The exceptions

Moderators: Chem_Mod, Chem_Admin

Posts: 51
Joined: Sat Aug 17, 2019 12:15 am

The exceptions

Postby derinceltik1K » Sun Oct 27, 2019 4:03 pm

Why are Copper and Chronium the exceptions when it comes to electron configuration ?

Ronak Naik
Posts: 103
Joined: Sat Jul 20, 2019 12:15 am

Re: The exceptions

Postby Ronak Naik » Sun Oct 27, 2019 4:11 pm

Chromium's d orbital technically rests in 3d4, however, due to electron stability, the element is more table when an electron from the s orbital is transferred into the d orbital to make the configuration 3d54s1. A half d orbital is more stable and therefore the s orbital will lose an electron that will be contributed to the d orbital. Similarly, Copper rests in the 3d9 orbital and with the same reasoning, a full d orbital is more stable. Thus, the actual electron configuration rests in 3d104s1.

Haley Fredricks 1B
Posts: 53
Joined: Sat Aug 24, 2019 12:16 am
Been upvoted: 2 times

Re: The exceptions

Postby Haley Fredricks 1B » Sun Oct 27, 2019 4:15 pm

For both Chromium and Copper, the 3d orbital is the last to be filled up with electrons (even though 4s is written after in the electron configuration). Despite this, it is more stable to have a half full or completely full 3d orbital with only a half full 4s orbital. Because of this, the 4s shell for both Chromium and Copper only has one electron.

Return to “Electron Configurations for Multi-Electron Atoms”

Who is online

Users browsing this forum: No registered users and 0 guests