$I E_{2}$ for an element is invariably higher than $I E_{1}$ because

The size of cations is smaller than its atom

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It is difficult to remove electron from cations

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Ionization energy is endothermic

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All of the above

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Solution

The correct options are
A The size of cations is smaller than its atom
B It is difficult to remove electron from cations
$I E_{2}$ is greater than $I E_{1}$ for an element because the size of the cation is smaller than its atoms so $Z_{e f f}$ is more for cation as result it is harder to remove a negatively charged electron from the positively charged cation.

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