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Assertion : Cyanides R - C -= N: are ver...

Assertion : Cyanides `R - C -= N`: are very much weaker bases than aliphatic bases.
Reason : This is due to the fact that as the nitrogen atom becomes more multiply bonded, the lone pair of electrons are accommodated in an orbital that has more 'S' character. The electron pair is thus drawn closer to the nitrogen nucleus, and held more lightly by it.

A

Both assertion and reason are correct, reason is the correct explanation of assertion

B

Both assertion and reason are correct and reason is not the correct explanation of assertion

C

Assertion is true reason is false

D

Assertion is false reason is true

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Statement 1 : In strongly acidic solutions, aniline becomes more reactive towards electrophilic reagents Statement 2 : The amino group is protonated in strongly acidic solution, and thus the lone pair of electron on the nitrogen is no longer available for resonance.

All aliphatic amines are more basic than ammonia but due to delocalization of lone pair of electrons of the nitrogen atom on the benzene ring, aniline is a weaker base than ammonia. The basic strength of the substituted anilines, however, depends upon the nature of the substituent. Whereas electron-donating groups tend to increase, electron-withdrawing groups tend to decrease the basic strength. The base strengthening effect of the electron-donating groups and base weakening effect of the electron-withdrawing groups is, however ,more pronounced at p-than at m-position. However, due to ortho effect, o-substituted anilines are weaker bases than anilines regardless of the nature of substituent whether electron-donating or electron-withdrawing. Among the following, the weakest base is

All aliphatic amines are more basic than ammonia but due to delocalization of lone pair of electrons of the nitrogen atom on the benzene ring, aniline is a weaker base than ammonia. The basic strength of the substituted anilines, however, depends upon the nature of the substituent. Whereas electron-donating groups tend to increase, electron-withdrawing groups tend to decrease the basic strength. The base strengthening effect of the electron-donating groups and base weakening effect of the electron-withdrawing groups is, however ,more pronounced at p-than at m-position. However, due to ortho effect, o-substituted anilines are weaker bases than anilines regardless of the nature of substituent whether electron-donating or electron-withdrawing. What is the order of basicity of I. p-methylaniline II. m-methylaniline III, aniline IV. o-methylaniline

All aliphatic amines are more basic than ammonia but due to delocalization of lone pair of electrons of the nitrogen atom on the benzene ring, aniline is a weaker base than ammonia. The basic strength of the substituted anilines, however, depends upon the nature of the substituent. Whereas electron-donating groups tend to increase, electron-withdrawing groups tend to decrease the basic strength. The base strengthening effect of the electron-donating groups and base weakening effect of the electron-withdrawing groups is, however ,more pronounced at p-than at m-position. However, due to ortho effect, o-substituted anilines are weaker bases than anilines regardless of the nature of substituent whether electron-donating or electron-withdrawing. Arrange the following amines in decreasing order of their basic strength

BRILLIANT PUBLICATION-ORGANIC CHEMISTRY: BASIC PRINCIPLES - PART II (REACTION MECHANISM)-LEVEL -II
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