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Related Concept Videos

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...
Catalysis02:50

Catalysis

The presence of a catalyst affects the rate of a chemical reaction. A catalyst is a substance that can increase the reaction rate without being consumed during the process. A basic comprehension of a catalysts’ role during chemical reactions can be understood from the concept of reaction mechanisms and energy diagrams.
Catalysis01:27

Catalysis

Catalysis influences the rate of chemical reactions by providing an alternative reaction pathway with lower activation energy. A catalyst speeds up a reaction, but it is not consumed during the process. The fundamental principle of catalysis is the ability of a catalyst to alter the reaction mechanism, often introducing a more efficient pathway than the uncatalyzed process.In a catalyzed reaction, the catalyst participates directly in the reaction mechanism. It interacts with reactants to form...
Heterogeneous Catalysis01:22

Heterogeneous Catalysis

Heterogeneous catalysis involves a catalyst in a different phase from the reactants. It is a process where the catalyst and the reactants are in distinct phases, typically solid and gas or liquid.Most heterogeneous catalysts are metals, metal oxides, or acids. The list includes transition metals like iron (Fe), cobalt (Co), nickel (Ni), palladium (Pd), platinum (Pt), chromium (Cr), manganese (Mn), tungsten (W), silver (Ag), and copper (Cu). These metals possess partially vacant d orbitals that...
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...
Ladder Diagrams: Redox Equilibria01:30

Ladder Diagrams: Redox Equilibria

Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...

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Precise Electrochemical Sizing of Individual Electro-Inactive Particles
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Published on: August 4, 2023

Deciphering competing elementary steps to correlate electrocatalyst chemical state with activity.

Yuanfu Ren1,2, Xingzhu Chen1,2, Shouwei Zuo1,2

  • 1Center for Renewable Energy and Storage Technologies (CREST), Physical Science and Engineering Division, King Abdullah University of Science and Technology (KAUST), Thuwal 23955-6900, Kingdom of Saudi Arabia.

Science Advances
|May 27, 2026
PubMed
Summary
This summary is machine-generated.

Researchers developed a new electrochemical method to untangle complex steps in electrocatalysis. This technique reveals the crucial role of lattice oxygen in the oxygen evolution reaction, improving catalyst design.

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Area of Science:

  • Heterogeneous electrocatalysis
  • Surface chemistry
  • Electrochemical reaction mechanisms

Background:

  • Overpotential in multielectron transfer electrocatalysis stems from complex thermodynamic and kinetic factors in elementary steps.
  • Deciphering coupled and competing elementary steps in electrocatalysis remains a significant challenge.

Purpose of the Study:

  • To establish an electrochemical deconvolution paradigm for resolving competing elementary steps in electrocatalytic reactions.
  • To investigate the electrochemical behavior of lattice oxygen in the oxygen evolution reaction (OER) using a model catalyst.

Main Methods:

  • Developed an electrochemical deconvolution paradigm based on charge accumulation, electron/proton transfer, and intermediate evolution.
  • Designed a model catalyst with isolated cation-anion vacancy pairs.
  • Utilized alternating current techniques to analyze reaction kinetics and thermodynamics.

Main Results:

  • Successfully resolved competing elementary steps in the oxygen evolution reaction.
  • Tracked the electrochemical behavior of lattice oxygen, disentangling it from adsorbed oxygen intermediates.
  • Identified lattice oxygen oxidation pathway originating from spontaneous deprotonation of water molecules.
  • Demonstrated that lattice oxygen oxidation, despite higher potential, exhibits faster kinetics than metal oxidation.
  • Established a direct correlation between the initial chemical state and catalytic activity.

Conclusions:

  • The study proves surface-confined lattice oxygen cycling and its superior catalytic activity.
  • The developed multidimensional framework enables disentanglement of thermodynamic and kinetic contributions.
  • This approach guides the rational optimization of complex multielectron transfer reactions.