NEETChemistryd and f Block Elements
Why is Cr 2+ reducing and Mn 3+ oxidizing when both have d 4 configuration?
Options
- ACr 2+ is reducing as its configuration changes from d 4 to d 3 (half-filled t 2g level) but the change from Mn
- BMn 3+ has a higher effective nuclear charge than Cr 2+ .
- CCr 2+ has a higher ionization energy than Mn 3+ .
- DMn 3+ has a greater number of unpaired electrons in its d-orbitals.
Correct answer
A. Cr 2+ is reducing as its configuration changes from d 4 to d 3 (half-filled t 2g level) but the change from Mn
Step-by-step solution
Correct Option is : (A) Cr 2+ is reducing as its configuration changes from d 4 to d 3 (half-filled t 2g level) but the change from Mn 3+ to Mn 2+ results in the half-filled (d 5 ) configuration which has extra stability.