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Revision as of 16:17, 10 January 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,074 edits Saving copy of the {{chembox}} taken from revid 470095425 of page Xenon_difluoride for the Chem/Drugbox validation project (updated: '').		Latest revision as of 23:24, 30 December 2024 edit Bernanke's Crossbow (talk | contribs)Extended confirmed users7,929 edits duplicate cite
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	{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}}
	{{chembox		{{chembox
			| Watchedfields = changed
	| verifiedrevid = 445367468
			| verifiedrevid = 470633358
	| Name = Xenon difluoride
	| ImageFile = Xenon-difluoride-2D.png		| Name = Xenon difluoride
			| ImageFile = XeF2 kristalle.png
	<!-- | ImageSize = 140px -->
	| ImageName = Xenon difluoride		| ImageName = {{chem|XeF|2}} crystals. 1962.
	| ImageFile1 = Xenon-difluoride-3D-vdW.png		| ImageFile1 = Xenon-difluoride-2D.png
			| ImageName1 = Xenon difluoride
	<!-- | ImageSize1 = 140px -->
	| ImageName1 = Xenon difluoride		| ImageFile2 = Xenon-difluoride-3D-vdW.png
	| IUPACName = Xenon difluoride<br/>Xenon(II) fluoride		| ImageName2 = Xenon difluoride
			| ImageFile3 = Xenon-difluoride-xtal-3D-vdW.png
	| OtherNames =
			| ImageName3 =
	| Section1 = {{Chembox Identifiers
			| IUPACName = Xenon difluoride<br/>Xenon(II) fluoride
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
			| OtherNames =
			|Section1={{Chembox Identifiers
			| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 75497		| ChemSpiderID = 75497
	| InChI = 1/F2Xe/c1-3-2		| InChI = 1/F2Xe/c1-3-2
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	| StdInChIKey = IGELFKKMDLGCJO-UHFFFAOYSA-N		| StdInChIKey = IGELFKKMDLGCJO-UHFFFAOYSA-N
	| CASNo = 13709-36-9		| CASNo = 13709-36-9
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
			| UNII_Ref = {{fdacite|correct|FDA}}
	| PubChem = 83674
	| SMILES = FF		| UNII = 6POJ14981P
			| PubChem = 83674
			| SMILES = FF
	}}		}}
	| Section2 = {{Chembox Properties		|Section2={{Chembox Properties
	| Xe = 1 | F = 2		| Xe=1 | F=2
	| Appearance = White solid		| Appearance = White solid
	| Density = 4.32 g/cm<sup>3</sup>, solid		| Density = 4.32 g/cm<sup>3</sup>, solid
	| Solubility = Decomposes		| Solubility = 25 g/L (0 °C)
			| MeltingPtC = 128.6
	| MeltingPt = 128.6 °C <ref>{{cite journal | author = Hindermann, D. K., Falconer, W. E. | title = Magnetic Shielding of 19F in XeF2 | journal = ] | volume = 50 | issue = 3 | page = 1203 | year = 1969 | doi = 10.1063/1.1671178 | bibcode = 1969JChPh..50.1203H}}</ref>
			| MeltingPt_ref = <ref>{{cite journal | author = Hindermann, D. K., Falconer, W. E. | title = Magnetic Shielding of 19F in XeF2 | journal = ] | volume = 50 | issue = 3 | page = 1203 | year = 1969 | doi = 10.1063/1.1671178 | bibcode = 1969JChPh..50.1203H}}</ref>
	| VaporPressure = 6.0×10<sup>2</sup> Pa<ref name="tramsek"/>
			| VaporPressure = {{val|6.0e2|u=Pa}}<ref name="tramsek"/>
	| pKa =
	| Viscosity =		| pKa =
			| Viscosity =
	}}		}}
	| Section3 = {{Chembox Structure		|Section3={{Chembox Structure
	| MolShape = ]		| MolShape = ]
	| CrystalStruct = parallel linear XeF<sub>2</sub> units		| CrystalStruct = parallel linear XeF<sub>2</sub> units
	| Dipole = 0 ]		| Dipole = 0 ]
	}}		}}
