Redox

A redox reaction is a chemical reaction that involves the transfer of electrons between two species, resulting in changes in oxidation states.

Oxidation is the process in which an atom, ion, or molecule loses electrons, resulting in an increase in oxidation state.

Reduction is the process in which an atom, ion, or molecule gains electrons, resulting in a decrease in oxidation state.

The oxidation number is a value assigned to an element in a compound that represents the number of electrons lost or gained by that element during a chemical reaction.

An electrolytic cell is an electrochemical cell that uses electrical energy to drive a non-spontaneous chemical reaction.

A voltaic cell, also known as a galvanic cell, is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions.

Oxidation occurs at the anode of an electrolytic cell.

Reduction occurs at the cathode of an electrolytic cell.

A salt bridge allows the flow of ions between the two half-cells, maintaining electrical neutrality and completing the circuit.

The standard electrode potential indicates the tendency of a species to be reduced, with higher values indicating a greater tendency to gain electrons.