Atjaunināt sīkdatņu piekrišanu

Chemistry: Structure and Dynamics 4th Revised edition, Textbook AND Student Solutions Manual [Hardback]

  • Formāts: Hardback, height x width: 284x224 mm, weight: 2175 g
  • Izdošanas datums: 05-Jul-2008
  • Izdevniecība: Wiley-Blackwell
  • ISBN-10: 047041068X
  • ISBN-13: 9780470410684
Citas grāmatas par šo tēmu:
  • Formāts: Hardback, height x width: 284x224 mm, weight: 2175 g
  • Izdošanas datums: 05-Jul-2008
  • Izdevniecība: Wiley-Blackwell
  • ISBN-10: 047041068X
  • ISBN-13: 9780470410684
Citas grāmatas par šo tēmu:
Promote a spirit of scientific discovery


New scientific discoveries do not usually begin with models; they begin with data and a spirit of intellectual curiosity. In much the same way, Spencer, Bodner, and Rickard's Chemistry: Structure & Dynamics, Third Edition presents data, and challenges students to derive the models. Built on the recommendations of the American Chemical Society's Task Force on the General Chemistry Curriculum, this innovative approach helps students get a feel for how chemists approach problems in the real world.


This Third Edition is now revised with a new chapter on materials science and increased coverage of nuclear chemistry.


Here's how it works:
* Data-driven approach: Unlike traditional books that present theory, questions, and then applications, this text starts with the data and derives the theory from it. Students start with observations, just like scientists.
* Concise, flexible format: The text is briefer than most current general chemistry texts. Coverage focuses on the core topics of general chemistry, with optional coverage of special topics also available.
* An emphasis on core themes: These themes include the process of science, the relationship between molecular structure and physical/chemical properties, and the relationship between the microscopic and macroscopic levels.

Also available

Chemistry: A Guided Inquiry, 3rd Edition

By Richard S. Moog and John J. Farrell

ISBN: 0-471-69941-1

Using a classroom-guided inquiry approach, this ideal accompaniment to Chemistry: Structure & Dynamics features 62 ChemActivities covering all the core general chemistry topics. These ChemActivities provide a variety of ways to promote a student-focused, active classroom.
Chapter 1 Elements and Compounds
1(36)
1.1 Chemistry: A Definition
2(1)
1.2 Elements, Compounds, and Mixtures
3(1)
1.3 Atomic Symbols
4(1)
1.4 Chemical Formulas
4(2)
1.5 Evidence for the Existence of Atoms
6(1)
1.6 The Structure of Atoms
7(1)
1.7 Atomic Number and Mass Number
8(1)
1.8 Isotopes
8(2)
1.9 The Difference between Atoms and Ions
10(1)
1.10 Polyatomic Ions
11(1)
1.11 Predicting the Formulas of Ionic Compounds
12(1)
1.12 The Periodic Table
13(2)
1.13 The Macroscopic, Atomic, and Symbolic Worlds of Chemistry
15(1)
1.14 The Mass of an Atom
16(1)
1.15 The Mole as the Bridge between the Macroscopic and Atomic Scales
17(1)
1.16 The Mole as a Collection of Atoms
18(2)
1.17 Converting Grams into Moles and Number of Atoms
20(2)
1.18 The Mole as a Collection of Molecules
22(3)
1.19 Percent by Mass
