Question

The increasing order of electron gain enthalpy of the following substances is:

O<S<Se<Te

If the order of bond dissociation enthalpy is correct, enter 1 else 0.

Solution
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Electron gain enthalpy is the amount of energy released when an element accepts an electron. The process is endothermic.

Lesser the electronic repulsion faced by an electron to get occupied in the outermost shell higher the amount of
energy released.

On moving down the group, the electron gain enthalpy decreases from S to Po. Oxygen has an unexpectedly low value of electron gain enthalpy.
Since oxygen is smaller in size than S, so incoming e on oxygen faces more electronic repulsion on oxygen outermost surface ( due to more e density) as a result electron affinity decreases.

The increasing order of electron gain enthalpy with negative sign is
O(141.4kJ/mol)<Po(174kJ/mol)<Te(190.0kJ/mol)<Se(195.5kJ/mol)<S(208.8kJ/mol)

Hence the correct answer is 0.

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