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(A) To determine the basic strength,we analyze the availability of the lone pair on the nitrogen atom:$(I)$ Piperidine: The nitrogen is $sp^3$ hybridi

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$I > II > III > IV$

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(A) To determine the basic strength,we analyze the availability of the lone pair on the nitrogen atom:$(I)$ Piperidine: The nitrogen is $sp^3$ hybridized. The lone pair is localized and available for donation. It is a strong secondary amine.$(II)$ Morpholine: The nitrogen is $sp^3$ hybridized,but the presence of an electronegative oxygen atom at the $4$-position exerts an inductive effect ($-I$ effect),which reduces the electron density on nitrogen,making it less basic than piperidine.$(III)$ Pyridine: The nitrogen is $sp^2$ hybridized. The lone pair is in an $sp^2$ orbital,which has more $s$-character than an $sp^3$ orbital,making it more electronegative and less basic.$(IV)$ Pyrrole: The lone pair on the nitrogen is involved in the aromatic sextet ($6\pi$ electrons). Therefore,it is not available for donation,making it the least basic.Thus,the order of basic strength is: $I > II > III > IV$.

Arrange the following compounds in the increasing order of their basic strength:

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