Xenon tetrafluoride

Short description: Chemical compound

Xenon tetrafluoride

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Names
IUPAC name

Xenon tetrafluoride

Identifiers

CAS Number

* 13709-61-0 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 109927 Y

PubChem CID

* 123324

UNII |

* O825AI8P4W Y

InChI

* InChI=1S/F4Xe/c1-5(2,3)4 Y

Key: RPSSQXXJRBEGEE-UHFFFAOYSA-N Y

* InChI=1/F4Xe/c1-5(2,3)4

Key: RPSSQXXJRBEGEE-UHFFFAOYAW

SMILES

* F[Xe](F)(F)F

Properties

Chemical formula

| XeF4
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]

Solubility in water

| Reacts
Structure

Coordination geometry

| D4h

Molecular shape

| square planar

Dipole moment

| 0 D
Thermochemistry

Std molar
entropy (S ~~o~~ 298)

| 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 YN ?)
Infobox references

Xenon tetrafluoride is a chemical compound with chemical formula XeF4. 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 F2 → XeF4

This reaction is exothermic, releasing an energy of 251 kJ/mol.[3]

Its discovery in 1962 was inspired [4] by the discovery earlier in the same year by Neil Bartlett of the first xenon compound, XePtF6, which showed that it was possible for a xenon commpound to exist.

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.

## Contents

* 1 Synthesis
* 2 Reactions
* 3 Applications
* 4 References
* 5 External links

## 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.[9] The nickel does not catalyze the reaction,[citation needed] but rather protects the container surfaces against fluoride corrosion. Controlling the process against impurities is difficult, as xenon difluoride (XeF2), tetrafluoride, and hexafluoride (XeF6) are all in chemical equilibrium, the difluoride favored at low temperatures and little fluorine and the hexafluoride favored at high temperatures and excess fluorine.[9][10] Fractional sublimation (xenon tetrafluoride is particularly involatile) or other equilibria generally allow purification of the product mixture.[9]

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.[9]

Alternatively, fluoroxenonium perfluorometallate salts pyrolyze to XeF4.[9]

## Reactions

Xenon tetrafluoride hydrolyzes at low temperatures to form elemental xenon, oxygen, hydrofluoric acid, and aqueous xenon trioxide:[11]

6XeF4+12H2O->2XeO3+4Xe↑+3O2↑+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 + XeF4 → CsXeF5

Reaction with bismuth pentafluoride (BiF5) forms the XeF+3 cation:[13]

BiF5 \+ XeF4 → XeF3BiF6

The XeF+3 cation in the salt XeF3Sb2F11 has been characterized by NMR spectroscopy.[14]

At 400 °C, XeF4 reacts with xenon to form XeF2:[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. XeF4 reacts with the silicone to form simple gaseous products, leaving a residue of metal impurities.[15]

