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General chemistry : principles and modern applications / Ralph H. Petrucci ... [et al.]

Contributor(s): Petrucci, Ralph H.
Material type: materialTypeLabelBook; Format: print Publisher: New Jersey : Prentice Hall, 2006Edition: 9th ed.Description: 2 v. + 2 discos compactos.ISBN: 0-13-198825-5 (Manual); 0-13-221075-4 (Virtual Chemlab : problems and assignments fro the virtual laboratory 2.5); 0-13-236938-9 (CD Virtual Chemlab); 0-13-149390-6 (Accelerator CD).Subject(s): QuímicaOnline resources: Material complementario online. (solicite clave de usuario en su Biblioteca)
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QUIMICA GRADO EN CIENCIAS AMBIENTALES Asignatura actualizada 2017-2018

QUÍMICA GRADO EN CIENCIAS DEL MAR Asignatura actualizada 2017-2018

QUÍMICA I GRADO EN INGENIERÍA QUÍMICA Asignatura actualizada 2017-2018

Manuales (7 días) 02. BIBLIOTECA CAMPUS PUERTO REAL
54/GEN (Browse shelf) Manual   Shelving location | Bibliomaps® BIBLIOG. RECOM. 3742690067
Manuales (7 días) 02. BIBLIOTECA CAMPUS PUERTO REAL
54/GEN (Browse shelf) Manual   Shelving location | Bibliomaps® BIBLIOG. RECOM. 3742686886
Manuales (7 días) 02. BIBLIOTECA CAMPUS PUERTO REAL
54/GEN (Browse shelf) Virtual Chemlab   Shelving location | Bibliomaps® BIBLIOG. RECOM. 3742550831

QUIMICA GRADO EN CIENCIAS AMBIENTALES Asignatura actualizada 2017-2018

QUÍMICA GRADO EN CIENCIAS DEL MAR Asignatura actualizada 2017-2018

Monografías 02. BIBLIOTECA CAMPUS PUERTO REAL
54/GEN (Browse shelf) Virtual Chemlab   Shelving location | Bibliomaps® PREST. LIBROS 374268999X
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Enhanced descriptions from Syndetics:

This edition introduces a number of innovative features, including new feature problems, and new follow-up practice exercises to accompany every in-chapter example.

Incluye acceso a contenidos on-line. Ver nota de ejemplar.

Índice

Manual. -- Virtual Chemlab : problems and assignments fro the virtual laboratory 2.5. -- CD Virtual Chemlab. -- Accelerator CD

For 2-semester or 3-quarter general chemistry courses. General Chemistry: Principles and Modern Applications is recognized for its superior problems, lucid writing, precision of argument, and precise and detailed treatment of the subject. Popular and innovative features include Feature Problems, follow-up A and B Practice Exercises to accompany every in-chapter Example, Focus On application boxes, and new Keep in Mind marginal notes.

