Statement (A) CO_2 has no dipole moment,where | vedclass

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(C) Statement $(A)$: $CO_2$ has a linear geometry,so the bond dipoles cancel each other,resulting in a net dipole moment of $0$. $SO_2$ has a bent geo

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Both $(A)$ and $(B)$ are correct

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(C) Statement $(A)$: $CO_2$ has a linear geometry,so the bond dipoles cancel each other,resulting in a net dipole moment of $0$. $SO_2$ has a bent geometry due to the presence of a lone pair on $S$,and $H_2O$ has a bent geometry due to two lone pairs on $O$,so both have a non-zero net dipole moment. Thus,Statement $(A)$ is correct.Statement $(B)$: According to Fajan's rule,the polarizing power of a cation increases with its charge. $Sn^{4+}$ has a higher charge than $Sn^{2+}$,so $SnCl_4$ exhibits significant covalent character,whereas $SnCl_2$ is predominantly ionic. Thus,Statement $(B)$ is correct.

Statement $(A)$ $CO_2$ has no dipole moment,whereas $SO_2$ and $H_2O$ have dipole moment.
Statement $(B)$ $SnCl_2$ is ionic,whereas $SnCl_4$ is covalent.
Which of the following is correct?

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Statement $(A)$ $CO_2$ has no dipole moment,whereas $SO_2$ and $H_2O$ have dipole moment.Statement $(B)$ $SnCl_2$ is ionic,whereas $SnCl_4$ is covalent.Which of the following is correct?