Lecture

Solid Surfaces in a Liquid: Surface Charge and Electrical Double Layer

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EE-515: Fundamentals of biosensors and electronic biochips

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Description

This lecture discusses the behavior of solid surfaces in a liquid environment, focusing on the presence of electrolytes, surface charge density, and the formation of the electrical double layer. It covers topics such as the density of counterions at the surface, the calculation of surface charge, the capacitance model at the interface, and the structure of the electrical double layer. The interaction between counterions and the solid surface, as well as the distribution of charges in the electrolyte, are explained in detail. Additionally, the lecture explores electron transfer at electrolyte/electrode interfaces and the different types of electrode interfaces. The concepts of nonpolarizable and polarizable interfaces are also addressed.

Instructor

Carlotta Guiducci

Teaching & PhD PhD Students Micaela Siria Cristofori, Edoardo Bargis, Yide Jiao, Seyyed Hamid Sadat Mansoury Past EPFL PhD Students Giulia Cappi, Enrico Accastelli, Anna Ferretti, Enrica Rollo, Samuel Kilchenmann, Elena-Diana Bojescu, Kevin Keim, Pierre-Emmanuel Marie Thiriet, Saurabh Tomar, Gloria Porro, Till Jonathan Ryser Past EPFL PhD Students as codirector Yüksel Temiz Courses Electrical systems and electronics I EE-295 The course has the aim to provide the fundamental knowledge and e

Official source

Ontological neighbourhood

Chemistry

Physical chemistry: Electrochemistry

Related concepts (32)

Electrode potential

In electrochemistry, electrode potential is the electromotive force of a galvanic cell built from a standard reference electrode and another electrode to be characterized. By convention, the reference electrode is the standard hydrogen electrode (SHE). It is defined to have a potential of zero volts. It may also be defined as the potential difference between the charged metallic rods and salt solution. The electrode potential has its origin in the potential difference developed at the interface between the electrode and the electrolyte.

Electrode

An electrode is an electrical conductor used to make contact with a nonmetallic part of a circuit (e.g. a semiconductor, an electrolyte, a vacuum or air). Electrodes are essential parts of batteries that can consist of a variety of materials depending on the type of battery. The electrophore, invented by Johan Wilcke, was an early version of an electrode used to study static electricity. Electrodes are an essential part of any battery. The first electrochemical battery made was devised by Alessandro Volta and was aptly named the Voltaic cell.

Standard hydrogen electrode

In electrochemistry, the standard hydrogen electrode (abbreviated SHE), is a redox electrode which forms the basis of the thermodynamic scale of oxidation-reduction potentials. Its absolute electrode potential is estimated to be 4.44 ± 0.02 V at 25 °C, but to form a basis for comparison with all other electrochemical reactions, hydrogen's standard electrode potential (E°) is declared to be zero volts at any temperature. Potentials of all other electrodes are compared with that of the standard hydrogen electrode at the same temperature.

Polarizer

A polarizer or polariser (see spelling differences) is an optical filter that lets light waves of a specific polarization pass through while blocking light waves of other polarizations. It can filter a beam of light of undefined or mixed polarization into a beam of well-defined polarization, that is polarized light. The common types of polarizers are linear polarizers and circular polarizers. Polarizers are used in many optical techniques and instruments, and polarizing filters find applications in photography and LCD technology.

Standard electrode potential

In electrochemistry, standard electrode potential , or , is a measure of the reducing power of any element or compound. The IUPAC "Gold Book" defines it as: "the value of the standard emf (electromotive force) of a cell in which molecular hydrogen under standard pressure is oxidized to solvated protons at the left-hand electrode". The basis for an electrochemical cell, such as the galvanic cell, is always a redox reaction which can be broken down into two half-reactions: oxidation at anode (loss of electron) and reduction at cathode (gain of electron).

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