The electron carrier’s role in energy transfer is to act as a middleman in the transfer of elections between reactions. A typical example of an electron carrier is Nicotinamide Adenine Dinucleotide (NAD+), which has an oxidized and reduced form (NADH). The term oxidation refers to the loss of electrons while reduction is the gain of electrons. For every oxidation, there must be a reduction because there cannot be any free electrons in the cell. The oxidized and reduced forms are called the “conjugate base pairs” within a reaction. Reduction potential, or the affinity for electrons, is determined experimentally using a volt meter to measure electron flow. It is related to the H+ ions in a reaction; if a reaction has a positive reduction potential, the oxidized form has a higher affinity for the electrons than H+. On the other hand, a negative reduction potential has an oxidized form with a lower affinity for electrons than H+. Additionally, a transfer of e- from molecules of low affinity to high affinity releases energy and is spontaneous.
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