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	{{chembox		{{chembox
			| Verifiedfields = changed
⚫	| verifiedrevid = 413816549
			| Watchedfields = changed
		⚫	| verifiedrevid = 442429986
	| Name =		| Name =
	| ImageFileL1 = Sulfur oxytetrafluoride.png		| ImageFile = Sulfur oxytetrafluoride.png
			| ImageName = Structure of thionyl tetrafluoride
	| ImageSizeL1 = 115px
	| ImageNameL1 = Structure of thionyl tetrafluoride		| ImageFileL1 = Thionyl-tetrafluoride-3D-balls.png
			| ImageNameL1 = Ball-and-stick model of thionyl tetrafluoride
	| ImageFileR1 = Thionyl-tetrafluoride-3D-balls.png		| ImageFileR1 = Thionyl-tetrafluoride-3D-SF.png
	| ImageSizeR1 = 125px
	| ImageNameR1 = Ball-and-stick model of thionyl tetrafluoride		| ImageNameR1 = Space-filling model of thionyl tetrafluoride
	| IUPACName = Thionyl tetrafluoride		| IUPACName = Thionyl tetrafluoride
	| SystematicName =		| SystematicName =
	| OtherNames =		| OtherNames =
	| Section1 = {{Chembox Identifiers		|Section1={{Chembox Identifiers
	| Abbreviations =		| Abbreviations =
			| CASNo_Ref = {{cascite|correct|??}}
	| CASNo = 13709-54-1		| CASNo = 13709-54-1
	| EINECS =		| EINECS =
	| EINECSCASNO =		| PubChem = 139557
			| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| PubChem =
	| SMILES =		| ChemSpiderID = 123077
			| SMILES = O=S(F)(F)(F)F
	| InChI =
			| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
			| StdInChI = 1S/F4OS/c1-6(2,3,4)5
			| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
			| StdInChIKey = DUGWRBKBGKTKOX-UHFFFAOYSA-N
	| RTECS =		| RTECS =
	| MeSHName =		| MeSHName =
			| ChEBI_Ref = {{ebicite|correct|EBI}}
	| ChEBI =		| ChEBI =
	| KEGG_Ref = {{keggcite|correct|kegg}}		| KEGG_Ref = {{keggcite|correct|kegg}}
	| KEGG =		| KEGG =
			}}
	| ATCCode_prefix =
		⚫	|Section2={{Chembox Properties
	| ATCCode_suffix =
	| ATC_Supplemental =}}
⚫	| Section2 = {{Chembox Properties
	| Formula = SOF<sub>4</sub>		| Formula = SOF<sub>4</sub>
	| MolarMass =		| MolarMass =
	| Appearance = colorless gas		| Appearance = colorless gas
	| Density = 1.653-0.0036T (°C) liquid<ref name=aiic/>		| Density = 1.653−0.0036T (°C) liquid<ref name=aiic/>
	| MeltingPt = -99.6°C		| MeltingPtC = −99.6
	| Melting_notes =		| MeltingPt_notes =
	| BoilingPt = -49°C		| BoilingPtC = −49
	| Boiling_notes = 5090 cal/mol heat of vapourisation<ref name=aiic/>		| BoilingPt_notes = 5090 cal/mol heat of vapourisation<ref name=aiic/>
	| Solubility =		| Solubility = reaction in water
	| SolubleOther =		| SolubleOther =
	| Solvent = ether, benzene		| Solvent = ether, benzene
	| LogP = 7.2349-859.58/T-26275/T²<ref name=aiic/>		| LogP = 7.2349−859.58/T−26275/T²<ref name=aiic/>
	| VaporPressure =		| VaporPressure =
	| HenryConstant =		| HenryConstant =
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	| pKa =		| pKa =
	| pKb = }}		| pKb = }}
	| Section3 = {{Chembox Structure		|Section3={{Chembox Structure
	| CrystalStruct =		| CrystalStruct =
	| Coordination =		| Coordination =
	| MolShape = distorted trigonal bipyramid}}		| MolShape = distorted trigonal bipyramid}}
	| Section4 = {{Chembox Thermochemistry		|Section7={{Chembox Hazards
	| DeltaHf =		| ExternalSDS =
	| DeltaHc =
	| Entropy =
	| HeatCapacity = }}
	| Section5 = {{Chembox Pharmacology
	| AdminRoutes =
	| Bioavail =
	| Metabolism =
	| HalfLife =
	| ProteinBound =
	| Excretion =
	| Legal_status =
	| Legal_US =
	| Legal_UK =
	| Legal_AU =
	| Legal_CA =
	| PregCat =
	| PregCat_AU =
