Which of the following has the smallest size?

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(D) All the given ions ($Na^{+}$,$Mg^{2+}$,$Al^{3+}$,$Si^{4+}$) are isoelectronic,meaning they all have $10$ electrons.For isoelectronic species,the i

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$Si^{4+}$

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(D) All the given ions ($Na^{+}$,$Mg^{2+}$,$Al^{3+}$,$Si^{4+}$) are isoelectronic,meaning they all have $10$ electrons.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.The atomic numbers are: $Na$ $(Z=11)$,$Mg$ $(Z=12)$,$Al$ $(Z=13)$,and $Si$ $(Z=14)$.Since $Si^{4+}$ has the highest nuclear charge $(Z=14)$,it exerts the strongest attraction on the electrons,resulting in the smallest ionic size.Therefore,the correct option is $(D)$.

$Column\, A$ (ion)	$Column\, B$ (radius)
$(i)$ $Li^{+}$	$(p)$ $216\, pm$
$(ii)$ $Na^{+}$	$(q)$ $195\, pm$
$(iii)$ $Br^{-}$	$(r)$ $60\, pm$
$(iv)$ $I^{-}$	$(s)$ $95\, pm$

Similar Questions

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 represents the correct order of atomic radii?

Between $Mg$ and $Mg^{2+}$,which has a smaller size? Why?

The reason for a cation to be smaller than its parent atom is

Match $Column\, A$ with $Column\, B$:
$Column\, A$ (ion) $Column\, B$ (radius)
$(i)$ $Li^{+}$ $(p)$ $216\, pm$
$(ii)$ $Na^{+}$ $(q)$ $195\, pm$
$(iii)$ $Br^{-}$ $(r)$ $60\, pm$
$(iv)$ $I^{-}$ $(s)$ $95\, pm$

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