Home
Class 12
CHEMISTRY
Why is Cr^(2+) reducing and Mn^(3+) oxid...

Why is `Cr^(2+)` reducing and `Mn^(3+)` oxidizing even though both have the same `d^(4)` electronic configuration.

Promotional Banner

Similar Questions

Explore conceptually related problems

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^4 configuration?

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^4 configuration?

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^(4) configuration ?

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^(4) configuration ?

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^(4) configuration ?

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^(4) configuration ?

Why is Cr^(2+) acts as reductant and Mn^(3+) as oxidant eventhough both have d^4 configuration ?

The ion Cr^(2+) is redusing agent while that of Mn^(3+) is an oxidising agent though both have 3d^(4) configuration. This is because