General chemistry

By:

Ebbing, Darrell D

Contributor(s):

Gammon, Steven D

Material type: Text

TextPublication details: Delhi ; Cengage Learning India Private Limited,: 2009.Edition: 9th editionDescription: xxxviii, 1030 Pages, [82] : ill. (some col.)ISBN:

9788131518700
8131518701

Subject(s):

Chemistry

DDC classification:

540 EBB

Online resources:

Contents:

I. Basics of Chemistry -- 1. Chemistry and Measurement -- 1.1. Modern Chemistry: A Brief Glimpse -- 1.2. Experiment and Explanation -- 1.3. Law of Conservation of Mass -- 1.4. Matter: Physical State and Chemical Constitution -- 1.5. Measurement and Significant Figures -- 1.6. SI Units -- 1.7. Derived Units -- 1.8. Units and Dimensional Analysis (Factor-Label Method) -- 2. Atoms, Molecules, and Ions -- 2.1. Atomic Theory of Matter -- 2.2. The Structure of the Atom -- 2.3. Nuclear Structure -- 2.4. Atomic Masses -- 2.5. Periodic Table of the Elements -- 2.6. Chemical Formulas -- 2.7. Organic Compounds -- 2.8. Naming Simple Compounds -- 2.9. Writing Chemical Equations -- 2.10. Balancing Chemical Equations -- 3. Calculations with Chemical Formulas and Equations -- 3.1. Molecular Mass and Formula Mass -- 3.2. The Mole Concept -- 3.3. Mass Percentages from the Formula -- 3.4. Elemental Analysis: Percentages of Carbon, Hydrogen, and Oxygen -- 3.5. Determining Formulas -- 3.6. Molar Interpretation of a Chemical Equation -- 3.7. Amounts of Substances in a Chemical Reaction -- 3.8. Limiting Reactant -- 4. Chemical Reactions -- 4.1. Ionic Theory of Solutions and Solubility Rules -- 4.2. Molecular and Ionic Equations -- 4.3. Precipitation Reactions -- 4.4. Acid-Base Reactions -- 4.5. Oxidation-Reduction Reactions -- 4.6. Balancing Simple Oxidation-Reduction Equations -- 4.7. Molar Concentration -- 4.8. Diluting Solutions -- 4.9. Gravimetric Analysis -- 4.10. Volumetric Analysis -- 5. The Gaseous State -- 5.1. Gas Pressure and Its Measurement -- 5.2. Empirical Gas Laws -- 5.3. The Ideal Gas Law -- 5.4. Stoichiometry Problems Involving Gas Volumes -- 5.5. Gas Mixtures -- 5.6. Kinetic Theory of an Ideal Gas -- 5.7. Molecular Speeds -- 5.8. Real Gases -- 6. Thermochemistry -- 6.1. Energy and Its Units -- 6.2. Heat of Reaction -- 6.3. Enthalpy and Enthalpy Change -- 6.4. Thermochemical Equations -- 6.5. Applying Stoichiometry to Heats of Reaction -- 6.6. Measuring Heats of Reaction -- 6.7. Hess's Law -- 6.8. Standard Enthalpies of Formation -- 6.9. Fuels -- Foods, Commercial Fuels, and Rocket Fuels -- II. Atomic and Molecular Structure -- 7. Quantum Theory of the Atom -- 7.1. The Wave Nature of Light -- 7.2. Quantum Effects and Photons -- 7.3. The Bohr Theory of the Hydrogen Atom -- 7.4. Quantum Mechanics -- 7.5. Quantum Numbers and Atomic Orbitals -- 8. Electron Configurations and Periodicity -- 8.1. Electron Spin and the Pauli Exclusion Principle -- 8.2. Building-Up Principle and the Periodic Table -- 8.3. Writing Electron Configurations Using the Periodic Table -- 8.4. Orbital Diagrams of Atoms -- 8.5. Mendeleev's Predictions from the Periodic Table -- 8.6. Some Periodic Properties -- 8.7. Periodicity in the Main-Group Elements -- 9. Ionic and Covalent Bonding -- 9.1. Describing Ionic Bonds -- 9.2. Electron Configurations of Ions -- 