Xenon tetrafluoride

Synthesis

The original synthesis of xenon tetrafluoride occurred through direct 1:5-molar-ratio combination of the elements in a nickel (Monel) vessel at 400 °C. The nickel does not catalyze the reaction, but rather protects the container surfaces against fluoride corrosion. Controlling the process against impurities is difficult, as xenon difluoride (), tetrafluoride, and hexafluoride () are all in chemical equilibrium, the difluoride favored at low temperatures and little fluorine and the hexafluoride favored at high temperatures and excess fluorine.{{cite journal | last1=Haner | first1=Jamie | last2=Schrobilgen | first2=Gary J. | title=The Chemistry of Xenon(IV) | journal=Chem. Rev. | volume=115 | issue=2 | date=2015 | pages=1255–1295 | issn=0009-2665 | doi=10.1021/cr500427p

The elements combine more selectively when γ- or UV-irradiated in a nickel container or dissolved in anhydrous hydrogen fluoride with catalytic oxygen. That reaction is believed selective because dioxygen difluoride at standard conditions is too weak an oxidant to generate xenon(VI) species.

Alternatively, fluoroxenonium perfluorometallate salts pyrolyze to XeF4.

Reactions

Xenon tetrafluoride hydrolyzes at low temperatures to form elemental xenon, oxygen, hydrofluoric acid, and aqueous xenon trioxide: :\rm \ 6XeF_4 + 12H_2O \rightarrow 2XeO_3 + 4Xe\uparrow + 3O_2\uparrow + 24HF

It is used as a precursor for synthesis of all tetravalent Xe compounds. Reaction with tetramethylammonium fluoride gives tetramethylammonium pentafluoroxenate, which contains the pentagonal anion. The anion is also formed by reaction with cesium fluoride:

:CsF + →

Reaction with bismuth pentafluoride () forms the cation:{{cite book : + → XeF3BiF6

The cation in the salt XeF3Sb2F11 has been characterized by NMR spectroscopy.

At 400 °C, reacts with xenon to form : :XeF4 + Xe → 2 XeF2

The reaction of xenon tetrafluoride with platinum yields platinum tetrafluoride and xenon: :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. reacts with the silicone to form simple gaseous products, leaving a residue of metal impurities.

References

References

1. (2001). "Inorganic Chemistry". Academic Press.
2. Zumdahl, Steven S.. (2009). "Chemical Principles". Houghton Mifflin Company.
3. Zumdahl. (2007). "Chemistry". Houghton Mifflin.
4. (Mar 1963). "Xenon Tetrafluoride: Reaction with Aqueous Solutions". Science.
5. (2002). "Elements of the ''p'' Block". Royal Society of Chemistry.
6. (1971). "Trifluoroxenon(IV) ''µ''-fluoro-bispentafluoroantimonate(V): the {{chem". Journal of the Chemical Society D: Chemical Communications.
7. (March 1997). "Xenon tetrafluoride as a decomposition agent for silicone rubber for isolation and atomic emission spectrometric determination of trace metals". Analytica Chimica Acta.