Schaum's Outline of Beginning Chemistry (Third Edition) / Edition 3

by David Goldberg

Overview

Students love Schaum's Outlines because they produce results. Each year, hundreds of thousands of students improve their test scores and final grades with these indispensable study guides. Get the edge on your classmates. Use Schaum's!

Having difficulty understanding basic concepts and turning knowledge into problem-solving skills? This book helps you: Brush up before tests, Find answers fast, Study quickly and more effectively, Get the big picture without spending hours poring over lengthy textbooks.

Schaum's Outlines give you the information your teachers expect you to know in a handy and succinct format-without overwhelming you with unnecessary detail. You get a complete overview of the subject. Plus, you get plenty of practice exercises to test your skill. Compatible with any classroom text, Schaum's let you study at your own pace and remind you of all the important facts you need to remember-fast! And Schaum's are so complete, they're perfect for preparing for graduate or professional exams.

Product Details

ISBN-13:	9780071447805
Publisher:	McGraw-Hill Companies, The
Publication date:	12/10/2004
Series:	Schaum's Outline Series
Edition description:	Third Edition
Pages:	384
Product dimensions:	8.10(w) x 10.80(h) x 0.54(d)

About the Author

David E. Goldberg, Ph.D. was a professor of chemistry at Brooklyn College in New York City and is the author of the McGraw-Hill Science/Engineering/Math textbook Fundamentals of Chemistry, Fourth Edition. He is also the author of Chemistry: Reactions, Structure, and Properties.

Table of Contents

Chapter 1	Basic Concepts	1
1.1	Introduction	1
1.2	The Elements	1
1.3	Matter and Energy	2
1.4	Properties	3
1.5	Classification of Matter	3
1.6	Representation of Elements	5
1.7	Laws, Hypotheses, and Theories	6
Chapter 2	Mathematical Methods in Chemistry	10
2.1	Introduction	10
2.2	Factor-Label Method	10
2.3	Metric System	12
2.4	Exponential Numbers	16
2.5	Significant Digits	17
2.6	Density	21
2.7	Temperature Scales	23
Chapter 3	Atoms and Atomic Masses	38
3.1	Introduction	38
3.2	Atomic Theory	38
3.3	Atomic Masses	39
3.4	Atomic Structure	40
3.5	Isotopes	41
3.6	Periodic Table	42
Chapter 4	Electronic Configuration of the Atom	51
4.1	Introduction	51
4.2	Bohr Theory	51
4.3	Quantum Numbers	53
4.4	Quantum Numbers and Energies of Electrons	54
4.5	Shells, Subshells, and Orbitals	55
4.6	Shapes of Orbitals	58
4.7	Buildup Principle	58
4.8	Electronic Structure and the Periodic Table	60
Chapter 5	Chemical Bonding	67
5.1	Introduction	67
5.2	Chemical Formulas	67
5.3	The Octet Rule	68
5.4	Ions	69
5.5	Electron Dot Notation	71
5.6	Covalent Bonding	72
5.7	Distinction Between Ionic and Covalent Bonding	74
5.8	Predicting the Nature of Bonding in Compounds	75
5.9	Detailed Electronic Configurations of Ions (Optional)	76
Chapter 6	Inorganic Nomenclature	86
6.1	Introduction	86
6.2	Binary Compounds of Nonmetals	87
6.3	Naming Ionic Compounds	88
6.4	Naming Inorganic Acids	93
6.5	Acid Salts	94
6.6	Hydrates	94
Chapter 7	Formula Calculations	102
7.1	Introduction	102
7.2	Molecules and Formula Units	102
7.3	Formula Masses	103
7.4	The Mole	103
7.5	Percent Composition of Compounds	106
7.6	Empirical Formulas	107
7.7	Molecular Formulas	108
Chapter 8	Chemical Equations	120
8.1	Introduction	120
8.2	Balancing Simple Equations	121
8.3	Predicting the Products of a Reaction	122
Chapter 9	Net Ionic Equations	134
9.1	Introduction	134
9.2	Writing Net Ionic Equations	134
Chapter 10	Stoichiometry	142
10.1	Mole-to-Mole Calculations	142
10.2	Calculations Involving Other Quantities	143
10.3	Limiting Quantities	144
10.4	Calculations Based on Net Ionic Equations	147
10.5	Heat Capacity and Heat of Reaction	147
Chapter 11	Molarity	162
11.1	Introduction	162
11.2	Molarity Calculations	162
11.3	Titration	164
11.4	Stoichiometry in Solution	166
Chapter 12	Gases	173
12.1	Introduction	173
12.2	Pressure of Gases	173
12.3	Boyle's Law	174
12.4	Graphical Representation of Data	175
12.5	Charles' Law	177
12.6	The Combined Gas Law	180
12.7	The Ideal Gas Law	181
12.8	Dalton's Law of Partial Pressures	183
Chapter 13	Kinetic Molecular Theory	195
13.1	Introduction	195
13.2	Postulates of the Kinetic Molecular Theory	195
13.3	Explanation of Gas Pressure, Boyle's Law, and Charles' Law	196
13.4	Graham's Law	197
Chapter 14	Oxidation and Reduction	201
14.1	Introduction	201
14.2	Assigning Oxidation Numbers	201
14.3	Periodic Relationships of Oxidation Numbers	203
14.4	Oxidation Numbers in Inorganic Nomenclature	205
14.5	Balancing Oxidation-Reduction Equations	205
14.6	Electrochemistry	209
Chapter 15	Solutions	219
15.1	Qualitative Concentration Terms	219
15.2	Molality	219
15.3	Mole Fraction	220
15.4	Equivalents	221
15.5	Normality	222
15.6	Equivalent Mass	223
Chapter 16	Rates and Equilibrium	230
16.1	Introduction	230
16.2	Rates of Chemical Reaction	230
16.3	Chemical Equilibrium	232
16.4	Equilibrium Constants	234
Chapter 17	Acid-Base Theory	246
17.1	Introduction	246
17.2	The Bronsted-Lowry Theory	246
17.3	Acid-Base Equilibrium	248
17.4	Autoionization of Water	249
17.5	The pH Scale	250
17.6	Buffer Solutions	251
Chapter 18	Organic Chemistry	261
18.1	Introduction	261
18.2	Bonding in Organic Compounds	261
18.3	Structural, Condensed, and Line Formulas	262
18.4	Hydrocarbons	264
18.5	Isomerism	266
18.6	Radicals and Functional Groups	267
18.7	Alcohols	269
18.8	Ethers	270
18.9	Aldehydes and Ketones	271
18.10	Acids and Esters	271
18.11	Amines	272
18.12	Amides	272
Chapter 19	Nuclear Reactions	280
19.1	Introduction	280
19.2	Natural Radioactivity	280
19.3	Half-Life	282
19.4	Radioactive Series	283
19.5	Nuclear Fission and Fusion	284
19.6	Nuclear Energy	285
Appendix	Scientific Calculations	292
A.1	Scientific Algebra	292
A.2	Calculator Mathematics	297
	Glossary	312
	Practice Quizzes	326
	Answers to Quizzes	330
	Index	335
	Conversions	348
	Table of the Elements	349
	Periodic Table	350