Two p-block elements X and Y form fluorides o | vedclass

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(B) Lewis acid is an electron-deficient species. $BF_3$ is a $p$-block fluoride where Boron has an incomplete octet ($6$ electrons), making it a Lewis

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$sp^2$ and $sp^3$

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(B) Lewis acid is an electron-deficient species. $BF_3$ is a $p$-block fluoride where Boron has an incomplete octet ($6$ electrons), making it a Lewis acid. Its hybridization is $sp^2$ due to $3$ bond pairs and $0$ lone pairs.$YF_3$ acts as a Lewis base because the central atom has a lone pair of electrons available for donation. $NF_3$ is a $p$-block fluoride where Nitrogen has $3$ bond pairs and $1$ lone pair, making it a Lewis base. Its hybridization is $sp^3$ due to $4$ electron domains ($3$ bond pairs + $1$ lone pair).Therefore, the hybridization of $XF_3$ $(BF_3)$ is $sp^2$ and $YF_3$ $(NF_3)$ is $sp^3$.

Two $p$-block elements $X$ and $Y$ form fluorides of the type $EF_3$. The fluoride compound $XF_3$ is a Lewis acid and $YF_3$ is a Lewis base. The hybridization of the central atoms of $XF_3$ and $YF_3$ respectively are

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