature of Electrons and Particle Nature of Photons o Heisenberg's Uncertainty Principle

7.4
The Quantum-Mechanical Model of the Atom o Atomic Orbital and Probable Location of the Electron o Quantum Numbers of an Orbital o Quantum Numbers and Energy Levels o Shapes of Atomic Orbitals o The Special Case of the H Atom
Concepts and Skills to Review Before You Study This Chapter
1. discovery of the electron and atomic nucleus (Section 2.4)
2. major features of atomic structure (Section 2.5)
3. changes in the energy state of a system (Section 6.1)

8.1
Characteristics of Many-Electron Atoms o The Electron-Spin Quantum Number o The Exclusion Principle o Electrostatic Effects and Energy-Level Splitting

8.2
The Quantum-Mechanical Model and the Periodic Table o Building Up Period 1 o Building Up Period 2 o Building Up Period 3 o Electron Configurations Within Groups o Building Up Period 4 o General Principles of Electron Configurations o Transition and Inner Transition Elements

8.3
Trends in Three Atomic Properties o Atomic Size o Ionization Energy o Electron Affinity

8.4
Atomic Properties and Chemical Reactivity o Trends in Metallic Behavior o Properties of Monatomic Ions
Concepts and Skills to Review Before You Study This Chapter
1. format of the periodic table (Section 2.6) characteristics of metals and nonmetals (Section 2.6) attractions, repulsions, and Coulomb's law (Section 2.7) characteristics of acids and bases (Section 4.4) rules for assigning quantum numbers (Section 7.4)

9.1
Atomic Properties and Chemical Bonds o The Three Ways Elements Combine o Lewis Symbols and the Octet Rule

2.
3.
4.
5.

9.2
The Ionic Bonding Model o Importance of Lattice Energy o Periodic Trends in Lattice Energy o How the Model Explains the Properties of Ionic Compounds

9.3
The Covalent Bonding Model o Formation of a Covalent Bond o Bonding Pairs and Lone Pairs o Bond Order, Energy, and Length o How the Model Explains the Properties of Covalent Substances

9.4
Bond Energy and Chemical Change o Where Does Come From? o Using Bond Energies to Calculate o Bond Strengths and Heat Released from Fuels and Foods

9.5
Between the Extremes: Electronegativity and Bond Polarity o Electronegativity o Bond Polarity and Partial Ionic Character o Gradation in Bonding Across a Period

9.6
An Introduction to Metallic Bonding o The Electron-Sea Model o How the Model Explains the Properties of Metals
Concepts and Skills to Review Before You Study This Chapter
1. characteristics of ionic and covalent substances; Coulomb's law (Section 2.7) polar covalent bonds and the polarity of water (Section 4.1)
Hess's law, , and (Sections 6.5 and 6.6) atomic and ionic electron configurations (Sections 8.2 and 8.4) trends in atomic properties and metallic behavior (Sections 8.3 and 8.4)
3.
4.
5.

10.1
Depicting Molecules and Ions with Lewis Structures o Applying the Octet Rule o Resonance o Formal Charge o Exceptions to the Octet Rule

10.2
Valence-Shell Electron-Pair Repulsion (VSEPR) Theory o Electron-Group Arrangements and Molecular Shapes o Molecular Shape with Two Electron Groups o Molecular Shapes with Three Electron Groups o Molecular Shapes with Four Electron Groups o Molecular Shapes with Five Electron Groups o Molecular Shapes with Six Electron Groups o Using VSEPR Theory to Determine Molecular Shape o Molecular Shapes with More o Than One Central Atom

10.3
Molecular Shape and Molecular Polarity o Bond Polarity, Bond Angle, and Dipole Moment o Molecular Polarity and Behavior
Concepts and Skills to Review Before You Study This Chapter
1.
2. electron configurations of main-group elements (Section 8.2) electron-dot symbols (Section 9.1) octet rule (Section 9.1) bond order, bond length, and bond energy (Section 9.3 and Section 9.4) polar covalent bonds and bond polarity (Section 9.5)

