Chapter 2 Question 51  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Taylor_Yamane_2L
Posts: 23
Joined: Wed Sep 21, 2016 3:00 pm
Been upvoted: 1 time

Chapter 2 Question 51

Postby Taylor_Yamane_2L » Thu Oct 20, 2016 4:08 pm

I am a little confused on exactly how to figure out how many unpaired electrons each element has. For example can someone please explain why Nickel has 2 unpaired electrons.

Thank you!!

Mizuno_Mikaela_1D
Posts: 29
Joined: Wed Sep 21, 2016 3:00 pm

Re: Chapter 2 Question 51  [ENDORSED]

Postby Mizuno_Mikaela_1D » Thu Oct 20, 2016 9:20 pm

When finding the number of unpaired electrons predicted for the ground-state configuration of an atom, you are basically writing out the electron configuration and using Hund's rule to determine how many orbitals in the subshells are occupied with only one electron.

So for Nickel, the electron configuration is [Ar]3d^8,4s^2 which means that in the 3 d subshell, since the d subshell has 5 orbitals and there are 8 electrons for 3d, that means that there are two electrons in the first orbital, two electrons in the second orbital, two electrons in the third orbital and only one electron in the fourth and fifth orbital which means there are two unpaired electrons.

Sorry the explanation was probably a bit confusing but here is a video that explains it better:

https://www.youtube.com/watch?v=gnZKiWgVHzk

Taylor_Yamane_2L
Posts: 23
Joined: Wed Sep 21, 2016 3:00 pm
Been upvoted: 1 time

Re: Chapter 2 Question 51

Postby Taylor_Yamane_2L » Sat Oct 22, 2016 11:10 pm

Wow that explanation was so helpful and so was the video, thank you so much!


Return to “Electron Configurations for Multi-Electron Atoms”

Who is online

Users browsing this forum: No registered users and 1 guest