Chemistry: The Molecular Nature of Matter and Change / Edition 6

Chemistry: The Molecular Nature of Matter and Change / Edition 6

4.0 3
by Martin Silberberg
     
 

ISBN-10: 0077431375

ISBN-13: 9780077431372

Pub. Date: 01/26/2011

Publisher: McGraw-Hill Higher Education

For five editions, the Silberberg brand has been recognized in the general chemistry market as an unparalleled classic. The sixth edition has been changed in many ways to keep pace with the evolution of student learning. The text still contains unprecedented macroscopic-to-microscopic molecular illustrations, consistent step-by-step worked exercises in every chapter,…  See more details below

Overview

For five editions, the Silberberg brand has been recognized in the general chemistry market as an unparalleled classic. The sixth edition has been changed in many ways to keep pace with the evolution of student learning. The text still contains unprecedented macroscopic-to-microscopic molecular illustrations, consistent step-by-step worked exercises in every chapter, and an extensive range of end-of-chapter problems, which provide engaging applications covering a wide variety of interests, including engineering, medicine, materials, and environmental studies. Changes have been made to the text and applications throughout to make them more succinct, to the artwork to make it more teachable and modern, and to the design to make it more simplistic and open.

Product Details

ISBN-13:
9780077431372
Publisher:
McGraw-Hill Higher Education
Publication date:
01/26/2011
Product dimensions:
8.40(w) x 10.90(h) x 1.40(d)

Table of Contents

Chemistry:

The Molecular Nature of Matter and Change

1 Keys to the Study of Chemistry

1.1 Some Fundamental Definitions

The Properties of Matter
The Three States of Matter
The Central Theme in Chemistry
The Importance of Energy in the Study of Matter

1.2 Chemical Arts and the Origins of Modern Chemistry

Prechemical Traditions
The Phlogiston Fiasco and the Impact of Lavoisier

1.3 The Scientific Approach: Developing a Model

1.4 Chemical Problem Solving

Units and Conversion Factors in Calculations
A Systematic Approach to Solving Chemistry Problems

1.5 Measurement in Scientific Study

General Features of SI Units
Some Important SI Units in Chemistry

1.6 Uncertainty in Measurement: Significant Figures

Determining Which Digits Are Significant
Working with Significant Figures in Calculations
Precision, Accuracy, and Instrument Calibration

Chapter Perspective

Chemical Connections to Interdisciplinary Science:Chemistry Problem Solving in the Real World

For Review and Reference

Problems

2
The Components of Matter

2.1 Elements, Compounds, and Mixtures: An Atomic Overview

2.2 The Observations That Led to an Atomic View of Matter

2.3 Dalton’s Atomic Theory

Postulates of the Atomic Theory
How the Theory Explains the Mass Laws
The Relative Masses of Atoms

2.4 The Observations That Led to the Nuclear Atom Model

Discovery of the Electron and ItsProperties
Discovery of the Atomic Nucleus

2.5 The Atomic Theory Today

Structure of the Atom
Atomic Number, Mass Number, and Atomic Symbol
Isotopes and Atomic Masses of the Elements

Tools of the Laboratory: Mass Spectrometry

A Modern Reassessment of the Atomic Theory

2.6 Elements: A First Look at the Periodic Table

2.7 Compounds: Introduction to Bonding

The Formation of Ionic Compounds
The Formation of Covalent Compounds
The Elements of Life

2.8 Compounds: Formulas, Names, and Masses

Types of Chemical Formulas
Some Advice about Learning Names and Formulas
Names and Formulas of Ionic Compounds
Names and Formulas of Binary Covalent Compounds
An Introduction to Naming Organic Compounds
Molecular Masses from Chemical Formulas

Gallery: Picturing Molecules

2.9 Mixtures: Classification and Separation

Tools of the Laboratory: Basic Separation Techniques

Chapter Perspective

For Review and Reference

Problems

3 Stoichiometry of Formulas and Equations

3.1 The Mole

Defining the Mole
Molar Mass
Interconverting Moles, Mass, and Number of Chemical Entities
Mass Percent from the Chemical Formula

