In which of the following molecules/ions is t | vedclass

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(C) To determine the hybridization,we use the formula: $	ext{Steric Number} = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electro

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$BF_3, NO_2^{-}$

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(C) To determine the hybridization,we use the formula: $	ext{Steric Number} = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electrons,$M$ is the number of monovalent atoms,$C$ is the cationic charge,and $A$ is the anionic charge.$1$. For $BF_3$: $	ext{Steric Number} = \frac{1}{2} [3 + 3 - 0 + 0] = 3$. This corresponds to $sp^2$ hybridization.$2$. For $NO_2^{-}$: $	ext{Steric Number} = \frac{1}{2} [5 + 0 - 0 + 1] = 3$. This corresponds to $sp^2$ hybridization.$3$. For $H_2O$: $	ext{Steric Number} = \frac{1}{2} [6 + 2 - 0 + 0] = 4$. This corresponds to $sp^3$ hybridization.$4$. For $NH_2^{-}$: $	ext{Steric Number} = \frac{1}{2} [5 + 2 - 0 + 1] = 4$. This corresponds to $sp^3$ hybridization.Thus,both $BF_3$ and $NO_2^{-}$ have $sp^2$ hybridized central atoms.

In which of the following molecules/ions is the central atom $sp^2$ hybridized?

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