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(B) The successive ionization enthalpies are given as $IE_1 = 800 \ kJ \ mol^{-1}$,$IE_2 = 2427 \ kJ \ mol^{-1}$,$IE_3 = 3658 \ kJ \ mol^{-1}$,$IE_4 =

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$3$

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(B) The successive ionization enthalpies are given as $IE_1 = 800 \ kJ \ mol^{-1}$,$IE_2 = 2427 \ kJ \ mol^{-1}$,$IE_3 = 3658 \ kJ \ mol^{-1}$,$IE_4 = 25024 \ kJ \ mol^{-1}$,and $IE_5 = 32824 \ kJ \ mol^{-1}$.$A$ large jump in ionization enthalpy indicates the removal of an electron from a stable,noble gas-like inner shell configuration.Comparing the values,we observe a significant increase (jump) between $IE_3$ and $IE_4$ $(25024 - 3658 = 21366 \ kJ \ mol^{-1})$.This indicates that the first $3$ electrons are valence electrons,and the $4^{th}$ electron is removed from a stable inner shell.Therefore,the number of valence electrons in the element is $3$.

The five successive ionization enthalpies of an element are $800, 2427, 3658, 25024$ and $32824 \ kJ \ mol^{-1}$. The number of valence electrons in the element is

Similar Questions

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