Xenon Oxytetrafluoride

Xenon oxytetrafluoride
Identifiers
CAS Number	13774-85-1 ;
3D model (JSmol)	Interactive image;
ChemSpider	10326200 ;
	InChI InChI=1S/F4OXe/c1-6(2,3,4)5 Key: ONRYXFFHIXYZMZ-UHFFFAOYSA-N ; 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
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	verify (what is ?)
	Infobox references

Xenon oxytetrafluoride (Xe O F₄) 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

↑ 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.
↑ ^2.0 ^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.
↑ ^3.0 ^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.
↑ ^4.0 ^4.1 Selig, Henry (Feb 1, 1966). "Complexes of Xenon Oxide Tetrafluoride". Inorg. Chem. 5 (2): 183–186. doi:10.1021/ic50036a004.
↑ Christe, Karl O.; Wilson, William W. (Apr 1988). "Convenient synthesis of xenon oxide tetrafluoride". Inorg. Chem. 27 (7): 1296–1297. doi:10.1021/ic00280a043.
↑ 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">
↑ 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">
↑ 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">
↑ Huston, John L. (Sep 1967). "Xenon dioxide difluoride: isolation and some properties". J. Phys. Chem. 71 (10): 3339–3341. doi:10.1021/j100869a035.

0.00

(0 votes)

Original source: https://en.wikipedia.orghttps://handwiki.org/wiki/ Xenon oxytetrafluoride. Read more

[martins1964-1] 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.

[smith1963-2] 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.

[ibers1965-3] 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.

[selig1966-4] 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.

[nielsen1990-6] 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.

[1]

[2]

[3]

[4]

[5]

[6]

[7]

[8]

[9]

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