对P2型氧化物阴极中离子电池离子电池氧化物氧化物的新见解
Zhi-Xiong Huang1,2, Kai Li3, Jun-Ming Cao1
1MOE Key Laboratory for UV Light-Emitting Materials and Technology, Northeast Normal University, Changchun, Jilin 130024, P.R. China.
Nano letters
|October 17, 2024
概括
这项研究通过结合和来设计用于离子电池 (SIB) 的新型阴极材料. 这种方法通过控制阳离子氧化还原反应来稳定结构并提高性能.
科学领域:
- 材料科学 材料科学 材料科学
- 电化学 电化学 电化学
- 固态化学 固态化学
背景情况:
- 分层过渡金属氧化物是离子电池 (SIB) 的有希望的阴极.
- 利用阴离子和阴离子的氧化还原反应可以增加阴极能量密度.
- 阳离子氧化还原反应往往导致不可逆转的氧气释放,限制了电池的性能.
研究的目的:
- 为SIBs设计一种稳定的阴极材料,以减轻 anionic redox 过程中不可逆转的氧气释放.
- 为了研究和共同替代在/基层氧化物中的作用.
- 阐明阳离子氧化还原反应的机制和Mg-O键的稳定作用.
主要方法:
- 合成一个Li-Mg共同替代的P2-Na0.67Li0.07Mg0.07Ni0.28Mn0.58O2材料.
- 密度函数理论 (DFT) 计算来分析电子结构和结合.
- 在现场电化学阻抗光谱 (EIS) 和静电电荷-放电 (GCD) 与dV/dQ分析.
主要成果:
- Ni3+/Ni4+氧化还原对和阳离子氧化还原反应表现出一种竞争关系.
- DFT计算显示Li的O2p非结合状态和Mg-O债券稳定了Ni-Oeg状态.
- 在现场EIS和dV/dQ测量显示了阳离子氧化还原机制和电阻变化.
结论:
- -Mg共同替代有效地稳定了SIBs的/基层氧化物.
- 该研究阐明了阴离子和阴离子氧化还原体之间的相互作用以及特定化学键的作用.
- 这项工作为下一代离子电池设计高能量密度,稳定的阴极提供了洞察力.
更多相关视频
10:03Characterization of Electrode Materials for Lithium Ion and Sodium Ion Batteries Using Synchrotron Radiation Techniques
Published on: November 11, 2013
25.4K
09:49A Protocol for Electrochemical Evaluations and State of Charge Diagnostics of a Symmetric Organic Redox Flow Battery
Published on: February 13, 2017
10.4K
相关概念视频
Electrolysis
26.1K
In a galvanic cell, the electrical work is done by a redox system on its surroundings as electrons produced by the spontaneous redox reactions are transferred through an external circuit. Alternatively, an external circuit does work on a redox system by imposing a voltage sufficient to drive an otherwise nonspontaneous reaction in a process known as electrolysis. For instance, recharging a battery involves the use of an external power source to drive the spontaneous (discharge) cell reaction in...
26.1K
Voltaic/Galvanic Cells
56.8K
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,...
56.8K
Standard Electrode Potentials
43.5K
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...
43.5K
Ladder Diagrams: Redox Equilibria
443
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+...
443
Oxidation-Reduction Reactions
64.4K
Oxidation–Reduction Reactions
64.4K
Electrodeposition
607
Electrodeposition is a technique used to separate an analyte from interferents by electrochemical processes. Here, the analyte is a metal ion that can be deposited on an electrode immersed in the sample solution. The electrochemical setup consists of an anode and a cathode. When an electric current is applied to the setup, oxidation occurs at the anode. At the cathode, which consists of a large metal surface, metal ions undergo reduction and deposit onto the surface.
Electrodeposition can...
Electrodeposition can...
607
