A) an increase from \[{{O}^{2-}}\] to F- and then decrease from \[N{{a}^{+}}\] to \[A{{l}^{3+}}\]
B) a decrease from \[{{O}^{2-}}\] to F- and then increase from \[N{{a}^{+}}\] to \[A{{l}^{3+}}\]
C) a significant increase from \[{{O}^{2-}}\] to \[A{{l}^{3+}}\]
D) a significant decrease from \[{{O}^{2-}}\] to \[A{{l}^{3+}}\]
Correct Answer: D
Solution :
On increasing atomic number of isoelectronic species ionic radii decreases due to increasing the effective nuclear charge \[({{Z}_{eff}})\] Radius \[\propto \,\,\frac{1}{{{Z}_{eff}}}\] So, by increasing the -ve charge ionic radii increases and by increasing the +ve charge ionic radii decreases. Hence, order of radii \[{{O}^{2-}}>{{F}^{-}}>N{{a}^{+}}>M{{g}^{2+}}>A{{l}^{3+}}\]
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