Manganese(III) fluoride (also known asManganese trifluoride) is theinorganic compound with the formula MnF3. This red/purplish solid is useful for convertinghydrocarbons intofluorocarbons, i.e., it is afluorination agent.[2] It forms a hydrate and many derivatives.
Likevanadium(III) fluoride, MnF3 features octahedral metal centers with the same average M-F bond distances. In the Mn compound, however, is distorted (and hence amonoclinic unit cell vs. a higher symmetry one) due to theJahn-Teller effect, with pairs of Mn-F distances of 1.79, 1.91, 2.09 Å.[5][6][7]
The hydrate MnF3.3H2O is obtained by crystallisation of MnF3 from hydrofluoric acid. The hydrate exists as two polymorphs, withspace groups P21/c and P21/a. Each consists of the salt [Mn(H2O)4F2]+[Mn(H2O)2F4]− ).[8]
MnF3 is Lewis acidic and forms a variety of derivatives. One example is K2MnF3(SO4).[9] MnF3 reacts withsodium fluoride to give the octahedral hexafluoride:[4]
3NaF + MnF3 → Na3MnF6
Related reactions salts of the anions MnF52− or MnF4−. These anions adopt chain and layer structures respectively, with bridging fluoride. Manganese remains 6 coordinate, octahedral, and trivalent in all of these materials.[4]
Manganese(III) fluoride fluorinates organic compounds including aromatic hydrocarbons,[10] cyclobutenes,[11] andfullerenes.[12]
^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.
^abcInorganic chemistry, Catherine E. Housecroft, A.G. Sharpe, pp.711-712, sectionManganese (III),googlebooks link
^M. A. Hepworth; K. H. Jack (1957). "The Crystal Structure of Manganese Trifluoride, MnF3".Acta Crystallographica.10 (5):345–351.doi:10.1107/S0365110X57001024.
^Molinier Michel; Massa Werner (1992). "Structures of two polymorphs of MnF3·3H2O".Journal of Fluorine Chemistry.57 (1–3):139–146.doi:10.1016/S0022-1139(00)82825-0.
^Junji Mizukado; Yasuhisa Matsukawa; Heng-dao Quan; Masanori Tamura; Akira Sekiya (2006). "Fluorination of Fluoro-Cyclobutene with High-Valency Metal Fluoride".Journal of Fluorine Chemistry.127:79–84.doi:10.1016/j.jfluchem.2005.10.007.
^V. É. Aleshina; A. Ya. Borshchevskii; E. V. Skokan; I. V. Arkhangel'skii; A.V. Astakhov; N.B. Shustova (2002). "Fluorination of the Cubic and Hexagonal C60 Modifications by Crystalline Manganese Trifluoride".Physics of the Solid State.44 (4):629–630.Bibcode:2002PhSS...44..629A.doi:10.1134/1.1470543.S2CID94250136.
^In situ time-resolved X-ray diffraction study of manganese trifluoride thermal decomposition, J.V. Raua, V. Rossi Albertinib, N.S. Chilingarova, S. Colonnab, U. Anselmi Tamburini, Journal of Fluorine Chemistry 4506 (2001) 1–4,online versionArchived 2017-12-30 at theWayback Machine
^Nachtigall, Olaf; Pataki, Astrid; Molski, Matthias; Lentz, Dieter; Spandl, Johann (2015). "Solvates of Manganese Trichloride Revisited - Synthesis, Isolation, and Crystal Structure of MnCl3(THF)3".Zeitschrift für Anorganische und Allgemeine Chemie.641 (6):1164–1168.doi:10.1002/zaac.201500106.
Knudsen Cell mass spectrometry study of Manganese Trifluoride vaporisation, High temperature corrosion and materials chemistry IV: proceedings of the International Symposium, pp. 521–525,google books
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