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Chemistry: Structure and Dynamics 5th edition [Hardback]

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(Franklin and Marshall College), (Purdue University), (Millersville University)
  • Formāts: Hardback, 928 pages, height x width x depth: 282x218x36 mm, weight: 2245 g
  • Izdošanas datums: 04-Mar-2011
  • Izdevniecība: John Wiley & Sons Inc
  • ISBN-10: 0470587113
  • ISBN-13: 9780470587119
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Chemistry: Structure and Dynamics 5th editionPalielināt
  • Formāts: Hardback, 928 pages, height x width x depth: 282x218x36 mm, weight: 2245 g
  • Izdošanas datums: 04-Mar-2011
  • Izdevniecība: John Wiley & Sons Inc
  • ISBN-10: 0470587113
  • ISBN-13: 9780470587119
Citas grāmatas par šo tēmu:
Permanent link: https://www.kriso.lv/db/9780470587119.html
Keywords:
The Spencer text is the only text that is built on independently researched pedagogy on the best way to teach General Chemistry. Chemistry: Structure and Dynamics, 5th Edition emphasizes deep understanding rather than comprehensive coverage along with a focus on the development of inquiry and reasoning skills. While most mainstream General Chemistry texts offer a breadth of content coverage, the Spencer author team, in contrast, focuses on depth and reader preparation for future studies.

The fifth edition is revised in keeping with our commitment to the chemical education community and specifically the POGIL (Process Oriented Guided Inquiry Learning) Project. This text reflects two core principles, first that the concepts that are covered are fundamental building blocks for understanding chemistry and second, that the concepts should be perceived by the readers as being directly applicable to their interests and careers. The authors further provide this "core" coverage using 1 of 3 models; data-driven, chemical theories and reader understanding, which allows for a more concrete foundation on which readers build conceptual understanding.

Chapter 1 Elements and Compounds
1(30)
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
5(1)
1.5 Evidence for the Existence of Atoms
6(1)
1.6 The Role of Measurement in Chemistry
7(2)
1.7 The Structure of Atoms
9(2)
1.8 Atomic Number and Mass Number
11(1)
1.9 Isotopes
12(2)
1.10 The Difference Between Atoms and Ions
14(2)
1.11 Polyatomic Ions
16(1)
1.12 The Periodic Table
16(2)
1.13 The Macroscopic, Atomic and Symbolic Worlds of Chemistry
18(1)
1.14 The Mass of an Atom
19(2)
1.15 Chemical Reactions and the Law of Conservation of Atoms
21(1)
1.16 Chemical Equations as a Representation of Chemical Reactions
21(1)
1.17 Balancing Chemical Equations
22(9)
Chapter 2 The Mole: The Link between the Macroscopic and the Atomic Worlds of Chemistry
31(40)
2.1 The Mole as the Bridge Between the Macroscopic and Atomic Scales
32(1)
2.2 The Mole as a Collection of Atoms
33(2)
2.3 Converting Grams into Moles and Number of Atoms
35(2)
