Chemistry & chemical reactivity / 5th ed.

[unit 1.] The basic tools of chemistry
1. Matter and measurement
Out of gas!
1.1. Elements and atoms
1.2. Compounds and molecules
1.3. Physical properties
1.4. Physical and chemical change
1.5. Classifying matter
1.6. Units of measurement
1.7. Using numerical information
1.8. Problem solving
2. Atoms and elements
Stardust
2.1. Protons, electrons, and neutrons : development of atomic structure
2.2. Atomic number and atomic mass
2.3. Isotopes
2.4. Atomic weight
2.5. Atoms and the mole
2.6. The periodic table
2.7. An overview of the elements, their chemistry,and the periodic table
2.8. Essential elements
3. Molecules, ions, and their compounds
Buckyball, a startling new molecule
3.1. Molecules, compounds, and formulas
3.2. Molecular models
3.3. Ionic compounds : formulas, names, and properties
3.4. Molecular compounds : formulas, names, and properties
3.5. Formulas, compounds, and the mole
3.6. Determining compound formulas
3.7. Hydrated compounds
4. Chemical equations and stoichiometry
Black smokers and the origin of life
4.1. Chemical equations
4.2. Balancing chemical equations
4.3. Mass relationships inchemical reactions : stoichiometry
4.4. Reactions in which one reactant is present in limited supply
4.5. Percent yield
4.6. Chemical equations and chemical analysis
5. Reactions in aqueous solution
Why is thesea salty?
5.1. Properties of compounds in aqueous solution
5.2. Precipitation reactions
5.3. Acids andbases
5.4. Reactions of acids and bases
5.5. Gas-forming reactions
5.6. Classifying reactions in aqueoussolution
5.7. Oxidation-reduction reactions
5.8. Measuring concentrations of compounds in solution
5.9. pH : a concentration scale for acids and bases
5.10. Stoichiometry of reactions in aqueous solution
6. Principles of reactivity : energy and chemical reactions
Abba's refrigerator
6.1. Energy : some basic principles
6.2. Specific heat capacity and heat transfer
6.3. Energy and changes of state
6.4. The first law of thermodynamics
6.5. Enthalpy changes in chemical reactions
6.6. Calorimetry
6.7. Hess's law
6.8. Standard enthalpies of formation
6.9. Product- or reactant-favored reactions and thermochemistry
6.10.Energy resources

[unit 2.] The structure of atoms and molecules
7. Atomic structure
Colors in the sky
7.1. Electromagnetic radiation
7.2. Planck, Einstein, energy,and protons
7.3. Atomic line spectra and Niels Bohr
7.4. Wave properties of the electron
7.5. Quantum mechanical view of the atom
7.6. The shapes of atomic orbitals
7.7. Atomic orbitals and chemistry
8. Atomic electron configurations and chemical periodicity --Everything in its place
8.1. Electron spin
8.2. Pauli exclusion principle
8.3. Atomic subshell energiesand electron assignments
8.4. Atomic electron configurations
8.5. Electron configurations of ions
8.6. Atomic properties and periodic trends
8.7. Periodic trends and chemical properties
9. Bonding and molecular structure : fundamental concepts
Sugar in space
9.1. Valence electrons
9.2. Chemical bond formation
9.3. Bonding in ionic compounds
9.4. Covalent bonding and Lewis structures
9.5. Resonance --9.6. Exceptions to the octet rule
9.7. Charge distribution in covalent bonds and molecules
9.8. Bond properties
9.9. Molecular shapes
9.10. Molecular polarity
9.11. The DNA story, revisited
10. Bonding and molecular structure : orbital hybridization and molecular orbitals
Linus Pauling : a life of chemical thought
10.1. Orbitals and bonding theories
10.2 Valence bond theory
10.3. Molecular orbital theory
10.4. Metals and semiconductors
11. Carbons : more thanjust another element
A colorful beginning
11.1. Why carbon?
11.2. Hydrocarbons
11.3. Alcohols, ethers, and amines
11.4. Compounds with a carbonyl group
11.5. Polymers

[unit 3.] States of matter
12. Gases and their properties
Up, up, and away!
12.1. The properties ofgases
12.2. Gas laws : experimental basis
12.3. Ideal gas law
12.4. Gas laws and chemical reactions
12.5. Gas mixtures and partial pressures
12.6. Kinetic-molecular theory of gases
12.7. Diffusion and effusion
12.8. Some applications of the gas laws and kinetic-molecular theory
12.9. Nonideal behavior : real gases
13. Intermolecular forces, liquids, and solids
The mystery of the disappearing fingerprints
13.1. States of matter and the kinetic-molecular theory
13.2. Intermolecular forces
13.3. Hydrogen bonding
13.4. Summary of intermolecular forces
13.5. Properties of liquids
13.6. Solid-state chemistry : metals
13.7. Solid-state chemistry : structures and formulas of ionic solids
13.8. Other kinds of solid materials
13.9. The physical properties of solids
13.10. Phase diagrams-- 14. Solutions and their behavior
The killer lakes ofCameroon
14.1. Units of concentration
14.2. Solutionprocess
14.3. Factors affecting solubility : pressure and temperature
14.4. Colligative properties
14.5. Colloids

