Organolead compounds are chemical compounds containing a chemical bond between carbon and lead. Organolead chemistry is the corresponding science. The first organolead was hexaethyldilead synthesised in 1858. Sharing the same group with carbon, lead is tetravalent.
Going down the carbon group the C–X (X = C, Si. Ge, Sn, Pb) bond becomes weaker and the bond length larger. The C–Pb bond in tetramethyllead is 222 pm long with a dissociation energy of 204 kcal/mol (854 kJ/mol). For comparison the C–Sn bond in tetramethyltin is 214 pm long with dissociation energy 297 kcal/mol (1.24 MJ/mol). The dominance of Pb(IV) in organolead chemistry is remarkable because inorganic lead compounds tend to have Pb(II) centers. The reason is that with inorganic lead compounds elements such as nitrogen, oxygen and the halides have a much higher electronegativity than lead itself and the partial positive charge on lead then leads to a stronger contraction of the 6s orbital than the 6p orbital making the 6s orbital inert. 
Organolead compounds can be derived from Grignard reagents and lead chloride. For example methylmagnesium chloride reacts with lead chloride to tetramethyllead, a water-clear liquid with boiling point 110 °C and density 1.995 g/cm³. Reaction of lead chloride with the lithium salt of pentamethylcyclopentadiene gives the lead metallocene plumbocene.
Certain arene compounds react directly with lead tetraacetate to aryl lead compounds in an electrophilic aromatic substitution. For instance anisole with lead tetraacetate forms p-methoxyphenyllead triacetate in chloroform and dichloroacetic acid:
Other compounds of lead are organolead halides of the type RnPbX(4-n), organolead sulfinates (RnPb(OSOR)(4−n)) and organolead hydroxides (RnPb(OH)(4−n)). Typical reactions are :
Derived from the hydroxides are the plumboxanes:
which give access to polymeric alkoxides:
The C–Pb bond is weak and for this reason homolytic cleavage of organolead compounds to free radicals is easy. In its anti-knocking capacity, its purpose is that of a radical initiator. General reaction types of aryl and vinyl organoleads are transmetalation for instance with boronic acids and acid-catalyzed heterocyclic cleavage. Organoleads find use in coupling reactions between arene compounds. They are more reactive than the likewise organotins and can therefore be used to synthesise sterically crowded biaryls.
In oxyplumbation, organolead alkoxides are added to polar alkenes:
The alkoxide is regenerated in the subsequent methanolysis and therefore acts as a catalyst.
The reaction requires the presence of a large excess of a coordinating amine such as pyridine which presumably binds to lead in the course of the reaction. The reaction is insensitive to radical scavengers and therefore a free radical mechanism can be ruled out. The reaction mechanism is likely to involve nucleophilic displacement of an acetate group by the phenolic group to a diorganolead intermediate which in some related reactions can be isolated. The second step is then akin to a Claisen rearrangement except that the reaction depends on the electrophilicity (hence the ortho preference) of the phenol.
The carbanion forms by proton abstraction of the acidic α-proton by pyridine (now serving a double role) akin to the Knoevenagel condensation. This intermediate displaces an acetate ligand to a diorganolead compound and again these intermediates can be isolated with suitable reactants as unstable intermediates. The second step is reductive elimination with formation of a new C–C bond and lead(II) acetate.
These intermediates break up by disproportionation.
Plumbylidines of the type RPb (formally Pb(I)) are ligands to other metals in LnMPbR compounds (compare to carbon metal carbynes).
|Core organic chemistry||Many uses in chemistry.|
|Academic research, but no widespread use||Bond unknown / not assessed.|
Environmental aspects of organolead compounds: Abadin, H.G.; Pohl, H.R. (2010). "Alkyllead conpounds and their environmental toxicology". Metal ions in life sciences (Cambridge: RSC publishing) 7, Organometallics in environment and toxicology: 153-164. ISBN 9781847551771.