We can produce this compound via the reaction of benzyl chloride with ammonia. Also, we can produce it by benzonitrile reduction. Moreover, this compound is a common precursor for organic synthesis and the production of many pharmaceuticals.
The key difference between aniline and benzylamine is that in aniline the amine group attaches with the benzene ring directly whereas in benzylamine the amine group attaches the benzene ring indirectly, through a —CH2- group. Moreover, we can produce aniline via nitration of benzene followed by hydrogenation nitrobenzene into aniline whereas we can produce benzylamine via reaction of benzyl chloride with ammonia.
Besides, a further difference between aniline and benzylamine is their odour. Aniline has the odour of rotten fish while the odour of benzylamine is similar to the odour of ammonia.
In summary, the key difference between aniline and benzylamine is that in aniline, the amine group attaches with the benzene ring directly whereas, in benzylamine, the amine group attaches the benzene ring indirectly, through a —CH 2 — group. With a mind rooted firmly to basic principals of chemistry and passion for ever evolving field of industrial chemistry, she is keenly interested to be a true companion for those who seek knowledge in the subject of chemistry.
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Now live: A fully responsive profile. Related 5. Hot Network Questions. Question feed. Chemistry Stack Exchange works best with JavaScript enabled. A third method of preparing amines involves the reaction of alkyl halides with ammonia or another amine. The reaction of methyl bromide with ammonia, Equation 3, is a simple example.
While reaction 3 looks simple, it is, in fact, tricky to obtain methylamine in good yield. The reason for this is that methyl amine is more reactive than ammonia; as soon as it is formed, it reacts with methyl bromide to produce dimethylamine. This, in turn, reacts with more methyl bromide to generate trimethylamine. Ultimately, tetramethyl ammonium bromide is formed as shown in Equation 4.
The trick required to obtain monoalkylation is to use a large excess of ammonia. Once all the methyl bromide has reacted, the excess ammonia, which has a lower boiling point than the methyl bromide, is boiled off, leaving the methyl amine behind. Ammonium bromide is also left behind from the reaction of the HBr that is produced in reaction 3 with some of the excess ammonia.
This is separated from the methyl bromide during the work-up of the reaction mixture. There are instances where multiple alkylation like that shown in reaction 4 are desireable. Equation 5 demonstrates a reaction where this "poly-alkylation" is used to advantage. These molecules are similar to soaps and lipids in that they have a polar "head" and a non-polar "tail". Figure 6 presents a cartoon of how a quaternary ammonium salt acts to transfer cyanide ion across the boundary between an aqueous phase and a less dense organic phase containing an alkyl bromide.
The non-polar "tail" of the salt projects into the non-polar organic phase, thus bringing the cationic "head" to the interface between the two layers. This, in turn, brings an anion to the interface where it is likely to encounter the alkyl bromide that is dissolved in the non-polar phase. Finally, amines may be prepared by reduction of imines, which, as we have seen , are readily prepared by the reaction of aldehydes and ketones with primary amines.
Equation 6 offers a simple example. Imines may also be reduced to amines with NaBH 4 or by catalytic hydrogenation.
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