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Chemistry Forums for Students => Inorganic Chemistry Forum => Topic started by: user1000 on November 13, 2014, 06:20:51 AM

Title: Why is standard reduction potential for Mn3+ to Mn2+ so big?
Post by: user1000 on November 13, 2014, 06:20:51 AM

Can someone explain this?

Thanks

Title: Re: Why is standard reduction potential for Mn3+ to Mn2+ so big?
Post by: Irlanur on November 13, 2014, 06:26:06 AM

whats the electronic configuration in the two species? which one do you expect to be more stable?

Title: Re: Why is standard reduction potential for Mn3+ to Mn2+ so big?
Post by: user1000 on November 13, 2014, 07:08:15 AM

Quote from: Irlanur on November 13, 2014, 06:26:06 AM

whats the electronic configuration in the two species? which one do you expect to be more stable?

Is Mn2+ more stable because it has both d orbital energy levels half filled while mn3+ does not?

Title: Re: Why is standard reduction potential for Mn3+ to Mn2+ so big?
Post by: Irlanur on November 13, 2014, 02:51:50 PM

both?

Title: Re: Why is standard reduction potential for Mn3+ to Mn2+ so big?
Post by: darayoush on November 14, 2014, 03:06:54 PM

but i think oxidation of Mn2+ to Mn3+ must be large.because Mn2+ is d5 and is half full.but Mn3+ is lower than half and Mn prefer the stable form.

Title: Re: Why is standard reduction potential for Mn3+ to Mn2+ so big?
Post by: kriggy on November 14, 2014, 03:38:54 PM

Yea its quite high
Mn3+(aq) + e- → Mn2+(aq) +1.51

But the form it prefers also depends on other factors. I mean, this redox reaction is going like all the time at biological conditions without much trouble