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Related Concept Videos

Processes at Electrodes01:30

Processes at Electrodes

The electrode interacts with ions in the electrolyte solution at its interface. The rate of oxidation and reduction depends on the speed at which electrons can transfer through this interface. As ions attach to or leave the electrode surface, the electrode acquires a charge, and an electrical potential forms across the interface, making the process more difficult to reach equilibrium. The charge on the electrode affects the local ion concentrations in the solution, though thermal motion...
Buffer Effectiveness02:19

Buffer Effectiveness

Buffer solutions do not have an unlimited capacity to keep the pH relatively constant . Instead, the ability of a buffer solution to resist changes in pH relies on the presence of appreciable amounts of its conjugate weak acid-base pair. When enough strong acid or base is added to substantially lower the concentration of either member of the buffer pair, the buffering action within the solution is compromised.
The buffer capacity is the amount of acid or base that can be added to a given volume...
Theory of Strong Electrolytes01:23

Theory of Strong Electrolytes

The interionic forces of the strong electrolytes depend on the solvent's dielectric constant, which is the ability of a solvent to store electrical energy, based on its polarizability. and the solution's concentration. In high-dielectric solvents and in dilute solutions, weak electrostatic forces keep ions apart. However, in low-dielectric solvents or concentrated solutions, stronger interionic forces may cause ions to pair up as ionic doublets despite being fully ionized. The theory of strong...
Buffers02:56

Buffers

A solution containing appreciable amounts of a weak conjugate acid-base pair is called a buffer solution, or a buffer. Buffer solutions resist a change in pH when small amounts of a strong acid or a strong base are added. A solution of acetic acid and sodium acetate is an example of a buffer that consists of a weak acid and its salt: CH3COOH (aq) + CH3COONa (aq). An example of a buffer that consists of a weak base and its salt is a solution of ammonia and ammonium chloride: NH3 (aq) + NH4Cl...
Standard Electrode Potentials03:02

Standard Electrode Potentials

On comparing the reactivity of silver and lead, it is observed that the two ionic species, Ag+ (aq) and Pb2+ (aq), show a difference in their redox reactivity towards copper: the silver ion undergoes spontaneous reduction, while the lead ion does not. This relative redox activity can be easily quantified in electrochemical cells by a property called cell potential. This property is commonly known as cell voltage in electrochemistry, and it is a measure of the energy which accompanies the charge...
The Electrical Double Layer01:30

The Electrical Double Layer

In the region where two bulk phases meet, an intricate electric charge distribution arises due to charge transfer, ion adsorption, molecular orientation, and charge distortion. This complex distribution is commonly referred to as the electrical double layer.When a solid electrode interfaces with ions in an electrolyte solution, the speed of electron transfer dictates the rates of oxidation and reduction. The electrode acquires a charge through the escape of atoms into the solution as cations or...

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Updated: Jun 20, 2026

Electrochemical Detection of Deuterium Kinetic Isotope Effect on Extracellular Electron Transport in Shewanella oneidensis MR-1
09:00

Electrochemical Detection of Deuterium Kinetic Isotope Effect on Extracellular Electron Transport in Shewanella oneidensis MR-1

Published on: April 16, 2018

The electron buffer effect for advanced electrocatalysis.

Weimo Li1,2,3, Xiwen Huang3, Lin Xu2

  • 1College of Physics and Electronic Information Engineering, Department of Materials Science and Engineering, Zhejiang Normal University Jinhua Zhejiang 321004 P. R. China liweimo@zjnu.edu.cn zqli@zjnu.edu.cn.

Chemical Science
|June 19, 2026
PubMed
Summary
This summary is machine-generated.

Catalyst electronic structures change during electrocatalysis, affecting performance. The electron buffer effect, like a chemical buffer, stabilizes active sites by regulating electron density, enhancing catalyst activity and stability.

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Area of Science:

  • Materials Science
  • Electrochemistry
  • Catalysis

Background:

  • Catalyst electronic structures often transform irreversibly during electrocatalysis, impacting performance.
  • The electron buffer effect, involving dynamic electron density regulation, is crucial for electrocatalytic enhancement.

Purpose of the Study:

  • To systematically review the mechanisms and applications of the electron buffer effect in electrocatalysis.
  • To provide guidance for designing advanced electrocatalytic materials.

Main Methods:

  • Literature review and systematic analysis of existing studies on electron buffer effects.
  • Categorization of buffer materials into metal-based and nonmetal-based systems.

Main Results:

  • The electron buffer effect stabilizes optimal valence states, mitigates over-oxidation/reduction, and optimizes intermediate adsorption/desorption.
  • Identified metal-based and nonmetal-based buffer systems and their roles in key electrocatalytic reactions.

Conclusions:

  • Understanding dynamic electronic structure design is essential for advanced electrocatalysis.
  • Further research on precise manipulation and characterization of electron buffer effects is needed for rational material design.