25(1)
1.20 Determining the Formula of a Compound
26(2)
1.21 Elemental Analysis
28(2)
Problems
30(7)
Chapter 2 The Mole: The Link between the Macroscopic and the Atomic World of Chemistry
37(28)
2.1 Chemical Reactions and the Law of Conservation of Atoms
38(1)
2.2 Chemical Equations as a Representation of Chemical Reactions
38(1)
2.3 Two Views of Chemical Equations: Molecules Versus Moles
39(1)
2.4 Balancing Chemical Equations
40(3)
2.5 Mole Ratios and Chemical Equations
43(2)
2.6 Stoichiometry
45(1)
Chemistry in the World Around Us: The Stoichiometry of the Breathalyzer
46(1)
2.7 The Nuts and Bolts of Limiting Reagents
47(3)
2.8 Density
50(1)
2.9 Solute, Solvent, and Solution
51(1)
2.10 Concentration
52(1)
2.11 Molarity as a Way of Counting Particles in Solution
53(2)
2.12 Dilution Calculations
55(1)
2.13 Solution Stoichiometry
56(4)
Problems
60(5)
Chapter 3 The Structure of the Atom
65(53)
3.1 Rutherford's Model of the Atom
66(1)
3.2 Particles and Waves
67(1)
3.3 Light and Other Forms of Electromagnetic Radiation
68(2)
3.4 Atomic Spectra
70(1)
3.5 Quantization of Energy
71(2)
3.6 The Bohr Model of the Atom
73(1)
3.7 The Energy States of the Hydrogen Atom
74(2)
Chemistry in the World Around Us: Color
76(1)
3.8 The First Ionization Energy
77(2)
3.9 The Shell Model
79(2)
3.10 The Shell Model and the Periodic Table
81(1)
3.11 Photoelectron Spectroscopy and the Structure of Atoms
82(2)
3.12 Electron Configurations from Photoelectron Spectroscopy
84(5)
3.13 Allowed Combinations of Quantum Numbers
89(2)
3.14 Shells and Subshells of Orbitals
91(2)
3.15 Orbitals and the Pauli Exclusion Principle
93(2)
3.16 Predicting Electron Configurations
95(1)
3.17 Electron Configurations and the Periodic Table
96(2)
3.18 Electron Configurations and Hund's Rules
98(1)
3.19 The Sizes of Atoms: Metallic Radii
99(1)
3.20 The Sizes of Atoms: Covalent Radii
100(1)
3.21 The Relative Sizes of Atoms and Their Ions
101(1)
3.22 Patterns in Ionic Radii
102(1)
3.23 Second, Third, Fourth, and Higher Ionization Energies
103(2)
3.24 Average Valence Electron Energy (AVEE)
105(1)
3.25 AVEE and Metallicity
106(1)
Problems
107(11)
Chapter 4 The Covalent Bond
118(55)
4.1 Valence Electrons
119(1)
4.2 The Covalent Bond
120(1)
4.3 How Does the Sharing of Electrons Bond Atoms?
121(1)
4.4 Using Lewis Structures to Understand the Formation of Bonds
122(1)
4.5 Drawing Skeleton Structures
123(1)
4.6 A Step-by-Step Approach to Writing Lewis Structures
124(2)
4.7 Molecules That Don't Seem to Satisfy the Octet Rule
126(4)
4.8 Bond Lengths
130(2)
4.9 Resonance Hybrids
132(2)
4.10 Electronegativity
134(2)
4.11 Partial Charge
136(1)
4.12 Formal Charge
137(3)
4.13 The Shapes of Molecules
140(1)
Chemistry in the World Around Us: The Shapes of Molecules
141(2)
4.14 Predicting the Shapes of Molecules (the Electron Domain Model)
143(2)
4.15 The Role of Nonbonding Electrons in the ED Model
145(4)
4.16 Bond Angles
149(1)
4.17 The Difference Between Polar Bonds and Polar Molecules
150(2)
Problems
152(8)
Special Topics
4A.1 Valence Bond Theory
160(1)
4A.2 Hybrid Atomic Orbitals
161(3)
4A.3 Molecules with Double and Triple Bonds
