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Chemistry 8th edition [Kõva köide]

  • Formaat: Hardback, 1200 pages, kõrgus x laius x paksus: 100x100x100 mm, kaal: 100 g
  • Ilmumisaeg: 12-Feb-2019
  • Kirjastus: Pearson
  • ISBN-10: 0134856236
  • ISBN-13: 9780134856230
Teised raamatud teemal:
  • Formaat: Hardback, 1200 pages, kõrgus x laius x paksus: 100x100x100 mm, kaal: 100 g
  • Ilmumisaeg: 12-Feb-2019
  • Kirjastus: Pearson
  • ISBN-10: 0134856236
  • ISBN-13: 9780134856230
Teised raamatud teemal:

For two-semester general chemistry courses (science majors).

 

Give students a robust conceptual foundation while building critical problem solving skills

Robinson/McMurry/Fay’s Chemistry, known for a concise and united author voice, conceptual focus, extensive worked examples, and thoroughly constructed connections between organic, biological, and general chemistry, highlights the application of chemistry to students’ lives and careers. Lead author Jill Robinson strengthens the student orientation by creating more engaging, active learning opportunities for students and faculty.

 

With the 8th Edition, Robinson draws upon her exceptional teaching skills to provide new interactive experiences that help identify and address students’ preconceptions. Robinson complements active engagement in the text with a new media program that increases student awareness of their learning process via Mastering Chemistry and the Pearson eText, allowing instructors to choose the level of interactivity appropriate for their classroom. Interactive experiences include activities that guide students in how to actively read a science text and that address common preconceptions, giving students opportunities to cultivate and practice problem-solving skills.

 

Also available with Mastering Chemistry

By combining trusted author content with digital tools and a flexible platform, Mastering personalizes the learning experience and improves results for each student.The fully integrated and complete media package allows instructors to engage students before they come to class, hold them accountable for learning during class, and then confirm that learning after class.

 

Note: You are purchasing a standalone product; Mastering Chemistry does not come packaged with this content. Students, if interested in purchasing this title with Mastering Chemistry, ask your instructor for the correct package ISBN and Course ID. Instructors, contact your Pearson representative for more information.

 

If you would like to purchase both the physical text and Mastering Chemistry, search for:

 

0135205069 / 9780135205068 Chemistry Plus Mastering Chemistry with Pearson eText -- Access Card Package

Package consists of:

  • 0134856236 / 9780134856230 Chemistry
  • 0135204631 / 9780135204634 Mastering Chemistry with Pearson eText -- ValuePack Access Card -- for Chemistry

 

