General, Organic, and Biological Chemistry / H. Stephen Stoker.

By:

Stoker, H. Stephen

Material type: Text

TextPublication details: Boston : Houghton Mifflin Company, c.2001.Edition: 2nd edDescription: 1 v. (various pagings) : ill. (chiefly col.) ; 29 cm. + 1 CD-ROM (4 3/4 in.)ISBN:

0618052062

Subject(s):

DDC classification:

540 STO

Holdings
Item type	Current library	Call number	Status	Date due	Barcode
Standard Loan	Moylish Library Main Collection	540 STO (Browse shelf(Opens below))	Available		39002000212416

Includes index.

Table of contents provided by Syndetics

Note: Organic and Biological Chemistry consists of Parts II and III (Chapters 1226) of General, Organic, and Biological Chemistry. Each chapter concludes with Concepts to Remember, Key Terms, Exercises and Problems, Additional Problems, and Grid Problems
I General Chemistry
1 Basic Concepts About Matter
1.1 Chemistry--The Study of Matter
1.2 Physical States of Matter
1.3 Properties of Matter
1.4 Changes in Matter Chemistry at a Glance: Use of the Terms Physical and Chemical
1.5 Pure Substances and Mixtures
1.6 Elements and Compounds Chemistry at a Glance: Classes and Properties of Matter
1.7 Discovery and Abundance of the Elements
1.8 Names and Symbols of the Elements
1.9 Atoms and Molecules
1.10 Chemical Formulas Chemical Connections: "Good" versus "Bad" Properties for a Chemical Substance
Elements Necessary for Human Life
2 Measurements in Chemistry
2.1 Measurement Systems
2.2 Metric System Units
2.3 Uncertainty in Measurement and Significant Figures
2.4 Significant Figures and Mathematical Operations
2.5 Scientific Notation Chemistry at a Glance: Important Concepts Associated with Measurement
2.6 Conversion Factors and Dimensional Analysis Chemistry at a Glance: Conversion Factors
2.7 Density
2.8 Temperature and Heat Energy Chemical Connections: Body Density and Percent Body Fat
Normal Human Body Temperature
3 Atomic Structure and the Periodic Table
3.1 Internal Structure of the Atom
3.2 Experimental Evidence for the Existence of Subatomic Particles
3.3 Atomic Number and Mass Number Chemistry at a Glance: Atomic Structure
3.4 The Periodic Law and the Periodic Table
3.5 Metals and Nonmetals
3.6 Electron Arrangements Within Atoms
3.7 Specification of Electronic Structure
3.8 The Electronic Basis for the Periodic Law and the Periodic Table
3.9 Classification of the Elements Chemistry at a Glance: Element Classification Schemes and the Periodic Table Chemical Connections: Pritium, Deuterium, and Tritium--
The Three Isotopes of Hydrogen
Calcium, Your Body, and the Periodic Law
Importance of Metallic and Nonmetallic Trace Elements for Human Health. Electrons in Excited States
4 Chemical Bonding: The Ionic Bond Model
4.1 Chemical Bonds
4.2 Valence Electrons and Lewis Structures
4.3 The Octet Rule
4.4 The Ionic Bond Model
4.5 Determination of Ionic Charge Magnitude
4.6 Ionic Compound Formation
4.7 Formulas for Ionic Compounds
4.8 The Structure of Ionic Compounds
4.9 Naming Binary Ionic Compounds Chemistry at a Glance: Ionic Bonds and Ionic Compounds
4.10 Polyatomic Ions
4.11 Formula and Names for Ionic Compounds Containing Polyatomic Ions Chemistry at a Glance: Nomenclature of Ionic Compounds Chemical Connections: Fresh Water, Seawater, Hard Water, and Soft Water: A Matter of Ions. Sodium Chloride: The World's Most Common Food Additive
5 Chemical Bonding: The Covalent Bond Model
5.1 The Covalent Bond Model
5.2 Lewis Structures for Molecular Compounds
5.3 Single, Double, and Triple Covalent Bonds
5.4 Valence Electrons and Number of Covalent Bonds Formed
5.5 Coordinate Covalent Bonds
5.6 Systematic Procedures for Drawing Lewis Structures
5.7 Bonding in Compounds with Polyatomic Ions Present
5.8 The Shapes of Molecules
5.9 Electronegativity Chemistry at a Glance: The Shape (Geometry) of Molecules
