在[Co6 Se8 (PEt3) 超原子中,电子和旋转转移
Yunyao Xu1, Jia Chen1, Alexander P Aydt1
1Department of Chemistry, Columbia University New York, New York, 10027, USA.
概括
这项研究研究了Co6Se8(PEt3) 6分子团,揭示了其电子结构和磁性. 这些发现突出了其设计新型超原子固体和单电子器件的潜力.
科学领域:
- 固态化学和材料科学 固态化学和材料科学
- 纳米科学和分子工程.
背景情况:
- 分子团可以作为"超原子"固体的构建块.
- 了解超原子的特性是设计新材料的关键.
研究的目的:
- 为了彻底研究Co6Se8(PEt3) 6超原子的结构,电子和磁性特性.
- 探索这个超原子在创造新型固态材料和设备方面的潜力.
主要方法:
- 固态核磁共振 (SSNMR) 光谱学 (59Co,31P,13C). 固态核磁共振 (SSNMR) 光谱学 (59Co,31P,13C). 固态核磁共振 (SSNMR) 光谱学 (59Co,31P,13C). 固态核磁共振 (SSNMR) 光谱学 (59Co,31P,13C). 固态核磁共振 (SSNMR) 光谱学 (59Co,31P,13C). 固态核磁共振 (SSNMR) 光谱学 (59Co,31P,13C). 固态核磁共振 (SSNMR) 光谱学 (59Co,31P,13C). 固态核磁共振 (SSNMR) 光谱学
- 量子化学计算 量子化学计算
- 连接物替代实验. 连接物替代实验.
主要成果:
- Co6Se8(PEt3) 6星团在其无机核心和绝缘联体外上呈现出非局部化的价值电子.
- 中性星团是二磁性和对称的,由非定位的HOMO轨道表示的芳香特征.
- 氧化到 +1 电荷状态会产生脱位的未配对电子,导致偏磁性和脱位旋转.
结论:
- 超原子 Co6Se8(PEt3) 6 由于电子移位而具有独特的电子和磁性.
- 它的核心结构在连接物修饰下保持稳定.
- 氧化集群中的外定位电子旋转显示出对单电子设备应用的前景.
相关概念视频
Valence Bond Theory
8.6K
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...
8.6K
Electron Configurations
16.7K
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,...
16.7K
Electron Configuration of Multielectron Atoms
41.7K
The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the 3s orbital, giving a 1s22s22p63s1 configuration. The electrons occupying the outermost shell orbital(s) (highest value of n) are called valence electrons, and those occupying the inner shell orbitals are called core electrons. Since the core electron shells correspond to noble gas electron configurations, we can abbreviate electron...
41.7K
Colors and Magnetism
11.7K
Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
11.7K
The Pauli Exclusion Principle
37.8K
The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that contains three pieces of information:
37.8K
The Aufbau Principle and Hund's Rule
49.2K
To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and continuing across the periods of the periodic table, we add one proton at a time to the nucleus and one electron to the proper subshell until we have described the electron configurations of all the elements. This procedure is called the aufbau principle, from the German word aufbau (“to build up”). Each added electron occupies the...
49.2K