2.4 The Mole as a Collection of Molecules
37(3)
2.5 Percent by Mass
40(1)
2.6 Determining the Formula of a Compound
41(4)
2.7 Two Views of Chemical Equations: Molecules Versus Moles
45(1)
2.8 Mole Ratios and Chemical Equations
46(2)
2.9 Stoichiometry
48(1)
2.10 The Stoichiometry of the Breathalyzer
49(1)
2.11 The Nuts and Bolts of Limiting Reagents
50(3)
2.12 Density
53(1)
2.13 Solute, Solvent, and Solution
54(1)
2.14 Concentration
55(1)
2.15 Molarity as a Way to Count Particles in a Solution
56(2)
2.16 Dilution Calculations
58(1)
2.17 Solution Stoichiometry
59(12)
Problems
63(8)
Chapter 3 The Structure of the Atom
71(52)
3.1 Rutherford's Model of the Atom
72(1)
3.2 Particles and Waves
73(1)
3.3 Light and Other Forms of Electromagnetic Radiation
74(2)
3.4 Atomic Spectra
76(1)
3.5 The Wave-Packet Model of Electromagnetic Radiation
77(2)
3.6 The Bohr Model of the Atom
79(1)
3.7 The Energy States of the Hydrogen Atom
80(2)
3.8 Electromagnetic Radiation and Color
82(1)
3.9 The First Ionization Energy
83(2)
3.10 The Shell Model
85(2)
3.11 The Shell Model and the Periodic Table
87(1)
3.12 Photoelectron Spectroscopy and the Structure of Atoms
88(1)
3.13 Electron Configurations from Photoelectron Spectroscopy
89(6)
3.14 Allowed Combinations of Quantum Numbers
95(1)
3.15 Shells and Subshells of Orbitals
96(2)
3.16 Orbitals and the Pauli Exclusion Principle
98(2)
3.17 Predicting Electron Configurations
100(1)
3.18 Electron Configurations and the Periodic Table
101(1)
3.19 Electron Configurations and Hund's Rules
102(2)
3.20 The Sizes of Atoms: Metallic Radii
104(1)
3.21 The Sizes of Atoms: Covalent Radii
104(1)
3.22 The Relative Sizes of Atoms and Their Ions
105(2)
3.23 Patterns in Ionic Radii
107(1)
3.24 Second, Third, Fourth, and Higher Ionization Energies
108(2)
3.25 Average Valence Electron Energy (AVEE)
110(1)
3.26 AVEE and Metallicity
111(12)
Problems
113(10)
Chapter 4 The Covalent Bond
123(54)
4.1 Valence Electrons
124(1)
4.2 The Covalent Bond
125(1)
4.3 How Does the Sharing of Electrons Bond Atoms?
126(1)
4.4 Using Lewis Structures to Understand the Formation of Bonds
127(1)
4.5 Drawing Skeleton Structures
128(1)
4.6 A Step-by-Step Approach to Writing Lewis Structures
129(2)
4.7 Molecules That Don't Seem to Satisfy the Octet Rule
131(3)
4.8 Bond Lengths
134(2)
4.9 Resonance Hybrids
136(3)
4.10 Electronegativity
139(2)
4.11 Partial Charge
141(1)
4.12 Formal Charge
142(3)
4.13 The Shapes of Molecules
145(3)
4.14 Predicting the Shapes of Molecules (The Electron Domain Model)
148(3)
4.15 The Role of Nonbonding Electrons in the ED Model
151(3)
4.16 Bond Angles
154(2)
4.17 The Difference Between Polar Bonds and Polar Molecules
156(21)
Problems
158(7)
Special Topics
4A.1 Valence Bond Theory
165(1)
4A.2 Hybrid Atomic Orbitals
166(3)
4A.3 Molecules with Double and Triple Bonds
169(1)
4A.4 Molecular Orbital Theory
170(6)
Problems
176(1)
Chapter 5 Ionic and Metallic Bonds
177(44)
5.1 Metals, Nonmetals, and Semimetals
178(1)
5.2 The Active Metals
178(2)
