What is Being Reduced?

[Sarah Zhari 1D]

For example, in the equation 2Fe3+(aq) + Cu(s) -> Cu2+(aq) + 2Fe2+ , would we have to say that Fe3+ is being reduced to Fe2+, or is it enough to say that iron is being reduced?

[Anika Chakrabarti 1A]

I think it's better to be specific and include the charges. You could also write out the half-reactions to show that Fe3+ is gaining one electron and is being reduced.

[chemboi]

Transition metals can occur in different oxidation states, so especially in their case it helps to clarify. In general for any species, I think it is helpful to clarify however (not just transition metals)

[Radha Patel 4I]

I think it is sufficient enough to mention how it is being reduced, so in this case it is reduced from 6+ to 4+ electrons

[Connor Chappell 2B]

It would most likely be safer to indicate the oxidation state of the compound especially in the instance of dealing with metals.

[Hui Qiao Wu 1I]

It might be better to include Fe3+ is being reduced to Fe2+, just to show that you know which iron is being reduced. In addition, some problems specifically ask you to include which species is reduced or oxidized and from what oxidation number to what.

[KHowe_1D]

I think it's safer to just be as specific as possible. It is being reduced because it is gaining the electron while Cu is being oxidized because it is losing the electrons.

[Angela Wu-2H]

Is reduction based on charges and electrons or is it based on moles?

[Helen Struble 2F]

In past chem classes, I was taught OILRIG: Oxidation Is Loss, Reduction Is Gain. Since reduction is gaining electrons, the Fe ion is being reduced because its positive charge decreases, so it is becoming, relative to the original species, more negative. This is because electrons have a negative charge, so gaining electrons makes a species more negative.

[SimranSangha4I]

You should try to be as specific as possible and show the redox half reactions to show and indicate you understand what is actually happening. I normally think of the reactions as OILRIG (oxidation is loss [of electrons]) (reduction is gain [of electrons]) so in this particular case, Fe is the one that's being reduced by the reaction.

[Ruby Richter 2L]

So just to clarify because Fe is the one that's being reduced by the reaction it is gaining electrons but its oxidation number goes down?