In which of the following arrangements are the ions arranged in decreasing order of ionic size?
The ions F\(^−\),Na\(^+\), Mg\(^{2+}\), Al\(^{3+}\) are isoelectronic species, meaning they all have the same number of electrons (10 electrons). For isoelectronic ions, the ionic size is determined by the nuclear charge (number of protons). As the number of protons increases, the attraction between the nucleus and the electrons becomes stronger, pulling the electrons closer and decreasing the ionic radius.
Order of Protons:
F\(^−\) = 9 protons (Lowest charge → Largest size
Na\(^+\)= 11 protons
Mg\(^{2+}\)=12 protons
Al\(^{3+}\)= 13 protons (Highest charge → Smallest size)
Therefore, the decreasing order of ionic size is F\(^−\), Na\(^+\), Mg\(^{2+}\), Al\(^{3+}\)
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