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electron configuration

Posted: Sun Oct 27, 2019 10:05 pm
by NHolmes3L
what are the exceptions, like copper, and why are they different?

Re: electron configuration

Posted: Sun Oct 27, 2019 10:09 pm
by Nicholas Chin 1G
It's because having 10 electrons in the d orbital and 1 in the s orbital is actually more stable than 9 electrons in the d orbital and 2 in the s orbital. This also applies for 5 electrons in the d orbital.

Re: electron configuration

Posted: Sun Oct 27, 2019 10:09 pm
by Sidharth D 1E
They are different because to achieve maximum stability, those atoms take an electron from the 4s subshell and place it in the 3d subshell, so that they can have a full 3d subshell and half full 4s subshell (3d10 and 4s1).

Re: electron configuration

Posted: Sun Oct 27, 2019 10:13 pm
by Venus_Hagan 2L
I think Copper and Chromium are the exceptions we have to worry about for this class. They are different because they almost have a half-filled or filled d orbital. Having a half-filled or filled d orbital is more stable than the filled 4 s orbital and so it takes one of the 4s electrons. The electron configuration for Copper would look like this [Ar] 3d10 4s1 and Chromium like this [Ar] 3d5 4s1.

Re: electron configuration

Posted: Sun Oct 27, 2019 10:14 pm
by 105311039
It is more stable to have 10 electrons in the D orbital, rather than 9 in the D orbital and 2 in the S orbital, therefore you move one electron to the D orbital to make it as stable as possible.

Re: electron configuration

Posted: Sun Oct 27, 2019 10:17 pm
by Prasanna Padmanabham 4I
For a list of atoms with different electron configurations check this website out: [url]https://www.scribd.com/doc/13771509/Electron-Configurations-of-Elements-Which-Are-Exceptions-to-the-Rule
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