Dimanganese decacarbonyl
10.png)
| |
| |
| Names | |
|---|---|
| IUPAC name
bis(pentacarbonylmanganese)(Mn—Mn)
| |
| Other names
Manganese carbonyl
Decacarbonyldimanganese | |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.030.392 |
PubChem CID
|
|
| UNII | |
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| Mn2(CO)10 | |
| Molar mass | 389.98 g/mol |
| Appearance | Yellow crystals |
| Density | 1.750 g/cm3 |
| Melting point | 154 °C (309 °F; 427 K) |
| Boiling point | sublimes 60 °C (140 °F; 333 K) at 0.5 mm Hg |
| Insoluble | |
| Structure[1] | |
| monoclinic | |
a = 14.68 Å, b = 14.16 Å, c = 7.16 Å α = 90°, β = 75°, γ = 90°
| |
Formula units (Z)
|
4 |
| 0 D | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
|
CO source |
| Related compounds | |
Related compounds
|
Re2(CO)10 Co2(CO)8 Fe3(CO)12 Fe2(CO)9 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Dimanganese decacarbonyl is the chemical compound with the formula Mn2(CO)10. This metal carbonyl is an important reagent in the organometallic chemistry of manganese.[2]
Synthesis
The compound was first prepared in low yield by the reduction of manganese iodide with magnesium under CO.[1] A more efficient preparation entails reduction of anhydrous MnCl2 with sodium benzophenone ketyl under 200 atmospheres of CO.[3] The availability of inexpensive methylcyclopentadienyl manganese tricarbonyl ("MMT") has led to a low pressure route to Mn2(CO)10.[4]
Structure
Mn2(CO)10 has no bridging CO ligands: it can be described (CO)5Mn-Mn(CO)5. There are two kinds of CO ligands; one CO on each Mn is coaxial with the Mn-Mn bond (293 pm), and four on each manganese that are perpendicular to it (equatorial). In the stable rotamer, the two Mn(CO)5 subunits are staggered. The overall molecule thus belongs to the point group D4d, which is an uncommon symmetry shared with S2F10.[5]
Reactions
Mn2(CO)10 is air stable as a crystalline solid, but solutions require Schlenk techniques. It finds limited use in organic synthesis.[6] Characteristic reactions:
- Reduction of Mn2(CO)10 gives the manganese pentacarbonyl anion, which can be isolated as a salt:
- Mn2(CO)10 + 2 Na → 2 Na[Mn(CO)5]
The anion is a versatile nucleophile. Protonation gives the hydride [HMn(CO)5], and methylation gives [(CH3)Mn(CO)5].
- Bromination of Mn2(CO)10 proceeds with scission of the Mn-Mn bond to give manganese pentacarbonyl bromide.
- Mn2(CO)10 + Br2 → 2[Mn(CO)5Br]
Safety
Mn2(CO)10 is a volatile source of a metal and a source of CO.
References
- ^ a b Brimm, E. O.; Lynch, M. A.; Sesny, W. J. "Preparation and Properties of Manganese Carbonyl" Journal of the American Chemical Society 1954, volume 76, page 3831 - 3835.
- ^ Elschenbroich, C. "Organometallics" (2006) Wiley-VCH: Weinheim. ISBN 978-3-527-29390-2
- ^ King, R. B. Organometallic Syntheses. Volume 1 Transition-Metal Compounds; Academic Press: New York, 1965. ISBN 0-444-42607-8
- ^ King, R. B.; Stokes, J. C.; Korenowski, T. F. "A Convenient Synthesis of Dimanganese Decarbonyl from Inexpensive Starting Materials at Atmospheric Pressure" Journal of Organometallic Chemistry 1968, volume 11, Pages 641-643.
- ^ L. F. Dahl, E. Ishishi, R. E. Rundle "Polynuclear Metal Carbonyls. I. Structures of Mn2(CO)10 and Re2(CO)10 J. Chem. Phys. 1957, volume 26, p. 1750. doi:10.1063/1.1743615
- ^ Pauson, P. L. "Decacarbonyldimanganese" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. doi:10.1002/047084289X.