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(C) All the given species are isoelectronic,meaning they all contain $10$ electrons.For isoelectronic species,the ionic radius decreases as the nuclea

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$Si^{4+}$

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(C) All the given species are isoelectronic,meaning they all contain $10$ electrons.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.As the positive charge on the cation increases,the effective nuclear charge increases,which pulls the electrons closer to the nucleus,resulting in a smaller size.Among the given species,$Si^{4+}$ has the highest atomic number $(Z = 14)$ and the highest positive charge,therefore it has the smallest size.

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

Which among the following isoelectronic species has the smallest size?
$O^{2-}, F^{-}, Ne, Na^{+}, Mg^{2+}, Al^{3+}, Si^{4+}$

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Which of the following has the largest ionic radius?

Which of the following is the correct increasing order of ionic radii for $Na, Rb, K,$ and $Mg$?

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

Identify the correct order in which the covalent radius of the following elements increases: $(I) \ Ti, (II) \ Ca, (III) \ Sc$.

Consider the following species: $N^{3-}, O^{2-}, F^{-}, Na^{+}, Mg^{2+}, Al^{3+}$
$(a)$ What is common in them?
$(b)$ Arrange them in the order of increasing ionic radii.

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Which among the following isoelectronic species has the smallest size?$O^{2-}, F^{-}, Ne, Na^{+}, Mg^{2+}, Al^{3+}, Si^{4+}$