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In coordination chemistry, a coordinate covalent bond, [1] also known as a dative bond, [2] dipolar bond, [1] or coordinate bond [3] is a kind of two-center, two-electron covalent bond in which the two electrons derive from the same atom. The bonding of metal ions to ligands involves this kind of interaction. [4]
A linear tetradentate ligand has the four donor atoms in a line and each subsequent donor is connected by one of three bridges. Such a ligand bound to a metal in tetrahedral coordination can only connect in one way, though if the ligand is unsymmetrical then there are two chiral arrangements.
However, these ligands also form dative covalent bonds like the L-type. [2] This type of ligand is not usually used because in certain situations it can be written in terms of L and X. For example, if a Z ligand is accompanied by an L type, it can be written as X 2. Examples of these ligands are Lewis acids, such as BR 3. [3]
Despite the low reactivity of the tetrafluoroborate anion in general, BF − 4 serves as a fluorine source to deliver an equivalent of fluoride. [2] The Balz–Schiemann reaction for the synthesis of aryl fluorides is the best known example of such a reaction. [3]
For example, calculations suggest that Fe 2 (CO) 9 lacks an iron–iron bond by virtue of a 3-center 2-electron bond involving one of three bridging CO ligands. [ 5 ] Representations of two kinds of μ-bridging ligand interactions, 3-center, 4-electron bond (left) and 3-center, 2-electron bonding.
3, X = F, Br, Cl, I) via a molecular orbital (MO) description, building on the concept of the "half-bond" introduced by Rundle in 1947. [4] [5] In this model, two of the four electrons occupy an all in-phase bonding MO, while the other two occupy a non-bonding MO, leading to an overall bond order of 0.5 between adjacent atoms (see Molecular ...
Oxidation of R 3 P–M complexes results in longer M–P bonds and shorter P–C bonds, consistent with π-backbonding. [11] In early work, phosphine ligands were thought to utilize 3d orbitals to form M–P pi-bonding, but it is now accepted that d-orbitals on phosphorus are not involved in bonding as they are too high in energy. [12] [13]
Formal charges in ozone and the nitrate anion. In chemistry, a formal charge (F.C. or q*), in the covalent view of chemical bonding, is the hypothetical charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms, regardless of relative electronegativity.