In which of the following pairs do both the s | vedclass

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(C) To determine the hybridization,we calculate the number of electron pairs around the central atom using the formula: $	ext{Number of electron pair

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$NF_{3}, H_{2}O$

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(C) To determine the hybridization,we calculate the number of electron pairs around the central atom using the formula: $	ext{Number of electron pairs} = 	ext{Number of bond pairs} + 	ext{Number of lone pairs}$.For $NF_{3}$: The central atom $N$ has $3$ bond pairs and $1$ lone pair,totaling $4$ electron pairs,which corresponds to $sp^{3}$ hybridization.For $H_{2}O$: The central atom $O$ has $2$ bond pairs and $2$ lone pairs,totaling $4$ electron pairs,which corresponds to $sp^{3}$ hybridization.Since both $NF_{3}$ and $H_{2}O$ have $4$ electron pairs,both are $sp^{3}$ hybridized.

In which of the following pairs do both the species have $sp^{3}$ hybridization?

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