Originally Posted by MatthijsM
I'm looking for the theoretical explication why aromatics, so carbon carbon double bounds are able to absorbe UV light.
Some of this is fact and some information is from my Chem classes oh so long ago and thus is not to be completely trusted.
Fact: In order for a UV photon to be absorbed by a bonded electron we have to have a fairly large band gap for the transition.
Memory: Double carbon bonds are fairly weak. Thus we would likely have a large gap from it to any other bonding level. (I'm trying to check this.)