Which of the following has the maximum bond a | vedclass

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(B) $1$. In $NH_3$,the nitrogen atom is $sp^3$ hybridized with one lone pair,resulting in a bond angle of approximately $107^{\circ}$.$2$. In $NH_4^+$

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$NH_4^+$

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(B) $1$. In $NH_3$,the nitrogen atom is $sp^3$ hybridized with one lone pair,resulting in a bond angle of approximately $107^{\circ}$.$2$. In $NH_4^+$,the nitrogen atom is $sp^3$ hybridized with no lone pairs,resulting in a perfect tetrahedral geometry with a bond angle of $109.5^{\circ}$.$3$. In $PCl_3$,the phosphorus atom is $sp^3$ hybridized with one lone pair,and due to the larger size of the $P$ atom and $Cl$ atoms,the bond angle is approximately $100^{\circ}$.$4$. In $SCl_2$,the sulfur atom is $sp^3$ hybridized with two lone pairs,resulting in a bent geometry with a bond angle of approximately $103^{\circ}$.$5$. Comparing these,$NH_4^+$ has the largest bond angle of $109.5^{\circ}$.

Which of the following has the maximum bond angle?

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