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[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.
Vanadium tetrafluoride has a similar structure to tin's [61] and disproportionates at 100–120 °C to the trifluoride and the pentafluoride. The tetrafluorides of iridium, platinum, palladium, and rhodium all share the same structure which was not known until 1975.
Because of its polymeric structure, PtCl 4 dissolves only upon breaking the chloride bridging ligands. Thus, addition of HCl give H 2 PtCl 6. Lewis base adducts of Pt(IV) of the type cis-PtCl 4 L 2 are known, but most are prepared by oxidation of the Pt(II) derivatives. [2]
Examples of Lewis dot diagrams used to represent electrons in the chemical bonds between atoms, here showing carbon (C), hydrogen (H), and oxygen (O). Lewis diagrams were developed in 1916 by Gilbert N. Lewis to describe chemical bonding and are still widely used today. Each line segment or pair of dots represents a pair of electrons.
Platinum is a chemical element; it has symbol Pt and atomic number 78. It is a dense, malleable, ductile, highly unreactive, precious, silverish-white transition metal. Its name originates from Spanish platina, a diminutive of plata "silver". [7] [8] Platinum is a member of the platinum group of elements and group 10 of the periodic table of ...
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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