The ionic radii (mathring{A}) of C^{4-} and O | vedclass

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(C) $C^{4-}$,$N^{3-}$,and $O^{2-}$ are isoelectronic species,all having $10$ electrons.The ionic radius of isoelectronic species decreases as the nucl

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$1.71$

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(C) $C^{4-}$,$N^{3-}$,and $O^{2-}$ are isoelectronic species,all having $10$ electrons.The ionic radius of isoelectronic species decreases as the nuclear charge (atomic number) increases.The atomic numbers are: $C (6)$,$N (7)$,and $O (8)$.Therefore,the order of ionic radii is: $C^{4-} > N^{3-} > O^{2-}$.Given the values $2.60 \ \mathring{A}$ for $C^{4-}$ and $1.40 \ \mathring{A}$ for $O^{2-}$,the value for $N^{3-}$ must lie between $1.40$ and $2.60$.Among the given options,$1.71 \ \mathring{A}$ is the correct value.

The ionic radii $(\mathring{A})$ of $C^{4-}$ and $O^{2-}$ respectively are $2.60$ and $1.40$. The ionic radius of the isoelectronic ion $N^{3-}$ would be........$\mathring{A}$

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