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Posted: Sat Nov 03, 2018 10:16 pm
by Mariam Baghdasaryan 4F
For example, the electron configuration for Selenium (Se) is [Ar] 3d10 4s2 4p4.

If I am looking at n=4, then l can be the 0 (s) ,1 (p), 2 (d) and 3 (f) subshells. Since Selenium goes up to 4p4, does that mean it has empty l=2 and l=3 subshells, or does it not have those subshells at all?

Re: Subshells

Posted: Sat Nov 03, 2018 11:25 pm
by 904936893
It does have access to its d and f subshells, those shells just aren't filled. This is why elements after row 2 can have an expanded octet (more than 8 electrons), because n=3, which means that l can equal 0,1, or 2 (s, p, and d orbital). Even though none of the elements in row three have any electrons in the d orbital, they still have access to them, allowing those shells to be filled with electrons if necessary.

Re: Subshells

Posted: Sat Nov 03, 2018 11:35 pm
by Saman Andalib 1H
It means that that particular element has empty subshells. The subshells always exist for the n=4 energy level, they just may not always be filled depending on the element.