Xenon oxytetrafluoride

Identifiers

CAS Number

* 13774-85-1 N

3D model (JSmol)

* Interactive image

ChemSpider |

* 10326200 Y

InChI

* InChI=1S/F4OXe/c1-6(2,3,4)5 Y

Key: ONRYXFFHIXYZMZ-UHFFFAOYSA-N Y

* InChI=1/F4OXe/c1-6(2,3,4)5

Key: ONRYXFFHIXYZMZ-UHFFFAOYAY

SMILES

* F[Xe](F)(F)(F)=O

Properties

Chemical formula

| XeOF4
Molar mass | 223.23 g/mol
Appearance  | colorless liquid
Density | 3.17 g/cm3, liquid
Melting point |  −46.2 °C (−51.2 °F; 227.0 K)

Solubility in water

| Reacts with water
Structure

Molecular shape

| square pyramidal[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 oxytetrafluoride (XeOF4) is an inorganic chemical compound. It is a colorless stable liquid[3][2] with a melting point of −46.2 °C[4] that can be synthesized by partial hydrolysis of XeF6, or the reaction of XeF6 with silica[3] or NaNO3:[5]

NaNO3 \+ XeF6 → NaF \+ XeOF4 \+ FNO2

A high-yield synthesis proceeds by the reaction of XeF6 with POF3 at −196 °C.[6]

As are most xenon oxides, it is extremely reactive and unstable, and hydrolyses in water to give dangerously hazardous and corrosive products, including hydrogen fluoride:

2 XeOF4 \+ 4 H2O → 2 Xe + 8 HF + 3 O2

In addition, some ozone and fluorine are also formed. This reaction is extremely dangerous, and xenon oxytetrafluoride should therefore be kept away from any trace of water or water vapour under all conditions.

## Reactions

XeOF4 reacts with H2O in a following steps:

XeOF4 \+ H2O → XeO2F2 \+ 2 HF
XeO2F2 \+ H2O → XeO3 \+ 2 HF

The XeO3 formed is a dangerous explosive, decomposing explosively to Xe and O2:

2 XeO3 → 2 Xe + 3 O2

In its liquid form, XeOF4 exhibits amphoteric behaviour, forming complexes with both strong Lewis bases like CsF and strong Lewis acids like SbF5.[7] It forms a 1:1 adduct with XeF2, isostructural with XeF2·IF5,[8] as well as various heavy alkali metal fluorides.[4]

The reaction of XeOF4 with XeO3 provides a convenient synthesis route for XeO2F2.[9]

## External links

* WebBook page for XeOF4

## References

1. ↑ Martins, Joseph; E. Bright Wilson Jr. (1964). "Microwave Spectrum of Xenon Oxytetrafluoride". J. Chem. Phys. 41 (570): 570–571. doi:10.1063/1.1725910. Bibcode: 1964JChPh..41..570M.
2. ↑ 2.0 2.1 D. F. Smith (24 May 1963). "Xenon Oxyfluoride". Science 140 (3569): 899–900. doi:10.1126/science.140.3569.899. PMID 17810680. Bibcode: 1963Sci...140..899S.
3. ↑ 3.0 3.1 Ibers, James A. (Oct 1965). "Molecular Structure". Annual Review of Physical Chemistry 16: 375–396. doi:10.1146/annurev.pc.16.100165.002111. Bibcode: 1965ARPC...16..375I.
4. ↑ 4.0 4.1 Selig, Henry (Feb 1, 1966). "Complexes of Xenon Oxide Tetrafluoride". Inorg. Chem. 5 (2): 183–186. doi:10.1021/ic50036a004.
5. ↑ Christe, Karl O.; Wilson, William W. (Apr 1988). "Convenient synthesis of xenon oxide tetrafluoride". Inorg. Chem. 27 (7): 1296–1297. doi:10.1021/ic00280a043.
6. ↑ Nielsen, Jon B.; Kinkead, Scott A.; Eller, P. Gary (Sep 1, 1990). "A New Synthesis of Xenon Oxytetrafluoride, XeOF4". Inorg. Chem. 29 (18): 3621–3622. doi:10.1021/ic00343a063.XeOF4&rft.jtitle=Inorg.+Chem.&rft.aulast=Nielsen&rft.aufirst=Jon+B.&rft.au=Nielsen, Jon+B.&rft.au=Kinkead, Scott+A.&rft.au=Eller, P.+Gary&rft.date=Sep+1,+1990&rft.volume=29&rft.issue=18&rft.pages=3621–3622&rft_id=info:doi/10.1021/ic00343a063&rfr_id=info:sid/en.wikibooks.org:Chemistry:Xenon_oxytetrafluoride">
7. ↑ D.Martin-Rovet; C.Angelié; M.Cauchetier; G.J.Schrobilgen (Sep 1982). "Various aspects of the reactivity of the xenon(VI) oxyfluoride: XeOF4". Journal of Fluorine Chemistry 21 (1): 10. doi:10.1016/S0022-1139(00)85330-0.XeOF4&rft.jtitle=Journal+of+Fluorine+Chemistry&rft.aulast=D.Martin-Rovet&rft.au=D.Martin-Rovet&rft.au=C.Angelié&rft.au=M.Cauchetier&rft.au=G.J.Schrobilgen&rft.date=Sep+1982&rft.volume=21&rft.issue=1&rft.pages=10&rft_id=info:doi/10.1016/S0022-1139(00)85330-0&rfr_id=info:sid/en.wikibooks.org:Chemistry:Xenon_oxytetrafluoride">
8. ↑ N. Bartlett; M. Wechsberg (Oct 1971). "The Xenon Difluoride Complexes XeF2 · XeOF4; XeF2 · XeF6 · AsF5 and XeF2 · 2 XeF6 · 2 AsF5 and Their Relevance to Bond Polarity and Fluoride Ion Donor Ability of XeF2 and XeF6". Z. Anorg. Allg. Chem. 385 (1). doi:10.1002/zaac.19713850103.XeF2+·+XeOF4;+XeF2+·+XeF6+·+AsF5+and+XeF2+·+2+XeF6+·+2+AsF5+and+Their+Relevance+to+Bond+Polarity+and+Fluoride+Ion+Donor+Ability+of+XeF2+and+XeF6&rft.jtitle=Z.+Anorg.+Allg.+Chem.&rft.aulast=N.+Bartlett&rft.au=N.+Bartlett&rft.au=M.+Wechsberg&rft.date=Oct+1971&rft.volume=385&rft.issue=1&rft_id=info:doi/10.1002/zaac.19713850103&rfr_id=info:sid/en.wikibooks.org:Chemistry:Xenon_oxytetrafluoride">
9. ↑ Huston, John L. (Sep 1967). "Xenon dioxide difluoride: isolation and some properties". J. Phys. Chem. 71 (10): 3339–3341. doi:10.1021/j100869a035.

* 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

|

Xenon(IV)|

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

| Organoxenon(IV) compounds|

* XeF2C6F5BF4

|

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

|

Rn(VI)|

* RnO3

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