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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