Introduction to Chemical Principles

ISBN-10: 0321666046

ISBN-13: 9780321666048

Edition: 10th 2011

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This solid, yet value-priced paperback gives students the background and confidence they need to succeed in chemistry. Stoker focuses on the most important topics omitting organic and biochemistry chapters and teaches the problem-solving skills students need. Each topic is developed at "ground level," and continues step by step until the level of sophistication required for a further chemistry course is attained.
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Book details

Edition: 10th
Copyright year: 2011
Publisher: Prentice Hall PTR
Publication date: 1/4/2010
Binding: Paperback
Pages: 736
Size: 8.00" wide x 10.00" long x 1.00" tall
Weight: 3.146
Language: English

NOTE: Each chapter concludes with a Summary, Key Terms, Practice Problems, and Multiple-Choice Practice Test
The Science of Chemistry
Chemistry���A Scientific Discipline
Scientific Research and Technology
The Scope of Chemistry and Chemical Technology
How Chemists Discover Things���The Scientific Method
The Limitations of the Scientific Method
The Limitations of Science
Numbers from Measurements
The Importance of Measurement
Exact and Inexact Numbers
Accuracy, Precision, and Error
Uncertainty in Measurements
Significant Figures
Significant Figures and Mathematical Operations
Scientific Notation
Mathematical Operations in Scientific Notation
Unit Systems and Dimensional Analysis
The Metric System of Units
Metric Units of Length
Metric Units of Mass
Metric Units of Volume
Units in Mathematical Operations
Conversion Factors
Dimensional Analysis
Equivalence Conversion Factors Other Than Density
Percentage and Percent Error
Temperature Scales
Basic Concepts About Matter
Chemistry���The Study of Matter
Physical States of Matter
Properties of Matter
Changes in Matter
Pure Substances and Mixtures
Heterogeneous and Homogeneous Mixtures
Elements and Compounds
Discovery and Abundance of the Elements
The Human Side of Chemistry 1: Joseph Priestley (1733���1804)
Names and Chemical Symbols of the Elements
The Human Side of Chemistry 2: Jöns Jakob Berzelius (1779���1848)
The Atom
The Human Side of Chemistry 3: John Dalton (1766���1844)
The Molecule
Natural and Synthetic Compounds
Chemical Formulas
Subatomic Particles, Isotopes, and Nuclear Chemistry
Subatomic Particles: Protons, Neutrons, and Electrons
Atomic Number and Mass Number
Atomic Masses
Evidence Supporting the Existence and Arrangement of Subatomic Particles
Nuclear Stability and Radioactivity
The Human Side of Chemistry 4: Ernest Rutherford (1871���1937)
Half-Life: A Measure of Nuclear stability
The Nature of Natural Radioactive Emissions
Equations for Radioactive Decay
Transmutation and Bombardment Reactions
Positron Emission and Electron Capture
Neutron-to-Proton Ratio and Type of Radioactive Decay
Radioactive Decay Series
Electronic Structure and Chemical Periodicity
The Periodic Law
The Periodic Table
The Human Side of Chemistry 5: Dmitri Ivanovich Mendeleev (1834���1907)
The Energy of an Electron
The Human Side of Chemistry 6: Erwin Schrödinger (1887���1961)
Electron Shells
Electron Subshells
Electron Orbitals
Electron Configurations
Orbital Diagrams
Electron Configurations and the Periodic Law
Electron Configurations and the Periodic Table
Classification Systems for the Elements
Chemical Periodicity
Chemical Bonds
Types of Chemical Bonds
Valence Electrons and Lewis Symbols
The Human Side of Chemistry 7: Gilbert Newton Lewis (1875���1946)
The Octet Rule
The Ionic Bond Model
The Sign and Magnitude of Ionic Charge
Lewis Structures for Ionic Compounds
Chemical Formulas for Ionic Compounds
Structure of Ionic Compounds
Polyatomic Ions
The Covalent Bond Model
Lewis Structures for Molecular Compounds
Single, Double, and Triple Covalent Bonds
Valence Electron Count and Number of Covalent Bonds Formed
Coordinate Covalent Bonds
Resonance Structures
Systematic Procedures for Drawing Lewis Structures
Molecular Geometry
The Human Side of Chemistry 8: Linus Carl Pauling (1901���1994)
Bond Polarity
Molecular Polarity
Chemical Nomenclature
Classification of Compounds for Nomenclature Purposes
Types of Binary Ionic Compounds
Nomenclature for Binary Ionic Compounds
Nomenclature for Ionic Compounds Containing Polyatomic Ions
