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Question

(A) The polarity of a molecule depends on the net dipole moment. $I$ $(CH_4)$ and $IV$ $(CCl_4)$ are symmetric tetrahedral molecules with a net dipole

Vedclass · Accepted Answer

$II > III > V > IV = I$

Vedclass · Answer

(A) The polarity of a molecule depends on the net dipole moment. $I$ $(CH_4)$ and $IV$ $(CCl_4)$ are symmetric tetrahedral molecules with a net dipole moment of $0$,making them non-polar. For the remaining molecules,the polarity depends on the electronegativity difference between the substituents and the central carbon atom. Fluorine is more electronegative than Chlorine,and Chlorine is more electronegative than Hydrogen. Comparing $II$ $(CF_2Cl_2)$,$III$ $(CF_2H_2)$,and $V$ $(CCl_2H_2)$: $II$ $(CF_2Cl_2)$ has the highest dipole moment due to the strong electronegativity of $F$ atoms and the asymmetry. $III$ $(CF_2H_2)$ is more polar than $V$ $(CCl_2H_2)$ because the $C-F$ bond is more polar than the $C-Cl$ bond. Thus,the order of decreasing polarity is $II > III > V > IV = I$.

Arrange the following molecules from most to least polar ($I$,$II$,$III$,$IV$,$V$ respectively): $CH_4$,$CF_2Cl_2$,$CF_2H_2$,$CCl_4$,$CCl_2H_2$.

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