Rapid Review of Chemistry for the Life Sciences and Engineering: With Select Applications

Cover
Half Title
Title Page
Copyright Page
Dedication
Table of Contents
Foreword
Preface
Authors
List of Solved Examples
Chapter 1 Introduction
	1.1 The Basics of Matter
	1.2 The Periodic Table: Basic Concepts, 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 Chemical Formulas
	1.4 Chemical Bonding
	1.5 Calculating Molar Masses and Avogadro’s Principle
	1.6 Determining the Percent Composition of a Compound
	1.7 Determining Empirical and Molecular Formulas from Percent Composition
	1.8 Solubility and Concentration Units for Aqueous Solutions
	1.9 Properties of Gases and the Gas Laws
		1.9.1 The Kinetic-Molecular Theory of Gases
		1.9.2 The General Gas Law
		1.9.3 The Ideal Gas Law
		1.9.4 Dalton’s Law of Partial Pressures
		1.9.5 Graham’s Law of Effusion
		1.9.6 Intermolecular Forces
			1.9.6.1 Two Special Cases
Chapter 2 Simple Categories of Inorganic Chemical Reactions
	2.1 Five General Categories of Chemical Reactions
	2.2 Oxidation–Reduction or RED-OX Reactions
	2.3 Writing and Balancing Chemical Reactions
	2.4 Simple Stoichiometry
		2.4.1 An Illustrative Example of a Decomposition Reaction—An Explosion
	2.5 Limiting Reagent
		2.5.1 Percent Yield
	2.6 Consecutive and Simultaneous Reactions
	2.7 Energy Change for Exothermic vs. Endothermic Reactions
Chapter 3 Acids, Bases, and Salts
	3.1 Acids and Bases
	3.2 Concentration Units and the pH Scale
	3.3 Calculations for Strong Acids and Bases
	3.4 Salts and Colligative Properties
	3.5 Boiling-Point Elevation
	3.6 Freezing-Point Depression
	3.7 Henry’s Law
	3.8 Raoult’s Law for Vapor-Pressure Lowering
	3.9 Osmotic Pressure
	3.10 Colloids: Dispersions and Suspensions
Chapter 4 Chemical Equilibrium
	4.1 Basic Concept
	4.2 The Meaning of K[sub(c)]
	4.3 Calculations for K[sub(c)]
	4.4 Predicting Equilibrium Using a Test Quotient
	4.5 Stresses and Le Chatelier’s Principle
	4.6 Dependence of K[sub(c)] on Temperature
	4.7 Calculations Involving Weak Acids and Bases
	4.8 Hydrolysis
	4.9 Buffer Solutions and the Henderson–Hasselbalch Equation
	4.10 Amphoterism
	4.11 Solubility Product Constants
	4.12 Definition of Solubility Product Constant K[sub(sp)]
	4.13 Calculating the Molar Solubility from K[sub(sp)]
	4.14 Common and Uncommon Ion and pH Effects
	4.15 Predicting Precipitation
	4.16 Complex Ion Formation
	4.17 Chelating and Sequestering Agents
Chapter 5 Chemical Thermodynamics and Thermochemistry
	5.1 Basic Concept
	5.2 Enthalpy and Hess’s Law
	5.3 The First Law and the Conservation of Energy
	5.4 The Second Law and Entropy
	5.5 The Third Law and Absolute Zero
	5.6 Gibbs Free Energy and the Spontaneity of a Reaction
Chapter 6 Chemical Kinetics
	6.1 Basic Concept
	6.2 Reaction Rate Laws, Orders, and Constants
	6.3 First- and Second-Order Reactions
	6.4 Half-Life of a Reaction
	6.5 Dependence on Temperature: The Arrhenius Equation
	6.6 Catalysis
Chapter 7 Electrochemistry and RED-OX Reactions
	7.1 Basic Concept
	7.2 The Nernst Equation
	7.3 A Simple Electrochemical Cell
		7.3.1 Useful Quantitative Relationships
Chapter 8 Organic Chemistry: Naming, Structure, and Isomerism
	8.1 Organic Compounds Compared to Inorganic Compounds
	8.2 The Need for Knowledge of Organic Chemistry
	8.3 Hydrocarbons: Aliphatic and Aromatic Hydrocarbons
		8.3.1 Alkanes
		8.3.2 Alkenes
		8.3.3 Alkynes
		8.3.4 Aromatic Hydrocarbons
		8.3.5 Cyclic Nonaromatic Hydrocarbons
	8.4 Structural Representation of Organic Compounds
	8.5 Naming Organic Compounds
	8.6 Isomers and Congeners
	8.7 Biofuels
Chapter 9 Asymmetric Centers, Functional Groups, and Characterization
