University chemistry / Brian B. Laird.

Table of Contents
Chapter 0: The Language of Chemistry
0.1 Chemistry Is the Study of Matter and Change
0.2 Matter Consists of Atoms and Molecules
0.3 Compounds Are Represented by Chemical Formulas
0.4 Reactions Are Represented by Balanced Chemical Equations
0.5 Quantities of Atoms or Molecules Can Be Described by Mass or Number
0.6 Stoichiometry Is the Quantitative Study of Mass and Mole Relationships in Chemical
Reactions

Chapter 1: The Quantum Theory of the Submicroscopic World
1.1 Classical Physics Does Not Adequately Describe the Interaction of Light with Matter
1.2 The Bohr Model Was an Early Attempt To Formulate a Quantum Theory of Matter
1.3 Matter Has Wavelike Properties
1.4 The Hydrogen Atom Is an Exactly Solvable Quantum-Mechanical System

Chapter 2: Many-Electron Atoms and the Periodic Table
2.1 The Wavefunctions of Many-Electron Atoms Can Be Described to a Good
Approximation Using Atomic Orbitals
2.2 Electron Configurations of Many-Electron Atoms Are Constructed Using the Aufbau (or
?Building-up?) Principle
2.3 The Periodic Table Predates Quantum Mechanics
2.4 Elements Can Be Classified by Their Position in the Periodic Table
2.5 The Properties of the Elements Vary Periodically across the Periodic Table

Chapter 3: The Chemical Bond
3.1 Atoms in a Molecule Are Held Together by Chemical Bonds
3.2 A Covalent Bond Involves the Sharing of Electrons between Atoms in a Molecule
3.3 Electronegativity Differences Determine the Polarity of Chemical Bonds
3.4 Drawing Correct Lewis Structures Is an Invaluable Skill for a Chemist
3.5 Molecular Orbital Theory Provides a Detailed Description of Chemical Bonding
Chapter 4: Molecular Structure and Interaction

4.1 The Basic Three-Dimensional Structure of a Molecule Can Be Predicted Using
the VSEPR Model
4.2 The Polarity of a Molecule Can Be Described Quantitatively by Its Dipole
Moment
4.3 Valence Bond Theory for Polyatomic Molecules Requires the Use of Hybrid
Orbitals
4.4 Isomers Are Compounds That Have the Same Molecular Formula but Different
Atomic Arrangements
4.5 Bonding in Polyatomic Molecules Can Be Explained Using Molecular Orbitals
4.6 The Interactions between Molecules Greatly Affect the Bulk Properties of
Materials

Chapter 5: The States of Matter I: Phase Diagrams and Gases
5.1 Pressure and Temperature Are Two Important Macroscopic Properties of Chemical
Systems
5.2 Substances and Mixtures Can Exist as Solid, Liquid, or Gas, Depending upon the
External Conditions
5.3 The Ideal Gas Equation Describes the Behavior of All Gases in the Limit of
Low Pressure
5.4 The Kinetic Theory of Gases Provides a Molecular Explanation for the Behavior of
Gases
5.5 Real Gases Exhibit Deviations from Ideal Behavior at High Pressure

Chapter 6: The States of Matter II: Liquids and Solids
6.1 The Structure and Properties of Liquids Are Governed by Intermolecular Interactions
6.2 The Molecules of a Crystal Are Located on a Regular Array Called a Crystal Lattice
6.3 The Properties of Crystalline Solids Are Determined Largely by Intermolecular
Interactions
6.4 Band Theory Accurately Explains the Conductivity of Metals, Semiconductors, and
Insulators

Chapter 7: Thermochemistry: Energy in Chemical Reactions
7.1 Thermodynamics Is the Study of Energy and Its Transformations in Macroscopic
Systems
7.2 The Energy Absorbed by a System as Heat in a Constant-Pressure Process Is
Equal to the Change in Enthalpy
7.3 The Temperature Change of a System upon Heating Is
Governed by Its Heat Capacity
7.4 The Enthalpy Changes in Reaction Can Be Calculated Using Standard Enthalpies
of Formation
7.5 The Reaction Enthalpies Can Be Estimated from Bond Enthalpies
7.6 Enthalpy Changes Also Accompany Physical Transformations
7.7 The Temperature Dependence of Reaction Enthalpies Can Be Determined from
Heat Capacity Data

