| View previous topic :: View next topic |
| Author |
Message |
asfi
Joined: 09 Jul 2008
Posts: 15
|
 Posted: Mon Jul 14, 2008 2:14 pm Post subject: Question 37 |
 |
|
| Isn't Mn the one with the half filled d orbital....Wouldn't Mn2+ only have three electrons in the d orbital? Why would the answer be choice d then? |
|
| Back to top |
|
 |
admin
Site Admin
Joined: 08 Dec 2003
Posts: 2176
|
| Posted: Thu Jul 17, 2008 6:45 am Post subject: |
|
|
Cr should be 4s2 3d4 but is 4s1 3d5
Mn is 4s2 3d5
Mn+ is 4s1 3d5
Mn++ is also 3d5 (see http://wwwchem.uwimona.edu.jm/courses/IC10Kec.html)
This is due to the unusual stability of a half filled d subshell. |
|
| Back to top |
|
|
CK
Guest
|
| Posted: Sun Aug 22, 2010 4:34 pm Post subject: Q37 PS Exam 5 |
|
|
I don't really under why the third ionization energy of manganese is represented as Mn2+ instead of Mn3+, as stated in the answer choices. Mn2+ means the second ionization energy right? I'm confused.
Thanks! |
|
| Back to top |
|
|
mohsinalam5969
Joined: 18 Apr 2011
Posts: 50
|
| Posted: Sun Jul 03, 2011 9:21 pm Post subject: |
|
|
The discussion is about the ionization potentials of:
Mn(2+): [Ar] 4s0 3d5
Since Mn(2+), with its electron configuration [Ar] 4s0 3d5, has the 3d orbital half filled, it is more stable. Therefore ionization energy of Mn(2+) would be the higher.
Note: Half filled d-orbitals are less stable than completely filled, but more stable than all the others. |
|
| Back to top |
|
|
|
FAQ
Search
Memberlist
Usergroups
Register
Profile
Log in to check your private messages
Log in
