Chemistry:Diethylaminosulfur trifluoride
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| Names | |||
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| Preferred IUPAC name
N,N-Diethyl-S,S,S-trifluoro-λ4-sulfanamine | |||
| Other names
diethyl(trifluorosulfido)amine
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| Identifiers | |||
3D model (JSmol)
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| Abbreviations | DAST | ||
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PubChem CID
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| Properties | |||
| C4H10F3NS | |||
| Molar mass | 161.19 g·mol−1 | ||
| Appearance | colourless oil | ||
| Density | 1.220 g/cm3 | ||
| Boiling point | 30 to 32 °C (86 to 90 °F; 303 to 305 K) at 3 mmHg | ||
| Reacts with water | |||
| Solubility | reacts with ethanol soluble[vague] in acetonitrile | ||
| Hazards | |||
| Main hazards | corrosive, flammable, can be explosive | ||
| GHS pictograms |   
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| GHS Signal word | Danger | ||
| H226, H302, H312, H314, H332 | |||
| P210, P233, P240, P241, P242, P243, P260, P261, P264, P270, P271, P280, P301+312, P301+330+331, P302+352, P303+361+353, P304+312, P304+340, P305+351+338, P310, P312, P321, P322, P330, P363 | |||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
 verify (what is   ?)
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| Infobox references | |||
Diethylaminosulfur trifluoride (DAST)[2] is the organosulfur compound with the formula Et2NSF3. This liquid is a fluorinating reagent used for the synthesis of organofluorine compounds. The compound is colourless; older samples assume an orange colour.
Use in organic synthesis
DAST converts alcohols to the corresponding alkyl fluorides as well as aldehydes and unhindered ketones to geminal difluorides. Carboxylic acids react no further than the acyl fluoride (sulfur tetrafluoride effects the transformation —CO2H → —CF3). DAST is used in preference to the more classical gaseous SF4, since as a liquid it is more easily handled. A slightly thermally more stable compound is morpho-DAST.[3] Acid-labile substrates are less likely to undergo rearrangement and elimination since DAST is less prone to contamination with acids. Reaction temperatures are milder as well – alcohols typically react at −78 °C and ketones around 0 °C.
Synthesis
DAST is prepared by the reaction of diethylaminotrimethylsilane and sulfur tetrafluoride:[4]
- Et2NSiMe3 + SF4 → Et2NSF3 + Me3SiF
The original paper calls for trichlorofluoromethane (Freon-11) as a solvent, a compound that has been banned under the Montreal Protocol and is no longer available as a commodity chemical. Diethyl ether is a green alternative that can be used with no decrease in yield.[5] Because of the dangers involved in the preparation of DAST (glass etching, possibility of exothermic events), it is often purchased from a commercial source. At one time Carbolabs[6] was one of the few suppliers of the chemical but a number of companies now sell DAST. Carbolabs was acquired by Sigma-Aldrich in 1998.
Safety and alternative reagents
Upon heating, DAST converts to the highly explosive (NEt2)2SF2 with expulsion of sulfur tetrafluoride. To minimize accidents, samples are maintained below 50 °C.[7] Bis-(2-methoxyethyl)aminosulfur trifluoride (trade name: Deoxo-Fluor) and difluoro(morpholino)sulfonium tetrafluoroborate (trade name: XtalFluor-M) are reagents derived from DAST with less explosive potential[8][9] XtalFluor-E has been jointly developed by OmegaChem Inc. and Manchester Organics Ltd. in 2009–2010.[8][9]
See also
References
- ↑ A. H. Fauq, "N,N-Diethylaminosulfur Trifluoride" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York.
- ↑ Middleton, William J. (1975-03-01). "New fluorinating reagents. Dialkylaminosulfur fluorides". The Journal of Organic Chemistry 40 (5): 574–578. doi:10.1021/jo00893a007. ISSN 0022-3263.
- ↑ Markovskii, LN; Pashinnik, VE; KIRSANOVA, NA (1975). "SULFUR BIS (DIALKYLAMINO) DIFLUORIDES". Zhurnal Organicheskoi Khimii 11: 74–77.
- ↑ W. J. Middleton, E. M. Bingham "Diethylaminosulfur Trifluoride" Organic Syntheses, Coll. Vol. 6, p.440; Vol. 57, p.50. Online version
- ↑ L. N. Markovskij; V. E. Pashinnik; A. V. Kirsanov (1973). "Application of Dialkylaminosulfur Trifluorides in the Synthesis of Fluoroorganic Compounds". Synthesis 1973 (12): 787–789. doi:10.1055/s-1973-22302.
- ↑ REACTION OF SULFOXIDES WITH DIETHYLAMINOSULFUR TRIFLUORIDE: FLUOROMETHYL PHENYL SULFONE, A REAGENT FOR THE SYNTHESIS OF FLUOROALKENES, Organic Syntheses, Coll. Vol. 9, p.446 (1998); Vol. 72, p.209 (1995)
- ↑ Messina, P. A.; Mange, K. C.; Middleton, W. J. (1989). "Aminosulfur trifluorides: relative thermal stability". Journal of Fluorine Chemistry 42 (1): 137–143. doi:10.1016/S0022-1139(00)83974-3.
- ↑ 8.0 8.1 l'Heureux, A.; Beaulieu, F.; Bennett, C.; Bill, D. R.; Clayton, S.; Laflamme, F. O.; Mirmehrabi, M.; Tadayon, S. et al. (2010). "Aminodifluorosulfinium Salts: Selective Fluorination Reagents with Enhanced Thermal Stability and Ease of Handling†,‡". The Journal of Organic Chemistry 75 (10): 3401–3411. doi:10.1021/jo100504x. PMID 20405933.
- ↑ 9.0 9.1 Beaulieu, F.; Beauregard, L. P.; Courchesne, G.; Couturier, M.; Laflamme, F. O.; l’Heureux, A. (2009). "Aminodifluorosulfinium Tetrafluoroborate Salts as Stable and Crystalline Deoxofluorinating Reagents". Organic Letters 11 (21): 5050–5053. doi:10.1021/ol902039q. PMID 19799406.
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