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    • Introduction: The Ambit of Chemistry
      • What Chemists Do
      • Handling Large and Small Numbers
      • The International System of Units (SI)
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      • Measurements, Quantities, and Unity Factors
      • Errors in Measurements
      • Volume
      • Density
      • Conversion Factors and Functions
    • Atoms, Molecules, and Chemical Reactions
      • Macroscopic Properties and Microscopic Models
      • The Atomic Theory
      • Macroscopic and Microscopic Views of a Chemical Reaction
      • Testing the Atomic Theory
      • Atomic Weights
      • The Amount of Substance: Moles
      • The Mole
      • The Amount of Substance
      • The Avogadro Constant
      • The Molar Mass
      • Formulas and Composition
      • Balancing Chemical Equations
    • Using Chemical Equations in Calculations
      • Equations and Mass Relationships
      • The Limiting Reagent
      • Percent Yield
      • Analysis of Compounds
      • Thermochemistry
      • Energy
      • Thermochemical Equations
      • Hess' Law
      • Standard Enthalpies of Formation
      • Solution Concentrations
      • Diluting and Mixing Solutions
      • Titrations
    • The Structure of Atoms
      • Groups of Related Elements
      • The Periodic Table
      • Valence
      • Exceptions to the Periodic Law
      • Implications of Periodicity for Atomic Theory
      • The Nuclear Atom
      • Radiation
      • The Electron
      • The Nucleus
      • Atomic Structure and Isotopes
      • Isotopes
      • Transmutation and Radioactivity
      • Average Atomic Weights
      • Measurement of Atomic Weights
    • The Electronic Structure of Atoms
      • Electrons and Valence
      • Lewis Diagrams
      • The Wave Nature of the Electron
      • Wave Mechanics
      • The Uncertainty Principle
      • Electron Waves in the Hydrogen Atom
      • Orbitals
      • Quantum Numbers
      • Coulomb's Law
      • Potential Energy
      • Electron Density and Potential Energy
      • Atoms Having More Than One Electron
      • Hydrogen, Helium, Lithium
      • Beryllium, Boron, Carbon
      • Electron Configurations
      • Electron Configurations and the Periodic Table
    • Chemical Bonding - Electron Pairs and Octets
      • Ionic Bonding
      • Energy and the Formation of Ions
      • The Ionic Crystal Lattice
      • Ions and Noble-Gas Electron Configurations
      • Periodic Variation of IE and EA
      • Ionization Energies
      • Ionization of Transition and Inner Transition Elements
      • Electron Affinities
      • Binary Ionic Compounds and Their Properties
      • The Octet Rule
      • Physical Properties
      • Chemical Properties
      • The Covalent Bond
      • Covalent Molecules and the Octet Rule
      • Writing Lewis Structures for Molecules
      • Polyatomic Ions
      • Ionic Compounds Containing Polyatomic Ions
      • Atomic Sizes
      • Ionic Sizes
    • Further Aspects of Covalent Bonding
      • Exceptions to the Octet Rule
      • The Shapes of Molecules
      • Molecules with Lone Pairs
      • Multiple Bonds and Molecular Shapes
      • Hybrid Orbitals
      • Orbital Descriptions of Multiple Bonds
      • Sigma and Pi Bonds
      • Polarizability
      • Polar Covalent Bonds
      • Electronegativity
      • Polarity in Polyatomic Molecules
      • Formal Charge and Oxidation Numbers
      • Resonance
    • Properties of Organic Compounds and Other Covalent Substances
      • Covalent Compounds and Intermolecular Forces
      • Dipole Forces
      • London Forces
      • Organic Compounds: Hydrocarbons
      • Alkanes
      • Cycloalkanes
      • Properties of Alkanes
      • Aromatic Hydrocarbons
      • Unsaturated Hydrocarbons
      • Hydrogen Bonding: Water
      • Ice and Water
      • Organic Compounds-Some Additional Classes
      • Alcohols
      • Ethers
      • Aldehydes and Ketones
      • Carboxylic Acids
      • Esters
      • Organic Nitrogen Compounds
      • Macromolecular Substances
      • Diamond and Graphite
      • Silicon Dioxide
      • Synthetic Macromolecules: Some Applied Organic Chemistry
      • Addition Polymers
      • Condensation Polymers
      • Cross-Linking
    • Gases
      • Properties of Gases
      • Pressure
      • Measurement of Pressure
      • Gas Laws
      • Avogadro's Law
      • Boyle's Law
      • Charles's Law
      • Gay-Lussac's Law
      • The Ideal Gas Equation
      • The Law of Combining Volumes
      • Dalton's Law of Partial Pressures
      • Postulates of the Kinetic Theory
      • The Total Molecular Kinetic Energy
      • Molecular Speeds
      • Graham's Law of Diffusion
      • The Distribution of Molecular Speeds
      • Deviations from the Ideal Gas Law
    • Solids, Liquids and Solutions
      • Solids
      • Lattices and Unit Cells
      • Crystal Systems
      • Closest-Packed Structures
      • Liquids
      • Viscosity
      • Amorphous Materials: Glasses
      • Phase Transitions
      • Enthalpy of Fusion and Enthalpy of Vaporization
      • Vapor-Liquid Equilibrium
      • Boiling Point
      • Critical Temperature and Pressure
      • Phase Diagrams
      • Solutions
      • Saturated and Supersaturated Solutions
      • Miscibility
      • Measuring the Composition of a Solution
      • Solubility and Molecular Structure
      • Raoult's Law
      • Chromatography
      • Colligative Properties of Solutions
      • Boiling and Freezing Points
      • Osmotic Pressure
      • Colloids
    • Reactions in Aqueous Solutions
      • Ions in Solution (Electrolytes)
      • Precipitation Reactions
      • Hydration of Ions
      • Hydrogen and Hydroxide Ions
      • Acid-Base Reactions
      • Acids
      • Bases
      • Strong Acids and Bases
      • Weak Acids
      • Weak Bases
      • Amphiprotic Species
      • Conjugate Acid-Base Pairs
      • Lewis Acids and Bases
      • Redox Reactions
