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(A) The dipole moment of a molecule depends on the vector sum of individual bond dipoles and the molecular geometry.$CCl_4$ is a tetrahedral molecule

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$CH_3Cl$

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(A) The dipole moment of a molecule depends on the vector sum of individual bond dipoles and the molecular geometry.$CCl_4$ is a tetrahedral molecule with a symmetric structure,resulting in a net dipole moment of $0 \ D$.In $CH_3Cl$,$CH_2Cl_2$,and $CHCl_3$,the $C-Cl$ bond is polar due to the high electronegativity of chlorine.$CH_3Cl$ has the highest dipole moment $(1.86 \ D)$ because the bond dipoles of the $C-H$ bonds and the $C-Cl$ bond reinforce each other in the same direction.As more $Cl$ atoms are substituted,the vector sum of the bond dipoles decreases due to the opposing directions of the $C-Cl$ bond moments.Therefore,the correct order of dipole moment is $CH_3Cl > CH_2Cl_2 > CHCl_3 > CCl_4$.

Among the following,the molecule with the highest dipole moment is

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