	| Section7 = {{Chembox Hazards		|Section4={{Chembox Thermochemistry
			| DeltaHf = −108&nbsp;kJ·mol<sup>−1</sup><ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7|page=A23}}</ref>
	| ExternalMSDS =
			| Entropy = 254&nbsp;J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=b1/>
	| MainHazards = Corrosive to exposed tissues. Releases toxic compounds on contact with moisture.<ref>{{cite web | publisher=BOC Gases | title = MSDS: xenon difluoride | accessdate = 2010-06-01 | url = http://www.vngas.com/pdf/g86.pdf }}</ref>
			}}
	| NFPA-H = 3
			|Section7={{Chembox Hazards
	| NFPA-F = 0
			| GHSPictograms = {{GHS05}}{{GHS06}}{{GHS03}}
	| NFPA-R = 1
	| NFPA-O = OX		| GHSSignalWord = Danger
			| HPhrases = {{H-phrases|272|301|314|330}}
			| PPhrases = {{P-phrases |210|220|221|260|264|270|271|280|284|301+310+330|303+361+353|304+340+310|305+351+338|331|363|370+378|403+233|405|501}}<ref>
			{{cite web |title=Sigma Aldrich Xenon Difluoride SDS |url=https://www.sigmaaldrich.com/US/en/sds/aldrich/394505 |website=Sigma Aldrich |publisher=Millipore Sigma |access-date=2 November 2022}}</ref>
			| ExternalSDS =
			| MainHazards = Corrosive to exposed tissues. Releases toxic compounds on contact with moisture.<ref>{{cite web|publisher=BOC Gases |title=MSDS: xenon difluoride |access-date=2010-06-01 |url=http://www.vngas.com/pdf/g86.pdf }}</ref>
			| NFPA-H = 3
			| NFPA-F = 0
			| NFPA-R = 1
			| NFPA-S = OX
	}}		}}
	| Section8 = {{Chembox Related		|Section8={{Chembox Related
	| OtherCpds = ]<br/>]		| OtherCompounds = ]<br/>]
	| OtherCations = ]		| OtherCations = ]<br/>]
			| OtherAnions = ]<br/>]
	}}		}}
	}}		}}
			'''Xenon difluoride''' is a powerful ] with the chemical formula {{chem|XeF|2}}, and one of the most stable ]. Like most ] inorganic ]s it is moisture-sensitive. It ] on contact with ], but is otherwise stable in storage. Xenon difluoride is a dense, colourless ]line solid.
			It has a nauseating odour and low ].<ref>{{cite book |author1=James L. Weeks |author2=Max S. Matheson |title=Inorganic Syntheses |chapter=Xenon Difluoride | doi = 10.1002/9780470132395.ch69| journal = ] | volume = 8|pages=260–264 |date=1966 |isbn=9780470132395 }}</ref>
			==Structure==
			Xenon difluoride is a ] molecule with an Xe–F bond length of {{val|197.73|0.15|u=]}} in the vapor stage, and 200&nbsp;pm in the solid phase. The packing arrangement in solid {{chem|XeF|2}} shows that the fluorine atoms of neighbouring molecules avoid the equatorial region of each {{chem|XeF|2}} molecule. This agrees with the prediction of ] theory, which predicts that there are 3 pairs of non-bonding electrons around the equatorial region of the xenon atom.<ref name="tramsek"/>
			At high pressures, novel, non-molecular forms of xenon difluoride can be obtained. Under a pressure of ~50&nbsp;], {{chem|XeF|2}} transforms into a semiconductor consisting of {{chem|XeF|4}} units linked in a two-dimensional structure, like ]. At even higher pressures, above 70&nbsp;GPa, it becomes metallic, forming a three-dimensional structure containing {{chem|XeF|8}} units.