Q. The table gives the first four ionization energies in $kJ \, mol^{- 1}$ of four elements (the letters are not the symbols for the elements). Which element occurs in Group 13 of the periodic table?

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A

$ & IE_{1} & IE_{2} \\ Element \, P & 502 & 4569 \, IE_{3} & IE_{4} \\ 6919 & 9550$

B

$ & IE_{1} & IE_{2} \\ Element \, Q & 526 & 7305 \, IE_{3} & IE_{4} \\ 11822 & -$

C

$ & IE_{1} & IE_{2} \\ Element \, R & 584 & 1823 \, IE_{3} & IE_{4} \\ 2751 & 11584$

D

$ & IE_{1} & IE_{2} \\ Element \, S & 796 & 1583 \, IE_{3} & IE_{4} \\ 3238 & 4362$

Solution:

After losing three electrons in element R, there is sudden huge increase in IE from 2751 to 11584 kJ/mol. It means that after three electrons, some stable configuration is achieved. This is applicable to group 13 elements with outer configuration of $ns^{2}np^{1}$ .

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