A) \[\text{Fe}\,\text{}\,\text{F}{{\text{e}}^{2+}}<F{{e}^{3+}}\]
B) \[F{{e}^{2+}}<F{{e}^{3+}}<Fe\]
C) \[Fe<F{{e}^{3+}}<F{{e}^{2+}}\]
D) \[F{{e}^{3+}}<F{{e}^{2+}}<Fe\]
Correct Answer: D
Solution :
Atomic or ionic radius\[\propto \frac{\text{1}}{\text{Effective}\,\text{nuclear}\,\text{charge}}\] As the effective nuclear charge increase, size decreases, \[\text{+ve}\] charge is increased when electrons are removed. As the electrons are removed the attraction of nucleus on the remaining electrons (effective nuclear charge) increases thats why the atomic or ionic radius decreases. So, the correct order will be: \[\text{Fe}\,\text{}\,F{{e}^{2+}}>F{{e}^{3+}}\]or \[F{{e}^{3+}}<F{{e}^{2+}}<Fe\]
You need to login to perform this action.
You will be redirected in
3 sec