[unit 4.] The control of chemical reactions
15. Principles of reactivity : chemical kinetics
Faster andfaster
15.1. Rates of chemical reactions
15.2. Reaction conditions and rate
15.3. Effect of concentration on reaction rate
15.4. Concentration-timerelationships : integrated rate laws
15.5. Particulate view of reaction rates
15.6. Reaction mechanisms
16.Principles of reactivity : chemical equilibria
Fertilizer and poison gas
16.1. Nature of the equilibrium state
16.2. The reaction quotient and equilibrium constant
16.3. Determining an equilibrium constant
16.4. Using equilibrium constants in calculations
16.5. More about balanced equations and equilibrium constants
16.6. Disturbing a chemical equilibrium
16.7. Applying the concepts of chemical equilibrium
17. Principles of reactivity : chemistry ofacids and bases
Nature's acids
17.1. Acids, bases, and the equilibrium concept
17.2. Brnsted concept of acids and bases
17.3. Water and the pH scale
17.4. Equilibrium constants for acids and bases
17.5. Equilibrium constants and acid-base reactions
17.6. Types of acid-base reactions
17.7. Calculations with equilibrium constants
17.8. Polyprotic acids and bases
17.9. Lewis concept of acids and bases
17.10. Molecular structure, bonding, and acid-base behavior
18. Principles of reactivity : other aspects of aqueous equilibria
Roses are red, violets are blue, and hydrangeas are red or blue
18.1. Common ion effect
18.2. Controlling pH : buffer solutions
18.3. Acid-basetitrations
18.4. Solubility of salts
18.5. Precipitation reactions
18.6. Solubility and complex ions
18.7. Solubility, ion separations, and qualitativeanalysis
19. Principles of reactivity : entropy and free energy
Perpetual motion machines
19.1. Spontaneous change and equilibrium
19.2. Heat and spontaneity
19.3. Entropy and the second law
19.4. Entropy and the third law of thermodynamics
19.5. Entropy changes
19.6. Gibbs free energy
19.7. (Delta)G{0} (Gibbs standard free energy), K (equilibrium constant), and product-favorability
19.8. Thermodynamics, time, and life
20. Principles of reactivity : electron transfer reactions
Blood gases --20.1. Oxidation-reduction reactions
20.2. Simple voltaic cells
20.3. Commercial voltaic cells
20.4. Standard electrochemical potentials
20.5. Electrochemical cells under nonstandard conditions
20.6. Electrochemistry and thermodynamics
20.7. Electrolysis : chemical change using electrical energy
20.8. Counting electrons

[unit 5.] The chemistry of the elements
21. The chemistry of the main group elements
Sulfur chemistry and life on the edge
21.1. The periodic table, a guide to the elements
21.2. Hydrogen
21.3. Sodium and potassium
21.4. Two alkaline earth elements : calcium and magnesium
21.5. Aluminum
21.6. Silicon
21.7. Nitrogen and phosphorus
21.8. Oxygen and sulfur
21.9. Chlorine
22. The chemistry of the transition elements
Memory metal
22.1. Properties of the transition elements
22.2. Metallurgy
22.3. Coordination compounds
22.4. Structures of coordinationcompounds
22.5. Bonding in coordination compounds
22.6. Colors of coordination compounds
23. Nuclear chemistry
Nuclear medicine
23.1. Natural radioactivity
23.2. Nuclear reactions and radioactive decay
23.3. Stability of atomic nuclei
23.4. Rates of nuclear decay
23.5. Artificial nuclear reactions
23.6. Nuclear fission
23.7. Nuclear fusion
23.8. Radiation health and safety
23.9. Applications of nuclear chemistry

Appendices
A. Some mathematical operations
B. Some important physical concepts
C. Abbreviations and usefulconversion factors
D. Physical constants
E. Naming organic compounds
F. Values for the ionization energiesand electron affinities of the elements
G. Vapor pressure of water at various temperatures
H. Ionizationconstants for weak acids at 25{0}C
I. Ionization constants for weak bases at 25{0}C
J. Solubility product constants for some inorganic compounds
K. Formation constants for some complex ions in aqueous solution
L. Selected thermodynamic values
M. Standard reduction potentials in aqueous solution at 25{0}C
N. Answers to exercises
O. Answers to selected study questions.