[Ru3(CN)3(CO)93-:用于多金属的构建块
Ping Wang1, Yu Zhang1, Toby Woods1
1School of Chemical Sciences, University of Illinois at Urbana-Champaign, Urbana, IL 61801, USA.
European journal of inorganic chemistry
|July 10, 2024
概括
一个新的集群连接体,Ru3 ((CN) 3 ((CO) 9) 3),作为合成新型金属化物子的多功能前体. 这些子包括镜,扩展镜,双和含有各种金属离子的超四面体.
科学领域:
- 无机化学 无机化学
- 协调化学 协调化学
- 超分子化学 超分子化学
背景情况:
- 金属化物集群是超分子化学中有价值的构建块.
- 从简单的前体合成复杂的结构仍然是一个关键的挑战.
研究的目的:
- 为了引入一个新的集群连接体,Ru3(CN) 3(CO) 93- ([1]3-),作为一个多功能前体.
- 使用 [1]3-. 探索各种μ-CN架构的合成.
- 描述由此产生的金属化物的结构多样性.
主要方法:
- 合成[Ru3(CN) 3(CO) 93- ([1]3-) 来自[Ru3(CO) 12和化物.
- [1]3-与各种金属离子 (Cu+,Ni2+,Fe2+,Fe2+) 反应形成结构.
- 使用适当的分析技术,对合成的子进行结构性表征.
主要成果:
- [1]3-被合成并被证明是μ-CN的前体.
- 形成一个镜 [Ru6(μ-CN) 3(CO) 183-在与[Ru3(CO) 12]反应后.
- 一个扩展镜{Cu3[Ru3(μ-CN) 3(CO) 9) 2}3-与Cu(I) 中心的合成.
- 形成具有八面体金属中心的双 {M[Ru3(μ-CN) 3(CO) 9}2}4- (M = Ni, Fe).
- 一个相互透的超四面体{Fe4(μ4-O) [Ru3(μ-CN) 3(CO) 9) 4}4-与FeII) 的合成.
结论:
- 集群连接体[Ru3(CN) 3 ((CO) 9) 3-是一种高效的构建块,用于构建各种金属化物超分子架构.
- 合成策略允许控制组装具有不同金属离子和几何形状的复杂子.
- 这项工作扩大了可访问的金属化物子库的库,在材料科学和催化学中具有潜在的应用.
相关概念视频
02:57Coordination Number and Geometry
15.7K
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.
15.7K
02:42Valence Bond Theory
8.5K
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...
8.5K
02:51Metal-Ligand Bonds
20.7K
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...
20.7K
02:37Metallic Solids
18.4K
Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
18.4K
03:02Colors and Magnetism
11.6K
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...
11.6K
02:54Coordination Compounds and Nomenclature
21.3K
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...
21.3K