Brstjjy

[R−N⊕≡C⊖:⟷R−N¨=C:]{displaystyle left[{ce {R}}-{overset {oplus }{ce {N}}}{ce {#}}{overset {ominus }{ce {C}}}{ce {:,<->R-{ddot {N}}=C{:}}}right]}

General resonance structure of an isocyanide

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.^[1] 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.

Properties

Structure and bonding

The C-N distance in isocyanides is very short, 1.158 Å in methyl isocyanide. The C-N-C angles are near 180°.^[2]

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. The π lone pair of the nitrogen, responsible for the zwitterionic structure, stabilizes the structure and is responsible of the linearity of isocyanides, although the reactivity of isocyanides reflects some carbene character, at least in a formal sense. Thus, both resonance structures are useful representations.^[3] They are susceptible to polymerization.^[3]

Spectroscopy

Isocyanides exhibit a strong absorption in their IR spectra in the range: 2165–2110 cm^−1[4]

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.^[4]

Odour

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 only little delay 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, but this is heavily outweighed by the fact that isonitriles can be detected even in traces, and that most of the routes leading to the formation of isonitriles were discovered through the odor of these compounds."^[5] Isocyanides have been investigated as potential non-lethal weapons.^[6]

Some isocyanides convey less offensive odours such as malt, natural rubber, creosote, mild cherry or old wood.^[7] Non-volatile derivatives such as tosylmethyl isocyanide do not have objectionable odors.^[8]

Toxicity

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".^[5]

Synthesis

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.^[9] Normally the alkylation of an alkali metal cyanide gives a nitrile, but the silver ion protects the carbon end of the cyanide.

RX + AgCN → RNC + AgX

From formamides

Commonly, isocyanides are synthesized by dehydration of formamides. The formamide can be dehydrated with toluenesulfonyl chloride, phosphorus oxychloride, phosgene, diphosgene, or the Burgess reagent in the presence of a base such as pyridine or triethylamine.^[10][11][12]

RNHC(O)H + ArSO₂Cl + 2C₅H₅N → RNC + [C₅H₅NH]⁺[ArSO₃]^– + [C₅H₅NH]⁺Cl^–

From dichlorocarbene

In the carbylamine reaction (also known as the Hofmann isocyanide synthesis) alkali base reacts with chloroform to produce dichlorocarbene. The carbene then converts primary amines to isocyanides. As it is only effective for primary amines this reaction can be used as a chemical test for their presence. Illustrative is the synthesis of tert-Butyl isocyanide from tert-butylamine in the presence of catalytic amount of the phase transfer catalyst benzyltriethylammonium chloride.^[13]

Me₃CNH₂ + CHCl₃ + 3 NaOH → Me₃CNC + 3 NaCl + 3 H₂O

Other methods

Another route to isocyanides entails deprotonation of oxazoles and benzoxazoles in the 2-position.^[7] The resulting organolithium compound exists in chemical equilibrium with the 2-isocyanophenolate, which can be captured by an electrophile such as an acid chloride.

Reactions

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.^[14]

Isocyanides participate in many multicomponent reactions of interest in organic synthesis, two of which are: the Ugi reaction and the Passerini reaction.

Isocyanides also participate in cycloaddition reactions, such as the [4+1] cycloaddition with tetrazines.^[15] Depending on the degree of substitution of the isocyanide, this reaction converts isocyanides into carbonyls or gives stable cycloadducts.^[16] They also undergo insertion into the C–Cl bonds of acyl chlorides in the Nef isocyanide reaction, a process that is believed to be concerted and illustrates their carbene character.

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.^[17]

The α position of isocyanides have substantial acidity. For example, benzyl isocyanide has a pK_a of 27.4. In comparison, benzyl cyanide has a pK_a of 21.9.^[18] In the gas phase, CH₃NC is 1.8 kcal/mol less acidic than CH₃CN.^[19]

Ligands in coordination chemistry

Technetium sestamibi is a commercial isocyanide complex that is used in medicine for imaging.

Isocyanides form coordination complexes with most transition metals.^[20] 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.^[21] 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.^[22]

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.^[23]

Xanthocillin is a rare natural product that contains an isocyanide group (two in fact).

Nomenclature

Whereas in IUPAC nomenclature in most cases the suffix "nitrile" or "carbonitrile" is used for organic cyanides (R-C≡N),^[24]
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.

The sometimes used term "carbylamine" conflicts with systematic nomenclature. An amine always has three single bonds,^[25] whereas an isocyanide has only one single and one multiple bond.

The isocyanamide functional group consists of a amino group attached to an isocyano moiety.

References