3.2 Determining the Formula of an Unknown Compound

Empirical Formulas
Molecular Formulas
Chemical Formulas and Molecular Structures

3.3 Writing and Balancing Chemical Equations

3.4 Calculating Amounts of Reactant and Product

Stoichiometrically Equivalent Molar Ratios from the Balanced Equation
Chemical Reactions That Occur in a Sequence
Chemical Reactions That Involve a Limiting Reactant
Chemical Reactions in Practice: Theoretical, Actual, and Percent Yields

3.5 Fundamentals of Solution Stoichiometry

Expressing Concentration in Terms of Molarity
Mole-Mass-Number Conversions Involving Solutions
Preparing and Diluting Molar Solutions
Stoichiometry of Chemical Reactions in Solution

Chapter Perspective

For Review and Reference

Problems

4 The Major Classes of Chemical Reactions

4.1 The Role of Water as a Solvent

The Polar Nature of Water
Ionic Compounds in Water
Covalent Compounds in Water

4.2 Writing Equations for Aqueous Ionic Reactions

4.3 Precipitation Reactions

The Key Event: Formation of a Solid from Dissolved Ions
Predicting Whether a Precipitate Will Form

4.4 Acid-Base Reactions

The Key Event: Formation of H2O from H+ and OH–
Acid-Base Titrations
Proton Transfer: A Closer Look at Acid-Base Reactions

4.5 Oxidation-Reduction (Redox) Reactions

The Key Event: Movement of Electrons Between Reactants
Some Essential Redox Terminology
Using Oxidation Numbers to Monitor the Movement of Electron Charge
Balancing Redox Equations
Redox Titrations

4.6 Elements in Redox Reactions

4.7 Reversible Reactions: An Introduction to Chemical Equilibrium

Chapter Perspective

For Review and Reference

Problems

5 Gases and the Kinetic-Molecular Theory

5.1 An Overview of the Physical States of Matter

5.2 Gas Pressure and Its Measurement

Laboratory Devices for Measuring Gas Pressure
Units of Pressure

5.3 The Gas Laws and Their Experimental Foundations

The Relationship Between Volume and Pressure: Boyle’s Law
The Relationship Between Volume and Temperature: Charles’s Law
The Relationship Between Volume and Amount: Avogardro’s Law
Gas Behavior at Standard Conditions

The Ideal Gas
Solving Gas Law Problems

5.4 Further Applications of the Ideal Gas Law

The Density of a Gas
The Molar Mass of a Gas
The Partial Pressure of a Gas in a Mixture of Gases

5.5 The Ideal Gas Law and Reaction Stoichiometry

5.6 The Kinetic-Molecular Theory: A Model for Gas Behavior

How the Kinetic-Molecular Theory Explains the Gas Laws
Effusion and Diffusion
The Chaotic World of Gases: Mean Free Path and Collision Frequency

Chemical Connections to Planetary Science: Structure and Composition of the Earth’s Atmosphere

5.7 Real Gases: Deviations from Ideal Behavior

Chapter Perspective

For Review and Reference

Problems

6 Thermochemistry: Energy Flow and Chemical Change

6.1 Forms of Energy and Their Interconversion

The System and Its Surroundings
Energy Flow to and from a System
Heat and Work: Two Forms of Energy Transfer
The Law of Energy Conservation
Units of Energy
State Functions and the Path Independence of the Energy Change

6.2 Enthalpy: Heats of Reaction and Chemical Change

The Meaning of Enthalpy
Comparing ¿E and ¿H
Exothermic and Endothermic Processes
Some Important Types of Enthalpy Change

6.3 Calorimetry: Laboratory Measurement of Heats of Reaction

Specific Heat Capacity
The Practice of Calorimetry

6.4 Stoichiometry of Thermochemical Equations

6.5 Hess’s Law of Heat Summation

6.6 Standard Heats of Reaction (¿Hrxn0)

Formation Equations and Their Standard Enthalpy Changes
Determining ¿Hrxn0 from ¿Hf0 Values of Reactants and Products

Chemical Connections to Environmental Science: The Future of Energy Use

Chapter Perspective

For Review and Reference

Problems

7 Quantum Theory and Atomic Structure

7.1 The Nature of Light

The Wave Nature of Light
The Particle Nature of Light

7.2 Atomic Spectra

The Bohr Model of the Hydrogen Atom
Limitations of the Bohr Model
The Energy States of the Hydrogen Atom

