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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.

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

Similar Questions

The correct order of ionic size of $N^{3-}$,$Na^{+}$,$F^{-}$,$Mg^{2+}$,and $O^{2-}$ is:

Arrange the following elements in the increasing order of their atomic radii:
$(i)$ $O, N, F, B, Be, Li, C$
$(ii)$ $P, S, Mg, Na, Al, Si, Cl$
$(iii)$ $K, Na, Li, Cs, Rb$
$(iv)$ $Cl, F, I, At, Br$

Which of the following atoms or ions has the smallest size?

The single bond covalent radius $(SBCR)$ of $P$ is $0.11 \ nm$. The single bond covalent radius of $Cl$ is:

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

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