11.1
Valence Bond (VB) Theory and Orbital Hybridization o Central Themes of VB Theory

4.
5.
6.
7. o Types of Hybrid Orbitals

11.2
Modes of Orbital Overlap and the Types of Covalent Bonds o Orbital Overlap in Single and Multiple Bonds o Orbital Overlap and Rotation Within a Molecule

11.3
Molecular Orbital (MO) Theory and Electron Delocalization o Central Themes of MO Theory o Homonuclear Diatomic Molecules of Period 2 Elements o Two Heteronuclear Diatomic Molecules: HF and NO o Two Polyatomic Molecules: Benzene and Ozone
Concepts and Skills to Review Before You Study This Chapter
1.
2.
3. atomic orbital shapes (Section 7.4) exclusion principle (Section 8.1)
Hund's rule (Section 8.2)
Lewis structures (Section 10.1) resonance in covalent bonding (Section 10.1) molecular shapes (Section 10.2) molecular polarity (Section 10.3)

12.1
An Overview of Physical States and Phase Changes

12.2
Quantitative Aspects of Phase Changes o Heat Involved in Phase Changes o Equilibrium Nature of Phase Changes o Phase Diagrams

12.3
Types of Intermolecular Forces o How Close Can Molecules Approach Each Other? o Ion-Dipole Forces o Dipole-Dipole Forces o The Hydrogen Bond o Polarizability and Induced Dipole Forces o Dispersion (London) Forces

12.4
Properties of the Liquid State o Surface Tension o Capillarity o Viscosity

12.5
The Uniqueness of Water o Solvent Properties o Thermal Properties o Surface Properties o Unusual Density of Solid Water

12.6
The Solid State: Structure, Properties, and Bonding o Structural Features o Crystalline Solids o Amorphous Solids o Bonding in Solids: Molecular Orbital Band Theory

12.7
Advanced Materials o Electronic Materials o Liquid Crystals o Ceramic Materials o Polymeric Materials o Nanotechnology
Concepts and Skills to Review Before You Study This Chapter
1. properties of gases, liquids, and solids (Section 5.1)
2.
3. kinetic-molecular theory of gases (Section 5.5) kinetic and potential energy (Section 6.1)

4.
5.
6.
7.
8.
9. enthalpy change, heat capacity, and Hess's law (Sections 6.2, 6.3, and 6.5) diffraction of light (Section 7.1)
Coulomb's law (Section 9.2) chemical bonding models (Chapter 9) molecular polarity (Section 10.3) molecular orbital treatment of diatomic molecules (Section 11.3)

13.1
Types of Solutions: Intermolecular Forces and Solubility o Intermolecular Forces in Solution o Liquid Solutions and Molecular Polarity o Gas and Solid Solutions

13.2
Intermolecular Forces and Biological Macromolecules o Structures of Proteins o Dual Polarity in Soaps, Membranes, and Antibiotics o Structure of DNA

13.3
Why Substances Dissolve: Breaking Down the Solution Process o Heat of Solution and Its Components o Heat of Hydration: Dissolving Ionic Solids in Water o Solution Process and Entropy Change

13.4
Solubility as an Equilibrium Process o Effect of Temperature on Solubility o Effect of Pressure on Solubility

13.5
Concentration Terms o Molarity and Molality o Parts of Solute by Parts of Solution o Interconverting Concentration Terms

13.6
Colligative Properties of Solutions o Nonvolatile Nonelectrolyte Solutions o Using Colligative Properties to Find Solute Molar Mass o Volatile Nonelectrolyte Solutions o Strong Electrolyte Solutions o Applications of Colligative Properties

13.7
Structure and Properties of Colloids
Concepts and Skills to Review Before You Study This Chapter
1. separation of mixtures (Section 2.9)
2.
3.
4.
5. calculations involving mass percent (Section 3.1) and molarity (Section 4.1) electrolytes; water as solvent (Section 4.1 and Section 12.5) mole fraction and Dalton's law (Section 5.4) intermolecular forces and polarizability (Section 12.3)
6. monomers and polymers (Section 12.7)
7. equilibrium nature of phase changes and vapor pressure of liquids; phase diagrams (Section
12.2)

