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Preface
Chapter 1  Essential Ideas
Introduction
1.1 Chemistry in Context
1.2 Phases and Classification of Matter
1.3 Physical and Chemical Properties
1.4 Measurements
1.5 Measurement Uncertainty, Accuracy, and Precision
1.6 Mathematical Treatment of Measurement Results
Key Terms
Key Equations
Summary
Exercises
Chapter 2  Atoms, Molecules, and Ions
Introduction
2.1 Early Ideas in Atomic Theory
2.2 Evolution of Atomic Theory
2.3 Atomic Structure and Symbolism
2.4 Chemical Formulas
2.5 The Periodic Table
2.6 Ionic and Molecular Compounds
2.7 Chemical Nomenclature
Key Terms
Key Equations
Summary
Exercises
Chapter 3  Composition of Substances and Solutions
Introduction
3.1 Formula Mass and the Mole Concept
3.2 Determining Empirical and Molecular Formulas
3.3 Molarity
3.4 Other Units for Solution Concentrations
Key Terms
Key Equations
Summary
Exercises
Chapter 4  Stoichiometry of Chemical Reactions
Introduction
4.1 Writing and Balancing Chemical Equations
4.2 Classifying Chemical Reactions
4.3 Reaction Stoichiometry
4.4 Reaction Yields
4.5 Quantitative Chemical Analysis
Key Terms
Key Equations
Summary
Exercises
Chapter 5  Thermochemistry
Introduction
5.1 Energy Basics
5.2 Calorimetry
5.3 Enthalpy
Key Terms
Key Equations
Summary
Exercises
Chapter 6  Electronic Structure and Periodic Properties of Elements
Introduction
6.1 Electromagnetic Energy
6.2 The Bohr Model
6.3 Development of Quantum Theory
6.4 Electronic Structure of Atoms (Electron Configurations)
6.5 Periodic Variations in Element Properties
Key Terms
Key Equations
Summary
Exercises
Chapter 7  Chemical Bonding and Molecular Geometry
Introduction
7.1 Ionic Bonding
7.2 Covalent Bonding
7.3 Lewis Symbols and Structures
7.4 Formal Charges and Resonance
7.5 Strengths of Ionic and Covalent Bonds
7.6 Molecular Structure and Polarity
Key Terms
Key Equations
Summary
Exercises
Chapter 8  Advanced Theories of Covalent Bonding
Introduction
8.1 Valence Bond Theory
8.2 Hybrid Atomic Orbitals
8.3 Multiple Bonds
8.4 Molecular Orbital Theory
Key Terms
Key Equations
Summary
Exercises
Chapter 9  Gases
Introduction
9.1 Gas Pressure
9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law
9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions
9.4 Effusion and Diffusion of Gases
9.5 The Kinetic-Molecular Theory
9.6 Non-Ideal Gas Behavior
Key Terms
Key Equations
Summary
Exercises
Chapter 10  Liquids and Solids
Introduction
10.1 Intermolecular Forces
10.2 Properties of Liquids
10.3 Phase Transitions
10.4 Phase Diagrams
10.5 The Solid State of Matter
10.6 Lattice Structures in Crystalline Solids
Key Terms
Key Equations
Summary
Exercises
Chapter 11  Solutions and Colloids
Introduction
11.1 The Dissolution Process
11.2 Electrolytes
11.3 Solubility
11.4 Colligative Properties
11.5 Colloids
Key Terms
Key Equations
Summary
Exercises
Chapter 12  Kinetics
Introduction
12.1 Chemical Reaction Rates
12.2 Factors Affecting Reaction Rates
12.3 Rate Laws
12.4 Integrated Rate Laws
12.5 Collision Theory
12.6 Reaction Mechanisms
12.7 Catalysis
Key Terms
Key Equations
Summary
Exercises
Chapter 13  Fundamental Equilibrium Concepts
Introduction
13.1 Chemical Equilibria
13.2 Equilibrium Constants
13.3 Shifting Equilibria: Le Châtelier’s Principle
13.4 Equilibrium Calculations
Key Terms
Key Equations
Summary
Exercises
Chapter 14  Acid-Base Equilibria
