4 posts • Page 1 of 1
In the cases of these atoms, a lower energy configuration is for each of the five 3d orbitals to be half-filled (Cr) or filled (Cu) and the 4s to have 1 electron rather than 2. I believe these energy level differences are quite small, so it is difficult to have an intuition for these exceptions beyond knowing which elements they are.
The atoms of Cu and Cr are the most stable when they half of their shell can be filled, meaning that if the atoms did not receive that extra electron they would essentially be volatile, which is bad for an atom. The s-block is already filled in the periods 1-3, and therefore the s-orbital is fairly stable already. Because the 3-d orbital is the first of the d-orbitals to be filled, the d shell is more unstable, so adding the electron from the s-block makes it more stable. Hopefully this helps.
Who is online
Users browsing this forum: No registered users and 1 guest