"the atomization energy is the energy associated with the "
"formation of 1 mole of gaseous atoms from 1 mole of gaseous"
"element in its standard state under standard conditions......"
"and the bond dissociation energy is the energy associated with" "the CLEAVAGE of 1 mole of gaseous bonds from 1 mole of"
"gaseous molecules to form 2 gaseous radicals........."
So there are our definitions; let's see if we can represent each process by an equation, using a bimolecular species, X_2, as our exemplar:
"ATOMIZATION:"
1/2X_2(g) + "E"_1rarr dotX(g)
DeltaE_1="something"
"DISSOCIATION:"
X-X(g) + "E"_2rarr 2dotX(g)
DeltaE_2="some other thing"
So given the definition, if we have a homonuclear diatomic, i.e. dihydrogen, dihalogen, etc, then DeltaE_2=2xxDeltaE_1. That is the "energy of atomization" is HALF the "bond dissociation energy" for gaseous homonuclear diatomic molecules.
