Why Does Cr2+ Reduce While Mn3+ Oxidizes Despite Both Having d4 Configuration?

RandomGuy1 · 2013-10-02T15:21:49+00:00

Why is Cr2+ reducing while Mn3+ oxidizing when they both have d4 configuration?

Thread starter RandomGuy1
Start date Oct 2, 2013
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Oxidation Reduction

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The discussion centers on the contrasting redox behaviors of Cr2+ and Mn3+, despite both having a d4 electron configuration. It emphasizes that the d4 configuration alone does not dictate whether an ion will act as a reducing or oxidizing agent. The reduction of Cr2+ is attributed to its lower ionization energy and favorable thermodynamics compared to Mn3+, which tends to oxidize due to its higher oxidation potential. Factors such as electronegativity, stability of oxidation states, and overall electron configuration play significant roles in these reactions. Understanding these nuances is crucial for predicting redox behavior in transition metals.

Oct 2, 2013

RandomGuy1

Why is Cr²⁺ reducing while Mn³⁺ oxidizing when they both have d⁴ configuration?

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Oct 2, 2013

Borek

Mentor

d⁴ is not the driving force behind oxidation and/or reduction.

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