Chemistry: Atoms First

by Burdge, Julia; Overby, Jason

• ISBN13: 9780073511160
• ISBN10: 0073511161
• Format: Hardcover
• Copyright: 2011-01-11
• Publisher: McGraw-Hill Science/Engineering/Math

Summary

The atoms first approach provides a consistent and logical method for teaching general chemistry. This approach starts with the fundamental building block of matter, the atom, and uses it as the stepping stone to understanding more complex chemistry topics. Once mastery of the nature of atoms and electrons is achieved, the formation and properties of compounds are developed. Only after the study of matter and the atom will students have sufficient background to fully engage in topics such as stoichiometry, kinetics, equilibrium, and thermodynamics. Thus, the Atoms First method empowers instructors to present the most complete and compelling story of general chemistry. This textbook will offer the same engaging writing style, modern and descriptive artwork, sound problem-solving approach and wide range of end-of-chapter problems that customers are accustomed to with the Burdge product. Jason Overby's involvement with this project was crucial as he has been teaching with this approach for over four years which allowed Julia and Jason to create a product that fits the need for this growing market.

Table of Contents

Chapter 1—Chemistry: The Science of Change

1.1 The Study of Chemistry

1.1 Classification of Matter

1.3 The Properties of Matter

1.4 Scientific Measurement

1.5 Uncertainty in Measurement

1.6 Using Units and Solving Problems

Chapter 2—Atoms and the Periodic Table

2.1 Atoms First

2.2 Subatomic Particles and Atomic Structure

2.3 Atomic Number, Mass Number, and Isotopes

2.4 Average Atomic Mass

2.5 The Periodic Table

2.6 The Mole and Molar Masses

Chapter 3—Quantum Theory and the Electronic Structure of Atoms

3.1 Energy and Energy Changes

3.2 The Nature of Light

3.3 Quantum Theory

3.4 Bohr’s Theory of the Hydrogen Atom

3.5 Wave Properties of Matter

3.6 Quantum Mechanics

3.7 Quantum Numbers

3.8 Atomic Orbitals

3.9 Electron Configuration

3.10 Electron Configurations and the Periodic Table

Chapter 4—Periodic Trends of the Elements

4.1 Development of the Periodic Table

4.2 The Modern Periodic Table

4.3 Effective Nuclear Charge

4.4 Periodic Trends in Properties of Atoms

4.5 Electron Configuration of Ions

4.6 Ionic Radius

Chapter 5—Ionic and Covalent Compounds

5.1 Compounds

5.2 Lewis Dot Symbols

5.3 Ionic Compounds and Bonding

5.4 Naming Ions and Ionic Compounds

5.5 Covalent Molecules and Bonding

5.6 Naming Molecular Compounds

5.7 Covalent Bonding in Ionic Species

5.8 Molecular and Formula Masses

5.9 Percent Composition of Compounds

5.10 The Mole and Molar Masses

Chapter 6—Representing Molecules

6.1 The Octet Rule

6.2 Electronegativity and Polarity

6.3 Drawing Lewis Structures

6.4 Lewis Structures and Formal Charge

6.5 Resonance

6.6 Exceptions to the Octet Rule

Chapter 7—Molecular Geometry and Bonding Theories

7.1 Molecular Geometry

7.2 Molecular Geometry and Polarity

7.3 Valence Bond Theory

7.4 Hybridization of Atomic Orbitals

7.5 Hybridization in Molecules Containing Multiple Bonds

7.6 Molecular Orbital Theory

7.7 Bonding Theories and Descriptions of Molecules with Delocalized Bonding

Chapter 8—Chemical Reactions

8.1 Chemical Equations

8.2 Combustion Analysis

8.3 Calculations with Balanced Chemical Equations

8.4 Limiting Reactants

8.5 Periodic Trends in Reactivity of the Main Group Elements

Chapter 9—Chemical Reactions in Aqueous Solutions

9.1 General Properties of Aqueous Solutions

9.2 Precipitation Reactions

9.3 Acid-Base Reactions

9.4 Oxidation–Reduction Reactions

9.5 Concentration of Solutions

9.6 Aqueous Reactions and Chemical Analysis

Chapter 10—Thermochemistry

10.1 Energy Changes in Chemical Reactions

10.2 Introduction to Thermodynamics

10.3 Enthalpy

10.4 Calorimetry

10.5 Hess’s Law

10.6 Standard Enthalpies of Formation

10.7 Bond Enthalpy and the Stability of Covalent Molecules

10.8 Lattice Energy and the Stability of Ionic Solids

Chapter 11—Gases

11.1 Properties of Gases

11.2 The Kinetic Molecular Theory of Gases