Preface xiii
For Instructors xvi
1 Chemical Tools: Experimentation and Measurement 1(32)
1.1 The Scientific Method: Nanoparticle Catalysts for Fuel Cells
2(3)
1.2 Measurements: SI Units and Scientific Notation
5(2)
1.3 Mass and Its Measurement
7(1)
1.4 Length and Its Measurement
8(1)
1.5 Temperature and Its Measurement
9(2)
1.6 Derived Units: Volume and Its Measurement
11(2)
1.7 Derived Units: Density and Its Measurement
13(1)
1.8 Derived Units: Energy and Its Measurement
14(2)
1.9 Accuracy, Precision, and Significant Figures in Measurement
16(2)
1.10 Significant Figures in Calculations
18(2)
1.11 Converting from One Unit to Another
20(3)
Inquiry: O What are the unique properties of nanoscale materials?
23(10)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
2 Atoms, Molecules, and Ions 33(50)
2.1 Chemistry and the Elements
34(2)
2.2 Elements and the Periodic Table
36(2)
2.3 Some Common Groups of Elements and Their Properties
38(3)
2.4 Observations Supporting Atomic Theory: The Conservation of Mass and the Law of Definite Proportions
41(2)
2.5 The Law of Multiple Proportions and Dalton's Atomic Theory
43(2)
2.6 Atomic Structure: Electrons
45(2)
2.7 Atomic Structure: Protons and Neutrons
47(2)
2.8 Atomic Numbers
49(2)
2.9 Atomic Weights and the Mole
51(4)
2.10 Measuring Atomic Weight: Mass Spectrometry
55(2)
2.11 Mixtures and Chemical Compounds; Molecules and Covalent Bonds
57(4)
2.12 Ions and Ionic Bonds
61(2)
2.13 Naming Chemical Compounds
63(6)
Inquiry: How can measurements of oxygen and hydrogen isotopes in ice cores determine past climates?
69(14)
Study Guide, Key Terms, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
3 Mass Relationships in Chemical Reactions 83(33)
3.1 Representing Chemistry on Different Levels
84(1)
3.2 Balancing Chemical Equations
85(3)
3.3 Molecular Weight and Molar Mass
88(2)
3.4 Stoichiometry: Relating Amounts of Reactants and Products
90(2)
3.5 Yields of Chemical Reactions
92(2)
3.6 Reactions with Limiting Amounts of Reactants
94(3)
3.7 Percent Composition and Empirical Formulas
97(3)
3.8 Determining Empirical Formulas: Elemental Analysis
100(3)
3.9 Determining Molecular Weights: Mass Spectrometry
103(2)
Inquiry: How is the principle of atom economy used to minimize waste in a chemical synthesis?
105(11)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
4 Reactions in Aqueous Solution 116(45)
4.1 Solution Concentration: Molarity
117(2)
4.2 Diluting Concentrated Solutions
119(2)
4.3 Electrolytes in Aqueous Solution
121(2)
4.4 Types of Chemical Reactions in Aqueous Solution
123(1)
4.5 Aqueous Reactions and Net Ionic Equations
124(1)
4.6 Precipitation Reactions and Solubility Guidelines
125(3)
4.7 Acids, Bases, and Neutralization Reactions
128(4)
4.8 Solution Stoichiometry
132(1)
4.9 Measuring the Concentration of a Solution: Titration
133(2)
4.10 Oxidation-Reduction (Redox) Reactions
135(3)
4.11 Identifying Redox Reactions
138(3)
4.12 The Activity Series of the Elements
141(3)
4.13 Redox Titrations
144(2)
4.14 Some Applications of Redox Reactions
146(2)
Inquiry: How do sports drinks replenish the substances lost in sweat?
148(13)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
5 Periodicity and the Electronic Structure of Atoms 161(47)
5.1 Wave Properties of Radiant Energy and the Electromagnetic Spectrum
162(4)
5.2 Particlelike Properties of Radiant Energy: The Photoelectric Effect and Planck's Postulate
166(3)
5.3 Atomic Line Spectra and Quantized Energy
169(4)
5.4 Wavelike Properties of Matter: de Broglie's Hypothesis
173(2)
5.5 The Quantum Mechanical Model of the Atom: Heisenberg's Uncertainty Principle
175(1)
5.6 The Quantum Mechanical Model of the Atom: Orbitals and Quantum Numbers
176(3)
5.7 The Shapes of Orbitals
179(5)