## References

1. ↑ Holleman, Arnold F.; Wiberg, Egon (2001). Wiberg, Nils. ed. Inorganic Chemistry. Academic Press. p. 394. ISBN 0-12-352651-5.
2. ↑ 2.0 2.1 Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
3. ↑ 3.0 3.1 Zumdahl (2007). Chemistry. Boston: Houghton Mifflin. p. 243. ISBN 978-0-618-52844-8.
4. ↑ 4.0 4.1 Claassen, H. H.; Selig, H.; Malm, J. G. (1962). "Xenon Tetrafluoride". J. Am. Chem. Soc. 84 (18): 3593. doi:10.1021/ja00877a042.
5. ↑ Chernick, C. L.; Claassen, H. H.; Fields, P. R.; Hyman, H. H.; Malm, J. G.; Manning, W. M.; Matheson, M. S.; Quarterman, L. A. et al. (1962). "Fluorine Compounds of Xenon and Radon". Science 138 (3537): 136–138. doi:10.1126/science.138.3537.136. PMID 17818399. Bibcode: 1962Sci...138..136C.
6. ↑ Brown, Thomas H.; Whipple, E. B.; Verdier, Peter H. (1963). "Xenon Tetrafluoride: Fluorine-19 High-Resolution Magnetic Resonance Spectrum". Science 140 (3563): 178. doi:10.1126/science.140.3563.178. PMID 17819836. Bibcode: 1963Sci...140..178B.
7. ↑ Ibers, James A.; Hamilton, Walter C. (1963). "Xenon Tetrafluoride: Crystal Structure". Science 139 (3550): 106–107. doi:10.1126/science.139.3550.106. PMID 17798707. Bibcode: 1963Sci...139..106I.
8. ↑ 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. Bibcode: 1963Sci...139.1208B.
9. ↑ 9.0 9.1 9.2 9.3 9.4 9.5 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.
10. ↑ 10.0 10.1 10.2 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. https://archive.org/details/standardpotentia0000unse/page/767.
11. ↑ Williamson; Koch, C. W. (Mar 1963). "Xenon Tetrafluoride: Reaction with Aqueous Solutions". Science 139 (3559): 1046–1047. doi:10.1126/science.139.3559.1046. ISSN 0036-8075. PMID 17812981. Bibcode: 1963Sci...139.1046W.
12. ↑ Harding, Charlie; Johnson, David Arthur; Janes, Rob (2002). Elements of the p Block. Molecular World. 9. Royal Society of Chemistry. p. 93. ISBN 0-85404-690-9.
13. ↑ Suzuki, Hitomi; Matano, Yoshihiro (2001). Organobismuth chemistry. Elsevier. p. 8. ISBN 0-444-20528-4.
14. ↑ 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.XeF+3+cation&rft.jtitle=Journal+of+the+Chemical+Society+D:+Chemical+Communications&rft.aulast=Gillespie&rft.aufirst=R.+J.&rft.au=Gillespie, R.+J.&rft.au=Landa, B.&rft.au=Schrobilgen, G.+J.&rft.date=1971&rft.issue=23&rft.pages=1543–1544&rft_id=info:doi/10.1039/C29710001543&rfr_id=info:sid/en.wikibooks.org:Chemistry:Xenon_tetrafluoride">
15. ↑ 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. Bibcode: 1997AcAC..340....1R.

