The following table shows the successive molar ionization energy `(kJ mol^(-1))` of five elements A to E

Which of two elements are most likely to be in the same group of the periodic table ?

Options

A. C and D
B. D and E
C. B and D
D. B and E

Answer

D

Explanation

In both elements B and E, `Delta_(i)H_(1)` are quite low but their `Delta_(i)H_(2) ` are quite large. This means that after the loss of first electron some stable (i.e., inert gas ) configuration is achieved. Therefore both of these belong to the same group (i.e., alkali metals ) of the periodic table . So option ( d) is correct.