5.3 Main-Group Metals and Their Ions
180(1)
5.4 Main-Group Nonmetals and Their Ions
181(3)
5.5 Transition Metals and Their Ions
184(1)
5.6 Chemistry and Color
184(1)
5.7 Predicting the Formulas of Ionic Compounds
185(1)
5.8 Predicting the Products of Reactions That Produce Ionic Compounds
186(2)
5.9 Oxides, Peroxides, and Superoxides
188(1)
5.10 The Ionic Bond
189(1)
5.11 Structures of Ionic Compounds
190(1)
5.12 Metallic Bonds
191(1)
5.13 The Relationship among Ionic, Covalent, and Metallic Bonds
192(5)
5.14 Bond-Type Triangles
197(4)
5.15 Properties of Metallic, Covalent, and Ionic Compounds
201(1)
5.16 Oxidation Numbers
201(3)
5.17 Calculating Oxidation Numbers
204(3)
5.18 Oxidation-Reduction Reactions
207(2)
5.19 Nomenclature
209(12)
Problems
213(8)
Chapter 6 Gases
221(43)
6.1 Temperature
222(1)
6.2 Temperature as a Property of Matter
223(1)
6.3 The States of Matter
224(1)
6.4 Elements or Compounds That Are Gases at Room Temperature
225(1)
6.5 The Properties of Gases
226(1)
6.6 Pressure versus Force
227(2)
6.7 Atmospheric Pressure
229(2)
6.8 Boyle's Law
231(1)
6.9 Amontons' Law
232(1)
6.10 Charles' Law
233(1)
6.11 Gay-Lussac's Law
234(1)
6.12 Avogadro's Hypothesis
234(2)
6.13 The Ideal Gas Equation
236(1)
6.14 Dalton's Law of Partial Pressures
237(3)
6.15 Ideal Gas Calculations: Part I
240(4)
6.16 Ideal Gas Calculations: Part II
244(2)
6.17 The Kinetic Molecular Theory
246(1)
6.18 How the Kinetic Molecular Theory Explains the Gas Laws
247(3)
6.19 Graham's Laws of Diffusion and Effusion
250(14)
Problems
252(7)
Special Topics
6A.1 Deviations from Ideal Gas Law Behavior: The van der Waals Equation
259(3)
6A.2 Analysis of the van der Waals Constants
262(1)
Problems
263(1)
Chapter 7 Making and Breaking of Bonds
264(49)
7.1 Energy
265(3)
7.2 Heat
268(1)
7.3 Heat and the Kinetic Molecular Theory
268(1)
7.4 Specific Heat
269(4)
7.5 State Functions
273(1)
7.6 The First Law of Thermodynamics
274(2)
7.7 Work
276(4)
7.8 The Enthalpy of a System
280(2)
7.9 Enthalpies of Reaction
282(3)
7.10 Enthalpy as a State Function
285(2)
7.11 Standard-State Enthalpies of Reaction
287(1)
7.12 Calculating Enthalpies of Reaction
288(1)
7.13 Enthalpies of Atom Combination
289(7)
7.14 Using Enthalpies of Atom Combination to Probe Chemical Reactions
296(3)
7.15 Bond Length and the Enthalpy of Atom Combination
299(1)
7.16 Hess's Law
300(1)
7.17 Enthalpies of Formation
301(12)
Problems
305(8)
Chapter 8 Liquids and Solutions
313(54)
8.1 The Structure of Gases, Liquids, and Solids
314(2)
8.2 Intermolecular Forces
316(4)
8.3 Relative Strengths of Intermolecular Forces
320(4)
8.4 The Kinetic Theory of Liquids
324(1)
8.5 The Vapor Pressure of a Liquid
325(3)
8.6 Melting Point and Freezing Point
328(2)
8.7 Boiling Point
330(2)
8.8 Phase Diagrams
332(1)
8.9 Hydrogen Bonding and the Anomalous Properties of Water
333(1)
8.10 Solutions: Like Dissolves Like
334(3)
8.11 Hydrophilic and Hydrophobic Molecules
337(2)
8.12 Soaps, Detergents, and Dry-Cleaning Agents
339(2)
