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For electrons that are in the D subshell, and if their ending electron configuration comes out to be 4d95s2, do we leave the answer like that or fill the D electron to making ending configuration 4d105s1? Which is right 4d95s2 or 4d105s1?
You would fill the d subshell in so it would be 4d10s1. This is because the stability of a completely filled d subshell (or a half filled d5 shell) is better for the electrons to exist at, as opposed to 4d95s2
This filling of the d orbital over the s orbital will also occur for elements such as chromium. Instead of being [Ar]3d44s2, the electron configuration will be [Ar]3d54s1.
In this case, you would fill the d subshell. You should try to completely fill or half fill the d subshell because doing this allows the atom to be as stable as possible. Because of this, 4d105s1 would be the correct electron configuration.
You would want to fill the d-shell so that the element is more stable. It is like the exceptions he discussed in the lecture, chromium and copper. You fill the d-shell half full or completely full before completing s-shell because they have lower energy than the s-shell.
Could someone explain to me why is it that when you start to include the d into our electron configuration the order is that d goes first then s. In highschool I was taught to just follow the order where it is s then p for the first 3 rows but then for the 4th row it would be s, d, p but I see that on the Solution Manual it places d first then s.
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