Oxidation states of D-Block complexes

Hi, could somebody please explain how to find the oxidation state of the d-block ion from these compounds:
(i) [CoCl2(NH3)4]+ (ii) [PtCl6] K2

Reply 1

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Original post by sbrennan988

Hi, could somebody please explain how to find the oxidation state of the d-block ion from these compounds:
(i) [CoCl2(NH3)4]+ (ii) [PtCl6] K2

Treat these just like any other compound or ion that you need to determine the oxidation state of one element. In both cases the oxidation states of everything but the transition metal ion.

For the cobalt complex you know:
ammonia ligand is a molecule and therefore has oxidation state of 0 overall. (You can separate the oxidation states of the nitrogen and hydrogen if you really want to make extra work for yourself)
The chloride ions each have an oxidation state of -1. There are two of these ions.
The overall charge is 1+.
You should be able to calculate the oxidaion state of the cobalt by fairly straightforward algebra.

For the platinum compound you know.:
The oxidation state of the potassium ions is each +1, and there are two of these ions. (All group I ions are in +1 state).
The chloride ions are -1 each and there are 6 of them.
The molecule has an overall charge of zero.
Again, use simple algebra to calculate your answer.