铁离子化中的Fe3d轨道演变:来自ΔSCF,EOES和轨道动量分布的洞察
Feng Wang1, Vladislay Vasilyev2
1School of Science, Computing and Emerging Technologies, Swinburne University of Technology, Melbourne, VIC 3122, Australia.
Molecules (Basel, Switzerland)
|September 13, 2025
概括
准确预测铁电离潜力需要先进的计算方法超出单粒子近似. 通过 ΔSCF 方法准确计算出铁.
科学领域:
- 计算化学的计算化学
- 量子化学 是一个量子化学.
- 物理化学 物理化学
背景情况:
- 铁素 (Fc) 电离是复杂的,因为它的多电子特征.
- 像库普曼定理和OVGF这样的标准方法对于准确的IP预测是不够的.
- 精确的铁电离电位 (IP) 计算对于理解其电子结构至关重要.
研究的目的:
- 使用先进的计算方法准确预测铁的第一个电离电位 (IP).
- 为了对各种计算模型进行基准测试,以确定它们在描述铁素电离化的准确性和效率.
- 为了研究电离后铁中电子结构的变化,专注于Fe 3d轨道的作用.
主要方法:
- 利用 ΔSCF 方法计算铁的第一个电离电位.
- 评估了42个计算模型,包括CCSD,CCSD(T) 和B3LYP方法与各种基础集.
- 纳入Fe特异性修改基础集,以改进对3d电子行为的描述.
- 进行了理论动量分布 (TMD) 和能量分解分析 (EDA).
主要成果:
- 该 ΔSCF 方法产生了 ~6.9 ± 0.1 eV 的第一个 IP,与实验值 (6.72-6.99 eV) 一致.
- B3LYP/m6-31G(d) 显示了精度和计算成本之间的最佳平衡.
- 确定了8a1'轨道,主要是Fe 3d字符,作为Fc+中单独占用的分子轨道 (SOMO).
- 分析揭示了Fe中心轨道的显著能量转移,以及电离后稳定的固态/保利条件.
结论:
- 该 ΔSCF 方法为铁电离潜力提供了准确的预测.
- 适当处理Fe 3d轨道对于精确的铁素电子结构计算至关重要.
- 8a1'轨道在铁电离中起着关键作用,发生了显著的电子结构重组.
相关概念视频
Electron Orbital Model
71.7K
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...
71.7K
Molecular Orbital Theory II
26.9K
Molecular Orbital Energy Diagrams
26.9K
Atomic Orbitals
43.2K
An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution function indicates the total probability of finding an electron within the thin shell at a distance r from the nucleus. The atomic orbitals have distinct shapes which are determined by l, the angular momentum quantum number. The orbitals are often drawn with a boundary surface, enclosing densest regions of the cloud.
43.2K
Molecular Orbital Theory I
46.9K
Overview of Molecular Orbital Theory
46.9K
The Energies of Atomic Orbitals
29.9K
In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are also observed. The attractive and repulsive forces are dependent on the distance between the particles, as well as the sign and magnitude of the charges on the individual particles. When the charges on the particles are opposite, they attract each other. If both particles have the same charge, they repel each other.
29.9K
Valence Bond Theory
11.2K
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...
11.2K


