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Propadiene, the simplest allene, is also known as allene

Allenes are organic compounds in which one carbon atom has double bonds with each of its two adjacent carbon centres.[1] Allenes are classified as cumulated dienes. The parent compound of this class is propadiene, which is itself also called allene. Compounds with an allene-type structure but with more than three carbon atoms are members of a larger class of compounds called cumulenes with X=C=Y bonding.

Structure and properties[edit]


3D view of propadiene (allene)

The central carbon atom of allenes forms two sigma bonds and two pi bonds. The central carbon is sp-hybridized, and the two terminal carbon atoms are sp2-hybridized. The bond angle formed by the three carbon atoms is 180°, indicating linear geometry for the central carbon atom. The two terminal carbon atoms are planar, and these planes are twisted 90° from each other. The structure can also be viewed as an "extended tetrahedral" with a similar shape to methane, an analogy that is continued into the stereochemical analysis of certain derivative molecules.


Allene symmetry.png

The symmetry and isomerism of allenes has long fascinated organic chemists.[2] For allenes with four identical substituents, there exist two twofold axes of rotation through the center carbon, inclined at 45° to the CH2 planes at either end of the molecule. The molecule can thus be thought of as a two-bladed propeller. A third twofold axis of rotation passes through the C=C=C bonds, and there is a mirror plane passing through both CH2 planes. Thus this class of molecules belong to the D2d point group. Because of the symmetry, an unsubstituted allene has no net dipole moment.

R and S configurations are determined by precedences of the groups attached to the axial section of the molecule when viewed along that axis. The front plane is given higher priority over the other and the final assignment is given from priority 2 to 3 (i.e. the relationship between the two planes).

An allene with two different substituents on each of the two carbon atoms will be chiral because there will no longer be any mirror planes. The chirality of these types of allenes was first predicted in 1875 by van 't Hoff, but not proven experimentally until 1935.[3] Where A has a greater priority than B according to the Cahn–Ingold–Prelog priority rules, the configuration of the axial chirality can be determined by considering the substituents on the front atom followed by the back atom when viewed along the allene axis. For the back atom, only the group of higher priority need be considered.

Chiral allenes have been recently used as building blocks in the construction of organic materials with exceptional chiroptical properties.[4]

Chemical and spectral properties[edit]

Allenes differ considerably from other alkenes in terms of their chemical properties. Compared to isolated and conjugated dienes, they are considerably less stable: comparing the isomeric pentadienes, the allenic 1,2-pentadiene has a heat of formation of 33.6 kcal/mol, compared to 18.1 kcal/mol for (E)-1,3-pentadiene and 25.4 kcal/mol for the isolated 1,4-pentadiene.[5]

The C–H bonds of allenes are considerably weaker and more acidic compared to typical vinylic C–H bonds: the bond dissociation energy is 87.7 kcal/mol (compared to 111 kcal/mol in ethylene), while the gas-phase acidity is 381 kcal/mol (compared to 409 kcal/mol for ethylene[6]), making it slightly more acidic than the propargylic C–H bond of propyne (382 kcal/mol).

The 13C NMR spectrum of allenes is characterized by the signal of the sp-hybridized carbon, resonating at a characteristic 200-220 ppm.[7]

Allenes possess a rich cycloaddition chemistry, including both [4+2] and [2+2] modes of addition,[8][9] as well as undergoing formal cycloaddition processes catalyzed by transition metals.[10][11] Allenes also serve as substrates for transition metal catalyzed hydrofunctionalization reactions.[12][13][14]


Although allenes often require specialized syntheses, the parent allene, propadiene is produced industrially on a large scale as an equilibrium mixture with methylacetylene:

H2C=C=CH2 ⇌ H3C–C≡CH

This mixture, known as MAPP gas, is commercially available. At 298 K, the Δ of this reaction is –1.9 kcal/mol, corresponding to Keq = 24.7.[15]

The first allene to be synthesized was glutinic acid (2,3-pentadienedioic acid), which was prepared by Burton and Pechmann in 1887. However, the structure was only correctly identified in 1954.[16]

Laboratory methods for the formation of allenes include:


Fucoxanthin, the most abundant of all carotinoids, is the light-absorbing pigment in the chloroplasts of brown algae, giving them a brown or olive-green color.

Numerous natural products contain the allene functional group. Noteworthy are the pigments fucoxanthin and peridinin. Little is known about the biosynthesis, although it is conjectured that they are often generated from alkyne precursors.[22]

Allenes serve as ligands in organometallic chemistry. A typical complex is Pt(η2-allene)(PPh3)2. Ni(0) reagents catalyze the cyclooligomerization of allene.[23] Using a suitable catalyst (e.g. Wilkinson's catalyst), it is possible to reduce just one of the double bonds of an allene.[24]

Delta convention[edit]

Many rings or ring systems are known by semisystematic names that assume a maximum number of noncumulative bonds. To unambiguously specify derivatives that include cumulated bonds (and hence fewer hydrogens than would be expected from the skeleton), a lowercase delta may be used with a subscript indicating the number of cumulated double bonds from that atom, e.g. 8δ2-Benzocyclononene. This may be combined with the λ-convention for specifying nonstandard valency states, e.g. 2λ4δ2,5λ4δ2-Thieno[3,4-c]thiophene.[25]

See also[edit]

  • Compounds with three or more adjacent carbon–carbon double bonds are called cumulenes.


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