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CITATION

Rosenberg, Jerome; Epstein, Lawrence; and Krieger, Peter. Schaum's Outline of College Chemistry. US: McGraw-Hill, 2013.

Schaum's Outline of College Chemistry

Authors: Jerome Rosenberg, Lawrence Epstein and Peter Krieger

Published:  May 2013

ISBN: 9780071810838 0071810838 9780071810821
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  • Cover
  • Title Page
  • Copyright Page
  • Contents
  • Chapter 1 Quantities and Units
  • Introduction
  • Systems of measurement
  • International system (SI) of units
  • Temperature
  • Other temperature scales
  • Use and misuse of units
  • Factor-label method
  • Estimation of numerical answers
  • Chapter 2 Atomic and Molecular Mass; Molar Mass
  • Atoms
  • Nuclei
  • Relative atomic masses
  • Mole
  • Symbols, formulas, molar masses
  • Chapter 3 Formulas and Composition Calculations
  • Empirical formula from composition
  • Composition from formula
  • Nonstoichiometric factors
  • Nuclidic molecular masses and chemical formulas
  • Chapter 4 Calculations from Chemical Equations
  • Introduction
  • Molecular relations from equations
  • Mass relations from equations
  • Limiting reactant
  • Types of chemical reactions
  • Chapter 5 Measurement of Gases
  • Gas volumes
  • Pressure
  • Standard atmospheric pressure
  • Pressure measurement
  • Standard conditions
  • Gas laws
  • Boyle’s law
  • Charles’ law
  • Gay-Lussac’s law
  • Combined gas law
  • Density of an ideal gas
  • Dalton’s law of partial pressures
  • Collecting gases over a liquid
  • Deviations from ideal behavior
  • Chapter 6 The Ideal Gas Law and Kinetic Theory
  • Avogadro’s hypothesis
  • Molar volume
  • Ideal gas law
  • Gas volume relations from equations
  • Gas stoichiometry involving mass
  • Basic assumptions of the kinetic theory of gases
  • Predictions of the kinetic theory
  • Chapter 7 Thermochemistry
  • Heat
  • Heat capacity
  • Calorimetry
  • Energy and enthalpy
  • Enthalpy changes for various processes
  • Rules of thermochemistry
  • Comment on thermochemical reactions
  • Chapter 8 Atomic Structure and the Periodic Law
  • Absorption and emission of light
  • Interaction of light with matter
  • Particles and waves
  • The Pauli principle and the periodic law
  • Aufbau principle
  • Electron configurations
  • Atomic radii
  • Ionization energies
  • Electron affinity
  • Magnetic properties
  • Chapter 9 Chemical Bonding and Molecular Structure
  • Introduction
  • Ionic compounds
  • Covalence
  • Valence-bond representation
  • Molecular-orbital representation
  • π bonding and multicenter π bonds
  • Shapes of molecules
  • Coordination compounds
  • Isomerism
  • Bonding in metals
  • Chapter 10 Solids and Liquids
  • Introduction
  • Crystals
  • Crystal forces
  • Ionic radii
  • Forces in liquids
  • Chapter 11 Oxidation-Reduction
  • Oxidation-reduction reactions
  • Oxidation number
  • Oxidizing and reducing agents
  • Ionic notation for equations
  • Balancing oxidation-reduction equations
  • Chapter 12 Concentration of Solutions
  • Composition of solutions
  • Concentrations expressed in physical units
  • Concentrations expressed in chemical units
  • Comparison of the concentration scales
  • Summary of concentration units
  • Dilution problems
  • Chapter 13 Reactions Involving Standard Solutions
  • Advantages of volumetric standard solutions
  • Solution stoichiometry
  • Chapter 14 Properties of Solutions
  • Introduction
  • Vapor pressure lowering
  • Freezing-point lowering,ΔT[sub(f)]
  • Boiling-point elevation,ΔT[sub(b)]
  • Osmotic pressure
  • Deviations from the laws of dilute solutions
  • Solutions of gases in liquids
  • Law of distribution
  • Chapter 15 Organic Chemistry and Biochemistry
  • Introduction
  • Nomenclature
  • Isomerism
  • Functional groups
  • Properties and reactions
  • Biochemistry
  • Chapter 16 Thermodynamics and Chemical Equilibrium
  • The first law
  • The second law
  • The third law
  • Standard states and reference tables
  • Chemical equilibrium
  • The equilibrium constant
  • Le Chatelier’s principle
  • Chapter 17 Acids and Bases
  • Acids and bases
  • Ionization of water
  • Hydrolysis
  • Buffer solutions and indicators
  • Weak polyprotic acids
  • Titration
  • Chapter 18 Complex Ions; Precipitates
  • Coordination complexes
  • Solubility product
  • Applications of solubility product to precipitation
  • Chapter 19 Electrochemistry
  • Electrical units
  • Faraday’s laws of electrolysis
  • Voltaic cells
  • Standard half-cell potentials
  • Combinations of couples
  • Free energy, nonstandard potentials, and the direction of oxidation-reduction reactions
  • Chapter 20 Rates of Reactions
  • Rate constants and the order of reactions
  • Energy of activation
  • Mechanism of reactions
  • Chapter 21 Nuclear Processes
  • Fundamental particles
  • Binding energies
  • Nuclear equations
  • Radiochemistry
  • Appendix A: Exponents
  • Appendix B: Significant Figures
  • Index
  • Table of Atomic Masses
  • Nuclidic Masses of Selected Radionuclides