164(1)
4A.4 Molecular Orbital Theory
165(6)
Problems
171(2)
Chapter 5 Ionic and Metallic Bonds
173(43)
5.1 Metals, Nonmetals, and Semimetals
174(1)
5.2 The Active Metals
174(2)
5.3 Main-Group Metals and Their Ions
176(1)
5.4 Main-Group Nonmetals and Their Ions
177(2)
5.5 Transition Metals and Their Ions
179(1)
Chemistry in the World Around Us: Paints and Pigments
180(1)
5.6 Predicting the Products of Reactions That Produce Ionic Compounds
181(2)
5.7 Oxides, Peroxides, and Superoxides
183(1)
5.8 The Ionic Bond
184(1)
5.9 Structures of Ionic Compounds
185(1)
5.10 Metallic Bonds
186(1)
5.11 The Relationship among Ionic, Covalent, and Metallic Bonds
187(6)
5.12 Bond-Type Triangles
193(3)
5.13 Properties of Metallic, Covalent, and Ionic Compounds
196(1)
5.14 Oxidation Numbers
197(3)
5.15 Calculating Oxidation Numbers
200(3)
5.16 Oxidation-Reduction Reactions
203(1)
5.17 Nomenclature
204(4)
Problems
208(8)
Chapter 6 Gases
216(43)
6.1 Temperature
217(1)
6.2 Temperature as a Property of Matter
218(1)
6.3 The States of Matter
219(1)
6.4 Elements or Compounds That Are Gases at Room Temperature
219(1)
6.5 The Properties of Gases
220(2)
6.6 Pressure versus Force
222(2)
6.7 Atmospheric Pressure
224(2)
6.8 Boyle's Law
226(1)
6.9 Amontons' Law
227(1)
6.10 Charles' Law
228(1)
6.11 Gay-Lussac's Law
229(1)
6.12 Avogadro's Hypothesis
229(2)
6.13 The Ideal Gas Equation
231(1)
6.14 Ideal Gas Calculations: Part I
232(3)
Chemistry in the World Around Us: Nitrous Oxide or "Laughing Gas,"
235(1)
6.15 Ideal Gas Calculations: Part II
236(2)
6.16 Dalton's Law of Partial Pressures
238(3)
6.17 The Kinetic Molecular Theory
241(1)
6.18 How the Kinetic Molecular Theory Explains the Gas Laws
242(3)
Problems
245(8)
Special Topics
6A.1 Graham's Laws of Diffusion and Effusion
253(1)
6A.2 Deviations from Ideal Gas Law Behavior: The van der Waals Equation
254(3)
6A.3 Analysis of the van der Waals Constants
257(1)
Problems
258(1)
Chapter 7 Making and Breaking of Bonds
259(48)
7.1 Energy
260(3)
7.2 Heat
263(1)
7.3 Heat and the Kinetic Molecular Theory
264(1)
7.4 Specific Heat
265(3)
7.5 State Functions
268(1)
7.6 The First Law of Thermodynamics
269(5)
7.7 The Enthalpy of a System
274(2)
7.8 Enthalpies of Reaction
276(3)
7.9 Enthalpy as a State Function
279(2)
7.10 Standard-State Enthalpies of Reaction
281(1)
7.11 Calculating Enthalpies of Reaction
282(1)
7.12 Enthalpies of Atom Combination
283(7)
7.13 Using Enthalpies of Atom Combination to Probe Chemical Reactions
290(3)
7.14 Bond Length and the Enthalpy of Atom Combination
293(1)
7.15 Hess's Law
294(2)
7.16 Enthalpies of Formation
296(3)
Problems
299(8)
Chapter 8 Liquids and Solutions
307(54)
8.1 The Structure of Gases, Liquids, and Solids
308(2)
8.2 Intermolecular Forces
310(4)
8.3 Relative Strengths of Intermolecular Forces
314(4)
8.4 The Kinetic Theory of Liquids
318(1)
8.5 The Vapor Pressure of a Liquid
319(3)
8.6 Melting Point and Freezing Point
322(1)
8.7 Boiling Point
323(3)
8.8 Phase Diagrams
326(1)
8.9 Hydrogen Bonding and the Anomalous Properties of Water
327(1)
8.10 Solutions: Like Dissolves Like
328(3)