<ref>{{Cite journal | doi = 10.1038/nchem.724 | pmid = 20729901 | title = Two- and three-dimensional extended solids and metallization of compressed XeF2 | year = 2010 | last1 = Kim | pages = 784–788 | first1 = M. | last2 = Debessai | volume = 2 | first2 = M. | last3 = Yoo | first3 = C. S. | journal = Nature Chemistry|bibcode = 2010NatCh...2..784K | issue=9}}</ref> However, a recent theoretical study has cast doubt on these experimental results.<ref>{{Cite journal | last1 = Kurzydłowski | first1 = D. | last2 = Zaleski-Ejgierd | first2 = P. | last3 = Grochala | first3 = W. | last4 = Hoffmann | first4 = R. | title = Freezing in Resonance Structures for Better Packing: XeF2Becomes (XeF+)(F−) at Large Compression | doi = 10.1021/ic200371a | journal = Inorganic Chemistry | volume = 50 | issue = 8 | pages = 3832–3840 | year = 2011 | pmid = 21438503}}</ref>
			The Xe–F bonds are weak. XeF<sub>2</sub> has a total bond energy of {{cvt|267.8|kJ/mol|kcal/mol}}, with first and second bond energies of {{cvt|184.1|kJ/mol|kcal/mol}} and {{cvt|83.68|kJ/mol|kcal/mol}}, respectively. However, XeF<sub>2</sub> is much more robust than KrF<sub>2</sub>, which has a total bond energy of only {{cvt|92.05|kJ/mol|kcal/mol}}.<ref>{{Cite book|title=The Chemistry of the Monatomic Gases|series=Pergamon Texts in Inorganic Chemistry|last1=Cockett|first1=A. H.|date=2013|publisher=Elsevier Science|last2=Smith|first2= K. C. |last3=Bartlett|first3= Neil|isbn=9781483157368|location=St. Louis, MO|oclc=953379200}}</ref>
			==Chemistry==
			===Synthesis===
			Synthesis proceeds by the simple reaction:
			:Xe + F<sub>2</sub> → XeF<sub>2</sub>
			The reaction needs heat, irradiation, or an electrical discharge. The product is a solid. It is purified by ] or selective condensation using a vacuum line.<ref name=SynthApps/>
			The first published report of XeF<sub>2</sub> was in October 1962 by Chernick, et al.<ref>{{cite journal |title=Fluorine Compounds of Xenon and Radon
			| author =Chernick, CL and Claassen, HH and Fields, PR and Hyman, HH and Malm, JG and Manning, WM and Matheson, MS and Quarterman, LA and Schreiner, F. and Selig, HH
			| journal =]
			| volume =138
			| pages =136–138
			| year =1962 |doi=10.1126/science.138.3537.136
			| issue =3537 |pmid=17818399|bibcode = 1962Sci...138..136C | s2cid =10330125
			|display-authors=etal}}</ref> However, though published later,<ref>{{cite journal
			| doi =10.1002/anie.196205992
			| title =Fluorination of Xenon
			|author1=Hoppe, R. |author2=Daehne, W. |author3=Mattauch, H. |author4=Roedder, K. | year = 1962
			| journal =]
			| volume =1
			| issue =11
			| pages =599}}</ref> XeF<sub>2</sub> was probably first created by ] at the ], Germany, in early 1962, by reacting fluorine and xenon gas mixtures in an electrical discharge.<ref>{{cite journal |first=R. |last=Hoppe |title=Die Valenzverbindungen der Edelgase |journal=Angewandte Chemie |year=1964 |volume=76 |issue=11 |page=455 |doi=10.1002/ange.19640761103|bibcode=1964AngCh..76..455H }} First review on the subject by the pioneer of covalent noble gas compounds.</ref> Shortly after these reports, Weeks, Chernick, and Matheson of ] reported the synthesis of XeF<sub>2</sub> using an all-nickel system with transparent ] windows, in which equal parts xenon and fluorine gases react at low pressure upon irradiation by an ] source to give XeF<sub>2</sub>.<ref>{{cite journal
			| title = Photochemical Preparation of Xenon Difluoride" Photochemical Preparation of Xenon Difluoride
