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(B) molecule has a zero dipole moment if its net dipole moment is zero. This occurs in highly symmetric molecules where the bond dipoles cancel each o

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$CCl_4, BF_3, CO_2, CS_2, 1,4$-dichlorobenzene only

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(B) molecule has a zero dipole moment if its net dipole moment is zero. This occurs in highly symmetric molecules where the bond dipoles cancel each other out.$1$. $CCl_4$: Tetrahedral geometry,all $C-Cl$ bond dipoles cancel. $\mu = 0$.$2$. $BF_3$: Trigonal planar geometry,all $B-F$ bond dipoles cancel. $\mu = 0$.$3$. $CHCl_3$: Asymmetric,$\mu 
eq 0$.$4$. $CS_2$: Linear geometry,$S=C=S$ bond dipoles cancel. $\mu = 0$.$5$. $NH_3$: Pyramidal geometry with a lone pair,$\mu 
eq 0$.$6$. $1,4$-dichlorobenzene: Para-substituted benzene,the two $C-Cl$ bond dipoles are equal and opposite. $\mu = 0$.$7$. $CO_2$: Linear geometry,$O=C=O$ bond dipoles cancel. $\mu = 0$.Thus,the molecules with zero dipole moment are $CCl_4, BF_3, CO_2, CS_2, 1,4$-dichlorobenzene.

The set of molecules among the following with zero dipole moment is $CCl_4$,$BF_3$,$CHCl_3$,$CS_2$,$NH_3$,$1,4$-dichlorobenzene,$CO_2$.

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