From: Michael M. Butler (butler@comp-lib.org)
Date: Fri Jul 06 2001 - 03:03:02 MDT
Stressed bonds are the usual suspects. XeF6 is relatively inert (aka "the most like Teflon"). XeO3, otoh, is highly
explosive. The trend seems relatively monotonic.
I'd be much more prone to worrying about fire or electrical sparks liberating the F. But the low end of that could
include some (possibly obscure) metabolic pathways...
Eugene Leitl wrote:
>
> On Thu, 5 Jul 2001, Spike Jones wrote:
>
> > No, that works fine Mike. I calculate the density of xenon
> > hexaflouride would be, lets see, 131 + 6*19 = 245, so if XeF6
> > is inert to tissues then we could pull the same gag with about
>
> "if XeF6 is inert to tissues". That's a rather large if. (You know,
> they're called noble gases for a reason). Why don't you do a little Google
> session, and pull up the chemical properties of xenon compounds,
> particularly halides?
>
> > 100 atmospheres instead of 190. Perhaps it would
> > also not have the anaesthetic effect of pure xenon?
>
> -- Eugen* Leitl leitl
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