s- electrons vs p- electrons [ENDORSED]
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s- electrons vs p- electrons
Can someone explain to me why s- electrons have lower energy than p-electrons in the same shell? Thanks!
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Re: s- electrons vs p- electrons [ENDORSED]
In many-electron atoms, electron-electron repulsion causes increasing orbitals to be increasing in energy (because electrons in "greater" orbitals are shielded from the full attraction of the nucleus & we know that when electrons are more strongly attracted to the nucleus, they are lower in energy). Also, s-electrons of any shell can penetrate through inner shells, while p-electrons penetrate much less.
In summary, s-orbital electrons are more tightly bound to the nucleus (shielding/penetration), and are therefore lower in energy than p-orbital electrons.
In summary, s-orbital electrons are more tightly bound to the nucleus (shielding/penetration), and are therefore lower in energy than p-orbital electrons.
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Re: s- electrons vs p- electrons
Basically, the s orbitals have fewer electrons standing between them and the nucleus, therefore, they are less shielded. The p orbitals are more shielded than the s orbitals of the same shell.that is why p orbitals have higher energy.
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Re: s- electrons vs p- electrons
From what I understand the further the atoms the electrons are from the nucleus, the more energy they have.
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Re: s- electrons vs p- electrons
For the most part it really just has to do with proximity to the nucleus. Closer the nucleus, more attraction between protons and electrons, lower energy.
Re: s- electrons vs p- electrons
Then how come even when the 4s orbitals are filled first, they still have a higher energy than the 3d orbital, hence why we write 3d before 4s?
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Re: s- electrons vs p- electrons
As for why the 4s has more energy than 3d, this is simply because it's in a higher energy shell. A higher n implies a higher energy level.
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