How would you account for the following:(i) Cr2+ is reducing in nature

1.	How would you account for the following:(i) Cr2+ is reducing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidising agent.(ii) In a transition series of metals, the metal which exhibits the greatest number of oxidation occurs in the middle of the series.
Answer» (i) Cr²⁺ is reducing as its configuration changes from d⁴ to d³, a more stable half filled t_2g configuration while Mn³⁺ is oxidising as Mn³⁺ to Mn²⁺results a more stable half filled d⁵ configuration. (ii) It is due to greater number of unpaired electrons in (n–1)d and ns orbitals at the middle of the series.

How would you account for the following:(i) Cr2+ is reducing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidising agent.(ii) In a transition series of metals, the metal which exhibits the greatest number of oxidation occurs in the middle of the series.

Answer»

(i) Cr²⁺ is reducing as its configuration changes from d⁴ to d³, a more stable half filled t_2g configuration while Mn³⁺ is oxidising as Mn³⁺ to Mn²⁺results a more stable half filled d⁵ configuration.

(ii) It is due to greater number of unpaired electrons in (n–1)d and ns orbitals at the middle of the series.

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How would you account for the following:(i) Cr2+ is reducing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidising agent.(ii) In a transition series of metals, the metal which exhibits the greatest number of oxidation occurs in the middle of the series.

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