NCERT Example question (d & f block)
In the NCERT textbook, the Example question no.4 has bothered me for a bit now.
The given solution states that Cr2+ prefers being oxidised to Cr3+ by losing an electron, as then it's t_2g orbital is half filled, giving it a stable configuration.
It then says that Mn3+, which has the same configuration as Cr2+, will instead gain electron to attain stable half filled d shell.
However, if the two ions have the same configuration, why do they not behave in the same manner? Furthermore, how will Cr2+ have the e_g and t_2g splitting if there is no ligand field, and we are considering only the ion in solution?
I feel the explanation in the text is insufficient for these reasons. I would appreciate an explanation or a source to refer to for this.
6 Replies
@Dexter
Note for OP
+solved @user1 @user2... to close the thread when your doubt is solved. Mention the users who helped you solve the doubt. This will be added to their stats.nature does what it wants. dead serious.
Btw have you checked this out in JD lee? perhaps a difference in E0 values in water led to this.
There's a stack exchange answer explaining exactly the same question and that too satisfactorily
Lemme shoot you the link a bit
https://chemistry.stackexchange.com/a/45168/141947
Here you go!
BTW good doubt
I had it too when I studied this 🙂
+solved @Varun_Arora
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