Chemistry: The Molecular Nature of Matter and Change - Rilegato

Silberberg, Martin

Rilegato

ISBN 10: 0073101699 ISBN 13: 9780073101699

Casa editrice: McGraw-Hill Education, 2005

Riassunto

Chemistry: The Molecular Nature of Matter and Change by Martin Silberberg has become a favorite among faculty and students. Silberberg’s 4th edition contains features that make it the most comprehensive and relevant text for any student enrolled in General Chemistry. The text contains unprecedented macroscopic to microscopic molecular illustrations, consistent step-by-step worked exercises in every chapter, an extensive range of end-of-chapter problems which provide engaging applications covering a wide variety of freshman interests, including engineering, medicine, materials, and environmental studies. All of these qualities make Chemistry: The Molecular Nature of Matter and Change the centerpiece for any General Chemistry course.

Su questo libro

L'autore:

Martin S. Silberberg received his B.S. in chemistry from the City University of New York in 1966 and his Ph.D. in chemistry from the University of Oklahoma, in 1971.  He then accepted a research position at the Albert Einstein College of Medicine, where he studied the chemical nature of neurotransmission and Parkinson's disease.  In 1977, Dr. Silberberg joined the faculty of Simon's Rock College of Bard (Massachusetts), a liberal arts college known for its excellence in teaching small classes of highly motivated students.  As Head of the Natural Sciences Major and Director of Premedical Studies, he taught courses in general chemistry, organic chemistry, biochemistry, and nonmajors chemistry.  The close student contact afforded him insights into how students learn chemistry, where they have difficulties, and what strategies can help them succeed.  In 1983, Dr. Silberberg decided to apply these insights in a broader context and established a text writing and editing company.  Before writing his own text, he worked on chemistry, biochemistry, and physics texts for several major college publishers.  He resides with his wife and child in Massachusetts.  For relaxation, he cooks, sings, and walks in the woods.

Contenuti:

Chemistry:

The Molecular Nature of Matter and Change

1 Keys to the Study of Chemistry

1.1 Some Fundamental Definitions

The Properties of Matter

The Three States of Matter

The Central Theme in Chemistry

The Importance of Energy in the Study of Matter

1.2 Chemical Arts and the Origins of Modern Chemistry

Prechemical Traditions

The Phlogiston Fiasco and the Impact of Lavoisier

1.3 The Scientific Approach: Developing a Model

1.4 Chemical Problem Solving

Units and Conversion Factors in Calculations

A Systematic Approach to Solving Chemistry Problems

1.5 Measurement in Scientific Study

General Features of SI Units

Some Important SI Units in Chemistry

1.6 Uncertainty in Measurement: Significant Figures

Determining Which Digits Are Significant

Working with Significant Figures in Calculations

Precision, Accuracy, and Instrument Calibration

Chapter Perspective

Chemical Connections to Interdisciplinary Science:Chemistry Problem Solving in the Real World

