Bridging ligand

In coordination chemistry, a bridging ligand is a ligand that connects two or more atoms, usually metal ions. The ligand may be atomic or polyatomic. Virtually all complex organic compounds can serve as bridging ligands, so the term is usually restricted to small ligands such as pseudohalides or to ligands that are specifically designed to link two metals.

In naming a complex wherein a single atom bridges two metals, the bridging ligand is preceded by the Greek letter mu, μ, with a subscript number denoting the number of metals bound to the bridging ligand. μ₂ is often denoted simply as μ. When describing coordination complexes care should be taken not to confuse μ with η ('eta'), which relates to hapticity. Ligands that are not bridging are called terminal ligands.

List of bridging ligands

Virtually all ligands are known to bridge, with the exception of amines and ammonia. Common bridging ligands include most of the common anions.

Many simple organic ligands form strong bridges between metal centers. Many common examples include organic derivatives of the above inorganic ligands (R = alkyl, aryl): , , , (imido), (phosphido, note the ambiguity with the preceding entry), (phosphinidino), and many more.

Examples

File:Ru-Cl.png, In this ruthenium complex ((benzene)ruthenium dichloride dimer), two chloride ligands are terminal and two are μ₂ bridging.
File:Creutz-Taube-Ion.svg, Pyrazine is a bridging ligand in this diruthenium compound, called the Creutz–Taube complex.
File:Mu3 compound.png, In the cobalt cluster , the ligand is triply bridging, although this aspect is typically not indicated in the formula.
File:Fe3(CO)12lessFe-Fe.png, In triiron dodecarbonyl, two CO ligands are bridging and ten are terminal ligands. The terminal and bridging CO ligands interchange rapidly.
File:Niobium-pentachloride-dimer-2D.png, In NbCl₅, there are two bridging and eight terminal chloride ligands.
File:Au6C(PPh3)6.png, The cluster features a μ₆- carbide ligand, although again, the designator "μ" is not usually used.
File:Aluminium-trifluoride-3D-polyhedra.png, In rhenium trioxide, the oxide ligands are all μ₂. These oxide ligands "glue" together the metal centres.
File:Zirconium-tetrachloride-3D-balls-A.png, In the case of , there are both terminal and doubly bridging chloride ligands.
File:Rhodium(II)-acetate-hydrate-dimer-from-xtal-1971-3D-balls.png, In rhodium(II) acetate, the four acetate groups are bridging ligands.
File:VO(HPO4)0.5H2O.tif, In , pairs of vanadium(IV) centers are bridged by water ligands.

Bonding

For doubly bridging (μ₂-) ligands, two limiting representation are 4-electron and 2-electron bonding interactions. These cases are illustrated in main group chemistry by and . Complicating this analysis is the possibility of metal–metal bonding. Computational studies suggest that metal-metal bonding is absent in many compounds where the metals are separated by bridging ligands. For example, calculations suggest that lacks an iron–iron bond by virtue of a 3-center 2-electron bond involving one of three bridging CO ligands.

Polyfunctional ligands

Polyfunctional ligands can attach to metals in many ways and thus can bridge metals in diverse ways, including sharing of one atom or using several atoms. Examples of such polyatomic ligands are the oxoanions and the related carboxylates, , and the polyoxometalates. Several organophosphorus ligands have been developed that bridge pairs of metals, a well-known example being {{chem2, link=dppm, Ph2PCH2PPh2.

See also

*Bridging carbonyl

References

Coordination chemistry