9.3. Ionic Radii -- 9.4. Describing Covalent Bonds -- 9.5. Polar Covalent Bonds -- 9.6. Writing Lewis Electron-Dot Formulas -- 9.7. Delocalized Bonding: Resonance -- 9.8. Exceptions to the Octet Rule -- 9.9. Formal Charge and Lewis Formulas -- 9.10. Bond Length and Bond Order -- 9.11. Bond Energy -- 10. Molecular Geometry and Chemical Bonding Theory -- 10.1. The Valence-Shell Electron-Pair Repulsion (VSEPR) Model -- 10.2. Dipole Moment and Molecular Geometry -- 10.3. Valence Bond Theory -- 10.4. Description of Multiple Bonding -- 10.5. Principles of Molecular Orbital Theory -- 10.6. Electron Configurations of Diatomic Molecules of the Second-Period Elements -- 10.7. Molecular Orbitals and Delocalized Bonding -- III. States of Matter and Solutions -- 11. States of Matter -- 11.1. Comparison of Gases, Liquids, and Solids -- 11.2. Phase Transitions -- 11.3. Phase Diagrams -- 11.4. Properties of Liquids: Surface Tension and Viscosity -- 11.5. Intermolecular Forces -- 11.6. Classification of Solids by Type of Attraction of Units -- 11.7. Crystalline Solids -- 11.8. Structures of Some Crystalline Solids -- 11.9. Calculations Involving Unit-Cell Dimensions -- 11.10. Determining Crystal Structure by X-Ray Diffraction -- 12. Solutions -- 12.1. Types of Solutions -- 12.2. Solubility and the Solution Process -- 12.3. Effects of Temperature and Pressure on Solubility -- 12.4. Ways of Expressing Concentration -- 12.5. Vapor Pressure of a Solution -- 12.6. Boiling-Point Elevation and Freezing-Point Depression -- 12.7. Osmosis -- 12.8. Colligative Properties of Ionic Solutions -- 12.9. Colloids -- IV. Chemical Reactions and Equilibrium -- 13. Rates of Reaction -- 13.1. Definition of Reaction Rate -- 13.2. Experimental Determination of Rate -- 13.3. Dependence of Rate on Concentration -- 13.4. Change of Concentration with Time -- 13.5. Temperature and Rate -- 13.6. Arrhenius Equation -- 13.7. Elementary Reactions -- 13.8. The Rate Law and the Mechanism -- 13.9. Catalysis -- 14. Chemical Equilibrium -- 14.1. Chemical Equilibrium -- A Dynamic Equilibrium -- 14.2. The Equilibrium Constant -- 14.3. Heterogeneous Equilibria -- 14.4. Qualitatively Interpreting the Equilibrium Constant -- 14.5. Predicting the Direction of Reaction -- 14.6. Calculating Equilibrium Concentrations -- 14.7. Removing Products or Adding Reactants -- 14.8. Changing the Pressure and Temperature -- 14.9. Effect of a Catalyst -- 15. Acids and Bases -- 15.1. Arrhenius Concept of Acids and Bases -- 15.2. Bronsted-Lowry Concept of Acids and Bases -- 15.3. Lewis Concept of Acids and Bases -- 15.4. Relative Strengths of Acids and Bases -- 15.5. Molecular Structure and Acid Strength -- 15.6. Self-Ionization of Water -- 15.7. Solutions of a Strong Acid or Base -- 15.8. The pH of a Solution -- 16. Acid-Base Equilibria -- 16.1. Acid-Ionization Equilibria -- 16.2. Polyprotic Acids -- 16.3. Base-Ionization Equilibria -- 16.4. Acid-Base Properties of Salt Solutions -- 16.5. Common-Ion Effect -- 16.6. Buffers -- 16.7. Acid-Base Titration Curves -- 17. Solubility and Complex-Ion Equilibria -- 17.1. The Solubility Product Constant -- 17.2. Solubility and the Common-Ion Effect -- 17.3. Precipitation Calculations -- 17.4. Effect of pH on Solubility -- 