通过D-P轨道合,用于持久的离子存储的平面封闭原子极
Shuai Li1, Ximeng Lv2, Keyan Hu1
1School of Mechanical and Electrical Engineering, Jingdezhen Ceramic University, Jingdezhen 333403, China.
ACS applied materials & interfaces
|December 30, 2025
概括
研究人员通过合d-p轨道开发了一种用于离子电池 (SIB) 的新型NbSnS2阳极材料. 这一策略增强了稳定性和离子扩散,克服了SIB阳极设计中的容量衰减权衡.
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
- 储能 储能 储能 储能 储能 储能
背景情况:
- 离子电池 (SIB) 面临着阳极材料的挑战,由于Na+容纳导致的结构退化,它们在高特异性容量和循环稳定性之间存在权衡.
- 现有的阳极材料在化/脱周期中经常遭受不可逆转的结构变化.
研究的目的:
- 为SIB设计一种新的阳极材料,克服容量稳定性权衡.
- 研究d-p轨道合对阳极材料电化学性能和结构完整性的影响.
主要方法:
- 采用d-p轨道合策略,将原子锡 (Sn) 化学限制在二硫化物 (NbS2) 主体内,创建一个NbSnS2架构.
- 进行了in-situ和ex-situ分析,以确认结构恢复并阐明间隙机制.
主要成果:
- NbSnS2阳极在0.44°C时表现出490mAhg-1的特定容量,初始库伦比克效率为93.1%.
- 观察到出色的高速率性能,在11°C的850个循环中保持340mAh的g-1,几乎100%的容量保留.
- 在Nb 4dz2和Sn 5p状态之间的轨道合增强了电子密度,抑制了Sn迁移并保持了晶格完整性.
结论:
- d-p轨道合策略有效地限制了原子Sn,增强了结构稳定性并促进了SIBs在NbSnS2阳极中的离子扩散.
- 这项工作引入了一个准拓间隔机制,并建立了轨道合作为设计高容量,耐用SIB阳极材料的范例.
相关概念视频
Crystal Field Theory - Tetrahedral and Square Planar Complexes
47.9K
Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
47.9K
Electron Orbital Model
71.5K
Orbitals are the areas outside of the atomic nucleus where electrons are most likely to reside. They are characterized by different energy levels, shapes, and three-dimensional orientations. The location of electrons is described most generally by a shell or principal energy level, then by a subshell within each shell, and finally, by individual orbitals found within the subshells.
The first shell is closest to the nucleus, and it has only one subshell with a single spherical orbital called the...
The first shell is closest to the nucleus, and it has only one subshell with a single spherical orbital called the...
71.5K
Ionic Bonds
127.3K
Overview
When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.
Opposing Charges Hold Ions Together in Ionic Compounds
Ionic bonds are reversible electrostatic interactions between ions...
When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.
Opposing Charges Hold Ions Together in Ionic Compounds
Ionic bonds are reversible electrostatic interactions between ions...
127.3K
Ionic Crystal Structures
16.7K
Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
16.7K
Valence Bond Theory
11.1K
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
11.1K