For Review and Reference

Problems

2The Components of Matter

2.1 Elements, Compounds, and Mixtures: An Atomic Overview

2.2 The Observations That Led to an Atomic View of Matter

2.3 Dalton’s Atomic Theory

Postulates of the Atomic Theory

How the Theory Explains the Mass Laws

The Relative Masses of Atoms

2.4 The Observations That Led to the Nuclear Atom Model

Discovery of the Electron and Its Properties

Discovery of the Atomic Nucleus

2.5 The Atomic Theory Today

Structure of the Atom

Atomic Number, Mass Number, and Atomic Symbol

Isotopes and Atomic Masses of the Elements

Tools of the Laboratory: Mass Spectrometry

A Modern Reassessment of the Atomic Theory

2.6 Elements: A First Look at the Periodic Table

2.7 Compounds: Introduction to Bonding

The Formation of Ionic Compounds

The Formation of Covalent Compounds

The Elements of Life

2.8 Compounds: Formulas, Names, and Masses

Types of Chemical Formulas

Some Advice about Learning Names and Formulas

Names and Formulas of Ionic Compounds

Names and Formulas of Binary Covalent Compounds

An Introduction to Naming Organic Compounds

Molecular Masses from Chemical Formulas

Gallery: Picturing Molecules

2.9 Mixtures: Classification and Separation

Tools of the Laboratory: Basic Separation Techniques

Chapter Perspective

For Review and Reference

Problems

3 Stoichiometry of Formulas and Equations

3.1 The Mole

Defining the Mole

Molar Mass

Interconverting Moles, Mass, and Number of Chemical Entities

Mass Percent from the Chemical Formula

3.2 Determining the Formula of an Unknown Compound

Empirical Formulas

Molecular Formulas

Chemical Formulas and Molecular Structures

3.3 Writing and Balancing Chemical Equations

3.4 Calculating Amounts of Reactant and Product

Stoichiometrically Equivalent Molar Ratios from the Balanced Equation

Chemical Reactions That Occur in a Sequence

Chemical Reactions That Involve a Limiting Reactant

Chemical Reactions in Practice: Theoretical, Actual, and Percent Yields

3.5 Fundamentals of Solution Stoichiometry

Expressing Concentration in Terms of Molarity

Mole-Mass-Number Conversions Involving Solutions

Preparing and Diluting Molar Solutions

Stoichiometry of Chemical Reactions in Solution

Chapter Perspective

For Review and Reference

Problems

4 The Major Classes of Chemical Reactions

4.1 The Role of Water as a Solvent

The Polar Nature of Water

Ionic Compounds in Water

Covalent Compounds in Water

4.2 Writing Equations for Aqueous Ionic Reactions

4.3 Precipitation Reactions

The Key Event: Formation of a Solid from Dissolved Ions

Predicting Whether a Precipitate Will Form

4.4 Acid-Base Reactions

The Key Event: Formation of H2O from H+ and OH–

Acid-Base Titrations

Proton Transfer: A Closer Look at Acid-Base Reactions

4.5 Oxidation-Reduction (Redox) Reactions

The Key Event: Movement of Electrons Between Reactants

Some Essential Redox Terminology

Using Oxidation Numbers to Monitor the Movement of Electron Charge

Balancing Redox Equations

Redox Titrations

4.6 Elements in Redox Reactions

4.7 Reversible Reactions: An Introduction to Chemical Equilibrium

Chapter Perspective

For Review and Reference

Problems

5 Gases and the Kinetic-Molecular Theory

5.1 An Overview of the Physical States of Matter

5.2 Gas Pressure and Its Measurement

Laboratory Devices for Measuring Gas Pressure

Units of Pressure

5.3 The Gas Laws and Their Experimental Foundations

The Relationship Between Volume and Pressure: Boyle’s Law

The Relationship Between Volume and Temperature: Charles’s Law

The Relationship Between Volume and Amount: Avogardro’s Law

Gas Behavior at Standard Conditions

The Ideal Gas

Solving Gas Law Problems

5.4 Further Applications of the Ideal Gas Law

The Density of a Gas

The Molar Mass of a Gas

The Partial Pressure of a Gas in a Mixture of Gases

5.5 The Ideal Gas Law and Reaction Stoichiometry

5.6 The Kinetic-Molecular Theory: A Model for Gas Behavior

How the Kinetic-Molecular Theory Explains the Gas Laws

Effusion and Diffusion

The Chaotic World of Gases: Mean Free Path and Collision Frequency

Chemical Connections to Planetary Science: Structure and Composition of the Earth’s Atmosphere

