Increasing order of atomic radii is

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(A) All the given species are isoelectronic,each containing $10 \ e^{-}$.For isoelectronic species,the ionic radius decreases as the nuclear charge (a

Vedclass · Accepted Answer

$Mg^{2+} < Na^{+} < Ne < F^{-} < O^{2-}$

Vedclass · Answer

(A) All the given species are isoelectronic,each containing $10 \ e^{-}$.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.$Mg^{2+}$ $(Z=12)$,$Na^{+}$ $(Z=11)$,$Ne$ $(Z=10)$,$F^{-}$ $(Z=9)$,$O^{2-}$ $(Z=8)$.As the nuclear charge increases,the electrons are pulled more strongly towards the nucleus,resulting in a smaller radius.Therefore,the increasing order of radii is $Mg^{2+} < Na^{+} < Ne < F^{-} < O^{2-}$.

Similar Questions

Assertion $(A)$: $Na^{+}$ and $Mg^{2+}$ ions are isoelectronic but the ionic radius of $Na^{+}$ is greater than that of $Mg^{2+}$.
Reason $(R)$: The effective nuclear charge of $Na^{+}$ ion is less than that of $Mg^{2+}$ ion.

What is the increasing order of atomic radii for $O, C, F, Cl,$ and $Br$?

Which of the following represents the correct order of ionic radii?

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In which of the following options,elements are correctly arranged in the increasing order of their atomic radius?

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