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For the ground state electron configurations for chromium and copper, we are supposed to put them in the form of d^5 and d^10. If we were finding electron configurations of ions, would we still try to complete a half full or full shell? How would the electron configuration look? More specifically, which orbital would we add/remove the electron to/from? Also, chromium and copper are in the 3d section; would we treat the 4d section the same as chromium and copper? Any help is appreciated!!
I'm not sure about the ion part, but all of the elements under Chromium and Copper (ex: Silver, Tungsten) would have the same type of ground state configuration where you want it to be d5s1, d10s1. So Silver is going to be [Kr]4d105s1.
For the ground state of Chromium and Copper, we write the configuration as 3d^5 4s^1, and 3d^10 4s^1 respectively. This is because it is more stable with a half full or full 3d shell and a half full 4s shell then it would be with an almost half full or full 3d shell and a full 4s shell. As for ions, elements in the d-block have a rule when forming cations that electrons are taken from the uppermost s shell before they are taken from the d shell. So for example, Nickel has an electron configuration of [Ar] 3d^8 4s^2, but when we form a Ni^3+ cation we see that its electron configuration is now [Ar] 3d^7. As for the rest of the d block, I believe Ag is similar to Cu and Mo is similar to Cr, but of course, professor Lavelle said we only need to know electron configurations up until n=4 so we shouldn't have to worry about that. Hope this helped!
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