No, its being oxidized. It has a lower reduction potential.
These are the half reactions from a standard half reaction chart:
I2 + 2e- -> 2I-
ClO- + 2e- -> Cl-
**I2 is being oxidized, so you need to reverse the reaction:
2I^- <- - -> I2 + 2e
ClO- + 2e- -> Cl-
Electrons are balanced.
Write the reduction half reaction for the redox reaction below.
ClO-(aq) + I-(aq) => Cl-(aq) + I2(s)
Is I- being reduced since Cl is losing an O?
4 answers
Ok I had the wrong idea, thanks so much!
I posted an answer/solution to another problem that you had. I think that it explains the concept of what you are suppose to be doing a little bit better, or it can be used as an additional resource to help you with similar problems.
I would like to add here that you had the right idea if you had followed through. Your statement that ClO is losing O is ok but since it is LOSING O is must be reduced. Gaining O is oxidation. Of course if O is nowhere in the oxidation it's tough to use that as a definition which is why you should stick to the definition that oxidation is the loss of electrons and reduction is the gain of electrons. Note that Cl is +1 oxidation state and Cl^- is -1 so the Cl has gained two electrons which makes it reduced.
2 answers