An isocyanide (also called isonitrile or carbylamine) is an organic compound with the functional group -N≡C. It is the isomer of the related cyanide (-C≡N), hence the prefix iso. The organic fragment is connected to the isocyanide group via the nitrogen atom, not via the carbon. They are used as building blocks for the synthesis of other compounds.
- 1 Properties
- 2 Synthesis of isocyanides
- 3 Reactions
- 4 Naturally occurring isocyanides
- 5 Nomenclature
- 6 References
Structure and bonding
Akin to carbon monoxide, isocyanides are described by two resonance structures, one with a triple bond between the nitrogen and the carbon and one with a double bond between. Surprisingly, the second one, with a carbenic character is the more important. Nevertheless, the π lone pair of the nitrogen, responsible of the zwitterionic structure, stabilizes the structure and is responsible of the linearity of isocyanides. Isocyanides are best shown as a mixture of both resonance structures. They are susceptible to polymerization.
Isocyanides exhibit a strong absorption in their IR spectra in the range: 2165–2110 cm−1
The electronic symmetry about the isocyanide 14N nucleus results in a slow quadrupolar relaxation so that 13C-14N nuclear spin coupling can be observed, with coupling constants of ca. 5 Hz for the isocyanide 13C nucleus and 5–14 Hz for the 13C nucleus which the isocyanide group is attached to.
Their disagreeable odour is legendary. To quote from Lieke, "Es besitzt einen penetranten, höchst unangenehmen Geruch; das Oeffnen eines Gefässes mit Cyanallyl reicht hin, die Luft eines Zimmers mehrere Tage lang zu verpesten, ..." (It has a penetrating, extremely unpleasant odour; the opening of a flask of allyl [iso]cyanide is enough to foul up the air in a room for several days). Note that in Lieke's day, the difference between isocyanide and nitrile was not fully appreciated.
Ivar Karl Ugi states that "The development of the chemistry of isocyanides has probably suffered ... through the characteristic odor of volatile isonitriles, which has been described by Hofmann and Gautier as 'highly specific, almost overpowering', 'horrible', and 'extremely distressing'. It is true that many potential workers in this field have been turned away by the odour." Isocyanides have been investigated as potential non-lethal weapons.
Some isocyanides convey less offensive odours such as malt, natural rubber, creosote, mild cherry or old wood. Non-volatile derivatives such as tosylmethyl isocyanide do not have objectionable odors.
While some isocyanides (e.g., cyclohexyl isocyanide) are toxic, others "exhibit no appreciable toxicity for mammals". Referring to ethyl isocyanide, toxicological studies in the 1960s at Bayer showed that "oral and subcutaneous doses of 500-5000 mg/kg can be tolerated by mice".
Synthesis of isocyanides
Silver cyanide route
The first isocyanide, allyl isocyanide, was reported in 1859 by the chemist Lieke from the reaction of allyl iodide and silver cyanide. Normally the alkylation of an alkali metal cyanide gives a nitrile, but the silver ion protects the carbon end of the cyanide.
- RNHC(O)H + POCl3 → RNC + "PO2Cl" + 2 HCl
In the carbylamine reaction (also known as the Hofmann isocyanide synthesis) potassium hydroxide reacts with chloroform to produce dichlorocarbene. This then converts primary amines to isocyanides. As it is only effective for primary amines it is used as a chemical test for their presence.
The benzoxazole deprotonates at the 2-position by n-butyllithium. The resulting organolithium compound exists in chemical equilibrium with the 2-isocyanophenolate, which can be captured by an electrophile such as an acid chloride. Being an ester the formed isocyanate in the example above behaves uncharacteristically with reportedly a mild cherry smell.
Isocyanides are stable to strong base (they are often made under strongly basic conditions), but they are sensitive to acid. In the presence of aqueous acid, isocyanides hydrolyse to the corresponding formamides:
- RNC + H2O → RN(H)C(O)H
This reaction is used to destroy odorous isocyanide mixtures. Some isocyanides can polymerize in the presence of Lewis and Bronsted acids.
