Question

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:

• A. Group 4
• B. Group 14
• C. Group 2
• D. Group 13

Hint:

A sharp increase in ionisation energy suggests that the element has reached a stable electron configuration (typically after the removal of the last valence electron).

Answer 1

The Correct Option is B

Ionisation energy increases with the removal of each electron, but there is a significant jump in ionisation energy when the element reaches a stable electron configuration. A sharp rise in ionisation energy, as seen after the second ionisation energy, indicates the removal of an electron from a stable configuration, which suggests that the element belongs to Group 14.

Final Answer: Group 14.