Table of contents provided by Syndetics

  • This is a preliminary Table of Contents
  • About the Authors
  • Preface
  • Student's Guide to Using this Text
  • 1 Matter Its Properties and Measurement
  • 1-1 The Scientific Method
  • 1-2 Properties of Matter
  • 1-3 Classification of Matter
  • 1-4 Measurement of Matter: SI (Metric) Units
  • 1-5 Density and Percent Composition: Their Use in Problem Solving
  • 1-6 Uncertainties in Scientific Measurements
  • 1-7 Significant Figures
  • Focus on The Scientific Method at Work: Polywater
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 2 Atoms and the Atomic Theory
  • 2-1 Early Chemical Discoveries and the Atomic Theory
  • 2-2 Electrons and Other Discoveries in Atomic Physics
  • 2-3 The Nuclear Atom
  • 2-4 Chemical Elements
  • 2-5 Atomic Masses
  • 2-6 Introduction to the Periodic Table
  • 2-7 The Concept of the Mole and the Avogadro Constant
  • 2-8 Using the Mole Concept in Calculations
  • Focus on Occurrence and Abundances of the Elements
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 3 Chemical Compounds
  • 3-1 Types of Chemical Compounds and Their Formulas
  • 3-2 The Mole Concept and Chemical Compounds
  • 3-3 Composition of Chemical Compounds
  • 3-4 Oxidation States: A Useful Tool in Describing Chemical Compounds
  • 3-5 Naming Compounds: Organic and Inorganic Compounds
  • 3-6 Names and Formulas of Inorganic Compounds
  • 3-7 Names and Formulas of Organic Compounds
  • Focus on Mass Spectrometry Determining Molecular Formulas
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 4 Chemical Reactions
  • 4-1 Chemical Reactions and Chemical Equations
  • 4-2 Chemical Equations and Stoichiometry
  • 4-3 Chemical Reactions in Solution
  • 4-4 Determining the Limiting Reactant
  • 4-5 Other Practical Matters in Reaction Stoichiometry
  • Focus on Industrial Chemistry
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 5 Introduction to Reactions in Aqueous Solutions
  • 5-1 The Nature of Aqueous Solutions
  • 5-2 Precipitation Reactions
  • 5-3 Acid Base Reactions
  • 5-4 Oxidation Reduction: Some General Principles
  • 5-5 Balancing Oxidation Reduction Equations
  • 5-6 Oxidizing and Reducing Agents
  • 5-7 Stoichiometry of Reactions in Aqueous Solutions: Titrations
  • Focus on Water Treatment
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 6 Gases
  • 6-1 Properties of Gases: Gas Pressure
  • 6-2 The Simple Gas Laws
  • 6-3 Combining the Gas Laws: The Ideal Gas Equation and the General Gas Equation
  • 6-4 Applications of the Ideal Gas Equation
  • 6-5 Gases in Chemical Reactions
  • 6-6 Mixtures of Gases
  • 6-7 Kinetic-Molecular Theory of Gases
  • 6-8 Gas Properties Relating to the Kinetic-Molecular Theory
  • 6-9 Nonideal (Real) Gases
  • Focus on Earth's Atmosphere
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 7 Thermochemistry 220
  • 7-1 Getting Started: Some Terminology
  • 7-2 Heat
  • 7-3 Heats of Reaction and Calorimetry
  • 7-4 Work
  • 7-5 The First Law of Thermodynamics
  • 7-6 Heats of Reaction: DU and DH
  • 7-7 Indirect Determination of DH: Hess's Law
  • 7-8 Standard Enthalpies of Formation
  • 7-9 Fuels as Sources of Energy
  • Focus on Fats, Carbohydrates, and Energy Storage
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 8 Electrons in Atoms
  • 8-1 Electromagnetic Radiation
  • 8-2 Atomic Spectra
  • 8-3 Quantum Theory
  • 8-4 The Bohr Atom
  • 8-5 Two Ideas Leading to a New Quantum Mechanics
  • 8-6 Wave Mechanics
  • 8-7 Quantum Numbers and Electron Orbitals
  • 8-8 Interpreting and Representing the Orbitals of the Hydrogen Atom
  • 8-9 Electron Spin: A Fourth Quantum Number
  • 8-10 Multielectron Atoms
  • 8-11 Electron Configurations
  • 8-12 Electron Configurations and the Periodic Table
  • Focus on Helium Neon Lasers
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 9 The Periodic Table and Some Atomic Properties
  • 9-1 Classifying the Elements: The Periodic Law and the Periodic Table
  • 9-2 Metals and Nonmetals and Their Ions
  • 9-3 The Sizes of Atoms and Ions
  • 9-4 Ionization Energy
  • 9-5 Electron Affinity
  • 9-6 Magnetic Properties
  • 9-7 Periodic Properties of the Elements
  • Focus on The Periodic Law and Mercury
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 10 Chemical Bonding I: Basic Concepts
  • 10-1 Lewis Theory: An Overview
  • 10-2 Covalent Bonding: An Introduction
  • 10-3 Polar Covalent Bonds and Electrostatic Potential Maps
  • 10-4 Writing Lewis Structures
  • 10-5 Resonance
  • 10-6 Exceptions to the Octet Rule
  • 10-7 Shapes of Molecules
  • 10-8 Bond Order and Bond Lengths
  • 10-9 Bond Energies
