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The minimum amount of energy required to remove the most loosely bound electron from an isolated atom in the gaseous state is known as ionisation energy or
P
W 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.

The first \( \left(\mathrm{IE}_{1}\right) \) and second \( \left(\mathrm{IE}_{2}\right) \) ionisation energies \( \left(\mathrm{kJ} \mathrm{mol}^{-1}\right) \) of a few elements are shown below -
\( \begin{array}{lll} & \mathbf{I E}_{\mathbf{1}} & \mathbf{I E}_{\mathbf{2}} \\ \text { (a) } & 2372 & 5251 \\ \text { (b) } & 520 & 7300 \\ \text { (c) } & 900 & 1760 \\ \text { (d) } & 1680 & 3380\end{array} \)
Which of the above elements is likely to be a noble gas -
(A) (a)
(B) (b)
(C) (c)
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