A) magnesium
B) boron
C) beryllium
D) aluminium
Correct Answer: C
Solution :
The electronic configuration of the given elements is as \[_{12}Mg=[Ne]\,\,3{{s}^{2}}\] \[_{5}B=[He]\,2{{s}^{2}},2\,{{p}^{1}}\] \[_{4}Be=[He]\,2{{s}^{2}}\] \[_{13}Al=[Ne]\,\,3{{s}^{2}}3{{p}^{1}}\] From the electronic configuration, it is clear that third ionisation energy of Mg and Be is higher as compared to Al and B as in them the third electron have to be removed from the stable inert gas configuration. Between Mg and Be, third IE of Be is higher because of its smaller size.
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