  • Focus on Molecules in Space: Measuring Bond Lengths
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 11 Chemical Bonding II: Additional Aspects
  • 11-1 What a Bonding Theory Should Do
  • 11-2 Introduction to the Valence-Bond Method
  • 11-3 Hybridization of Atomic Orbitals
  • 11-4 Multiple Covalent Bonds
  • 11-5 Molecular Orbital Theory
  • 11-6 Delocalized Electrons: Bonding in the Benzene Molecule
  • 11-7 Bonding in Metals
  • 11-8 Some Unresolved Issues Can Electron Charge-Density Plots Help
  • Focus on Photoelectron Spectroscopy
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 12 Liquids, Solids, and Intermolecular Forces
  • 12-1 Intermolecular Forces and Some Properties of Liquids
  • 12-2 Vaporization of Liquids: Vapor Pressure
  • 12-3 Some Properties of Solids
  • 12-4 Phase Diagrams
  • 12-5 Van der Waals Forces
  • 12-6 Hydrogen Bonding
  • 12-7 Network Covalent Solids and Ionic Solids
  • 12-8 Crystal Structures
  • 12-9 Energy Changes in the Formation of Ionic Crystals
  • Focus on Liquid Crystals
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 13 Solutions and Their Physical Properties
  • 13-1 Types of Solutions: Some Terminology
  • 13-2 Solution Concentrations
  • 13-3 Intermolecular Forces and the Solution Process
  • 13-4 Solution Formation and Equilibrium
  • 13-5 Solubilities of Gases
  • 13-6 Vapor Pressures of Solutions
  • 13-7 Osmotic Pressure
  • 13-8 Freezing-Point Depression and Boiling-Point Elevation of Nonelectrolyte Solutions
  • 13-9 Solutions of Electrolytes
  • 13-10 Colloidal Mixtures
  • Focus on Chromatography
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 14 Chemical Kinetics
  • 14-1 Rate of a Chemical Reaction
  • 14-2 Measuring Reaction Rates
  • 14-3 Effect of Concentration on Reaction Rates: The Rate Law
  • 14-4 Zero-Order Reactions
  • 14-5 First-Order Reactions
  • 14-6 Second-Order Reactions
  • 14-7 Reaction Kinetics: A Summary
  • 14-8 Theoretical Models for Chemical Kinetics
  • 14-9 The Effect of Temperature on Reaction Rates
  • 14-10 Reaction Mechanisms
  • 14-11 Catalysis
  • Focus on Combustion and Explosions
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 15 Principles of Chemical Equilibrium
  • 15-1 Dynamic Equilibrium
  • 15-2 The Equilibrium Constant Expression
  • 15-3 Relationships Involving Equilibrium Constants
  • 15-4 The Magnitude of an Equilibrium Constant
  • 15-5 The Reaction Quotient, Q: Predicting the Direction of Net Change
  • 15-6 Altering Equilibrium Conditions: Le Chtelier's Principle
  • 15-7 Equilibrium Calculations: Some Illustrative Examples
  • Focus on The Nitrogen Cycle and the Synthesis of Nitrogen Compounds
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 16 Acids and Bases
  • 16-1 Arrhenius Theory: A Brief Review
  • 16-2 Bransted Lowry Theory of Acids and Bases
  • 16-3 Self-Ionization of Water and the pH Scale
  • 16-4 Strong Acids and Strong Bases
  • 16-5 Weak Acids and Weak Bases
  • 16-6 Polyprotic Acids
  • 16-7 Ions as Acids and Bases
  • 16-8 Molecular Structure and Acid Base Behavior
  • 16-9 Lewis Acids and Bases
  • Focus on Acid Rain
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 17 Additional Aspects of Acid Base Equilibria
  • 17-1 The Common-Ion Effect in Acid Base Equilibria
  • 17-2 Buffer Solutions
  • 17-3 Acid Base Indicators
  • 17-4 Neutralization Reactions and Titration Curves
  • 17-5 Solutions of Salts of Polyprotic Acids
  • 17-6 Acid Base Equilibrium Calculations: A Summary
  • Focus on Buffers in Blood
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 18 Solubility and Complex-Ion Equilibria
  • 18-1 Solubility Product Constant,
  • 18-2 Relationship Between Solubility and
  • 18-3 Common-Ion Effect in Solubility Equilibria
  • 18-4 Limitations of the Concept
  • 18-5 Criteria for Precipitation and Its Completeness
  • 18-6 Fractional Precipitation
  • 18-7 Solubility and pH
  • 18-8 Equilibria Involving Complex Ions
  • 18-9 Qualitative Cation Analysis
  • Focus on Shells, Teeth, and Fossils
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 19 Spontaneous Change: Entropy and Free Energy
  • 19-1 Spontaneity: The Meaning of Spontaneous Change
  • 19-2 The Concept of Entropy
  • 19-3 Evaluating Entropy and Entropy Changes
  • 19-4 Criteria for Spontaneous Change: The Second Law of Thermodynamics
  • 19-5 Standard Free Energy Change, DG
  • 19-6 Free Energy Change and Equilibrium
  • 19-7 DG and as Functions of Temperature
  • 19-8 Coupled Reactions
  • Focus on Coupled Reactions in Biological Systems
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 20 Electrochemistry