14.1
Hydrogen, the Simplest Atom o Where Hydrogen Fits in the Periodic Table o Highlights of Hydrogen Chemistry

14.2
Trends Across the Periodic Table: The Period 2 Elements

14.3
Group 1A(1): The Alkali Metals o Why the Alkali Metals Are Unusual Physically o Why the Alkali Metals Are So Reactive

14.4
Group 2A(2): The Alkaline Earth Metals o How the Alkaline Earth and Alkali Metals Compare Physically o How the Alkaline Earth and Alkali

o Metals Compare Chemically o Diagonal Relationships: Lithium and Magnesium

14.5
Group 3A(13): The Boron Family o How Transition Elements Influence This Group's Properties o Features That First Appear in This Group's Chemical Properties o Highlights of Boron Chemistry o Diagonal Relationships: Beryllium and Aluminum

14.6
Group 4A(14): The Carbon Family o How Type of Bonding Affects Physical Properties o How Bonding Changes in This Group's Compounds o Highlights of Carbon Chemistry o Highlights of Silicon Chemistry o Diagonal Relationships: Boron and Silicon

14.7
Group 5A(15): The Nitrogen Family o The Wide Range of Physical Behavior o Patterns in Chemical Behavior o Highlights of Nitrogen Chemistry o Highlights of Phosphorus Chemistry

14.8
Group 6A(16): The Oxygen Family o How the Oxygen and Nitrogen Families Compare Physically o How the Oxygen and Nitrogen Families Compare Chemically o Highlights of Oxygen Chemistry o Highlights of Sulfur Chemistry

14.9
Group 7A(17): The Halogens o Physical Behavior of the Halogens o Why the Halogens Are So Reactive o Highlights of Halogen Chemistry

14.10
Group 8A(18): The Noble Gases o How the Noble Gases and Alkali Metals Contrast Physically o How Noble Gases Can Form Compounds
Concepts and Skills to Review Before You Study This Chapter
1. acids, bases, and salts (Section 4.4)
2.
3. redox behavior and oxidation states (Section 4.5) electron configurations (Section 8.2)
6.
7.
8.
4. trends in atomic size, ionization energy, metallic behavior, and electronegativity (Sections 8.3,
8.4, and 9.5)
5. trends in element properties and type of bonding (Sections 8.4 and 9.5) models of ionic, covalent, and metallic bonding (Sections 9.2, 9.3, 9.6, and 12.6) resonance and formal charge (Section 10.1) molecular shape and polarity (Sections 10.2 and 10.3)
9. orbital hybridization and modes of orbital overlap (Sections 11.1 and 11.2)
10. phase changes and phase diagrams, intermolecular forces, and crystalline solids (Sections 12.2,
12.3, and 12.6)

15.1
The Special Nature of Carbon and the Characteristics of Organic Molecules o Structural Complexity of Organic Molecules o Chemical Diversity of Organic Molecules

15.2
The Structures and Classes of Hydrocarbons o Carbon Skeletons and Hydrogen Skins o Alkanes o Dispersion Forces and the Physical Properties of Alkanes o Constitutional Isomerism o Chiral Molecules and Optical Isomerism o Alkenes o Geometric ( Cis-Trans ) Isomerism o Alkynes

o Aromatic Hydrocarbons o Catenated Inorganic Hydrides

15.3
Some Important Classes of Organic Reactions o Types of Organic Reactions o Organic Redox Reactions

15.4
Properties and Reactivities of Common Functional Groups o Groups with Only Single Bonds o Groups with Double Bonds o Groups with Both Single and Double Bonds o Groups with Triple Bonds

15.5
The Monomer-Polymer Theme I: Synthetic Macromolecules o Addition Polymers o Condensation Polymers

15.6
The Monomer-Polymer Theme II: Biological Macromolecules o Sugars and Polysaccharides o Amino Acids and Proteins o Nucleotides and Nucleic Acids
Concepts and Skills to Review Before You Study This Chapter
1.
2.
3. naming straight-chain alkanes (Section 2.8) constitutional isomerism (Section 3.2)
∆EN and bond polarity (Section 9.5)
4.
5. resonance structures (Section 10.1)
VSEPR theory (Section 10.2)
6.
7. orbital hybridization (Section 11.1)
σ and π bonding (Section 11.2)
8. intermolecular forces and synthetic and biological macromolecules (Sections 12.3, 12.7, and
13.2)
9. properties of the Period 2 elements (Section 14.2)
10. properties of the Group 4A(14) elements (Section 14.6)

