通过离子双极相互作用实现的破裂溶解主导效应,使离子电池中的长寿命氧化阳极成为离子电池中的氧化阳极
Shengwei Dong1, Lingfeng Shi1, Shenglu Geng1
1State Key Laboratory of Space Power-Sources, School of Chemistry and Chemical Engineering, Harbin Institute of Technology, Harbin, 150001, People's Republic of China.
Nano-micro letters
|December 26, 2024
概括
一种新的基于succinonitrile的电解质通过减少体积膨胀来改善氧化阳极的稳定性. 这提高了先进的储能应用的电池循环寿命.
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
- 计算化学计算化学
背景情况:
- 微米大小的氧化 (SiO) 阳极面临着显著的体积扩张问题,阻碍了它们在大型电池应用中的使用.
- 需要有效的策略来提高SiO阳极的循环稳定性和寿命.
研究的目的:
- 为提高氧化阳极性能,引入一种基于苏奇尼尼特 (SN) 的新型深电解质.
- 研究新的电解质中的离子溶解相互作用和固体电解质相间形成机制.
主要方法:
- 密度函数理论 (DFT) 的计算用于研究Li+和SN之间的离子双极相互作用.
- 分子动力学 (MD) 模拟来分析离子溶解结构和相互作用.
- 在基于SN的电解质中制造和电化学测试SiO阳极.
- 微型计算机断层扫描 (Micro-CT) 来评估SiO体积膨胀.
主要成果:
- DFT证实了Li+和SN之间强烈的离子双极相互作用.
- MD模拟显示,乙烯碳酸盐 (FEC) 优化了Li+溶解,导致由FEC和TFSI-.丰富的复合固体电解质介相 (SEI).
- 产生的电解质有效地抑制了SiO体积膨胀.
- 二氧化 (SiO) 和二氧化 (LiCoO2) 完整电池表现出优异的电化学性能和延长的循环稳定性.
结论:
- 一种基于succinonitrile的深度环氧电解质提供了一种有效的策略,以提高氧化阳极的循环稳定性.
- 优化的Li+溶解结构和复合SEI形成是减轻体积膨胀的关键.
- 这项研究为使用氧化阳极的下一代电池提高性能铺平了道路.
相关概念视频
03:45Formation of Complex Ions
23.0K
A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
23.0K
02:55Solubility of Ionic Compounds
61.9K
Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.
61.9K
03:24Common Ion Effect
40.7K
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:
40.7K
02:12Solvating Effects
7.2K
An understanding of the solvating effect helps rationalize the relation between solvation and acidity of the compound. In addition, this also explains the relative stability of conjugate bases for compounds with different pKa values. This lesson details, in-depth, the principle of solvating effects. The strength of an acid and the stability of its corresponding conjugate base are determined using pKa values. This observed relationship is a consequence of solvation, which is the interaction...
7.2K
03:13Intermolecular Forces
55.4K
Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen...
55.4K
01:19Ionic Strength: Effects on Chemical Equilibria
1.2K
The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary...
In this solution, the primary...
1.2K