Tools of the Laboratory: Spectrophotometry in Chemical Analysis

7.3 The Wave-Particle Duality of Matter and Energy

The Wave Nature of Electrons and the Particle Nature of Photons
The Heisenberg Uncertainty Principle

7.4 The Quantum-Mechanical Model of the Atom

The Atomic Orbital and the Probable Location of the Electron
Quantum Numbers of an Atomic Orbital
Shapes of Atomic Orbitals
Energy Levels of the Hydrogen Atom

Chapter Perspective

For Review and Reference

Problems

8 Electron Configuration and Chemical Periodicity

8.1 Development of the Periodic Table

8.2 Characteristics of Many-Electron Atoms

The Electron-Spin Quantum Number
The Exclusion Principle
Electrostatic Effects and the Energy-Level Splitting

8.3 The Quantum-Mechanical Model and the Periodic Table

Building Up Periods 1 and 2
Building Up Period 3
Electron Configurations Within Groups
The First d-Orbital Transition Series: Building Up Period 4
General Principles of Electron Configurations
Unusual Configurations: Transition and Inner Transition Elements

8.4 Trends in Three Key Atomic Properties

Trends in Atomic Size
Trends in Ionization Energy
Trends in Electron Affinity

8.5 Atomic Structure and Chemical Reactivity

Trends in Metallic Behavior
Properties of Monatomic Ions

Chapter Perspective

For Review and Reference

Problems

9
Models of Chemical Bonding

9.1 Atomic Properties and Chemical Bonds

The Three Types of Chemical Bonding
Lewis Electron-Dot Symbols: Depicting Atoms in Chemical Bonding

9.2 The Ionic Bonding Model

Energy Considerations in Ionic Bonding: The Importance of Lattice Energy
Periodic Trends in Lattice Energy
How the Model Explains the Properties of Ionic Compounds

9.3 The Covalent Bonding Model

The Formation of a Covalent Bond
Properties of a Covalent Bond: Bond Energy and Bond Length
How the Model Explains the Properties of Covalent Compounds

Tools of the Laboratory: Infrared Spectroscopy

9.4 Bond Energy and Chemical Change

Changes in Bond Strength: Where Does ¿Hrxn0 Come From?
Using Bond Energies to Calculate ¿Hrxn0
Relative Bond Strengths in Fuels and Foods

9.5 Between the Extremes: Electronegativity and Bond Polarity

Electronegativity
Polar Covalent Bonds and Bond Polarity
The Partial Ionic Character of Polar Covalent Bonds
The Continuum of Bonding Across a Period

9.6 An Introduction to Metallic Bonding

The Electron-Sea Model
How the Model Explains the Properties of Metals

Chapter Perspective

For Review and Reference

Problems

10
The Shapes of Molecules

10.1 Depicting Molecules and Ions with Lewis Structures

Using the Octet Rule to Write Lewis Structures
Resonance: Delocalized Electron-Pair Bonding
Formal Charge: Selecting the Most Important (?) Resonance Structure
Lewis Structures for Exceptions to the Octet Rule

10.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory and Molecular Shape

Electron-Group Arrangements and Molecular Shapes
The Molecular Shape with Two Electron Groups (Linear Arrangement)
Molecular Shapes with Three Electron Groups (Trigonal Planar Arrangement)
Molecular Shapes with Four Electron Groups (Tetrahedral Arrangement)
Molecular Shapes with Five Electron Groups (Trigonal
Bipyramidal Arrangement)
Molecular Shapes with Six Electron Groups (Octahedral Arrangement)
Using VSEPR Theory to Determine Molecular Shape
Molecular Shapes with More Than One Central Atom

Gallery: Molecular Beauty: Odd Shapes with Useful Functions

10.3 Molecular Shape and Molecular Polarity

Bond Polarity, Bond Angle, and Dipole Moment

The Effect of Molecular Polarity on Behavior

Chapter Perspective

Chemical Connections in Sensory Physiology: Molecular Shape, Biological Receptors, and the Sense of Smell

For Review and Reference

Problems

11
Theories of Covalent Bonding

11.1 Valence Bond (VB) Theory and Orbital Hybridization

The Central Themes of VB Theory
Types of Hybrid Orbitals

11.2 The Mode of Orbital Overlap and the Types of Covalent Bonds

Orbital Overlap in Single and Multiple Bonds
Orbital Overlap and Molecular Rotation

