Na^+,Mg^{2+},Al^{3+},and Si^{4+} are isoelect | vedclass

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Question

(C) For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases. All the given ions ($Na^+$,$Mg^{2+}$,$Al^{3+

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$Na^+ > Mg^{2+} > Al^{3+} > Si^{4+}$

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(C) For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases. All the given ions ($Na^+$,$Mg^{2+}$,$Al^{3+}$,$Si^{4+}$) have $10$ electrons. The atomic numbers are: $Na (11)$,$Mg (12)$,$Al (13)$,and $Si (14)$. As the nuclear charge increases,the electrostatic attraction between the nucleus and the electrons increases,causing the ionic radius to decrease. Therefore,the order of ionic radii is $Na^+ > Mg^{2+} > Al^{3+} > Si^{4+}$.

Ion	Radius $(pm)$
$Q^{a+}$	$53$
$X^{b+}$	$66$
$Y^{c+}$	$40$
$Z^{d+}$	$100$

$Na^+$,$Mg^{2+}$,$Al^{3+}$,and $Si^{4+}$ are isoelectronic. What is the order of their ionic radii?

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