Bridging ligand

Source: Wikipedia, the free encyclopedia.
An example of a μ2 bridging ligand, represented with the red letter "L"

In

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

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.[3] Common bridging ligands include most of the common anions.

Bridging ligand Name Example
OH− hydroxide [Fe2(OH)2(H2O)8]4+, see olation
O2− oxide
[Cr2O7]2−, see polyoxometalate
SH− hydrosulfido Cp2Mo2(SH)2S2
NH−2
amido
 HgNH2Cl
N3− nitride [Ir3N(SO4)6(H2O)3]4−, see metal nitrido complex
CO
carbonyl
 Fe2(CO)9, see bridging carbonyl
Cl− chloride
halide ligands
H− hydride B2H6
CN− cyanide approx. Fe7(CN)18 (prussian blue), see cyanometalate
PPh−2 diphenylphosphide see transition metal phosphido complexes

Many simple organic ligands form strong bridges between metal centers. Many common examples include organic derivatives of the above inorganic ligands (R = alkyl, aryl):

NR−2
, NR2− (imido), PR−2 (phosphido, note the ambiguity with the preceding entry), PR2− (phosphinidino), and many more.

Examples

  • Compounds and complexes with bridging ligands
  • In this ruthenium complex ((benzene)ruthenium dichloride dimer), two chloride ligands are terminal and two are μ2 bridging.
    In this ruthenium complex (
    (benzene)ruthenium dichloride dimer), two chloride
    ligands are terminal and two are μ2 bridging.
  • Pyrazine is a bridging ligand in this diruthenium compound, called the Creutz–Taube complex.
    Pyrazine is a bridging ligand in this diruthenium compound, called the Creutz–Taube complex.
  • In the cobalt cluster Co3(CO)9(CtBu), the CtBu ligand is triply bridging, although this aspect is typically not indicated in the formula.
    In the cobalt cluster Co3(CO)9(CtBu), the
    CtBu
     ligand is triply bridging, although this aspect is typically not indicated in the formula.
  • In triiron dodecacarbonyl, two CO ligands are bridging and ten are terminal ligands. The terminal and bridging CO ligands interchange rapidly.
    In triiron dodecacarbonyl, two CO ligands are bridging and ten are terminal ligands. The terminal and bridging CO ligands interchange rapidly.
  • In NbCl5, there are two bridging and eight terminal chloride ligands.
    In
    NbCl5
    , there are two bridging and eight terminal chloride ligands.
  • The cluster [Au6C(PPh3)6]2+ features a μ6-carbide ligand, although again, the designator "μ" is not usually used.
    The cluster [Au6C(PPh3)6]2+ features a μ6-carbide ligand, although again, the designator "μ" is not usually used.
  • In rhenium trioxide, the oxide ligands are all μ2. These oxide ligands "glue" together the metal centres.
    In rhenium trioxide, the oxide ligands are all μ2. These oxide ligands "glue" together the metal centres.
  • In the case of ZrCl4, there are both terminal and doubly bridging chloride ligands.
    In the case of ZrCl4, there are both terminal and doubly bridging chloride ligands.
  • In rhodium(II) acetate, the four acetate groups are bridging ligands.
    In rhodium(II) acetate, the four acetate groups are bridging ligands.
  • In VO(HPO4)·0.5H2O, pairs of vanadium(IV) centers are bridged by water ligands.[4]
    In VO(HPO4)·0.5H2O, pairs of vanadium(IV) centers are bridged by water ligands.[4]

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 [Me2Al(μ2-Cl)]2 and [Me2Al(μ2-Me)]2. 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 Fe2(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.[5]

Bridge-terminal exchange

The interchange of bridging and terminal ligands is called bridge-terminal exchange. The process is invoked to explain the fluxional properties of

cobalt carbonyl and cyclopentadienyliron dicarbonyl dimer
:

Co2(μ-CO)2(CO)6 ⇌ Co2(μ-CO)2(CO)4(CO)2
(C5H5)2Fe2(μ-CO)2(CO)2 ⇌ (C5H5)2Fe2(μ-CO)2(CO)2

These dynamic processes, which are degenerate, proceed via an intermediate where the CO ligands are all terminal, i.e. (CO)4Co−Co(CO)4 and (C5H5)(CO)2Fe−Fe(CO)2C5H5.

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

Ph2PCH2PPh2
.

See also

  • Bridging carbonyl

References

  1. doi:10.1351/goldbook.B00741
  2. ISBN 0-85404-438-8. pp. 163–165. Electronic version.
  3. PMID 14966876
    .
  4. PMID 12206689
    .
  5. ^
    PMID 23047247
    .
  6. doi:10.1021/ja00801a012
    .
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