Why no has an oxidation state of +1 brown ring complex?
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coordination-compounds oxidation-state
In the standard brown ring test for the nitrate ion, the brown ring complex is :
[Fe(H2O)5 (NO)]2+[Fe(HX2O)X5 (NO)]X2+
In this compound, the nitrosyl ligand is positively charged, and iron is in a +1+1 oxidation state.
Now, iron has stable oxidation states +2 and +3. Nitrosyl, as a ligand, comes in many flavours, of which a negatively charged nitrosyl is one.
I see no reason why the iron doesn't spontaneously oxidise to +3 and reduce the NONO to -1 to gain stability. But I don't know how to analyse this situation anyway. I think that there may be some nifty backbonding increasing the stability, but I'm not sure.
So, why is iron in +1 here when we can have a seemingly stable situation with iron in +3
hope it helps!☺️
In the standard brown ring test for the nitrate ion, the brown ring complex is :
[Fe(H2O)5 (NO)]2+[Fe(HX2O)X5 (NO)]X2+
In this compound, the nitrosyl ligand is positively charged, and iron is in a +1+1 oxidation state.
Now, iron has stable oxidation states +2 and +3. Nitrosyl, as a ligand, comes in many flavours, of which a negatively charged nitrosyl is one.
I see no reason why the iron doesn't spontaneously oxidise to +3 and reduce the NONO to -1 to gain stability. But I don't know how to analyse this situation anyway. I think that there may be some nifty backbonding increasing the stability, but I'm not sure.
So, why is iron in +1 here when we can have a seemingly stable situation with iron in +3
hope it helps!☺️
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