The successive 5 ionisation energies of an el | vedclass

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Question

(B) The successive ionization energies are $IE_1 = 800 \ kJ/mol$,$IE_2 = 2427 \ kJ/mol$,$IE_3 = 3658 \ kJ/mol$,$IE_4 = 25024 \ kJ/mol$,and $IE_5 = 328

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Group $13$

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(B) The successive ionization energies are $IE_1 = 800 \ kJ/mol$,$IE_2 = 2427 \ kJ/mol$,$IE_3 = 3658 \ kJ/mol$,$IE_4 = 25024 \ kJ/mol$,and $IE_5 = 32824 \ kJ/mol$. There is a large jump in energy between the $3^{rd}$ and $4^{th}$ ionization energy $(IE_4 - IE_3 = 25024 - 3658 = 21366 \ kJ/mol)$. This indicates that the $4^{th}$ electron is being removed from a stable noble gas core. Therefore,the element has $3$ valence electrons,which places it in Group $13$.

The successive $5$ ionisation energies of an element are $800, 2427, 3658, 25024$ and $32824 \ kJ/mol$,respectively. By using the above values,predict the group in which the above element is present:

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