What is the oxidation state of the metal centre in $[F e {(O H_{2})}_{5} (N C S)] S O_{4}$ $[Fe(OH_2)_5(NCS)]SO_4$ ?

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What is the oxidation state of the metal centre in $[F e {(O H_{2})}_{5} (N C S)] S O_{4}$ $[Fe(OH_2)_5(NCS)]SO_4$ ?

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Answer 1 · 2017-05-01T15:31:22

We have $ferric ion$ $"ferric ion"$ , i.e. $F e (+ I I I)$ $Fe(+III)$ .

Explanation:

We have ${[F e {(O H_{2})}_{5} (N C S)]}_{5}^{2 +} S O_{4}^{2 -}$ $[Fe(OH_2)_5(NCS)]^(2+)SO_4^(2-)$ .

And the actual complex ion is ${[F e {{(O H)}_{2}}_{5} (N C S)]}_{5}^{2 +}$ $[Fe{(OH)_2}_5(NCS)]^(2+)$ after we remove the $S O_{4}^{2 -}$ $SO_4^(2-)$ counterion. The water ligands are neutral, but the thiocyanate ion has a formal $- 1$ $-1$ charge. And thus we have an $F e^{3 +}$ $Fe^(3+)$ centre. Capisce?

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What is the oxidation state of the metal centre in $[F e {(O H_{2})}_{5} (N C S)] S O_{4}$ $[Fe(OH_2)_5(NCS)]SO_4$ ?

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What is the oxidation state of the metal centre in [Fe(OH2)5(NCS)]SO4[Fe(OH_2)_5(NCS)]SO_4?

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What is the oxidation state of the metal centre in $[F e {(O H_{2})}_{5} (N C S)] S O_{4}$ $[Fe(OH_2)_5(NCS)]SO_4$ ?