Introduction to Chemical Principles
Häftad, Engelska, 2013
4 099 kr
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Newly updated based on extensive reviewer feedback, this affordable introductory text remains focused on the essentials necessary for success in General Chemistry. Introduction to Chemistry Principles, Eleventh Edition focuses on the most important topics — omitting organic and biochemistry chapters — and teaches the problem-solving skills readers need. Each topic is introduced and developed step by step until reaching the level of sophistication required for further course work. Note: There is no difference in content between the version with the plain cover and the version with the white and orange cover.
Produktinformation
- Utgivningsdatum2013-02-06
- Mått200 x 260 x 250 mm
- Vikt1 738 g
- FormatHäftad
- SpråkEngelska
- Antal sidor800
- Upplaga11
- FörlagPearson Education (US)
- ISBN9780321814630
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- NOTE: Each chapter concludes with Concepts to Remember, Key Terms, Practice Problems, Multi-Concept Problems and Multiple-Choice Practice Test.Chapter 1: The Science of Chemistry1.1 Chemistry-A Scientific Discipline1.2 Scientific Research and Technology1.3 The Scope of Chemistry1.4 How Chemists Discover Things-The Scientific Method1.5 The Limitations of the Scientific Method1.6 Application Limitations for Methods of ScienceChapter 2: Numbers from Measurements2.1 The Importance of Measurement2.2 Exact and Inexact Numbers2.3 Accuracy, Precision, and Error2.4 Uncertainty in Measurements2.5 Significant Figures2.6 Significant Figures and Mathematical Operations2.7 Expressing Numbers in Scientific Notation2.8 Mathematical Operations in Scientific NotationChapter 3: Unit Systems and Dimensional Analysis3.1 The Metric System of Units3.2 Metric Units of Length3.3 Metric Units of Mass3.4 Metric Units of Volume3.5 Units in Mathematical Operations3.6 Conversion Factors3.7 Dimensional Analysis3.8 Density3.9 Equivalence Conversion Factors Other Than Density3.10 Percentage and Percent Error3.11 Temperature ScalesChapter 4: Basic Concepts About Matter4.1 Chemistry-The Study of Matter4.2 Physical States of Matter4.3 Properties of Matter4.4 Changes in Matter4.5 Pure Substances and Mixtures4.6 Heterogeneous and Homogeneous Mixtures4.7 Elements and Compounds4.8 Discovery and Abundance of the ElementsTHE HUMAN SIDE OF CHEMISTRY 1: Joseph Priestley (1733-1804)4.9 Names and Chemical Symbols of the ElementsTHE HUMAN SIDE OF CHEMISTRY 2: Jöns Jakob Berzelius (1779-1848)Chapter 5: Atoms, Molecules, and Subatomic Particles5.1 The AtomTHE HUMAN SIDE OF CHEMISTRY 3: John Dalton (1766-1844)5.2 The Molecule5.3 Natural and Synthetic Compounds5.4 Chemical Formulas5.5 Subatomic Particles: Protons, Neutrons, and Electrons5.6 Atomic Number and Mass Number5.7 Isotopes5.8 Atomic Masses5.9 Evidence Supporting the Existence and Arrangement of Subatomic ParticlesTHE HUMAN SIDE OF CHEMISTRY 4: Ernest Rutherford (1871-1937)Chapter 6: Electronic Structure and Chemical Periodicity6.1 The Periodic Law6.2 The Periodic TableTHE HUMAN SIDE OF CHEMISTRY 5: Dmitri Ivanovich Mendeleev (1834-1907)6.3 The Energy of an ElectronTHE HUMAN SIDE OF CHEMISTRY 6: Erwin Schrödinger (1887-1961)6.4 Electron Shells6.5 Electron Subshells6.6 Electron Orbitals6.7 Electron Configurations6.8 Electron Orbital Diagrams6.9 Electron Configurations and the Periodic Law6.10 Electron Configurations and the Periodic Table6.11 Classification Systems for the Elements6.12 Chemical PeriodicityChapter 7: Chemical Bonds7.1 Types of Chemical Bonds7.2 Valence Electrons and Lewis SymbolsTHE HUMAN SIDE OF CHEMISTRY 7: Gilbert Newton Lewis (1875-1946)7.3 The Octet Rule7.4 The Ionic Bond Model7.5 The Sign and Magnitude of Ionic Charge7.6 Lewis Structures for Ionic Compounds7.7 Chemical Formulas for Ionic Compounds7.8 Structure of Ionic Compounds7.9 Polyatomic Ions7.10 The Covalent Bond Model7.11 Lewis Structures for Molecular Compounds7.12 Single, Double, and Triple Covalent Bonds7.13 Valence Electron Count and Number of Covalent Bonds Formed7.14 Coordinate Covalent Bonds7.15 Resonance Structures7.16 Systematic Procedures for Drawing Lewis Structures7.17 Molecular Geometry7.18 ElectronegativityTHE HUMAN SIDE OF CHEMISTRY 8: Linus Carl Pauling (1901-1994)7.19 Bond Polarity7.20 Molecular PolarityChapter 8: Chemical Nomenclature8.1 Classification of Compounds for Nomenclature Purposes8.2 Types of Binary Ionic Compounds8.3 Nomenclature for Binary Ionic Compounds8.4 Chemical Formulas for Polyatomic Ions8.5 Nomenclature for Ionic Compounds Containing Polyatomic Ions8.6 Nomenclature for Binary Molecular Compounds8.7 Nomenclature for Acids8.8 System Procedures for Using Nomenclature