  • 20-1 Electrode Potentials and Their Measurement
  • 20-2 Standard Electrode Potentials
  • 20-3 DG, and
  • 20-4 as a Function of Concentrations
  • 20-5 Batteries: Producing Electricity Through Chemical Reactions
  • 20-6 Corrosion: Unwanted Voltaic Cells
  • 20-7 Electrolysis: Causing Nonspontaneous Reactions to Occur
  • 20-8 Industrial Electrolysis Processes
  • Focus on Membrane Potentials
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 21 Chemistry of the Main-Group Elements I: Groups 1, 2, 13, and 14
  • 21-1 Group 1: The Alkali Metals
  • 21-2 Group 2: The Alkaline Earth Metals
  • 21-3 Ions in Natural Waters: Hard Water
  • 21-4 Group 13 Metals: The Boron Family
  • 21-5 Group 14 Metals: The Carbon Family
  • Focus on Gallium Arsenide
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 22 Main-Group Elements II: Groups 18, 17, 16, 15, and Hydrogen
  • 22-1 Group 18: The Noble Gases
  • 22-2 Group 17: The Halogens
  • 22-3 Group 16: The Oxygen Family
  • 22-4 Group 15: The Nitrogen Family
  • 22-5 Hydrogen: A Unique Element
  • Focus on The Ozone Layer and Its Environmental Role
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 23 The Transition Elements
  • 23-1 General Properties
  • 23-2 Principles of Extractive Metallurgy
  • 23-3 Metallurgy of Iron and Steel
  • 23-4 First-Row Transition Metal Elements: Scandium to Manganese
  • 23-5 The Iron Triad: Iron, Cobalt, and Nickel
  • 23-6 Group 11: Copper, Silver, and Gold
  • 23-7 Group 12: Zinc, Cadmium, and Mercury
  • 23-8 Lanthanides
  • Focus on High Temperature Superconductors
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 24 Complex Ions and Coordination Compounds
  • 24-1 Werner's Theory of Coordination Compounds: An Overview
  • 24-2 Ligands
  • 24-3 Nomenclature
  • 24-4 Isomerism
  • 24-5 Bonding in Complex Ions: Crystal Field Theory
  • 24-6 Magnetic Properties of Coordination Compounds and Crystal Field Theory
  • 24-7 Color and the Colors of Complexes
  • 24-8 Aspects of Complex-Ion Equilibria
  • 24-9 Acid Base Reactions of Complex Ions
  • 24-10 Some Kinetic Considerations 1
  • 24-11 Applications of Coordination Chemistry
  • Focus on Colors in Gemstones
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 25 Nuclear Chemistry
  • 25-1 Radioactivity
  • 25-2 Naturally Occurring Radioactive Isotopes
  • 25-3 Nuclear Reactions and Artificially Induced Radioactivity
  • 25-4 Transuranium Elements
  • 25-5 Rate of Radioactive Decay
  • 25-6 Energetics of Nuclear Reactions
  • 25-7 Nuclear Stability
  • 25-8 Nuclear Fission
  • 25-9 Nuclear Fusion
  • 25-10 Effect of Radiation on Matter
  • 25-11 Applications of Radioisotopes
  • Focus on Radioactive Waste Disposal
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 26 Organic Chemistry
  • 26-1 Organic Compounds and Structures: An Overview
  • 26-2 Alkanes
  • 26-3 Alkenes and Alkynes
  • 26-4 Aromatic Hydrocarbons
  • 26-5 Alcohols, Phenols, and Ethers
  • 26-6 Aldehydes and Ketones
  • 26-7 Carboxylic Acids and Their Derivatives
  • 26-8 Amines
  • 26-9 Heterocyclic Compounds
  • 26-10 Nomenclature of Stereoisomers in Organic Compounds
  • 26-11 An Introduction to Substitution Reactions at Hybridized Carbon Atoms
  • 26-12 Synthesis of Organic Compounds
  • 26-13 Polymerization Reactions
  • Focus on Natural And Synthetic Dyes
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • 27 Chemistry of the Living State
  • 27-1 Chemical Structure of Living Matter: An Overview
  • 27-2 Lipids
  • 27-3 Carbohydrates
  • 27-4 Proteins
  • 27-5 Aspects of Metabolism
  • 27-6 Nucleic Acids
  • Focus on Protein Synthesis and the Genetic Code
  • Summary
  • Integrative Example
  • Exercises
  • Integrative and Advanced Exercises
  • Feature Problems
  • Self Assessment Questions eMedia Exercises
  • Appendixes
  • A Mathematical Operations
  • A-1 Exponential Arithmetic
  • A-2 Logarithms
  • A-3 Algebraic Operations
  • A-4 Graphs
  • A-5 Using Conversion Factors (Dimensional Analysis)
  • B Some Basic Physical Concepts
  • B-1 Velocity and Acceleration
  • B-2 Force and Work
  • B-3 Energy
  • B-4 Magnetism
  • B-5 Static Electricity
  • B-6 Current Electricity
  • B-7 Electromagnetism
  • C SI Units
  • C-1 SI Base Units
  • C-2 SI Prefixes
  • C-3 Derived SI Units A
  • C-4 Units to Be Discouraged or Abandoned A16
  • D Data Tables
  • D-1 Ground-State Electron Configurations
  • D-2 Thermodynamic Properties of Substances at 298.15 K
  • D-3 Equilibrium Constants
  • D-4 Standard Electrode (Reduction) Potentials at 25 C
  • E Concept Mapping
  • F Glossary
  • G Answers to Practice Examples and Selected Exercises
  • Photo Credits
  • Index

