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Xenon hexafluoroplatinate

Xenon hexafluoroplatinate
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 platinum hexafluoride and xenon in an experiment that proved the chemical reactivity of the noble gases. 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.



"Xenon hexafluoroplatinate" is prepared from Xe and platinum hexafluoride (PtF6) as gaseous solutions in SF6. The reactants were combined at 77K and slowly warmed, presumably to allow for a controlled reaction.


The structure of "xenon hexafluoroplatinate" is likely not Xe+[PtF6]. The main problem with this formulation is "Xe+", which would be a radical and would dimerize or abstract an F atom to give XeF+. Thus, Bartlett discovered that Xe undergoes chemical reactions, but the nature of his initial mustard yellow product is complex.[1] Further work indicates that Bartlett's product probably contained [XeF+][PtF6], [XeF+][Pt2F11], [Xe2F3+][PtF6].[2] The title "compound" is a salt, consisting of an octahedral anionic fluoride complex of platinum and various xenon cations.[3]

It has been proposed that the platinum fluoride forms a negatively charged polymeric network with xenon or xenon fluoride cations held in its instices. A preparation of "XePtF6" in 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]


Main article: Noble gas compound

In 1962, Neil Bartlett discovered that a mixture of platinum hexafluoride gas and oxygen formed a red solid.[4][5] The red solid turned out to be dioxygenyl hexafluoroplatinate, O2+[PtF6]-. Bartlett later surmized that the ionization energies for O2 molecule and Xe were similar. He then asked his colleagues to give him some xenon "so that he could try out some reactions",[citation needed] whereupon he established that xenon indeed reacts with PtF6. Although, as discussed above, the product was probably highly impure, Bartlett's discovery was the first proof that compounds could be prepared from a noble gas. His discovery illustrates that the discovery of new chemical methods often lead Initially to impure products. Since Bartlett's discovery, many well-defined compounds of xenon have been reported including XeF2, XeF4, and XeF6.


  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.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Xenon_hexafluoroplatinate". A list of authors is available in Wikipedia.
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