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Xenon tetrafluoride
Names
	IUPAC name Xenon tetrafluoride
Identifiers
CAS Number	13709-61-0 ;
3D model (JSmol)	Interactive image;
ChemSpider	109927 ;
ECHA InfoCard	100.033.858
PubChem CID	123324;
UNII	O825AI8P4W ;
CompTox Dashboard (EPA)	DTXSID50160062 ;
	InChI InChI=1S/F4Xe/c1-5(2,3)4 Key: RPSSQXXJRBEGEE-UHFFFAOYSA-N ; InChI=1/F4Xe/c1-5(2,3)4 Key: RPSSQXXJRBEGEE-UHFFFAOYAW;
	SMILES F[Xe](F)(F)F;
Properties
Chemical formula	XeF; 4
Molar mass	207.2836 g mol−1
Appearance	White solid
Density	4.040 g cm−3, solid
Melting point	117 °C (243 °F; 390 K) sublimes
Solubility in water	Reacts
Structure
Coordination geometry	D4h
Molecular shape	square planar
Dipole moment	0 D
Thermochemistry
Std molar; entropy (S⦵298)	146 J·mol−1·K−1
Std enthalpy of; formation (ΔfH⦵298)	−251 kJ·mol−1
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

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

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]

{\rm {\ 6XeF_{4}+12H_{2}O\rightarrow 2XeO_{3}+4Xe\uparrow +3O_{2}\uparrow +24HF}}

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 cesium 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

^ Holleman, Arnold F.; Wiberg, Egon (2001). Wiberg, Nils (ed.). Inorganic Chemistry. Translated by Eagleson, Mary; Brewer, William. Academic Press. p. 394. ISBN 0-12-352651-5.
^ ^a ^b Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
^ ^a ^b Zumdahl (2007). Chemistry. Boston: Houghton Mifflin. p. 243. ISBN 978-0-618-52844-8.
^ Claassen, H. H.; Selig, H.; Malm, J. G. (1962). "Xenon Tetrafluoride". J. Am. Chem. Soc. 84 (18): 3593. doi:10.1021/ja00877a042.
^ Chernick, C. L.; Claassen, H. H.; Fields, P. R.; Hyman, H. H.; Malm, J. G.; Manning, W. M.; Matheson, M. S.; Quarterman, L. A.; Schreiner, F.; Selig, H. H.; Sheft, I.; Siegel, S.; Sloth, E. N.; Stein, L.; Studier, M. H.; Weeks, J. L.; Zirin, M. H. (1962). "Fluorine Compounds of Xenon and Radon". Science. 138 (3537): 136–138. Bibcode:1962Sci...138..136C. doi:10.1126/science.138.3537.136. PMID 17818399. S2CID 10330125.
^ Brown, Thomas H.; Whipple, E. B.; Verdier, Peter H. (1963). "Xenon Tetrafluoride: Fluorine-19 High-Resolution Magnetic Resonance Spectrum". Science. 140 (3563): 178. Bibcode:1963Sci...140..178B. doi:10.1126/science.140.3563.178. PMID 17819836. S2CID 35981023.
^ Ibers, James A.; Hamilton, Walter C. (1963). "Xenon Tetrafluoride: Crystal Structure". Science. 139 (3550): 106–107. Bibcode:1963Sci...139..106I. doi:10.1126/science.139.3550.106. PMID 17798707. S2CID 42119788.
^ Burns, John H.; Agron, P. A.; Levy, Henri A (1963). "Xenon Tetrafluoride Molecule and Its Thermal Motion: A Neutron Diffraction Study". Science. 139 (3560): 1208–1209. Bibcode:1963Sci...139.1208B. doi:10.1126/science.139.3560.1208. PMID 17757912. S2CID 35858682.
^ ^a ^b ^c Haner, Jamie; Schrobilgen, Gary J. (2015). "The Chemistry of Xenon(IV)". Chem. Rev. 115 (2): 1255–1295. doi:10.1021/cr500427p. ISSN 0009-2665. PMID 25559700.
^ ^a ^b ^c Bard, Allen J.; Parsons, Roger; Jordan, Joseph; International Union of Pure and Applied Chemistry (1985). Standard Potentials in Aqueous Solution. CRC Press. pp. 767–768. ISBN 0-8247-7291-1.
^ 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.
^ Harding, Charlie; Johnson, David Arthur; Janes, Rob (2002). Elements of the p Block. Molecular World. Vol. 9. Royal Society of Chemistry. p. 93. ISBN 0-85404-690-9.
^ Suzuki, Hitomi; Matano, Yoshihiro (2001). Organobismuth chemistry. Elsevier. p. 8. ISBN 0-444-20528-4.
^ 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.
^ 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.