	9.1 Asymmetric Centers: Enantiomers and Diastereomers
	9.2 Separation of Enantiomers
	9.3 Further Classification of Organic Compounds—Functional Groups
	9.4 Some Common Products and Functional Groups
	9.5 Structural Analysis
		9.5.1 Nuclear Magnetic Resonance (or NMR) Spectroscopy
		9.5.2 Infrared (or IR) Spectroscopy
		9.5.3 Mass Spectroscopy (or MS)
		9.5.4 Gas Chromatography–Mass Spectroscopy (or GC–MS) and High-Performance Liquid Chromatography (or HPLC)
	9.6 Organic Solvents
Chapter 10 The Essentials of Polymer Chemistry
	10.1 The Basics
	10.2 Addition Polymers
	10.3 Condensation Polymers
	10.4 Common Polymers
	10.5 Polymer Types
	10.6 Polymer Problems
	10.7 Plastic Waste and the Recycling of Plastics
	10.8 The Problem of Microplastics
Chapter 11 Radioactivity and Nuclear Chemistry
	11.1 Types of Radioactivity
	11.2 Half-Life
	11.3 Units of Radiation
		11.3.1 Decay Rate
		11.3.2 Absorbed Radiation
		11.3.3 Radiation Exposures
	11.4 Radiation in the Field: Decay Series of Uranium
Chapter 12 The Atmosphere and the Chemistry of Air
	12.1 The Composition of the Atmosphere
	12.2 Definitions of Gases, Fumes, Vapors, Aerosols, and Mists
	12.3 Primary Air Pollutants from Stationary and Mobile Sources
		12.3.1 Carbon Dioxide
		12.3.2 Sources of Carbon Dioxide
		12.3.3 Carbon Dioxide and Global Warming
		12.3.4 SOx and NOx
		12.3.5 Ozone
		12.3.6 Photochemical Smog
		12.3.7 Fly Ash and Related Environmental Hazards
	12.4 Indoor Air Quality (IAQ)
	12.5 Eight Major Indoor Air Pollutants
Chapter 13 Water Quality and Water Pollution
	13.1 Chemistry of Water: Summary of Chemical and Physical Properties
	13.2 Solutes, Solvents, and Solutions
	13.3 Colloids
	13.4 Common Sources of Contamination of Water Supplies
	13.5 COD and BOD
		13.5.1 COD Measurements
		13.5.2 Biochemical Oxygen Demand
	13.6 Carbon Dioxide Pollution
	13.7 Environmental Fate and Transport of Selected Water Pollutants
		13.7.1 DDT
		13.7.2 Pharmaceutical Pollution
		13.7.3 Dioxins
Chapter 14 The Chemistry of Hazardous Materials
	14.1 Background
	14.2 The Chemistry of Four Common Elements
		14.2.1 Hydrogen
		14.2.2 Oxygen
		14.2.3 Chlorine
		14.2.4 Sulfur
	14.3 The Chemistry of Some Corrosive Materials
		14.3.1 The Nature of Corrosivity
		14.3.2 The Nature and Properties of Acids and Bases
		14.3.3 Select Weak Acids of Interest
		14.3.4 Select Bases of Interest
		14.3.5 Anhydrides of Acids and Bases
	14.4 The Chemistry of Pyrophoric Substances
	14.5 The Chemistry of Flammable Substances
		14.5.1 OSHA Classification System
		14.5.2 NFPA Classification System
	14.6 The Chemistry of Explosives
	14.7 Green Chemistry
	14.8 Nanotechnology
	14.9 Three Important “Environmental” Disasters
		14.9.1 West Virginia MCHM Leak of 2014
		14.9.2 British Petroleum and the Deepwater Horizon Accident of 2010
		14.9.3 Union Carbide and Bhopal, India of 1984—The Worst Chemical Accident Ever
Chapter 15 Introduction to Basic Toxicology
	15.1 The Problem
		15.1.1 Five Immediate Conclusions
	15.2 Basic Concepts
	15.3 More Terms and Definitions
	15.4 The Dose–Response Relationship
	15.5 Multiple Chemical Sensitivity (MCS) Syndrome
	15.6 Pesticides: Two Examples—Atrazine, Arsenic
		15.6.1 Atrazine
		15.6.2 The Persistence of Arsenic—A Crossover Chemical—A Pesticide and More
	15.7 Endocrine-Disrupting Chemicals (EDCs): BPA, DEHP, and DOP
	15.8 Emerging Contaminants: Two Examples—1,4 Dioxane, and Per and Poly Fluorinated Alkyl Substances (PFAS)
		15.8.1 1 ,4 Dioxane
		15.8.2 Perfluoroalkyl and Polyfluoroalkyl Substances—PFAS
	15.9 Three Examples of Calculations or Conversions
Appendix A
Appendix B
Appendix C
Appendix D
Appendix E
Bibliography
Index