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Electron configurations for ions

Posted: Tue Nov 10, 2015 1:09 pm
by chemgal4L
I have a really hard tim figuring out the electron configurations for ions. How do you know whether the ion will lose valence electrons from the d orbital first or if it will lose them from the s orbital first. I know there are exceptions to copper and chromium, but how about all of the other d block metals.

Re: Electron configurations for ions

Posted: Tue Nov 10, 2015 3:29 pm
by Christina Quigg 4G
For the d block electrons, with the exception of chromium and copper, the 4s electrons will be lost first. This is because the 4s orbital is the outer orbital, even though it is filled up before the 3d orbital. I hope this helps.

Re: Electron configurations for ions

Posted: Sun Nov 29, 2015 6:08 pm
by Anne Cam 3A
4s electrons are lost first only from group 1 and 2 metals like K and Ca, because there are no electrons in 3d orbitals. But with d-block transition metals, as the 3d orbitals gain electrons they become lower energy than 4s.

Cr is [Ar]3d54s1 and Cu is [Ar]3d104s1 because they are more stable with half-filled and filled 3d orbitals, respectively. They are not exceptions to losing 4s electrons; because the 4s orbital is the outermost one (just like it is for other d-block metals), it would lose electrons first as well. So Cu+ would be [Ar]3d10.

Re: Electron configurations for ions

Posted: Sun Jul 03, 2016 11:22 am
by Bella Fuentes 1D
Is it always necessary to eliminate the amount of valence electrons to maintain the elements ionization in the electron configuration?

Re: Electron configurations for ions

Posted: Mon Jul 04, 2016 7:29 pm
by Chem_Mod
I am not sure by what you are trying to ask. To get the ion's electron configuration, write the electron configuration for the atom and then remove/add the necessary number of electrons to the next highest/lowest orbital.