Chromium, Copper, etc.

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Raymond Le 2G
Posts: 16
Joined: Fri Sep 25, 2015 3:00 am

Chromium, Copper, etc.

Postby Raymond Le 2G » Sat Oct 10, 2015 4:58 pm

Why is it for these elements and others such as silver that their ground state electron configuration is d10s1 or d5s1?

Janae Yip 3G
Posts: 15
Joined: Fri Sep 25, 2015 3:00 am

Re: Chromium, Copper, etc.

Postby Janae Yip 3G » Sat Oct 10, 2015 9:18 pm

Elements want to achieve the lowest energy electron configuration, otherwise known as the ground state. This can be done by either having a half full d^5 or full d^10 subshell. When chromium takes one electron from the 4s orbital and puts it into the 3d shell, the element can now complete 2 half full electron shells. It is much more stable than if both shells were not filled. Same goes for copper; with [Ar]3d^10 4s^1, the element now has 1 full shell and 1 half full shell. This goes for most of the elements in the same rows as copper and chromium, but we are only responsible for knowing the rules for these two elements.

KVu 3G
Posts: 12
Joined: Fri Sep 25, 2015 3:00 am

Re: Chromium, Copper, etc.

Postby KVu 3G » Sat Oct 10, 2015 11:12 pm

For elements such as Chromium or Copper, they will have a filled or half filled d orbital. Electrons prefer to be in either a half filled or full d-orbital because it is more stable due to symmetry. For example, Copper will have an electron configuration of [Ar]3d10 4s1 because it is more stable with fully filled d-orbitals.


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