Isocyanides also participate in cycloaddition reactions, such as the [4+1] cycloaddition with tetrazines. Depending on the degree of substitution of the isocyanide, this reaction converts isocyanides into carbonyls or gives stable cycloadducts.
Isocyanides have also been shown to be a useful reagent in palladium catalysed reactions with a wide variety of compounds being formed using this method.
Ligands in coordination chemistry
Isocyanides form coordination complexes with most transition metals. They behave as electron-rich analogues of carbon monoxide. For example tert-Butyl isocyanide forms Fe2(tBuNC)9, which is analogous to Fe2(CO)9. Although structurally similar, the analogous carbonyls differ in several ways, mainly because t-BuNC is a better donor ligand than CO. Thus, Fe(tBuNC)5 is easily protonated, whereas its counterpart Fe(CO)5 is not.
Naturally occurring isocyanides
Only few naturally occurring compounds exhibit the isocyanide functionality. The first was discovered in 1957 in an extract of the mold Penicillium notatum Westling. The compound xanthocillin later was used as an antibiotic. Since then numerous other isocyanides have been isolated. Most of the marine isocyanides are terpenoid, while some of the terrestrial isocyanides originate from α-aminoacids.
Whereas in IUPAC nomenclature in most cases the suffix "nitrile" or "carbonitrile" is used for organic cyanides (R-C≡N), names for isocyanides have the prefix "isocyano". IUPAC names become isocyanomethane, isocyanoethane, isocyanopropane, etc.
The suffix "isonitrile" can be ambiguous, since the carbon counting is different from "nitrile". For example, ethanenitrile ( CH3CN) and ethaneisonitrile (C2H5NC) are not isomers, as the prefix "iso" in the suffix might suggest. In contrast, "isocyanide" does not have this ambiguity: ethyl cyanide (C2H5CN) and ethyl isocyanide (C2H5NC) are indeed isomers.
- IUPAC Goldbook isocyanides
- Kessler, M.; Ring, H.; Trambarulo, R.; Gordy, W. (1950). "Microwave Spectra and Molecular Structures of Methyl Cyanide and Methyl Isocyanide". Physical Review 79: 54–56. doi:10.1103/PhysRev.79.54.
- Ramozzi, R.; Chéron, N.; Braïda, B.; Hiberty, P. C.; Fleurat-Lessard, P. (2012). "A Valence Bond View of Isocyanides' Electronic Structure". New Journal of Chemistry 36 (5): 1137–1340. doi:10.1039/C2NJ40050B.
- Stephany, R. W.; de Bie, M. J. A.; Drenth, W. (1974). "A 13C-NMR and IR study of isocyanides and some of their complexes". Organic Magnetic Resonance 6 (1): 45–47. doi:10.1002/mrc.1270060112. Cite uses deprecated parameter
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- B. E. Hoogenboom, O. H. Oldenziel, and A. M. van Leusen "Toluenesulfonylmethyl isocyanide" Organic Syntheses, Coll. Vol. 6, p.987 (1988).
- Lieke, W. (1859). "Über das Cyanallyl". Annalen der Chemie und Pharmacie (C.F. Winter'sche) 112 (3): 316–321. doi:10.1002/jlac.18591120307.
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- Eric Singleton, Hester E. Oosthuizen "Metal Isocyanide Complexes"Advances in Organometallic Chemistry 1983, Volume 22, Pages 209–310. doi:10.1016/S0065-3055(08)60404-9
- Bassett, J.M.; Barker, G.K.; Green, M.; Howard, J.A.; Stone, G.A.; Wolsey, W.C. "Chemistry of low-valent metal isocyanide complexes" J.C.S. Dalton, 1981, 219-227.
- Bassett, J.-M.; Farrugia, L. J.; Stone, F. G. A. "Protonation of pentakis(t-butyl isocyanide)iron" J.C.S. Dalton, 1980, 1789-1790. doi:10.1039/DT9800001789
- Scheuer, P. J. (1992). "Isocyanides and Cyanides as Natural Products". Accounts of Chemical Research 25 (10): 433–439. doi:10.1021/ar00022a001.
- IUPAC Nomenclature of Organic Compounds (Recommendations 1993)
- IUPAC Nomenclature of Organic Compounds (Recommendations 1993)