Introduction
14.1 Brønsted-Lowry Acids and Bases
14.2 pH and pOH
14.3 Relative Strengths of Acids and Bases
14.4 Hydrolysis of Salts
14.5 Polyprotic Acids
14.6 Buffers
14.7 Acid-Base Titrations
Key Terms
Key Equations
Summary
Exercises
Chapter 15  Equilibria of Other Reaction Classes
Introduction
15.1 Precipitation and Dissolution
15.2 Lewis Acids and Bases
15.3 Coupled Equilibria
Key Terms
Key Equations
Summary
Exercises
Chapter 16  Thermodynamics
Introduction
16.1 Spontaneity
16.2 Entropy
16.3 The Second and Third Laws of Thermodynamics
16.4 Free Energy
Key Terms
Key Equations
Summary
Exercises
Chapter 17  Electrochemistry
Introduction
17.1 Review of Redox Chemistry
17.2 Galvanic Cells
17.3 Electrode and Cell Potentials
17.4 Potential, Free Energy, and Equilibrium
17.5 Batteries and Fuel Cells
17.6 Corrosion
17.7 Electrolysis
Key Terms
Key Equations
Summary
Exercises
Chapter 18  Representative Metals, Metalloids, and Nonmetals
Introduction
18.1 Periodicity
18.2 Occurrence and Preparation of the Representative Metals
18.3 Structure and General Properties of the Metalloids
18.4 Structure and General Properties of the Nonmetals
18.5 Occurrence, Preparation, and Compounds of Hydrogen
18.6 Occurrence, Preparation, and Properties of Carbonates
18.7 Occurrence, Preparation, and Properties of Nitrogen
18.8 Occurrence, Preparation, and Properties of Phosphorus
18.9 Occurrence, Preparation, and Compounds of Oxygen
18.10 Occurrence, Preparation, and Properties of Sulfur
18.11 Occurrence, Preparation, and Properties of Halogens
18.12 Occurrence, Preparation, and Properties of the Noble Gases
Key Terms
Summary
Exercises
Chapter 19  Transition Metals and Coordination Chemistry
Introduction
19.1 Occurrence, Preparation, and Properties of Transition Metals and Their Compounds
19.2 Coordination Chemistry of Transition Metals
19.3 Spectroscopic and Magnetic Properties of Coordination Compounds
Key Terms
Summary
Exercises
Chapter 20  Organic Chemistry
Introduction
20.1 Hydrocarbons
20.2 Alcohols and Ethers
20.3 Aldehydes, Ketones, Carboxylic Acids, and Esters
20.4 Amines and Amides
Key Terms
Summary
Exercises
Chapter 21  Nuclear Chemistry
Introduction
21.1 Nuclear Structure and Stability
21.2 Nuclear Equations
21.3 Radioactive Decay
21.4 Transmutation and Nuclear Energy
21.5 Uses of Radioisotopes
21.6 Biological Effects of Radiation
Key Terms
Key Equations
Summary
Exercises
1.1.A
Calculate quantities of a
substance or its relative
number of particles using
dimensional analysis and the
mole concept.
1.1.A.1
One cannot count particles directly while
performing laboratory work. Thus, there must
be a connection between the masses of
substances reacting and the actual number of
particles undergoing chemical changes.
1.1.A.2
Avogadro’s number (N = 6.022 × 1023 mol−1
)
provides the connection bet A
ween the number
of moles in a pure sample of a substance and
the number of constituent particles (or formula
units) of that substance.
1.1.A.3
Expressing the mass of an individual atom
or molecule in atomic mass units (amu) is
useful because the average mass in amu of
one particle (atom or molecule) or formula
unit of a substance will always be numerically
equal to the molar mass of that substance
in grams. Thus, there is a quantitative
connection between the mass of a substance
and the number of particles that the
substance contains.
EQN: n = m/M