| |
Energy Definitions |
It should be noted that many of
the energy definitions can be considered in the reverse direction
with a corresponding change of sign for the energy. Bond formation
= exothermic ΔH negative, bond cleavage = endothermic ΔH
positive |
|
|
|
| |
Enthalpy of vaporisation |
The energy required to vaporise one mole of a liquid |
| |
|
|
| |
Enthalpy of atomisation |
The energy required to produce one mole of gaseous atoms
from an element in its standard state |
| |
|
|
| |
Bond dissociation enthalpy |
The energy change when one mole of a specific bond in
a given molecule is broken or created |
| |
|
|
| |
Bond enthalpy |
The average energy change when one mole of a specific
type of bond is broken or created. |
| |
|
|
| |
Enthalpy of Combustion |
The energy released when one mole of a compound
is burned in excess oxygen |
| |
|
|
| |
Enthalpy of formation |
The energy change when one mole of a compound is formed
from its constituent elements in their standard states |
| |
|
|
| |
Enthalpy of solution |
The energy change when one mole of a substance is dissolved
in an infinite amount of water |
| |
|
|
| |
Hydration enthalpy |
The energy change when a particle is taken from infinite
separation in the gaseous state to its position in an aqueous lattice |
| |
|
|
| |
Ionisation energy |
The energy required to produce one mole of gaseous ions
from one mole of gaseous atoms by removal of one mole of electrons |
| |
|
|
| |
Lattice enthalpy |
The energy change when one mole of an ionic substance is broken
into its constituent atoms at infinite separation.
|
| |
|
|
