The basicity of amines is determined by the availability of the lone pair of electrons on the nitrogen atom for donation. The more available the lone pair, the stronger the base.

1. Trimethylamine: This is a tertiary amine with three methyl groups attached to the nitrogen atom. The electron-donating alkyl groups increase electron density on the nitrogen, making the lone pair more available for donation.

2. Pyrrole: In pyrrole, the nitrogen's lone pair of electrons is part of an aromatic system (it's involved in resonance). This makes the lone pair less available for donation, so pyrrole is a weak base.

3. Aniline: In aniline, the nitrogen's lone pair of electrons is delocalized into the benzene ring, making it less available for donation. Therefore, aniline is a weak base.

4. Pyridine: In pyridine, the nitrogen atom is a part of the aromatic ring, but its lone pair of electrons is not involved in the aromatic system, making it more available for donation. However, the electron-withdrawing effect of the aromatic ring makes pyridine less basic than simple alkyl amines.

So, among the given options, Trimethylamine is the strongest base.

Question

The basicity of amines is determined by the availability of the lone pair of electrons on the nitrogen atom for donation. The more available the lone pair, the stronger the base.

1. Trimethylamine: This is a tertiary amine with three methyl groups attached to the nitrogen atom. The electron-donating alkyl groups increase electron density on the nitrogen, making the lone pair more available for donation.

2. Pyrrole: In pyrrole, the nitrogen's lone pair of electrons is part of an aromatic system (it's involved in resonance). This makes the lone pair less available for donation, so pyrrole is a weak base.

3. Aniline: In aniline, the nitrogen's lone pair of electrons is delocalized into the benzene ring, making it less available for donation. Therefore, aniline is a weak base.

4. Pyridine: In pyridine, the nitrogen atom is a part of the aromatic ring, but its lone pair of electrons is not involved in the aromatic system, making it more available for donation. However, the electron-withdrawing effect of the aromatic ring makes pyridine less basic than simple alkyl amines.

So, among the given options, Trimethylamine is the strongest base.

Knowee AI · Accepted Answer

The basicity of amines is determined by the availability of the lone pair of electrons on the nitrogen atom for donation. The more available the lone pair, the stronger the base.

1. Trimethylamine: This is a tertiary amine with three methyl groups attached to the nitrogen atom. The electron-donating alkyl groups increase electron density on the nitrogen, making the lone pair more available for donation.

2. Pyrrole: In pyrrole, the nitrogen's lone pair of electrons is part of an aromatic system (it's involved in resonance). This makes the lone pair less available for donation, so pyrrole is a weak base.

3. Aniline: In aniline, the nitrogen's lone pair of electrons is delocalized into the benzene ring, making it less available for donation. Therefore, aniline is a weak base.

4. Pyridine: In pyridine, the nitrogen atom is a part of the aromatic ring, but its lone pair of electrons is not involved in the aromatic system, making it more available for donation. However, the electron-withdrawing effect of the aromatic ring makes pyridine less basic than simple alkyl amines.

So, among the given options, Trimethylamine is the strongest base.

Which of the following amines is the strongest base?Select answer from the options belowTrimethylaminePyrroleAnilinePyridine

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