Thermodynamics - Enthalpy definitions

Enthalpy Change of formation
Elements in standard states and standard conditions -> 1 mol of compound
1 of 12
Atomisation of an element
Element in standard state -> 1 mole of gaseous atoms (e.g. ½Cl2 (g)-> Cl (g)
2 of 12
First ionisation energy
1 mole of gaseous atoms -> 1 mol of gaseous 1+ ions
3 of 12
Second ionisation energy
1 mol of gaseious 1+ ions -> 1 mol of gaseous 2+ ions
4 of 12
First electron affinity
1 mol of gaseous atoms -> 1 mol of gaseous 1- ions
5 of 12
Enthalpy change of hydration
1 mol of gaseous ions -> 1 mol of aqueous ions.
6 of 12
Bond dissociation enthalpy
When all the bonds of the same type in 1 mol of gaseous molecules are broken
7 of 12
Atomisation of a compound
1 mol of a compound in its standard state is converted into gaseous atoms.
8 of 12
Second electron affinity
When 1 mol of gaseous 1- ions forms 1 mol of gaseous 2- ions
9 of 12
Enthalpy change of solution
When 1 mol of solute is dissolved in enough solvent so that no further enthalpy change happens when more solvent is added. E.g. NaCl (g) -> NaCl (aq)
10 of 12
Lattice enthalpy of formation
gaseous ions under standard condition--> 1 mol of a solid ionic compound
11 of 12
Lattice enthalpy of dissociation
1 mole of a solid ionic compound-> constituent gaseous ions under standard conditions
12 of 12

Other cards in this set

Card 2

Front

Element in standard state -> 1 mole of gaseous atoms (e.g. ½Cl2 (g)-> Cl (g)

Back

Atomisation of an element

Card 3

Front

1 mole of gaseous atoms -> 1 mol of gaseous 1+ ions

Back

Preview of the back of card 3

Card 4

Front

1 mol of gaseious 1+ ions -> 1 mol of gaseous 2+ ions

Back

Preview of the back of card 4

Card 5

Front

1 mol of gaseous atoms -> 1 mol of gaseous 1- ions

Back

Preview of the back of card 5
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