11.3 Molecular Orbital (MO) Theory and Electron Delocalization

The Central Themes of MO Theory
Homonuclear Diatomic Molecules of the Period 2 Elements
MO Description of Some Heteronuclear Diatomic Molecules
MO Descriptions of Ozone and Benzene

Chapter Perspective

For Review and Reference

Problems

12 Intermolecular Forces: Liquids, Solids, and Phase Changes

12.1 An Overview of Physical States and Phase Changes

A Kinetic-Molecular View of the Three States
Types of Phase Changes

12.2 Quantitative Aspects of Phase Changes

Heat Involved in Phase Changes: A Kinetic-Molecular Approach
The Equilibrium Nature of Phase Changes
Phase Diagrams: Effect of Pressure and Temperature on Physical State

12.3 Types of Intermolecular Forces

Ion-Dipole Forces
Dipole-Dipole Forces
The Hydrogen Bond
Polarizability and Charge-Induced Dipole Forces
Dispersion (London) Forces

12.4 Properties of the Liquid State

Surface Tension
Capillarity
Viscosity

12.5 The Uniqueness of Water

Gallery: Properties of Liquids

Solvent Properties of Water
Thermal Properties of Water
Surface Properties of Water
The Density of Solid and Liquid Water

12.6 The Solid State: Structure, Properties, and Bonding

Structural Features of Solids

Tools of the Laboratory: X-Ray Diffraction Analysis and Scanning Tunneling Microscopy

Types and Properties of Crystalline Solids
Amorphous Solids
Bonding in Solids: Molecular Orbital Band Theory

12.7 Advanced Materials

Electronic Materials
Liquid Crystals
Ceramic Materials
Polymeric Materials
Nanotechnology: Designing Materials Atom by Atom

Chapter Perspective

For Review and Reference

Problems

13
The Properties of Mixtures: Solutions and Colloids

13.1 Types of Solutions: Intermolecular Forces and Predicting Solubility

Intermolecular Forces in Solution
Liquid Solutions and the Role of Molecular Polarity
Gas Solutions and Solid Solutions

13.2 Intermolecular Forces and Biological Macromolecules

The Structure of Proteins
The Structure of the Cell Membrane (?)
The Structure of DNA
The Structure of Cellulose

13.3 Energy Changes in the Solution Process

Heats of Solution and Solution Cycles
Heats of Hydration: Ionic Solids in Water
The Solution Process and the Change in Entropy

13.4 Solubility as an Equilibrium Process

Effect of Temperature on Solubility
Effect of Pressure on Solubility

13.5 Quantitative Ways of Expressing Concentration

Molarity and Molality
Parts of Solute by Parts of Solution
Converting Units of Concentration

13.6 Colligative Properties of Solutions

Colligative Properties of Nonvolatile Nonelectrolyte Solutions

Gallery: Colligative Properties in Industry and Biology

Using Colligative Properties to Find Solute Molar Mass
Colligative Properties of Volatile Nonelectrolyte Solutions
Colligative Properties of Electrolyte Solutions

13.7 The Structure and Properties of Colloids

Chemical Connections in Sanitary Engineering: Solutions and Colloids in Water Purification

Chapter Perspective

For Review and Reference

Problems

Interchapter: A Perspective on the Properties of the Elements

Topic 1
The Key Atomic Properties

Topic 2
Characteristics of Chemical Bonding

Topic 3
Metallic Behavior

Topic 4
Acid-Base Behavior of the Element Oxides

Topic 5
Redox Behavior of the Elements

Topic 6
Physical States and Changes of State

14
Periodic Patterns in the Main-Group Elements: Bonding, Structure, and Reactivity

14.1 Hydrogen, the Simplest Atom

Where Does Hydrogen Fit in the Periodic Table?
Highlights of Hydrogen Chemistry

14.2 Trends Across the Periodic Table: The Period 2 Elements

14.3 Group 1A(1): The Alkali Metals

Why Are the Alkakli Metals Soft, Low Melting, and Lightweight?
Why Are the Alkali Metals So Reactive?
The Anomalous Behavior of Lithium

