Buch, Englisch, 256 Seiten, Format (B × H): 221 mm x 276 mm, Gewicht: 652 g
Buch, Englisch, 256 Seiten, Format (B × H): 221 mm x 276 mm, Gewicht: 652 g
ISBN: 978-1-394-32119-3
Verlag: Wiley John + Sons
Enables students to understand, apply, and retain key concepts in general chemistry
Understanding Essential Chemistry offers a unique and approachable supplement to standard general chemistry textbooks, designed specifically to aid students in mastering fundamental principles. Drawing on extensive classroom experience, chemistry professor Max Diem presents key concepts in an uninterrupted flow, allowing students to follow a clear and straightforward path to comprehension. With a logical, algebraic framework, the book is structured to build students’ confidence by breaking down complex topics into manageable pieces and encouraging critical thinking at every step.
Aimed at STEM majors, this book includes checkpoints with example problems and final answers to reinforce concepts and promote independent problem-solving skills. By methodically emphasizing basic understanding, this hands-on guide gives students the tools to grasp the core chemistry principles necessary for success in their courses, labs, and future studies. A must-have “survival guide” to boost student confidence in the subject, the text: - Presents chemistry concepts in a streamlined, continuous format for easier comprehension and retention
- Encourages independent critical thinking with targeted example problems with provided solutions
- Supports any primary general chemistry textbook, making it adaptable for various curricula
- Allows students to assess their understanding at key points in the material
- Includes additional math tutorials in the Chapter for students needing a refresher in essential mathematical skills
This guide is an essential supplement for undergraduate first-year Chemistry courses for STEM majors, especially those in pre-medical, engineering, and science programs.
Autoren/Hrsg.
Fachgebiete
Weitere Infos & Material
Preface xi
About the Companion Website xiii
1 The Metric System and Mathematical Tools 1
1.1 Scientific Notation and Significant Figures 1
1.2 The Metric System 2
1.3 Manipulations of Exponential Expressions 4
1.4 Equations, Proportionality, and Graphs 5
1.5 Quadratic, Cubic, and Quartic Equations 7
1.6 Exponential Functions and Logarithms 8
1.7 Radial and Spherical Polar Coordinates 11
1.8 Differential and Integral Calculus 12
1.9 Differential Equations 14
1.10 Complex Numbers 15
2 Atoms, Elements, and the Periodic System 17
2.1 Subatomic Particles and Atoms 17
2.2 Elements, Isotopes, and Ions 18
2.3 The Periodic Chart and Periodic Properties of the Elements 21
2.4 Definition of Atomic Masses, Avogadro’s Number, and the Mole 26
Further Reading 28
3 Molecules, Compounds, Bonding, and Percent Composition 29
3.1 Ionic Compounds 29
3.2 Molecules with Covalent Bonds 30
3.3 Molecules with Polar Covalent Bonds and Lewis Structures 31
3.4 Molecular Compounds and the (Gram) Molecular Mass 37
3.5 Percent Composition and Empirical Formulae 38
Further Reading 39
4 Chemical Reactions 41
4.1 Chemical Reaction and Stoichiometry 41
4.2 Limiting Reagents, Theoretical Yield, and Percent Yield 42
4.3 Solutions: General Aspects 43
4.4 Solution Stoichiometry: Molarity, Molality, Mole Fraction, Dilutions 45
4.5 Precipitation Reactions 47
Further Reading 49
5 Electronic Structure of Atoms 51
5.1 Description of Light as an Electromagnetic Wave 51
5.2 Particle Properties of Light and Wave-particle Duality 52
5.3 The Hydrogen Atom Emission Spectrum: Stationary Atomic States 55
