內容簡介

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.

作者簡介

目次

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