d vs s orbitals

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Malia Shitabata 1F
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d vs s orbitals

Postby Malia Shitabata 1F » Sat Oct 19, 2019 11:29 pm

Professor Lavelle mentioned writing the d orbital before the s orbital when doing electron configurations, and he used chromium as an example so it was 3d4s. For elements further down in the periodic table like molybdenum which is right below it, it would end in 4d5s but do we still write it as 3d4s even if it's in the middle?

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Re: d vs s orbitals

Postby san_2F » Sat Oct 19, 2019 11:59 pm

The one he was talking about was a specific exception regarding chromium. I believe for certain elements, you would write 4s before 3d because 4s has a slightly lower energy, but for others, it would be normal and you would write 4s after 3d.

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Re: d vs s orbitals

Postby ZainAlrawi_1J » Sun Oct 20, 2019 12:02 am

For elements that are considered exceptions, you write 4s --> 3d because 4s has less energy, but most of the time it you would just do 3d --> 4s

Maggie Eberhardt - 2H
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Re: d vs s orbitals

Postby Maggie Eberhardt - 2H » Sun Oct 20, 2019 11:31 am

Which elements are considered exceptions/how do we know if an element is an exception?

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Re: d vs s orbitals

Postby JasonKwon_3k » Sun Oct 20, 2019 12:30 pm

The rows of Chromium and Copper are the exceptions, and I feel that this is just memorization. You need to know that they are exceptions.

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Re: d vs s orbitals

Postby KarineKim2L » Sun Oct 20, 2019 12:45 pm

For all electron configurations, I believe Dr. Lavelle wants us to write 3d before 4s regardless of which one is the higher energy level. I believe we simply write it in order of ascending n.

erica thompson 4I
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Re: d vs s orbitals

Postby erica thompson 4I » Sun Oct 20, 2019 5:44 pm

The reasoning behind the order is that you're supposed to write it in order of lowest energy to highest energy. Because shells that are further away from the nucleus have less electrostatic attraction, further shells have less energy (double-check me on this?).

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