(A) The electronic configuration of $Be^{2+}$ is $[He]$,$Na^{+}$ is $[Ne]$,$Cl^{-}$ is $[Ar]$ and $Br^{-}$ is $[Kr]$.As we move down the group,the num

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$Br^{-} > Cl^{-} > Na^{+} > Be^{2+}$

(A) The electronic configuration of $Be^{2+}$ is $[He]$,$Na^{+}$ is $[Ne]$,$Cl^{-}$ is $[Ar]$ and $Br^{-}$ is $[Kr]$.As we move down the group,the number of shells increases,leading to an increase in ionic radius.Since $Be^{2+}$ has $2$ shells,$Na^{+}$ has $3$ shells,$Cl^{-}$ has $4$ shells,and $Br^{-}$ has $5$ shells,the order of ionic radii is $Br^{-} > Cl^{-} > Na^{+} > Be^{2+}$.

Class 11 Chemistry Classification of Elements and Periodicity in Properties Atomic and Ionic radii

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Arrange the following ions in the correct order with respect to their ionic radii.

TS EAMCET 2020 All TS EAMCET

A
$Br^{-} > Cl^{-} > Na^{+} > Be^{2+}$
B
$Be^{2+} > Na^{+} > Cl^{-} > Br^{-}$
C
$Cl^{-} > Br^{-} > Na^{+} > Be^{2+}$
D
$Na^{+} > Be^{2+} > Br^{-} > Cl^{-}$

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Class 11

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Classification of Elements and Periodicity in Properties

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Atomic and Ionic radii

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Arrange the following ions in the correct order with respect to their ionic radii.

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