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Trichloroacetonitrile

Trichloroacetonitrile is an organic compound with the formula CCl3CN. It is a colourless liquid, although commercial samples often are brownish. It is used commercially as a precursor to the fungicide etridiazole. It is prepared by dehydration of trichloroacetamide.[1] As a bifunctional compound, trichloroacetonitrile can react at both the trichloromethyl and the nitrile group. The electron-withdrawing effect of the trichloromethyl group activates the nitrile group for nucleophilic additions. The high reactivity makes trichloroacetonitrile a versatile reagent, but also causes its susceptibility towards hydrolysis.

Trichloroacetonitrile
Names
Preferred IUPAC name
Trichloroacetonitrile
Other names
trichlorocyanomethane, trichloroethanenitrile, cyanochloroform, trichloromethyl cyanide, trichloroethyl nitrile
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.008.078 Edit this at Wikidata
UNII
  • InChI=1S/C2Cl3N/c3-2(4,5)1-6
    Key: DRUIESSIVFYOMK-UHFFFAOYSA-N
  • ClC(Cl)(Cl)C#N
Properties
C2Cl3N
Molar mass 144.38 g·mol−1
Appearance colourless liquid
Density 1.44 g/mL
Melting point −42 °C (−44 °F; 231 K)
Boiling point 83 to 84 °C (181 to 183 °F; 356 to 357 K)
insoluble
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 GHS06, GHS09
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
4
1
0
Flash point 195 °C (383 °F; 468 K)
Safety data sheet (SDS) MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Synthesis

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The production of trichloroacetonitrile by dehydration of trichloroacetamide was first described in 1873 by L. Bisschopinck at the Katholieke Universiteit Leuven.[2]

Trichloroacetonitrile via trichloracetamide 

Trichloroacetonitrile can be obtained by chlorination of acetonitrile on a zinc, copper and alkaline earth metal halide-impregnated activated carbon catalyst at 200–400 °C with a 54% yield.[3]

Trichloroacetonitrile via acetonitrile 

The high temperatures required by this process favours the formation of byproducts, such as tetrachloromethane. In contrast, the chlorination of acetonitrile saturated with hydrogen chloride leads to pure trichloroacetonitrile even at 50–80 °C in good yields.[4]

Like other halogenated acetonitriles, trichloroacetonitrile is produced from organic substances such as algae, humic acids and proteinaceous material in the disinfecting chlorination of water from natural sources.[5][6]

Properties

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Rounded bond lengths and angles of trichloroacetonitrile

Freshly-distilled trichloroacetonitrile is a colorless liquid with a pungent odor that discolours rapidly yellowish to light brown. It is sensitive towards water, acids and bases.

The bond lengths are 146.0 pm (C–C), 116.5 pm (C≡N) and 176.3 pm (C–Cl). The bond angle is 110.0° (Cl–C–Cl).[7]

Use

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The substitution of all electronegative substituents in trichloroacetonitrile by nucleophilic attack of alkoxide anions produces orthocarbonic acid esters in high yield.

Due to the high reactivity of the chlorine atoms, trichloroacetonitrile can be used (especially in combination with triphenylphosphine) to convert allylic alcohols into the corresponding allylic chlorides.[8]

Allyl chloride via propenol 

With carboxylic acids, acyl chlorides are obtained.[9]

Due to the mild reaction conditions, the Cl3CCN/PPh3 system is also suitable for the activation of carboxylic acids and their linkage with supported amino compounds to amides (peptides) in solid-phase syntheses.[10] From sulfonic acids, the corresponding sulfochlorides are formed analogously.[11] In an analogous manner, the activation of diphenylphosphoric acid with Cl3CCN/PPh3 and reaction with alcohols or amines proceeds to the corresponding phosphoric acid esters or amides in a gentle and efficient one-pot reaction.[12]

Also, phenolic hydroxy groups in nitrogen-containing aromatics can be converted into the chlorine compounds.[13]

2-Chloropyridine via trichloroacetonitrile 

In a Hoesch reaction, aromatic hydroxyketones are formed in the reaction of substituted phenols with trichloroacetonitrile, for example from 2-methyl phenol the 2-trichloroacyl derivative in 70% yield.[14]

Hydroxyketones via trichloroacetonitrile 

The electron-withdrawing effect of the trichloromethyl group activates the nitrile group of trichloroacetonitrile for the attack of nucleophilic oxygen, nitrogen and sulfur compounds. For example, alcohols give O-alkyltrichloroacetimidates under basic catalysis in a direct and reversible addition,[15] which can be isolated as stable and less hydrolysis-sensitive adducts.

Trichloroacetimidate formation 

With primary and secondary amines, N-substituted trichloroacetamidines are formed in a smooth reaction with good yields, which can be purified by vacuum distillation and are obtained as colorless, malodorous liquids.[16] Reaction with ammonia and then with anhydrous hydrogen chloride gives the solid trichloroacetamidine hydrochloride, the starting compound for the fungicide etridiazole.