11.3 Pressure

11.4 The Gas Laws

11.5 The Ideal Gas Equation

11.6 Real Gases

11.7 Gas Mixtures

11.8 Reactions with Gaseous Reactants and Products

Chapter 12—Intermolecular Forces and the Physical Properties of Condensed Phases

12.1 Intermolecular Forces

12.2 Properties of Liquids

12.3 Crystal Structure

12.4 Types of Crystals

12.5 Amorphous Solids

12.6 Phase Changes

12.7 Phase Diagrams

Chapter 13—Physical Properties of Solutions

13.1 Types of Solutions

13.2 A Molecular View of the Solution Process

13.3 Concentration Units

13.4 Factors that Affect Solubility

13.5 Colligative Properties

13.6 Calculations Using Colligative Properties

13.7 Colloids

Chapter 14—Chemical Kinetics

14.1 Reaction Rates

14.2 Collision Theory of Chemical Reactions

14.3 Measuring Reaction Progress and Expressing Reaction Rate

14.4 Dependence of Reaction Rate on Reactant Concentration

14.5 Dependence of Reactant Concentration on Time

14.6 Dependence of Reaction Rate on Temperature

14.7 Reaction Mechanisms

14.8 Catalysis

Chapter 15—Chemical Equilibrium

15.1 The Concept of Equilibrium

15.2 The Equilibrium Constant

15.3 Equilibrium Expressions

15.4 Using Equilibrium Expressions to Solve Problems

15.5 Factors That Affect Chemical Equilibrium

Chapter 16—Acids and Bases

16.1 Brønsted Acids and Bases

16.2 Molecular Structure and Acid Strength

16.3 The Acid-Base Properties of Water

16.4 The pH Scale

16.5 Strong Acids and Bases

16.6 Weak Acids and Acid Ionization Constants

16.7 Weak Bases and Base Ionization Constants

16.8 Conjugate Acid–Base Pairs

16.9 Diprotic and Polyprotic Acids

16.10 Acid–Base Properties of Salt Solutions

16.11 Acid–Base Properties of Oxides and Hydroxides

16.12 Lewis Acids and Bases

Chapter 17—Acid-Base Equilibria and Solubility Equilibria

17.1 The Common Ion Effect

17.2 Buffer Solutions

17.3 Acid–Base Titrations

17.4 Solubility Equilibria

17.5 Factors Affecting Solubility

17.6 Separation of Ions Using Differences in Solubility

Chapter 18—Entropy, Free Energy, and Equilibrium

18.1 Spontaneous Processes

18.2 Entropy

18.3 Entropy Changes in a System

18.4 Entropy Changes in the Universe

18.5 Predicting Spontaneity

18.6 Free Energy and Chemical Equilibrium

18.7 Thermodynamics in Living Systems

Chapter 19—Electrochemistry

19.1 Balancing Redox Reactions

19.2 Galvanic Cells

19.3 Standard Reduction Potentials

19.4 Spontaneity of Redox Reactions Under Standard-State Conditions

19.5 Spontaneity of Redox Reactions Under Conditions Other than Standard-State

19.6 Batteries

19.7 Electrolysis

19.8 Corrosion

Chapter 20—Nuclear Chemistry

20.1 Nuclei and Nuclear Reactions

20.2 Nuclear Stability

20.3 Natural Radioactivity

20.4 Nuclear Transmutation

20.5 Nuclear Fission

20.6 Nuclear Fusion

20.7 Uses of Isotopes

20.8 Biological Effects of Radiation

Chapter 21—Metallurgy and the Chemistry of Metals

21.1 Occurrence of Metals

21.2 Metallurgical Processes

21.3 Band Theory of Conductivity

21.4 Periodic Trends in Metallic Properties

21.5 The Alkali Metals

21.6 The Alkaline Earth Metals

21.7 Aluminum

Chapter 22—Coordination Chemistry

22.1 Coordination Compounds

22.2 Structure of Coordination Compounds

22.3 Bonding in Coordination Compounds: Crystal Field Theory

22.4 Reactions of Coordination Compounds

22.5 Applications of Coordination Compounds

Chapter 23—Nonmetallic Elements and Their Compounds

23.1 General Properties of Nonmetals

23.2 Hydrogen

23.3 Carbon

23.4 Nitrogen and Phosphorus

23.5 Oxygen and Sulfur

23.6 The Halogens

Chapter 24—Organic Chemistry

24.1 Why Carbon is Different

24.2 Classes of Organic Compounds

24.3 Representing Organic Molecules

24.4 Isomerism

24.5 Organic Reactions

24.6 Organic Polymers

Chapter 25—Materials

25.1 Polymers

25.2 Ceramics and Composite Materials

25.3 Liquid Crystals

25.4 Biomedical Materials

25.5 Nanotechnology

25.6 Semiconductors

25.7 Superconductors

Appendix

Appendix 1 – Mathematical Operations

Appendix 2 – Thermodynamic Data at 1 ATM and 25°C

Appendix 3 – Ionization Constants of Weak Acids and Bases at 25°C

Appendix 4 – Solubility Product Constants at 25°C