Which of the following orders is incorrect fo | vedclass

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(D) Ionic size depends on the number of shells and the effective nuclear charge. $1$. For $Se^{-2} > Cl^{-} > O^{-2} > Na^{+}$,the order is correct as

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$S^{-2} > Ca^{+2} > K^{+} > Ba^{+2}$

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(D) Ionic size depends on the number of shells and the effective nuclear charge. $1$. For $Se^{-2} > Cl^{-} > O^{-2} > Na^{+}$,the order is correct as $Se^{-2}$ and $Cl^{-}$ have $4$ and $3$ shells respectively,while $O^{-2}$ and $Na^{+}$ are isoelectronic with $10$ electrons but $O^{-2}$ has a smaller nuclear charge than $Na^{+}$. $2$. For $Li^{+} > Mg^{+2} > Al^{+3}$,the order is correct as $Li^{+}$ has $2$ shells,while $Mg^{+2}$ and $Al^{+3}$ have $3$ shells,but $Mg^{+2}$ is larger than $Al^{+3}$ due to lower nuclear charge. $3$. For $P^{-3} > N^{-3} > Mg^{+2}$,the order is correct as $P^{-3}$ has $3$ shells,$N^{-3}$ has $2$ shells,and $Mg^{+2}$ has $2$ shells with higher nuclear charge than $N^{-3}$. $4$. For $S^{-2} > Ca^{+2} > K^{+} > Ba^{+2}$,this is incorrect because $Ba^{+2}$ has $5$ shells,making it significantly larger than $S^{-2}$ ($3$ shells),$Ca^{+2}$ ($3$ shells),and $K^{+}$ ($3$ shells).

Which of the following orders is incorrect for ionic size?

Similar Questions

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

Identify the correct orders regarding atomic radii:
$i$. $Cl > F > Li$
$ii$. $P > C > N$
$iii$. $Tm > Sm > Eu$
$iv$. $Sr > Ca > Mg$

Which of the following is the correct order of ionic radii for ${N^{3-}}, {O^{2-}}, {F^-},$ and ${Na^+}$?

The ionic radii of $N^{3-}$,$O^{2-}$,$F^{-}$,and $Na^{+}$ follow the order:

The ionic sizes decrease in the order :-

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