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Help with properties of transition metal please

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
Reply 1
any ideas guys :smile:
Original post by chemrev
any ideas guys :smile:


Titanium doesn't actually have a +5 oxidation state. Yes iron is more stable in those states, that is why they are the common oxidation states of iron. Iron species in the +4/5/6 state do exist though, http://en.wikipedia.org/wiki/High-valent_iron , they just aren't common.
Reply 3
Original post by ThisIsOurDecision
Titanium doesn't actually have a +5 oxidation state. Yes iron is more stable in those states, that is why they are the common oxidation states of iron. Iron species in the +4/5/6 state do exist though, http://en.wikipedia.org/wiki/High-valent_iron , they just aren't common.


Ok so the +5 state for titanium is a mistake on the textbook and does not exist.
and thanks for answering the question, you cleared a few things up

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