# Predict the valence configuration of this element using the first five ionization energies [closed]

If the first five ionization energies of an element are, respectively: $$\pu{1.09 kJ/mol}$$, $$\pu{2.35 kJ/mol}$$, $$\pu{4.62 kJ/mol}$$, $$\pu{6.22 kJ/mol}$$ and $$\pu{37.83 kJ/mol}$$, to which group of the periodic table does this element belong? Predict the valence configuration of this element. Justify your reasoning

I don't understand how to solve this. How do I relate ionization energy to finding the element, then predicting the valence configuration?

• Those ionization values are too small. Did you copy them correctly? Mar 1, 2021 at 8:07

There is a third way to solve this: look up values in a table of ionization energies. It helps ensure accuracy to have "second and third opinions", so this is a good exercise. From the Wikipedia (in $$\pu{kJ/mol}$$), the values are 1086.5, 2352.6, 4620.5, 6222.7 37831, 47277.0.