Electrodes

Electrode potential: The difference in electric potential between an electrode and its surroundings, measured in volts.

Half-cell reactions: The oxidation and reduction reactions that occur at each electrode in an electrochemical cell.

Anode and cathode: The electrodes where oxidation and reduction reactions occur, respectively.

Electrolyte: The solution or medium that conducts electricity between the electrodes in an electrochemical cell.

Galvanic cell: A type of electrochemical cell that converts chemical energy into electrical energy.

Electrolytic cell: A type of electrochemical cell that uses electricity to drive non-spontaneous redox reactions.

Faraday's laws of electrolysis: The relationship between the amount of substance produced or consumed during an electrolysis reaction and the quantity of electrical charge consumed or produced.

Standard electrode potential: The electrode potential of a half-cell under standard conditions, which helps predict the direction and extent of redox reactions.

Nernst equation: A mathematical equation that relates the electrode potential, ion concentration, and temperature to the equilibrium constant of a redox reaction.

Reference electrode: An electrode with a constant, known electrode potential, used to measure the electrode potential of other half-cells.

pH electrode: An electrode that measures hydrogen ion concentration in a solution, used in acid-base and redox reactions.

Working electrode: The electrode where the chemical reaction of interest takes place in electrochemical experiments.

Impedance spectroscopy: A method of analyzing the electrical response of an electrochemical system to a range of frequencies or applied potentials.

Voltammetry: A technique used to measure the current as a function of applied voltage in an electrochemical cell, commonly used to study kinetics and thermodynamics of redox reactions.

Bioelectrochemistry: The study of electrochemical reactions involving biological molecules and systems, with applications in biosensors, bioenergy, and bioremediation.

Reference Electrodes: Reference electrodes are used as a standard point of reference in electrochemical cells. They have a stable potential and do not contribute to the electrochemical reaction. They are typically made of metals or metal ions in solution.

Working Electrodes: The working electrode is where the electrochemical reaction takes place. They are typically made of metals, carbon, or conductive polymers.

Indicator Electrodes: Indicator electrodes are used to detect a specific ion or molecule in a sample. They are coated with a membrane that selectively interacts with the analyte.

Ion-selective Electrodes: Ion-selective electrodes (ISEs) are used to measure the concentration of a specific ion in a sample. They are similar to indicator electrodes, but are optimized for a specific ion.

Gas-sensing Electrodes: Gas-sensing electrodes are used to measure the concentration of a gas in a sample. They typically consist of a metal oxide film that interacts with the gas and produces a measurable response.

pH Electrodes: PH electrodes are used to measure the acidity or alkalinity of a sample. They work by measuring the voltage difference between a pH-sensitive membrane and a reference electrode.

Enzyme Electrodes: Enzyme electrodes are used to measure the concentration of an enzyme in a sample. They work by immobilizing the enzyme on the surface of the electrode, and measuring the current or potential produced as the enzyme reacts with its substrate.

Biosensors: Biosensors are miniaturized analytical devices that use biological molecules, such as enzymes or antibodies, to detect analytes. They typically consist of a working electrode, a reference electrode, and a biosensing layer.

Conductivity Electrodes: Conductivity electrodes are used to measure the conductivity of a solution. They typically consist of two electrodes separated by a distance, and measure the current flowing between the electrodes.

Potentiometric Electrodes: Potentiometric electrodes measure the potential difference between two electrodes immersed in the same solution. They are used to measure the concentration of an analyte that produces a measurable voltage difference.