I was reading this paper by Gonzalez and Lima about Methylene Blue's role in the electron transport chain.
http://www.dose-resp...nzalez Lima.pdf
They have some nice charts about how it cycles between oxydized and reduced states, and participates in the electron chain
http://acumensoftwar...om/mb_cycle.png
http://acumensoftwar...donor_chain.png
They then note, that the cycle breaks down, if there is too much MB, because it no longer cycles between states, but instead just takes electrons away from the chain:
At low doses, there is MB‐MBH2 equilibrium (electron
cycling) and MBH2 can donate electrons to ETC
complexes and oxygen, leading to enhanced energy
metabolism and decreased superoxide formation
• At high doses, equilibrium is impaired and MB can take
electrons away from ETC complexes, leading to
decreased activity of these complexes and more
oxidative stress
The chemistry for C60 would work the same with the difference that if C60 acquired too many electrons, it would cause an electrical charge on the mitochondria. The electrical charge would eventually prevent it from acquiring more electrons, thus limiting the amount it could acquire.
Put another way, the C60 adducts in the membrane of the mitochondria should never accept so many electrons that they hinder the electron chain, because they are limited to the surface of the mitochondria, and the electrical charge prevents them from accepting too many electrons. In contract MB, is distributed all over the cell, and the oxidized (charged) form, is hydrophilic, and will be surrounded by H2O which has a large dialectric constant.
Any thoughts?