Oxidation state/charge confusion Watch

DavidMorgan
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Hi

I'm finding it hard to fully grasp oxidation states/charges etc.

Q1) Firstly, I get that Al(NO3)3 is made up of Al3+ ions and three nitrates to balance the charge.

But if Al has a 3+ charge, where have its 3 electrons gone?

Secondly, I understood that oxidation states are due to electronegativity; eg in H-Cl, the electron of hydrogen is pulled closer to the electronegative chlorine, ie H has 'lost' its 1 electron and therefore is in +1 oxidation state

However, the following complexes

[Fe(H 2 O)6] 2+Pale green
[Fe(H 2 O)6] 3+ Yellow/brown


both have the same ligands, but different oxidation states. The description before doesn't hold true here. What makes the Iron +2 and +3? I think I may be misunderstanding several different theories here

Sorry if these are stupid questions
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amy.louise
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Right I hope I help...
firstly to the where have te 3 electrons gone?... No3 ions have a 1- charge hence why there are three of them. They have each gained one electron making them negative.
secondly... Iron can come in 2+ or 3+ ions. The colour comes from the precipitate that they produce. When there is fe(II) the solution absorbs different colours from the spectrum that when an fe(III) is produced. It is the loss of electron by fe(II) that causes the colour change.
I really hope the second bit makes sense doesn't confuse you even more
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Borek
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(Original post by DavidMorgan)
But if Al has a 3+ charge, where have its 3 electrons gone?
Why does it matter? It was oxidized by something. Doesn't matter what compound it is in right now. It was oxidized earlier.
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