I viewed an image showing all the possible oxidation states of each element in the first row of transition metals, and the main oxidation states highlighted in a different colour.
I noticed all elements Sc to Cr had in common a 3+ main oxidation state, and from Mn to Zn 2+ was the common main oxidation state.
The reason stated for this in my good textbook was 2+ oxidation state become more stable relative to 3+ oxidation state, I can't quite understand why.
So Q : why does 2+ oxidation state become more stable relative to 3+ oxidation state for first row of transition metals?
I had drawn the electron - in -boxes configuartion for all elements in the first row, and looked at Hund's rule and partially and fully filled orbtals, but I have not really seen a clear, fundamental explanation of why, for this question.