Understanding Redox Reactions: Gain and Loss of Electrons

Redox is a term used in chemistry to describe the transfer of electrons from one molecule to another. The word "redox" comes from the phrase "reduction-oxidation," which refers to the gaining or losing of electrons by a molecule.

In a redox reaction, one molecule (the reducing agent) loses electrons and another molecule (the oxidizing agent) gains electrons. This transfer of electrons can result in a change in the oxidation state of one or both of the molecules involved in the reaction.

Redox reactions are common in many areas of chemistry, including electrochemistry, organic chemistry, and biochemistry. They are also important in many industrial processes, such as the production of batteries and fuel cells.

Some examples of redox reactions include:

* The oxidation of glucose to produce energy in cells
* The reduction of iron(III) ions to form iron(II) ions in rusting
* The oxidation of hydrogen gas to form water in a fuel cell
* The reduction of oxygen gas to form water in the electrolysis of water.