8.11 Why Do Some Solids Dissolve in Water?
331(3)
8.12 Solubility Equilibria
334(2)
8.13 Solubility Rules
336(1)
8.14 Net Ionic Equations
337(2)
8.15 Hydrophilic and Hydrophobic Molecules
339(2)
Chemistry in the World Around Us: Soaps, Detergents, and Dry-Cleaning Agents
341(2)
Problems
343(8)
Special Topics
8A.1 Colligative Properties
351(1)
8A.2 Depression of the Partial Pressure of a Solvent
352(3)
8A.3 Boiling Point Elevation
355(2)
8A.4 Freezing Point Depression
357(2)
Problems
359(2)
Chapter 9 Solids
361(42)
9.1 Solids
362(1)
9.2 Molecular and Network Covalent Solids
363(3)
9.3 The Relationship between the Physical Properties of Molecular and Network Covalent Solids
366(1)
9.4 Metallic Solids
367(2)
9.5 Physical Properties That Result from the Structure of Metals
369(1)
9.6 The Structure of Metals
369(3)
9.7 Coordination Numbers and the Structures of Metals
372(1)
9.8 Unit Cells: The Simplest Repeating Unit in a Crystal
373(2)
9.9 Solid Solutions and Intermetallic Compounds
375(1)
9.10 Semimetals
376(1)
9.11 Ionic Solids
376(4)
9.12 The Search for New Materials
380(1)
Chemistry in the World Around Us: The Search for High Temperature Superconductors
381(2)
9.13 Measuring the Distance between Particles in a Unit Cell
383(1)
9.14 Determining the Unit Cell of a Crystal
384(2)
9.15 Calculating the Size of an Atom or Ion
386(1)
Problems
387(5)
Special Topics
9A.1 Defects
392(1)
9A.2 Metals, Semiconductors, and Insulators
393(3)
9A.3 Thermal Conductivity
396(1)
9A.4 Thermal Expansion
397(1)
9A.5 Glass and Other Ceramics
398(4)
Problems
402(1)
Chapter 10 The Connection Between Hinetics and Equilibrium
403(55)
10.1 Reactions That Don't Go to Completion
404(2)
10.2 Gas Phase Reactions
406(2)
10.3 The Rate of a Chemical Reaction
408(2)
10.4 The Collision Theory of Gas Phase Reactions
410(3)
10.5 Equilibrium Constant Expressions
413(4)
10.6 Reaction Quotients: A Way to Decide Whether a Reaction Is at Equilibrium
417(2)
10.7 Changes in Concentration That Occur as a Reaction Comes to Equilibrium
419(5)
10.8 Hidden Assumptions That Make Equilibrium Calculations Easier
424(5)
10.9 The Effect of Temperature on an Equilibrium Constant
429(1)
10.10 Le Chatelier's Principle
429(4)
10.11 Le Chatelier's Principle and the Haber Process
433(1)
10.12 What Happens When a Solid Dissolves in Water?
434(1)
10.13 The Solubility Product Expression
435(1)
10.14 The Relationship between Ksp and the Solubility of a Salt
436(2)
10.15 The Role of the Ion Product (Qsp) in Solubility Calculations
438(2)
10.16 The Common-Ion Effect
440(2)
Problems
442(11)
Special Topics
10A.1 A Rule of Thumb for Testing the Validity of Assumptions
453(2)
10A.2 What Do We Do When the Approximation Fails?
455(2)
Problems
457(1)
Chapter 11 Acids and Bases
458(63)
11.1 Properties of Acids and Bases
459(1)
11.2 The Arrhenius Definition of Acids and Bases
459(1)
11.3 The Brønsted-Lowry Definition of Acids and Bases
460(2)
11.4 Conjugate Acid-Base Pairs
462(2)
11.5 The Role of Water in the Brønsted Model
464(1)
