F325 Energy Definitions

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  • Energy
    • Lattice Enthalpy
      • The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
      • Always exothermic, ionic bonds are being formed.
        • Cannot be measured directly, impossible to form one mole of an ionic lattice from it's gaseous ions.
    • Enthalpy Change of Formation
      • Enthalpy change when one mole of a compound is formed from it's constituent elements under standard conditions.
    • Enthalpy change of Atomisation
      • Enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state.
    • Enthalpy Change of Solution
      • The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions.
    • Enthalpy Change of Hydration
      • The enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water forming one mole of aqueous ions under standard conditions.
    • First Ionisation Energy
      • The enthalpy change accompanying the removal of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
    • Second Ionisation Energy
      • The enthalpy change accompanying the removal of one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions.
    • First Electron Affinity
      • The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions.
      • Second Electron Affinity
        • The enthalpy change accompanying the addition of one electron to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions.
    • Entropy
      • The quantitative measure of the degree of disorder in a system.
    • Free Energy Change
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