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Pd and Ni are in the same group, but electron configuration for Nickel is [ ]3d8 4s2, and electron configuration for Pd is [ ]4d10. Why does the electron from the s-orbitals from Pd move to d-orbitals to fill the full-shell, but the electrons in Ni don't?
I think this might has to do with the 4th energy level and how energy level differences become smaller as it gets higher. I think the 4th level is close enough to the 5th energy level that maybe the 4d and the 5s are extremely close but the 4d is filled first because it’s lower.
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