17.5. Complex-Ion Formation -- 17.6. Complex Ions and Solubility -- 17.7. Qualitative Analysis of Metal Ions -- 18. Thermodynamics and Equilibrium -- 18.1. First Law of Thermodynamics -- 18.2. Entropy and the Second Law of Thermodynamics -- 18.3. Standard Entropies and the Third Law of Thermodynamics -- 18.4. Free Energy and Spontaneity -- 18.5. Interpretation of Free Energy -- 18.6. Relating ?G to the Equilibrium Constant -- 18.7. Change of Free Energy with Temperature -- 19. Electrochemistry -- 19.1. Balancing Oxidation-Reduction Reactions in Acidic and Basic Solutions -- 19.2. Construction of Voltaic Cells -- 19.3. Notation for Voltaic Cells -- 19.4. Cell Potential -- 19.5. Standard Cell Potentials and Standard Electrode Potentials -- 19.6. Equilibrium Constants from Cell Potentials -- 19.7. Dependence of Cell Potential on Concentration -- 19.8. Some Commercial Voltaic Cells -- 19.9. Electrolysis of Molten Salts -- 19.10. Aqueous Electrolysis -- 19.11. Stoichiometry of Electrolysis -- V. Nuclear Chemistry and Chemistry of the Elements -- 20. Nuclear Chemistry -- 20.1. Radioactivity -- 20.2. Nuclear Bombardment Reactions -- 20.3. Radiations and Matter: Detection and Biological Effects -- 20.4. Rate of Radioactive Decay -- 20.5. Applications of Radioactive Isotopes -- 20.6. Mass-Energy Calculations -- 20.7. Nuclear Fission and Nuclear Fusion -- 21. Chemistry of the Main-Group Elements -- 21.1. General Observations About the Main-Group Elements -- 21.2. Metals: Characteristics and Production -- 21.3. Bonding in Metals -- 21.4. Group IVA: The Alkali Metals -- 21.5. Group IIA: The Alkaline Earth Metals -- 21.6. Group IIIA and Group IVA Metals -- 21.7. Hydrogen -- 21.8. Group IVA: The Carbon Family -- 21.9. Group VA: Nitrogen and the Phosphorous Family -- 21.10. Group VIA: Oxygen and the Sulfur Family -- 21.11. Group VIIA: The Halogens -- 21.12. Group VIIIA: The Noble Gases -- 22. The Transition Elements and Coordination Compounds -- 22.1. Periodic Trends in the Transition Elements -- 22.2. The Chemistry of Two Transition Elements -- 22.3. Formation and Structure of Complexes -- 22.4. Naming Coordination Compounds -- 22.5. Structure and Isomerism in Coordination Compounds -- 22.6. Valence Bond Theory of Complexes -- 22.7. Crystal Field Theory -- 23. Organic Chemistry -- 23.1. The Bonding of Carbon -- 23.2. Alkanes and Cycloalkanes -- 23.3. Alkenes and Alkynes -- 23.4. Aromatic Hydrocarbons -- 23.5. Naming Hydrocarbons -- 23.6. Organic Compounds Containing Oxygen -- 23.7. Organic Compounds Containing Nitrogen -- 24. Polymer Materials: Synthetic and Biological -- 24.1. Synthesis of Organic Polymers -- 24.2. Electrically Conducting Polymers -- 24.3. Proteins -- 24.4. Nucleic Acids -- Appendix A. Mathematical Skills -- Appendix B. Vapor Pressure of Water at Various Temperatures -- Appendix C. Thermodynamic Quantities for Substances and Ions at 25 C -- Appendix D. Electron Configurations of Atoms in the Ground State -- Appendix E. Acid-Ionization Constants at 25 C -- Appendix F. Base-Ionization Constants at 25 C -- Appendix G. Solubility Product Constants at 25 C -- Appendix H. Formation Constants of Complex Ions at 25 C -- Appendix I. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25 C.

