Entropy Definitions Flashcards
First Ionisation Energy
The energy required to remove 1 electron from every atom in 1 mole of gaseous atoms to form gaseous 1+ ions.
Standard Enthalpy of Formation
The enthalpy change when 1 mole of a substance is formed from its elements in their standard states.
Standard Enthalpy of Combustion
The enthalpy change when 1 mole of a substance is completely burned in oxygen under standard conditions.
Enthalpy Change
The heat energy change under constant pressure.
Hess’ Law
Enthalpy change is independent of the route taken.
Second Ionisation Energy
Enthalpy change when 1 electron is removed for each uni positive ion in 1 mole of gaseous ions to form doubly charged ions.
Enthalpy of Atomisation of an Element
Enthalpy change when 1 mole of free gaseous atoms is produced from that element in its standard state.
Enthalpy of Atomisation of a Compound
Enthalpy change when 1 mole of free gaseous atoms is produced from a compound in its standard state.
First Electron Affinity
Enthalpy change when 1 electron is added to each free gaseous atom in 1 mole of that element.
Second Electron Affinity
Enthalpy change when 1 electron is added to each free gaseous uni negative ion in 1 mole of that element.
Bond Dissociation Energy
Mean Enthalpy change when 1 mole of covalent bonds is broken homolytically resulting in free gaseous atoms.
Lattice Dissociation Enthalpy
Enthalpy change when 1 mole of an ionic compound is completely dissociated into free gaseous ions.
Lattice Association Energy
Enthalpy change when 1 mole of a solid ionic compound is formed from its ions in the gaseous state under standard conditions.
Enthalpy of Hydration
Enthalpy change when 1 mole of free gaseous ions is added to an excess of water.
Enthalpy of Solution
Enthalpy change when 1 mole of an ionic compound is completely dissolved in an excess of water.
