Which of the following compounds is polar and | vedclass

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(A) $1$. Analyze the hybridization and polarity of each compound:- $H_2CO_3$: The central carbon atom is bonded to three oxygen atoms (one double bond

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$H_2CO_3$

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(A) $1$. Analyze the hybridization and polarity of each compound:- $H_2CO_3$: The central carbon atom is bonded to three oxygen atoms (one double bond,two single bonds). It has $3$ sigma bonds and $0$ lone pairs,resulting in $sp^2$ hybridization. Due to the difference in electronegativity between $C$,$O$,and $H$,the molecule is polar.- $SiF_4$: The central silicon atom has $4$ sigma bonds and $0$ lone pairs,resulting in $sp^3$ hybridization. It is non-polar due to its tetrahedral geometry.- $BF_3$: The central boron atom has $3$ sigma bonds and $0$ lone pairs,resulting in $sp^2$ hybridization. It is non-polar due to its symmetrical trigonal planar geometry.- $HClO_4$: The central chlorine atom is bonded to four oxygen atoms,resulting in $sp^3$ hybridization.$2$. Conclusion: $H_2CO_3$ is the only compound that is polar and has a central atom with $sp^2$ hybridization.

Which of the following compounds is polar and has a central atom with $sp^2$ hybridization?

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