Which of the following has the smallest bond | vedclass

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(B) To determine the bond angle,we look at the hybridization and the number of lone pairs on the central atom: $1$. $BeF_2$: $sp$ hybridization,linear

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$H_2O$

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(B) To determine the bond angle,we look at the hybridization and the number of lone pairs on the central atom: $1$. $BeF_2$: $sp$ hybridization,linear geometry,bond angle = $180^{\circ}$. $2$. $CH_4$: $sp^3$ hybridization,tetrahedral geometry,bond angle = $109.5^{\circ}$. $3$. $NH_3$: $sp^3$ hybridization,one lone pair,bond angle = $107^{\circ}$. $4$. $H_2O$: $sp^3$ hybridization,two lone pairs,bond angle = $104.5^{\circ}$. Due to the presence of two lone pairs on the oxygen atom in $H_2O$,the lone pair-lone pair repulsion is greater than the lone pair-bond pair repulsion,which compresses the bond angle to $104.5^{\circ}$,the smallest among the given options.

Which of the following has the smallest bond angle?

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