5.4 Hydrogen Atom Orbitals 58
5.5 Atoms with Multiple Electrons: The Aufbau Principle Revisited 62
Further Reading 67
6 Chemical Bonding: Covalent Bonding, Molecular Geometries, and Polarity 69
6.1 General Aspects of Covalent Bonding 69
6.2 Lewis and VB Theory 69
6.3 Hybridization and Multiple Bonding 70
6.4 VSEPR Model 73
6.5 Molecular Polarity 75
6.6 MO Theory 76
Further Reading 81
7 Solids and Liquids: Bonding and Characteristics 83
7.1 Metals and Semiconductors 83
7.2 Ionic Solids 85
7.3 Covalent Solids 86
7.4 Intermolecular Forces 87
7.4.1 Hydrogen Bonding 87
7.4.2 Dipole–Dipole Interactions 88
7.4.3 London Dispersion Forces (Induced Dipole Forces) 89
7.5 Macromolecular Solids 89
7.6 Liquids and Solutions 90
7.6.1 General Aspects of Solutions and Solvation 90
7.6.2 Colligative Properties 90
Further Reading 93
8 The Gaseous State 95
8.1 General Properties of Gases 95
8.2 Empirical Gas Laws 97
8.3 The Ideal Gas Law 99
8.4 Real Gases 100
8.5 Gaseous Mixtures and Partial Pressures 101
8.6 Kinetic Theory of Gases 102
8.7 Diffusion and Effusion of Gases 104
Further Reading 106
9 Chemical Equilibrium 107
9.1 What Is a System “at Equilibrium”? 107
9.2 Liquid–Vapor Phase Equilibrium: Vapor Pressure 108
9.3 Temperature Dependence of Vapor Pressure 110
9.4 Chemical Equilibrium and the Equilibrium Constant 113
9.5 Equilibrium Calculations 115
9.6 Direction of a Chemical Reaction and the Concentration Quotient Q 119
9.7 Numerical Determination of Equilibrium Constants from Experimental Data 120
9.8 Perturbations of Equilibria: Le Chatelier’s Principle 120
9.9 Solubility and Solubility Product 122
9.9.1 The Solubility Product Constant, Ksp 123
9.9.2 Solubility Calculations 123
9.9.3 Common Ion Effect 124
9.9.4 Experimental Determination of Ksp 125
9.9.5 Precipitation Reactions 126
Further Reading 127
10 Acids and Bases 129
10.1 What Are Acids/Bases? 129
10.2 Strong Acids and Bases; Definition of pH and pOH 130
10.3 Weak Acids/Bases 131
10.4 The Relationship Between pH and pOH: Self-dissociation of Water 134
10.5 Common Ion Effect 135
10.6 Acidic and Basic Salts 136
10.7 Buffers 138
10.8 Acid–Base Titrations 140
10.8.1 Titration of a Strong Acid with a Strong Base 141
10.8.2 Titration of a Weak Acid with a Strong Base 143
10.8.3 Acid–Base Indicators 145
Further Reading 146
11 Thermodynamics: Energy, Energy Conversions, and Spontaneity 147
11.1 Energetics of Chemical Reactions 147
11.2 Thermochemistry 147
11.2.1 Definition of Energy, Work, and Heat 147
11.2.2 Calorimetry: Measurement of Heat Flow 150
11.3 The First Law of Thermodynamics 152
11.4 State Functions 153
11.5 Definition of Enthalpy 153
11.6 Hess’ Law and Reaction Enthalpies 154
11.6.1 Enthalpy of Crystal Formation: Lattice Energy of MgO 156
11.7 Enthalpy of Phase Transitions 157
11.8 Entropy 158
11.8.1 Entropy and Probability 161
11.8.2 Entropy and Heat Flow 162
11.8.3 Entropy as an Indicator of Energy Exhaustion 163
11.9 Free Enthalpy 164
11.10 Free Enthalpy and Equilibrium 165
Further Reading 168
12 Reduction–Oxidation (Redox) Reactions and Electrochemistry 169
12.1 Oxidation State and Oxidation Numbers: Balancing Redox Equations 170
12.2 Galvanic Cells, Electric Work, and Electromotive Force 173
12.3 Batteries 177
12.3.1 Alkaline Dry Cell (AA Battery) 177
12.3.2 Lead–Acid Battery 178
12.3.3 Lithium-ion Battery 180
12.4 Relationship Between Cell Potential and Free Enthalpy 181
12.5 Concentration and Temperature Dependence of EMF 181
Further Reading 183
13 Chemical Kinetics: Rates of Reactions and Reaction Mechanisms 185
13.1 Scope of K
