Electron Configuration for Cr and Cu

[EriMizuguchi2K]

Hi,

I was wondering if all the elements in the same columns as Cr and Cu follow the same pattern when writing the electron configuration? (For example, for elements in Cr's column, it would be nd^5(n-1)s^1 and for elements in Cu's column, it would be nd^10(n-1)s^1)?

[Neeti Indiresan 3I]

I think in general yes, because they all share the same number of valence electrons and would therefore all benefit from having a half full or full d-subshell.

[Leo Chang 2H]

Hi,

To answer your question, I believe that all of the elements in the same groups as Cr and Cu will exhibit the same properties. This is because the concept of stability stays the same regardless of how far down a group you go; the elements in those groups will still reach their most stable state by having a full/half-filled d orbital.

I hope this helps!

[Evan L 2B]

I believe all the elements in the same columns as Cr and Cu follow the same pattern. This pattern exists to maintain stability in the atom. Also, there are other elements that are exceptions and don't follow the basic rules(ex. elements 44, 45, 46). I don't think these will be tested but it might be worth checking out.

[Hudson2J]

I think yes, but the interactions between electrons get more complicated as you go down the table. That said, it would make sense for the higher level d shells to still be lower energy than s shells at half-full or full.

[Rainy Liu Ruoshui_2K]

For ground state atoms, they want to have the lowest energy level. In this case, a half-full or full subshell 3d would have lower energy.

[Maxwell Yao]

Since we want to minimize the energy for atoms, a half full or full 3d subshell will have lower energy.

That's why both Cr and Cu end in 3d54s1 and 3d104s1 respectively.

Hope this helps

[Minoo Bastani 2J]

I think that this holds true for all the elements in the group even though it gets more complex going down because it logically makes sense that the ground-state atoms will be looking to minimize energy by maximizing the stability, which can be done by having a half-full or full sub shell.

[Ashley Tonthat 2B]

Hello,

Yes, all the elements in the same column as Cr and Cu have the same ns^1d^5 and ns^1d^10 configuration. For example in Cu, usually the electron configuration would be written 4s^23d^4. But since there's electron repulsion in the s orbital, according to Hund's rule electrons tend to want their own orbital (meaning they want to be unpaired due to electron repulsion). So it is a more stable state to move one electron from the s orbital to the d orbital so all of them will be unpaired. Hope this helps.

[Sean Sanders 1E]

I believe so because atoms are more stable with a half-full and filled d-subshell and partially filled s-subshell than with a full s-subshell and unfilled d-subshell.

[gracebinder3I]

Hi!
That is correct! In order to maintain the lowest energy possible as to satisfy and best fill orbital shells, the electron configurations of these two groups will follow these patterns.
I hope this helps!

[Lindsey Walter 3E]

Yes! They should all follow that pattern since the number of valence electrons is the same (even though they are found in different energy levels).