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(D) $(i)$ According to Drago's rule,as the electronegativity of the central atom decreases,the bond angle decreases. Thus,$NH_3 > PH_3 > AsH_3$. The s

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$AsH_3, O_3^+, O_3, SOF_2$

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(D) $(i)$ According to Drago's rule,as the electronegativity of the central atom decreases,the bond angle decreases. Thus,$NH_3 > PH_3 > AsH_3$. The smallest bond angle is in $AsH_3$.$(ii)$ In $O_3$,there is a lone pair on the central oxygen atom,whereas in $O_3^+$,there is a single electron. The lone pair-bond pair repulsion is greater than single electron-bond pair repulsion,leading to a smaller bond angle in $O_3$ compared to $O_3^+$. Thus,$O_3$ has the smallest bond angle.$(iii)$ According to Bent's rule,more electronegative substituents prefer orbitals with more $p$-character. In $NO_2^-$,the $N-O$ bond has more $p$-character than in $O_3$. Consequently,the bond angle in $NO_2^-$ is smaller than in $O_3$.$(iv)$ In $SOF_2$ and $SOCl_2$,the $S-F$ bond is more polar and has more $p$-character than the $S-Cl$ bond. According to Bent's rule,the bond angle decreases as the $p$-character of the bonding orbitals increases. Therefore,$SOF_2$ has a smaller $X-S-X$ bond angle than $SOCl_2$.

Select from each set the molecule or ion having the smallest bond angle:
$(i)$ $NH_3, PH_3$ or $AsH_3$
$(ii)$ $O_3^+, O_3$
$(iii)$ $NO_2^-$ or $O_3$
$(iv)$ $X-S-X$ angle in $SOCl_2$ and $SOF_2$

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Select from each set the molecule or ion having the smallest bond angle:$(i)$ $NH_3, PH_3$ or $AsH_3$$(ii)$ $O_3^+, O_3$$(iii)$ $NO_2^-$ or $O_3$$(iv)$ $X-S-X$ angle in $SOCl_2$ and $SOF_2$