Enthalpy definitions

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lattice dissociation enthalpy

the energy to completely break apart an ionic lattice into it’s gaseous ions under standard conditions

lattice formation enthalpy

the energy to form an ionic lattice from its ions under standard conditions

enthalpy

the heat energy change of a reaction under constant pressure. Its units are kJmol-1

enthalpy change of formation

the enthalpy change when 1 mole of a compound is made from its elements in their standard states and under standard conditions

enthalpy of atomisation

enthalpy change when one mole of a element in its standard state is made into gaseous atoms under standard conditions

first ionisation energy

the enthalpy change when 1 mole of the most loosely held electrons are removed from 1 mole of gaseous atoms to form gaseous 1+ ions under standard conditions

second ionisation energy

the enthalpy change when 1 mole of the most loosely held electrons are removed from 1 mole of gaseous 1+ ions to form gaseous 2+ ions under standard conditions

first electron affinity

the enthalpy change when 1 mole of gaseous atoms gains an electron to form gaseous 1- ions under standard conditions

second electron affinity

the enthalpy change when 1 mole of gaseous 1- ions gain an electron to form gaseous 2- ions under standard conditons

enthalpy of hydration

enthalpy change when 1 mole of gaseous ions are dissolved in water to form 1 mole of aqueous ions under standard conditions

enthalpy of solution

the enthalpy change when 1 mole of an ionic compound is dissolved into its ions to infinite dilution so that its ions no longer interact under standard conditions

bond dissociation enthalpy

the average enthalpy change when all bonds of one type in 1 mole of gaseous molecules are broken under standard conditions

atomisation of a compound enthalpy

the enthalpy change when 1 mole of a compound is converted into its gaseous atoms under standard conditions

entropy

measure of disorder within a compound