11.6 To What Extent Does Water Dissociate to Form Ions?
465(3)
11.7 pH as a Measure of the Concentration of H3O+ Ion
468(3)
11.8 Relative Strengths of Acids and Bases
471(4)
11.9 Relative Strengths of Conjugate Acid-Base Pairs
475(1)
11.10 Relative Strengths of Different Acids and Bases
475(5)
11.11 Relationship of Structure to Relative Strengths of Acids and Bases
480(3)
11.12 Strong Acid pH Calculations
483(1)
11.13 Weak Acid pH Calculations
484(5)
11.14 Base pH Calculations
489(4)
11.15 Mixtures of Acids and Bases: Buffers
493(1)
11.16 Buffers and Buffer Capacity
494(3)
Chemistry in the World Around Us: Buffers in The Body
497(1)
11.17 Acid-Base Reactions
497(3)
11.18 pH Titration Curves
500(3)
Problems
503(9)
Special Topics
11A.1 Diprotic Acids
512(3)
11A.2 Diprotic Bases
515(3)
11A.3 Compounds That Could Be Either Acids or Bases
518(1)
Problems
519(2)
Chapter 12 Oxidation---Reduction Reactions
521(52)
12.1 Common Oxidation-Reduction Reactions
522(2)
12.2 Determining Oxidation Numbers
524(1)
12.3 Recognizing Oxidation-Reduction Reactions
525(4)
12.4 Voltaic Cells
529(2)
12.5 Oxidizing and Reducing Agents
531(2)
12.6 Relative Strengths of Oxidizing and Reducing Agents
533(4)
12.7 Standard Cell Potentials
537(2)
Chemistry in the World Around Us: Batteries
539(3)
12.8 Electrochemical Cells at Nonstandard Conditions: The Nernst Equation
542(4)
12.9 Electrolysis and Faraday's Law
546(3)
12.10 Balancing Oxidation-Reduction Equations
549(1)
12.11 Redox Reactions in Acidic Solutions
550(3)
12.12 Redox Reactions in Basic Solutions
553(2)
12.13 Molecular Redox Reactions
555(1)
Problems
556(11)
Special Topics
12A.1 Electrolysis of Molten NaCl
567(1)
12A.2 Electrolysis of Aqueous NaCl
568(2)
12A.3 Electrolysis of Water
570(1)
Problems
571(2)
Chapter 13 Chemical Thermodynamics
573(42)
13.1 Spontaneous Chemical and Physical Processes
574(1)
13.2 Entropy and Disorder
575(1)
13.3 Entropy and the Second Law of Thermodynamics
575(4)
13.4 Standard-State Entropies of Reaction
579(1)
13.5 The Third Law of Thermodynamics
579(1)
13.6 Calculating Entropy Changes for Chemical Reactions
580(5)
13.7 Gibbs Free Energy
585(5)
13.8 The Effect of Temperature on the Free Energy of a Reaction
590(2)
13.9 Beware of Oversimplifications
592(1)
13.10 Standard-State Free Energies of Reaction
592(1)
13.11 Equilibria Expressed in Partial Pressures
593(3)
13.12 Interpreting Standard-State Free Energy of Reaction Data
596(1)
13.13 The Relationship Between Free Energy and Equilibrium Constants
597(5)
13.14 The Temperature Dependence of Equilibrium Constants
602(4)
13.15 Gibbs Free Energies of Formation and Absolute Entropies
606(2)
Problems
608(7)
Chapter 14 Hinetics
615(50)
14.1 The Forces That Control a Chemical Reaction
616(1)
14.2 Chemical Kinetics
617(1)
