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| Names | |||
|---|---|---|---|
| IUPAC name
Thionyl fluoride
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| Identifiers | |||
3D model (JSmol)
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| ChemSpider | |||
| ECHA InfoCard | 100.029.088 | ||
| EC Number |
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PubChem CID
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| UNII | |||
CompTox Dashboard (EPA)
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| Properties | |||
| F2OS | |||
| Molar mass | 86.06 g·mol−1 | ||
| Appearance | colorless gas | ||
| Melting point | −110.5 °C (−166.9 °F; 162.7 K) | ||
| Boiling point | −43.8 °C (−46.8 °F; 229.3 K) | ||
| hydrolysis | |||
| Solubility | soluble in ethanol, ether, benzene | ||
| Vapor pressure | 75.7 kPa (-50 °C)[1] | ||
| Structure | |||
| trigonal pyramidal | |||
| Thermochemistry | |||
Std molar
entropy (S⦵298) |
278.6 J/mol·K[2] | ||
Std enthalpy of
formation (ΔfH⦵298) |
-715 kJ/mol[2] | ||
Std enthalpy of
combustion (ΔcH⦵298) |
56.8 J/mol·K[2] | ||
| Hazards | |||
| GHS labelling: | |||
 
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| Danger | |||
| H300, H310, H314, H330 | |||
| P260, P262, P264, P270, P271, P280, P284, P301+P310, P301+P330+P331, P302+P350, P303+P361+P353, P304+P340, P305+P351+P338, P310, P320, P321, P322, P330, P361, P363, P403+P233, P405, P501 | |||
| Related compounds | |||
Related oxohalides
|
Thionyl chloride Thionyl bromide | ||
Related compounds
|
Nitrosyl fluoride Carbonyl fluoride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Thionyl fluoride is the inorganic compound with the formula SOF
2. 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. Thionyl chloride and thionyl bromide have similar structures, although these compounds are liquid at room temperature. Mixed halides are also known, such as SOClF, thionyl chloride fluoride.[3]
YouTube Encyclopedic
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1/3Views:51 41018 591312
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Make a Lithium Thionyl Chloride Battery
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Is ClF3 Polar or Nonpolar ?
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Sodium iodide
Transcription
Greetings fellow nerds In this video we're going to make a simple and crude lithium thionyl chloride battery. These are not rechargeable but have a very long shelf life. To do this, we first need a saturated solution of Thionyl chloride and lithium tetrachloroaluminate. Thionyl chloride is extremely toxic and must be handled inside a fumehood. Here we have a rod of the lithium metal itself to serve as one electrode. And this carbon rod serves as the counter electrode. Alright, let's first measure the voltage of this battery. The lithium metal is the negative electrode, the thionyl chloride solution is the electrolyte and the carbon rod is the positive electrode. We need to give it a few moments to stabilize here. And it looks the like the voltage is around 2.8 volts. It's not very stable and it should be closer to 3.5 volts but this solution of thionyl chloride is very impure resulting in these poor readings. Nonetheless, we can still make a useful battery out of this. In this case, we're going to power this green light emitting diode. First, the negative end of the diode is pushed into the lithium rod. Lithium is actually a very soft and this is as easy as pushing a pin through clay. Second the other pin of the diode is wrapped around the carbon rod to make a connection. Now the assembly is dropped into the thionyl chloride solution. Let me get the lights. As you can see, this is generating enough power to light this diode. Here's a close up of the entire assembly. Thanks for watching please subscribe, rate and comment.
Synthesis and reactions
Thionyl fluoride can be produced by the reaction of thionyl chloride with fluoride sources such as antimony trifluoride.[4][5]
Alternatively, it arises via the fluorination of sulfur dioxide:[5]
- 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.[6]
As expected from the behavior of the other thionyl halides, this compound hydrolyzes readily, giving hydrogen fluoride and sulfur dioxide:[5]
- 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.
References
- ^ Thionyl fluoride in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2014-05-11)
- ^ a b c "Thionyl fluoride".
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ W. C. Smith, E. L. Muetterties "Thionyl Fluoride" Inorganic Syntheses 1960, Volume 6, pages: 162-163. doi:10.1002/9780470132371.ch50
- ^ a b c Holleman, Arnold F. (2001). Inorganic Chemistry. Academic Press. p. 542. ISBN 978-0-12-352651-9. Retrieved 2008-07-29.
- ^ Pepi, Federico; Andreina Ricci; Marco Di Stefano; Marzio Rosi; Giuseppe D'Arcangelo (September 18, 2002). "Thionyl Fluoride from Sulfur Hexafluoride Corona Discharge Decomposition: Gas-Phase Chemistry of (SOF2)H+ Ions". Journal of Physical Chemistry A. 106 (40): 9261–9266. Bibcode:2002JPCA..106.9261P. doi:10.1021/jp021074v.
External links
This page was last edited on 29 January 2023, at 12:39