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In that case one or more binding sites of the ligand are unused. Such sites can be used to form a bond with another chemical species. Bidentate (also called didentate) ligands bind with two atoms, an example being ethylenediamine. Structure of the pharmaceutical Oxaliplatin, which features two different bidentate ligands.
A classic bidentate ligand is ethylenediamine, which is derived by the linking of two ammonia groups with an ethylene (−CH 2 CH 2 −) linker. A classic example of a polydentate ligand is the hexadentate chelating agent EDTA, which is able to bond through six sites, completely
The two phosphorus atoms (orange) of dppe have a bite angle of 85.8° on the palladium atom (blue) in [PdCl 2 (dppe)].. In coordination chemistry, the bite angle is the angle on a central atom between two bonds to a bidentate ligand.
It is commonly encountered as a bidentate ligand. When the oxalate chelates to a single metal center, it always adopts the planar conformation. As a bidentate ligand, it forms a 5-membered MC 2 O 2 ring. An illustrative complex is potassium ferrioxalate, K 3 [Fe(C 2 O 4) 3].
The bidentate ligand acetylacetonate is often abbreviated acac. Typically both oxygen atoms bind to the metal to form a six-membered chelate ring. The simplest complexes have the formula M(acac) 3 and M(acac) 2. Mixed-ligand complexes, e.g. VO(acac) 2, are also numerous.
The acetylacetonate anion is a bidentate ligand. IUPAC recommended pK a values for this equilibrium in aqueous solution at 25 °C are 8.99 ± 0.04 (I = 0), 8.83 ± 0.02 (I = 0.1 M NaClO 4) and 9.00 ± 0.03 (I = 1.0 M NaClO 4; I = Ionic strength). [9] Values for mixed solvents are available.
Diars is a bidentate ligand used in coordination chemistry. It was first described in 1939, [2] but was popularized by R. S. Nyholm for its ability to stabilize metal complexes with unusual oxidation states and coordination numbers, e.g. TiCl 4 (diars) 2. High coordination numbers arise because diars is fairly compact and the As-M bonds are ...
Peroxide is a common ligand in metal complexes. Within the area of transition metal dioxygen complexes, O 2− 2 functions as a bidentate ligand. [4] Many transition metal dioxygen complexes are best described as adducts of peroxide. [5] Some complexes mix oxide and peroxide ligands: for example, chromium(VI) oxide peroxide (CrO 2) 2 O).