Originally posted by not_important
Ok, thanks guy! I suspected the possibility of Mn(III) simply because none of the complexes of higher oxidation states had colours in the right range.
This isn't going to be easy, Mn forms polynuclear complexes. As an example, even though it's done at 100 K, here is one with two Mn(III) and four
Mn(II)
http://scripts.iucr.org/cgi-bin/paper?gk2005&buy=1
Note that the ligands ketones and carboxylic acids, previous to finding this and your experiment with Mn(OH)2, I wondered if oxyidised glycerol is at
least part of the complex, even though Mn does complex with polyols. This doesn't discourage me from thinking that.
edit -
I suspect Mn(III) or a mixed state complex. But it is possible that there are higher states, complexing may lower the cost of getting there enough
that even air oxidation can reach them; think of the Co(III) complexes.
[Edited on 6-8-2006 by not_important] |