Question

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 please.

I = 896 kj/mol
I2 = 1752 kj/mol
I3 = 14807 kj/mol
I4 = 17948 kj/mol

Answer 1

Do you see the successive ionizations increase? Do you know why? The huge jump between the 2nd and 3rd ionizations tells us that removing the first two electrons is relatively easy, but removing the third takes a bunch more energy. There's a very good reason for that...

Answer 2

So because it is difficult to remove more than 2 new electrons it suggests that this is for elements that lose 2 electrons meaning group 2a which is the alkaline earth metals???

Answer 3

correctamundo

Answer 4

:)

Answer 5

the huge jump in IE between 2 and 3 indicates that the 3rd electron comes from a different level than the first two. So only the first 2 electrons that get removed come from the valence level, making the element come from Group 2A

Answer 6

ok thank you so much!!