What is the increasing order of dipole moment | vedclass

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Question

(A) The dipole moment $(\mu)$ depends on the polarity of bonds and the bond angle.$(iv)$ $p$-dichlorobenzene: The two $C-Cl$ bonds are at $180^{\circ}

Vedclass · Accepted Answer

$IV < I < II < III$

Vedclass · Answer

(A) The dipole moment $(\mu)$ depends on the polarity of bonds and the bond angle.$(iv)$ $p$-dichlorobenzene: The two $C-Cl$ bonds are at $180^{\circ}$, so their dipole moments cancel out, $\mu = 0$.$(i)$ Toluene: It has a small dipole moment due to the electron-donating methyl group, $\mu \approx 0.4 \ D$.$(ii)$ $m$-dichlorobenzene: The bond angle is $120^{\circ}$, resulting in a net dipole moment.$(iii)$ $o$-dichlorobenzene: The bond angle is $60^{\circ}$, which results in the highest dipole moment among the isomers due to the vector addition of the two $C-Cl$ bond dipoles.Thus, the increasing order is $IV < I < II < III$.

What is the increasing order of dipole moment for the following compounds? $(i)$ Toluene $(ii)$ $m$-dichlorobenzene $(iii)$ $o$-dichlorobenzene $(iv)$ $p$-dichlorobenzene

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