8.13 Why Do Some Solids Dissolve in Water?
341(3)
8.14 Solubility Equilibria
344(2)
8.15 Solubility Rules
346(1)
8.16 Net Ionic Equations
347(20)
Problems
349(8)
Special Topics
8A.1 Colligative Properties
357(1)
8A.2 Depression of the Partial Pressure of a Solvent
358(3)
8A.3 Boiling Point Elevation
361(2)
8A.4 Freezing Point Depression
363(2)
Problems
365(2)
Chapter 9 Solids
367(41)
9.1 Types of Solids
368(1)
9.2 Molecular and Network Covalent Solids
369(3)
9.3 The Physical Properties of Molecular and Network Covalent Solids
372(1)
9.4 Metallic Solids
373(1)
9.5 Physical Properties That Result from the Structure of Metals
374(1)
9.6 The Structure of Metals
375(3)
9.7 Coordination Numbers and the Structures of Metals
378(1)
9.8 Unit Cells: The Simplest Repeating Unit in a Crystal
379(1)
9.9 Solid Solutions and Intermetallic Compounds
380(1)
9.10 Semimetals
381(1)
9.11 Ionic Solids
382(3)
9.12 The Search for New Materials
385(3)
9.13 Measuring the Distance Between Particles in a Unit Cell
388(1)
9.14 Determining the Unit Cell of a Crystal
389(2)
9.15 Calculating the Size of an Atom or Ion
391(17)
Problems
392(5)
Special Topics
9A.1 Defects
397(1)
9A.2 Metals, Semiconductors, and Insulators
398(3)
9A.3 Thermal Conductivity
401(1)
9A.4 Thermal Expansion
402(1)
9A.5 Glass and Other Ceramics
403(4)
Problems
407(1)
Chapter 10 The Connection Between Kinetics and Equilibrium
408(60)
10.1 Reactions That Don't Go to Completion
409(2)
10.2 Gas-Phase Reactions
411(2)
10.3 The Rate of a Chemical Reaction
413(2)
10.4 The Collision Theory Model of Gas-Phase Reactions
415(3)
10.5 Equilibrium Constant Expressions
418(5)
10.6 Reaction Quotients: A Way to Decide Whether a Reaction is at Equilibrium
423(2)
10.7 Changes in Concentration That Occur as a Reaction Comes to Equilibrium
425(5)
10.8 Hidden Assumptions That Make Equilibrium Calculations Easier
430(4)
10.9 What Do We Do When the Assumption Fails?
434(2)
10.10 The Effect of Temperature on an Equilibrium Constant
436(1)
10.11 Le Chatelier's Principle
437(6)
10.12 Le Chatelier's Principle and the Haber Process
443(2)
10.13 What Happens When a Solid Dissolves in Water?
445(1)
10.14 The Solubility Product Expression
446(2)
10.15 The Relationship Between Ksp and the Solubility of a Salt
448(3)
10.16 The Role of the Ion Product (Qsp) in Solubility Calculations
451(2)
10.17 The Common-Ion Effect
453(15)
Problems
458(10)
Chapter 11 Acids and Bases
468(72)
11.1 Properties of Acids and Bases
469(1)
11.2 The Arrhenius Definition of Acids and Bases
469(1)
11.3 The Brønsted-Lowry Definition of Acids and Bases
470(2)
11.4 Conjugate Acid-Base Pairs
472(2)
11.5 The Role of Water in the Brønsted Model
474(1)
