How do you determine the oxidation state of metal ions?

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How do you determine the oxidation state of metal ions?

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Answer 1 · 2016-08-14T16:50:50

Well, for $M^{2 +}$ $M^(2+)$ and $M^{3 +}$ $M^(3+)$ it's easy, we have $I I +$ $II+$ and $I I I +$ $III+$ oxidation states.

Explanation:

For complex ions such as $M n O_{4}^{-}$ $MnO_4^-$ and $C r_{2} O_{7}^{2 -}$ $Cr_2O_7^(2-)$ you have to do a little more work, but most of it is routine. Oxygen, in all its oxides, assumes an oxidation state of $- I I$ $-II$ . Thus the oxidation state of the metal in these oxides is the Group oxidation number, i.e. the maximum oxidation numbers, $M n (V I I +)$ $Mn(VII+)$ , and $C r (V I +)$ $Cr(VI+)$ . Are you clear on how these designations were obtained?

Can you tell me the metal oxidation states in: $M n O_{2}$ $MnO_2$ ; $Z r C l_{4}$ $ZrCl_4$ ; $P t C l_{4}$ $PtCl_4$ ; $F e_{2} O_{3}$ $Fe_2O_3$ ; $P d {(P P h_{3})}_{4}$ $Pd(PPh_3)_4$ ; and ${[F e {(C \equiv N)}_{6}]}_{6}^{3 -}$ $[Fe(C-=N)_6]^(3-)$ ?

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How do you determine the oxidation state of metal ions?

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