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Question: $[(\text{H}_2\text{O})_4\text{Co}(\text{O}_2)_2\text{Co}(\text{H}_2\text{O})_4](\text{SO}_4)_2 \xri...

[(H2O)4Co(O2)2Co(H2O)4](SO4)2→[X] reagent[(H2O)4Co(O2)2Co(H2O)4](SO4)[(\text{H}_2\text{O})_4\text{Co}(\text{O}_2)_2\text{Co}(\text{H}_2\text{O})_4](\text{SO}_4)_2 \xrightarrow{[\text{X}]\text{ reagent}} [(\text{H}_2\text{O})_4\text{Co}(\text{O}_2)_2\text{Co}(\text{H}_2\text{O})_4](\text{SO}_4). In both the complex Co has t2g6eg0t_{2g}^6e_g^0configuration. Which option is incorrect? (I) (II)

A

Complex (I) is Paramagnetic

B

Complex (II) is Diamagnetic

C

(X) is oxidising agent

D

(X) is reducing agent

Answer

(X) is oxidising agent

Explanation

Solution

The given reaction involves a change in the oxidation state of the oxygen ligands coordinated to Cobalt (Co).

  • Complex I: [(H2O)4Co(O2)2Co(H2O)4](SO4)2[(\text{H}_2\text{O})_4\text{Co}(\text{O}_2)_2\text{Co}(\text{H}_2\text{O})_4](\text{SO}_4)_2 contains superoxo ligands (O2−\text{O}_2^{-}), making it paramagnetic.
  • Complex II: [(H2O)4Co(O2)2Co(H2O)4](SO4)[(\text{H}_2\text{O})_4\text{Co}(\text{O}_2)_2\text{Co}(\text{H}_2\text{O})_4](\text{SO}_4) contains peroxo ligands (O22−\text{O}_2^{2-}), making it diamagnetic.

The conversion of superoxo to peroxo involves a reduction process (gain of electrons). Therefore, reagent X must be a reducing agent, not an oxidizing agent.