| What is lattice enthalpy | the formation of one mole of an ionic compound from its gaseous ion under standard conditions |
| The standard enthalpy of atomisation | formation of one mole of gaseous atoms from the element in its standard states under standard conditions. |
| standard enthalpy of formation | when one mole of a compound is formed from its consituent elements in standard states under standard conditions |
| first ionisation energy | removal of one electron from one mole of gaseous atoms to form one mole of gaseous plus ions |
| enthalpy change of solution | one mole of a compound is dissolved in water under standard conditions |
| q= | mc delta T |
| BREAKING UP a lattice = | endothermic |
| formation of lattice = | exothermic |
| the standard enthalpy change of hydration | one mole of gaseous ions is dissolved in water forming mole of aqueous ions under standard c |
| factors affecting hydration | ionic size -ionic radius increases attraction between ions and water decreases hydration enegry is more possitive
ionic charge - ionic charge increases attraction with water mols increase so hydration energy is more negative |
| how to recognise lattice enthalpy by state symbols | gaseous to solid |
| The first electron affinity | the addition of one electron to each atom in one mol of gaseous atoms to form 1- |
| What are key features of lattice enthalpy | -exothermic change
indicates strength of ionic lattice bond strength |
| formation of lattice is exo or endo | exo |
| breaking of lattice | endothermic |
| second ionisation energy | the removal one of one elctron form each ion in mole of gaseous 1+ ions to form mole of gaseous 2+ ions |
| Working out enthalpy change of solution | calculate energy change in solution by q=mcdeltaT
calculate the moles
work out delta of solution by q/ moles |
