Xenon hexafluoroplatinate
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| Names | |
|---|---|
| Other names
Xenon(I) hexafluoroplatinate
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| Identifiers | |
3D model (JSmol)
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| Properties | |
| Xe+[PtF6]− | |
| Molar mass | 440.367 |
| Appearance | orange solid |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Xenon hexafluoroplatinate is the product of the reaction of platinum hexafluoride with xenon, in an experiment that proved the chemical reactivity of the noble gases. This experiment was performed by Neil Bartlett at the University of British Columbia, who formulated the product as "Xe+[PtF6]−", although subsequent work suggests that Bartlett's product was probably a salt mixture and did not in fact contain this specific salt.[1]
Preparation
[edit]"Xenon hexafluoroplatinate" is prepared from xenon and platinum hexafluoride (PtF6) as gaseous solutions in SF6. The reactants are combined at 77 K and slowly warmed to allow for a controlled reaction.
Structure
[edit]The material described originally as "xenon hexafluoroplatinate" is probably not Xe+[PtF6]−. The main problem with this formulation is "Xe+", which would be a radical and would dimerize or abstract a fluorine atom to give XeF+. Thus, Bartlett discovered that Xe undergoes chemical reactions, but the nature and purity of his initial mustard yellow product remains uncertain.[2] Further work indicates that Bartlett's product probably also contained products of further oxidation by PtF6, platinum(V) derivatives PtF5, [XeF]+[PtF5]−, and [XeF]+[Pt2F11]−.[2][3] The title "compound" is a salt, consisting of an octahedral anionic fluoride complex of platinum and various xenon cations.[4]
It has been proposed that the platinum fluoride forms a negatively charged polymeric anion with xenon fluoride cations. A preparation of "XePtF6" by reaction of XeF2 and PtF4 in anhydrous HF solution results in a solid which has been characterized as a [PtF
5]−
polymeric or oligomeric anion associated with XeF+. Such F-bridged polymeric chains and tetrameric ring with pendant XeF+ units have been observed in the crystal structures of the analogous compounds XeCrF6 (XeF2∙CrF4)[5] and XeMnF6 (XeF2∙MnF4),[6] respectively. These structures could serve as structural models for XePtF6.
History
[edit]In 1962, Neil Bartlett discovered that a mixture of platinum hexafluoride gas and oxygen formed a red solid.[7][8] The red solid turned out to be dioxygenyl hexafluoroplatinate, O+
2[PtF6]−. Bartlett noticed that the ionization energy for O2 (1175 kJ mol−1) was very close to the ionization energy for Xe (1170 kJ mol−1). He then asked his colleagues to give him some xenon "so that he could try out some reactions",[9][10] whereupon he established that xenon indeed reacts with PtF6. Although, as discussed above, the product was probably a mixture of several compounds, Bartlett's work was the first proof that compounds could be prepared from a noble gas. Since Bartlett's observation, many well-defined compounds of xenon have been reported including XeF2, XeF4, and XeF6.[3]
See also
[edit]References
[edit]- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth–Heinemann. ISBN 0080379419.
- ^ a b Graham, Lionell; Graudejus, Oliver; Jha, Narendra K.; Bartlett, Neil (2000). "Concerning the nature of XePtF6". Coordination Chemistry Reviews. 197 (1): 321–334. doi:10.1016/S0010-8545(99)00190-3.
- ^ a b Holleman, Arnold Frederick; Wiberg, Egon (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 0-12-352651-5.
- ^ Sampson, Mark T. (May 23, 2006). Neil Bartlett and the Reactive Noble Gases (PDF). National Historic Chemical Landmarks. American Chemical Society. Archived (PDF) from the original on April 18, 2016. Retrieved June 12, 2017.
- ^ Lutar, K.; Leban, I.; Ogrin, T.; Žemva, B. "XeF2·CrF4 and (XeF5+CrF5–)4·XeF4: Syntheses, Crystal Structures and Some Properties". European Journal of Solid State and Inorganic Chemistry. 29 (4–5): 713–727.
- ^ Motaln, Klemen; Gurung, Kshitij; Brázda, Petr; Kokalj, Anton; Radan, Kristian; Dragomir, Mirela; Žemva, Boris; Palatinus, Lukáš; Lozinšek, Matic (2024-09-25). "Reactive Noble-Gas Compounds Explored by 3D Electron Diffraction: XeF2–MnF4 Adducts and a Facile Sample Handling Procedure". ACS Central Science. 10 (9): 1733–1741. doi:10.1021/acscentsci.4c00815. ISSN 2374-7943. PMC 11428288. PMID 39345812.
- ^ Bartlett, Neil (1962). "Xenon hexafluoroplatinate(V) Xe+[PtF6]−". Proceedings of the Chemical Society. 1962 (6): 197–236. doi:10.1039/PS9620000197.
- ^ Bartlett, Neil; Lohmann, D. H. (1962). "Dioxygenyl hexafluoroplatinate(V), O+
2[PtF6]−". Proceedings of the Chemical Society. 1962 (3): 97–132. doi:10.1039/PS9620000097. - ^ Clugston, Michael; Flemming, Rosalind (2000). Advanced Chemistry. Oxford University Press. p. 355. ISBN 978-0199146338.
- ^ Hargittai, István (2009). "Neil Bartlett and the first noble-gas compound". Structural Chemistry. 20 (6): 953–959. doi:10.1007/s11224-009-9526-9. ISSN 1040-0400.