			|author1=Weeks, J. |author2=Matheson, M. |author3=Chernick, C. | journal = ]
			| volume = 84
			| issue = 23
			| pages = 4612–4613
			| year = 1962
			| doi = 10.1021/ja00882a063 }}</ref> Williamson reported that the reaction works equally well at atmospheric pressure in a dry ] glass bulb using sunlight as a source. It was noted that the synthesis worked even on cloudy days.<ref>{{cite book | last1 = Williamson | first1 = Stanley M. | last2 = Sladky | first2 = Friedrich O. | last3 = Bartlett | first3 = Neil | title = Inorganic Syntheses | chapter = Xenon Difluoride | journal = ] | volume = 11 | pages = 147–151 | year = 1968 | doi = 10.1002/9780470132425.ch31| isbn = 9780470132425 }}</ref>
			In the previous syntheses the fluorine gas reactant had been purified to remove ]. Šmalc and Lutar found that if this step is skipped the reaction rate proceeds at four times the original rate.<ref>{{cite book | last1 = Šmalc | first1 = Andrej | last2 = Lutar | first2 = Karel | last3 = Kinkead | first3 = Scott A. | title = Inorganic Syntheses | chapter = Xenon Difluoride (Modification) | doi = 10.1002/9780470132609.ch1 | journal = ] | pages = 1–4 | volume = 29| date = 2007 | isbn = 9780470132609 }}</ref>
			In 1965, it was also synthesized by reacting xenon gas with ].<ref>{{Cite journal | doi = 10.1021/ic50027a038 | title = The Reaction of Xenon with Dioxygen Difluoride. A New Method for the Synthesis of Xenon Difluoride | year = 1965 | last1 = Morrow | first1 = S. I. | last2 = Young | first2 = A. R. | journal = Inorganic Chemistry | volume = 4 | issue = 5| pages = 759–760 }}</ref>
			===Solubility===
			{{chem|XeF|2}} is soluble in solvents such as ], ], ], anhydrous ], and ], without reduction or oxidation. Solubility in hydrogen fluoride is high, at 167&nbsp;g per 100&nbsp;g HF at 29.95&nbsp;°C.<ref name="tramsek">{{cite journal
			| author = Melita Tramšek
			| author2 = Boris Žemva
			| title = Synthesis, Properties and Chemistry of Xenon(II) Fluoride
			| year = 2006 | journal = Acta Chim. Slov.
			| volume = 53
			| issue = 2
			| pages = 105–116
			| doi = 10.1002/chin.200721209
			| url = http://acta-arhiv.chem-soc.si/53/53-2-105.pdf}}</ref>
			===Derived xenon compounds===
			Other xenon compounds may be derived from xenon difluoride. The unstable ] compound {{chem|Xe(CF|3|)|2}} can be made by irradiating ] to generate {{chem|CF|3|•}} ] and passing the gas over {{chem|XeF|2}}. The resulting waxy white solid decomposes completely within 4 hours at room temperature.<ref name="harding">{{cite book
			| title = Elements of the ''p'' block
			| first1 = Charlie
			| last1 = Harding
			| first2 = David Arthur
			| last2 = Johnson
			| first3 = Rob
			| last3 = Janes
			| publisher = Royal Society of Chemistry, Open University
			| year = 2002
			| isbn = 978-0-85404-690-4
			}}</ref>
			The XeF<sup>+</sup> cation is formed by combining xenon difluoride with a strong fluoride acceptor, such as an excess of liquid ] ({{chem|SbF|5}}):
			: {{chem|XeF|2}} + {{chem|SbF|5}} → {{chem|XeF|+}} + {{chem|SbF|6|−}}
