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2.22 Which of the following are isoelectronic species i.e., those having the same number of electrons?

$\textup{Na}^{+},\ \textup{K}^{+}, \ \textup{Mg}^{2+}, \ \textup{Ca}^{2+}, \ \textup{S}^{2-},\ \textup{Ar}$

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Calculating the number of electrons for each species.

$Na$ has 11 electrons then, $Na^{+}$ will have $(11-1) =10$ electrons.

$K$ has 19 electrons then, $K^{+}$ will have $(19-1) =18$ electrons.

$Mg$ has 12 electrons then, $Mg^{2+}$ will have $(12-2) =10$ electrons.

$Ca$ has 20 electrons then, $Ca^{2+}$ will have $(20-2) =18$ electrons.

$S$ has 16 electrons then, $S^{2-}$ will have $(16+2) =18$ electrons.

$Ar$ has 18 electrons.

Hence, the following are isoelectronic species:

$Na^{+}\ and\ Mg^{2+}$ having 10 electrons each.

$K^{+},\ Ca^{2+}, S^{2-}, and\ Ar$ having 18 electrons each.

Posted by

Divya Prakash Singh

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