Trimer (chemistry)

In chemistry, a trimer (/ˈtraɪmər/; from Ancient Greek tri- 'three', and -mer 'parts') is a molecule or polyatomic anion formed by combination or association of three molecules or ions of the same substance. In technical jargon, a trimer is a kind of oligomer derived from three identical precursors often in competition with polymerization.

Examples

Alkyne trimerisation

Further information: Alkyne trimerisation

 

The trimerization cyclization reaction can be understood with this scheme.

In 1866, Marcellin Berthelot reported the first example of cyclotrimerization, the conversion of acetylene to benzene.^[1] This process was commercialized:

 

Nitrile trimerization

Symmetrical 1,3,5-triazines are prepared by trimerization of certain nitriles such as cyanogen chloride.

Cyanogen chloride and cyanogen bromide each trimerize at elevated temperatures over a carbon catalyst.^[1] The chloride gives cyanuric chloride:

 

The bromide has an extended shelflife when refrigerated. Like the chloride, it undergoes ab exothermic trimerisation to form cyanuric bromide. This reaction is catalyzed by traces of bromine, metal salts, acids and bases.^[2] For this reason, experimentalists avoid brownish samples.^[3]

 

An industrial route to cyanuric acid entails the thermal decomposition of urea, with release of ammonia. The conversion commences at approximately 175 °C:^[4]

${\displaystyle {\ce {3 H2N-CO-NH2 -> [C(O)NH]3 + 3 NH3}}}$ 

The endothermic synthesis of melamine can be understood in two steps.

 

First, urea decomposes into cyanic acid and ammonia in an endothermic reaction:

${\displaystyle {\ce {(NH2)2CO -> HOCN + NH3}}}$ 

Then in the second step, cyanic acid polymerizes to form cyanuric acid, which condenses with the liberated ammonia from the first step to release melamine and water.

${\displaystyle {\ce {3 HOCN -> [C(O)NH]3}}}$ 

${\displaystyle {\ce {[C(O)NH]3 + 3 NH3 -> C3H6N6 + 3 H2O}}}$ 

This water then reacts with cyanic acid present, which helps drive the trimerization reaction, generating carbon dioxide and ammonia.

${\displaystyle {\ce {3 HOCN + 3 H2O -> 3 CO2 + 3NH3}}}$ 

In total, the second step is exothermic:

${\displaystyle {\ce {6 HCNO + 3 NH3 -> C3H6N6 + 3 CO2 + 3NH3}}}$ 

but the overall process is endothermic.

Diene trimerisation

The 1,5,9-trans-trans-cis isomer of cyclododecatriene, which has some industrial importance is obtained by cyclotrimerization of butadiene with titanium tetrachloride and an organoaluminium co-catalyst:^[5]

 

Breaking carbon-hetero double bonds forms symmetrical saturated 1,3,5-heterocycles

Cyclotrimerization of formaldehyde affords 1,3,5-Trioxane:

 

1,3,5-Trithiane is the cyclic trimer of the otherwise unstable species thioformaldehyde. This heterocycle consists of a six-membered ring with alternating methylene bridges and thioether groups. It is prepared by treatment of formaldehyde with hydrogen sulfide.^[6]

Three molecules of acetaldehyde condense to form paraldehyde, a cyclic trimer containing C-O single bonds.

Catalyzing and dehydrating by sulfuric acid, trimerization of acetone via aldol condensation affords mesitylene^[7]

Trisiloxanes

Dimethylsilanediol dehydrates to a trimer of Me₂SiO as well as polydimethylsiloxane. The reaction illustrates the competition between trimerization and polymerization. The polymer and trimer are formally derived from the hypothetical sila-ketone Me₂Si=O, although this species is not an intermediate.

Coordination chemistry

The dithiobenzoate complexes [M(S₂CPh)₂] crystallize as trimers (M = Ni, Pd).^[8]

 

Structure of the trimer [Ni(S₂CPh)₂]₃.

See also

• Oligomer
• Protein trimer

References

1. Hillis O. Folkins (2005). "Benzene". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_475. ISBN 3527306730.
2. Morris, Joel; Kovács, Lajos; Ohe, Kouichi (2015). "Cyanogen Bromide". Encyclopedia of Reagents for Organic Synthesis. pp. 1–8. doi:10.1002/047084289X.rc269.pub3. ISBN 9780470842898.
3. Joel Morris; Lajos Kovács (2008). "Cyanogen Bromide". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rc269.pub2. ISBN 978-0471936237.
4. Klaus Huthmacher, Dieter Most "Cyanuric Acid and Cyanuric Chloride" Ullmann's Encyclopedia of Industrial Chemistry" 2005, Wiley-VCH, Weinheim. doi 10.1002/14356007.a08 191
5. Industrial Organic Chemistry, Klaus Weissermel, Hans-Jurgen Arpe John Wiley & Sons; 3rd 1997 ISBN 3-527-28838-4
6. Bost, R. W.; Constable, E. W. "sym-Trithiane" Organic Syntheses, Collected Volume 2, p.610 (1943). (PDF). Archived from the original (PDF) on 2012-03-29. Retrieved 2014-05-05.{{cite web}}: CS1 maint: archived copy as title (link)
7. Cumming, W. M. (1937). Systematic organic chemistry (3E). New York, USA: D. Van Nostrand Company. p. 57.
8. Bonamico, M.; Dessy, G.; Fares, V.; Scaramuzza, L. (1975). "Structural Studies of Metal Complexes with Sulphur-Containing Bidentate Ligands. Part I. Crystal and Molecular Structures of Trimeric Bis-(dithiobenzoato)-nickel(II) and -palladium(II)". Journal of the Chemical Society, Dalton Transactions (21): 2250–2255. doi:10.1039/DT9750002250.

 

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