Bioenergetics and redox — In cellular metabolism, what does a positive standard redox potential (E°' > 0) indicate about a substance's tendency regarding electrons?

Introduction / Context:
Redox (reduction–oxidation) reactions power metabolism by transferring electrons from donors to acceptors. The standard redox potential, E°', is a quantitative measure of how strongly a redox couple attracts electrons under biochemical standard conditions. Understanding the sign of E°' is crucial for predicting electron flow through the electron transport chain and many dehydrogenase reactions.

Given Data / Assumptions:

• E°' is reported at pH 7.0, 25 °C, 1 atm, and defined reactant/product activities.
• Electron transfer spontaneously proceeds from a lower potential (more negative E°') to a higher potential (more positive E°').
• Reduction means electron gain; oxidation means electron loss.

Concept / Approach:
E°' compares a redox couple’s tendency to be reduced relative to a reference (typically the standard hydrogen electrode in classical electrochemistry; in biochemistry, values are adjusted to pH 7 and denoted with double prime). A positive E°' signifies a strong oxidizing agent, meaning the oxidized form of the couple has a high tendency to accept electrons. Conversely, a very negative E°' indicates a strong reducing agent that readily donates electrons.

Step-by-Step Solution:

Verification / Alternative check:
In mitochondrial electron transport, NADH/NAD+ has a relatively negative E°', whereas O2/H2O has a highly positive E°'. Electrons flow from NADH to O2, consistent with the concept that more positive potentials represent stronger electron acceptors.

Why Other Options Are Wrong:

Common Pitfalls:
Confusing the sign convention; assuming “positive” equals “more reduced” rather than “more easily reduced” (i.e., stronger oxidant).

Final Answer:
Higher affinity for electrons (tends to accept).