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d orbitals

Posted: Sun Oct 20, 2019 12:17 pm
by JustinHorriat_4f
Why do electrons in the d orbitals have less energy than electrons in the s orbitals such as why does it go 3d^2 4s^2

Re: d orbitals

Posted: Sun Oct 20, 2019 12:23 pm
by vpena_1I
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.

Re: d orbitals

Posted: Sun Oct 20, 2019 12:45 pm
by Sidharth D 1E
Furthermore, it is written in that way, because if that element would lose an electron, it would lose it from the 4s2 orbital, not the 3d orbital.

Re: d orbitals

Posted: Sun Oct 20, 2019 1:15 pm
by TheresaDsilva4A
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!

Re: d orbitals

Posted: Sun Oct 20, 2019 1:54 pm
by Ethan Lam 4A
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.