Which of the following pairs of molecules is | vedclass

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(A) To be isoelectronic,the species must have the same number of electrons.$NO_3^-: 7 + (3 	imes 8) + 1 = 32 \ e^-$$CO_3^{2-}: 6 + (3 	imes 8) + 2 =

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

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(A) To be isoelectronic,the species must have the same number of electrons.$NO_3^-: 7 + (3 	imes 8) + 1 = 32 \ e^-$$CO_3^{2-}: 6 + (3 	imes 8) + 2 = 32 \ e^-$$ClO_3^-: 17 + (3 	imes 8) + 1 = 42 \ e^-$$SO_3: 16 + (3 	imes 8) = 40 \ e^-$Thus,$NO_3^-$ and $CO_3^{2-}$ are isoelectronic.Both $NO_3^-$ and $CO_3^{2-}$ have a central atom with $sp^2$ hybridization and no lone pairs,resulting in a trigonal planar geometry.Therefore,$NO_3^-$ and $CO_3^{2-}$ are both isoelectronic and isostructural.

Which of the following pairs of molecules is isoelectronic as well as isostructural?

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The pairs among $A = [SO_3^{2-}, CO_3^{2-}]$, $B = [O_2^{2-}, F_2]$, $C = [CN^-, CO]$, $D = [NH_3, H_3O^+]$ and $E = [MnO_4^{2-}, CrO_4^{2-}]$ that do not have similar Lewis dot structures are:

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Arrange the following in the decreasing order of their bond enthalpy: $H_2, O_2, N_2$.

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$NO_3^{-}, CO_3^{2-}, ClO_3^{-}, SO_3, NO_2^{-}$

Chemical bond implies

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