Which of the following has the maximum dipole | vedclass

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(B) The dipole moment depends on the vector sum of individual bond dipoles. $p$-dichlorobenzene and $p$-dinitrobenzene have dipole moments close to ze

Vedclass · Accepted Answer

o-dinitrobenzene

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(B) The dipole moment depends on the vector sum of individual bond dipoles. $p$-dichlorobenzene and $p$-dinitrobenzene have dipole moments close to zero because the bond dipoles are in opposite directions and cancel each other out. In $o$-dichlorobenzene and $o$-dinitrobenzene,the dipoles are at an angle of $60^{\circ}$,resulting in a non-zero net dipole moment. Comparing $o$-dichlorobenzene and $o$-dinitrobenzene,the $-NO_2$ group is a much stronger electron-withdrawing group than the $-Cl$ atom,leading to a larger individual bond dipole for the $C-NO_2$ bond compared to the $C-Cl$ bond. Therefore,$o$-dinitrobenzene has the maximum dipole moment among the given options.

Which of the following has the maximum dipole moment?

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Assertion : Molecules of larger size have higher polarizability.
Reason : Polarizability is observed only in those molecules which have a permanent dipole moment.

The dipole moment of $o-$,$p-$ and $m-$dichlorobenzene will be in the order:

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