Nitroalkane
Nitroalkane
The nitroalkanes
are colorless (when pure), pleasant-smelling liquids which are sparingly
soluble in water. Most of them can be distilled at atmospheric pressure.
Nomenclature
The nitroalkanes
are named as nitro-derivative of the corresponding alkane, the positions of the
nitro-groups being indicated by numbers, e.g.
CH3NO2 nitromethane
NO2 NO2
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CH3CHCH2CHCH2CH3 2,4-dinitrohexane
The nitroalkanes,
the structure of which is RNO2, are isomeric with the alkyl
nitrites, RONO. The evidence that may be adduced for these respective formulas
is to be found in the study of the reactions of these two groups of compounds. It
is, however, worthwhile at this stage to mention the reaction which most
clearly indicates their respective structures, viz., reduction. When alkyl
nitrites are reduced, an alcohol and ammonia or hydroxylamines are formed. This
shows that the alkyl group in nitrites is attached to an oxygen atom:
R-ONO (e; H+) ⟶ ROH
+ NH3 + H2O
On the other
hand, when nitroalkanes are reduced, a primary amine is formed. This shows that
the alkyl group is attached to the nitrogen atom, since the structure of a
primary amine is known to be R-NH2 from its method of preparation:
RNO2 (e; H+) ⟶ RNH2 +
2H2O
For most
purposes, however, the non-commercial formula RNO2, is satisfactory.
General method of preparation
1. By heating
an alkyl halide with silver nitrite in aqueous ethanolic solution:
RX +
AgONO ⟶ RNO2 +
RONO + AgX
This method
is only useful for the preparation of primary nitroalkanes. With s-halides the
yield is about 15 per cent, and with t-halides 0-5 per cent; the yield of nitrite
increases from primary to tertiary halides.
2. Nitro-compounds are prepared industrially by direct nitration, which is carried
out in two ways.
In liquid-phase
nitration, the hydrocarbon is heated with concentrated nitric acid under
pressure at 140oC. Nitration under these conditions is always slow,
and a large amount of polynitro-compounds is produced.
In vapour-phase
nitration, the hydrocarbon is heated with nitric acid at 150-475oC;
each hydrocarbon has its optimum temperature.
Vapor-phase
nitration is more satisfactory than liquid-phase nitration.
3. Kornblum
et al. (1956) have prepared t-nitro-compounds by the oxidation of
t-carbinamines with potassium permanganate
R3CNH2 (KMnO4) ⟶ R3CNO2 (70-80%)
Reactions
1. nitroalkanes are reduced catalytically, by lithium aluminium hydride, or by
metal in acid solution to primary amines.
RNO2 ⟶ RNH2 + 2H2O
When the
reaction with metal is carried out in neutral solution, e.g., with zinc dust
and ammonium chloride solution, nitro-compounds are converted into an
N-alkylhydroxylamine.
RNO2 (Zn/NH4Cl) ⟶ RNHOH
+ H2O
2. Primary
nitro-compounds are hydrolysed by boiling hydrochloric acid or by 85 per cent
sulphuric acid to a carboxylic acid and hydroxylamine:
RCH2NO2 + H2O (HCl)⟶ RCO2H + NH2OH
This
reaction is used for manufacturing hydroxylamine.
Secondary nitro-compounds
are hydrolysed by boiling hydrochloric acid to ketones and nitrous oxide:
2R2CHNO2 (HCl) ⟶ 2R2CO + N2O + H2O
Tertiary nitro-compounds
are generally unaffected by hydrochloric acid.
3. Primary
and secondary nitro-compounds are readily halogenated in alkaline solution in
the a-position only:
R2C=NO2-Na+ + Br2 (NaOH)⟶ R2CBrNO2
+ NaBr
Primary nitro-compounds
can form the mono- and dibromo-derivatives, whereas secondary form only the
monobromo-derivative: nitromethane is exceptional in that it can form the
tribromo-derivative.
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