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$(C)$ The dipole moment $(\mu)$ depends on the polarity of the bonds and the molecular geometry. $1$. In $trans$-but-$2$-ene and $trans$-$1,2$-dichlor

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$cis$-$1,2$-dichloroethene

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$(C)$ The dipole moment $(\mu)$ depends on the polarity of the bonds and the molecular geometry. $1$. In $trans$-but-$2$-ene and $trans$-$1,2$-dichloroethene, the bond moments cancel each other out due to symmetry, resulting in $\mu = 0 \ D$. $2$. In $cis$-but-$2$-ene, the dipole moment is small $(\mu = 0.33 \ D)$ due to the small difference in electronegativity between $C$ and $H$. $3$. In $cis$-$1,2$-dichloroethene, the $C-Cl$ bonds are highly polar and their dipole moments add up in the same direction, resulting in a high dipole moment of $\mu = 1.89 \ D$. Therefore, $cis$-$1,2$-dichloroethene has the highest dipole moment.

Which one of the following has the highest dipole moment?

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