Electrochemistry Fundamentals

Electrochemistry explores the link between chemical energy and electrical energy, investigating their conversions.

A device where chemical energy from a Redox reaction is transformed into electrical energy.

An electrolytic cell converts electrical energy into chemical energy.

The potential difference between a metal plate and its ion solution.

Factors affecting electrode potential are: electrode material, solution temperature, and concentration of metal ions.

A standardized electrode potential measured under specific conditions.

The conditions for S.E.P. are 25°C temperature, 1 atm pressure, and unity concentration of ions.

S.E.P. is symbolized as E°.

Redox reactions involve the transfer of electrons between species.

Oxidation is the loss of electrons by a species.

Reduction is the gain of electrons by a species.

In an electrochemical cell, oxidation occurs at the anode.

In an electrochemical cell, reduction occurs at the cathode.

The driving force behind the flow of electrons in an electrochemical cell.

The difference in electrode potentials between the anode and cathode.

The cell potential determines the direction of electron flow in an electrochemical cell.

A positive cell potential indicates a spontaneous reaction.

A negative cell potential indicates a non-spontaneous reaction.

Electrolytic cells use external energy sources to drive non-spontaneous reactions.

Understanding electrochemistry is crucial for application in batteries, fuel cells, corrosion, and electroplating.