16.1
Focusing on Reaction Rate

16.2
Expressing the Reaction Rate o Average, Instantaneous, and Initial Rates o Rate and Concentration

16.3
The Rate Law and Its Components o Laboratory Methods for Determining Initial Rate o Determining Reaction Orders o Determining the Rate Constant

16.4
Integrated Rate Laws: Concentration Changes over Time o First-, Second-, and Zero-Order Reactions o Determining Reaction Order o Reaction Half-Life

16.5
Theories of Chemical Kinetics o Collision Theory o Transition State Theory

16.6
Reaction Mechanisms: The Steps from Reactant to Product o Elementary Reactions and Molecularity o The Rate-Determining Step o The Mechanism and the Rate Law

16.7
Catalysis: Speeding Up a Reaction o Basis of Catalytic Action o Homogeneous Catalysis o Heterogeneous Catalysis o Biological Catalysis
Concepts and Skills to Review Before You Study This Chapter

1. influence of temperature on molecular speed and collision frequency (Section 5.5)
4.
5.
6.

17.1
The Equilibrium State and the Equilibrium Constant

17.2
The Reaction Quotient and the Equilibrium Constant o The Changing Value of the Reaction Quotient o Writing the Reaction Quotient ( Q )

17.3
Expressing Equilibria with Pressure Terms: Relation between K c
and K p

17.4
Comparing Q and K to Determine Reaction Direction

17.5
How to Solve Equilibrium Problems o Using Quantities to Find K o Using K to Find Quantities o Problems Involving Mixtures of Reactants and Products

17.6
Reaction Conditions and Equilibrium: Le Châtelier's Principle o Change in Concentration o Change in Pressure (Volume) o Change in Temperature o Lack of Effect of a Catalyst o Synthesis of Ammonia
Concepts and Skills to Review Before You Study This Chapter
1.
2.
3. reversibility of reactions (Section 4.7) equilibrium vapor pressure (Section 12.2) equilibrium nature of a saturated solution (Section 13.4) dependence of rate on concentration (Sections 16.2 and 16.5) rate laws for elementary reactions (Section 16.6) function of a catalyst (Section 16.7)

18.1
Acids and Bases in Water o Arrhenius Acid-Base Definition o Acid-Dissociation Constant ( K a
) o Relative Strengths of Acids and Bases

18.2
Autoionization of Water and the pH Scale o Autoionization and K w o The pH Scale

18.3
Proton Transfer and the Brønsted-Lowry Acid-Base Definition o Conjugate Acid-Base Pairs o Net Direction of Acid-Base Reactions

18.4
Solving Problems Involving Weak-Acid Equilibria o Finding K a
Given Concentrations o Finding Concentrations Given K a o Extent of Acid Dissociation o Polyprotic Acids

18.5
Molecular Properties and Acid Strength o Nonmetal Hydrides o Oxoacids o Hydrated Metal Ions

18.6
Weak Bases and Their Relation to Weak Acids o Ammonia and the Amines o Anions of Weak Acids o Relation Between K a
and K b

18.7
Acid-Base Properties of Salt Solutions o Salts That Yield Neutral Solutions o Salts That Yield Acidic Solutions o Salts That Yield Basic Solutions o Salts of Weakly Acidic Cations and Weakly Basic Anions o Salts of Amphiprotic Anions

18.8
Generalizing the Brønsted-Lowry

2.
3.
4. o Concept: The Leveling Effect

18.9
Electron-Pair Donation and the o Lewis Acid-Base Definition o Molecules as Lewis Acids o Metal Cations as Lewis Acids o Overview of Acid-Base Definitions
Concepts and Skills to Review Before You Study This Chapter
1. role of water as solvent (Section 4.1)
5.
6. writing ionic equations (Section 4.2) acids, bases, and acid-base reactions (Section 4.4) proton transfer in acid-base reactions (Section 4.4) properties of an equilibrium constant (Section 17.2) solving equilibrium problems (Section 17.5)

