Lattice Enthalpy

HideShow resource information
  • Created by: annam29
  • Created on: 21-03-15 20:34

DEFINITIONS

STANDARD ENTHALPY OF FORMATION 

Enthalpy change when one mole of a compound is formed from its elements in their standard state, under standard conditions. 

STANDARD ENTHAPLY OF COMBUSTION 

Enthalpy change when one mole of an element or compound in its standard state, reacts completely with oxygen under standard conditions. 

HESS'S LAW 

The enthalpy change of a reaction is independent of the path taken provided the initial and final conditions remain the same.

STANDARD BOND DISSOCIATION ENTHALPY 

Energy change when one mole of covalent bond is broken in the gaseous state. 

FIRST IONISATION ENERGY 

Energy required to convert one mole of gaseous atoms into gaseous ions with a single positive charge. 

FIRST ELECTRON AFFINITY 

Energy change when one mole of gaseous atoms is converted into gaseous ions with a single negative charge. 

THE STANDARD ENTHALPY OF ATOMISATION

The heat change that accompanies the production of one mole of gaseous atoms from the element in its standard state. 

THE STANDARD LATTICE ENTHALPY 

The energy required to split up one mole of a solid crystal lattice into its gaseous ions. 

THE STANDARD ENTHALPY OF HYDRATION 

The heat change per mole for the hydration of the gaseous ion with enough water for there to be no further heat change on dilution. 

THE STANDARD ENTHALPY OF SOLUTION 

The enthalpy change when one mole of solute is dissolved in a solvent, forming an infinitely dilute solution. 

ENTROPY 

The amount of disorder or randomness within a chemical system. 

1 of 1

Comments

No comments have yet been made

Similar Chemistry resources:

See all Chemistry resources »See all Enthalpy resources »