14.4 Group 2A(2): The Alkaline Earth Metals

How Do the Physical Properties of the Alkaline Earth and Alkali Metals Compare?
How Do the Chemical Properties of the Alkaline Earth and Alkali Metals Compare?
The Anomalous Behavior of Beryllium
Diagonal Relationships: Lithium and Magnesium
Looking Backward and Forward: Groups 1A(1), 2A(2), and 3A(13)

14.5 Group 3A(13): The Boron Family

How Do the Transition Elements Influence Group 3A(13) Properties?
What New Features Appear in the Chemical Properties of Group 3A(13)?
Highlights of Boron Chemistry
Diagonal Relationships: Beryllium and Aluminum

14.6 Group 4A(14): The Carbon Family

How Does the Bonding in an Element Affect Physical Properties?
How Does the Type of Bonding Change in Group 4A(14) Compounds?
Highlights of Carbon Chemistry
Highlights of Silicon Chemistry
Diagonal Relationships: Boron and Silicon
Looking Backward and Forward: Groups 3A(13), 4A(14), and 5A(15)

Gallery: Silicate Minerals and Silicone Polymers

14.7 Group 5A(15): The Nitrogen Family

What Accounts for the Wide Range of Physical Behavior in Group 5A(15)?
What Patterns Appear in the Chemical Behavior of Group 5A(15)?
Highlights of Nitrogen Chemistry
Highlights of Phosphorus Chemistry: Oxides and Oxoacids

14.8 Group 6A(16): The Oxygen Family

How Do the Oxygen and Nitrogen Families Compare Physically?
How Do the Oxygen and Nitrogen Families Compare Chemically?
Highlights of Oxygen Chemistry: Range of Oxide Properties
Highlights of Sulfur Chemistry: Oxides, Oxoacids, and Sulfides
Looking Backward and Forward: Groups 5A(15), 6A(16), and 7A(17)

14.9 Group 7A(17): The Halogens

What Accounts for the Regular Changes in the Halogens’ Physical Properties?
Why Are the Halogens So Reactive?
Highlights of Halogen Chemistry

14.10 Group 8A(18): The Noble Gases

How Can Noble Gases Form Compounds?
Looking Backward and Forward: Groups 7A(17), 8A(18), and 1A(1)

Chapter Perspective

For Review and Reference

Problems

15
Organic Compounds and the Atomic Properties of Carbon

15.1 The Special Nature of Carbon and the Characteristics of Organic Molecules

The Structural Complexity of Organic Molecules
The Chemical Diversity of Organic Molecules

15.2 The Structures and Classes of Hydrocarbons

Carbon Skeletons and Hydrogen Skins
Alkanes: Hydrocarbons with Only Single Bonds
Constitutional Isomerism and the Physical Properties of Alkanes
Chiral Molecules and Optical Isomerism
Alkenes: Hydrocarbons with Double Bonds

Chemical Connections to Sensory Physiology: Geometric Isomers and the Chemistry of Vision

Alkynes: Hydrocarbons with Triple Bonds
Aromatic Hydrocarbons: Cyclic Molecules with Delocalized ¿ Electrons
Variations on a Theme: Catenated Inorganic Hydrides

Tools of the Laboratory: Nuclear Magnetic Resonance (NMR) Spectroscopy

15.3 Some Important Classes of Organic Reactions

Types of Organic Reactions
The Redox Process in Organic Reactions

15.4 Properties and Reactivities of Common Functional Groups

Functional Groups with Only Single Bonds [?]
Functional Groups with Double Bonds
Functional Groups with Single and Double Bonds
Functional Groups with Triple Bonds

15.5 The Monomer-Polymer Theme I: Synthetic Macromolecules

Addition Polymers
Condensation Polymers

15.6 The Monomer-Polymer Theme II: Biological Macromolecules

Sugars and Polysaccharides
Amino Acids and Proteins
Nucleotides and Nucleic Acids

Chapter Perspective

Chemical Connections to Genetics: DNA Sequencing and the Human Genome Project

For Review and Reference

Problems

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

16.5 The Effect of Temperature on Reaction Rate

16.6 Explaining the Effects of Concentration and Temperature

Collision Theory: Basis of the Rate Law
Transition State Theory: Molecular Nature of the Activated Complex

16.7 Reaction Mechanisms: Steps in the Overall Reaction

Elementary Reactions and Molecularity
The Rate-Determining Step of a Reaction Mechanism
Correlating the Mechanism with the Rate Law