Author notes provided by Syndetics

Ralph H. Petrucci

Ralph Petrucci received his B.S. in Chemistry from Union College, Schenectady, NY, and his Ph.D. from the University of Wisconsin Madison. Following ten years of teaching, research, consulting, and directing the NSF Institutes for Secondary School Science Teachers at Case Western Reserve University, Cleveland, OH, Dr. Petrucci joined the planning staff of the new California State University campus at San Bernardino in 1964. There, in addition to his faculty appointment, he served as Chairman of the Natural Sciences Division and Dean of Academic Planning. Professor Petrucci, now retired from teaching, is also a coauthor of General Chemistry with John W. Hill, Terry W. McCreary, and Scott S. Perry.

William S. Harwood

Bill Harwood received his B.Sc. from the University of Massachusetts, Amherst and his Ph.D. in Inorganic Chemistry from Purdue University in 1986. He is currently a Professor of Science Education at Indiana University, Bloomington. Previously, Dr. Harwood was at the Department of Chemistry and Biochemistry at the University of Maryland, College Park. In his current role, Dr. Harwood continues to teach chemistry and conduct research in chemical education. He has received several awards for teaching excellence. Dr. Harwood is also active in the American Chemical Society and the Division of Chemical Education and was a consultant to AAAS project 2061. He is involved in the science reform efforts at both the pre-college and college levels. His research focuses on how best to use technology to improve learning in chemistry.

F. Geoffrey Herring

Geoff Herring received his B.Sc. and his Ph.D. in Physical Chemistry, both from the University of London. He is currently a Professor in the Department of Chemistry of the University of British Columbia, Vancouver. Dr. Herring has research interests in the area of biophysical chemistry and has published over 100 papers in the area of physical chemistry and chemical physics. Recently, Dr. Herring has undertaken studies in the use of information technology and interactive engagement methods in teaching general chemistry with a view to improving student comprehension and learning. Dr. Herring has taught chemistry from undergraduate to graduate levels for 30 years and has twice been the recipient of the Killam Prize for Excellence in Teaching.

Jeffry D. Madura

Jeffry D. Madura received his B.A. from Thiel College and his Ph.D. in Physical Chemistry from Purdue University, He is currently Professor and Chair in the Department of Chemistry and Biochemistry of Duquesne University in Pittsburgh, PA. Dr. Madura's research interests are in the area of computational chemistry and biophysical chemistry, and he has published over 70 papers in the area of physical chemistry and chemical physics. Recently, Dr. Madura has undertaken studies in the use of technology and interactive personal response systems in teaching general and physical chemistry with the goal of improving student comprehension and learning. Dr. Madura has taught chemistry from undergraduate to graduate levels for 15 years and has been the recipient of a Dreyfus Teacher-Scholar Award.

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