Nitro compound

Aromatic nitro compounds are typically synthesized by nitration. Nitration is achieved using a mixture of nitric acid and sulfuric acid, which produce the nitronium ion (NO+
2), which the electrophile:

  +  

 

 H⁺

 

The nitration product produced on the largest scale, by far, is nitrobenzene. Many explosives are produced by nitration including trinitrophenol (picric acid), trinitrotoluene (TNT), and trinitroresorcinol (styphnic acid).[1] Another but more specialized method for making aryl–NO₂ group starts from halogenated phenols, is the Zinke nitration.

Aliphatic nitro compounds can be synthesized by various methods; notable examples include:

• Free radical nitration of alkanes.[2] The reaction produces fragments from the parent alkane, creating a diverse mixture of products; for instance, nitromethane, nitroethane, 1-nitropropane, and 2-nitropropane are produced by treating propane with nitric acid in the gas phase (e.g. 350–450 °C and 8–12 atm).
• Nucleophilic substitution reactions between halocarbons[3] or organosulfates[4] with silver or alkali nitrite salts.

Structural details of nitrobenzene, distances in picometers.[5]

• Nitromethane can be produced in the laboratory by treating sodium chloroacetate with sodium nitrite.[6]
• Oxidation of oximes[7] or primary amines.[8]
• Reduction of β-nitro alcohols[9] or nitroalkenes.[10]
• By decarboxylation of α-nitro carboxylic acids formed from nitriles and ethyl nitrate.[11][12]

In nucleophilic aliphatic substitution, sodium nitrite (NaNO₂) replaces an alkyl halide. In the so-called Ter Meer reaction (1876) named after Edmund ter Meer,[13] the reactant is a 1,1-halonitroalkane:

The reaction mechanism is proposed in which in the first slow step a proton is abstracted from nitroalkane 1 to a carbanion 2 followed by protonation to an aci-nitro 3 and finally nucleophilic displacement of chlorine based on an experimentally observed hydrogen kinetic isotope effect of 3.3.[14] When the same reactant is reacted with potassium hydroxide the reaction product is the 1,2-dinitro dimer.[15]

Chloramphenicol is a rare example of a naturally occurring nitro compound. At least some naturally occurring nitro groups arose by the oxidation of amino groups.[16] 2-Nitrophenol is an aggregation pheromone of ticks.

Examples of nitro compounds are rare in nature. 3-Nitropropionic acid found in fungi and plants (Indigofera). Nitropentadecene is a defense compound found in termites. Nitrophenylethane is found in Aniba canelilla.[17] Nitrophenylethane is also found in members of the Annonaceae, Lauraceae and Papaveraceae.[18]

Despite the occasional use in pharmaceuticals, the nitro group is associated with mutagenicity and genotoxicity and therefore is often regarded as a liability in the drug discovery process.[19]

Nitro compounds participate in several organic reactions, the most important being their reduction to the corresponding amines:

RNO₂ + 3 H₂ → RNH₂ + 2 H₂O

The α-carbon of nitroalkanes is somewhat acidic. The pK_a values of nitromethane and 2-nitropropane are respectively 17.2 and 16.9 in dimethyl sulfoxide (DMSO) solution. These values suggest an aqueous pK_a of around 11.[20] In other words, these carbon acids can be deprotonated in aqueous solution. The conjugate base is called a nitronate, they are formed as intermediates in the nitroaldol reaction and Nef reactions.

Nitromethane undergoes base-catalyzed additions to aldehydes in 1,2-addition in the nitroaldol reaction. Similarly, it adds to alpha-beta unsaturated carbonyl compounds as a 1,4-addition in the Michael reaction as a Michael donor. Nitroalkenes are Michael acceptors in the Michael reaction with enolate compounds.[21][22]

Many flavin-dependent enzymes are capable of oxidizing aliphatic nitro compounds to less-toxic aldehydes and ketones. Nitroalkane oxidase and 3-nitropropionate oxidase oxidize aliphatic nitro compounds exclusively, whereas other enzymes such as glucose oxidase have other physiological substrates.[23]

Explosive decomposition of organo nitro compounds are redox reactions, wherein both the oxidant (nitro group) and the fuel (hydrocarbon substituent) are bound within the same molecule. The explosion process generates heat by forming highly stable products including molecular nitrogen (N₂), carbon dioxide, and water. The explosive power of this redox reaction is enhanced because these stable products are gases at mild temperatures. Many contact explosives contain the nitro group.