16.8 Catalysis: Speeding Up a Chemical Reaction

Homogeneous Catalysis
Heterogeneous Catalysis

Chemical Connections to Enzymology: Kinetics and Function of Biological Catalysts

Chemical Connections to Atmospheric Science: Depletion of the Earth’s Ozone Layer

Chapter Perspective

For Review and Reference

Problems

7
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

17.5 How to Solve Equilibrium Problems

Using Quantities to Determine the Equilibrium Constant
Using the Equilibrium Constant to Determine Quantities
Mixtures of Reactants and Products: Determining Reaction Direction

17.6 Reaction Conditions and the Equilibrium State: Le Châtelier’s Principle

The Effect of a Change in Concentration
The Effect of a Change in Pressure (Volume)
The Effect of a Change in Temperature
The Lack of Effect of a Catalyst

Chemical Connections to Cellular Metabolism: Design and Control of a Metabolic Pathway

Chemical Connections to Industrial Production: The Haber Process for the Synthesis of Ammonia

Chapter Perspective

For Review and Reference

Problems

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 Brønsted-Lowry Acid-Base Definition

The Conjugate Acid-Base Pair
Relative 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

18.5 Weak Bases and Their Relation to Weak Acids

Molecules as Weak Bases: Ammonia and the Amines
Anions of Weak Acids as Weak Bases
The Relation Between Ka and Kb of a Conjugate Acid-Base Pair

18.6 Molecular Properties and Acid Strength

Trends in Acid Strength of Nonmetal Hydrides
Trends in Acid Strength of Oxoacids
Acidity of Hydrated Metal Ions

18.7 Acid-Base Properties of Salt Solutions

Salts That Yield Neutral Solutions
Salts That Yield Acidic Solutions
Salts That Yield Basic Solutions
Salts of Weakly Acidic Cations and Weakly Basic Anions

18.8 Generalizing the Brønsted-Lowry Concept: The Leveling Effect

18.9 Electron-Pair Donation and the Lewis Acid-Base Definition

Molecules as Lewis Acids
Metal Cations as Lewis Acids
An Overview of Acid-Base Definitions

Chapter Perspective

For Review and Reference

Problems

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

19.5 Ionic Equilibria in Chemical Analysis

Selective Precipitation
Qualitative Analysis: Identifying Ions in Complex Mixtures

Chapter Perspective

For Review and Reference

Problems

20
Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

20.1 The Second Law of Thermodynamics: Predicting Spontaneous Change

Limitations of the First Law of Thermodynamics
The Sign of ¿H Cannot Predict Spontaneous Change
Freedom of Motion and Dispersal of Energy
Entropy and the Number of Microstates
Entropy and the Second Law of Thermodynamics Standard Molar Entropies and the Third Law

20.2 Calculating the Change in Entropy of a Reaction

Entropy Changes in the System: Standard Entropy of Reaction (¿Srxn0)
Entropy Changes in the Surroundings: The Other Part of the Total
The Entropy Change and the Equilibrium State

Chemical Connections to Biology: Do Living Things Obey the Laws of Thermodynamics?

Spontaneous Exothermic and Endothermic Reactions: A Summary

20.3 Entropy, Free Energy, and Work

Free Energy Change and Reaction Spontaneity
Calculating Standard Free Energy Changes
¿G and the Work a System Can Do
The Effect of Temperature on Reaction Spontaneity
Coupling of Reactions to Drive a Nonspontaneous Change

Chemical Connections to Biological Energetics: The Universal Role of ATP

20.4 Free Energy, Equilibrium, and Reaction Direction

Chapter Perspective

For Review and Reference

Problems

21
Electrochemistry: Chemical Change and Electrical Work

21.1 Half-Reactions and Electrochemical Cells

A Quick Review of Oxidation-Reduction Concepts
Half-Reaction Method for Balancing Redox Reactions
An Overview of Electrochemical Cells

21.2 Voltaic Cells: Using Spontaneous Reactions to Generate Electrical Energy

Construction and Operation of a Voltaic Cell
Notation for a Voltaic Cell
Why Does a Voltaic Cell Work?

