Trends in Increasing Reducing Ability

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Emilie Hoffman 1E
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Joined: Fri Sep 29, 2017 6:04 am

Trends in Increasing Reducing Ability

Postby Emilie Hoffman 1E » Fri Feb 23, 2018 12:23 am

To compare this between different elements, do we need to compare the same increase in oxidation number? For example, if we were comparing Cu and Cr, do we have to use Cu2+ ---> Cu in comparison with Cr2+ ---> Cr, or can we compare between different oxidation state changes?

Deap Bhandal L1 S1J
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Re: Trends in Increasing Reducing Ability

Postby Deap Bhandal L1 S1J » Fri Feb 23, 2018 12:31 pm

I believe you would use the equation where it the ion goes to neutral. So like In3+ to In instead of In3+ to In2+.

Emilie Hoffman 1E
Posts: 55
Joined: Fri Sep 29, 2017 6:04 am

Re: Trends in Increasing Reducing Ability

Postby Emilie Hoffman 1E » Sat Feb 24, 2018 3:47 pm

So is there any importance in comparing equal oxidation states going to a neutral atom? For example, would Cu2+ ---> Cu and Cr3+ ---> Cr be just as valid a comparison as Cu2+ ---> Cu and Cr2+ ---> Cr?

Christine Wastila 1H
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Re: Trends in Increasing Reducing Ability

Postby Christine Wastila 1H » Sat Feb 24, 2018 8:05 pm

I think you would want to compare using two equations where the amount of electrons transferred is the same.

Shreya Ramineni 2L
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Re: Trends in Increasing Reducing Ability

Postby Shreya Ramineni 2L » Mon Feb 26, 2018 1:39 pm

The more negative in potential, the more likely the substance is to be oxidized/work as a reducing agent. Therefore it has more of a reducing power.

mayasinha1B
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Re: Trends in Increasing Reducing Ability

Postby mayasinha1B » Wed Mar 07, 2018 11:36 am

The more negative the E standard for a given half reaction is, the less likely that reaction is to take place in the given reduction state. If you think about it, a more negative E standard yields a more positive delta G with a lowered likelihood of spontaneity. So the higher value will be reduced and the lower value will be oxidized.


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