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And why are there atoms that don't fill the number of electrons given by 2n^2 in the shells, don't they have to overpass the max the go into the next shell?
You mean like 2 electron in the first shell (K), 3 in the second (L) and 6 in the third (M)? Or are you talking about the orbitals. E.g 1s, 2s, 2p etc...?
Are you asking why the diagram is as it is? Where did you find it?
i just found an element: ruthenium and its shell structure goes like this:188.8.131.52.1,...sorry, you cannot view external links. To see them, please
REGISTER or LOGIN, why does that happens? would not the positive charge attract the electrons an squeeze then into the lower shell?
If you want me to do the ruthenium example, I can show you. 
Electrons fill orbitals of lowest energy first. The order of in which electrons fill sublevels is:1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p → 5s → 4d → 5p → 6s → 4f → 5d → 6p → 7s → 5f → 6d