Chemistry in quantitive language;fundamentals of general chemistry calculations
Chemical equations Chemical reactions Chemistry SCIENCE Problems and exercises
Oxford University Press
EISBN 9780199709816
1. Essential Mathematics; 1.1. Significant Figures; 1.2. Significant Figures and Mathematical Operations; 1.3. Scientific Notation and Exponents; 1.4. Logarithms; 1.5. Algebraic Equations; 1.6. Problems; 2. Systems of Measurement; 2.1. Measurements in Chemistry; 2.2. Measurement of Mass, Length, and Time; 2.3. Temperature; 2.4. Derived Units; 2.5. Density and Specific Gravity; 2.6. Dimensional Analysis and Conversion Factors; 2.7. Problems; 3. Atomic Structure and Isotopes; 3.1. Atomic Theory; 3.2. The Structure of the Atom; 3.3. Isotopes; 3.4. Relative Atomic Mass; 3.5. Problems.
10.5. The Quantum-Mechanical Description of the Hydrogen Atom10.6. Quantum Mechanics and Atomic Orbitals; 10.7. Electronic Configuration of Multielectron Atoms; 10.8. Problems; 11. Gas Laws; 11.1. Standard Temperature and Pressure; 11.2. Boyle's Law: Pressure vs. Volume; 11.3. Charles's Law: Temperature vs. Volume; 11.4. The Combined Gas Law; 11.5. Gay-Lussac's Law and Reactions Involving Gases; 11.6. Avogadro's Law; 11.7. The Ideal Gas Law; 11.8. Density and Molecular Mass of a Gas; 11.9. Molar Volume of an Ideal Gas; 11.10. Dalton's Law of Partial Pressures.
11.11. Partial Pressure and Mole Fraction11.12. Real Gases and Deviation from the Gas Laws; 11.13. Graham's Law of Diffusion; 11.14. Problems; 12. Liquids and Solids; 12.1. The Liquid State; 12.2. Polar Covalent Bonds and Dipole Moment; 12.3. Vapor Pressure and the Clausius-Clapeyron Equation; 12.4. The Solid State; 12.5. The Crystal System; 12.6. Calculations Involving Unit Cell Dimensions; 12.7. Ionic Crystal Structure; 12.8. Radius Ratio Rule for Ionic Compounds; 12.9. Determination of Crystal Structure by X-ray Diffraction; 12.10. Problems; 13. Solution Chemistry.
4. Formula and Molecular Mass4.1. Formula Mass; 4.2. Molecular Mass; 4.3. Molar Mass; 4.4. Problems; 5. Measuring Chemical Quantities: the Mole; 5.1. The Mole and Avogadro's Number; 5.2. The Mole and Molar Mass; 5.3. Calculating the Number of Moles; 5.4. Problems; 6. Formulas of Compounds and Percent Composition; 6.1. Percent Composition; 6.2. Empirical Formula; 6.3. Molecular Formula; 6.4. Problems; 7. Chemical Formulas and Nomenclature; 7.1. General Background; 7.2. Chemical Formula; 7.3. Oxidation Numbers; 7.4. Writing the Formulas of Compounds; 7.5. Nomenclature of Inorganic Compounds.
7.6. Problems8. Chemical Equations; 8.1. Writing Chemical Equations; 8.2. Balancing Chemical Equations; 8.3. Types of Chemical Reactions; 8.4. Problems; 9. Stoichiometry; 9.1. Reaction Stoichiometry; 9.2. Information from a Balanced Equation; 9.3. Types of Stoichiometric Problems; 9.4. Limiting Reagents; 9.5. Reaction Yields: Theoretical, Actual, and Percent Yields; 9.6. Problems; 10. Structure of the Atom; 10.1. Electronic Structure of the Atom; 10.2. Electromagnetic Radiation; 10.3. The Nature of Matter and Quantum Theory; 10.4. The Hydrogen Atom.
A concise summary of important concepts in chemistry along with a detailed guide to understanding every type of calculation likely to arise in a general chemistry course.
10.5. The Quantum-Mechanical Description of the Hydrogen Atom10.6. Quantum Mechanics and Atomic Orbitals; 10.7. Electronic Configuration of Multielectron Atoms; 10.8. Problems; 11. Gas Laws; 11.1. Standard Temperature and Pressure; 11.2. Boyle's Law: Pressure vs. Volume; 11.3. Charles's Law: Temperature vs. Volume; 11.4. The Combined Gas Law; 11.5. Gay-Lussac's Law and Reactions Involving Gases; 11.6. Avogadro's Law; 11.7. The Ideal Gas Law; 11.8. Density and Molecular Mass of a Gas; 11.9. Molar Volume of an Ideal Gas; 11.10. Dalton's Law of Partial Pressures.
11.11. Partial Pressure and Mole Fraction11.12. Real Gases and Deviation from the Gas Laws; 11.13. Graham's Law of Diffusion; 11.14. Problems; 12. Liquids and Solids; 12.1. The Liquid State; 12.2. Polar Covalent Bonds and Dipole Moment; 12.3. Vapor Pressure and the Clausius-Clapeyron Equation; 12.4. The Solid State; 12.5. The Crystal System; 12.6. Calculations Involving Unit Cell Dimensions; 12.7. Ionic Crystal Structure; 12.8. Radius Ratio Rule for Ionic Compounds; 12.9. Determination of Crystal Structure by X-ray Diffraction; 12.10. Problems; 13. Solution Chemistry.
4. Formula and Molecular Mass4.1. Formula Mass; 4.2. Molecular Mass; 4.3. Molar Mass; 4.4. Problems; 5. Measuring Chemical Quantities: the Mole; 5.1. The Mole and Avogadro's Number; 5.2. The Mole and Molar Mass; 5.3. Calculating the Number of Moles; 5.4. Problems; 6. Formulas of Compounds and Percent Composition; 6.1. Percent Composition; 6.2. Empirical Formula; 6.3. Molecular Formula; 6.4. Problems; 7. Chemical Formulas and Nomenclature; 7.1. General Background; 7.2. Chemical Formula; 7.3. Oxidation Numbers; 7.4. Writing the Formulas of Compounds; 7.5. Nomenclature of Inorganic Compounds.
7.6. Problems8. Chemical Equations; 8.1. Writing Chemical Equations; 8.2. Balancing Chemical Equations; 8.3. Types of Chemical Reactions; 8.4. Problems; 9. Stoichiometry; 9.1. Reaction Stoichiometry; 9.2. Information from a Balanced Equation; 9.3. Types of Stoichiometric Problems; 9.4. Limiting Reagents; 9.5. Reaction Yields: Theoretical, Actual, and Percent Yields; 9.6. Problems; 10. Structure of the Atom; 10.1. Electronic Structure of the Atom; 10.2. Electromagnetic Radiation; 10.3. The Nature of Matter and Quantum Theory; 10.4. The Hydrogen Atom.
A concise summary of important concepts in chemistry along with a detailed guide to understanding every type of calculation likely to arise in a general chemistry course.
