Which of the following pairs are isoelectroni | vedclass

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(A) To be isoelectronic,species must have the same number of electrons.To be isostructural,species must have the same hybridization and geometry.$1$.

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$NO_3^{-}, CO_3^{2-}$

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(A) To be isoelectronic,species must have the same number of electrons.To be isostructural,species must have the same hybridization and geometry.$1$. $NO_3^{-}$: Electrons = $7 + (3 	imes 8) + 1 = 32$. Hybridization = $sp^2$,Geometry = Trigonal planar.$2$. $CO_3^{2-}$: Electrons = $6 + (3 	imes 8) + 2 = 32$. Hybridization = $sp^2$,Geometry = Trigonal planar.$3$. $ClO_3^{-}$: Electrons = $17 + (3 	imes 8) + 1 = 42$. Hybridization = $sp^3$,Geometry = Trigonal pyramidal.$4$. $SO_3$: Electrons = $16 + (3 	imes 8) = 40$. Hybridization = $sp^2$,Geometry = Trigonal planar.$5$. $NO_2^{-}$: Electrons = $7 + (2 	imes 8) + 1 = 24$. Hybridization = $sp^2$,Geometry = Bent.Comparing these,$NO_3^{-}$ and $CO_3^{2-}$ both have $32$ electrons and are trigonal planar.

Which of the following pairs are isoelectronic and isostructural?
$NO_3^{-}, CO_3^{2-}, ClO_3^{-}, SO_3, NO_2^{-}$

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Which of the following pairs are isoelectronic and isostructural?$NO_3^{-}, CO_3^{2-}, ClO_3^{-}, SO_3, NO_2^{-}$