硬软界面上的协调化学:基于氧化的稀土/过渡金属复合体
Rwitabrita Panda1, Franziska Flecken1, Christina Papke1
1Institute for Inorganic Chemistry, Karlsruhe Institute of Technology, Engesserstr. 15, Karlsruhe 76131, Germany.
ACS omega
|March 16, 2026
概括
这项研究使用四二胺氧化物 (PPO) 合成了稀土 (RE) 金属复合物. 研究人员开发了一种创新的方法来创建RE/Mo异金属复合物,证明了溶剂控制的结构多样性.
科学领域:
- 无机化学 无机化学
- 协调化学 协调化学
- 材料科学 材料科学 材料科学
背景情况:
- 甲二单氧化物 (PPO) 作为协调化学中的多功能连接体.
- 稀土 (RE) 和过渡金属 (TM) 复合物在各种催化和材料应用中至关重要.
- 合成具有不同金属中心的异金属复合物存在重大挑战.
研究的目的:
- 为了合成和表征新的单金属RE-PPO复合物.
- 为了探索RE/TM异金属组件的构造.
- 研究溶剂环境对这些复合物的结构多样性的影响.
主要方法:
- 合成和表征与PPO的Al (III),Sm (III),Dy (III),Er (III) 和Yb (III) 复合体.
- 在RE-PPO合成器中直接纳入软TM (Cu(I,Au(I)) 的探索.
- 使用预合成的Mo-PPO合成子用于RE/Mo异金属复合体形成的替代路线的开发.
- 在不同的溶剂环境 (二甲,THF,MeCN) 中合成的复合物的结构分析.
主要成果:
- 直接将Cu ((I) 和Au ((I) 纳入RE-PPO合成器具有挑战性,产生了不必要的基于TM的物种.
- 通过使用预合成的Mo-PPO合成器成功建立了RE/Mo异金属复合物的途径.
- 溶剂选择显著影响了分子结构;非协调溶剂 (如二甲) 导致桥RE2复合体,而协调溶剂 (THF,MeCN) 没有.
- 这种依赖于溶剂的结构分歧提供了一种控制金属核性的方法.
结论:
- 该研究强调了这些挑战,并为合成RE/Mo异金属复合物提供了一个成功的策略.
- 溶剂控制组装提供了一个简单的方法来调节金属复合物的核和结构.
- 这些发现有助于合理设计具有可调节性质的复杂无机材料.
更多相关视频
10:52Line Shape Analysis of Dynamic NMR Spectra for Characterizing Coordination Sphere Rearrangements at a Chiral Rhenium Polyhydride Complex
Published on: July 27, 2022
3.4K
10:51The Synthesis, Characterization and Reactivity of a Series of Ruthenium N-triphosPh Complexes
Published on: April 10, 2015
12.8K
相关概念视频
Metal-Ligand Bonds
25.3K
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
25.3K
Coordination Number and Geometry
19.5K
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.
19.5K
Valence Bond Theory
11.5K
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...
11.5K
Coordination Compounds and Nomenclature
27.8K
In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...
27.8K
Colors and Magnetism
14.5K
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...
14.5K
Complexation Equilibria: The Chelate Effect
1.5K
In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
1.5K
