We know that Mn2+ is stable as compared to Mn3+ and because of this MnO should be a more stable oxide than Mn203 and Mn3O4. However it is observed that synthesis is MnO is quite difficult and one has to perform the synthesis with nitrogen atmosphere; or else the reaction ends up producing Mn2O3 and Mn3O4. Why is it so?
Dear Kashmiri Deka,
I have worked a lot on the crystal structure of Fe3O4 see on my ResearchGate site: “Atoms and Crystal Structures”. Finally it appears that we have 2FeII in octahedral site and one FeIV in tetrahedral site, section 6.8. I think that you will have benefit to look at this work to understand your case. Perhaps there are some differences but the main reasons of the two sites must be the same.
Xavier
Yours
Under aerobic atmosphere you will always find the di or trimanganese oxide & controlled oxidation will produce MnO. CFSE determination and electron distribution of different MN ions help you to explain in favour of such existence.
Dear Kashmiri Deka,
Since your puzzling question I find an answer to it. As you know there are Xenon compounds and this allows to propose a new explanation of the valence three of La and Ln. The xenon shell of these elements is involved in their compounds see “The Crystal Structure of Er2O3 and the Lanthanum Coordination”. But the crystal structure of sesquioxide of Er is also that of (Fe,Mn)2O3 the bixbyite, this leads to transpose to the 3d metals and their Ar shell the analysis of the Ln valance.
As a result it the logic that “Mn2O3 and Mn3O4 end up being the more favored products instead of MnO during synthesis”.
See also “From Ln valence to that of nd”.
Xavier
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