制备,光谱表征和高价值非氧化 (Co) (IV) 和正式Co (V) 复合物的反应性
Jindou Yang1, Virginia A Larson2, Daniel G Castella2
1Department of Chemistry and Nano Science, Ewha Womans University, Seoul 03760, Korea.
JACS Au
|August 1, 2025
概括
这项研究合成了新的高价值复合物,Co(IV),使用独特的电子捐赠配体,PCAPD. 这些复合物缺乏轴性氧基,在氧化反应中表现出明显的反应性.
科学领域:
- 无机化学 无机化学 有机化学
- 有机金属化学 有机金属化学
- 频谱学是一种光谱学.
背景情况:
- 高价值的-oxo和-imido复合物通常使用人工氧化剂形成.
- 在没有轴性或imido配体的情况下获得高价值的物种是一个合成的挑战.
研究的目的:
- 为了合成和表征没有轴性或imido群的新型高价值中间体.
- 为了研究这些独特的物种的电子结构和反应性.
主要方法:
- 使用强烈的电子捐赠配体PCAPD (bis-[2-] 1H-pyrrol-2-carboxamido) -o-phenylenediamine) 合成复合物.
- 一个Co(III) 前体的氧化与人工氧化剂,如基 (PhIO) 和N-tosiliminophenyliodinane (PhINTs).
- 使用光谱技术进行表征,包括EPR,CSI-MS,MCD,XAS和EXAFS,以及理论计算.
主要成果:
- 正式成功合成了Co(V) 和Co(IV) 的中间体,以及CoIV (PCAPD•+) -OH) 2 -和CoIV (PCAPD) -OH) 2 - - .
- 光谱和EXAFS数据揭示了一个六坐标的Co ((IV) 中心,带有轴性氧化连接体和一个电子氧化连接体,显著缺乏氧基.
- 与其他复合物相比,这些高价值物种在原子和氧原子转移反应中表现出明显较低的反应性.
结论:
- 这项工作报告了首次合成高价值复合物 (正式名为Co(V和Co(IV)) 没有轴性或imido配体.
- 描述的物种[CoIV ((PCAPD•+) - ((OH) 2) - 和[CoIV ((PCAPD) - ((OH) 2) 2 - 具有独特的电子结构和降低的反应性.
- 这些发现扩大了对氧化状态及其相关联联体环境的理解.
更多相关视频
10:51The Synthesis, Characterization and Reactivity of a Series of Ruthenium N-triphosPh Complexes
Published on: April 10, 2015
12.3K
08:40Synthesis of Metal Nanoparticles Supported on Carbon Nanotube with Doped Co and N Atoms and its Catalytic Applications in Hydrogen Production
Published on: December 6, 2021
3.7K
相关概念视频
Valence Bond Theory
9.7K
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...
9.7K
Colors and Magnetism
12.3K
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...
12.3K
Coordination Compounds and Nomenclature
22.2K
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...
22.2K
Properties of Transition Metals
27.2K
Transition metals are defined as those elements that have partially filled d orbitals. As shown in Figure 1, the d-block elements in groups 3–12 are transition elements. The f-block elements, also called inner transition metals (the lanthanides and actinides), also meet this criterion because the d orbital is partially occupied before the f orbitals.
27.2K
Properties of Organometallic Compounds
1.1K
Organometallic compounds are compounds that contain a carbon–metal bond. Carbon belongs to an organyl group like alkyl, aryl, allyl, or benzyl groups. The metal can be from Group I or Group II of the periodic table, a transition metal, or a semimetal.
1.1K
Coordination Number and Geometry
16.7K
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.
16.7K