      • Oxidation Numbers and Redox Reactions
      • Balancing Redox Equations
      • Common Oxidizing Agents
      • Common Reducing Agents
      • Substances Which Are Both Oxidizing and Reducing Agents
      • Redox Couples
    • Chemistry of the Representative Elements
      • Group IA: Alkali Metals
      • Group IIA: Alkaline Earths
      • Group IIIA
      • Group IVA
      • Group VA
      • Group VIA: Chalcogens
      • Group VIIA: Halogens
      • Group VIIIA: Noble Gases
    • Chemical Equilibrium
      • The Equilibrium State
      • The Equilibrium Constant
      • The Law of Chemical Equilibrium
      • The Equilibrium Constant in Terms of Pressure
      • Calculating the Extent of a Reaction
      • Successive Approximation
      • Predicting the Direction of a Reaction
      • The Effect of a Change in Pressure
      • The Effect of a Change in Temperature
      • Effect of Adding a Reactant or Product
      • The Molecular View of Equilibrium
    • Ionic Equilibria in Aqueous Solutions
      • Ionization of Water
      • pH and pOH
      • The pH of Solutions of Weak Acids
      • The pH of Solutions of Weak Bases
      • Polyprotic Acids and Bases
      • Conjugate Acid-Base Pairs and pH
      • Buffer Solutions
      • Indicators
      • Titration Curves
      • The Solubility Product
      • The Common-Ion Effect
      • The Solubilities of Salts of Weak Acids
    • Thermodynamics: Atoms, Molecules and Energy
      • Heat Capacities
      • Heat Capacity and Microscopic Changes
      • Internal Energy
      • Thermodynamic Terms and Conventions
      • Enthalpy
      • Measuring the Enthalpy Change
      • State Functions
      • Standard Pressure
      • Bond Enthalpies
      • Bond Enthalpies and Exothermic or Endothermic Reactions
      • Fossil Fuels and the Energy Crisis
      • Photosynthesis
    • Entropy and Spontaneous Reactions
      • Spontaneous Processes and Molecular Probability
      • Atoms, Molecules, and Probability
      • Rates of Spontaneous Processes
      • Thermodynamic Probability W and Entropy
      • Getting Acquainted with Entropy
      • Standard Molar Entropies
      • Dependence of S on Molecular Structure
      • Some Trends In Entropy Values
      • Entropy Changes in Gaseous Reactions
      • Entropy, Randomness, and Disorder
      • Measuring the Entropy
      • Including the Surroundings
      • The Free Energy
      • Maximum Useful Work
      • Equilibrium Constants Revisited
    • Electrochemical Cells
      • Electrolysis
      • Electrolysis of Brine
      • Aluminum Production
      • Refining of Copper
      • Electroplating
      • Quantitative Aspects of Electrolysis
      • Galvanic Cells
      • Cell Notation and Conventions
      • Electromotive Force of Galvanic Cells
      • Storage Batteries
      • Fuel Cells
      • Galvanic Cells and Free Energy
      • Cells at Non-Standard Conditions
    • Chemical Kinetics
      • The Rate of Reaction
      • The Rate Equation
      • Microscopic View of Chemical Reactions
      • Unimolecular Processes
      • Bimolecular Processes
      • Termolecular Processes
      • Reaction Mechanisms
      • Increasing the Rate of a Reaction
      • The Effect of Temperature
      • Catalysis
      • Heterogeneous Catalysis
      • Enzymes
    • Nuclear Chemistry
      • Naturally Occurring Radioactivity
      • Radioactive Series
      • Artificially Induced Nuclear Reactions
      • Bombardment with Positive Ions
      • Neutron Bombardment
      • Further Modes of Decay
      • Nuclear Stability
      • The Rate of Radioactive Decay
      • Instruments for Radiation Detection
      • Units of Radiation Dose
      • Uses of Artificial Isotopes
      • Mass-Energy Relationships
      • Nuclear Fission
      • Nuclear Power Plants
      • Breeder Reactors
      • Nuclear Fusion
    • Molecules in Living Systems
      • The Elements of Life
      • The Building Blocks of Biochemistry
      • Fats and Lipids
      • Nonpolar Lipids
      • Polar Lipids
      • Carbohydrates
      • Simple Sugars
      • Disaccharides
      • Polysaccharides
      • Proteins
      • Polypeptide Chains
      • The Amino Acids
      • Primary Protein Structure
      • Secondary Protein Structure
      • Higher-Order Structure
      • Nucleic Acids
      • Nuceic Acid Structure
      • The Double Helix
      • Information Storage
      • DNA Replication
      • Transcription and Translation
    • Spectra and Structure of Atoms and Molecules
      • The Nature of Electromagnetic Radiation
      • Atomic Spectra and the Bohr Theory
      • Bohr Theory of the Atom
      • The Spectra of Molecules: Infrared
      • The Visible and Ultraviolet Spectra of Molecules: Molecular Orbitals
      • Molecular Orbitals
      • Delocalized Electrons
      • Conjugated Systems
    • Metals
      • Metallic Bonding
      • Metallurgy
      • Beneficiation
      • Reduction of Metals
      • Refining of Metals
      • Corrosion
      • Coordination Compounds
      • Geometry of Complexes
      • Chelating Agents
      • Transitional Metal Ions in Aqueous Solutions
  • Quick Resources
    • Glossary
    • Physical Constants
    • Atomic Radii and Ionic Radii
    • General Rules for Predicting Electron Configurations
    • Ground State Electron Configurations
    • Covalently Bonded Polyatomic Ions
    • Table of Electronegativities
    • Rules for Finding Oxidation Numbers
    • Postulates of the Kinetic Theory of Gases
    • Ionization Energies and Electron Affinities
    • Table of Some Standard Enthalpies of Formation at 25°C
    • Table of Molar Enthalpies of Fusion and Vaporization
    • Table of Standard Molar Entropies
    • Series of Oxidation Activity for Some Common Metals
    • Table of Solubility Products for Some Sparingly Soluble Salts at 25°C
    • Table of Some Standard Free Energies of Formation at 298.15 K (25°C)
    • Table of Standard Reduction Potentials
    • Table of Acid and Base Constants
  • Periodic Table Live!

