according to the picture below showing oxidation of d-block metal ions
Titanium can have a +5 oxidation state, i do not understand this,
i can understand why it would have a + 1,2,3,4 oxidation state as it would loose the electrons first from the 4s orbital then the remaining 2 electrons from the 3d orbital,
but i do not understand how the +5 oxidation state is achieved, what electron configuration would that give titanium
The same applies for Fe in oxidation states +4,+5,+6, would it not be more stable in a +2 , or +3 , with a empty 4s orbital or a half full 3d orbital
if anyone could answer this or attempt an explanation i would be great full and u will get a +ve rep - a2 chemistry ocr