Choose the polar molecule from the following:

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(D) molecule is polar if it has a net dipole moment,i.e.,$\mu 
eq 0$.$1$. $CCl_4$ has a tetrahedral geometry where the bond dipoles of four $C-Cl$ bo

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$CHCl_3$

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(D) molecule is polar if it has a net dipole moment,i.e.,$\mu 
eq 0$.$1$. $CCl_4$ has a tetrahedral geometry where the bond dipoles of four $C-Cl$ bonds cancel each other out,making it non-polar $(\mu = 0)$.$2$. $CO_2$ is a linear molecule where the two $C=O$ bond dipoles are equal and opposite,canceling each other out,making it non-polar $(\mu = 0)$.$3$. $CH_2=CH_2$ (ethene) is a planar molecule with a symmetric distribution of charge,making it non-polar $(\mu = 0)$.$4$. $CHCl_3$ (chloroform) has a tetrahedral geometry,but due to the presence of three $Cl$ atoms and one $H$ atom,the bond dipoles do not cancel each other out. Thus,it has a net dipole moment $(\mu 
eq 0)$ and is a polar molecule.

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