Ground state vs excited state

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Ground state vs excited state

Postby Maldonado3K » Sun Oct 15, 2017 11:27 pm

Can someone please explain how I can figure out if an electron configuration represents the excited state or the ground state? (Relates to problem 29).

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Re: Ground state vs excited state

Postby jennywu » Sun Oct 15, 2017 11:52 pm

Electrons in the ground state will fill up orbitals starting with the lowest energy orbital 1s, 2s, 2p, 3s, 3p, 4s, 3d etc.
Check the electron configuration and see if there have been any electrons excited to a higher energy level/ if there are any electron orbitals in lower energy states that have not been filled.

Emily Oren 3C
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Re: Ground state vs excited state

Postby Emily Oren 3C » Wed Oct 18, 2017 9:45 pm

If an electron is in its ground state, for example 1s, and is excited, is there a difference in energy between being excited to the 2s vs 2p orbitals? We were told in class that the first quantum number is the one that determines energy but also that electrons fill the s orbitals before the p orbitals. How does this relate to the Rydberg equation?

Jason Muljadi 2C
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Re: Ground state vs excited state

Postby Jason Muljadi 2C » Thu Oct 19, 2017 2:23 am

The Rydberg Formula is basically used to find or predict the wavelength of the light from an electron as the electron moves from one energy level to another. If you remember Rydberg's formula, there was an n1 and an n2 energy level. Those are the principle quantum numbers that tells you the energy level of the atom. However, I believe that this formula is used specifically for hydrogen or hydrogen-like atoms. You can relate the energy level 1s to Rydberg's equation, but I don't believe it can be applied to anything else. If it is used for other atoms, there will be a discrepancy between the inner and outer electrons levels that gives way to a lot of inaccuracies and errors to this equation

This website has a cool summary of the Rydberg Formula. Hope this answer clarifies some things!

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