The successive 5 ionisation energies of an element are 800, 2427, 3658, 25024 and 32824 kJ/mol, respectively. By using the above values predict the group in which the above element is present :

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YESPYQ · Accepted Answer

Correct answer: d) Group 13. Ionization enthalpy = the energy required to remove one electron from an isolated gaseous atom. General trend: Increases across a period (left → right) Decreases down a group Electron gain enthalpy = energy released when an atom gains an electron. More negative = stronger tendency to gain electrons Small size of fluorine Fluorine's atomic radius is very small. When an extra electron is added to fluorine, it goes into the already crowded 2p orbital, where electron–electron repulsion is very high. This reduces the stability gained by accepting that electron. 2. Chlorine has larger size Chlorine's 3p orbital is bigger, so it can accommodate the incoming electron more easily with less repulsion. Hence, it releases more energy (i.e., more negative electron gain enthalpy). Both Statement-I and Statement-II are true

The successive 5 ionisation energies of an element are 800, 2427, 3658, 25024 and 32824 kJ/mol, respectively. By using t…

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