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The material is formed by heating silicon and sulfur or by the exchange reaction between SiO 2 and Al 2 S 3.The material consists of chains of edge-shared tetrahedra, -Si(μ-S) 2 Si(μ-S) 2-.
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
3) are very useful synthetic intermediates in the production of more complicated silicon-containing compounds: the latter is a colourless crystalline ionic solid containing K + cations and SiH − 3 anions in the NaCl structure, and is made by the reduction of silane by potassium metal. [9] Additionally, the reactive hypervalent species SiH −
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Inosilicates (from Greek ἴς is [genitive: ἰνός inos] 'fibre'), or chain silicates, have interlocking chains of silicate tetrahedra with either SiO 3, 1:3 ratio, for single chains or Si 4 O 11, 4:11 ratio, for double chains. The Nickel–Strunz classification is 09.D – examples include:
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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.
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