Manganese(III) fluoride
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| Manganese(III) fluoride | |
|---|---|
| Image:Manganese(III) fluoride.jpg | |
| General | |
| Systematic name | Manganese(III) fluoride |
| Other names | Manganese trifluoride |
| Molecular formula | F3Mn |
| Molar mass | 111.938 g/mol |
| Appearance | purple-pink powder |
| CAS number | [7783-53-1] |
| Properties | |
| Density and phase | 3.54 g/cm3, solid |
| Solubility in water | hydrolysis |
| Other solvents | 0.164 g/100 mL in HF |
| Melting point | ?°C (? K) |
| Structure | |
| Coordination geometry |
distorted octahedral |
| Crystal structure | VF3 |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | toxic fumes |
| NFPA 704 | |
| R/S statement | R: 8-20/21/22-36/37/38 S: 17-26-36/37/39 |
| RTECS number | OP0882600 |
| Related compounds | |
| Related compounds | Manganese acetylacetonate Cobalt(III) fluoride |
| Except where noted otherwise, data are given for materials in their standard state (at 25°C, 100 kPa) Infobox disclaimer and references |
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Manganese trifluoride is the chemical compound with the formula MnF3. This purplish solid is highly reactive, being unstable in moist air and liberating F2 upon heating. MnF3 is useful for converting hydrocarbons into fluorocarbons, i.e. it is a fluorination agent.[1]
- R3C-H + 2 MnF3 → R3C-F + HF + 2MnF2
A related fluorinating reagent is CoF3.
Contents |
[edit] Synthesis and reactions
MnF3 can be prepared by treating a solution of MnF2 in anhydrous hydrogen fluoride with fluorine:[2]
- MnF2 + 0.5 F2 → MnF3
In the crystalline state, MnF3 resembles vanadium(III) fluoride: both feature octahedal metal centers with the same average M-F bond distances. In the Mn compound, however, is distorted (and hence a monoclinic unit cell vs a higher symmetry one) due to the Jahn-Teller effect, with pairs of Mn-F distances of 1.79, 1.91, 2.09 A.[3][4][5] Jahn-Teller distortions are characteristic of the presence of four d-electrons in the valence shell.
[edit] Related Mn(III) and Mn(IV) compounds
The fluorination of MnF2 in HF, if conducted in the presence of UV-irradiation, gives MnF4. This tetrafluoride is a relatively rare Mn(IV) species, the most famous example being manganese dioxide.
Other manganese(III) compounds include manganese(III) acetate (CAS #993-02-2) manganese acetylacetonate (CAS# 14284-89-0), Both are employed as oxidants in organic synthesis. MnF3 is Lewis acidic and forms a variety of derivatives. Two examples are K2MnF3(SO4)[6] and K2MnF5.
[edit] Safety considerations
Like other reactive inorganic fluorides, MnF3 should be stored in a polyethylene bottles.
[edit] References
- ^ Burley, G. A.; Taylor, R. "Manganese(III) fluoride" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.
- ^ Z. Mazej (2002). "Room temperature syntheses of MnF3, MnF4 and hexafluoromanganete(IV) salts of alkali cations". Journal of Fluorine Chemistry 114 (1): 75-80. DOI:10.1016/S0022-1139(01)00566-8.
- ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ^ Hepworth, M. A.; Jack, K. H.; Nyholm, R. S. ”Interatomic Bonding in Manganese Trifluoride” Nature 1957, 179, 211 - 212. doi:10.1038/179211b0
- ^ M. A. Hepworth, K. H. Jack (1957). "The crystal structure of manganese trifluoride, MnF3". Acta Crystallographica 10: 345-351. DOI:10.1107/S0365110X57001024.
- ^ Bhattacharjee, M. N; Chaudhuri, M. K. “Dipotassium Trifluorosulfatomanganate(III)” Inorganic Syntheses, 1990, volume 27, pages 312-313. ISBN 0-471-50976-0
[edit] External links
- National Pollutant Inventory - Fluoride and compounds fact sheet
- National Pollutant Inventory - Manganese and compounds Fact Sheet
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