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Oxidation is discussed in the context of a chemical reaction.
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I mislead the discussion by misinterpreting oxidative state as oxidizing agent. It wasn't intentional. Oxidative state applies to, "... already-bonded molecules". I think when I mentioned electronegativity, you were thinking about oxygen's valence shell and how it is a very good electron acceptor due to lacking an electron.
It is interesting how this explanation conflicts as the textbooks I'm reading states that oxygen as the terminal electron acceptor that exists in Complex IV is present in the neutral molecular state as you explained in your previous post: . Therefore the perspective of electronegativity as an aspect of electron attraction via valence electrons doesn't quite satisfy the overall view of the metabolic reaction.
The notion of oxygen fulfilling its electronegative requirement as a radical, such as a superoxide anion, is also incorrect in the fact that such elements are dangerous free radicals and are reduced by enzymes such as superoxide dismutase to form peroxide and molecular oxygen.
In the instance where we have mutual understanding, generalizing oxygen in a biological context as being naturally electronegative is conducive to putting a band-aid on a gaping wound. Perhaps the juvenile biological premise is a gross generalization that never took into account the individual electron transfers that occur at each Complex in the biochemical pathway. When I have time to read through more explanations, I'll write you a visitor message if you are still interested in continuing this conversation. But I think that was what you were trying to get at previously, if I'm not mistaken.
