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  • GenChem Textbook
    • Introduction: The Ambit of Chemistry
      • What Chemists Do
      • Handling Large and Small Numbers
      • The International System of Units (SI)
      • SI Prefixes
      • 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!
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Term of the Day

ionic radius
An estimate of the size of an ionAn atom or covalently bonded set of atoms that carries an overall net charge. in an ionic compoundA compound containing oppositely charged ions held together by electrostatic attraction. Usually the ions are in a crystal lattice with positive ions surrounded by negative ions and negative ions surrounded by positive ions.; found from the internuclear distanceThe distance between the nuclei of nearest-neighbor atoms or ions in an element or compound. Bond distances and ionic radii are calculated from this quantity because atoms have no discrete edges. between ions in a crystal latticeAn orderly, repeating arrangement of points in 3-D space in which each p;oint has surroundings identical to every other point. A crystal's constituent atoms, molecules, and ions are arranged about each lattice point..

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