Ionization Energy

Moderators: Chem_Mod, Chem_Admin

Alejandra_Vasquez_1B
Posts: 15
Joined: Wed Sep 21, 2016 2:56 pm

Ionization Energy

Postby Alejandra_Vasquez_1B » Sun Oct 16, 2016 8:45 pm

I am having difficulty understanding how to determine the ionization energy level of an atom. Is there any way to figure out which atom has a lower ionization level for a lewis structure?

Kevin Tam 1J
Posts: 23
Joined: Wed Sep 21, 2016 2:59 pm

Re: Ionization Energy

Postby Kevin Tam 1J » Mon Oct 17, 2016 8:03 am

As for determining the exact ionization energy level of each element, I don't know if such a task is within or beyond the scope of this course.

These are the general trends for ionization energy.

As you go across a period, the ionization energy generally increases. The exceptions for this periodic trend include Be and B, and N and O.
As for the Be and B exception, this can be explained by the fact that removing an e- from B is easier than removing an e- from Be because the e- from B is entering a new subshell, the p-subshell, thus making this e- easier to remove than the e- that completes the s-subshell of Be.
As for the N and O exception, this can be explained by the fact that removing an e- from O is easier than removing an e- from N because the e- from O experiences electron-electron repulsion, thus making this e- easier to remove than an e- from N that experiences no repulsion.

As you go down a group, the ionization energy generally decreases. This is because you are adding a new shell as you go down a group. This new shell of electrons, since it is farther away from the nucleus, will have electrons that are easier to remove and thus require less energy to remove.


Return to “Lewis Structures”

Who is online

Users browsing this forum: No registered users and 1 guest