Xenon tetrafluoride is produced by heating a mixture of xenon and fluorine in a 1:5 ratio in a nickel container to 400 °C. Some xenon hexafluoride, XeF 6, is also produced, and this production is increased with an increased fluorine concentration in the input mixture. The nickel is not a catalyst for this reaction; nickel containers are used because they react with fluorine to form a protective, non-peeling layer of nickel fluorideNiF 2 on their interior surfaces.
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.
^Arnold F. Holleman; Egon Wiberg (2001). Nils Wiberg (ed.). Inorganic chemistry. Translated by Mary Eagleson; William Brewer. Academic Press. p. 394. ISBN0-12-352651-5.
^ abZumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin Company. p. A23. ISBN0-618-94690-X.
^C. L. Chernick; H. H. Claassen; P. R. Fields; H. H. Hyman; J. G. Malm; W. M. Manning; M. S. Matheson; L. A. Quarterman; F. Schreiner; H. H. Selig; I. Sheft; S. Siegel; E. N. Sloth; L. Stein; M. H. Studier; J. L. Weeks & M. H. Zirin (1962). "Fluorine Compounds of Xenon and Radon". Science. 138 (3537): 136–138. Bibcode:1962Sci...138..136C. doi:10.1126/science.138.3537.136. PMID17818399.
^Gillespie, R. J.; B. Landa; G. J. Schrobilgen (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. doi:10.1016/S0003-2670(96)00563-6.