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In this case, the electrons are in different shells, as seen by the principle quantum number, n. As n increases, so does energy. If you were looking at electrons in the same shell, then s would have less energy than d. s<p<d<f.
TheresaDsilva4A wrote:If the 3d orbital is filled after the 4s orbital, then why does it have less energy? Wouldn't electrons tend to fill subshells with lower energy first? Can someone please explain why this is the case? Thank you!
Before the electrons fill up the orbitals, the 4s orbital has less energy than the 3d orbital. However, after the electrons fill up the orbitals then the 3d orbital has less energy than the 4s orbital.
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