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Si + 3 HCl → HSiCl 3 + H 2. The trichlorosilane is then converted to a mixture of silane and silicon tetrachloride: 4 HSiCl 3 → SiH 4 + 3 SiCl 4. This redistribution reaction requires a catalyst. The most commonly used catalysts for this process are metal halides, particularly aluminium chloride. This is referred to as a redistribution ...
[1] [2] It is also known as the Pimentel–Rundle three-center model after the work published by George C. Pimentel in 1951, [3] which built on concepts developed earlier by Robert E. Rundle for electron-deficient bonding. [4] [5] An extended version of this model is used to describe the whole class of hypervalent molecules such as phosphorus ...
The dominant examples come from the Direct process, i.e., (CH 3) 4-x SiCl x. Another important member is trichlorosilane (SiHCl 3). Organosilanes are a class of charge-neutral organosilicon compounds. Example: tetramethylsilane (Si(CH 3) 4) By tradition, compounds with Si-O-Si bonds are usually not referred to as silanes. Instead, they are ...
Lone pairs Electron domains (Steric number) Shape Ideal bond angle (example's bond angle) Example Image 2 0 2 linear: 180° CO 2: 3 0 3 trigonal planar: 120° BF 3: 2 1 3 bent: 120° (119°) SO 2: 4 0 4 tetrahedral: 109.5° CH 4: 3 1 4 trigonal pyramidal: 109.5° (106.8°) [10] NH 3: 2 2 4 bent: 109.5° (104.48°) [11] [12] H 2 O: 5 0 5 ...
In chemistry, a trigonal bipyramid formation is a molecular geometry with one atom at the center and 5 more atoms at the corners of a triangular bipyramid. [1] This is one geometry for which the bond angles surrounding the central atom are not identical (see also pentagonal bipyramid), because there is no geometrical arrangement with five terminal atoms in equivalent positions.
Valence shell electron pair repulsion (VSEPR) theory (/ ˈ v ɛ s p ər, v ə ˈ s ɛ p ər / VESP-ər, [1]: 410 və-SEP-ər [2]) is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. [3]
This would result in the geometry of a regular tetrahedron with each bond angle equal to arccos(− 1 / 3 ) ≈ 109.5°. However, the three hydrogen atoms are repelled by the electron lone pair in a way that the geometry is distorted to a trigonal pyramid (regular 3-sided pyramid) with bond angles of 107°.
Gilbert N. Lewis introduced the concepts of both the electron pair and the covalent bond in a landmark paper he published in 1916. [1] [2] MO diagrams depicting covalent (left) and polar covalent (right) bonding in a diatomic molecule. In both cases a bond is created by the formation of an electron pair.