11.6 To What Extent Does Water Dissociate to Form Ions?
475(3)
11.7 pH as a Measure of the Concentration of the H3O+Ion
478(3)
11.8 Relative Strengths of Acids and Bases
481(4)
11.9 Relative Strengths of Conjugate Acid-Base Pairs
485(1)
11.10 Relative Strengths of Different Acids and Bases
486(4)
11.11 Relationship of Structure to Relative Strengths of Acids and Bases
490(4)
11.12 Strong Acid pH Calculations
494(1)
11.13 Weak Acid pH Calculations
494(6)
11.14 Base pH Calculations
500(4)
11.15 Mixtures of Acids and Bases: Buffers
504(2)
11.16 Buffers and Buffer Capacity
506(4)
11.17 Buffers in the Body
510(1)
11.18 Acid-Base Reactions
511(2)
11.19 pH Titration Curves
513(27)
Problems
520(10)
Special Topics
11A.1 Diprotic Acids
530(4)
11A.2 Diprotic Bases
534(2)
11A.3 Compounds That Could Be Either Acids or Bases
536(3)
Problems
539(1)
Chapter 12 Oxidation---Reduction Reactions
540
12.1 Common Oxidation-Reduction Reactions
541(1)
12.2 Determining Oxidation Numbers
542(2)
12.3 Recognizing Oxidation-Reduction Reactions
544(4)
12.4 Voltaic Cells
548(3)
12.5 Standard Cell Potentials
551(2)
12.6 Oxidizing and Reducing Agents
553(1)
12.7 Relative Strengths of Oxidizing and Reducing Agents
554(5)
12.8 Batteries
559(4)
12.9 Electrochemical Cells at Nonstandard Conditions: The Nernst Equation
563(4)
12.10 Electrolysis and Faraday's Law
567(4)
12.11 Electrolysis of Molten NaCl
571(1)
12.12 Electrolysis of Aqueous NaCl
572(2)
12.13 Electrolysis of Water
574(1)
12.14 The Hydrogen Economy
575
Problems
576(9)
Special Topics
12.A1 Balancing Oxidation-Reduction Equations
585(1)
12.A2 Redox Reactions in Acidic Solutions
585(4)
12.A3 Redox Reactions in Basic Solutions
589(1)
12.A4 Molecular Redox Reactions
590(2)
Problems
592
Chapter 13 Chemical Thermodynamics
534(106)
13.1 Spontaneous Chemical and Physical Processes
595(1)
13.2 Entropy and Disorder
596(1)
13.3 Entropy and the Second Law of Thermodynamics
597(3)
13.4 Standard-State Entropies of Reaction
600(1)
13.5 The Third Law of Thermodynamics
600(1)
13.6 Calculating Entropy Changes for Chemical Reactions
601(5)
13.7 Gibbs Free Energy
606(6)
13.8 The Effect of Temperature on the Free Energy of a Reaction
612(1)
13.9 Beware of Oversimplifications
613(1)
13.10 Standard-State Free Energies of Reaction
613(2)
13.11 Equilibria Expressed in Partial Pressures
615(4)
13.12 Interpreting Standard-State Free Energy of Reaction Data
619(1)
13.13 The Relationship between Free Energy and Equilibrium Constants
620(6)
13.14 The Temperature Dependence of Equilibrium Constants
626(4)
13.15 Gibbs Free Energies of Formation and Absolute Entropies
630(10)
Problems
632(8)
Chapter 14 Kinetics
640(48)
14.1 The Forces That Control a Chemical Reaction
641(1)
14.2 Chemical Kinetics
642(1)
14.3 Is the Rate of Reaction Constant?
642(2)
14.4 Instantaneous Rates of Reaction
644(1)
14.5 Rate Laws and Rate Constants
645(1)
14.6 The Rate Law Versus the Stoichiometry of a Reaction
646(1)
14.7 Order and Molecularity
647(3)
14.8 A Collision Theory Model of Chemical Reactions
650(2)
14.9 The Mechanisms of Chemical Reactions
652(2)
14.10 Zero-Order Reactions
654(1)
14.11 Determining the Order of a Reaction from Rates of Reaction
655(3)
14.12 The Integrated Form of Zero-, First-, and Second-Order Rate Laws
658(5)
14.13 Determining the Order of a Reaction with the Integrated Form of Rate Laws
663(3)
14.14 Reactions That Are First-Order in Two Reactants
666(1)
14.15 The Activation Energy of Chemical Reactions
667(2)
14.16 Catalysts and the Rates of Chemical Reactions
669(2)
14.17 Determining the Activation Energy of a Reaction
671(2)
14.18 The Kinetics of Enzyme-Catalyzed Reactions
673(15)
Problems
675(11)
Special Topics
14A.1 Deriving the Integrated Rate Laws
686(2)
Chapter 15 Nuclear Chemistry
688(35)
15.1 Radioactivity
689(1)
15.2 The Structure of the Atom
690(2)
15.3 Modes of Radioactive Decay
692(2)
15.4 Neutron-Rich Versus Neutron-Poor Nuclides
694(3)
15.5 Binding Energy Calculations
697(3)
15.6 The Kinetics of Radioactive Decay
700(3)
15.7 Dating by Radioactive Decay
703(2)
15.8 Ionizing Versus Nonionizing Radiation
705(1)
15.9 Biological Effects of Ionizing Radiation
706(3)
15.10 Natural Versus Induced Radioactivity
709(4)
15.11 Nuclear Fission
713(2)
15.12 Nuclear Fusion
715(2)
15.13 Nuclear Synthesis
717(2)
15.14 Nuclear Medicine
719(4)
Problems
720(3)
