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 :

Question

Dr. Abubacker · Accepted Answer

[Solution by Dr. Abubacker] There is a very large jump between the third ($3658$) and fourth ($25024$) ionisation energies, showing that the first three electrons are valence electrons and the fourth comes from a stable inner shell. So the element has three valence electrons and belongs to group 13. Answer (1).

Q. 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 :

Explanation

Reviewed by Dr. Abubacker

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