In academic research, trichloroacetonitrile is used as a reagent in the Overman rearrangement, converting allylic alcohols into allylic amines.[17][18][19] The reaction is based on a [3,3]-sigmatropic and diastereoselective rearrangement.

Benzyl trichloroacetimidate is easily accessible from benzyl alcohol and trichloroacetonitrile.[20] Benzyl trichloroacetimidate is useful as a benzylating reagent for sensitive alcohols under mild conditions and to preserve chirality.[21]

O-Glycosyl-trichloroacetimidates for the activation of carbohydrates

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R. R. Schmidt and co-workers[22] have described the selective anomeric activation of O-protected hexopyranoses (glucose, galactose, mannose, glucosamine, galactosamine), hexofuranoses and pentopyranoses with trichloroacetonitrile in the presence of a base, as well as glycosylations under acid catalysis.[23][24][25]

Under kinetic control[26] with potassium carbonate as the base, β-trichloroacetimidates are formed selectively, whereas with sodium hydride, caesium carbonate or potassium hydroxide[27] and in the presence of phase-transfer catalysts[28] only α-trichloroacetimidates are obtained (thermodynamically controlled).

α-Glycosyltrichloracetimidate 

The trichloroacetimidates are reacted between −40 °C and room temperature with boron trifluoride etherate in dichloromethane with O-protected sugars. This method usually gives better results than the Koenigs–Knorr method using silver salts or the Helferich method which uses problematic mercury salts. Since an inversion occurs at the anomeric center, the reaction leads to β-O-glycosides (when using α-trichloroacetimidates). The trichloroacetimidate method often produces sterically uniform glycosides under mild reaction conditions in very good yields.

Octaacetyltrehalose 

Thioacetic acid reacts with acetyl-protected α-galactosyl trichloroacetimidate even without additional acid catalysis to thioglycoside, from which (after cleavage of the protective groups) 1-thio-β-D-galactose is easily accessible, which is useful for the separation of racemates of amino acids.[29]

Thiogalactose synthesis 

Trichloroacetonitrile was an important fumigant in the first half of the 20th century, but today it has become obsolete for this application.[30]

