Which of the following species are isostructu | vedclass

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(D) To determine if species are isostructural,we calculate the hybridization and the number of lone pairs on the central atom.$1$. $NO^{-}_3$: Central

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Both $b$ and $c$

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(D) To determine if species are isostructural,we calculate the hybridization and the number of lone pairs on the central atom.$1$. $NO^{-}_3$: Central atom $N$ has $5$ valence electrons. Hybridization = $\frac{1}{2}(5 + 1 + 0) = 3$ $(sp^2)$. It has $0$ lone pairs. Geometry: Trigonal planar.$2$. $CO^{2-}_3$: Central atom $C$ has $4$ valence electrons. Hybridization = $\frac{1}{2}(4 + 2 + 0) = 3$ $(sp^2)$. It has $0$ lone pairs. Geometry: Trigonal planar.$3$. $SO_3$: Central atom $S$ has $6$ valence electrons. Hybridization = $\frac{1}{2}(6 + 0 + 0) = 3$ $(sp^2)$. It has $0$ lone pairs. Geometry: Trigonal planar.$4$. $ClO^{-}_3$: Central atom $Cl$ has $7$ valence electrons. Hybridization = $\frac{1}{2}(7 + 1 + 0) = 4$ $(sp^3)$. It has $1$ lone pair. Geometry: Pyramidal.Since $NO^{-}_3, CO^{2-}_3,$ and $SO_3$ all have $sp^2$ hybridization and $0$ lone pairs,they are isostructural (trigonal planar). Therefore,both $b$ and $c$ are correct pairs.

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

Which of the following species are isostructural: $NO^{-}_3, CO^{2-}_3, ClO^{-}_3,$ and $SO_3$?

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