Metal phosphine complex

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In coordination chemistry phosphines are L-type ligands. Unlike most metal ammine complexes, metal phosphine complexes tend to be lipophilic, displaying good solubility in organic solvents. They also are compatible with metals in multiple oxidation states. Because of these two features, metal phosphine complexes are useful in homogeneous catalysis.[1] Prominent examples of metal phosphine complexes include Wilkinson's catalyst (Rh(PPh3)3Cl), Grubbs' catalyst, and tetrakis(triphenylphosphine)palladium(0).[2]

Wilkinson's catalyst, a popular catalyst for hydrogenation.


The first phosphine complexes were cis- and trans-PtCl2(PEt3)2 reported by Cahours and Gal in 1870.[3]

A popular phosphine ligand is triphenylphosphine, a shelf-stable solid that undergoes oxidation in air relatively slowly.

Many complexes continue to be prepared from metal halides. For example, treatment of palladium chloride with triphenylphosphine yields monomeric bis(triphenylphosphine)palladium(II) chloride units.[4]

[PdCl2]n + 2n PPh3 → n PdCl2(PPh3)2

M-PR3 bonding[edit]

Phosphines primarily function as Lewis bases, interacting with metals as σ donor ligands.

TEP for selected phosphines[5]
L ν(CO) cm−1
P(t-Bu)3 2056.1
PMe3 2064.1
PPh3 2068.9
P(OEt)3 2076.3
PCl3 2097.0
PF3 2110.8

Phosphine ligands are also π-acceptors. Their π-acidity arises from overlap of P-C σ* anti-bonding orbitals with filled metal orbitals. Aryl- and fluorophosphines are stronger π-acceptors than alkylphosphines. Trifluorophosphine (PF3) is a strong π-acid with bonding properties akin to those of the carbonyl ligand.[6] 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.[7] The energy of the σ* orbitals is lower for phosphines with electronegative substituents, and for this reason phosphorus trifluoride is a particularly good π-acceptor.[8]

Steric properties[edit]

Cone angle is a common and useful parameter for evaluating the steric properties of phosphine ligands.

By changes in one or more of the three organic substituents, the steric and electronic properties of phosphine ligands can be manipulated. These properties are manifested in the catalytic properties of the host metal center.[9] The steric properties of phosphine ligands can be ranked by their steric properties. The Tolman cone angle is widely used.[10]


Phosphine ligands are usually "spectator" rather than "actor" ligands. They generally do not participate in reactions, except to dissociate from the metal center. In certain high temperature hydroformylation reactions, the scission of P-C bonds is observed however.[11] The thermal stability of phosphines ligands is enhanced when they are incorporated into pincer complexes.

Applications to homogeneous catalysis[edit]

One of the first applications of phosphine ligands in catalysis was the use of triphenylphosphine in “Reppe” chemistry (1948), which included reactions of alkynes, carbon monoxide, and alcohols.[12] In his studies, Reppe discovered that this reaction more efficiently produced acrylic esters using NiBr2(PPh3)2 as a catalyst instead of NiBr2. Shell developed cobalt-based catalysts modified with trialkylphosphine ligands for hydroformylation (now a rhodium catalyst is more commonly used for this process).[13] The success achieved by Reppe and his contemporaries led to many industrial applications.[14]

Complexes of other organophosphorus ligands[edit]

The popularity and usefulness of phosphine complexes has led to the popularization of complexes of many related organophosphorus ligands.[3] Complexes of arsines have also been widely investigated, but are avoided in practical applications because of concerns about toxicity.

Complexes of primary and secondary phosphines[edit]

Most work focuses on complexes of triorganophosphines, but primary and secondary phosphines, respectively RPH2 and R2PH, also function as ligands. Such ligands are less basic and have small cone angles. These complexes are susceptible to deprotonation leading to phosphido-bridged dimers and oligomers:

2 LnM(PR2H)Cl → [LnM(μ-PR2)]2 + 2 HCl

Complexes of PRx(OR')3−x[edit]

Nickel(0) complexes of phosphites, e.g., Ni[P(OEt)3]4 are useful catalysts for hydrocyanation of alkenes. Related complexes are known for phosphinites (R2P(OR')) and phosphonites (RP(OR')2).

Diphosphine complexes[edit]

Due to the chelate effect, ligands with two phosphine groups bind more tightly to metal centers than do two monodentate phosphines. The conformation of diphosphines is restricted, and for this reason many are used in asymmetric catalysis, e.g. Noyori asymmetric hydrogenation. Several diphosphines have been developed; many of these diphosphines have two arylphosphines linked by a short alkylidene bridge, e.g. 1,2-bis(diphenylphosphino)ethane (dppe). 1,1'-Bis(diphenylphosphino)ferrocene is interesting, because it uses a ferrocene unit as the linker. Several trans-spanning ligands like xantphos and spanphos are known as well. The complex dichloro(1,3-bis(diphenylphosphino)propane)nickel is useful in Kumada coupling.


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