Related Experiment Video
Updated: Dec 29, 2025
10:03
Characterization of Electrode Materials for Lithium Ion and Sodium Ion Batteries Using Synchrotron Radiation Techniques
Published on: November 11, 2013
25.9K
Reversible Anionic Redox Activities in Conventional LiNi1/3 Co1/3 Mn1/3 O2 Cathodes
Gi-Hyeok Lee1, Jinpeng Wu2,3, Duho Kim4
1Department of Energy and Materials Engineering, Dongguk University-Seoul, Seoul, 04620, Republic of Korea.
Angewandte Chemie (International Ed. in English)
|February 8, 2020
Summary
Reversible oxygen redox reactions were discovered in conventional lithium-ion battery electrodes, challenging the focus on cation reactions. This finding opens new avenues for developing high-capacity lithium-ion batteries.
Area of Science:
- Materials Science
- Electrochemistry
- Inorganic Chemistry
Background:
- Oxygen redox reactions are crucial for lithium-excess layered oxide electrodes.
- Conventional electrodes primarily rely on cationic redox reactions.
- Anionic redox is often overlooked in practical electrode materials.
Purpose of the Study:
- To provide evidence for reversible anionic redox reactions in LiNi 1/3 Co 1/3 Mn 1/3 O 2.
- To elucidate the role of oxygen redox in conventional layered electrodes.
- To explore the potential of anionic redox for high-capacity batteries.
Main Methods:
- Electrochemical analysis of LiNi 1/3 Co 1/3 Mn 1/3 O 2.
- Investigation of redox mechanisms at high potentials.
- Cycling stability tests over multiple cycles.
Main Results:
- Unambiguous evidence of reversible anionic redox reactions was observed.
- Oxygen redox was 75% reversible during the initial cycle and 63% retained after 10 cycles.
- Both cationic and anionic reactions contribute to high-potential mechanisms.
Conclusions:
- Anionic redox reactions are significant in conventional layered electrodes.
- Reversible oxygen redox offers potential for high-capacity lithium-ion batteries.
- This work clarifies reaction mechanisms and highlights a new design strategy.
Keywords:
X-ray absorption spectroscopyelectrochemistrylithium-ion batteriesredox chemistryresonant inelastic X-ray scatteringMore Related Videos
05:47Preparation of Polyoxometalate-based Photo-responsive Membranes for the Photo-activation of Manganese Oxide Catalysts
Published on: August 7, 2018
8.0K
07:55Elemental-sensitive Detection of the Chemistry in Batteries through Soft X-ray Absorption Spectroscopy and Resonant Inelastic X-ray Scattering
Published on: April 17, 2018
13.1K
Related Concept Videos
01:30Ladder Diagrams: Redox Equilibria
705
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+...
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+...
705
01:24Redox Reactions
58.0K
Oxidation-reduction or redox reactions involve the transfer of electrons from one molecule or atom to another. When an atom gains an electron, another atom must lose an electron, meaning oxidation and reduction must occur together. Since the redox occurs in pairs, the atom that gets oxidized is also called the reducing agent or reductant, and the atom that is reduced is also called the oxidizing agent or oxidant. A straightforward way to remember the definitions of oxidation and reduction is...
58.0K
01:27Redox Reactions
773
Redox reactions are vital biochemical processes that underpin energy metabolism in cells. These reactions involve the transfer of electrons between molecules, occurring in tandem as oxidation and reduction. Oxidation refers to the loss of electrons, while reduction denotes their gain. This coupling ensures the seamless flow of electrons through metabolic pathways. For example, in bacterial metabolism, glucose undergoes oxidation to carbon dioxide, while oxygen is simultaneously reduced to...
773
02:47Voltaic/Galvanic Cells
62.7K
Spontaneous Chemical Reactions
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
62.7K
01:23Redox Equilibria: Overview
1.5K
A reduction-oxidation reaction is commonly called a redox reaction. In a redox reaction, electrons are transferred from one species to another rather than being shared between or among atoms. The reducing agent or reductant is the species that loses electrons and gets oxidized in the process. The species that gains electrons and gets reduced in the process is the oxidizing agent or oxidant. Redox reactions are represented as two separate equations called half-reactions, where one equation...
1.5K
01:26Redox Titration: Other Oxidizing and Reducing Agents
1.3K
Besides iodine, other oxidizing or reducing agents can serve as titrants in redox titrations. Common oxidizing titrants include KMnO4, cerium(IV), and K2Cr2O7. The choice of oxidizing titrants depends on factors like stability, cost, analyte strength, and reaction rate between the analyte and titrant. KMnO4 is a strong oxidizing titrant that reduces from Mn(VII) to Mn(II) in a highly acidic solution, simultaneously oxidizing the analyte to a higher oxidation state. In this case, KMnO4 acts as a...
1.3K