21thnks again......so we have to remember E0 values.
this is an example question from the ncert textbook-
"Why is Cr2+ reducing and Mn3+ oxidising when both have d4 configuration?
Cr2+ is reducing as its configuration changes from d4 to d3, the latter
having a half-filled t2g level (see Unit 9) . On the other hand, the change from Mn2+ to Mn3+ results in the half-filled (d5) configuration which has extra stability."
my question is that why the reverse cant be true i-e Cr+2 is oxidising and Mn+3 is reducing or it is an experimental thing?
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3 Answers
29No the reverse is not true...this is based upon E° values of the ions..
29no..dont mug up those E° values..it can be explained on the basis of stability as mentioned in NCERT and moreover u may see the common reactions ..like Cr exist in +3 and +6 state generally and Mn in +2, +4 and +7...