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(C) molecule shows a dipole moment if it has a net non-zero dipole moment due to its geometry and the electronegativity difference between atoms.$CH_4

Vedclass · Accepted Answer

Chloroform

Vedclass · Answer

(C) molecule shows a dipole moment if it has a net non-zero dipole moment due to its geometry and the electronegativity difference between atoms.$CH_4$ (Methane) and $CCl_4$ (Carbon tetrachloride) have a tetrahedral geometry,which results in the cancellation of individual bond dipoles,leading to a net dipole moment of $0$.$CO_2$ (Carbon dioxide) is a linear molecule where the two $C=O$ bond dipoles cancel each other out,resulting in a net dipole moment of $0$.$CHCl_3$ (Chloroform) has a tetrahedral geometry,but because the atoms attached to the central carbon are not identical ($3$ $Cl$ atoms and $1$ $H$ atom),the bond dipoles do not cancel out,resulting in a net dipole moment. Thus,the correct option is $(C)$.

Which of the following molecules will show a dipole moment?

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