			Adding xenon gas to this pale yellow solution at a pressure of 2–3 ] produces a green solution containing the paramagnetic {{chem|Xe|2|+}} ion,<ref>{{Cite journal| first1 = D. R.| first2 = M. J.| first3 = A. J.| first4 = R. C.| first5 = A. R.| last1 = Brown| first6 = J. R.| first7 = L. .| title = The dixenon(1+) cation: formation in the condensed phases and characterization by ESR, UV-visible, and Raman spectroscopy| journal = Inorganic Chemistry| volume = 31| issue = 24| pages = 5041–5052| year = 1992| doi = 10.1021/ic00050a023| last2 = Clegg| last3 = Downs| last4 = Fowler| last5 = Minihan| last6 = Norris| last7 = Stein}}</ref> which contains a Xe−Xe bond: ("apf" denotes solution in liquid {{chem|SbF|5}})
			: 3 Xe<sub>(g)</sub> + {{chem|XeF|+}}<sub>(apf)</sub> + {{chem|SbF|5}}<sub>(l)</sub> {{eqm}} 2&nbsp;{{chem|Xe|2|+}}<sub>(apf)</sub> + {{chem|SbF|6|−}}<sub>(apf)</sub>
			This reaction is reversible; removing xenon gas from the solution causes the {{chem|Xe|2|+}} ion to revert to xenon gas and {{chem|XeF|+}}, and the color of the solution returns to a pale yellow.<ref>{{Cite journal| first1 = L. | first2 = W. W.| title = Production of dixenon cation by reversible oxidation of xenon| last1 = Stein| journal = Journal of the American Chemical Society| volume = 102| issue = 8| pages = 2856–2857| year = 1980| doi = 10.1021/ja00528a065| last2 = Henderson| bibcode = 1980JAChS.102.2856S}}</ref>
			In the presence of liquid ], dark green crystals can be precipitated from the green solution at −30&nbsp;°C:
			: {{chem|Xe|2|+}}<sub>(apf)</sub> + 4&nbsp;{{chem|SbF|6|−}}<sub>(apf)</sub> → {{chem|Xe|2|+|Sb|4|F|21|−}}<sub>(s)</sub> + 3&nbsp;{{chem|F|−}}<sub>(apf)</sub>
			] indicates that the Xe–Xe bond length in this compound is 309&nbsp;], indicating a very weak bond.<ref name="harding" /> The {{chem|Xe|2|+}} ion is ] with the {{chem|I|2|−}} ion, which is also dark green.<ref>{{cite book
			| title = Introduction to modern inorganic chemistry
			| first1 = Kenneth Malcolm | last1 = Mackay
			| first2 = Rosemary Ann| last2 = Mackay
			| first3 = W.| last3 = Henderson
			| edition = 6th
			| publisher = CRC Press
			| year = 2002
			| isbn = 978-0-7487-6420-4
			}}</ref><ref>{{cite book
			| title = Inorganic chemistry
			| author1 = Egon Wiberg
			| author2 = Nils Wiberg
			| author3 = Arnold Frederick Holleman
			| publisher = Academic Press
			| year = 2001
			| isbn = 978-0-12-352651-9
			| page = 422
			}}</ref>
			===Coordination chemistry===
			Bonding in the XeF<sub>2</sub> molecule is adequately described by the ] model.
			XeF<sub>2</sub> can act as a ] in ] of metals.<ref name="tramsek" /> For example, in HF solution:
			:Mg(AsF<sub>6</sub>)<sub>2</sub> + 4&nbsp;XeF<sub>2</sub> → (AsF<sub>6</sub>)<sub>2</sub>
			Crystallographic analysis shows that the magnesium atom is coordinated to 6 fluorine atoms. Four of the fluorine atoms are attributed to the four xenon difluoride ligands while the other two are a pair of ''cis''-{{chem|AsF|6|-}} ligands.<ref>{{cite journal | doi = 10.1021/ic034826o |pmid=14731032 |author1=Tramšek, M. |author2=Benkič, P. |author3=Žemva, B. | journal = ] | volume = 43 | issue = 2 | pages = 699–703 | year = 2004 | title = First Compounds of Magnesium with XeF<sub>2</sub>}}</ref>
			A similar reaction is:
			:Mg(AsF<sub>6</sub>)<sub>2</sub> + 2&nbsp;XeF<sub>2</sub> → (AsF<sub>6</sub>)<sub>2</sub>
			In the crystal structure of this product the magnesium atom is ] and the XeF<sub>2</sub> ligands are axial while the {{chem|AsF|6|-}} ligands are equatorial.
