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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.
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.
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