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In case of substituted aniline the gr...

In case of substituted aniline the group which decreases the basic strength is

A

`-OCH_(3)`

B

`-CH_(3)`

C

`-NH_(2)`

D

`-C_(6)H_(5)`

Text Solution

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The correct Answer is:
D
Electron releasing groups like `--NH_(2), --OCH_(3), --CH_(3)` increase electron density at N-atom hence, such substituents increases basic nature of of aromatic amines.
Electron -withdrawing groups like,
`-NO_(2),SO_(3)H,-COOH,-X-C_(5)H_(5))`
derease electron density at N-atom thus,
decreasing basic nature of aromatic amines.
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The decreasing order of basic strength is

Amines are basic in nature due to the presence of lone pair of electrons on N atom of -NH_(2) group. The basic strength of amines can be expressed by their dissociation constant, K_(b) or pK_(b) . RNH_(2) + H_(2) to R NH_(3)^(+) + OH^(-) K_(b) = ([RHH_(3)^(+)][OH^(-)])/([RNH_(2)]) and pK_(b) = -log K_(b) Greater the K_(b) value or smaller the pK_(b) value, more is the basic strength of amine. Aliphatic amines are stronger bases than ammonia due to the electron releasing effect of alkyl groups. The basic strength among amines decreases as : 2^(@) gt 1^(@) gt 3^(@) Aryl amines such as aniline are less basic than aliphatic amines due to the involvement of lone pair of electrons on N atom with the resonance in benzene. In derivatives of aniline, the electron releasing groups increase the basic strength while electron withdrawing groups decrease the basic strength. The base weakening effect of electron withdrawing group and base strengthening effect of electron releasing group is more marked at p-position than at m-position. Every o- substituted aniline is less basic than aniline due to ortho effect. Which of the following group does not decrease the basic strength of aniline ?

Amines are basic in nature due to the presence of lone pair of electrons on N atom of -NH_(2) group. The basic strength of amines can be expressed by their dissociation constant, K_(b) or pK_(b) . RNH_(2) + H_(2) to R NH_(3)^(+) + OH^(-) K_(b) = ([RHH_(3)^(+)][OH^(-)])/([RNH_(2)]) and pK_(b) = -log K_(b) Greater the K_(b) value or smaller the pK_(b) value, more is the basic strength of amine. Aliphatic amines are stronger bases than ammonia due to the electron releasing effect of alkyl groups. The basic strength among amines decreases as : 2^(@) gt 1^(@) gt 3^(@) Aryl amines such as aniline are less basic than aliphatic amines due to the involvement of lone pair of electrons on N atom with the resonance in benzene. In derivatives of aniline, the electron releasing groups increase the basic strength while electron withdrawing groups decrease the basic strength. The base weakening effect of electron withdrawing group and base strengthening effect of electron releasing group is more marked at p-position than at m-position. Every o- substituted aniline is less basic than aniline due to ortho effect. Which of the following statement is not correct?

Amines are basic in nature due to the presence of lone pair of electrons on N atom of -NH_(2) group. The basic strength of amines can be expressed by their dissociation constant, K_(b) or pK_(b) . RNH_(2) + H_(2) to R NH_(3)^(+) + OH^(-) K_(b) = ([RHH_(3)^(+)][OH^(-)])/([RNH_(2)]) and pK_(b) = -log K_(b) Greater the K_(b) value or smaller the pK_(b) value, more is the basic strength of amine. Aliphatic amines are stronger bases than ammonia due to the electron releasing effect of alkyl groups. The basic strength among amines decreases as : 2^(@) gt 1^(@) gt 3^(@) Aryl amines such as aniline are less basic than aliphatic amines due to the involvement of lone pair of electrons on N atom with the resonance in benzene. In derivatives of aniline, the electron releasing groups increase the basic strength while electron withdrawing groups decrease the basic strength. The base weakening effect of electron withdrawing group and base strengthening effect of electron releasing group is more marked at p-position than at m-position. Every o- substituted aniline is less basic than aniline due to ortho effect. The strongest base among the following is

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