Radon fluoride

Krypton difluoride cannot be synthesized by the standard high pressure-high temperature means used to prepare xenon fluorides because of the low thermal stabitity of KrF. There are three low temperature methods which have proven practical for the preparation of gram and greater amounts of KrF (141—143). Radon fluoride is most conveniently prepared by reaction of radon gas with a tiquid halogen fluoride (CIE, CIE, CIE, BrE, or lE ) at room temperature (144,145). 

Fields, P. R., Stein, L., and Zirin, M. H., Radon Fluoride Further Tracer Experiments with Radon, in Noble-Gas Compounds (H. H. Hyman, ed), pp. 113-119, University of Chicago Press, Chicago, IL (1963). 

Stein, L., Hydrolytic Reactions of Radon Fluorides, Inorg. Chem. 23 3670 (1984). 

Because radon is inert and radioactive, there are not many useful compounds. The only one confirmed so far is radon fluoride (RnF). 

Chemists are trying to make compounds of radon, but the task is difficult. One compound that has been made is radon fluoride. In any event, such compounds are laboratory curiosities and have no commercial uses. 

The early characterization of a low-volatility radon-fluorine compound by combination of radon with fluorine at 400 °C 68 l01) was followed by work which showed that 222Rn is oxidized by chlorine and bromine fluorides, IF7102 105> or [NiF6]2- 103 -105> in HF to give stable solutions of radon fluoride. On the basis of electromigration studies it has been suggested that the radon in these solutions is present as [RnF]+ or [Rn]2+ 104-105), but [Rn2F3]+ also seems a likely possibility. The application of relativistic quantum mechanics to radon fluoride structures also shows that ionic formulations are favoured 106>. 

A radon fluoride of unknown composition is found to form readily, but it decomposes rapidly during attempts to vaporize it for further study. 

The only confirmed compound of radon is radon fluoride, RnF. One reason that it is difficult to study the chemistry of radon is that all isotopes of radon are radioactive so it is dangerous to handle the substance. Can you suggest another reason why there are so few known radon compounds Hint Radioactive decays are exothermic processes.)... 

Reimann C, Hall GEM, Siewers U, Bjorvatn K, Moriand K, Skarphagen H and Strand T (1996) Radon, fluoride and 62 dements as determined by ICP-MS in 145 Norwegian hard rock Groundwater samples. Sci Total Environ 192 ... 

Radon fluoride is most conveniently prepared by reaction of radon gas with a liquid halogen fluoride (CIP, CIF3, CIF5, BrPs, or IF7) at room temperature. Millicurie or larger amounts of radon react spontaneously with gaseous or liquid fluorine in a small volume (25 or 50 mL flask) within about 30 min. The radon behaves as both activator and reactant. The product is nonvolatile and hence remains in the reaction vessel when the excess reagent is removed by vacuum distillation. 

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