	| PregCat_US = }}
	| Section6 = {{Chembox Explosive
	| ShockSens =
	| FrictionSens =
	| ExplosiveV =
	| REFactor = }}
	| Section7 = {{Chembox Hazards
	| ExternalMSDS =
	| EUClass =
	| EUIndex =
	| MainHazards =		| MainHazards =
	| NFPA-H =		| NFPA-H =
	| NFPA-F =		| NFPA-F =
	| NFPA-R =		| NFPA-R =
	| NFPA-O =		| NFPA-S =
			| GHSPictograms = {{GHS05}}{{GHS06}}
	| RPhrases = {{R36/37/38}}<ref name="ox">
			| GHSSignalWord = Danger
	{{cite web |url= http://msds.chem.ox.ac.uk/TH/thionyl_tetraluoride.html |title= Safety (MSDS) data for thionyl tetrafluoride
			| HPhrases = {{H-phrases|300|310|314|330}}
	| accessdate=2008-07-29 |publisher= Oxford University |date=2005-09-02 }}
			| PPhrases = {{P-phrases|260|262|264|270|271|280|284|301+310|301+330+331|302+350|303+361+353|304+340|305+351+338|310|320|321|322|330|361|363|403+233|405|501}}
	</ref>
	| SPhrases =		| GHS_ref =
	| RSPhrases =
	| FlashPt =		| FlashPt =
	| Autoignition =		| AutoignitionPt =
	| ExploLimits =		| ExploLimits =
	| LD50 =		| LD50 =
	| PEL = }}		| PEL = }}
	| Section8 = {{Chembox Related		|Section8={{Chembox Related
	| OtherAnions =		| OtherAnions =
	| OtherCations =		| OtherCations =
	| OtherFunctn = ]<br>]		| OtherFunction = ]<br>]
	| Function = oxohalides		| OtherFunction_label = oxohalides
	| OtherCpds = ]<br>]<br>]}}		| OtherCompounds = ]<br>]<br>]}}
	}}		}}
			'''Thionyl tetrafluoride''', also known as '''sulfur tetrafluoride oxide''', is an ] with the ] {{chem2|SOF4|auto=1}}. It is a colorless ].
⚫	'''Thionyl tetrafluoride''' is an ] gas with the ] ]]]<sub>4</sub>. It is also known as '''sulfur tetrafluoride oxide'''. The shape of the molecule is a distorted trigonal bipyramid. The oxygen is found on the equator. The atoms on the equator have shorter bond lengths than the fluorine atoms on the axis. The sulfur oxygen bond is 1.409Å. A S-F bond on the axis has length 1.596Å and the S-F bond on the equator has length 1.539Å. The angle between the equatorial fluorine atoms is 112.8°. The angle between axial fluorine and oxygen is 97.7°. The angle between oxygen and equatorial fluorine is 123.6° and between axial and equatorial fluorine is 85.7°.<ref>Lise Hedberg and Kenneth Hedberg "Thionyl tetrafluoride. Reanalysis of the molecular structure and resolution of the multiple model problem" ''the Journal of Physical Chemistry'' March 1982 vol 86 page 598 doi 10.1021/j100394a004 </ref> The fluorine atoms only produce one ] line, probably because they ].<ref name=aiic/>
		⚫	The shape of the molecule is a distorted trigonal bipyramid, with the oxygen found on the equator. The atoms on the equator have shorter bond lengths than the fluorine atoms on the axis. The sulfur oxygen bond is 1.409Å. A S−F bond on the axis has length 1.596Å and the S−F bond on the equator has length 1.539Å. The angle between the equatorial fluorine atoms is 112.8°. The angle between axial fluorine and oxygen is 97.7°. The angle between oxygen and equatorial fluorine is 123.6° and between axial and equatorial fluorine is 85.7°.<ref>{{cite journal |last1=Hedberg |first1=Lise |last2=Hedberg |first2=Kenneth |title=Thionyl tetrafluoride. Reanalysis of the molecular structure and resolution of the multiple model problem |journal=The Journal of Physical Chemistry |date=March 1982 |volume=86 |issue=5 |pages=598–602 |doi=10.1021/j100394a004}}</ref> The fluorine atoms only produce one ] line, probably because they ].<ref name=aiic/> It is isoelectronic with ].