Summary: Helps students master quantitative skills and build a conceptual understanding of key chemical concepts

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Annexed index.

I. Basics of Chemistry --
1. Chemistry and Measurement --
1.1. Modern Chemistry: A Brief Glimpse --
1.2. Experiment and Explanation --
1.3. Law of Conservation of Mass --
1.4. Matter: Physical State and Chemical Constitution --
1.5. Measurement and Significant Figures --
1.6. SI Units --
1.7. Derived Units --
1.8. Units and Dimensional Analysis (Factor-Label Method) --
2. Atoms, Molecules, and Ions --
2.1. Atomic Theory of Matter --
2.2. The Structure of the Atom --
2.3. Nuclear Structure --
2.4. Atomic Masses --
2.5. Periodic Table of the Elements --
2.6. Chemical Formulas --
2.7. Organic Compounds --
2.8. Naming Simple Compounds --
2.9. Writing Chemical Equations --
2.10. Balancing Chemical Equations --
3. Calculations with Chemical Formulas and Equations --
3.1. Molecular Mass and Formula Mass --
3.2. The Mole Concept --
3.3. Mass Percentages from the Formula --
3.4. Elemental Analysis: Percentages of Carbon, Hydrogen, and Oxygen --
3.5. Determining Formulas --
3.6. Molar Interpretation of a Chemical Equation --
3.7. Amounts of Substances in a Chemical Reaction --
3.8. Limiting Reactant --
4. Chemical Reactions --
4.1. Ionic Theory of Solutions and Solubility Rules --
4.2. Molecular and Ionic Equations --
4.3. Precipitation Reactions --
4.4. Acid-Base Reactions --
4.5. Oxidation-Reduction Reactions --
4.6. Balancing Simple Oxidation-Reduction Equations --
4.7. Molar Concentration --
4.8. Diluting Solutions --
4.9. Gravimetric Analysis --
4.10. Volumetric Analysis --
5. The Gaseous State --
5.1. Gas Pressure and Its Measurement --
5.2. Empirical Gas Laws --
5.3. The Ideal Gas Law --
5.4. Stoichiometry Problems Involving Gas Volumes --
5.5. Gas Mixtures --
5.6. Kinetic Theory of an Ideal Gas --
5.7. Molecular Speeds --
5.8. Real Gases --
6. Thermochemistry --
6.1. Energy and Its Units --
6.2. Heat of Reaction --
6.3. Enthalpy and Enthalpy Change --
6.4. Thermochemical Equations --
6.5. Applying Stoichiometry to Heats of Reaction --
6.6. Measuring Heats of Reaction --
6.7. Hess's Law --
6.8. Standard Enthalpies of Formation --
6.9. Fuels --
Foods, Commercial Fuels, and Rocket Fuels --
II. Atomic and Molecular Structure --
7. Quantum Theory of the Atom --
7.1. The Wave Nature of Light --
7.2. Quantum Effects and Photons --
7.3. The Bohr Theory of the Hydrogen Atom --
7.4. Quantum Mechanics --
7.5. Quantum Numbers and Atomic Orbitals --
8. Electron Configurations and Periodicity --
8.1. Electron Spin and the Pauli Exclusion Principle --
8.2. Building-Up Principle and the Periodic Table --
8.3. Writing Electron Configurations Using the Periodic Table --
8.4. Orbital Diagrams of Atoms --
8.5. Mendeleev's Predictions from the Periodic Table --
8.6. Some Periodic Properties --
8.7. Periodicity in the Main-Group Elements --
9. Ionic and Covalent Bonding --
9.1. Describing Ionic Bonds --
9.2. Electron Configurations of Ions --
9.3. Ionic Radii --
9.4. Describing Covalent Bonds --
9.5. Polar Covalent Bonds --
9.6. Writing Lewis Electron-Dot Formulas --
9.7. Delocalized Bonding: Resonance --
