--- id: 752124b6-4522-4161-8f01-694c8f9fc10c title: 'Manganese(IV) Fluoride: Chemical Properties and Applications' abstract: This document provides a technical overview of Manganese(IV) fluoride, also known as manganese tetrafluoride. It details the compound's chemical identifiers, preparation methods, decomposition characteristics, and other chemical reactions. The content also covers its practical applications and the formation of fluromanganate(IV) complexes. classification: primary: '546' secondary: - '541' - '54' udc_main_class: '5' tags: - Manganese(IV) fluoride - Inorganic chemistry - Chemical compound - Fluoride - Manganese topics: - Chemistry - Inorganic Compounds - Natural Sciences author: '' created_at: '2026-06-01T00:24:25.478592' updated_at: '2026-06-01T02:12:58.434660' sources: - type: url uri: https://en.wikipedia.org/wiki/Manganese(IV)_fluoride format: url_fetch udc_label: Applied chemistry version: '1' --- ## Card: Manganese(IV) Fluoride: Chemical Properties and Applications This document provides a technical overview of Manganese(IV) fluoride, also known as manganese tetrafluoride. It details the compound's chemical identifiers, preparation methods, decomposition characteristics, and other chemical reactions. The content also covers its practical applications and the formation of fluromanganate(IV) complexes. ## Classification Primary: 546 | Secondary: 541, 54 | Tags: Manganese(IV) fluoride, Inorganic chemistry, Chemical compound, Fluoride, Manganese | Topics: Chemistry, Inorganic Compounds, Natural Sciences ## Content Manganese(IV) fluoride - Wikipedia Jump to content Main menu Main menu move to sidebar hide Navigation Main page Contents Current events Random article About Wikipedia Contact us Contribute Help Learn to edit Community portal Recent changes Upload file Special pages Search Search Appearance Donate Create account Log in Personal tools Donate Create account Log in Contents move to sidebar hide (Top) 1 Preparation 2 Chemistry Toggle Chemistry subsection 2.1 Decomposition 2.2 Other reactions 3 Applications 4 Fluoromanganate(IV) complexes 5 Notes and references Toggle Notes and references subsection 5.1 Notes 5.2 References 5.3 Further reading Toggle the table of contents Manganese(IV) fluoride 16 languages العربية تۆرکجه Čeština Deutsch Español فارسی हिन्दी Português Русский Srpskohrvatski / српскохрватски Simple English Српски / srpski தமிழ் اردو Tiếng Việt 中文 Edit links Article Talk English Read Edit View history Tools Tools move to sidebar hide Actions Read Edit View history General What links here Related changes Upload file Permanent link Page information Cite this page Get shortened URL Print/export Download as PDF Printable version In other projects Wikimedia Commons Wikidata item Appearance move to sidebar hide From Wikipedia, the free encyclopedia Manganese(IV) fluoride Names IUPAC name manganese tetrafluoride Other names manganese(IV) fluoride Identifiers CAS Number 15195-58-1 3D model ( JSmol ) Interactive image ChemSpider 14941034 ECHA InfoCard 100.356.905 PubChem CID 10129971 CompTox Dashboard ( EPA ) DTXSID101045561 InChI InChI=1S/4FH.Mn/ h4*1H;/q;;;;+4/p-4 Key: KWKYNMDHPVYLQQ-UHFFFAOYSA-J InChI=1/4FH.Mn/h4*1H;/q;;;;+4/p-4 Key: KWKYNMDHPVYLQQ-XBHQNQODAK SMILES [F-].[F-].[F-].[F-].[Mn+4] Properties [ 2 ] [ 3 ] Chemical formula MnF 4   Molar mass 130.93 g mol −1     Appearance blue solid Density 3.61 g cm −3 (calc.) [ 1 ] Melting point 70 °C (158 °F; 343 K) decomposes Solubility in water reacts violently Structure Crystal structure tetragonal , tI80 [ 1 ] [ 4 ] Space group I4 1 / a (No. 88) [ Note 1 ] Lattice constant a  = 1263 pm, c  = 604.9 pm Related compounds Other cations Manganese(II) fluoride Manganese(III) fluoride Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references Chemical compound Manganese tetrafluoride , MnF 4 , is the highest fluoride of manganese . It is a powerful oxidizing agent and is used as a means of purifying elemental fluorine . [ 3 ] [ 6 ] Preparation [ edit ] Manganese tetrafluoride was first unequivocally prepared in 1961 [ Note 2 ] by the reaction of manganese(II) fluoride (or other Mn II compounds) with a stream of fluorine gas at 550 °C: the MnF 4 sublimes into the gas stream and condenses onto a cold finger . [ 2 ] [ 8 ] This is still the commonest method of preparation, although the sublimation can be avoided by operating