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Coordination Number and Geometry02:57

Coordination Number and Geometry

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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.
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Coordination Compounds and Nomenclature02:54

Coordination Compounds and Nomenclature

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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...
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Metallic Solids02:37

Metallic Solids

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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....
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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...
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The structure of a crystalline solid, whether a metal or not, is best described by considering its simplest repeating unit, which is referred to as its unit cell. The unit cell consists of lattice points that represent the locations of atoms or ions. The entire structure then consists of this unit cell repeating in three dimensions. The three different types of unit cells present in the cubic lattice are illustrated in Figure 1.
Types of Unit Cells
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Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”. 
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Dae-Hyun Nam1, Oleksandr S Bushuyev1, Jun Li1,2

  • 1Department of Electrical and Computer Engineering , University of Toronto , 10 King's College Road , Toronto , Ontario M5S 3G4 , Canada.

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概括

研究人员开发了一种使用金属有机框架 (MOF) 创建铜 (Cu) 集群的新方法. 这种策略增强了电化学二氧化碳减排反应 (CO2RR),用于生产有价值的多碳产品,如乙烯.

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科学领域:

  • 材料科学
  • 电化学
  • 催化剂

背景情况:

  • 电化学二氧化碳还原反应 (CO2RR) 对于将二氧化碳转化为有价值的化学物质至关重要.
  • 铜 (Cu) 集群是CO2RR的有希望的催化剂,但控制它们的选择性,特别是对于多碳产品,仍然具有挑战性.
  • Cu活性位点的表面协调数 (CN) 显著影响CO2RR结果.

研究的目的:

  • 通过金属有机框架 (MOF) 制定规范Cu集群形成的策略,以提高CO2RR向多碳产品.
  • 通过控制聚物的前体结构来促进缺乏协调的位.
  • 在Cu集群CN和CO2RR选择性之间建立结构-活动关系.

主要方法:

  • 使用HKUST-1,一个金属有机框架 (MOF),作为Cu集群形成的模板.
  • 用热处理的HKUST-1将对称的立方体扭曲成不对称的图案,从而产生低协调的位点.
  • 使用电子磁共振 (EPR) 和现场X射线吸收光谱 (XAS) 来描述Cu星团及其电子状态.
  • 研究了不同材料加工条件对立体结构和CO2RR性能的影响.

主要成果:

  • 从HKUST-1中的扭曲Cu二元中成功促进了低协调数 (CN) 的Cu集群的形成.
  • 使用这些MOF衍生的Cu聚合催化剂,实现了C2H4 (乙烯) 生产的创纪录的45%法拉达效率 (FE).
  • 证明调节 Cu-Cu CN 在 Cu 集群是控制 CO2RR 选择性的关键.

结论:

  • MOF规范的合成策略有效地控制了Cu集群的形成,并促进了缺乏协调的活跃地点.
  • 这种方法提供了一种选择性地从二氧化碳电解产生多碳产品的途径.
  • 已建立的结构-活动关系为设计CO2RR的先进Cu催化剂提供了洞察力.