Nomenclature for Binary Molecular Compounds
Nomenclature for Acids
Nomenclature Rules���A Summary
Chemical Calculations: the Mole Concept and Chemical Formulas
The Law of Definite Proportions
The Human Side of Chemistry 9: Joseph-Louis Proust (1754���1826)
Calculation of Formula Masses
Significant Figures and Atomic Mass
Percent Composition of a Compound
The Mole: the Chemist's Counting Unit
The Human Side of Chemistry 10: Lorenzo Romano Amedeo Carlo Avogadro (1776���1856)
The Mass of a Mole
Significant Figures and Avogadro's Number
Relationship between Atomic Mass Units and Gram Units
The Mole and Chemical Formulas
The Mole and Chemical Calculations
Purity of Samples
Empirical and Molecular Formulas
Determination of Empirical Formulas
Determination of Molecular Formulas
Chemical Calculations Involving Chemical Equations
The Law of Conservation of Mass
The Human Side of Chemistry 11: Antoine-Laurent Lavoisier (1743���1794)
Writing Chemical Equations
Chemical Equation Coefficients
Balancing Procedures for Chemical Equations
Special Symbols Used in Chemical Equations
Classes of Chemical Reactions
Chemical Equations and the Mole Concept
Balanced Chemical Equations and the Law of Conservation of Mass
Calculations Based on Chemical Equations���Stoichiometry
The Limiting Reactant Concept
Yields: Theoretical, Actual, and Percent
Simultaneous and Sequential Chemical Reactions
States of Matter
Factors That Determine Physical State
Property Differences among Physical States
The Kinetic Molecular Theory of Matter
The Solid State
The Liquid State
The Gaseous State
A Comparison of Solids, Liquids, and Gases
Endothermic and Exothermic Changes of State
Heat Energy and Specific Heat
Temperature Changes as a Substance Is Heated
Energy and Changes of State
Heat Energy Calculations
Evaporation of Liquids
Vapor Pressure of Liquids
Boiling and Boiling Points
Intermolecular Forces in Liquids
Hydrogen Bonding and the Properties of Water
Gas Laws
Properties of Some Common Gases
Gas Law Variables
Boyle's Law: A Pressure Volume Relationship
The Human Side of Chemistry 12: Robert Boyle (1627���1691)
Charles's Law: A Temperature Volume Relationship
The Human Side of Chemistry 13: Jacques Alexandre Cÿsar Charles (1746���1823)
Gay-Lussac's Law: A Temperature Pressure Relationship
The Human Side of Chemistry 14: Joseph Louis Gay-Lussac (1778���1850)
The Combined Gas Law
Avogadro's Law
An Ideal Gas
The Ideal Gas Law
Modified Forms of the Ideal Gas Law Equation
Volumes of Gases in Chemical Reactions
Volumes of Gases and the Limiting Reactant Concept
Molar Volume of a Gas
Chemical Calculations Using Molar Volume
Mixtures of Gases
Dalton's Law of Partial Pressures
Characteristics of Solutions
Solution Formation
Solubility Rules
Solution Concentrations
Concentration: Percentage of Solute
Concentration: Parts per Million and Parts per Billion
Concentration: Molarity
Concentration: Molality
Molarity and Chemical Equations
Calculations Involving Volume: A Summary
Acids, Bases, and Salts
Arrhenius Acid Base Theory
The Human Side of Chemistry 15: Svante August Arrhenius (1859���1927)
Brinsted Lowry Acid Base Theory
Conjugate Acids and Bases
Mono-, Di-, and Triprotic Acids
Strengths of Acids and Bases
Reactions of Acids
Reactions of Bases
Reactions of Salts
Self-Ionization of Water
The pH Scale
Hydrolysis of Salts
Acid Base Titrations
Chemical Equations: Net Ionic and Oxidation-Reduction
Types of Chemical Equations
Ionic and Net Ionic Equations
Oxidation Reduction Terminology
Oxidation Numbers
Redox and Nonredox Chemical Reactions
Balancing Oxidation Reduction Equations
Oxidation Number Method for Balancing Redox Equations
Half-Reaction Method for Balancing Redox Equations
Disproportionation Reactions
Stoichiometric Calculations Involving Ions
Reaction Rates and Chemical Equilibrium
Collision Theory
Endothermic and Exothermic Chemical Reactions
Factors That Influence Chemical Reaction Rates
Chemical Equilibrium
Equilibrium Mixture Stoichiometry
Equilibrium Constants
Equilibrium Position
Temperature Dependency of Equilibrium Constants
Le Chotelier's Principle
The Human Side of Chemistry 16: Henri-Louis Le Chotelier (1850���1936)
Forcing Chemical Reactions to Completion
Answer to Odd-Numbered Problems and All Self-Test Problems
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