Question

So i have used all day trying to figure out how I can determine the element out of a given function when asked "Which element has the following series of ionization energies I1, I2, I3 and I4?". Can you please explain briefly? With examples

This is a typical problem I will get. I only want explanation and steps for how to solve such problems. I only want explanation of how to solve problems like that, I dont have an example.

Answer 1

Ionization energy is the energy required when a atom in its complete gaseous form loses one electron from its most external orbital or valence shell. So for a element to have I1, I2, I3, I4 it needs to have at least 4 such electrons in its valence shell that it can lose.

Usually elements like Si, Ge, Sn who has ns²np² electronic structure in its valence shell can lose electrons one by one to give I1, I2, I3 and I4 till they can get a stable octate in their most outer shell (valence shell).

For example:

Si ([Ne]3s²3p²) - e = Si⁺  ([Ne]3s²3p¹) I1

Si ([Ne]3s²3p¹) - e = Si²⁺  ([Ne]3s²) I2

Si²⁺ ([Ne]3s²) - e = Si³⁺  ([Ne]3s¹)​​​​​​​ I3

Si³⁺ ([Ne]3s¹) - e = Si⁴⁺  ([Ne])​​​​​​​ I4

Similarly some of the transition metals can as well undergo such ionizations having (n-1)d^xns² electronic configurations where x is generally from 2 to 9. For an example Ti ([Xe]3d²4s²) shows such type of ionization.