5.8 Electron Spin and the Pauli Exclusion Principle
184(1)
5.9 Orbital Energy Levels in Multielectron Atoms
185(2)
5.10 Electron Configurations of Multielectron Atoms
187(2)
5.11 Anomalous Electron Configurations
189(1)
5.12 Electron Configurations and the Periodic Table
189(3)
5.13 Electron Configurations and Periodic Properties: Atomic Radii
192(3)
Inquiry: How does knowledge of atomic emission spectra help us build more efficient light bulbs?
195(13)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
6 Ionic Compounds: Periodic Trends and Bonding Theory 208(30)
6.1 Electron Configurations of Ions
209(3)
6.2 Ionic Radii
212(2)
6.3 Ionization Energy
214(2)
6.4 Higher Ionization Energies
216(2)
6.5 Electron Affinity
218(2)
6.6 The Octet Rule
220(2)
6.7 Ionic Bonds and the Formation of Ionic Solids
222(4)
6.8 Lattice Energies in Ionic Solids
226(2)
Inquiry: How do ionic liquids lead to more environmentally friendly processes?
228(10)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
7 Covalent Bonding and Electron-Dot Structures 238(40)
7.1 Covalent Bonding in Molecules
239(1)
7.2 Strengths of Covalent Bonds
240(2)
7.3 Polar Covalent Bonds: Electronegativity
242(4)
7.4 A Comparison of Ionic and Covalent Compounds
246(1)
7.5 Electron-Dot Structures: The Octet Rule
247(3)
7.6 Procedure for Drawing Electron-Dot Structures
250(4)
7.7 Drawing Electron-Dot Structures for Radicals
254(1)
7.8 Electron-Dot Structures of Compounds Containing Only Hydrogen and Second-Row Elements
255(2)
7.9 Electron-Dot Structures and Resonance
257(4)
7.10 Formal Charges
261(4)
Inquiry: How does bond polarity affect the toxicity of organophosphate insecticides?
265(13)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
8 Covalent Compounds: Bonding Theories and Molecular Structure 278(49)
8.1 Molecular Shapes: The VSEPR Model
279(7)
8.2 Valence Bond Theory
286(1)
8.3 Hybridization and spa Hybrid Orbitals
287(3)
8.4 Other Kinds of Hybrid Orbitals
290(5)
8.5 Polar Covalent Bonds and Dipole Moments
295(3)
8.6 Intermolecular Forces
298(8)
8.7 Molecular Orbital Theory: The Hydrogen Molecule
306(2)
8.8 Molecular Orbital Theory: Other Diatomic Molecules
308(4)
8.9 Combining Valence Bond Theory and Molecular Orbital Theory
312(2)
Inquiry: Which is better for human health, natural or synthetic vitamins?
314(13)
Study Guide, Key Terms, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
9 Thermochemistry: Chemical Energy 327(47)
9.1 Energy and Its Conservation
328(2)
9.2 Internal Energy and State Functions
330(2)
9.3 Expansion Work
332(2)
9.4 Energy and Enthalpy
334(2)
9.5 Thermochemical Equations and the Thermodynamic Standard State
336(2)
9.6 Enthalpies of Chemical and Physical Changes
338(3)
9.7 Calorimetry and Heat Capacity
341(4)
9.8 Hess's Law
345(3)
9.9 Standard Heats of Formation
348(2)
9.10 Bond Dissociation Energies
350(2)
9.11 An Introduction to Entropy
352(3)
9.12 An Introduction to Free Energy
355(4)
Inquiry: How do we determine the energy content of biofuels?
359(15)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
10 Gases: Their Properties and Behavior 374(48)
10.1 Gases and Gas Pressure
375(5)
10.2 The Gas Laws
380(5)
10.3 The Ideal Gas Law
385(2)
10.4 Stoichiometric Relationships with Gases
387(3)
10.5 Mixtures of Gases: Partial Pressure and Dalton's Law
390(3)
10.6 The Kinetic-Molecular Theory of Gases
393(2)
10.7 Gas Diffusion and Effusion: Graham's Law
395(2)
10.8 The Behavior of Real Gases
397(1)
10.9 The Earth's Atmosphere and the Greenhouse Effect
398(3)
10.10 Greenhouse Gases
401(2)
10.11 Climate Change
403(4)
Inquiry: How do inhaled anesthetics work?
407(15)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
11 Liquids and Phase Changes 422(28)
11.1 Properties of Liquids
423(1)
11.2 Vapor Pressure and Boiling Point