at increased fluorine pressure (4.5–6 bar at 180–320 °C) and mechanically agitating the powder to avoid sintering of the grains. [ 3 ] [ 9 ] The reaction can also be carried out starting from manganese powder in a fluidized bed . [ 10 ] [ 11 ] Other preparations of MnF 4 include the fluorination of MnF 2 with krypton difluoride , [ 12 ] or with F 2 in liquid hydrogen fluoride solution under ultraviolet light . [ 13 ] Manganese tetrafluoride has also been prepared (but not isolated) in an acid–base reaction between antimony pentafluoride and K 2 MnF 6 as part of a chemical synthesis of elemental fluorine. [ 14 ] K 2 MnF 6 + 2 SbF 5 → MnF 4 + 2 KSbF 6 Chemistry [ edit ] Decomposition [ edit ] Manganese tetrafluoride is in equilibrium with manganese(III) fluoride and elemental fluorine : MnF 4 ⇌ MnF 3 + ⁠ 1 / 2 ⁠ F 2 Decomposition is favoured by increasing temperature, and disfavoured by the presence of fluorine gas, but the exact parameters of the equilibrium are unclear, with some sources saying that MnF 4 will decompose slowly at room temperature, [ 15 ] [ 16 ] others placing a practical lower temperature limit of 70 °C, [ 3 ] [ 17 ] and another claiming that MnF 4 is essentially stable up to 320 °C. [ 18 ] The equilibrium pressure of fluorine above MnF 4 at room temperature has been estimated at 10 −4  Pa (10 −9  bar), and the enthalpy change of reaction at +44(8) kJ mol −1 . [ 19 ] [ Note 3 ] Other reactions [ edit ] Manganese tetrafluoride reacts violently with water and even with sodium-dried petroleum ether . It immediately decomposes on contact with moist air. [ 2 ] Reaction with alkali metal fluorides or concentrated hydrofluoric acid gives the yellow hexafluoromanganate(IV) anion [MnF 6 ] 2− . [ 18 ] MnF 4 reacts with XeF 2 to form Lewis acid-base adducts : 3XeF 2 ∙2MnF 4 , XeF 2 ∙MnF 4 , and XeF 2 ∙2MnF 4 . [ 21 ] [ 22 ] A tetrameric F-bridged ring with XeF 2 molecules coordinated to metal atoms, observed in the crystal structure of XeF 2 ∙MnF 4 (XeMnF 6 ) adduct, could serve as a structural model for the currently unknown structure of the first noble-gas compound , XePtF 6 . [ 22 ] Applications [ edit ] The main application of manganese tetrafluoride is in the purification of elemental fluorine . Fluorine gas is produced by electrolysis of anhydrous hydrogen fluoride (with a small amount of potassium fluoride added as a support electrolyte) in a Moissan cell . The technical product is contaminated with HF, much of which can be removed by passing the gas over solid KF, but also with oxygen (from traces of water) and possibly heavy-metal fluorides such as arsenic pentafluoride (from contamination of the HF). These contaminants are particularly problematic for the semiconductor industry, which uses high-purity fluorine for etching silicon wafers. Further impurities, such as iron , nickel , gallium and tungsten compounds, can be introduced if unreacted fluorine is recycled. [ 6 ] The technical-grade fluorine is purified by reacting it with MnF 3 to form manganese tetrafluoride. As this stage, any heavy metals present will form involatile complex fluorides, while the HF and O 2 are unreactive. Once the MnF 3 has been converted, the excess gas is vented for recycling, carrying the remaining gaseous impurities with it. The MnF 4 is then heated to 380 °C to release fluorine at purities of up to 99.95%, reforming MnF 3 , which can be reused. [ 3 ] [ 6 ] By placing two reactors in parallel, the purification process can be made continuous, with one reactor taking in technical fluorine while the other delivers high-grade fluorine. [ 6 ] Alternatively, the manganese tetrafluoride can be isolated and transported to where the fluorine is needed, at lower cost and greater safety than pressurized fluorine gas. [ 3 ] [ 9 ] Fluoromanganate(IV) complexes [ edit ] The yellow hexafluoromanganate(2−) of alkali metal and alkaline earth metal cations have been known since 1899, and can be prepared by the fluorination of MnF 2 in the presence of the fluoride of the appropriate cation. [ 13 ] [ 23 ] [ 24 ] [ 25 ] They are much more stable than manganese tetrafluoride. [ 14 ] Potassium hexafluoromanganate(IV), K 2 MnF 6 , can also be prepared by the controlled reduction of potassium permanganate in 50% aqueous hydrofluoric acid . [ 26 ] [ 27 ] 2 KMnO 4 + 2 KF + 10 HF + 3 H 2 O 2 → 2 K 2 MnF 6 + 8 H 2 O + 3 O 2 The