Xenon hexafluoroplatinate



Xenon hexafluoroplatinate
Properties
Molecular formula PtF6Xe
Molar mass 440.3604 g/mol
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references
Xenon hexafluoroplatinate is the description of the product obtained from the combination of Neil Bartlett at the University of British Columbia formulated the product as "Xe+[PtF6]−", although subsequent work suggests that Bartlett's product was probably a mixture and did not in fact contain this specific salt.

Preparation

"Xenon hexafluoroplatinate" is prepared from Xe and K and slowly warmed, presumably to allow for a controlled reaction.

Structure

The structure of "xenon hexafluoroplatinate" is likely not Xe+[PtF6]−. The main problem with this formulation is "Xe+", which would be a platinum and various xenon cations.[3]

It has been proposed that the platinum fluoride forms a negatively charged HF solution results in a solid which has been characterized as a [PtF5-]n polymeric network associated with XeF+. This result is evidence for such a polymeric structure of xenon hexafluoroplatinate.[1]

History

Main article: Noble gas compound

In 1962, XeF4, and XeF6.

References

  1. ^ a b Graham, L.; Graudejus, O., Jha N.K., and Bartlett, N. (2000). "Concerning the nature of XePtF6". Coordination Chemistry Reviews 197: 321–334. doi:10.1016/S0010-8545(99)00190-3.
  2. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  3. ^ The American Chemical Society "molecule of the week" (2006)."Xenon Hexafluoroplatinate"
  4. ^ Bartlett, N. (June 1962). "Xenon hexafluoroplatinate (V) Xe+[PtF6]−". Proceedings of the Chemical Society (6): 218. London: Chemical Society. doi:10.1039/PS9620000197.
  5. ^ Neil Bartlett and D. H. Lohmann (March 1962). "Dioxygenyl hexafluoroplatinate (V), O2+[PtF6]−". Proceedings of the Chemical Society (3): 115. London: Chemical Society. doi:10.1039/PS9620000097.
 
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