	==Formation==		==Formation==
	] reacting with ] gas can produce thionyl tetrafluoride.<ref name=aiic>] and A.G. Sharpe ''Advances in Inorganic Chemistry Volume 2'' Academic Press 1960 page 117 </ref> This was how the gas was first discovered by Moissan and Lebeau in 1902. They identified the formula by the pressure changes resulting from the reaction. ] and ] are capable of catalyzing the reaction.		] reacting with ] gas can produce thionyl tetrafluoride.<ref name="aiic">] and A.G. Sharpe ''Advances in Inorganic Chemistry Volume 2'' Academic Press 1960 page 117 </ref> This was how the gas was first discovered by Moissan and Lebeau in 1902. They identified the formula by the pressure changes resulting from the reaction. ] and ] are capable of catalyzing the reaction.
	It can also be formed by heating ] with air to 400°.<ref>{{cite web|url=http://www.sayedsaad.com/substation/sf6_gas_properties.htm|title=SF6 Gas Properties}}</ref> This can happen when inhaling through a lit cigarette. Or the reaction of ] with thionyl fluoride at 200 degrees.<ref>http://pubs.acs.org/doi/abs/10.1021/ja01589a013</ref> Another way to form it is by electrolyzing ] with a solution of ], which also made ] and ].<ref>Shunji Nagase Fluorination of Inorganic Sulfur Compounds ''Bulletin of the Chemical Society of Japan'' vol 42 page 2062 1968</ref> Also ] or ] electrolyzed with hydrogen fluoride produced even more of the gas.		It can also be formed the reaction of ] with ] at {{convert|200|C|F|order=flip}},<ref>{{cite journal|doi=10.1021/ja01589a013 | volume=78 | issue=8 | title=Pentafluorosulfur Hypofluorite and Thionyl Tetrafluoride | journal=Journal of the American Chemical Society | pages=1553–1557 | last1 = Dudley | first1 = F. B.| year=1956 }}</ref> or by electrolyzing ] with a solution of ], which also made ] and ]. ] or thionyl fluoride electrolyzed with hydrogen fluoride produced even more of the gas.<ref>{{cite journal |last1=Nagase |first1=Shunji |last2=Abe |first2=Takashi |last3=Baba |first3=Hajime |title=Fluorination of Inorganic Sulfur Compounds |journal=Bulletin of the Chemical Society of Japan |date=1 July 1969 |volume=42 |issue=7 |pages=2062–2064 |doi=10.1246/bcsj.42.2062}}</ref>
	==Reactions==		==Reactions==
	Thionyl tetrafluoride reacts with water to make ], ], and ]. Mercury can strip off fluoride to make thionyl fluoride and ]. Strong bases result in formation of fluoride and fluorosulfate ions.<ref name=aiic/>		Thionyl tetrafluoride reacts with water to make ], ], and ]. Mercury can strip off fluoride to make thionyl fluoride and ]. Strong bases result in formation of fluoride and ] ions.<ref name=aiic/>
			Reactions with the strong Lewis acids, such as ] and ], result in the formation SOF<sub>3</sub><sup>+</sup> cation and the corresponding salts SOF<sub>3</sub> and SOF<sub>3</sub>, respectively.<ref>{{Cite journal |last=Brownstein |first=M. |last2=Dean |first2=P. A. W. |last3=Gillespie |first3=R. J. |date=1970-01-01 |title=The trifluorosulphur(VI) oxide cation, SOF3+ |url=https://pubs.rsc.org/en/content/articlelanding/1970/c2/c29700000009 |journal=Journal of the Chemical Society D: Chemical Communications |language=en |issue=1 |pages=9–9 |doi=10.1039/C29700000009 |issn=0577-6171}}</ref>
			=== Click chemistry ===
			Thionyl tetrafluoride can be used in ] through reactions with primary amines known as sulfur(VI) fluoride exchange (SuFEx).<ref>{{Cite journal|last1=Li|first1=Suhua|last2=Wu|first2=Peng|last3=Moses|first3=John E.|last4=Sharpless|first4=K. Barry|date=2017-02-01|title=Multidimensional SuFEx Click Chemistry: Sequential Sulfur(VI) Fluoride Exchange Connections of Diverse Modules Launched From An SOF4 Hub|journal=Angewandte Chemie International Edition|language=en|pages=2903–2908|doi=10.1002/anie.201611048|pmid=28165188|pmc=5434761|issn=1521-3773|volume=56|issue=11}}</ref> This kind of reaction was the first "click" reaction to generate a three-dimensional core.
	==References==		==References==
	<references/>		<references/>
			{{Sulfur compounds}}
	*http://www.freepatentsonline.com/2946661.html
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