Chapter 16 Organic Chemistry
723
16.1 What Is an Organic Compound?
724(2)
16.2 The Saturated Hydrocarbons or Alkanes
726(3)
16.3 Rotation Around C---C Bonds
729(1)
16.4 The Nomenclature of Alkanes
730(3)
16.5 The Unsaturated Hydrocarbons: Alkenes and Alkynes
733(2)
16.6 Aromatic Hydrocarbons and Their Derivatives
735(2)
16.7 The Chemistry of Petroleum Products
737(3)
16.8 The Chemistry of Coal
740(2)
16.9 Functional Groups
742(4)
16.10 Oxidation-Reduction Reactions
746(4)
16.11 Alkyl Halides
750(2)
16.12 Alcohols and Ethers
752(3)
16.13 Aldehydes and Ketones
755(2)
16.14 Reactions at the Carbonyl Group
757(2)
16.15 Carboxylic Acids and Carboxylate Ions
759(2)
16.16 Esters
761(2)
16.17 Amines, Alkaloids, and Amides
763(2)
16.18 Alkene Stereoisomers
765(3)
16.19 Stereogenic Atoms
768(3)
16.20 Optical Activity
771
Problems
774
Appendix A
A.1 Systems of Units
2(4)
The English Units of Measurement
2(1)
SI Units of Measurement
3(1)
Derived SI Units
4(1)
Non-SI Units
4(1)
Conversion Factors
5(1)
A.2 Uncertainty in Measurement
6(2)
Systematic and Random Errors
6(1)
Accuracy and Precision
7(1)
A.3 Significant figures
8(2)
Addition and Subtraction with Significant Figures
9(1)
Multiplication and Division with Significant Figures
10(1)
Rounding Off
10(1)
A.4 Scientific Notation
10(2)
A.5 The Graphical Treatment of Data
12(3)
A.6 Significant Figures and Unit Conversion Worksheet
15
Significant Figures
15(1)
Counting Significant Figures in a Measurement
15(3)
Measurements versus Definitions
18(1)
Unit Conversions
19
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 Equilibrium 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 Configuration of the First 86 Elements
26(2)
Table B.16 Standard-State Enthalpy of Formation, Free Energy of Formation and Absolute Entropy Data
28
Appendix C Answers to Selected Problems
1(1)
Appendix D Answers to Checkpoints
1(1)
Photo Credits 1(1)
Index 1
Dr. James Spencer is a professor of chemistry at Franklin and Marshall College. He has received a number of awards and commendations including the Lindback Award for Distinguished Teaching, Bradley R. Dewey Award for Outstanding Scholarship, and the Chemical Manufacturers Association National Award for Teaching. Dr. Spencer was a founding member of the Council on Undergraduate Research, a national organization dedicated to promoting research in all disciplines by undergraduates. He was appointed chair of the ACS Task Force on the General Chemistry Curriculum, served as a member and chair of the Advanced Placement Chemistry Committee and now chairs the Advanced Placement Redesign Panel for Chemistry.