See also

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References

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  1. ^ Pollak, Peter; Romeder, Gérard; Hagedorn, Ferdinand; Gelbke, Heinz-Peter (2002). "Nitriles". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_363. ISBN 978-3527306732.
  2. ^ Bisschopinck, L. (1873). "Ueber die gechlorten Acetonitrile". Berichte der Deutschen Chemischen Gesellschaft. 6: 731–734. doi:10.1002/cber.187300601227.
  3. ^ US patent 2375545, R. T. Foster, "Process for the preparation of trichloroacetonitrile", issued 1945-05-08, assigned to Imperial Chemical Industries 
  4. ^ US patent 2745868, G. Käbisch, "Process for the production of trichloroacetonitrile", issued 1956-05-15, assigned to Deutsche Gold- und Silber-Scheideanstalt, formerly Roessler 
  5. ^ Guidelines for Drinking Water Quality (PDF). Recommendations. Vol. 1 (3rd ed.). Geneva: World Health Organization. 2004. ISBN 9-2415-4638-7.
  6. ^ Frank Bernsdorff (2007). Untersuchungen zur abiotischen Bildung von Acetonitril, Haloacetonitrilen und Trichlornitromethan [Investigations into abiotic formation of acetonitrile, haloacetonitriles and trichloronitromethane] (in German). GRIN. p. 5. ISBN 9783638383431.
  7. ^ Lide, David R., ed. (2010). "Structure of Free Molecules in the Gas Phase". CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, FL: CRC Press/Taylor and Francis. pp. 9–46.
  8. ^ Matveeva, E. D.; et al. (1995). "Regioselective and stereoselective substitution of hydroxyl group for halogen in allyl alcohols". Russian Journal of Organic Chemistry. 31 (8): 1121–1125.
  9. ^ Jang, D. O.; et al. (1999). "A mild and efficient procedure for the preparation of acid chlorides from carboxylic acids". Tetrahedron Letters. 40 (29): 5323–5326. doi:10.1016/S0040-4039(99)00967-3.
  10. ^ Vago, J.; Greiner, J. (2002). "A useful acylation method using trichloroacetonitrile and triphenylphosphine for solid phase organic synthesis". Tetrahedron Letters. 43 (34): 6039–6041. doi:10.1016/S0040-4039(02)01241-8.
  11. ^ Chantarasriwong, O.; et al. (2006). "A practical and efficient method for the preparation of sulfonamides utilizing Cl3CCN/PPh3". Tetrahedron Letters. 47 (42): 7489–7492. doi:10.1016/j.tetlet.2006.08.036.
  12. ^ Kasemsuknimit, A.; et al. (2011). "Efficient amidation and esterification of phosphoric acid using Cl3CCN/Ph3P". Bulletin of the Korean Chemical Society. 32 (9): 3486–3488. doi:10.5012/bkcs.2011.32.9.3486.
  13. ^ Kijrungphaiboon, W.; et al. (2006). "Cl3CCN/PPh3 and CBr4/PPh3: two efficient reagent systems for the preparation of N-heteroaromatic halides". Tetrahedron Letters. 53 (6): 674–677. doi:10.1016/j.tetlet.2011.11.123.
  14. ^ Martin, R. (2011), Aromatic Hydroxyketones: Preparation and Physical Properties. Vol. 1 Hydroxybenzophenones (in German) (3rd ed.), Springer, doi:10.1007/978-1-4020-9787-4, ISBN 978-1-4020-9787-4
  15. ^ Nef, J. U. (1895). Annalen der Chemie. 287: 274. {{cite journal}}: Missing or empty |title= (help)
  16. ^ Grivas, John C.; Taurins, Alfred (1958). "Reaction of trichloroacetonitrile with primary and secondary amines. Part I. Preparation of some trichloroacetamidines". Canadian Journal of Chemistry. 36 (5): 771–774. doi:10.1139/v58-113. ISSN 0008-4042.
  17. ^ Nishikawa, T.; Asai, M.; Ohyabu, N.; Isobe, M. (1998). "Improved Conditions for Facile Overman Rearrangement". The Journal of Organic Chemistry. 63 (1): 188–192. doi:10.1021/jo9713924. PMID 11674062.
  18. ^ "Overman Rearrangement". Organic Chemistry Portal. organic-chemistry.org. Retrieved 2012-11-15.
  19. ^ Chen, Y. K.; Lurain, A. E.; Walsh, P. J. (2002). "A general, highly enantioselective method for the synthesis of D and L alpha-amino acids and allylic amines". Journal of the American Chemical Society. 124 (41): 12225–12231. doi:10.1021/ja027271p. PMID 12371863.
  20. ^ Schaefer, Fred C.; Peters, Grace A. (1961). "Base-Catalyzed Reaction of Nitriles with Alcohols. A Convenient Route to Imidates and Amidine Salts". The Journal of Organic Chemistry. 26 (2): 412–418. doi:10.1021/jo01061a034.
  21. ^ Eckenberg, E. P.; et al. (1993). "A useful application of benzyl trichloroacetimidate for the benzylation of alcohols". Tetrahedron. 49 (8): 1619–1624. doi:10.1016/S0040-4020(01)80349-5.
  22. ^ Schmidt, R. R.; Michel, J. (1980). "Einfache Synthese von α- und β-O-Glycosylimidaten. Herstellung von Glykosiden und Disacchariden" [Simple synthesis of α- and β-O-glycosylimidates. Manufacture of glycosides and disaccharides]. Angewandte Chemie. 92 (9): 763–764. Bibcode:1980AngCh..92..763S. doi:10.1002/ange.19800920933.
  23. ^ Schmidt, R. R. (1986). "Neue Methoden zur Glycosid- und Oligosaccharidsynthese – gibt es Alternativen zur Koenigs-Knorr-Methode?" [New methods for glycoside and oligosaccharide synthesis – are there alternatives to the Koenigs–Knorr method?]. Angewandte Chemie. 98 (3): 213–236. Bibcode:1986AngCh..98..213S. doi:10.1002/ange.19860980305.
  24. ^ Schmidt, R. R.; Kinzy, W. (1994). "Anomeric-oxygen activation for glycoside synthesis – the trichloroacetimidate method". Advances in Carbohydrate Chemistry and Biochemistry. 50: 21–123. doi:10.1016/S0065-2318(08)60150-X. ISBN 9780120072507. PMID 7942254.
  25. ^ Schmidt, R. R.; Jung, K.-H. (1997). "Oligosaccharide synthesis with trichloroacetimidates". In Hanessian, S. (ed.). Preparative Carbohydrate Chemistry. New York, NY: Marcel Dekker. pp. 283–312. ISBN 0-8247-9802-3.
  26. ^ Schmidt, R. R.; Michel, J. (1984). "Glycosylimidate, 12 Direkte Synthese vonO-α- undO-β-Glycosyl-imidaten". Liebigs Annalen der Chemie. 1984 (7): 1343–1357. doi:10.1002/jlac.198419840710.
  27. ^ Urban, F. J.; et al. (1990). "Synthesis of tigogenyl β-O-cellobioside heptaacetate and glycoside tetraacetate via Schmidt's trichloroacetimidate method; some new observatons [sic]". Tetrahedron Letters. 31 (31): 4421–4424. doi:10.1016/S0040-4039(00)97637-8.
  28. ^ Patil, V. J. (1996). "A simple access to trichloroacetimidates". Tetrahedron Letters. 37 (9): 1481–1484. doi:10.1016/0040-4039(96)00044-5.
  29. ^ Jegorov, A.; et al. (1994). "1-Thio-β-D-galactose as a chiral derivatization agent for the resolution of D,L-aminoacid enantiomers". Journal of Chromatography A. 673 (2): 286–290. doi:10.1016/0021-9673(94)85045-3.
  30. ^ Sax, N. M.; Lewis, R. J., eds. (1987). Hawley's Condensed Chemical Dictionary (11th ed.). New York, NY: Van Nostrand Reinhold. pp. 261, 1175.
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