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(A) The dipole moment of a molecule depends on the vector sum of the individual bond dipoles. For $1,4$-dichlorobenzene $(D)$,the two $C-Cl$ bond dipo

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$1,2,4$-trichlorobenzene

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(A) The dipole moment of a molecule depends on the vector sum of the individual bond dipoles. For $1,4$-dichlorobenzene $(D)$,the two $C-Cl$ bond dipoles are equal and opposite,so they cancel each other out,resulting in a net dipole moment of $0 \ D$. For $1,3,5$-trichlorobenzene $(C)$,the three $C-Cl$ bond dipoles are oriented at $120^\circ$ to each other,and their vector sum is also $0$. For $1,2,3$-trichlorobenzene $(B)$,the dipole moments of the two outer $Cl$ atoms partially cancel the dipole of the middle $Cl$ atom,but they do not cancel completely. For $1,2,4$-trichlorobenzene $(A)$,the arrangement of the three $Cl$ atoms results in a significant net dipole moment because the vectors do not cancel each other out as effectively as in the other isomers. Therefore,$1,2,4$-trichlorobenzene has the maximum dipole moment.

Which of the following molecules has the maximum dipole moment?

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