424(4)
11.3 Phase Changes between Solids, Liquids, and Gases
428(3)
11.4 Energy Changes during Phase Transitions
431(2)
11.5 Phase Diagrams
433(3)
11.6 Liquid Crystals
436(3)
Inquiry: How is caffeine removed from coffee?
439(11)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
12 Solids and Solid-State Materials 450(44)
12.1 Types of Solids
451(2)
12.2 Probing the Structure of Solids: X-Ray Crystallography
453(2)
12.3 The Packing of Spheres in Crystalline Solids: Unit Cells
455(4)
12.4 Structures of Some Ionic Solids
459(3)
12.5 Structures of Some Covalent Network Solids
462(2)
12.6 Bonding in Metals
464(4)
12.7 Semiconductors
468(3)
12.8 Semiconductor Applications
471(4)
12.9 Superconductors
475(2)
12.10 Ceramics and Composites
477(5)
Inquiry: What are quantum dots, and what controls their color?
482(12)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
13 Solutions and Their Properties 494(44)
13.1 Solutions
495(1)
13.2 Enthalpy Changes and the Solution Process
496(2)
13.3 Predicting Solubility
498(3)
13.4 Concentration Units for Solutions
501(5)
13.5 Some Factors That Affect Solubility
506(4)
13.6 Physical Behavior of Solutions: Colligative Properties
510(1)
13.7 Vapor-Pressure Lowering of Solutions: Raoult's Law
511(6)
13.8 Boiling-Point Elevation and Freezing-Point Depression of Solutions
517(4)
13.9 Osmosis and Osmotic Pressure
521(4)
Inquiry: How does hemodialysis cleanse the blood of patients with kidney failure?
525(13)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
14 Chemical Kinetics 538(63)
14.1 Reaction Rates
539(5)
14.2 Rate Laws and Reaction Order
544(2)
14.3 Method of Initial Rates: Experimental Determination of a Rate Law
546(4)
14.4 Integrated Rate Law: Zeroth-Order Reactions
550(2)
14.5 Integrated Rate Law: First-Order Reactions
552(5)
14.6 Integrated Rate Law: Second-Order Reactions
557(3)
14.7 Reaction Rates and Temperature: The Arrhenius Equation
560(4)
14.8 Using the Arrhenius Equation
564(3)
14.9 Reaction Mechanisms
567(3)
14.10 Rate Laws for Elementary Reactions
570(3)
14.11 Rate Laws for Overall Reactions
573(4)
14.12 Catalysis
577(3)
14.13 Homogeneous and Heterogeneous Catalysts
580(3)
Inquiry: How do enzymes work?
583(18)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
15 Chemical Equilibrium 601(53)
15.1 The Equilibrium State
603(2)
15.2 The Equilibrium Constant Kc
605(5)
15.3 The Equilibrium Constant Kp
610(2)
15.4 Heterogeneous Equilibria
612(2)
15.5 Using the Equilibrium Constant
614(10)
15.6 Factors That Alter the Composition of an Equilibrium Mixture: Le Chitelier's Principle
624(1)
15.7 Altering an Equilibrium Mixture: Changes in Concentration
625(4)
15.8 Altering an Equilibrium Mixture: Changes in Pressure and Volume
629(2)
15.9 Altering an Equilibrium Mixture: Changes in Temperature
631(3)
15.10 The Link between Chemical Equilibrium and Chemical Kinetics
634(3)
Inquiry: How does high altitude affect oxygen transport in the body?
637(17)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
16 Aqueous Equilibria: Acids and Bases 654(54)
16.1 Acid-Base Concepts: The Bronsted-Lowry Theory
655(3)
16.2 Acid Strength and Base Strength
658(3)
16.3 Factors That Affect Acid Strength
661(3)
16.4 Dissociation of Water
664(2)
16.5 The pH Scale
666(2)
16.6 Measuring pH
668(1)
16.7 The pH in Solutions of Strong Acids and Strong Bases
669(2)
16.8 Equilibria in Solutions of Weak Acids
671(2)
16.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids
673(4)
16.10 Percent Dissociation in Solutions of Weak Acids
677(1)
16.11 Polyprotic Acids
678(4)
16.12 Equilibria in Solutions of Weak Bases
682(2)
16.13 Relation Between K and Kb
684(2)
16.14 Acid-Base Properties of Salts
686(5)
16.15 Lewis Acids and Bases
691(3)
Inquiry: Has the problem of acid rain been solved?
