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  • Format: Paperback
  • Copyright: 1992-07-01
  • Publisher: Barrons Educational Series
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This book covers 90 key topics in summary fashion, including chemical equations, atomic structure, phase transitions, acids and bases, and much more. For more than a decade, titles in this handy, quick study series have helped many college freshmen and others taking introductory 101alevel college courses. Designed to be compatible with virtually all standard textbooks in their target subjects, "EZa101 Study Keys" outline and organize subject material so that it resembles classroom lecture notes taken by attentive students. As such, these books provide a general overview of course material, and are ideal for brush-up and review study sessions before taking examinations or writing class papers.

Table of Contents

The science of chemistryp. 1
Fields of chemistryp. 2
The scientific methodp. 3
Measurementsp. 4
The International System of Unitsp. 5
Length and massp. 6
Pressure and temperaturep. 8
Significant figuresp. 10
Conversion factors and dimensional analysisp. 11
Matterp. 13
Pure substancesp. 14
Mixturesp. 15
Chemical and physical changesp. 16
Energyp. 17
Energyp. 18
Kinetic and potential energyp. 19
Electromagnetic radiation and lightp. 20
Wave-particle dualityp. 21
Stoichiometryp. 22
Dalton's atomic theoryp. 23
Atomic and formula massesp. 24
Empirical formulap. 26
Percent compositionp. 28
Chemical equationsp. 29
The equationp. 30
Stoichiometry calculationsp. 31
Limiting reagent, theoretical and percent yieldp. 32
Enthalpy changesp. 33
Atomic structurep. 36
Historical backgroundp. 37
The modern atomp. 38
The Bohr model of the atomp. 39
The wave mechanical picture of the atomp. 40
Quantum numbersp. 41
The electronic structure of atomsp. 42
The periodic tablep. 43
Historical basisp. 44
The modern periodic tablep. 45
Periodic trendsp. 48
The chemical bondp. 49
Ionic bondingp. 50
Covalent bondingp. 51
Lewis structures, resonancep. 52
Bond polarityp. 53
Valence shell electron pair repulsion theoryp. 54
Valence bond theory and hybridizationp. 55
Molecular orbitalsp. 56
Gasesp. 57
The gaseous statep. 58
The gas lawsp. 59
The ideal gas lawp. 61
The kinetic molecular theoryp. 64
Deviations from ideal behaviorp. 65
Solids, liquids, and phase transitionsp. 66
The solid statep. 67
The structure of solidsp. 69
The liquid statep. 70
Intermolecular forcesp. 71
Classification of solidsp. 72
Phase diagramsp. 73
Solutionsp. 74
The dissolving processp. 75
Solubilityp. 77
Concentration expressionsp. 78
Concentration calculationsp. 80
Net ionic equationsp. 82
Solution stoichiometryp. 83
Colligative propertiesp. 85
Chemical equilibriump. 86
The law of chemical equilibriump. 87
The magnitude of the equilibrium constantp. 88
Le Chatelier's principlep. 90
Heterogeneous equilibriap. 92
Acids and basesp. 93
Classification of acids and basesp. 94
Equilibria involving acids and basesp. 96
Acid strengthp. 98
Equilibrium calculationsp. 99
The pH scalep. 100
Reactions of acids and basesp. 101
Titration reactionsp. 102
Buffer solutionsp. 103
Thermodynamicsp. 104
The first law of thermodynamicsp. 105
Entropyp. 106
Free energy and spontaneityp. 107
Free energy and temperaturep. 108
Free energy and equilibriump. 109
Chemical kineticsp. 110
The rates of chemical reactionsp. 111
Time dependence of reactant concentrationsp. 112
Temperature dependence of reaction ratep. 114
Reaction mechanismp. 116
Oxidation-reduction reactions and electrochemistryp. 117
Oxidation statesp. 118
Oxidation-reduction reactionsp. 119
Balancing oxidation-reduction equationsp. 120
Galvanic electrochemical cellsp. 121
Standard half-cell potentialsp. 122
Spontaneity of oxidation-reduction reactionsp. 123
The Nernst equationp. 125
Electrolytic cellsp. 126
Organic chemistryp. 127
Alkanesp. 128
Alkenes and alkynesp. 129
Aromatic hydrocarbonsp. 130
Functional groupsp. 132
Isomers and optical activityp. 133
Glossaryp. 135
Indexp. 153
Table of Contents provided by Syndetics. All Rights Reserved.

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