9.8. Exceptions to the Octet Rule --
9.9. Formal Charge and Lewis Formulas --
9.10. Bond Length and Bond Order --
9.11. Bond Energy --
10. Molecular Geometry and Chemical Bonding Theory --
10.1. The Valence-Shell Electron-Pair Repulsion (VSEPR) Model --
10.2. Dipole Moment and Molecular Geometry --
10.3. Valence Bond Theory --
10.4. Description of Multiple Bonding --
10.5. Principles of Molecular Orbital Theory --
10.6. Electron Configurations of Diatomic Molecules of the Second-Period Elements --
10.7. Molecular Orbitals and Delocalized Bonding --
III. States of Matter and Solutions --
11. States of Matter --
11.1. Comparison of Gases, Liquids, and Solids --
11.2. Phase Transitions --
11.3. Phase Diagrams --
11.4. Properties of Liquids: Surface Tension and Viscosity --
11.5. Intermolecular Forces --
11.6. Classification of Solids by Type of Attraction of Units --
11.7. Crystalline Solids --
11.8. Structures of Some Crystalline Solids --
11.9. Calculations Involving Unit-Cell Dimensions --
11.10. Determining Crystal Structure by X-Ray Diffraction --
12. Solutions --
12.1. Types of Solutions --
12.2. Solubility and the Solution Process --
12.3. Effects of Temperature and Pressure on Solubility --
12.4. Ways of Expressing Concentration --
12.5. Vapor Pressure of a Solution --
12.6. Boiling-Point Elevation and Freezing-Point Depression --
12.7. Osmosis --
12.8. Colligative Properties of Ionic Solutions --
12.9. Colloids --
IV. Chemical Reactions and Equilibrium --
13. Rates of Reaction --
13.1. Definition of Reaction Rate --
13.2. Experimental Determination of Rate --
13.3. Dependence of Rate on Concentration --
13.4. Change of Concentration with Time --
13.5. Temperature and Rate --
13.6. Arrhenius Equation --
13.7. Elementary Reactions --
13.8. The Rate Law and the Mechanism --
13.9. Catalysis --
14. Chemical Equilibrium --
14.1. Chemical Equilibrium --
A Dynamic Equilibrium --
14.2. The Equilibrium Constant --
14.3. Heterogeneous Equilibria --
14.4. Qualitatively Interpreting the Equilibrium Constant --
14.5. Predicting the Direction of Reaction --
14.6. Calculating Equilibrium Concentrations --
14.7. Removing Products or Adding Reactants --
14.8. Changing the Pressure and Temperature --
14.9. Effect of a Catalyst --
15. Acids and Bases --
15.1. Arrhenius Concept of Acids and Bases --
15.2. Bronsted-Lowry Concept of Acids and Bases --
15.3. Lewis Concept of Acids and Bases --
15.4. Relative Strengths of Acids and Bases --
15.5. Molecular Structure and Acid Strength --
15.6. Self-Ionization of Water --
15.7. Solutions of a Strong Acid or Base --
15.8. The pH of a Solution --
16. Acid-Base Equilibria --
16.1. Acid-Ionization Equilibria --
16.2. Polyprotic Acids --
16.3. Base-Ionization Equilibria --
16.4. Acid-Base Properties of Salt Solutions --
16.5. Common-Ion Effect --
16.6. Buffers --
16.7. Acid-Base Titration Curves --
17. Solubility and Complex-Ion Equilibria --
17.1. The Solubility Product Constant --
17.2. Solubility and the Common-Ion Effect --
17.3. Precipitation Calculations --
17.4. Effect of pH on Solubility --
17.5. Complex-Ion Formation --
17.6. Complex Ions and Solubility --
17.7. Qualitative Analysis of Metal Ions --
18. Thermodynamics and Equilibrium --
18.1. First Law of Thermodynamics --
