3 posts • Page 1 of 1
In today's lecture, Professor Lavelle's PowerPoint noted two exceptions that we need to know when determining atomic states/orbitals. Under "need to know two exceptions," the slide said "half full d^5 and full d^10 subshell have lower energy." Did I misunderstand what the two exceptions are? If these are the two exceptions, can someone explain why these are considered exceptions?
To add onto it, they are exceptions because when you consider electron configuration and energy levels, because 3d will end up being in the inner orbital of the electron orbitals, you would want to stabilize that one before stabilizing the others. Therefore, for copper and chromium, the one electron from the 4s shell is Brought to the 3d shell so that entire orbital will have either all 5 lines filled with one or two electrons.
Who is online
Users browsing this forum: No registered users and 1 guest