过渡金属 (Co,Mn) 碳酸与 (III) 酸的双金属中性和离子复合物
Maxim A Faraonov1, Evgeniya I Yudanova1, Alexey V Kuzmin2
1Federal Research Center of Problems of Chemical Physics and Medicinal Chemistry RAS, Chernogolovka, Moscow Region, 142432, Russia. maksimfaraonov@yandex.ru.
Dalton transactions (Cambridge, England : 2003)
|August 15, 2023
概括
合成了含有 () (III) 的新型异金属复合物. 这些复合体表现出独特的电子和磁性特性,其中一个由于激进的氨酸和 (II) 离子而表现出对磁性.
科学领域:
- 无机化学 无机化学
- 材料科学 材料科学 材料科学
- 协调化学 协调化学
背景情况:
- () (Pc) 作为新型异金属复合物的基本成分.
- 过渡金属碳基被用作这些先进材料的合成中的前体.
研究的目的:
- 合成和表征新型的合金复合物,其中包括,,,,,和.
- 研究这些复杂物体的电子和磁性特性,这些复杂物体是单个和双重还原过程中产生的.
主要方法:
- 不同金属复合物的结晶 {[Co(CO) 4) -[InIII(Pc2-) ]} (1) 和 (Cp*2Cr+) {[Mn(CO) 5) -[InIII(Pc•3-) ]}·2C6H4Cl2 (2).
- 通过单次和双次还原合成的化在过渡金属碳基的存在下.
- 使用光学光谱,晶体结构分析和磁性测量进行表征.
主要成果:
- 综合体1的特点是二离子酸 (Pc2-) 和二磁性[Co(CO) 4]-离子.
- 复合体2含有异金属{[Mn(CO) 5}-[InIII(Pc•3-) ]-离子和偏磁Cp*2Cr+对抗,表示双重减少.
- 复合体2在Pc Q波段呈现蓝色转移,在1005nm处呈现新的NIR波段,这是Pc•3-的特征,磁矩为4.24μB.
结论:
- 合成复合物的电子配置和磁性特性通过光谱和磁性数据得到证实.
- 综合体1是二磁性,而综合体2是二磁性,由结合的S=1/2 (Pc•3-) 和S=3/2 (Cp*2Cr+) 旋转产生的.
- 该研究表明,成功合成了基于(III) 甲的异金属复合物,具有可调节的电子和磁性特征.
相关概念视频
Metal-Ligand Bonds
21.0K
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...
21.0K
Colors and Magnetism
11.9K
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...
11.9K
Valence Bond Theory
8.7K
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...
8.7K
Formation of Complex Ions
23.7K
A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
23.7K
Complexation Equilibria: Factors Influencing Stability of Complexes
402
In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
402
Complexometric Titration: Overview
7.3K
Complexometric titration involves the formation of a complex by reacting a metal ion with one or more ligands. A visual indicator often detects the end point of a complexometric titration. It is added to the metal solution before the titration, forming a stable metal–indicator complex and imparting color to the solution. As the titration approaches the equivalence point, the excess of the added ligand displaces the indicator from the metal–indicator complex, releasing the free...
7.3K