			Many such reactions with products of the form (AF<sub>6</sub>)<sub>''x''</sub> have been observed, where M can be ], ], ], ], ], ], or ] and A can be ], ] or ]. Some of these compounds feature extraordinarily high ]s at the metal center.<ref>{{cite journal|via=]|page=1640|journal=Chemical Society Reviews|volume=36|issue=10|date=Oct 2007|title=Atypical compounds of gases, which have been called 'noble'|first=Wojciech|last=Grochala|orig-date=12 April 2007|doi=10.1039/b702109g|publisher=Royal Society of Chemistry|pmid=17721587}}</ref>
			In 2004, results of synthesis of a solvate where part of cationic centers were coordinated solely by XeF<sub>2</sub> fluorine atoms were published.<ref>{{cite journal | doi = 10.1002/anie.200453802 |pmid=15221838 |author1=Tramšek, M. |author2=Benkič, P. |author3=Žemva, B. | journal = ] | volume = 43 | issue = 26 | pages = 3456–8 | year = 2004 | title = The First Compound Containing a Metal Center in a Homoleptic Environment of XeF<sub>2</sub> Molecules| doi-access = free }}</ref> Reaction can be written as:
			:2&nbsp;Ca(AsF<sub>6</sub>)<sub>2</sub> + 9&nbsp;XeF<sub>2</sub> → Ca<sub>2</sub>(XeF<sub>2</sub>)<sub>9</sub>(AsF<sub>6</sub>)<sub>4</sub>.
			This reaction requires a large excess of xenon difluoride. The structure of the salt is such that half of the Ca<sup>2+</sup> ions are coordinated by fluorine atoms from xenon difluoride, while the other Ca<sup>2+</sup> ions are coordinated by both XeF<sub>2</sub> and {{chem|AsF|6|-}}.
			==Applications==
			===As a fluorinating agent===
			Xenon difluoride is a strong fluorinating and oxidizing agent.<ref>{{cite book|first=D. F.|last= Halpem |contribution=Xenon(II) Fluoride |title=Encyclopedia of Reagents for Organic Synthesis |editor-first=L. |editor-last=Paquette |date=2004 |publisher=J. Wiley & Sons |location=New York, NY}}</ref><ref>{{cite journal| title = Recent Advances in Electrophilic Fluorination|author1=Taylor, S. |author2= Kotoris, C. |author3=Hum, G. | journal = Tetrahedron| volume = 55| issue = 43| pages = 12431–12477| year = 1999| doi = 10.1016/S0040-4020(99)00748-6 }}</ref> With fluoride ion acceptors, it forms {{chem|XeF|+}} and {{chem|Xe|2|F|3|+}} species which are even more powerful fluorinators.<ref name="tramsek" />
			Among the fluorination reactions that xenon difluoride undergoes are:
			* ''Oxidative fluorination'':
			::Ph<sub>3</sub>TeF + XeF<sub>2</sub> → Ph<sub>3</sub>TeF<sub>3</sub> + Xe
			* ''Reductive fluorination'':
			::2&nbsp;CrO<sub>2</sub>F<sub>2</sub> + XeF<sub>2</sub> → 2&nbsp;CrOF<sub>3</sub> + Xe +O<sub>2</sub>
			* ''Aromatic fluorination'':
			::]
			::]
			* ''Alkene fluorination'':
			::]
