Which of the following is most basic?

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(D) To determine the basicity,we look at the availability of the lone pair of electrons on the nitrogen atom for protonation.$A$. In Pyrrole,the lone

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Piperidine

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(D) To determine the basicity,we look at the availability of the lone pair of electrons on the nitrogen atom for protonation.$A$. In Pyrrole,the lone pair on the nitrogen atom is involved in the aromatic sextet,making it unavailable for protonation. Thus,it is very weakly basic.$B$. In Aniline,the lone pair on the nitrogen atom is in conjugation with the benzene ring,which reduces its availability for protonation.$C$. In Pyridine,the lone pair is in an $sp^2$ hybridized orbital. Although it is not involved in the aromatic system,the $sp^2$ character makes it less basic than aliphatic amines.$D$. In Piperidine,the nitrogen atom is $sp^3$ hybridized and there is no resonance or aromaticity to delocalize the lone pair. Therefore,the lone pair is highly available for protonation,making Piperidine the most basic among the given options.

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