Redox behavior definition

Experimentally, such a square scheme (Scheme 1) can be deduced from a real CV titration. The fact that the guest s reduction gets easier is indicated by a shift toward more positive potentials. For oxidations, the shift would be toward more negative potentials. This redox-shift behavior definitively indicates that the complex gets more stable after the ET. Therefore, it is fair to use the formal redox potentials observed from the CVs as the true thermodynamic values in the square scheme that is, E. The H G stability can be independently measured using typical methods, allowing the stability of the reduced (or oxidized) complex (i.e., 3 " ) to be calculated from the three measured parameters 1, 2). 

The definitive study on this topic was reported by Saveant and coworkers117. They note a dichotomy between behavior of reagents believed to be involved in outer-sphere (redox) and inner-sphere (chemical) electron transfer processes. Outer-sphere reagents such as... 

Examples of electroactive NP materials discussed in the review include Ti02, Mn02, iron oxides, other metal oxides, hydroxides and oxyhydroxides and Prussian Blue. We use the term electroactive N Ps to refer to the faradaic electroactivity in such materials and to distinguish them from NPs comprised of metals (such as Au, Ag, Pt, Co, etc.) or semiconductors (such as CdS, CdSe, etc.). This distinction is based on the ability of many electroactive NPs to undergo faradaic oxidation or reduction of all of the metal (redox) centers in the NP. This is in contrast to the behavior of many metal and semiconductor NPs for which oxidation or reduction is fundamentally an interfacial, double-layer process. This definition is somewhat arbitrary, since the smallest metal and semiconductor NPs behave molecularly, blurring the distinction... 

---