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(B) The correct order is $O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$.All these ions are isoelectronic species,meaning they have the same number of e

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$O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$

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(B) The correct order is $O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$.All these ions are isoelectronic species,meaning they have the same number of electrons ($10$ electrons) and the same electronic configuration $(1s^2, 2s^2, 2p^6)$.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.The nuclear charges for these ions are: $O^{2-} (+8)$,$F^{-} (+9)$,$Na^{+} (+11)$,$Mg^{2+} (+12)$,and $Al^{3+} (+13)$.Since the nuclear charge increases from $O^{2-}$ to $Al^{3+}$,the attraction between the nucleus and the electrons increases,leading to a decrease in the ionic radius.

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

Similar Questions

Explain covalent radius and ionic radius with examples.

Which of the following is correct regarding the ionic radii of the given species?

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.

Arrange the following elements in increasing order of their atomic radius: $Na$,$K$,$Mg$,$Rb$.

In the main group elements $(i)$ as we proceed down the same group in the periodic table and $(ii)$ as we proceed from left to right in the same period,the atomic radius

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