Xenon_tetrafluoride

Xenon tetrafluoride

Xenon tetrafluoride

Chemical compound

Xenon tetrafluoride is a chemical compound with chemical formula XeF
4. It was the first discovered binary compound of a noble gas.[3] It is produced by the chemical reaction of xenon with fluorine:[4][5]

Xe + 2 F
2 → XeF
4
Quick Facts Names, Identifiers ...

This reaction is exothermic, releasing an energy of 251 kJ/mol.[3]

Xenon tetrafluoride is a colorless crystalline solid that sublimes at 117 °C. Its structure was determined by both NMR spectroscopy and X-ray crystallography in 1963.[6][7] The structure is square planar, as has been confirmed by neutron diffraction studies.[8] According to VSEPR theory, in addition to four fluoride ligands, the xenon center has two lone pairs of electrons. These lone pairs are mutually trans.

Synthesis

Xenon tetrafluoride is produced by heating a mixture of xenon and fluorine in a 1:5 molar ratio in a nickel container to 400 °C. Some xenon difluoride (XeF
2) and xenon hexafluoride (XeF
6) is also produced, where increased temperature or decreased fluorine concentration in the input mixture favors XeF
2 production, and decreased temperature or increased fluorine concentration favors XeF
6.[9][10] The nickel is not a catalyst for this reaction; nickel containers are used because they react with fluorine to form a protective, non-peeling passivation layer of nickel(II) fluoride NiF
2 on their interior surfaces. The low volatility of XeF
4 compared to XeF
2 and XeF
6 allows it to be purified by fractional sublimation.[9]

Reactions

Xenon tetrafluoride hydrolyzes at low temperatures to form elemental xenon, oxygen, hydrofluoric acid, and aqueous xenon trioxide.[11]

It is used as a precursor for synthesis of all tetravalent Xe compounds.[9] Reaction with tetramethylammonium fluoride gives tetramethylammonium pentafluoroxenate, which contains the pentagonal XeF−
5 anion. The XeF−
5 anion is also formed by reaction with caesium fluoride:[12]

CsF + XeF
4 → CsXeF
5

Reaction with bismuth pentafluoride (BiF
5) forms the XeF+
3 cation:[13]

BiF
5 + XeF
4 → XeF3BiF6

The XeF+
3 cation in the salt XeF3Sb2F11 has been characterized by NMR spectroscopy.[14]

At 400 °C, XeF
4 reacts with xenon to form XeF
2:[10]

XeF4 + Xe → 2 XeF2

The reaction of xenon tetrafluoride with platinum yields platinum tetrafluoride and xenon:[10]

XeF4 + Pt → PtF4 + Xe

Applications

Xenon tetrafluoride has few applications. It has been shown to degrade silicone rubber for analyzing trace metal impurities in the rubber. XeF
4 reacts with the silicone to form simple gaseous products, leaving a residue of metal impurities.[15]

References

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    Claassen, H. H.; Selig, H.; Malm, J. G. (1962). "Xenon Tetrafluoride". J. Am. Chem. Soc. 84 (18): 3593. doi:10.1021/ja00877a042.
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    Williamson; Koch, C. W. (Mar 1963). "Xenon Tetrafluoride: Reaction with Aqueous Solutions". Science. 139 (3559): 1046–1047. Bibcode:1963Sci...139.1046W. doi:10.1126/science.139.3559.1046. ISSN 0036-8075. PMID 17812981. S2CID 33320384.
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    Gillespie, R. J.; Landa, B.; Schrobilgen, G. J. (1971). "Trifluoroxenon(IV) µ-fluoro-bispentafluoroantimonate(V): the XeF+
    3     cation". Journal of the Chemical Society D: Chemical Communications (23): 1543–1544. doi:10.1039/C29710001543.
  15. [15]
    Rigin, V.; Skvortsov, N. K.; Rigin, V. V. (March 1997). "Xenon tetrafluoride as a decomposition agent for silicone rubber for isolation and atomic emission spectrometric determination of trace metals". Analytica Chimica Acta. 340 (1–3): 1–3. Bibcode:1997AcAC..340....1R. doi:10.1016/S0003-2670(96)00563-6.
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