Chemistry for environmental engineering

1. Fundamentals of chemistry I.
1.1 Introduction: the fundamental proposition of chemistry and matter.
1.2 Basic concepts: the periodic table, symbols and notation, and common quantities and their units.
1.2.1 Symbols and notation.
1.2.2 Common quantities and units of measurement.
1.3 Writing chemical formulas and names.
1.3.1 Inorganic nomenclature and formula writing.
1.3.2 Calculating oxidation states from formulas.
1.4 Calculating molar masses and Avogadro's principle.
1.5 Determining the percent composition of a compound.
1.6 Determining empirical and molecular formulas from percent composition.
1.7 Solubility and concentration units for aqueous solutions.
1.8 Gas laws.
1.8.1 The kinetic molecular theory of gases.
1.8.2 The general gas law.
1.8.3 The ideal gas law.
1.8.4 Dalton's law of partial pressures.
1.8.5 Graham's law of effusion.
1.8.6 Intermolecular forces.
1.9 Chemical reactions.
1.9.1 Five categories of chemical reactions.
1.9.2 Oxidation-reduction or RED-OX reactions.
1.9.3 Writing and balancing chemical reactions.
1.9.4 Simple stoichiometry.
1.9.5 An illustrative example of a decomposition reaction, an explosion.
1.9.6 Limiting reagents.
1.9.7 Percent yield.
1.9.8 Consecutive and simultaneous reactions.
1.9.9 Energy change for exothermic vs endothermic reactions.
1.10 Colligative properties of solutions.
1.10.1 Basic concept.
1.10.2 Boiling-point elevation.
1.10.3 Freezing-point depression.
1.10.4 Henry's law.
1.10.5 Raoult's law for vapor-pressure lowering.
1.10.6 Osmotic pressure.
1.11 Acids, bases, and salts.
1.11.1 Basic concept.
1.11.2 Concentration units and the pH scale.
1.11.3 Calculations for strong acids and bases.
2. Fundamentals of chemistry.
2.1 Chemical equilibrium.
2.1.1 Basic concept.
2.1.2 The meaning of Kc.
2.1.3 Calculations for Kc.
2.1.4 Predicting equilibrium using a test quotient.
2.2 Stresses and Le Chatelier's principle.
2.2.1 Dependence of Kc on temperature.
2.3 Calculations for weak acids and bases.
2.3.1 Hydrolysis.
2.3.2 Buffer solutions and the Henderson-Hasselbalch equation.
2.3.3 Amphoterism.
2.4 Solubility product constants.
2.4.1 Basic concept.
2.4.2 Definition of solubility product constant, Ksp.
2.4.3 Calculating the molar solubility from Ksp.
2.4.4 Common and uncommon ion, and pH effects.
2.4.5 Predicting precipitation.
2.5 Complex ion formation.
2.5.1 Basic concept.
2.5.2 Chelating and sequestering agents.
2.6 Chemical kinetics.
2.6.1 Basic concept.
2.6.2 Reaction rate laws, orders, and constants.
2.6.3 First and second-order reactions.
2.6.4 Half-life of a reaction.
2.6.5 Dependence on temperature: the arrhenius equation.
2.6.6 Catalysis.
2.7 Chemical thermodynamics and thermochemistry.
2.7.1 Basic concept.
2.7.2 Enthalpy and Hess's law.
2.7.3 The first law and the conservation of energy.
2.7.4 The second law and entropy.
2.7.5 The third law and absolute zero.
2.7.6 Gibbs free energy and the spontaneity of a reaction.
2.8 Electrochemistry and Red-Ox reactions.
2.8.1 Basic concept.
2.8.2 The Nernst equation.
2.8.3 A simple electrochemical cell.
3. Organic chemistry and essentials of polymer chemistry.
3.1 Alkanes, simple carbon chains.
3.1.1 Drawing organic molecules.
3.2 Functional groups.
3.2.1 Alkenes.
3.2.2 Alkynes.
3.2.3 Other groups.
3.2.4 Branches.
3.3 Aromatic compounds.
3.4 Isomers and congeners.
3.5 Essentials of polymer chemistry.
3.5.1 Addition polymers.
3.5.2 Condensation polymers.
3.5.3 Common polymers.
3.5.4 Polymer concerns.
Index.
This book presents the basic principles of chemistry in a quick and clear presentation. All introductory chemistry topics are discussed, as are some organic chemistry topics, which are necessary for a good foundation to understand engineering applications. Readers will find quick and clear explanations, and many solved problems for reference.