Xenon tetrafluoride

Xenon tetrafluoride
IUPAC name

Xenon tetrafluoride
Identifiers
CAS number 13709-61-0 Y
PubChem 123324
ChemSpider 109927 Y
Jmol-3D images Image 1
Properties
Molecular formula XeF4
Molar mass 207.2836 g mol−1
Appearance White solid
Density 4.040 g cm−3, solid
Melting point

117 °C sublimates (390 K)[1]
Structure
Coordination
geometry		 D4h
Molecular shape square planar
Dipole moment 0 D
Thermochemistry
Std enthalpy of
formation ΔfHo298		 −284 kJ/mol[1]
Hazards
Flash point  ? °C
 Y (verify) (what is: Y/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Xenon tetrafluoride is a chemical compound with chemical formula XeF4. It was the first discovered binary compound of a noble gas.[2] It is produced by the chemical reaction of xenon with fluorine, F2, according to the chemical equation:[3][4]

Xe + 2 F2 → XeF4

This reaction is exothermic, releasing an energy of 251 kJ/mol of xenon.[2]

Xenon tetrafluoride is a colorless crystalline substance under ordinary conditions. Its crystalline structure was determined by both NMR spectroscopy and X-ray crystallography in 1963.[5][6] The structure is square planar, as has been confirmed by neutron diffraction studies,[7] and is justified by VSEPR theory because xenon has two lone pairs of electrons above and below the plane of the molecule.

Xenon tetrafluoride sublimes at a temperature of 115.7 °C (240.26 °F).

The formation of xenon tetrafluoride, like the other xenon fluorides, is exergonic. They are stable at normal temperatures and pressures. All of them readily react with water, releasing pure xenon gas, hydrogen fluoride, and molecular oxygen. This reaction occurs in slightly moist air; hence, all xenon fluorides must be kept in anhydrous atmospheres.

Contents

Synthesis

Xenon tetrafluoride is produced by heating a mixture of xenon and fluorine in a 1:3 ratio in a nickel container to 400 °C. Some xenon hexafluoride, XeF6, is also produced, and this production is increased with an increased fluorine concentration in the input mixture.[8] 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 fluoride NiF4 on their interior surfaces.

Chemistry

Xenon tetrafluoride is hydrolyzed by water at low temperatures to form elemental xenon, oxygen, hydrofluoric acid, and aqueous xenon trioxide.[9]

Reaction with tetramethylammonium fluoride forms tetramethylammonium pentafluoroxenate, which contains the pentagonal XeF−
5 anion. The XeF−
5 anion is also formed by reaction with caesium fluoride:[10]

CsF + XeF4 → CsXeF5

Reaction with bismuth pentafluoride (BiF5) forms the XeF+
3 cation:[11]

BiF5 + XeF4 → XeF+
3BiF−
6

The XeF+
3 cation has also been identified in the salt [XeF+
3][Sb2F−
11] by NMR spectroscopy.[12]

At 400 °C, XeF4 reacts with xenon gas to form XeF2.[8]

The reaction of xenon tetrafluoride with platinum yields platinum tetrafluoride (PtF4) and xenon gas.[8]

Applications

Xenon tetrafluoride is used as a decomposition agent of silicone rubber for analysing trace metal impurities in the rubber. XeF4 reacts with the silicone structure that makes up the backbone of silicone rubber to form simple gaseous products, leaving behind any content of metal impurities.[13]

References

  1. ^ a b Arnold F. Holleman; Egon Wiberg (2001). Nils Wiberg. ed. Inorganic chemistry. translated by Mary Eagleson, William Brewer. Academic Press. p. 394. ISBN 0123526515. 
  2. ^ a b Zumdahl (2007). Chemistry. Boston: Houghton Mifflin. p. 243. ISBN 0-618-52844-X. 
  3. ^ Claassen, H. H.; Selig, H.; Malm, J. G. (1962). "Xenon Tetrafluoride". J. Am. Chem. Soc. 84 (18): 3593. doi:10.1021/ja00877a042. 
  4. ^ C. L. Chernick, H. H. Claassen, P. R. Fields 1, 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, and M. H. Zirin (1962). "Fluorine Compounds of Xenon and Radon". Science 138 (3537): 136–138. doi:10.1126/science.138.3537.136. PMID 17818399. 
  5. ^ Thomas H. Brown, E. B. Whipple, and Peter H. Verdier (1963). "Xenon Tetrafluoride: Fluorine-19 High-Resolution Magnetic Resonance Spectrum". Science 140 (3563): 178. doi:10.1126/science.140.3563.178. PMID 17819836. 
  6. ^ James A. Ibers and Walter C. Hamilton (1963). "Xenon Tetrafluoride: Crystal Structure". Science 139 (3550): 106–107. doi:10.1126/science.139.3550.106. PMID 17798707. 
  7. ^ 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. doi:10.1126/science.139.3560.1208. PMID 17757912. 
  8. ^ a b c Allen J. Bard; Roger Parsons; Joseph Jordan; International Union of Pure and Applied Chemistry (1985). Standard Potentials in Aqueous Solution. CRC Press. pp. 767–768. ISBN 0824772911. 
  9. ^ 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.  edit
  10. ^ Charlie Harding; David Arthur Johnson; Rob Janes (2002). Elements of the p block (Volume 9 of Molecular world). Royal Society of Chemistry. p. 93. ISBN 0854046909. 
  11. ^ Hitomi Suzuki; Yoshihiro Matano (2001). Organobismuth chemistry. Elsevier. p. 8. ISBN 0444205284. 
  12. ^ 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.  edit
  13. ^ Rigin, V.; Nikolaj K. Skvortsov; Vassili V. Rigin (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.  edit

External links