5.10 Bond Polarity Chemistry at a Glance: Covalent Bonds and Molecular Compounds
5.11 Molecular Polarity
5.12 Naming Binary Molecular Compounds Chemical Connections: Nitric Oxide: A Molecule Whose Bonding Does Not Follow "The Rules. "Molecular Shape and Odor
6 Chemical Calculations: Formula Masses, Moles, and Chemical Equations
6.1 Formula Masses
6.2 The Mole: A Counting Unit for Chemists
6.3 The Mass of a Mole
6.4 The Mole and Chemical Formulas
6.5 The Mole and Chemical Calculations
6.6 Writing and Balancing Chemical Equations
6.7 Chemical Equations and the Mole Concept
6.8 Chemical Calculations Using Chemical Equations Chemistry at a Glance: Relationships Involving the Mole Concept Chemical Connections: "Laboratory-Sized" Amounts Versus "Industrial Chemistry-Sized" Amounts
7 Gases, Liquids and Solids
7.1 The Kinetic Molecular Theory of Matter
7.2 Kinetic Molecular Theory and Physical States
7.3 Gas Law Variables
7.4 Boyle's Law: A Pressure-Volume Relationship
7.5 Charles's Law: A Temperature-Volume Relationship
7.6 The Combined Gas Law
7.7 The Ideal Gas Law
7.8 Dalton's Law of Partial Pressures Chemistry at a Glance: The Gas Laws
7.9 Changes of State
7.10 Evaporation of Liquids
7.11 Vapor Pressure of Liquids
7.12 Boiling and Boiling Point
7.13 Intermolecular Forces in Liquids Chemistry at a Glance: Intermolecular Forces Chemical Connections: The Importance of Gas Densities
The Exchange of the Respiratory Gases, Oxygen and Carbon Dioxide
8 Solutions
8.1 Characteristics of Solutions
8.2 Solubility and Saturated Solutions
8.3 Solution Formation
8.4 Solubility Rules
8.5 Solution Concentration Units Chemistry at a Glance: Solutions and Solution Concentrations
8.6 Colloidal Dispersions
8.7 Colligative Properties of Solutions
8.8 Osmosis and Osmotic Pressure Chemistry at a Glance: Colligative Properties of Solutions
8.9 Dialysis Chemical Connections: Factors Affecting Gas Solubility. Solubility of Vitamins
Controlled-Release Drugs: Regulating Concentration, Rate, and Location of Release
9 Chemical Reactions
9.1 Types of Chemical Reactions
9.2 Redox and Nonredox Reactions Chemistry at a Glance: Types of Reactions
9.3 Terminology Associated with Redox Processes
9.4 Collision Theory and Chemical Reactions
9.5 Exothermic and Endothermic Reactions
9.6 Factors That Influence Reaction Rates Chemistry at a Glance: Factors That Influence Reaction Rates
9.7 Chemical Equilibrium
9.8 Equilibrium Constants
9.9 Altering Equilibrium Conditions: LeChacirc;telier's Principle Chemical Connections: Smog Formation: A Set of Simple Reactions
Stratospheric Ozone: An Equilibrium Situation. Oxygen, Hemoglobin, Equilibrium, and LeChacirc;telier's Principle
10 Acids, Bases and Salts
10.1 Arrhenius Acid-Base Theory
10.2 Bronsted-Lowry Acid-Base Theory
10.3 Mono-, Di-, and Triprotic Acids
10.4 Strengths of Acids and Bases
10.5 Ionization Constants for Acids and Bases
10.6 Salts
10.7 Acid-Base Neutralization Reactions
10.8 Self-Ionization of Water
10.9 The pH Concept
10.10 pKa Method for Expressing Acid Strength Chemistry at a Glance: Acids and Acid Solutions
10.11 the pH of Aqueous Salt Solutions
10.12 Buffers Chemistry at a Glance: Buffer Systems
10.11 The Henderson-Hasselbalch Equation
10.12 Electrolytes
10.15 Acid-Base Titrations Chemical Connections: Acid Rain: Excess Acidity
Blood Plasma pH and Hydrolysis
Buffering Action in Human Blood. Electrolytes and Body Fluids
11 Nuclear Chemistry
11.1 Stable and Unstable Nuclides
11.2 The Nature of Radioactivity
11.3 Radioactive Decay
11.4 Rate of Radioactive Decay
11.5 Transmutation and Bombardment Reactions
11.6 Radioactive Decay Series
11.7 Ionizing Effects of Radiation Chemistry at a Glance: Terminology Associated with Nuclear Reactions
11.8 Biological Effects of Radiation Chemistry at a Glance: Ionizing Radiation
11.9 Detection of Radiation
11.10 Sources of Radiation Exposure
11.11 Nu