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(D) The successive ionisation energies are given as: $IE_1 = 165 \ kcal$,$IE_2 = 190 \ kcal$,$IE_3 = 550 \ kcal$,and $IE_4 = 595 \ kcal$. There is a l

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$[Ne] 3s^2$

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(D) The successive ionisation energies are given as: $IE_1 = 165 \ kcal$,$IE_2 = 190 \ kcal$,$IE_3 = 550 \ kcal$,and $IE_4 = 595 \ kcal$. There is a large jump in ionisation energy between the second $(IE_2)$ and third $(IE_3)$ ionisation energies ($190 \ kcal$ to $550 \ kcal$). This significant increase indicates that the first two electrons are removed from the valence shell,and the third electron is removed from a more stable,inner shell. Therefore,the element $A$ has $2$ valence electrons. Among the given options,the configuration $[Ne] 3s^2$ corresponds to an element with $2$ valence electrons.

If the successive ionisation energies of an element $A$ are $165$,$190$,$550$ and $595 \ kcal$,respectively,then the ground state electronic configuration of element $A$ is

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