Anion electron configuration  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Rain Taganas 1J
Posts: 22
Joined: Fri Sep 29, 2017 7:05 am

Anion electron configuration

Postby Rain Taganas 1J » Wed Oct 25, 2017 12:23 am

What is the electron configuration if you run out of orbitals from adding electrons? For example, say you have iodine.

I: [Kr] 4d10 5s2 5p5
I-: [Kr] 4d10 5s2 5p6

How about I 2-? Do we add 6s1 or 5d1?

Posts: 17949
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 406 times

Re: Anion electron configuration  [ENDORSED]

Postby Chem_Mod » Wed Oct 25, 2017 12:38 pm

Iodine simply does not form an I2- oxidation state. However, to continue filling orbitals, you would continue to fill according to relative energies which would lead you to begin filling 6s.

Susie Lee 2I
Posts: 20
Joined: Fri Sep 29, 2017 7:05 am

Re: Anion electron configuration

Postby Susie Lee 2I » Thu Oct 26, 2017 12:58 pm

Can someone also explain why anions are bigger than cations? Is it because of the number of protons?

Kourtney Nham 1L
Posts: 20
Joined: Fri Sep 29, 2017 7:04 am

Re: Anion electron configuration

Postby Kourtney Nham 1L » Thu Oct 26, 2017 5:15 pm

Cations are smaller because when you remove an electron to form cations the effective nuclear charge increases (protons can pull electrons closer because there are less of them). Conversely, adding an electron to form anions reduces the effective nuclear charge because there are now more electrons than protons making it more difficult to pull them in and there is increased electron-electron repulsion, making them larger.

Return to “Electron Configurations for Multi-Electron Atoms”

Who is online

Users browsing this forum: No registered users and 1 guest