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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,http://www.webelements.com/ruthenium/atoms.html, 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