Chapter 8: Entropy, Free Energy, and the Second Law of Thermodynamics
8.1 The Entropy of an Isolated System Always Increases in Any Spontaneous Process
8.2 The Entropy Change for a Process Can Be Calculated Using the Thermodynamic
Definition of Entropy
8.3 The Third Law of Thermodynamics Allows Us to Determine Absolute Entropies
8.4 The Spontaneity of a Process at Constant Temperature and Pressure Is Governed
by the Gibbs Free Energy
8.5 The Mixing of Pure Substances Leads to an Increase in the Entropy and a
Decrease in the Gibbs Free Energy
8.6 In Living Systems, Spontaneous Reactions Are Used to Drive Other
Nonspontaneous, but Essential, Biochemical Processes

Chapter 9: Physical Equilibrium
9.1 The Phase Boundaries in Pure Systems Can Be Predicted Using Thermodynamics
9.2 The Solubility of a Substance Is Determined by Temperature, Pressure, and the
Types of Intermolecular Forces Present in the Solution
9.3 The Liquid-Vapor Phase Equilibrium of a Solution Can Be Understood in Terms
of the Entropy of Mixing and the Intermolecular Interactions
9.4 Colligative Properties Are Properties of Solution Phase Equilibria That Depend
Only upon the Number of Solute Molecules, Not Their Type

Chapter 10: Chemical Equilibrium
10.1 The Equilibrium Constant Governs the Concentration of Reactants and Products
at Equilibrium
10.2 The Equilibrium Constant Can be Used to Predict the Direction and Equilibrium
Concentrations of a Chemical Reaction
10.3 The Equilibrium Constant for a Reaction Can Be Determined from the Standard
Gibbs Free Energy Change
10.4 The Response of an Equilibrium System to a Change in Conditions Can be
Determined Using Le Ch¿telier?s Principle

Chapter 11: Acids and Bases
11.1 Many Processes in Chemistry Are Acid-Base Reactions
11.2 The Acid-Base Properties of Aqueous Solutions Are Governed by the
Autoionization Euilibrium of Water
11.3 The Strengths of Acid and Bases Are Measured by Their Ionization Constants
11.4 The pH of an Acid or Base Can Be Calculated If Its Ionization Constant Is Known
11.5 The Strength of an Acid Is Determined in Part by Molecular Structure
11.6 many Salts Have Acid-Base Properties in Aqueous Solution
11.7 Oxide and Hydroxide Compounds Can be Acidic or Basic in Aqueous Solution
Depending on Their Composition

Chapter 12: Acid-Base Equilibria and Solubility
12.1 Ionization of Weak Acids and Bases Is Suppressed by the Addition of a Common
Ion
12.2 The pH of a Buffer Solution Is Resistant to Large Changes in pH
12.3 The Concentration of an Unknown Acid or Base Can Be Determined by Titration
12.4 An Acid-Base Indicator Is a Substance That Changes Color at a Specific pH
12.5 A Precipitation Reaction Occurs when a Reaction in Solution Leads to an
Insoluble Product
12.6 The Solubility Product Is the Equilibrium Constant for the Dissolution Process
12.7 The Solubility of a Substance Is Affected by a Number of Factors
12.8 The Solubility Product Principle Can Be Applied to Qualitative Analysis

Chapter 13: Electrchemistry
13.1 Oxidation-Reduction (Redox) Involve a Transfer of Electrons from One Species
to Another
13.2 Redox Reactions Can Be Used to Generate Electric Current in a Galvanic Cell
13.3 The Standard Emf of Any Electrochemical Cell Can Be Determined If the
Standard Reduction Potentials for the Half-Reactions Are Known
13.4 The Emf of An Electrochemical Cell Is Directly Related to the Gibbs Free-Energy
Change of the Redox Reaction
13.5 The Concentration Dependence of the Emf Can Be Determined Using the Nernst
Equation
13.6 Batteries Use Electrochemical Reactions to Produce a Ready Supply of Electric
Current
13.7 In Electrolysis, an Electric Current Is Used to Drive a Nonspontaneous Reaction
Chapter 14: Chemical Kinetics

