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A dimer (/ˈdaɪmər/) (di-, "two" + -mer, "parts") is an oligomer consisting of two monomers joined by bonds that can be either strong or weak, covalent or intermolecular. Dimers also have significant implications in polymer chemistry, inorganic chemistry, and biochemistry.

The term homodimer is used when the two molecules are identical (e.g. A–A) and heterodimer when they are not (e.g. A–B). The reverse of dimerisation is often called dissociation. When two oppositely charged ions associate into dimers, they are referred to as Bjerrum pairs, after Niels Bjerrum.

Noncovalent dimers

Anhydrous carboxylic acids form dimers by hydrogen bonding of the acidic hydrogen and the carbonyl oxygen. For example, acetic acid forms a dimer in the gas phase, where the monomer units are held together by hydrogen bonds. Under special conditions, most OH-containing molecules form dimers, e.g. the water dimer.

Excimers and exciplexes are excited structures with a short lifetime. For example, noble gases do not form stable dimers, but they (dimers) do form the excimers Ar₂*, Kr₂* and Xe₂* under high pressure and electrical stimulation.

Covalent dimers

Molecular dimers are often formed by the reaction of two identical compounds e.g.: 2A → A−A. In this example, monomer "A" is said to dimerise to give the dimer "A−A". An example is a diaminocarbene, which dimerise to give a tetraaminoethylene:

${\displaystyle {\ce {2 C(NR2)2 -> (R2N)2C=C(NR2)2}}}$

Carbenes are highly reactive and readily form bonds.

Dicyclopentadiene is an asymmetrical dimer of two cyclopentadiene molecules that have reacted in a Diels-Alder reaction to give the product. Upon heating, it "cracks" (undergoes a retro-Diels-Alder reaction) to give identical monomers:

${\displaystyle {\ce {C10H12 -> 2 C5H6}}}$

Many nonmetallic elements occur as dimers: hydrogen, nitrogen, oxygen, the halogens, i.e. fluorine, chlorine, bromine and iodine. Noble gases can form dimers linked by van der Waals bonds, for example dihelium or diargon. Mercury occurs as a mercury(I) cation (Hg2+2), formally a dimeric ion. Other metals may form a proportion of dimers in their vapour. Known metallic dimers include dilithium (Li₂), disodium (Na₂), dipotassium (K₂), dirubidium (Rb₂) and dicaesium (Cs₂).

Such elemental dimers are homonuclear diatomic molecules.

Many small organic molecules, most notably formaldehyde, easily form dimers. The dimer of formaldehyde (CH₂O) is dioxetane (C₂H₄O₂).

Borane (BH₃) occurs as the dimer diborane (B₂H₆), due to the high Lewis acidity of the boron center.

Polymer chemistry

In the context of polymers, "dimer" also refers to the degree of polymerization 2, regardless of the stoichiometry or condensation reactions.

One case where this is applicable is with disaccharides. For example, cellobiose is a dimer of glucose, even though the formation reaction produces water:

${\displaystyle {\ce {2 C6H12O6 -> C12H22O11 + H2O}}}$

Here, the resulting dimer has a stoichiometry different from the initial pair of monomers.

Amino acids can also form dimers, which are called dipeptides. An example is glycylglycine, consisting of two glycine molecules joined by a peptide bond. Other examples include aspartame and carnosine.

Inorganic dimers

Group 13 Dimers

Boranes

Diborane (B₂H₆) is a classic example of an inorganic dimer. Borane does not exist alone as BH₃, even though it is often written in that way. B₂H₆ exists as a structure where two hydrogen atoms bridge the two boron atoms. The bridging B-H bonds are lower in bond order than what would be expected for a regular B-H bond (they are lower in bond order than the terminal B-H bonds). This is explained by the bond having three centers but only two electrons, "banana bond", instead of the typical single bond with two centers and two electrons.

Aluminium

Organoaluminium complexes can exist as either monomers or dimers based on the steric bulk of the groups attached. For example, methyl or ethylaluminium exists as a dimer, but when a bulkier group is added, the complex exists as a monomer, such as trimesitylaluminium.

Biochemical dimers

Pyrimidine Dimers

Pyrimidine dimers (also known as thymine dimers) are formed by a photochemical reaction from pyrimidine DNA bases when DNA is exposed to ultraviolet light. This cross-linking causes DNA mutations which can be carcinogenic, causing skin cancers. When pyrimidine dimers are present they can block polymerases which decreases DNA functionality until it is repaired.

Protein Dimers

Protein dimers arise from the interaction of two proteins which can then interact further to make larger more complex oligomer. For example, tubulin is formed by the dimerization of α-tubulin and β-tubulin and this dimer can then polymerize further to make microtubules. For symmetric proteins the larger protein complex can be broken down into smaller identical protein subunits which then dimerize in order to decrease the amount of genetic code required to make the functional protein.

G protein-coupled Receptors

As the largest and most diverse family of receptors within the human genome, G protein-coupled receptors (GPCR) have been studied extensively, with recent studies supporting their ability to form dimers. GPCR dimers include both homodimers and heterodimers formed from related members of the GPCR family. While not all, some GPCRs require dimerization to function, such as GABA_B-receptor, emphasizing the importance of dimers in biological systems.

Receptor Tyrosine Kinase

Much like for G protein-coupled receptors, dimerization is essential for receptor tyrosine kinases (RTK) to perform their function in signal transduction, affecting many different cellular processes. RTKs typically exist as monomers, but undergo a conformational change upon ligand binding, allowing them to dimerize with nearby RTKs. The dimerization activates the cytoplasmic kinase domains that are responsible for further signal transduction.

See also

• Monomer
• Trimer
• Polymer
• Protein dimer
• Oligomer

References

• "IUPAC "Gold Book" definition". doi:10.1351/goldbook.D01744. S2CID 242984652. Retrieved 2009-04-30. {{cite journal}}: Cite journal requires |journal= (help)

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• Chemical compounds
• Dimers (chemistry)