21.3 Cell Potential: Output of a Voltaic Cell

Standard Cell Potentials
Relative Strengths of Oxidizing and Reducing Agents

21.4 Free Energy and Electrical Work

Standard Cell Potential and the Equilibrium Constant
The Effect of Concentration on Cell Potential
Changes in Potential During Cell Operation
Concentration Cells

21.5 Electrochemical Processes in Batteries

Primary (Nonrechargeable) Batteries
Secondary (Rechargeable) Batteries
Fuel Cells

21.6 Corrosion: A Case of Environmental Electrochemistry

The Corrosion of Iron
Protecting Against the Corrosion of Iron

21.7 Electrolytic Cells: Using Electrical Energy to Drive Nonspontaneous Reactions

Construction and Operation of an Electrolytic Cell
Predicting the Products of Electrolysis
The Stoichiometry of Electrolysis: The Relation Between Amounts of Charge and Product

Chemical Connections to Biological Energetics: Cellular Electrochemistry and the Production of ATP

Chapter Perspective

For Review and Reference

Problems

22 The Elements in Nature and Industry

22.1 How the Elements Occur in Nature

Earth’s Structure and the Abundance of the Elements
Sources of the Elements

22.2 The Cycling of Elements Through the Environment

The Carbon Cycle
The Nitrogen Cycle
The Phosphorus Cycle

22.3 Metallurgy: Extracting a Metal from Its Ore

Pretreating the Ore
Converting Mineral to Element
Refining and Alloying the Element

22.4 Tapping the Crust: Isolation and Uses of the Elements

Producing the Alkali Metals: Sodium and Potassium
The Indispensable Three: Iron, Copper, and Aluminum
Mining the Sea: Magnesium and Bromine
The Many Sources and Uses of Hydrogen

22.5 Chemical Manufacturing: Two Case Studies

Sulfuric Acid, the Most Inportant Chemical
The Chlor-Alkali Process

Chapter Perspective

For Review and Reference

Problems

23 The Transition Elements and Their Coordination Compounds

23.1 Properties of the Transition Elements

Electron Configurations of the Transition Metals and Their Ions
Atomic and Physical Properties of the Transition Elements
Chemical Properties of the Transition Metals

23.2 The Inner Transition Elements

The Lanthanides
The Actinides

23.3 Highlights of Selected Transition Metals

Chromium
Manganese
Silver
Mercury

23.4 Coordination Compounds

Complex Ions: Coordination Numbers, Geometries, and Ligands
Formulas and Names of Coordination Compounds
A Historical Perspective: Alfred Werner and Coordination Theory
Isomerism in Coordination Compounds

23.5 Theoretical Basis for the Bonding and Properties of Complexes

Application of Valence Bond Theory to Complex Ions
Crystal Field Theory

Chapter Perspective

Chemical Connections to Nutritional Science: Transition Metals as Essential Dietary Trace Elements

For Review and Reference

Problems

24
Nuclear Reactions and Their Applications

24.1 Radioactive Decay and Nuclear Stability

The Components of the Nucleus: Terms and Notation
The Discovery of Radioactivity and the Types of Emissions
Types of Radioactive Decay; Balancing Nuclear Equations
Nuclear Stability and the Mode of Decay

24.2 The Kinetics of Radioactive Decay

The Rate of Radioactive Decay

Tools of the Laboratory: Counters for the Detection of Radioactive Emissions

Radioisotopic Dating

24.3 Nuclear Transmutation: Induced Changes in Nuclei

Early Transmutation Experiments; Discovery of the Neutron
Particle Accelerators and the Transuranium Elements

24.4 The Effects of Nuclear Radiation on Matter

The Effects of Radioactive Emissions: Excitation and Ionization
Effects of Ionizing Radiation on Living Matter

24.5 Applications of Radioisotopes

Radioactive Tracers: Applications of Nonionizing Radiation
Applications of Ionizing Radiation

24.6 The Interconversion of Mass and Energy

The Mass Defect
Nuclear Binding Energy

24.7 Applications of Fission and Fusion

The Process of Nuclear Fission
The Promise of Nuclear Fusion

Chemical Connections to Cosmology: Origin of the Elements in the Stars

Chapter Perspective

For Review and Reference

Problems

Appendix A
Common Mathematical Operations in Chemistry

Appendix B
Standard Thermodynamic Values for Selected Substances at 298 K

Appendix C
Equilibrium Constants at 298 K

Appendix D
Standard Electrode (Half-Cell) Potentials at 298 K

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