Which of the following has the largest ionic | vedclass

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(B) The ionic radius increases as we move down a group in the periodic table due to the addition of new electron shells. $Na^{+}$ and $Mg^{2+}$ belong

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$Cs^{+}$

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(B) The ionic radius increases as we move down a group in the periodic table due to the addition of new electron shells. $Na^{+}$ and $Mg^{2+}$ belong to the $3^{rd}$ period,while $Ca^{2+}$ belongs to the $4^{th}$ period and $Cs^{+}$ belongs to the $6^{th}$ period. Since $Cs^{+}$ has the highest number of electron shells (principal quantum number $n=6$),it has the largest ionic radius among the given options.

Which of the following has the largest ionic radius?

Similar Questions

The incorrect decreasing order of atomic radii is:

The ions $O^{2-}, F^{-}, Na^{+}, Mg^{2+}$ and $Al^{3+}$ are isoelectronic. Their ionic radii show

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

The ionic radii of $Li^{+}$,$Be^{2+}$,and $B^{3+}$ follow the order:

The smallest among the following ions is

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