The molecule with non-zero dipole moment is

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(D) The dipole moment $(\mu)$ of a molecule depends on its geometry and the polarity of its bonds.$BCl_3$ has a trigonal planar geometry,$BeCl_2$ has

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$NCl_3$

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(D) The dipole moment $(\mu)$ of a molecule depends on its geometry and the polarity of its bonds.$BCl_3$ has a trigonal planar geometry,$BeCl_2$ has a linear geometry,and $CCl_4$ has a tetrahedral geometry. These are highly symmetrical molecules where the individual bond dipoles cancel each other out,resulting in a net dipole moment of $\mu = 0$.$NCl_3$ has a trigonal pyramidal geometry with a lone pair on the nitrogen atom. Due to the presence of the lone pair and the unsymmetrical arrangement of $N-Cl$ bonds,the bond dipoles do not cancel out,resulting in a non-zero net dipole moment $(\mu 
eq 0)$.

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