Xenon tetrafluoride

Source: Wikipedia, the free encyclopedia.
Xenon tetrafluoride
XeF 4 crystals. 1962.
Names
IUPAC name
Xenon tetrafluoride
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.033.858 Edit this at Wikidata
UNII
  • InChI=1S/F4Xe/c1-5(2,3)4 checkY
    Key: RPSSQXXJRBEGEE-UHFFFAOYSA-N checkY
  • InChI=1/F4Xe/c1-5(2,3)4
    Key: RPSSQXXJRBEGEE-UHFFFAOYAW
  • F[Xe](F)(F)F
Properties
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[1]
Reacts
Structure
D4h
square planar
0 D
Thermochemistry
146 J·mol−1·K−1[2]
Std enthalpy of
formation
(ΔfH⦵298)
 −251 kJ·mol−1[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Xenon tetrafluoride is a

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

kJ/mol.[3]

Xenon tetrafluoride is a colorless

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

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

  1. ISBN 0-12-352651-5
    .
  2. ^
    ISBN 978-0-618-94690-7
    .
  3. ^
    ISBN 978-0-618-52844-8
    .
  4. doi:10.1021/ja00877a042
    .
  5. S2CID 10330125
    .
  6. S2CID 35981023
    .
  7. S2CID 42119788
    .
  8. S2CID 35858682
    .
  9. ^
    PMID 25559700
    .
  10. ^
    ISBN 0-8247-7291-1
    .
  11. S2CID 33320384
    .
  12. ISBN 0-85404-690-9
    .
  13. ISBN 0-444-20528-4
    .
  14. doi:10.1039/C29710001543
    .
  15. doi:10.1016/S0003-2670(96)00563-6
    .

External links
Retrieved from "https://en.wikipedia.org/w/index.php?title=Xenon_tetrafluoride&oldid=1211971191"