Electron Configuration for Silver?
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 102
- Joined: Wed Sep 30, 2020 9:35 pm
Electron Configuration for Silver?
Why is the electron configuration for Silver: [Kr]4d^(10)5^(1) and not [Kr]4d^(9)5s^(2)?
-
- Posts: 107
- Joined: Wed Sep 30, 2020 9:35 pm
- Been upvoted: 1 time
Re: Electron Configuration for Silver?
It's considered one of the exceptions for writing e configurations; it's more stable to fill the d^5 or d^10 , because when they're filled they have lower energy, so the electron from the 5s "jumps" down to the 4d orbital.
-
- Posts: 131
- Joined: Wed Sep 30, 2020 9:49 pm
- Been upvoted: 1 time
Re: Electron Configuration for Silver?
Silver is an exception. You just have to remember that because it can fill up the shell it would want to do that because it will make the molecule more stable. So instead of filling up the s subshell it will fill up the d subshell and then leave one empty in the s subshell.
-
- Posts: 101
- Joined: Wed Sep 30, 2020 9:43 pm
Re: Electron Configuration for Silver?
Same is for chromium. Instead of a [Kr] 3d^4 4s^2. One electron will jump down from 4s orbital to create a more stable orbital in 3d because all electrons will be parallel.
-
- Posts: 102
- Joined: Wed Sep 30, 2020 9:35 pm
Re: Electron Configuration for Silver?
Oh okay. For V; Vanadium does the 4s2 give electrons to the 3d3 to make a half full 3d orbital then?
-
- Posts: 101
- Joined: Wed Sep 30, 2020 9:59 pm
Re: Electron Configuration for Silver?
Jenaye Brelland 2L wrote:Oh okay. For V; Vanadium does the 4s2 give electrons to the 3d3 to make a half full 3d orbital then?
Vanadium’s electron configuration would actually still be [Ar] 3d3 4s2. Only the atoms that are one electron away from 3d5 or 3d10 would take away an electron from 4s, so only the groups of chromium and copper would do so. Hope this helps!
Re: Electron Configuration for Silver?
You always want the configuration to be the most stable it can so you would want to fill all of the d subshell instead of having an incomplete d and s subshell!
-
- Posts: 52
- Joined: Wed Sep 30, 2020 10:02 pm
Re: Electron Configuration for Silver?
We learned that chromium and copper were two exceptions for electron configurations, but I think Dr. Lavelle said that the elements in the same group as those two also follow that exception. I believe having a 4d shell that is half full or completely full makes it more stable, so you would pull an electron from the 5s orbital to make that 4d shell half full or completely full.
-
- Posts: 60
- Joined: Wed Sep 30, 2020 9:33 pm
Re: Electron Configuration for Silver?
The electron configuration for silver (Ag) is because an atom of an element is more stable (less energy) when an electron fills up the d-orbital to or . Thus, an atom of silver prefers that one electron from the 5s-orbital be donated or passed down to the 4d-orbital to achieve this state of lower energy. This is simply applying the concepts we learned about chromium and copper, both of which are exceptions to typical electron configuration, to elements of their group. This is why both copper and silver have similar electron configurations where an electron is passed down from the respective s-orbital to complete the d-orbital with 10 electrons. In terms of chromium and other elements in its group, their electron configurations function the same way, except the electron is being donated to fill the d-orbital up to 5 electrons.
Return to “Electron Configurations for Multi-Electron Atoms”
Who is online
Users browsing this forum: No registered users and 6 guests