5.7 Real Gases: Deviations from Ideal Behavior

Chapter Perspective

For Review and Reference

Problems

6 Thermochemistry: Energy Flow and Chemical Change

6.1 Forms of Energy and Their Interconversion

The System and Its Surroundings

Energy Flow to and from a System

Heat and Work: Two Forms of Energy Transfer

The Law of Energy Conservation

Units of Energy

State Functions and the Path Independence of the Energy Change

6.2 Enthalpy: Heats of Reaction and Chemical Change

The Meaning of Enthalpy

Comparing ¿E and ¿H

Exothermic and Endothermic Processes

Some Important Types of Enthalpy Change

6.3 Calorimetry: Laboratory Measurement of Heats of Reaction

Specific Heat Capacity

The Practice of Calorimetry

6.4 Stoichiometry of Thermochemical Equations

6.5 Hess’s Law of Heat Summation

6.6 Standard Heats of Reaction (¿Hrxn0)

Formation Equations and Their Standard Enthalpy Changes

Determining ¿Hrxn0 from ¿Hf0 Values of Reactants and Products

Chemical Connections to Environmental Science: The Future of Energy Use

Chapter Perspective

For Review and Reference

Problems

7 Quantum Theory and Atomic Structure

7.1 The Nature of Light

The Wave Nature of Light

The Particle Nature of Light

7.2 Atomic Spectra

The Bohr Model of the Hydrogen Atom

Limitations of the Bohr Model

The Energy States of the Hydrogen Atom

Tools of the Laboratory: Spectrophotometry in Chemical Analysis

7.3 The Wave-Particle Duality of Matter and Energy

The Wave Nature of Electrons and the Particle Nature of Photons

The Heisenberg Uncertainty Principle

7.4 The Quantum-Mechanical Model of the Atom

The Atomic Orbital and the Probable Location of the Electron

Quantum Numbers of an Atomic Orbital

Shapes of Atomic Orbitals

Energy Levels of the Hydrogen Atom

Chapter Perspective

For Review and Reference

Problems

8 Electron Configuration and Chemical Periodicity

8.1 Development of the Periodic Table

8.2 Characteristics of Many-Electron Atoms

The Electron-Spin Quantum Number

The Exclusion Principle

Electrostatic Effects and the Energy-Level Splitting

8.3 The Quantum-Mechanical Model and the Periodic Table

Building Up Periods 1 and 2

Building Up Period 3

Electron Configurations Within Groups

The First d-Orbital Transition Series: Building Up Period 4

General Principles of Electron Configurations

Unusual Configurations: Transition and Inner Transition Elements

8.4 Trends in Three Key Atomic Properties

Trends in Atomic Size

Trends in Ionization Energy

Trends in Electron Affinity

8.5 Atomic Structure and Chemical Reactivity

Trends in Metallic Behavior

Properties of Monatomic Ions

Chapter Perspective

For Review and Reference

Problems

9Models of Chemical Bonding

9.1 Atomic Properties and Chemical Bonds

The Three Types of Chemical Bonding

Lewis Electron-Dot Symbols: Depicting Atoms in Chemical Bonding

9.2 The Ionic Bonding Model

Energy Considerations in Ionic Bonding: The Importance of Lattice Energy

Periodic Trends in Lattice Energy

H ow the Model Explains the Properties of Ionic Compounds

9.3 The Covalent Bonding Model

The Formation of a Covalent Bond

Properties of a Covalent Bond: Bond Energy and Bond Length

How the Model Explains the Properties of Covalent Compounds

Tools of the Laboratory: Infrared Spectroscopy

9.4 Bond Energy and Chemical Change

Changes in Bond Strength: Where Does ¿Hrxn0 Come From?

Using Bond Energies to Calculate ¿Hrxn0

Relative Bond Strengths in Fuels and Foods

9.5 Between the Extremes: Electronegativity and Bond Polarity

Electronegativity

Polar Covalent Bonds and Bond Polarity

The Partial Ionic Character of Polar Covalent Bonds

The Continuum of Bonding Across a Period

9.6 An Introduction to Metallic Bonding

The Electron-Sea Model

How the Model Explains the Properties of Metals

Chapter Perspective

For Review and Reference

Problems

10The Shapes of Molecules

10.1 Depicting Molecules and Ions with Lewis Structures

Using the Octet Rule to Write Lewis Structures

Resonance: Delocalized Electron-Pair Bonding

Formal Charge: Selecting the Most Important (?) Resonance Structure

Lewis Structures for Exceptions to the Octet Rule

10.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory and Molecular Shape

Electron-Group Arrangements and Molecular Shapes

The Molecular Shape with Two Electron Groups (Linear Arrangement)

Molecular Shapes with Three Electron Groups (Trigonal Planar Arrangement)

Molecular Shapes with Four Electron Groups (Tetrahedral Arrangement)

Molecular Shapes with Five Electron Groups (Trigonal

Bipyramidal Arrangement)

Molecular Shapes with Six Electron Groups (Octahedral Arrangement)

Using VSEPR Theory to Determine Molecular Shape

Molecular Shapes with More Than One Central Atom

Gallery: Molecular Beauty: Odd Shapes with Useful Functions

10.3 Molecular Shape and Molecular Polarity

Bond Polarity, Bond Angle, and Dipole Moment

The Effect of Molecular Polarity on Behavior

Chapter Perspective

Chemical Connections in Sensory Physiology: Molecular Shape, Biological Receptors, and the Sense of Smell

For Review and Reference

Problems

Su questa edizione

• Editore: McGraw-Hill Education
• Data di pubblicazione: 2005
• ISBN 10: 0073101699
• ISBN 13: 9780073101699
• Rilegatura: Copertina rigida
• Numero edizione: 4
• Numero di pagine: 1088