19.1
Equilibria of Acid-Base Buffers o Common-Ion Effect o Henderson-Hasselbalch Equation o Buffer Capacity and Range o Preparing a Buffer

19.2
Acid-Base Titration Curves o Acid-Base Indicators o Strong Acid –Strong Base Titrations o Weak Acid –Strong Base Titrations o Weak Base –Strong Acid Titrations o Polyprotic Acid Titrations o Amino Acids as Polyprotic Acids

19.3
Equilibria of Slightly Soluble Ionic Compounds o Solubility-Product Constant ( K sp
) o Calculations Involving K sp o Effect of a Common Ion o Effect of pH o Formation of a Limestone Cave o Predicting Precipitate Formation: Q sp
vs. K sp o Selective Precipitation and Simultaneous Equilibria

19.4
Equilibria Involving Complex Ions o Formation of Complex Ions o Complex Ions and Solubility o Amphoteric Hydroxides
Concepts and Skills to Review Before You Study This Chapter
1.
2. solubility rules for ionic compounds (Section 4.3) equilibrium nature of a saturated solution (Section 13.4)
3.
4. effect of concentration on equilibrium position (Section 17.6) conjugate acid-base pairs (Section 18.3)
5.
6. calculations for weak-acid and weak-base equilibria (Sections 18.4 and 18.6) acid-base properties of salt solutions (Section 18.7)
7. Lewis acids and bases (Section 18.9)

20.1
The Second Law of Thermodynamics: Predicting Spontaneous Change o The First Law Does Not Predict Spontaneous Change o The Sign of ∆ H Does Not Predict Spontaneous Change o Freedom of Motion and Dispersal of Kinetic Energy o Entropy and the Number of Microstates o Entropy and the Second Law o Standard Molar Entropies and the Third Law

1.
2.
3.
4.
5. o Predicting Relative S ° of a System

20.2
Calculating the Change in Entropy of a Reaction o Standard Entropy of Reaction o Entropy Changes in the Surroundings o Entropy Change and the Equilibrium State o Spontaneous Exothermic and Endothermic Reactions

20.3
Entropy, Free Energy, and Work o Free Energy Change and Reaction Spontaneity o Standard Free Energy Changes o Free Energy and Work o Temperature and Reaction Spontaneity o Coupling of Reactions

20.4
Free Energy, Equilibrium, and Reaction Direction
Concepts and Skills to Review Before You Study This Chapter
1.
2.
3. internal energy, heat, and work (Section 6.1) state functions (Section 6.1) and standard states (Section 6.6) enthalpy, ∆ H , and Hess's law (Sections 6.2 and 6.5)
4. entropy and solution formation (Section 13.3)
5. comparing Q and K to find reaction direction (Section 17.4)

21.1
Redox Reactions and Electrochemical Cells o Oxidation-Reduction Review o Half-Reaction Method for Balancing Redox Reactions o Electrochemical Cells

21.2
Voltaic Cells: Using Spontaneous Reactions to Generate Electrical Energy o Cell Construction and Operation o Cell Notation o Why Does the Cell Work?

21.3
Cell Potential: Output of a Voltaic Cell o Standard Cell Potential ( ) o Strengths of Oxidizing and Reducing Agents o Writing Spontaneous Redox Reactions o Explaining the Activity Series

21.4
Free Energy and Electrical Work o and the Equilibrium Constant o Effect of Concentration on E cell o Following Changes in E cell o Concentration Cells

21.5
Electrochemical Processes in Batteries o Primary (Nonrechargeable) Batteries o Secondary (Rechargeable) Batteries o Fuel Cells

21.6
Corrosion: An Environmental Voltaic Cell o Corrosion of Iron o Protecting Against Corrosion

21.7
Electrolytic Cells: Using Electrical Energy to Drive Nonspontaneous Reactions o Cell Construction and Operation o Predicting Electrolysis Products o Stoichiometry of Electrolysis
Concepts and Skills to Review Before You Study This Chapter redox terminology (Section 4.5) activity series of the metals (Section 4.6) trends in ionization Energy (Section 8.3) and electronegativity (Section 9.5) free energy, work, and equilibrium (Sections 20.3 and 20.4)
Q vs. K (Section 17.4) and ∆ G vs. ∆ G ° (Section 20.4)

4.
5.
6.
7.
2.
3.
4.
5.

