Final answer:
Redox potential is a key chemical concept that measures the tendency of a species to gain electrons, related to free energy change and equilibrium constant, and is used to predict the direction of electron flow in redox reactions.
Step-by-step explanation:
The concept of redox potential, also known as oxidation-reduction potential, in chemistry is a measure of the tendency of a chemical species to acquire electrons and be reduced. The redox potential is indicative of the energy level associated with the gain or loss of electrons in a redox reaction. This potential is measured relative to the standard hydrogen electrode which has an assigned potential of zero volts under standard conditions.
Redox potential is directly related to the free energy change (ΔG) and the equilibrium constant (K) for a given redox process. In the context of electrochemistry, the redox potential can be calculated using the Nernst equation, which takes into account the number of electrons transferred in the reaction (n), the concentrations of the reacting species (Q), and the temperature (T). This relationship is fundamental to determining the direction and extent of chemical reactions.
Compounds with a positive redox potential compared to hydrogen tend to be poor electron donors, whereas those with a negative potential are better electron donors. This differential potential governs the direction of electron flow during redox reactions, contributing significantly to the stability and energy of compounds involved.