694(14)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
17 Applications of Aqueous Equilibria 708(60)
17.1 Neutralization Reactions
709(3)
17.2 The Common-Ion Effect
712(4)
17.3 Buffer Solutions
716(4)
17.4 The Henderson-Hasselbalch Equation
720(3)
17.5 pH Titration Curves
723(1)
17.6 Strong Acid-Strong Base Titrations
724(3)
17.7 Weak Acid-Strong Base Titrations
727(5)
17.8 Weak Base-Strong Acid Titrations
732(1)
17.9 Polyprotic Acid-Strong Base Titrations
733(5)
17.10 Solubility Equilibria for Ionic Compounds
738(1)
17.11 Measuring Ksp and Calculating Solubility from Ksp
739(3)
17.12 Factors That Affect Solubility
742(8)
17.13 Precipitation of Ionic Compounds
750(1)
17.14 Separation of Ions by Selective Precipitation
751(1)
17.15 Qualitative Analysis
752(2)
Inquiry: What is causing ocean acidification?
754(14)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
18 Thermodynamics: Entropy, Free Energy, and Spontaneity 768(45)
18.1 Spontaneous Processes
769(1)
18.2 Enthalpy, Entropy, and Spontaneous Processes
770(3)
18.3 Entropy and Probability
773(4)
18.4 Entropy and Temperature
777(2)
18.5 Standard Molar Entropies and Standard Entropies of Reaction
779(2)
18.6 Entropy and the Second Law of Thermodynamics
781(3)
18.7 Free Energy and the Spontaneity of Chemical Reactions
784(3)
18.8 Standard Free-Energy Changes for Reactions
787(2)
18.9 Standard Free Energies of Formation
789(3)
18.10 Free-Energy Changes for Reactions under Nonstandard-State Conditions
792(2)
18.11 Free Energy and Chemical Equilibrium
794(4)
Inquiry: Does the formation of highly ordered molecules violate the second law of thermodynamics?
798(15)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
19 Electrochemistry 813(57)
19.1 Balancing Redox Reactions by the Half-Reaction Method
814(5)
19.2 Galvanic Cells
819(5)
19.3 Shorthand Notation for Galvanic Cells
824(1)
19.4 Cell Potentials and Free-Energy Changes for Cell Reactions
825(2)
19.5 Standard Reduction Potentials
827(3)
19.6 Using Standard Reduction Potentials
830(3)
19.7 Cell Potentials under Nonstandard-State Conditions: The Nernst Equation
833(3)
19.8 Electrochemical Determination of pH
836(2)
19.9 Standard Cell Potentials and Equilibrium Constants
838(2)
19.10 Batteries
840(3)
19.11 Corrosion
843(3)
19.12 Electrolysis and Electrolytic Cells
846(3)
19.13 Commercial Applications of Electrolysis
849(3)
19.14 Quantitative Aspects of Electrolysis
852(2)
Inquiry: How do hydrogen fuel cells work?
854(16)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
20 Nuclear Chemistry 870(34)
20.1 Nuclear Reactions and Their Characteristics
871(1)
20.2 Radioactivity
872(3)
20.3 Nuclear Stability
875(2)
20.4 Radioactive Decay Rates
877(4)
20.5 Dating with Radioisotopes
881(1)
20.6 Energy Changes during Nuclear Reactions
882(4)
20.7 Nuclear Fission and Fusion
886(4)
20.8 Nuclear Transmutation
890(1)
20.9 Detecting and Measuring Radioactivity
891(3)
Inquiry: How are radioisotopes used in medicine?
894(10)
Study Guide, Key Terms, Key Equations, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
21 Transition Elements and Coordination Chemistry 904(50)
21.1 Electron Configurations
906(2)
21.2 Properties of Transition Elements
908(4)
21.3 Oxidation States of Transition Elements
912(1)
21.4 Coordination Compounds
913(2)
21.5 Ligands
915(3)
21.6 Naming Coordination Compounds
918(3)
21.7 Isomers
921(5)
21.8 Enantiomers and Molecular Handedness
926(3)
21.9 Color of Transition Metal Complexes
929(1)
21.10 Crystal Field Theory
930(6)
21.11 Bonding in Complexes: Valence Bond Theory
936(4)
Inquiry: How does cisplatin kill cancer cells?
940(14)
Study Guide, Key Terms, Key Equation, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
22 The Main-Group Elements 954(49)
