Do anions follow the same rule as cations for electron configuration?

[Jay20155555]

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For cations, you remove electrons from the highest numbered shell, does this rule apple when talking about anions. Like would you add electrons to the highest numbered shell? I used this tool

https://www.caymanchem.com/app/template/chemAssistant,Tool.vm/itemid/4001

to get the electron configuration of Fe2- and it added 2 electrons to the 4s orbital making it 4s4...

 

[DAT Destroyer]

For cations, you remove electrons from the highest numbered shell, does this rule apple when talking about anions. Like would you add electrons to the highest numbered shell? I used this tool

https://www.caymanchem.com/app/template/chemAssistant,Tool.vm/itemid/4001

to get the electron configuration of Fe2- and it added 2 electrons to the 4s orbital making it 4s4...

Yes.....why not ? Let us consider the Chloride anion......it has the configuration 1s22s22p63s23p6.....If we were to remove an electron, we would remove it from the outermost region, namely the 3p sublevel.

Hope this helps.

Dr. Romano

 

[Jay20155555]

I mean in the case of adding an electron which creates an anion.

Sorry if I was to vague

 

[Lnguyen7]

For cations, you remove electrons from the highest numbered shell, does this rule apple when talking about anions. Like would you add electrons to the highest numbered shell? I used this tool

https://www.caymanchem.com/app/template/chemAssistant,Tool.vm/itemid/4001

to get the electron configuration of Fe2- and it added 2 electrons to the 4s orbital making it 4s4...

s orbital can only have maximum 2 electrons, so s4 is not possible.
Fe is a metal, which tend to give up electrons, so Fe2- is not correct.

Lets write the electron configuration of F-. F- will have the electron configuration of Ne, so
F-: 1s2 2s2 2p6 or short [Ne]
F: 1s2 2s2 2p5 (for comparison)

Another example Se2-: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 or [Kr]