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(D) The first ionization energy $(IE_1)$ of an element is the energy required to remove the first electron,and the second ionization energy $(IE_2)$ i

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$K$

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(D) The first ionization energy $(IE_1)$ of an element is the energy required to remove the first electron,and the second ionization energy $(IE_2)$ is the energy required to remove the second electron.For alkali metals like potassium $(K)$,the electronic configuration is $[Ar] 4s^1$.After the removal of the first electron,it achieves the stable noble gas configuration of argon $([Ar])$.Removing the second electron requires breaking this stable octet,which demands a very high amount of energy.Therefore,the difference between $IE_2$ and $IE_1$ is exceptionally large for alkali metals compared to alkaline earth metals or transition metals.

Element	$A, B, C$
$IE_1$	$400, 550, 1150$
$IE_2$	$2650, 1070, 2090$

The element having the greatest difference between its first and second ionization energies is:

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Element $A, B, C$

$IE_1$ $400, 550, 1150$

$IE_2$ $2650, 1070, 2090$

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