A) \[NO_{3}^{-},CO_{3}^{2-}\]
B) \[S{{O}_{3}},NO_{3}^{-}\]
C) \[ClO_{3}^{-},CO_{3}^{2-}\]
D) \[CO_{3}^{2-},S{{O}_{3}}\]
Correct Answer: A
Solution :
Number of electron in \[NO_{3}^{-}=7+24+1=32\] Number of electron in \[CO_{3}^{2-}=6+24+2=32\] Hence, they are isoelectronic Total number of valence \[{{e}^{-}}\] in \[NO_{3}^{-}\] \[=5+6\times 3+1=24\] Total number of valence \[{{e}^{-}}\] in \[CO_{3}^{2-}\] \[=4+6\times 3+2=24\] Now \[24\div 8=3({{Q}_{1}})+0({{R}_{1}})\] Hence, Hybridisation of central atom in both cases is \[s{{p}^{2}}\]. Hence they are isostructural also.You need to login to perform this action.
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