ディケチミナートシリコン (((II) と,ニッケル (((0) の協調球で生成される関連するNHSiリガンド
Antje Meltzer1, Carsten Präsang, Matthias Driess
1Institute of Chemistry, Metalorganics and Inorganic Materials, Technische Universitat Berlin, Strasse des 17. Juni 135, Sekr. C2, D-10623 Berlin, Germany.
Journal of the American Chemical Society
|May 28, 2009
まとめ
研究者らは,新しいシリコン (((II) 水酸化物と,ニッケルに調整可能なNHSiリガンドを合成した. これらのリンガンドは,調節可能なドナー/受容体特性を発揮し,有機金属化学における新たな可能性を提供します.
科学分野:
- 有機金属化学 有機金属化学
- メイングループ 化学
背景:
- シリコンベースのリガンドは,協調化学において極めて重要です.
- リガンドの電子特性を調節することは,触媒設計の鍵です.
研究 の 目的:
- 新しいシリコン (((II) 水酸化物とNHSiリガンドを合成し,特徴づけること.
- ニッケル複合体内のこれらのリガンドの電子調節性を調査する.
主な方法:
- NHSi-トリカルボニルニッケル複合体の合成.
- 水やその他の反応剤を電子性添加.
- 顕微鏡特性 (NMR,IR) とX線結晶学.X線結晶学.
主要な成果:
- 最初のシリコン (((II)) 水酸化物と関連するNHSiリガンドの合成が成功しました.
- 置換に基づくリガンドの調整可能なドナー/受容体の能力を実証した.
- ルイス酸処理の結果,PF(3) 類似のリガンドが生み出され,水/酸添加により,ドナーで安定した複合体が生み出されました.
結論:
- 調節可能な電子特性を持つ新しいシリコン ((II) リガンドが開発されました.
- これらのリガンドは,特異な特性を持つ有機金属複合体の設計のための新しいプラットフォームを提供します.
- この発見は,協調化学におけるシリコンベースのリガンドの適用範囲を拡大する.
関連する概念動画
Structural Isomerism
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can be...
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can be...
Valence Bond Theory
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...
Coordination Compounds and Nomenclature
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...
Metal-Ligand Bonds
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...
Coordination Number and Geometry
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.
Crystal Field Theory - Tetrahedral and Square Planar Complexes
Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...

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