Metal carbonyl

Metal carbonyls are coordination complexes of transition metals with carbon monoxide ligands. They occur as neutral complexes, as positively charged metal carbonyl cations or as negatively charged metal carbonylates. The carbon monoxide ligand may be bound terminally to a single metal atom or bridging to two or more metal atoms. These complexes may be homoleptic, that is containing only CO ligands, such as nickel carbonyl (Ni(CO)₄), but more commonly metal carbonyls are heteroleptic and contain a mixture of ligands.

Metal carbonyls are useful in organic synthesis and as catalysts or catalyst precursors in homogeneous catalysis, such as hydroformylation and Reppe chemistry. In the Mond process, nickel carbonyl is used to produce pure nickel. In organometallic chemistry, metal carbonyls serve as precursors for the preparation of other organometalic complexes.

Metal carbonyls are toxic by skin contact, inhalation or ingestion, in part because of their ability to carbonylate hemoglobin to give carboxyhemoglobin, which prevents the binding of O₂.

In metalic carbonyls, metals are in zero oxidation state.

Metal carbonyls of transition elements constitute another important class of organometallic compounds. All d-block elements which contain only carbonyl ligands are called homoleptic carbonyls.

Amond in 1890 prepared the first homoleptic carbonyl, Ni(CO)₄. Later on a large number of neutral binary carbonyl like, Fe(CO)₅, Cr(CO)₆, Mo(CO)₆, W(CO)₆ were prepared. In addition to mononuclear metal carbonyls mentioned above, transition metals from many polynuclear metal carbonyls such as Fe₃(CO)₁₂, Mn₂(CO)₁₀. The metal carbon bonds in metal carbonyls possess both σ and π character.

Classification of metal carbonyls

Metal carbonyls are classified into two types:

(i) Mononuclear (or monomeric) carbonyls: these are such compounds which contain only one metallic atom per molecule. For example, V(CO)₆, Cr(CO)₆, etc.

(ii) Polynuclear carbonyls: these contain two or more metallic atoms per molecule and are of the type M_x(CO)_y. These carbonyls are also sometimes called as bridged carbonyls. Polynuclear carbonyls may be homonuclear e.g., Fe₃(CO)₁₂ or heteronuclear e.g.,MnCo(CO)₉, MnRe(CO)₁₀.

Nomenclature of metal carbonyls

(i) In metal carbonyls the metal atom is in zero oxidation sate therefore it may not be mentioned.

(ii) If the metal atom appears two or more times than the word di, ter etc is added before the name of metal atom.

(iii) If the CO groups act as bridge between the two metals atoms then the Greek letter mu () is written before their names.

(iv) When the metal-metal bond is present between similar atoms than the multiple prefixes, bis, tris, etc. are taken.

(v) While writing the names of π bonded organometallic compounds the symbol prefixes, hapto (η) is used before the name of molecule indicating the number of carbon atoms in the carbon bonded ligand.

Some examples are given below to illustrate the above points.
                                           
Ni(CO)₄ Tetracarbonylnickel
                                 
Mn₂(CO)₁₀ decacarbonyl dimanganese
                                     
Co₂(CO)₈ Octacarbonyl dicobalt
                                      
Fe(CO)₉ Enneacarbonyldiiron
                      
(CO)₃-Co-(CO)₂-Co(CO)₃ Di--carbonyl bis (tricarbonyl cobalt)
                           
(CO)₄Co-Co-(CO)₄ Bis (tetracarbonyl cobalt)
                          
(CO)₃Fe(CO)₃Fe(CO)₃ Tri--Carbonyl bis (tricarbonyl iron)
                         
(C₆H₆) Cr(CO)₃ (η₆-benzene) tricarbonyl chromium   
                         
Fe(CO₃) (C₄H₆) (η₄-butadiene) tricarbonyl iron.

Bonding in metal carbonyl

As already mentioned, the M-C bond in metal carbonyls has σ as well as π character. The metal-carbon σ bond is formed by the donation of lone pair of electrons on the carbonyl carbon into a vacant orbital of the metal. The metal-carbon π bond is formed by the donation of a pair of electrons from a filled d-orbital of metal into the vacant antibonding pi-molecular orbital (π) of carbon monoxide.

The metal to ligand bonding generates a synergic effect that reinforces the bond between CO and the metal.

Preparation of metal carbonyls

Finely divided nickel reacts with CO at room temperature to form Ni(CO)₄.
                                                 
Ni + 4CO    Ni(CO)₄

Iron reacts with CO at higher temperature and pressure.
                                                 
Fe + 5CO    Fe(CO)₅

Nickel can be purified by first converting it into volatile Ni(CO)₄ and subsequent thermal decomposition of Ni(CO)₄. This process is known as Mond process.

Properties of metal carbonyls

1. Metal carbonyls are generally solids at room temperature and pressure. However Nickel carbonyls are liquids.

2. The mononuclear carbonyls are unstable and noxious.

3. Mononuclear carbonyls are either colourless or light coloured whereas polynuclear carbonyls are more deeply coloured. For example, Fe(CO)₅ is light straw coloured liquid while Fe₃(CO)₁₂ is a deep green solid.

4. With exception of Fe2(CO)₉, carbonyls are soluble in hydrocarbon solvents.