Quick Resources

  • Atomic Radii and Ionic Radii
  • Postulates of the Kinetic Theory of Gases
  • Covalently Bonded Polyatomic Ions
  • General Rules for Predicting Electron Configurations
  • Ionization Energies and Electron Affinities
  • Rules for Finding Oxidation Numbers
  • Table of Electronegativities
  • Table of Molar Enthalpies of Fusion and Vaporization
  • Table of Some Standard Enthalpies of Formation at 25°C
  • Table of Standard Molar Entropies
  • Ground State Electron Configurations
  • Physical Constants
  • Series of Oxidation Activity for Some Common Metals
  • Table of Acid and Base Constants
  • Table of Solubility Products for Some Sparingly Soluble Salts at 25°C
  • Table of Some Standard Free Energies of Formation at 298.15 K (25°C)
  • Table of Standard Reduction Potentials

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Quick Resources

Submitted by ChemPRIME Staff on Thu, 12/09/2010 - 13:58

Here are some Resources (typically found in your appendix).

  • Atomic Radii and Ionic Radii
  • Postulates of the Kinetic Theory of Gases
  • Covalently Bonded Polyatomic Ions
  • General Rules for Predicting Electron Configurations
  • Ionization Energies and Electron Affinities
  • Rules for Finding Oxidation Numbers
  • Table of Electronegativities
  • Table of Molar Enthalpies of Fusion and Vaporization
  • Table of Some Standard Enthalpies of Formation at 25°C
  • Table of Standard Molar Entropies
  • Ground State Electron Configurations
  • Physical Constants
  • Series of Oxidation Activity for Some Common Metals
  • Table of Acid and Base Constants
  • Table of Solubility Products for Some Sparingly Soluble Salts at 25°C
  • Table of Some Standard Free Energies of Formation at 298.15 K (25°C)
  • Table of Standard Reduction Potentials
Atomic Radii and Ionic Radii ›
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Term of the Day

degree of ionization
The extent to which a species in solutionA mixture of one or more substances dissolved in a solvent to give a homogeneous mixture. ionizes. Often applied to the ionizationA process in which an atom, molecule, or negative ion loses an electron; a process in which a covalent molecule reacts with a solvent to form positive and negative ions; for example, a weak acid reacting with water to form its conjugate base (an anion) and a hydrogen (hydronium) ion. reactions of acids and bases.

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