尺寸和形状对Ni-Pt纳米合金中的化学排序的影响
Pamela Camilos1, Céline Varvenne1,2, Christine Mottet1
1Aix-Marseille University/CNRS, CINaM UMR 7325, Campus de Luminy, Marseille 13288, France. christine.mottet@univ-amu.fr.
Physical chemistry chemical physics : PCCP
|May 20, 2024
概括
数字模拟显示,- (Ni-Pt) 纳米合金表现出复杂的原子排序和表面分离. 由于原子应变效应,异形形状特别促进金表面分离.
科学领域:
- 材料科学 材料科学 材料科学
- 计算化学的计算化学
- 纳米技术纳米技术
背景情况:
- 了解纳米合金的原子结构和化学排序对于设计先进材料至关重要.
- -白金 (Ni-Pt) 合金由于其独特的特性而引起人们的兴趣,但它们在纳米尺度上的行为是复杂的.
研究的目的:
- 研究Ni-Pt纳米合金的原子结构和化学排序.
- 探索大小,形状和温度对合金行为的影响.
- 了解这些纳米粒子中的表面分离现象.
主要方法:
- 使用蒙特卡洛方法进行数值模拟.
- 对Ni-Pt相互作用应用一个现实的原子间潜力.
- 分析不同尺寸和形状的纳米粒子,包括二面体,八面体和截断的八面体结构.
主要成果:
- 在面中心立方 (fcc) 纳米粒子中,Ni-Pt纳米合金保留了批量订购趋势.
- 表面重建导致化学排序挫折,取决于集群大小和形状.
- 观察到 (Pt) 表面分离的反向温度依赖.
- 在icosahedral纳米粒子中,Ni因原子应变而分离到核心,而Pt则分离到表面.
- 与八面体和截断的八面体结构相比,二面体形状促进了Pt表面分离.
结论:
- Ni-Pt纳米合金的原子结构和化学排序受到大小,形状和温度的显著影响.
- 表面效应和原子应变在分离行为中起着至关重要的作用,特别是在非散装结构的结构中,例如icosahedra.
- 形状依赖的分离现象为定制纳米合金特性提供了途径.
相关概念视频
Metallic Solids
18.4K
Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
18.4K
Valence Bond Theory
8.5K
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...
8.5K
Coordination Number and Geometry
15.7K
For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
15.7K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
42.4K
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,...
42.4K
Ionic Crystal Structures
14.3K
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...
14.3K
Electron Configurations
16.6K
Electron configurations and orbital diagrams can be determined by applying the Aufbau principle (each added electron occupies the subshell of lowest energy available), Pauli exclusion principle (no two electrons can have the same set of four quantum numbers), and Hund’s rule of maximum multiplicity (whenever possible, electrons retain unpaired spins in degenerate orbitals).
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p,...
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p,...
16.6K


