Oxidation-Reduction Reactions and Electrochemistry

Key vocabulary and concepts related to oxidation-reduction reactions, electrochemistry, and voltaic/electrolytic cells.

Redox Reaction

An oxidation-reduction reaction that involves the transfer of electrons from one atom to another.

Oxidation

The loss of electrons from atoms of a substance.

Redox Reaction

An oxidation-reduction reaction that involves the transfer of electrons from one atom to another.

Oxidation

The loss of electrons from atoms of a substance.

Reduction

The gain of electrons by the atoms of a substance.

Oxidation Number

The number of electrons lost or gained by the atom when it forms an ion in an ionic compound.

Oxidizing Agent

The substance that oxidizes another substance by accepting its electrons.

Reducing Agent

The substance that reduces another substance by losing its electrons.

Disproportionation

A process in which a substance acts as both an oxidizing agent and a reducing agent.

Electrochemistry

The study of the redox processes by which chemical energy is converted to electrical energy and vice versa.

Voltaic Cell

A type of electrochemical cell that converts chemical energy to electrical energy by a spontaneous redox reaction.

Anode

The electrode where oxidation takes place.

Cathode

The electrode where reduction occurs.

Salt Bridge

A pathway to allow the passage of ions from one side to another, so that ions do not build up around the electrodes.

Volt

A unit used to measure cell potential—the force from the difference in electric potential energy between two electrodes.

Reduction Potential

The tendency of a substance to gain electrons.

Standard Hydrogen Electrode (SHE)

The standard half-cell used as a reference for determining the relative potential of other half-reactions.

Electrolytic Cell

If electrical energy is required to produce a redox reaction in an electrochemical cell

Electroplating

A metal ion is reduced and a solid metal is deposited on a surface