[mrdoovde1]

Ok, so I am posed the following statement and am asked to give the oxidation states:



A = [Fe(H₂O)₆]^2- - Oxidation state of Fe is in +2

B = [Fe(CN)₆]^-6 - Oxidation state is 0

C = Ignore as complex isn't important in this case. Oxidation state is +3

D = Fe(SCN)^- - Oxidation state is +1

Are the complexes and oxixdation states

Also, what do the colours in the statement tell you about the complex?

Thanks

[Borek]

I am afraid most of your answers are wrong, I guess you are misunderstanding some of the basic principles.

First of all - changing the ligand doesn't change the oxidation state, for the change of the oxidation state you need a redox reaction, there is only one such reaction here.

Please elaborate why you think the formula of hexaaqua ion is Fe(H₂O)₆]^2-, and why you think oxidation state of Fe in this ion is +2.

[mrdoovde1]

I am afraid most of your answers are wrong, I guess you are misunderstanding some of the basic principles.

First of all - changing the ligand doesn't change the oxidation state, for the change of the oxidation state you need a redox reaction, there is only one such reaction here.

Please elaborate why you think the formula of hexaaqua ion is Fe(H₂O)₆]^2-, and why you think oxidation state of Fe in this ion is +2.

How do you identify a redox reaction?

Also since the Fe atom was initially in an oxidation state +2, when the 6 H2O ligands are attached to it, it will remain in a +2 oxidation state. This mean that the overall charge must be -2 since H2O ligands are neutral


Edit: Just realised I made a mistake. For the reason mentioned above, it should be Fe(H₂O)₆]^{2+ not 2-}

[Borek]

How do you identify a redox reaction?

Not a thing easy to answer without a specific context. However, the way the question is worded it looks like A and B are compounds of Fe(II), while C and D are compounds of Fe(III).