In which of the following species is the bond | vedclass

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(B) In $NH_4^+$,the nitrogen atom undergoes $sp^3$ hybridization and has no lone pair of electrons,resulting in a tetrahedral bond angle of $109^\circ

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$NH_4^+$

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(B) In $NH_4^+$,the nitrogen atom undergoes $sp^3$ hybridization and has no lone pair of electrons,resulting in a tetrahedral bond angle of $109^\circ 28'$. In $NH_3$,the presence of one lone pair reduces the bond angle to $107^\circ$. In $PCl_3$,the bond angle is approximately $100^\circ$ due to the larger size of the central atom and lone pair repulsion. In $SCl_2$,the bond angle is approximately $103^\circ$. Therefore,$NH_4^+$ has the maximum bond angle.

List-$I$ (Species)	List-$II$ (Number of lone pairs of electrons on the central atom)
$(a)$ $XeF_{2}$	$(i)$ $0$
$(b)$ $XeO_{2}F_{2}$	$(ii)$ $1$
$(c)$ $XeO_{3}F_{2}$	$(iii)$ $2$
$(d)$ $XeF_{4}$	$(iv)$ $3$

In which of the following species is the bond angle maximum?

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