			* '']'' in radical decarboxylative fluorination reactions,<ref name=SynthApps>{{Cite journal|title = Xenon difluoride in synthesis|journal = Tetrahedron|year = 1995|pages = 6605–6634|volume = 51|issue = 24|doi = 10.1016/0040-4020(95)00362-C|first = M. A.|last = Tius}}</ref> in ] where xenon difluoride is used to generate the radical intermediate as well as the fluorine transfer source,<ref>{{Cite journal|title = Fluorination of activated aromatic systems with cesium fluoroxysulfate|journal = J. Org. Chem.|year = 1986|pages = 3242–3244|volume = 51|issue = 16|doi = 10.1021/jo00366a044|first1 = T. B.|last1 = Patrick|first2 = D. L.|last2 = Darling}}</ref> and in generating aryl radicals from aryl silanes:<ref>{{Cite journal|title = Rapid fluorodesilylation of aryltrimethylsilanes using xenon difuoride: An efficient new route to aromatic fluorides|journal = Synlett|year = 1993|pages = 753–755|volume = 1993|issue = 10|doi = 10.1055/s-1993-22596|first1 = A. P.|last1 = Lothian|first2 = C. A.|last2 = Ramsden| s2cid=196734038 }}</ref>
			::]
			::]
			{{chem|XeF|2}} is selective about which atom it fluorinates, making it a useful reagent for fluorinating heteroatoms without touching other substituents in organic compounds. For example, it fluorinates the arsenic atom in ], but leaves the ]s untouched:<ref>{{cite book
			| title = Main group chemistry
			| url = https://archive.org/details/maingroupchemist00hend_891
			| url-access = limited
			| author = W. Henderson
			| location = Great Britain
			| publisher = Royal Society of Chemistry
			| year = 2000
			| isbn = 978-0-85404-617-1
			| page =
			}}</ref>
			:{{chem|(CH|3|)|3|As}} + {{chem|XeF|2}} → {{chem|(CH|3|)|3|AsF|2}} + Xe
			XeF<sub>2</sub> can similarly be used to prepare ''N''-fluoroammonium salts, useful as fluorine transfer reagents in organic synthesis (e.g., ]), from the corresponding tertiary amine:<ref>{{Cite journal|last1=Shunatona|first1=Hunter P.|last2=Früh|first2=Natalja|last3=Wang|first3=Yi-Ming|last4=Rauniyar|first4=Vivek|last5=Toste|first5=F. Dean|date=2013-07-22|title=Enantioselective Fluoroamination: 1,4-Addition to Conjugated Dienes Using Anionic Phase-Transfer Catalysis|journal=Angewandte Chemie International Edition|language=en|volume=52|issue=30|pages=7724–7727|doi=10.1002/anie.201302002|pmid=23766145|issn=1521-3773|doi-access=free}}</ref>
			: + XeF<sub>2</sub> + NaBF<sub>4</sub> → <sub>2</sub> + NaF + Xe
			{{chem|XeF|2}} will also oxidatively decarboxylate ]s to the corresponding ]:<ref>{{cite journal | doi = 10.1139/v86-024 | last1 = Patrick | first1 = Timothy B. | last2 = Johri | first2 = Kamalesh K. | last3 = White | first3 = David H. | last4 = Bertrand | first4 = William S. | last5 = Mokhtar | first5 = Rodziah | last6 = Kilbourn | first6 = Michael R. | last7 = Welch | first7 = Michael J. | title = Replacement of the carboxylic acid function with fluorine | journal = ] | year = 1986 | volume = 64 | pages = 138–141}}</ref><ref>{{cite journal | doi = 10.1021/jo01260a040 | last1 = Grakauskas | first1 = Vytautas | title = Aqueous fluorination of carboxylic acid salts | journal = ] | year = 1969 | volume = 34 | issue = 8 | pages = 2446–2450}}</ref>
			:RCOOH + XeF<sub>2</sub> → RF + CO<sub>2</sub> + Xe + HF
			] has been found to act as a catalyst in fluorination by {{chem|XeF|2}}.<ref>{{cite journal
			| journal = Fusso Kagaku Toronkai Koen Yoshishu
			| id = Journal code: F0135B; accession code: 99A0711841
			| author = Tamura Masanori
