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The minimum amount of energy required to remove the most loosely bound electron from an isolated atom
\( \mathrm{P} \) in the gaseous state is known as ionisation energy or

W. first ionisation energy or ionisation enthalpy (IE \( { }_{1} \) ) of the element. The energy required to remove the second electron from the monvalent cation is called second ionisation enthalpy ( \( \left.\mathrm{IE}_{2}\right) \). Similarly, we have third, fourth ..... ionistion enthalpies. The values of ionisation energy depends on a number of factors such as (i) size of the atom (ii) screening effect (iii) nuclear charge (iv) half filled and fully filled orbitals.
In a group, the ionisation energy decreases from top to bottom. In a period, the value of ionisation energy increases from left to right which breaks where atoms have somewhat stable configurations.

Compared to the second ionisation energy ( \( \mathrm{IE}_{2} \) ) of an atom, the third ionisation energy \( \left(\mathrm{IE}_{3}\right) \) is
(A) The same
(B) Greater
(C) Smaller
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