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

Vedclass · Accepted Answer

$1.71$

Vedclass · Answer

(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........$\mathring{A}$

Similar Questions

Which of the following radius order is not correct?

Consider the following species: $N^{3-}, O^{2-}, F^{-}, Na^{+}, Mg^{2+}, Al^{3+}$
$(a)$ What is common in them?
$(b)$ Arrange them in the order of increasing ionic radii.

In which of the following ionic pairs,is the second ion smaller in size than the first ion?

The correct order of ionic size of $N^{3-}$,$Na^{+}$,$F^{-}$,$Mg^{2+}$,and $O^{2-}$ is:

Which of the following species is the smallest in size?

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