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(C) The successive ionization energies are $IE_1 = 191 \ kcal$,$IE_2 = 578 \ kcal$,$IE_3 = 872 \ kcal$,and $IE_4 = 5962 \ kcal$. $A$ large jump in ion

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$3$

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(C) The successive ionization energies are $IE_1 = 191 \ kcal$,$IE_2 = 578 \ kcal$,$IE_3 = 872 \ kcal$,and $IE_4 = 5962 \ kcal$. $A$ large jump in ionization energy occurs between the third and fourth ionization energies $(IE_4 - IE_3 = 5962 - 872 = 5090 \ kcal)$. This indicates that the first three electrons are removed from the valence shell,while the fourth electron is removed from a stable inner shell. Therefore,the element has $3$ valence electrons.

The first four ionisation energy values of an element are $191$,$578$,$872$ and $5962 \ kcal$. The number of valence electrons in the element is :-

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