Nitrile

In

Inorganic compounds containing the −C≡N group are not called nitriles, but cyanides instead.^[2] Though both nitriles and cyanides can be derived from cyanide salts, most nitriles are not nearly as toxic.

Structure and basic properties

The N−C−C geometry is linear in nitriles, reflecting the sp hybridization of the triply bonded carbon. The C−N distance is short at 1.16 

The first compound of the homolog row of nitriles, the nitrile of formic acid, hydrogen cyanide was first synthesized by C. W. Scheele in 1782.^[4][5] In 1811 J. L. Gay-Lussac was able to prepare the very toxic and volatile pure acid.^[6] Around 1832 benzonitrile, the nitrile of benzoic acid, was prepared by Friedrich Wöhler and Justus von Liebig, but due to minimal yield of the synthesis neither physical nor chemical properties were determined nor a structure suggested. In 1834 Théophile-Jules Pelouze synthesized propionitrile, suggesting it to be an ether of propionic alcohol and hydrocyanic acid.^[7] The synthesis of benzonitrile by Hermann Fehling in 1844 by heating ammonium benzoate was the first method yielding enough of the substance for chemical research. Fehling determined the structure by comparing his results to the already known synthesis of hydrogen cyanide by heating ammonium formate. He coined the name "nitrile" for the newfound substance, which became the name for this group of compounds.^[8]

Synthesis

Industrially, the main methods for producing nitriles are ammoxidation and hydrocyanation. Both routes are green in the sense that they do not generate stoichiometric amounts of salts.

Ammoxidation

In

The cyanohydrins are a special class of nitriles. Classically they result from the addition of alkali metal cyanides to aldehydes in the cyanohydrin reaction. Because of the polarity of the organic carbonyl, this reaction requires no catalyst, unlike the hydrocyanation of alkenes. O-Silyl cyanohydrins are generated by the addition trimethylsilyl cyanide in the presence of a catalyst (silylcyanation). Cyanohydrins are also prepared by transcyanohydrin reactions starting, for example, with acetone cyanohydrin as a source of HCN.^[10]

Dehydration of amides

Nitriles can be prepared by the dehydration of primary amides. Common reagents for this include phosphorus pentoxide (P₂O₅)^[11] and thionyl chloride (SOCl₂).^[12] In a related dehydration, secondary amides give nitriles by the von Braun amide degradation. In this case, one C-N bond is cleaved.

From aldehydes and oximes

The conversion of

In specialised cases the Van Leusen reaction can be used. Biocatalysts such as aliphatic aldoxime dehydratase are also effective.

Sandmeyer reaction

Aromatic nitriles are often prepared in the laboratory from the aniline via

• A commercial source for the cyanide group is diethylaluminum cyanide Et₂AlCN which can be prepared from triethylaluminium and HCN.^[16] It has been used in nucleophilic addition to ketones.^[17] For an example of its use see: Kuwajima Taxol total synthesis
• Cyanide ions facilitate the coupling of dibromides. Reaction of α,α′-dibromoadipic acid with sodium cyanide in ethanol yields the cyano cyclobutane:^[18]

  

• Aromatic nitriles can be prepared from base hydrolysis of trichloromethyl aryl ketimines (RC(CCl₃)=NH) in the Houben-Fischer synthesis^[19]
• Nitriles can be obtained from
  oxidation. Common methods include the use of potassium persulfate,^[20] Trichloroisocyanuric acid,^[21] or anodic electrosynthesis.^[22]
• α-Amino acids form nitriles and carbon dioxide via various means of oxidative decarboxylation.^[23][24] Henry Drysdale Dakin discovered this oxidation in 1916.^[25]
• From aryl carboxylic acids (Letts nitrile synthesis)

Reactions

Nitrile groups in organic compounds can undergo a variety of reactions depending on the reactants or conditions. A nitrile group can be hydrolyzed, reduced, or ejected from a molecule as a cyanide ion.

Hydrolysis

The hydrolysis of nitriles RCN proceeds in the distinct steps under acid or base treatment to first give carboxamides RC(=O)NH₂ and then carboxylic acids RCOOH. The hydrolysis of nitriles to carboxylic acids is efficient. In acid or base, the balanced equations are as follows:

${\displaystyle {\ce {RCN + 2H2O + HCl -> RCO2H + NH4Cl}}}$

${\displaystyle {\ce {RCN + H2O + NaOH -> RCO2Na + NH3}}}$

Strictly speaking, these reactions are mediated (as opposed to catalyzed) by acid or base, since one equivalent of the acid or base is consumed to form the ammonium or carboxylate salt, respectively.

