A) Sr
B) As
C) Xe
D) S
Correct Answer: A
Solution :
The electronic configuration of the given elements are as \[_{38}Sr=[Kr]\,5{{s}^{2}}\] \[33As=[Ar]\,3{{d}^{10}}4{{s}^{2}}4{{p}^{3}}\] \[_{54}Xe=5{{s}^{2}}5{{p}^{6}}\] \[S=[Ne]\,3{{s}^{2}}3{{p}^{4}}\] As the distance of outer electron from nucleus (n) increases, it becomes very easy to remove an electron. Thus, ionisation potential decreases. Hence, ionisation potential of Sr is lowest among the given elements. (Xe has the completely filled shell, that's why it requires a large amount of energy to release an electron).
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