## External links

* WebBook page for XeF4

* v
* t
* e

Xenon compounds

Xenon(0)|

* AuXe4(Sb2F11)2

Xenon(I)|

* XePtF6
* XeRhF6
* XeRuF6
* XePuF6
* XeF

Xenon(II)|

* XeF2
* XeFPtF5
* XeFPt2F11
* Xe2F3PtF6
* XeCl2
* XeBr2

| Organoxenon(II) compounds|

* XeC6F5F
* XeC6F5C2F3
* XeC6F5CF3
* Xe(C6F5)2
* XeC6F5C6H2F3
* XeC6F5CN
* Xe(CF3)2

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Xenon(IV)|

* XeO2
* XeF4
* XeOF2
* N(CH3)4XeF5
* XeCl4

| Organoxenon(IV) compounds|

* XeF2C6F5BF4

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Xenon(VI)|

* XeO3
* XeF6
* XeOF4
* H2XeO4
* (NO)2XeF8
* CsXeF7
* RbXeF7

Xenon(VIII)|

* XeO4
* H4XeO6

Category:Xenon compounds

* v
* t
* e

Noble gas compounds

Helium compounds|

* helium compounds
* HeH+
* LiHe
* Na2He
* He2
* He3

Neon compounds|

* neon compounds

Argon compounds|

* argon compounds
* ArH+
* HArF
* MgAr+
* ArCF22+

Krypton compounds|

* KrF2
* HKrCN
* HKrC2H
* Kr(OTeF5)2
* HCNKrF2

Xenon compounds|

| Xe(0)|

* AuXe4(Sb2F11)2

|

Xe(I)|

* XePtF6
* XeRhF6

Xe(II)|

* XeF2
* XeFPtF5
* XeFPt2F11
* Xe2F3PtF6
* XeCl2
* Organoxenon(II) compounds

Xe(IV)|

* XeO2
* XeF4
* XeOF2
* N(CH3)4XeF5
* Organoxenon(IV) compounds

Xe(VI)|

* XeO3
* XeF6
* XeOF4
* H2XeO4
* (NO)2XeF8

Xe(VIII)|

* XeO4
* H4XeO6

Radon compounds|

| Rn(II)|

* RnF2
* RnFSb2F11

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Rn(VI)|

* RnO3

* v
* t
* e

Fluorine compounds

| HF |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  | He

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LiF | BeF2 |  |  |  |  |  |  |  |  |  |  | BF3
B2F4 | CF4 | NF3 | OF2 | F− | Ne
NaF | MgF2 |  |  |  |  |  |  |  |  |  |  | AlF3 | SiF4 | PF3
PF5 | SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF2 | ScF3 | TiF3
TiF4 | VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5 | MnF2
MnF3 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF3 | GeF4 | AsF3
AsF5 | SeF4
SeF6 | BrF3
BrF5 | KrF2
RbF | SrF2 | YF3 | ZrF4 | NbF4
NbF5 | MoF5
MoF6 | TcF6 | RuF3
RuF4
RuF5
RuF6 | RhF6 | PdF2 | AgF
AgF2
Ag2F | CdF2 | InF3 | SnF2
SnF4 | SbF3
SbF5 | TeF4 | IF
IF3
IF5
IF7 | XeF2
XeF4
XeF6
CsF | BaF2 | *  | HfF4 | TaF5 | WF4
WF6 | ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF3
IrF5
IrF6 | PtF4
PtF6 | AuF3
Au2F10
AuF5·F2
| HgF2
Hg2F2 | TlF
TlF3 | PbF2
PbF4 | BiF3
BiF5 | Po | At | RnF2
Fr | Ra | **  | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og
|  | ↓ |  |  |  |  |  |  |  |  |  |  |  |  |  |  |
| * | LaF3 | CeF3 | Pr | NdF3 | PmF3 | SmF3
| Eu | Gd | Tb | DyF3 | Ho | Er | Tm | YbF3
| Lu |
| ** | AcF3 | ThF4 | Pa | UF3
UF4
UF5
UF6 | NpF3
NpF4
NpF5
NpF6
| PuF3
PuF4
PuF5
PuF6 | AmF3
AmF4 | CmF3 | Bk | Cf | Es | Fm | Md | No | Lr |

Other|

* AgBF4
* AgPF6
* Cs2AlF5
* K3AlF6
* Na3AlF6
* KAsF6
* LiAsF6
* NaAsF6
* HBF4
* KBF4
* LiBF4
* NaBF4
* RbBF4
* Ba(BF4)2
* Ni(BF4)2
* Pb(BF4)2
* Sn(BF4)2
* BaClF
* BaSiF6
* BaGeF6
* BrOF3
* BrO2F
* CBrF3
* CBr2F2
* CBr3F
* CClF3
* CCl2F2
* CCl3F
* CFN
* CF2O
* CF3I
* CHF3
* CH2F2
* CH3F
* C2Cl3F3
* C2H3F
* C6H5F
* C7H5F3
* C15F33N
* ClFO2
* CrFO4
* CrF2O2
* CsBF4
* NH4F
* FNO
* FNO2
* FNO3
* KHF2
* NaHF2
* ThOF2
* NH5F2
* (NH4)2SiF6
* F2OS
* F3OP
* PSF3
* HPF6
* HSbF6
* NH4PF6
* KPF6
* KSbF6
* LiPF6
* NaPF6
* NaSbF6
* Na2SiF6
* Na2TiF6
* Na2ZrF6
* TlPF6
* IOF3
* K2NbF7
* K2TaF7
* IO3F
* UO2F2

Chemical formulas

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