Electrochemistry

Electrochemistry

The branch of chemistry that deals with the relationship between electrical energy and chemical reactions.

Standard Hydrogen Electrode (SHE)

An electrode that establishes a reference potential of 0.00 V against which other electrodes can be measured.

Electrode potential (E°)

The ability of an electrode to gain or lose electrons, measured in volts.

Reducing Agent

A substance that donates electrons in a chemical reaction and reduces another species.

Half-Cell

A part of an electrochemical cell consisting of a single electrode in a solution of its ions.

Reactivity Series

A list of metals arranged in order of decreasing reactivity.

Nernst Equation

An equation that relates the cell potential (E) to standard electrode potential (E°) and the concentrations of the species involved.

Gibbs Free Energy (ΔG)

A thermodynamic potential that measures the maximum reversible work obtainable from a closed system at constant temperature and pressure.

Faraday's Constant (F)

The amount of charge per mole of electrons, approximately 96485 C/mol.

Oxidation

The process in which an atom or ion loses electrons.

Reduction

The process in which an atom or ion gains electrons.

Voltaic Cell

An electrochemical cell that generates electrical energy from spontaneous chemical reactions.

Salt Bridge

A device used to connect the oxidation and reduction half-cells of a galvanic cell.

Electrolysis

The breakdown of a compound in solution or molten state by passing an electric current through it.

Anode

The electrode where oxidation occurs in an electrochemical cell.

Cathode

The electrode where reduction occurs in an electrochemical cell.

Cation

A positively charged ion that moves towards the cathode.

Anion

A negatively charged ion that moves towards the anode.

Cell Potential (E_cell)

The difference in electrical potential between two electrodes in an electrochemical cell.

Combining Half-Cells

The process of adding the standard electrode potentials of two half-cells to obtain the cell potential.

Reactive Metals

Metals that readily lose electrons and are strong reducing agents.

Inert Electrode

An electrode that does not participate in the reaction but helps to conduct electricity.