Question

The electron gain enthalpy of groups 16 and 17 varies to become less negative as you move down a group, because of the change in the atomic size, nuclear charge. An example of the same would be that of O where the electron gain enthalpy is -141 kJ/mol, while S has -200 kJ/mol, as the newly added electron goes into the smaller n=2 kernel. Since the small size of the element, the interelectronic repulsion increases, thus increasing the electron gain enthalpy in the process.

Is the above text true?

Answer 1

Answer:

yes the above context is true