It would be the first time I've every seen it, but "something a little different" is kind of what they like to do. If you're a memorizer, that can be dangerous, but if you understand it doesn't matter. Larger, more positive or less negative E values mean the specie on the reactant side of the half-reaction wants to be reduced relatively more than whatever you are comparing to ; Lower, less positive or more negative E values mean the specie on the reactant side of the half-reaction wants to be reduced LESS than what you are comparing to, so it will be oxidized in that pair. Great electrochemistry take homes:
1. Flipping the half-reaction flips the sign of the E value
2. oxidation to reduction or vice versa flips the sign of the E value
3. NO STOICHIOMETRY! For the Hess's Law half-reactions in genchem you must multiply the deltaG, deltaH or entropy by the coefficient, but with electrochem the E is whatever it is no matter how many moles of electrons.
4. REDOX = PAIRS ONLY: There has to be two (2) things! It's either a cell connecting two solutions/ions or its two species in a RXN. ONE thing never does REDOX anything; so if something is happening (i.e., X is getting reduced), the opposite is happening to someone else (something called Y has to be getting oxidized. The electrons have to come from some where, we aren't creating matter!) If I had a penny every time a student started talking about Fe3+ or Cu+ "doing REDOX" With whom I ask? What do you mean? they say...