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Edited on Mon Aug-24-09 11:31 PM by NNadir
Oxygen difluoride holds a very special place in the history of chemistry in my view, owing to the fact that its existence stimulated the great chemist Neil Bartlett, at UC Berkeley, to develop the chemistry of the noble gases.
Recognizing that the ionization potential of oxygen and xenon were very close, Barlett surmised that xenon should have chemistry: Until that time it was thought that all of the noble gases, helium, neon, argon, krypton and xenon (and to be complete, radon) were unable to form chemical compounds. Bartlett recognized that if oxygen could form a cationic compound with fluorine, then it was very likely that xenon could do so well.
Bartlett then synthesized Xe+(PtF6-), the very first stable chemically bonded compound of a noble gas. Later many other noble gas compounds were identified, such as xenon hexafluoride, xenon difluoride, krypton difluoride (about which I'll say a little more below).
Maybe Bartlett's noble work deserved a Nobel, but for some reason, he didn't win it.
Xenon hexafluoride is an interesting and somewhat dangerous compound inasmuch as if it gets wet it is rapidly hydrolyzed to give HF and XeO3 (in equilibrium with "xenic acid," which is if it is allowed to dry, can and does spontaneously explode, leaving not a trace of its existence. (This is why xenon headlights should be banned, for their terrorist potential, but no, let's not go there.)
Anyway, about oxygen difluoride: I have always thought of it as a laboratory curiosity of no practical significance until now.
On another website where I read and write sometimes, I was recently discussing the fluorination of molten salts from the MSRE, the molten salt reactor experiment, where uranium was decontaminated from fission products in a matter of hours by distillation in a stream of fluorine gas.
I have always assumed that the plutonium was carried with the uranium, at least partially, but apparently according to those who have delved into the particular ORNL documents more than I have, this was not true.
The problem is that while PuF6 is stable in a stream of fluorine gas, it is only slowly formed from PuF4 by direct fluorination. This made a problem for the ORNL guys in removing the plutonium from their molten salt mixture.
Not to worry though. I checked back through my files and found a paper out of Los Alamos by Mills and Reese touching on this point, Journal of Alloys and Compounds, 213/214 (1994) 360-362 "Separation of plutonium and americium by low-temperature fluorination"
The fluorinating agent in this case is well, oxygen difluoride, which is made by direct reaction using a cryogenic trap, between fluorine and oxygen. When the oxygen fluoride gas is allowed to boil off on to plutonium tetrafluoride, the volatile plutonium hexafluoride gas.
This is considered an excellent way to remove plutonium from americium (and curium), since americium and curium both are more "lanthanide like" than plutonium, even if americium has a well defined +5 oxidation state. (Separations of curium and americium are more difficult, by the way.)
Thus in a modern pyroprocessing system, avoiding the limitations of solvent based extraction systems, which suffer limited stability in high radiation fields. (This is not true, by the way of so called "ionic liquids" in which it is possible to form plutonium electride salts in high radiation fields.) This sort of thing will become increasingly important should humanity seriously attempt to address climate change. Interestingly this chemistry should be very clean, resulting only in HF and plutonium oxide with no residual solvents. HF is easily neutralized with calcium carbonate to give insoluble CaF2, the mineral fluorite from which most fluorine is currently mined and carbon dioxide.
Another paper that touches on exotic compounds being used to make plutonium hexafluoride is work by Yu. V. Drobyshevskii, V. N. Prusakov and V. F. Serik out of the I. V. Kurchatov Institute of Atomic Energy, out of so called "classified abstracts." These scientists observed PuF4 in equilibrium with very low temperature KrF2 and found that there was a solid phase reaction at the interface between the two solids to give gaseous PuF6.
Esoteric I guess, but cool nonetheless.
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