I just lost an explanation of more of how this works after 2 hrs of typing. I'm going hunting, will return with more group theory later.
Thanks for taking the time CZ, I'll watch for your update.
I don't know the chemistry behind it, but chances are the iron oxide that's formed to appear as colors is in a stable molecular form, -O3? How much light energy would have to be applied to make that molecule take up an oxygen atom and convert to -O4? I'm asking because you mentioned that light energy and the availability of oxygen were the cause of light degradation of case colors.
If the iron oxide isn't converted, but some crystalline structure that the iron oxide formed is disrupted, what is the O2 oxidizing, and how much energy does that take? I think I've seen it start at lower temps, but there's some mention by pro finishers, in Ken's links, to keep tempering temps at 400*, more will fade colors. Can ambient light add that much energy?
Just asking is all. I believe, subjectively, light does fade case colors, but by how much?
