Positive electrode potential and negative electrode potential are terms used in electrochemistry to describe the electrical potential (voltage) of electrodes in an electrochemical cell. These terms are often referred to in the context of standard electrode potentials and cell potentials.
- Positive Electrode Potential: The positive electrode potential, also known as the oxidation potential or anode potential, refers to the potential difference between a given electrode and the standard hydrogen electrode (SHE) when the electrode is involved in an oxidation reaction (losing electrons). It indicates the tendency of the electrode to lose electrons and undergo oxidation.
- Negative Electrode Potential: The negative electrode potential, also known as the reduction potential or cathode potential, refers to the potential difference between a given electrode and the standard hydrogen electrode (SHE) when the electrode is involved in a reduction reaction (gaining electrons). It indicates the tendency of the electrode to gain electrons and undergo reduction.
In simpler terms, positive electrode potential relates to the ease of losing electrons (oxidation), while negative electrode potential relates to the ease of gaining electrons (reduction).
These potentials are measured in volts and are crucial in determining the direction and feasibility of electrochemical reactions. The larger the positive electrode potential, the more likely the electrode is to undergo oxidation. Conversely, the more negative the negative electrode potential, the more likely the electrode is to undergo reduction.
It's important to note that the terms "positive" and "negative" electrode potentials are relative to the standard hydrogen electrode (SHE), which has a defined potential of 0 volts. All other electrode potentials are measured with respect to the SHE.
In summary, positive electrode potential represents the tendency of an electrode to undergo oxidation, while negative electrode potential represents the tendency to undergo reduction. These potentials are essential in understanding and predicting the behavior of electrochemical cells and reactions.
