d orbitals

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JustinHorriat_4f
Posts: 111
Joined: Wed Sep 18, 2019 12:19 am

d orbitals

Postby JustinHorriat_4f » Sun Oct 20, 2019 12:17 pm

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

vpena_1I
Posts: 109
Joined: Sat Aug 24, 2019 12:15 am

Re: d orbitals

Postby vpena_1I » Sun Oct 20, 2019 12:23 pm

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.

Sidharth D 1E
Posts: 98
Joined: Sat Aug 24, 2019 12:17 am

Re: d orbitals

Postby Sidharth D 1E » Sun Oct 20, 2019 12:45 pm

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.

TheresaDsilva4A
Posts: 53
Joined: Thu Jul 25, 2019 12:17 am

Re: d orbitals

Postby TheresaDsilva4A » Sun Oct 20, 2019 1:15 pm

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!

Ethan Lam 4A
Posts: 69
Joined: Thu Jul 11, 2019 12:17 am

Re: d orbitals

Postby Ethan Lam 4A » Sun Oct 20, 2019 1:54 pm

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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