Thionyl fluoride
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| verifiedrevid = 464361711
| Name =
| ImageFileR1 = Thionyl-fluoride-3D-balls.png
| ImageSizeR1 =
| ImageNameR1 = structure
| ImageFileL1 = SOF2.png
| ImageSizeL1 = 150px
| ImageNameL1 = Ball-and-stick model
| IUPACName = Thionyl fluoride
| SystematicName =
| OtherNames =
|Section1={{Chembox Identifiers
| Abbreviations =
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 22954
| InChI = 1/F2OS/c1-4(2)3
| InChIKey = LSJNBGSOIVSBBR-UHFFFAOYAL
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/F2OS/c1-4(2)3
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = LSJNBGSOIVSBBR-UHFFFAOYSA-N
| CASNo_Ref = {{cascite|changed|??}}
| CASNo = 7783-42-8
| EC_number = 231-997-2
| PubChem = 24548
| SMILES = FS(F)=O
| RTECS =
| MeSHName =
| ChEBI_Ref = {{ebicite|correct|EBI}}
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| KEGG_Ref = {{keggcite|correct|kegg}}
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| UNII = 2O8P7K5BE8
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|Section2={{Chembox Properties
| Formula = {{chem2|SOF2}}
| S=1 | O=1 | F=2
| Appearance = colorless gas
| Density =
| MeltingPtC = -110.5
| MeltingPt_notes =
| BoilingPtC = -43.8
| BoilingPt_notes =
| Solubility = hydrolysis
| SolubleOther = soluble in ethanol, ether, benzene
| Solvent =
| LogP =
| VaporPressure = 75.7 kPa (-50 °C){{nist|name=Thionyl fluoride|id=C7783428|accessdate=2014-05-11|mask=FFFF|units=SI}}
| HenryConstant =
| AtmosphericOHRateConstant =
| pKa =
| pKb =
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|Section3={{Chembox Structure
| CrystalStruct =
| Coordination =
| MolShape = trigonal pyramidal
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|Section4={{Chembox Thermochemistry
| Thermochemistry_ref = {{cite web |title=Thionyl Fluoride |url=http://chemister.ru/Databases/Chemdatabase/properties-en.php?dbid=1&id=8280 |website=chemister.ru database}}{{better citation needed|date=September 2024}}
| DeltaHf = −715 kJ/mol
| DeltaHc = 56.8 J/(mol·K)
| Entropy = 278.6 J/(mol·K)
| HeatCapacity =
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|Section5={{Chembox Pharmacology
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|Section6={{Chembox Explosive
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|Section7={{Chembox Hazards
| ExternalSDS =
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| GHSPictograms = {{GHS05}}{{GHS06}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|300|310|314|330}}
| 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}}
| FlashPt =
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| PEL = }}
|Section8={{Chembox Related
| OtherAnions =
| OtherCations =
| OtherFunction = Thionyl chloride
Thionyl bromide
| OtherFunction_label = oxohalides
| OtherCompounds = Thiothionyl fluoride
Nitrosyl fluoride
Carbonyl fluoride}}
}}
Thionyl fluoride is the inorganic compound with the formula {{chem2|SOF2|auto=1}}. This colourless gas is mainly of theoretical interest, but it is a product of the degradation of sulfur hexafluoride, an insulator in electrical equipment. The molecule adopts a distorted pyramidal structure, with Cs symmetry. The S-O and S-F distances are 1.42 and 1.58 Å, respectively. The O-S-F and F-S-F angles are 106.2 and 92.2°, respectively.{{cite book |last=Holleman |first=A.F.|editor-last1=Holleman |editor-first1=A.F. |editor-last2=Wiberg |editor-first2=Egon |editor-last3=Wiberg |editor-first3=Nils
|title=Inorganic Chemistry |date=2001 |edition=1st |publisher=Academic Press|location=San Diego, CA|isbn=0-12-352651-5}}{{page needed|date=September 2024}}
Synthesis and reactions
Thionyl fluoride can be produced by the reaction of thionyl chloride with fluoride sources such as antimony trifluoride.{{cite book |last1=Smith |first1=W. C. |last2=Muetterties |first2=E. L. |last3=Park |first3=J. D. |last4=Settine |first4=Robert |title=Inorganic Syntheses |chapter=Thionyl Fluoride |date=January 1960 |volume=6 |pages=162–163 |doi=10.1002/9780470132371.ch50|isbn=978-0-470-13165-7}}{{rp|542}}
:{{chem2|3 SOCl2 + 2 SbF3 -> 3 SOF2 + 2 SbCl3}}
Alternatively, it arises via the fluorination of sulfur dioxide:{{rp|542}}
:{{chem2|SO2 + PF5 -> SOF2 + POF3}}
Thionyl fluoride arises as a fleeting intermediate from the decomposition of sulfur hexafluoride as the result of electrical discharges which generate sulfur tetrafluoride. SF4 hydrolyzes to give thionyl fluoride, which in turn hydrolyzes further as described below.{{cite journal| last = Pepi| first = Federico | author2=Andreina Ricci |author3=Marco Di Stefano |author4=Marzio Rosi |author5=Giuseppe D'Arcangelo | date = September 18, 2002| title = Thionyl Fluoride from Sulfur Hexafluoride Corona Discharge Decomposition: Gas-Phase Chemistry of (SOF2)H+ Ions| journal = Journal of Physical Chemistry A| volume = 106| issue = 40| pages = 9261–9266| doi = 10.1021/jp021074v| bibcode =2002JPCA..106.9261P}}
As expected from the behavior of the other thionyl halides, this compound hydrolyzes readily, giving hydrogen fluoride and sulfur dioxide:{{rp|542}}
:{{chem2|SOF2 + H2O -> 2 HF + SO2}}
In contrast to thionyl chloride and bromide, thionyl fluoride is not useful for halogenation. The related derivative, sulfur tetrafluoride is however useful for that purpose.{{Citation needed|date=September 2024}}
References
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External links
{{Commons category|Thionyl fluoride}}
{{sulfur compounds}}
{{fluorine compounds}}