22.1
How the Elements Occur in Nature o Earth's Structure and Elements' Abundance o Sources of the Elements

22.2
The Cycling of Elements Through the Environment o Carbon Cycle o Nitrogen Cycle o Phosphorus Cycle

22.3
Metallurgy: Extracting a Metal from Its Ore o Pretreating the Ore o Converting Mineral to Element o Refining and Alloying

22.4
Tapping the Crust: Isolation and Uses of Selected Elements o Sodium and Potassium o Iron, Copper, and Aluminum o Magnesium o Hydrogen

22.5
Chemical Manufacturing: Two Case Studies o Sulfuric Acid o Chlor-Alkali Process
Concepts and Skills to Review Before You Study This Chapter
1. trends in atomic properties (Sections 8.3, 8.4, 9.2, and 9.5) catalysts and reaction rate (Section 16.7)
Le Châtelier's principle (Section 17.6) acid-base equilibria (Sections 18.3 and 18.4)
6.
7. solubility and complex-ion equilibria (Sections 19.3 and 19.4) temperature and reaction spontaneity (Section 20.3) free energy and equilibrium (Section 20.4)
1.
2.
3.
8. standard electrode potentials (Section 21.3)
9. electrolysis of molten salts and aqueous salt solutions (Section 21.7)

23.1
Properties of the Transition Elements o Electron Configurations o Atomic and Physical Properties o Chemical Properties

23.2
The Inner Transition Elements o The Lanthanides o The Actinides

23.3
Coordination Compounds o Complex Ions o Formulas and Names o Isomerism

23.4
Theoretical Basis for the Bonding and Properties of Complexes o Valence Bond Theory o Crystal Field Theory
Concepts and Skills to Review Before You Study This Chapter properties of light (Section 7.1) electron shielding of nuclear charge (Section 8.1) electron configuration, ionic size, and magnetic behavior (Sections 8.2 to 8.4) valence bond theory (Section 11.1) constitutional, geometric, and optical isomerism (Section 15.2)
Lewis acid-base concepts (Section 18.9) complex-ion formation (Section 19.4)

8. redox behavior and standard electrode potentials (Section 21.3)

24.1
Radioactive Decay and Nuclear Stability o Chemical vs. Nuclear Change o Components of the Nucleus o Types of Radioactive Emissions o Modes of Radioactive Decay; Nuclear Equations o Nuclear Stability and Mode of Decay

24.2
The Kinetics of Radioactive Decay o Detection and Measurement of Radioactivity o Rate of Radioactive Decay o Radioisotopic Dating

24.3
Nuclear Transmutation: Induced Changes in Nuclei o Early Transmutation Experiments; Nuclear Shorthand Notation o Particle Accelerators

24.4
Ionization: Effects of Nuclear Radiation on Matter o Effects of Ionizing Radiation on Living Tissue o Background Sources of Ionizing Radiation o Assessing the Risk from Ionizing Radiation

24.5
Applications of Radioisotopes o Radioactive Tracers o Additional Applications of Ionizing Radiation

24.6
The Interconversion of Mass and Energy o Mass Difference Between a Nucleus and Its Nucleons o Nuclear Binding Energy and Binding Energy per Nucleon

24.7
Applications of Fission and Fusion o Nuclear Fission o Nuclear Fusion
Concepts and Skills to Review Before You Study This Chapter
1. discovery of the atomic nucleus (Section 2.4)
2.
3. protons, neutrons, mass number, and the notation (Section 2.5) half-life and first-order reaction rate (Section 16.4)