			| author2 = Takagi Toshiyuki
			| author3 = Shibakami Motonari
			| author4 = Quan Heng-Dao
			| author5 = Sekiya Akira
			| title = Fluorination of olefins with xenon difluoride-silicon tetrafluoride
			| volume = 22
			| year = 1998
			| pages = 62–63
			| language = ja
			}}</ref>
			===As an etchant===
			Xenon difluoride is also used as an isotropic gaseous ] for ], particularly in the production of ] (MEMS), as first demonstrated in 1995.<ref>{{cite book|last1=Chang |first1=F. |last2=Yeh |first2=R. |first3=Lin |last3=G. |last4=Chu |first4=P. |last5=Hoffman |first5=E. |last6=Kruglick |first6=E. |last7=Pister |first7=K. |last8=Hecht |first8=M. |chapter=Gas-phase silicon micromachining with xenon difluoride |editor1-first=Wayne |editor1-last=Bailey |editor2-first=M. Edward |editor2-last=Motamedi |editor3-first=Fang-Chen |editor3-last=Luo |doi=10.1117/12.220933 |title=Microelectronic Structures and Microelectromechanical Devices for Optical Processing and Multimedia Applications |journal=SPIE Proc. |volume=2641 |date=1995 |pages=117–128|bibcode=1995SPIE.2641..117C |s2cid=39522253 }}</ref> Commercial systems use pulse etching with an expansion chamber<ref>{{cite conference|last1=Chu |first1=P. |last2=Chen |first2=J. |last3=Chu |first3=P. |last4=Lin |first4=G. |last5=Huang |first5=J. |last6=Warneke |first6=B |last7=Pister |first7=K. |title=Controlled Pulse-Etching with Xenon Difluoride |conference=Int. Conf. Solid State Sensors and Actuators (Transducers 97) |date=1997 |pages=665–668}}</ref>
			Brazzle, Dokmeci, et al. describe this process:<ref>{{cite conference|last1=Brazzle |first1=J. D. |last2=Dokmeci |first2=M. R. |last3=Mastrangelo |first3=C. H. |title=17th IEEE International Conference on Micro Electro Mechanical Systems. Maastricht MEMS 2004 Technical Digest |doi=10.1109/MEMS.2004.1290690 |chapter=Modeling and characterization of sacrificial polysilicon etching using vapor-phase xenon difluoride |conference=17th IEEE International Conference on Micro Electro Mechanical Systems (MEMS) |date=2004 |pages=737–740|isbn=0-7803-8265-X }}</ref>
			The mechanism of the etch is as follows. First, the XeF<sub>2</sub> adsorbs and dissociates to xenon and fluorine atoms on the surface of silicon. Fluorine is the main etchant in the silicon etching process. The reaction describing the silicon with XeF<sub>2</sub> is
			:2&nbsp;XeF<sub>2</sub> + Si → 2&nbsp;Xe + SiF<sub>4</sub>
			XeF<sub>2</sub> has a relatively high etch rate and does not require ] or external energy sources in order to etch silicon.
			==References==
			{{reflist|30em}}
			==Further reading==
			*{{cite book
			| last1 = Greenwood
			| first1 = Norman Neill
			| last2 = Earnshaw
			| first2 = Alan
			| title = Chemistry of the Elements
			| url = https://archive.org/details/chemistryelement00earn_612
			| url-access = limited
			| edition = 2nd
			| year = 1997
			| page =
			| publisher = Butterworth-Heinemann
			| isbn = 978-0-7506-3365-9
			}}
			==External links==
			*
			{{Xenon compounds}}
			{{Noble gas compounds}}
			{{fluorine compounds}}
			]
			]
			]
			]