Which of the following options represents the | vedclass

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(C) The species $N^{3-}, O^{2-}$, and $F^{-}$ are isoelectronic, meaning they all contain $10$ electrons.For isoelectronic species, the ionic radius d

Vedclass · Accepted Answer

$1.71, 1.40$ and $1.36$

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(C) The species $N^{3-}, O^{2-}$, and $F^{-}$ are isoelectronic, meaning they all contain $10$ electrons.For isoelectronic species, the ionic radius decreases as the nuclear charge (number of protons) increases.$N^{3-}$ has $7$ protons, $O^{2-}$ has $8$ protons, and $F^{-}$ has $9$ protons.Since the nuclear charge increases from $N^{3-}$ to $F^{-}$, the attraction between the nucleus and the electrons increases, leading to a decrease in ionic size.Therefore, the correct order of ionic radii is $N^{3-} (1.71 \mathring{A}) > O^{2-} (1.40 \mathring{A}) > F^{-} (1.36 \mathring{A})$.

Which of the following options represents the correct ionic radii in $\mathring{A}$ of $N^{3-}, O^{2-}$ and $F^{-}$, respectively?

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