An element has successive ionization enthalpi | vedclass

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(C) The successive ionization enthalpies are: $IE_1 = 940$,$IE_2 = 2080$,$IE_3 = 3090$,$IE_4 = 4140$,$IE_5 = 7030$,$IE_6 = 7870$,$IE_7 = 16000$,$IE_8

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$16$

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(C) The successive ionization enthalpies are: $IE_1 = 940$,$IE_2 = 2080$,$IE_3 = 3090$,$IE_4 = 4140$,$IE_5 = 7030$,$IE_6 = 7870$,$IE_7 = 16000$,$IE_8 = 19500 \, kJ \, mol^{-1}$.We observe the jump in ionization energy by calculating the differences: $IE_2 - IE_1 = 1140$$IE_3 - IE_2 = 1010$$IE_4 - IE_3 = 1050$$IE_5 - IE_4 = 2890$$IE_6 - IE_5 = 840$$IE_7 - IE_6 = 8130$$A$ large jump in ionization energy occurs between the $6^{th}$ and $7^{th}$ ionization enthalpies,indicating that the $7^{th}$ electron is being removed from a stable inner shell.This implies the element has $6$ valence electrons.Elements with $6$ valence electrons belong to group $16$ of the periodic table.

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