Question

how do you know which element will display an unusually large jump in ionization energy values between \(I_3\) and \(I_4\)

Answer 1

In general, valence electrons are easy to remove, since they are the farthest from the nucleus. It gets harder and harder to remove additional electrons from an atom, so IE generally gets larger as more electrons are taken away. Huge jumps in IE usually come when the valence electrons have run out, and the next electron comes from a full core level that was originally beneath the valence level. An atom with 3 valence electrons will have a large jump in IE for the 4th ionization. By that logic, any atom in the same group as aluminum should have a large jump in IE that you are describing

Answer 2

so can you tell me why aluminum is larger than silicon?

Answer 3

i assume cause silicon has more protons and thus more charge which holds electrons together so he contracts more its electrons. when you look at the ionic radius of Al and Si you firs of all se that Al is 3+ and Si is 4+ and now you see that Si has one more proton to attract same amount of electrons

Answer 4

i think i chose silicon because the fourth ionization energy disrupts the stability..idk..i cant remember :(