The correct order of increasing ionic radii i | vedclass

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Question

(A) The given ions $N^{3-}$,$O^{2-}$,$F^{-}$,$Na^{+}$,and $Mg^{2+}$ are isoelectronic species,as each contains $10$ electrons.For isoelectronic specie

Vedclass · Accepted Answer

$Mg^{2+} < Na^{+} < F^{-} < O^{2-} < N^{3-}$

Vedclass · Answer

(A) The given ions $N^{3-}$,$O^{2-}$,$F^{-}$,$Na^{+}$,and $Mg^{2+}$ are isoelectronic species,as each contains $10$ electrons.For isoelectronic species,the ionic radius increases as the nuclear charge (atomic number) decreases.The atomic numbers are: $N(7)$,$O(8)$,$F(9)$,$Na(11)$,$Mg(12)$.Since the nuclear charge follows the order $N O^{2-} > F^{-} > Na^{+} > Mg^{2+}$.Therefore,the correct order of increasing ionic radii is $Mg^{2+} < Na^{+} < F^{-} < O^{2-} < N^{3-}$.

The correct order of increasing ionic radii is .... .

Similar Questions

If the ionic radii of $K^{+}$ and $F^{-}$ are nearly the same (i.e.,$1.34 \ \mathring{A}$),then the atomic radii of $K$ and $F$ respectively are

The correct order of radii is

Assertion $(A)$: The ionic radii of $Na^{+}$ and $F^{-}$ are same.
Reason $(R)$: Both $Na^{+}$ and $F^{-}$ are isoelectronic species.
The correct answer is:

Which of the following orders is incorrect for ionic size?

Which one of the following species possesses maximum size?

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