Kinetic studies show that the second-order rate constant for hydroxide-ion catalyzed hydrolysis of acetonitrile to acetamide is 1.6×10⁻⁶ M⁻¹ s⁻¹, which is slower than the hydrolysis of the amide to the carboxylate (7.4×10⁻⁵ M⁻¹ s⁻¹). Thus, the base hydrolysis route will afford the carboxylate (or the amide contaminated with the carboxylate). On the other hand, the acid catalyzed reactions requires a careful control of the temperature and of the ratio of reagents in order to avoid the formation of polymers, which is promoted by the exothermic character of the hydrolysis.^[26] The classical procedure to convert a nitrile to the corresponding primary amide calls for adding the nitrile to cold concentrated sulfuric acid.^[27] The further conversion to the carboxylic acid is disfavored by the low temperature and low concentration of water.

${\displaystyle {\ce {RCN + H2O -> RC(O)NH2}}}$

Two families of enzymes catalyze the hydrolysis of nitriles. Nitrilases hydrolyze nitriles to carboxylic acids:

${\displaystyle {\ce {RCN + 2 H2O -> RCO2H + NH3}}}$

${\displaystyle {\ce {RCN + H2O -> RC(O)NH2}}}$

These enzymes are used commercially to produce acrylamide.

The "anhydrous hydration" of nitriles to amides has been demonstrated using an oxime as water source:^[28]

${\displaystyle {\ce {RCN + R'C(H)=NOH -> RC(O)NH2 + R'CN}}}$

Reduction

Nitriles are susceptible to

Deprotonation

Alkyl nitriles are sufficiently acidic to undergo deprotonation of the C-H bond adjacent to the CN group.

• with an
  organozinc compound in the Blaise reaction
• with alcohols in the Pinner reaction.
• with amines, e.g. the reaction of the amine sarcosine with cyanamide yields creatine^[32]
• Nitriles react in Friedel–Crafts acylation in the
  Houben–Hoesch reaction
  to ketones

Miscellaneous methods and compounds

• In reductive decyanation the nitrile group is replaced by a proton.
  reducing agents such as lithium aluminium hydride.^[33]
• In the so-called Franchimont Reaction (developed by the Belgian doctoral student Antoine Paul Nicolas Franchimont (1844-1919) in 1872), an α-cyanocarboxylic acid heated in acid hydrolyzes and decarboxylates to a dimer.^[35]
• Nitriles self-react in presence of base in the Thorpe reaction in a nucleophilic addition
• In organometallic chemistry nitriles are known to add to alkynes in carbocyanation:^[36]

Complexation

Nitriles are precursors to transition metal nitrile complexes, which are reagents and catalysts. Examples include tetrakis(acetonitrile)copper(I) hexafluorophosphate ([Cu(MeCN)₄]⁺) and bis(benzonitrile)palladium dichloride (PdCl₂(PhCN)₂).^[37]

Nitrile derivatives

Organic cyanamides

Cyanamides are N-cyano compounds with general structure R¹R²N−C≡N and related to the parent cyanamide.^[38]

Nitrile oxides

Nitrile oxides have the

Occurrence and applications

Nitriles occur naturally in a diverse set of plant and animal sources. Over 120 naturally occurring nitriles have been isolated from terrestrial and marine sources. Nitriles are commonly encountered in fruit pits, especially almonds, and during cooking of Brassica crops (such as cabbage, Brussels sprouts, and cauliflower), which release nitriles through hydrolysis. Mandelonitrile, a cyanohydrin produced by ingesting almonds or some fruit pits, releases hydrogen cyanide and is responsible for the toxicity of cyanogenic glycosides.^[41]

Over 30 nitrile-containing pharmaceuticals are currently marketed for a diverse variety of medicinal indications with more than 20 additional nitrile-containing leads in clinical development. The types of pharmaceuticals containing nitriles are diverse, from vildagliptin, an antidiabetic drug, to anastrozole, which is the gold standard in treating breast cancer. In many instances the nitrile mimics functionality present in substrates for enzymes, whereas in other cases the nitrile increases water solubility or decreases susceptibility to oxidative metabolism in the liver.^[42] The nitrile functional group is found in several drugs.

• 
  Structure of periciazine, an antipsychotic studied in the treatment of opiate dependence.
• 
  Structure of citalopram, an antidepressant drug of the selective serotonin reuptake inhibitor (SSRI) class.
• 
  Structure of cyamemazine, an antipsychotic drug.
• 
  Structure of fadrozole, an aromatase inhibitor for the treatment of breast cancer.
• 
  Structure of letrozole, an oral nonsteroidal aromatase inhibitor for the treatment of certain breast cancers.

See also

• Protonated nitriles: Nitrilium
• Deprotonated nitriles: Nitrile anion
• Cyanocarbon
• Nitrile ylide

References