Standard Electrode Potential
The potential of a half-cell measured against the standard hydrogen electrode under standard conditions.
Formula / equation
E° at 298 K, 1 M, 1 bar
Unit
V
In depth
By convention these are quoted as reduction potentials, so a more positive value indicates a stronger tendency to be reduced and hence a stronger oxidising agent. Because only differences are measurable, all values are relative to the arbitrary zero of the hydrogen electrode.
Examples in the real world
F₂/F⁻ at +2.87 V is the strongest common oxidant; Li⁺/Li at −3.04 V is the strongest reductant.