14.3 Is the Rate of Reaction Constant?
618(1)
14.4 Instantaneous Rates of Reaction
619(1)
14.5 Rate Laws and Rate Constants
620(1)
14.6 A Physical Analog of Kinetic Systems
621(1)
14.7 The Rate Law versus the Stoichiometry of a Reaction
622(2)
14.8 Order and Molecularity
624(2)
14.9 A Collision Theory of Chemical Reactions
626(2)
14.10 The Mechanisms of Chemical Reactions
628(2)
14.11 Zero-Order Reactions
630(1)
14.12 Determining the Order of a Reaction from Rates of Reaction
631(2)
14.13 The Integrated Form of Zero-, First-, and Second-Order Rate Laws
633(5)
14.14 Determining the Order of a Reaction with the Integrated Form of Rate Laws
638(3)
14.15 Reactions That Are First Order in Two Reactants
641(1)
14.16 The Activation Energy of Chemical Reactions
642(2)
Chemistry in the World Around Us: NO and NO2 in the Atmosphere
644(2)
14.17 Catalysts and the Rates of Chemical Reactions
646(2)
14.18 Determining the Activation Energy of a Reaction
648(2)
14.19 The Kinetics of Enzyme-Catalyzed Reactions
650(2)
Problems
652(11)
Special Topic
14A.1 Deriving the Integrated Rate Laws
663(2)
Chapter 15 Nuclear Chemistry
665(35)
15.1 Radioactivity
666(1)
15.2 The Structure of the Atom
667(2)
15.3 Modes of Radioactive Decay
669(2)
15.4 Neutron-Rich versus Neutron-Poor Nuclides
671(3)
15.5 Binding Energy Calculations
674(4)
15.6 The Kinetics of Radioactive Decay
678(2)
15.7 Dating by Radioactive Decay
680(2)
15.8 Ionizing versus Nonionizing Radiation
682(1)
15.9 Biological Effects of Ionizing Radiation
683(2)
15.10 Natural versus Induced Radioactivity
685(4)
15.11 Nuclear Fission
689(3)
15.12 Nuclear Fusion
692(1)
15.13 Nuclear Synthesis
693(2)
Chemistry in the World Around Us: Nuclear Medicine
695(2)
Problems
697(3)
Chapter 16 Chemical Analysis
700
16.1 Methods of Analysis
701(1)
16.2 Separation of Mixtures
701(1)
16.3 The Olive Oil Caper
702(4)
16.4 The Great Apple Scare of '89
706(6)
16.5 Fighting Crime with Chemistry
712(5)
16.6 Interaction of Electromagnetic Radiation with Matter: Spectroscopy
717(1)
16.7 The Fox River Mystery
718(3)
16.8 An Off-Color Fatty Alcohol
721(5)
16.9 The Search for New Compounds
726(4)
16.10 The Search for the Northwest Passage---The Franklin Expedition
730(1)
16.11 Dead Cats
731(2)
Problems
733
Appendix A
A.1 Systems of Units
2(2)
English Units of Measurement
2(1)
The Metric System
2(1)
SI Units of Measurement
3(1)
Derived SI Units
3(1)
Non-SI Units
4(1)
A.2 Uncertainty in Measurement
4(2)
Systematic and Random Errors/Accuracy and Precision
5(1)
Accuracy and Precision
6(1)
A.3 Significant Figures
6(3)
Addition and Subtraction with Significant Figures
7(1)
Multiplication and Division with Significant Figures
8(1)
The Difference between Measurements and Definitions
8(1)
Rounding Off
9(1)
A.4 Scientific Notation
9(2)
A.5 The Graphical Treatment of Data
11(3)
A.6 Significant Figures and Unit Conversion Worksheet
14
Significant Figures
14(4)
Unit Conversion
18
Appendix B
Table B.1 Values of Selected Fundamental Constants
2(1)
Table B.2 Selected Conversion Factors
2(1)
Table B.3 The Vapor Pressure of Water
3(1)
Table B.4 Radii of Atoms and Ions
4(2)
Table B.5 Ionization Energies
6(2)
Table B.6 Electron Affinities
8(1)
Table B.7 Electronegativities
9(1)
Table B.8 Acid-Dissociation Equilibrium Constants
10(1)
Table B.9 Base-Ionization Constants
11(1)
Table B.10 Solubility Product Equilibrium Constants
12(1)
Table B.11 Complex Formation Equilibrium Constants
13(1)
Table B.12 Standard Reduction Potentials
14(3)
Table B.13 Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination
17(8)
Table B.14 Bond-Dissociation Enthalpies
25(1)
Table B.15 Electron Configurations of the First 86 Elements
26(2)
Table B.16 Standard-State Enthalpies, Free Energies, and Entropies of Formation
28
Appendix C
Answers to Selected Problems
1(1)
Appendix D
Answers to Checkpoints
1(1)
Photo Credits 1(1)
Index 1