14.1 Chemical Knetics Is the Study of the Rates at Which Chemical Reactions Occur
14.2 The Rate Law Gives the Dependence of the Reaction Rate on the Reactant
Concentration
14.3 Integrated Rate Laws Specify the Relationship between Reactant Concentration
and Time
14.4 The Arrhenius Equation Gives the Temperature Dependence of Rate Constants
14.5 The Reaction Mechanism Is the Sequence of Elementary Steps That Lead to
Product Formation
14.6 Reaction Rates Can Often Be Increased by the Addition of a Catalyst

Chapter 15: The Chemistry of Transition Metals
15.1 Transition Metals Have Electron Configurations with Incomplete d or f Shells
15.2 Transition Metals Can Form a Variety of Coordination Compounds
15.3 Bonding in Coordination Compounds Can Be Described by Crystal Field Theory
15.4 The Reactions of Coordination Compounds Have a Wide Number of Useful
Applications

Chapter 16: Organic and Polymer Chemistry
16.1 Hydrocarbons Are Organic Compounds Containing Only Hydrogen and Carbon
16.2 Hydrocarbons Undergo a Number of Important Chemical Reactions
16.3 The Structure and Properties of Organic Compounds Are Greatly Influenced by
the Presence of Functional Groups
16.4 Polymers Are Large Molecular Weight Compounds Formed from the Joining
Together of Many Subunits Called Monomers

16.5 Proteins Are Polymer Chains Composed of Amino Acid Monomers
16.6 DNA and RNA Are Polymers Composed of Nucleic Acids

Chapter 17: Nuclear Chemistry
17.1 Nuclear Chemistry Is the Study of Changes Involving Atomic Nuclei
17.2 The Stability of a Nucleus Is Determined Primarily by Its Neutron-to-Proton
Ratio
17.3 Radioactive Decay Is a First-Order Kinetic Process
17.4 New Isotopes Can Be Produced Through the Process of Nuclear Transmutation
17.5 In Nuclear Fission, a Large Nucleus Is Split into Smaller Nuclei
17.6 In Nuclear Fusion, Energy Is Produced When Light Nuclei Combine to Form
Heavier Ones
17.7 Radioactive and Stable Isotopes Alike Have many Applications in Science and
Medicine
17.8 The Biological Effects of Radiation Can Be Quite Dramatic

Appendix 1: Measurement and Mathematical Background
A1.1 Measurement
A1.2 Mathematical Background
Appendix 2: Thermodynamic Data at 1 Bar and 25°C
Appendix 3: Derivation of the Names of the Elements
Appendix 4: Isotopes of the First Ten Elements
List of Applications
Distribution of Elements on Earth and in Living Systems 18
Important Experimental Technique: The Mass Spectrometer 46
Laser?The Splendid Light 92
Important Experimental Technique: Electron Microscopy 109
The Third Liquid Element? 156
Discovery of the Noble Gases 163
Major Experimental Technique: Microwave Spectroscopy 186
Just Say NO 198
Major Experimental Technique: Infrared Spectroscopy 238
cis-trans Isomerization in the Vision Process 254
Buckyball, Anyone? 262
Super-Cold Atoms 316
Why Do Lakes Freeze from the Top Down? 340
High- Temperature Superconductors 358
Fuel Values of Foods and Other Substances 390
The Efficiency of Heat Engines: The Carnot Cycle 438
The Thermodynamics of a Rubber Band 456
The Killer Lake 483
Life at High Altitudes and Hemoglobin Production 545
Antacids and the pH Balance in Your Stomach 602
Maintaining the pH of Blood 620
Dental Filling Discomfort 680
Femtochemistry 753
Coordination Compounds in Living Systems 784
Cisplatin?an Anticancer Drug 795
Important Experimental Technique: Nuclear Magnetic Resonance Spectroscopy 824
Sickle Cell Anemia: A Molecule Disease 840
DNA Fingerprinting 843
Nature?s Own Fission Reactor 881
Food Irradiation