Originally Posted by Astronut
Another closed mind, unwilling to accept independent evidence, color me surprised. Here's where you're probably going wrong, alexander.
You seem to think the equivalent of delta H is the bond energy, and since UV light is > delta H on this graph, titanium will disintegrate. The true binding energy is given by E sub A. You need at least that much energy, a much higher value than UV light can provide, to disintegrate titanium. You will end up spending a net amount of energy equal to a much lower value, delta H, because when the bond breaks it will release most of the energy back.
Or you could have just accepted the mountains of independent video and photographic evidence of ISS that shows you're doing something wrong in your observations.
I'm not sure what your delta H is a reference to Astronut but it could be the energy absorbed when a bond is formed. Some reactions are endothermic. But this has nothing to do with the matter at hand.
As for what bond energy actually is, take the following quote from Wikipedia:
"Another example: an O–H bond of a water molecule (H–O–H) has 493.4 kJ mol-1 of bond dissociation energy, and 424.4 kJ mol-1 is needed to cleave the remaining O–H bond. The bond energy of the O–H bonds in water is 458.9 kJ mol-1, which is the average of the values."