22.1 A Review of General Properties and Periodic Trends
955(2)
22.2 Distinctive Properties of the Second-Row Elements
957(2)
22.3 Group 1A: Hydrogen
959(3)
22.4 Group 1A: Alkali Metals and Group 2A: Alkaline Earth Metals
962(3)
22.5 Group 3A Elements
965(2)
22.6 Group 4A Elements
967(7)
22.7 Group 5A Elements
974(6)
22.8 Group 6A Elements
980(7)
22.9 Group 7A: The Halogens
987(2)
22.10 Group 8A: Noble Gases
989(1)
Inquiry: What are the barriers to a hydrogen economy?
990(13)
Study Guide, Key Terms, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
23 Organic and Biological Chemistry 1003
23.1 Organic Molecules and Their Structures: Consitutional Isomers
1004(4)
23.2 Stereoisomers: Chiral Molecules
1008(3)
23.3 Families of Organic Compounds: Functional Groups
1011(3)
23.4 Carbohydrates: A Biological Example of Isomers
1014(3)
23.5 Valence Bond Theory and Orbital Overlap Pictures
1017(4)
23.6 Lipids: A Biological Example of Cis- Trans Isomerism
1021(4)
23.7 Formal Charge and Resonance in Organic Compounds
1025(5)
23.8 Conjugated Systems
1030(4)
23.9 Proteins: A Biological Example of Conjugation
1034(4)
23.10 Aromatic Compounds and Molecular Orbital Theory
1038(3)
23.11 Nucleic Acids: A Biological Example of Aromaticity
1041(4)
Inquiry: Why do enantiomers have different biological responses?
1045
Study Guide, Key Terms, Practice Test, Conceptual Problems, Section Problems, Multiconcept Problems
Appendix A: Mathematical Operations A-1
A.1 Scientific Notation
A-1
A.2 Logarithms
A-4
A.3 Straight-Line Graphs and Linear Equations
A-6
A.4 Quadratic Equations
A-7
A.5 Calculus Derivations of Integrated Rate Laws
A-7
Appendix B: Thermodynamic Properties at 25 °C A-9
Appendix C: Equilibrium Constants at 25 °C A-14
Appendix D: Standard Reduction Potentials at 25 °C A-18
Appendix E: Properties of Water A-20
Answers to Selected Problems A-21
Glossary G-1
Index I-1
Photo/ Text Credits C-1
About our authors Jill K. Robinson received her Ph.D. in analytical and atmospheric chemistry from the University of Colorado at Boulder. She is a senior lecturer at Indiana University and teaches general, analytical, and environmental chemistry courses. Her clear and relatable teaching style has been honored with several awards including the Presidents Award for Distinguished Teaching at Indiana University and the J. Calvin Giddings Award for Excellence in Education from the American Chemical Society Division of Analytical Chemistry. She leads workshops to help faculty transition from lecture-based instruction to student-centered pedagogies.

John McMurry, educated at Harvard and Columbia, has taught more than 20,000 students in general and organic chemistry over a 40-year period. An emeritus professor of chemistry at Cornell University, Dr. McMurry previously spent 13 years on the faculty at the University of California at Santa Cruz. He has received numerous awards, including the Alfred P. Sloan Fellowship (196971), the National Institute of Health Career Development Award (197580), the Alexander von Humboldt Senior Scientist Award (198687), and the Max Planck Research Award (1991).

Robert C. Fay, professor emeritus at Cornell University, taught general and inorganic chemistry at Cornell for 45 years beginning in 1962. Known for his clear, well-organized lectures, Dr. Fay was the 1980 recipient of the Clark Distinguished Teaching Award. He has also taught as a visiting professor at Harvard University and the University of Bologna (Italy). A Phi Beta Kappa graduate of Oberlin College, Dr. Fay received his Ph.D. from the University of Illinois. He has been an NSF Science Faculty Fellow at the University of East Anglia and the University of Sussex (England) and a NATO/Heineman Senior Fellow at Oxford University.