RulesChapter 9: Chemical Calculations: The Mole Concept and Chemical Formulas9.1 The Law of Definite ProportionsTHE HUMAN SIDE OF CHEMISTRY 9: Joseph-Louis Proust (1754-1826)9.2 Calculation of Formula Masses9.3 Significant Figures and Atomic Mass9.4 Mass Percent Composition of a Compound9.5 The Mole: The Chemist's Counting UnitTHE HUMAN SIDE OF CHEMISTRY 10: Lorenzo Romano Amedeo Carlo Avogadro (1776--1856)9.6 The Mass of a Mole9.7 Significant Figures and Avogadro's Number9.8 Relationship between Atomic Mass Units and Gram Units9.9 The Mole and Chemical Formulas9.10 The Mole and Chemical Calculations9.11 Purity of Samples9.12 Empirical and Molecular Formulas9.13 Determination of Empirical Formulas9.14 Determination of Molecular FormulasChapter 10: Chemical Calculations Involving Chemical Equations10.1 The Law of Conservation of MassTHE HUMAN SIDE OF CHEMISTRY 11: Antoine-Laurent Lavoisier (1743-1794)10.2 Writing Chemical Equations10.3 Chemical Equation Coefficients10.4 Balancing Procedures for Chemical Equations10.5 Special Symbols Used in Chemical Equations10.6 Classes of Chemical Reactions10.7 Chemical Equations and the Mole Concept10.8 Balanced Chemical Equations and the Law of Conservation of Mass10.9 Calculations Based on Chemical Equations-Stoichiometry10.10 The Limiting Reactant Concept10.11 Yields: Theoretical, Actual, and Percent10.12 Simultaneous and Sequential Chemical ReactionsChapter 11: States of Matter11.1 Factors That Determine Physical State11.2 Property Differences among Physical States11.3 The Kinetic Molecular Theory of Matter11.4 The Solid State11.5 The Liquid State11.6 The Gaseous State11.7 A Comparison of Solids, Liquids, and Gases11.8 Endothermic and Exothermic Changes of State11.9 Heat Energy and Specific Heat11.10 Temperature Changes as a Substance Is Heated11.11 Energy and Changes of State11.12 Heat Energy Calculations11.13 Evaporation of Liquids11.14 Vapor Pressure of Liquids11.15 Boiling and Boiling Points11.16 Intermolecular Forces in Liquids11.17 Hydrogen Bonding and the Properties of WaterChapter 12: Gas Laws12.1 Properties of Some Common Gases12.2 Gas Law Variables12.3 Boyle's Law: A Pressure--Volume RelationshipTHE HUMAN SIDE OF CHEMISTRY 12: Robert Boyle (1627-1691)12.4 Charles's Law: A Temperature--Volume RelationshipTHE HUMAN SIDE OF CHEMISTRY 13: Jacques Alexandre César Charles (1746-1823)12.5 Gay-Lussac's Law: A Temperature--Pressure RelationshipTHE HUMAN SIDE OF CHEMISTRY 14: Joseph Louis Gay-Lussac (1778-1850)12.6 The Combined Gas Law12.7 Avogadro's Law12.8 An Ideal Gas12.9 The Ideal Gas Law12.10 Modified Forms of the Ideal Gas Law Equation12.11 Volumes of Gases in Chemical Reactions12.12 Volumes of Gases and the Limiting Reactant Concept12.13 Molar Volume of a Gas12.14 Chemical Calculations Using Molar Volume12.15 Mixtures of Gases12.16 Dalton's Law of Partial PressuresChapter 13: Solutions13.1 Characteristics of Solutions13.2 Solubility13.3 Solution Formation13.4 Solubility Rules13.5 Solution Concentrations13.6 Percentage Concentration Unit13.7 Parts per Million and Parts per Billion Concentration Unit13.8 Molarity Concentration Units13.9 Molality and Chemical Reactions in Solution13.10 Dilution Calculations13.11 Molarity Concentration UnitChapter 14: Acids, Bases, and Salts14.1 Arrhenius Acid--Base TheoryTHE HUMAN SIDE OF CHEMISTRY 15: Svante August Arrhenius (1859-1927)14.2 Brønsted--Lowry Acid--Base Theory14.3 Conjugate Acids and Bases14.4 Mono-, Di-, and Triprotic Acids14.5 Strengths of Acids and Bases14.6 Salts14.7 Reactions of Acids14.8 Reactions of Bases14.9 Reactions of Salts14.10 Self-Ionization of Water14.11 The pH Scale14.12 Hydrolysis of Salts14.13 Buffers14.14 Acid-Base TitrationsChapter 15: Chemical Equations: Net Ionic and Oxidation-Reduction15.1 Types of Chemical Equations15.2 Electrolytes15.3 Ionic and Net Ionic Equations15.4 Oxidation--Reduction Terminology15.5 Oxidation Numbers15.6 Redox and Nonredox Chemical Reactions15.7 Balancing Oxidation--Reduction Equations15.8 Oxidation Number Method for Balancing Redox Equations15.9 Half-Reaction Method for Balancing Redox Equations15.10 Disproportionation Reactions15.11 Stoichiometric Calculations Involving IonsChapter 16: Reaction Rates and Chemical Equilibrium16.1 Collision Theory16.2 Endothermic and Exothermic Chemical Reactions16.3 Factors That Influence Chemical Reaction Rates16.4 Chemical Equilibrium16.5 Equilibrium Mixture Stoichiometry16.6 Equilibrium Constants16.7 Equilibrium Position16.8 Temperature Dependency of Equilibrium Constants16.9 Le Châtelier's PrincipleTHE HUMAN SIDE OF CHEMISTRY 16: Henri-Louis Le Châtelier (1850-1936)16.10 Forcing Chemical Reactions to CompletionGlossaryAnswer to Odd-Numbered Problems and All Self-Test ProblemsIndex