18.2. Entropy and the Second Law of Thermodynamics --
18.3. Standard Entropies and the Third Law of Thermodynamics --
18.4. Free Energy and Spontaneity --
18.5. Interpretation of Free Energy --
18.6. Relating ?G to the Equilibrium Constant --
18.7. Change of Free Energy with Temperature --
19. Electrochemistry --
19.1. Balancing Oxidation-Reduction Reactions in Acidic and Basic Solutions --
19.2. Construction of Voltaic Cells --
19.3. Notation for Voltaic Cells --
19.4. Cell Potential --
19.5. Standard Cell Potentials and Standard Electrode Potentials --
19.6. Equilibrium Constants from Cell Potentials --
19.7. Dependence of Cell Potential on Concentration --
19.8. Some Commercial Voltaic Cells --
19.9. Electrolysis of Molten Salts --
19.10. Aqueous Electrolysis --
19.11. Stoichiometry of Electrolysis --
V. Nuclear Chemistry and Chemistry of the Elements --
20. Nuclear Chemistry --
20.1. Radioactivity --
20.2. Nuclear Bombardment Reactions --
20.3. Radiations and Matter: Detection and Biological Effects --
20.4. Rate of Radioactive Decay --
20.5. Applications of Radioactive Isotopes --
20.6. Mass-Energy Calculations --
20.7. Nuclear Fission and Nuclear Fusion --
21. Chemistry of the Main-Group Elements --
21.1. General Observations About the Main-Group Elements --
21.2. Metals: Characteristics and Production --
21.3. Bonding in Metals --
21.4. Group IVA: The Alkali Metals --
21.5. Group IIA: The Alkaline Earth Metals --
21.6. Group IIIA and Group IVA Metals --
21.7. Hydrogen --
21.8. Group IVA: The Carbon Family --
21.9. Group VA: Nitrogen and the Phosphorous Family --
21.10. Group VIA: Oxygen and the Sulfur Family --
21.11. Group VIIA: The Halogens --
21.12. Group VIIIA: The Noble Gases --
22. The Transition Elements and Coordination Compounds --
22.1. Periodic Trends in the Transition Elements --
22.2. The Chemistry of Two Transition Elements --
22.3. Formation and Structure of Complexes --
22.4. Naming Coordination Compounds --
22.5. Structure and Isomerism in Coordination Compounds --
22.6. Valence Bond Theory of Complexes --
22.7. Crystal Field Theory --
23. Organic Chemistry --
23.1. The Bonding of Carbon --
23.2. Alkanes and Cycloalkanes --
23.3. Alkenes and Alkynes --
23.4. Aromatic Hydrocarbons --
23.5. Naming Hydrocarbons --
23.6. Organic Compounds Containing Oxygen --
23.7. Organic Compounds Containing Nitrogen --
24. Polymer Materials: Synthetic and Biological --
24.1. Synthesis of Organic Polymers --
24.2. Electrically Conducting Polymers --
24.3. Proteins --
24.4. Nucleic Acids --
Appendix A. Mathematical Skills --
Appendix B. Vapor Pressure of Water at Various Temperatures --
Appendix C. Thermodynamic Quantities for Substances and Ions at 25 C --
Appendix D. Electron Configurations of Atoms in the Ground State --
Appendix E. Acid-Ionization Constants at 25 C --
Appendix F. Base-Ionization Constants at 25 C --
Appendix G. Solubility Product Constants at 25 C --
Appendix H. Formation Constants of Complex Ions at 25 C --
Appendix I. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25 C.

Helps students master quantitative skills and build a conceptual understanding of key chemical concepts

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