The successive ionization energies for an unknown element are listed below. to which family in the periodic table does the unknown element likely belong. explain your reasoning .

i = 896 kj/mol
i2 = 1752 kj/mol
i3 = 14807 kj/mol
i4 = 17948 kj/mol

Belongs to the group 2A

Explanation:

As you can see, the first two ionization energies are close and low, meaning that this element ionizates easily.

Not only loses easily the first electron, but the second too

To remove the third electron you requiered a huge amount of energy

Now, elements easily ionizable are the ones from group IA, group 2A and transition metals.

The last ones have mixed characteristics in matter of how many electrons you can remove from them, so they are not a family.

Now the question: group I or group II ?

The elements of group I have low  ionization energies  for the first electron but high energies for the second ones.

Being all that said, the unknown element belongs to the Group 2A

wavelength variability is the right one

they should be similar or the same