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

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Question

(B) For isoelectronic species,the ionic size decreases as the nuclear charge (atomic number) increases.All these ions have $10$ electrons ($1s^2 2s^2

Vedclass · Accepted Answer

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

Vedclass · Answer

(B) For isoelectronic species,the ionic size decreases as the nuclear charge (atomic number) increases.All these ions have $10$ electrons ($1s^2 2s^2 2p^6$ configuration).The atomic numbers are: $Na (Z=11)$,$Mg (Z=12)$,$Al (Z=13)$,and $Si (Z=14)$.As the nuclear charge increases,the electrostatic attraction between the nucleus and the electrons increases,which pulls the electron cloud closer to the nucleus,resulting in a smaller ionic radius.Therefore,the order of ionic size is $Na^{+} > Mg^{2+} > Al^{3+} > Si^{4+}$.

$Na^{+}$,$Mg^{2+}$,$Al^{3+}$,and $Si^{4+}$ are isoelectronic. Their ionic size follows the order:

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