pentafluoromanganate(1−) salts of potassium , rubidium and caesium , MMnF 5 , can be prepared by fluorination of MMnF 3 or by the reaction of [MnF 4 (py)(H 2 O)] with MF. [ 25 ] [ 27 ] The lemon-yellow heptafluoromanganate(3−) salts of the same metals, M 3 MnF 7 , have also been prepared. [ 28 ] When potassium hexafluoromanganate is doped into potassium fluorosilicate it forms a narrow band red phosphor. [ 29 ] Notes and references [ edit ] Notes [ edit ] ^ The space group has also been given as R3 c (No. 161) or R 3 c (No. 167); a β-form crystallizes in the rhombohedral system. [ 1 ] [ 5 ] ^ Reports of the preparation of MnF 4 date back to the nineteenth century, [ 7 ] but are inconsistent with the now-known chemistry of the genuine compound. ^ These two results are inconsistent with one another, as Δ r H o would have to be about +80 kJ mol −1 for p eq (F 2 ) ≈ 10 −9  bar at 298 K, given that the overwhelming contribution to Δ r S o is S o (F 2 ) = 202.791(5) J K −1 mol −1 . [ 20 ] The quoted value of Δ r H o is consistent with most reported decomposition temperatures. References [ edit ] ^ a b c Müller, B. G.; Serafin, M. (1987), "Die Kristallstruktur von Mangantetrafluorid", Z. Naturforsch. B , 42 (9): 1102– 6, doi : 10.1515/znb-1987-0908 , S2CID   95703093 . ^ a b c Hoppe, Rudolf ; Dähne, Wolfgang; Klemm, Wilhelm (1961), "Mangantetrafluorid, MnF 4 ", Naturwissenschaften , 48 (11): 429, Bibcode : 1961NW.....48..429H , doi : 10.1007/BF00621676 , S2CID   30724467 . ^ a b c d e f WO patent 2006033480 , Torisu, Junichi; Oka, Masakazu & Kuznetsov, Andrey Sergeyevich et al., "Method of manufacturing manganese tetrafluoride", published 2006-03-30,  assigned to Astor Electronics  and Showa Denko   . ^ Edwards, A. J. (1983), "Solid-State Structures of the Binary Fluorides of the Transition Metals", Adv. Inorg. Chem. Radiochem. , Advances in Inorganic Chemistry, 27 : 83– 112, doi : 10.1016/S0898-8838(08)60105-1 , ISBN   9780120236275 {{ citation }} : CS1 maint: work parameter with ISBN ( link ) . ^ Kraus, Florian; Ivlev, Sergei I.; Bandemehr, Jascha; Sachs, Malte; Pietzonka, Clemens; Conrad, Matthias; Serafin, Michael; Müller, Bernd G. (2020-09-30). "Synthesis and Characterization of Manganese Tetrafluoride β-MnF 4 " . Zeitschrift für anorganische und allgemeine Chemie . 646 (18): 1481– 1489. doi : 10.1002/zaac.202000048 . ISSN   0044-2313 . ^ a b c d WO patent 2009074562 , Seseke-Koyro, Ulrich; Garcia-Juan, Placido & Palsherm, Stefan et al., "Process for the purification of elemental fluorine", published 2009-06-18,  assigned to Solvay Fluor   . ^ Melville, W. H. (1876), "Contribution towards the History of the Fluorides of Manganese" , Proc. Am. Acad. Arts Sci. , 12 : 228– 34, doi : 10.2307/25138452 , JSTOR   25138452 . ^ Hoppe, Rudolf ; Dähne, Wolfgang; Klemm, Wilhelm (1962), "Mangantetrafluorid mit einem Anhang über LiMnF 5 und LiMnF 4 ", Justus Liebigs Ann. Chem. , 658 (1): 1– 5, doi : 10.1002/jlac.19626580102 . ^ a b WO application 2009074560 , Seseke-Koyro, Ulrich; Garcia-Juan, Placido & Palsherm, Stefan et al., "Method for preparing manganese tetrafluoride", published 2009-06-18,  assigned to Solvay Fluor   . ^ Roesky, H.; Glemser, O. (1963), "A New Preparation of Manganese Tetrafluoride", Angew. Chem. Int. Ed. Engl. , 2 (10): 626, doi : 10.1002/anie.196306262 . ^ Roesky, Herbert W.; Glemser, Oskar; Hellberg, Karl-Heinz (1965), "Darstellung von Metallfluoriden in der Wirbelschicht", Chem. Ber. , 98 (6): 2046– 48, doi : 10.1002/cber.19650980642 . ^ Lutar, Karel; Jesih, Adolf; Žemva, Boris (1988), "KrF 2 /MnF 4 adducts from KrF 2 /MnF 2 interaction in HF as a route to high purity MnF 4 ", Polyhedron , 7 (13): 1217– 19, doi : 10.1016/S0277-5387(00)81212-7 . ^ a b Mazej, Z. (2002), "Room temperature syntheses of MnF 3 , MnF 4 and hexafluoromanganete(IV) salts of alkali cations", J. Fluorine Chem. , 114 (1): 75– 80, doi : 10.1016/S0022-1139(01)00566-8 . ^ a b Christe, Karl O. (1986), "Chemical synthesis of elemental fluorine", Inorg. Chem. , 25 (21): 3721– 24, doi : 10.1021/ic00241a001 . ^ Cotton, F. Albert ; Wilkinson, Geoffrey (1980), Advanced Inorganic Chemistry (4th ed.), New York: Wiley, p. 745, ISBN   0-471-02775-8 . ^ Housecroft, Catherine E.; Sharpe, Alan G. (2007), Inorganic Chemistry (3rd ed.), New York: Prentice Hall, p. 710, ISBN   978-0131755536 . ^ Rakov, E. G.; Khaustov, S. V.; Pomadchin, S. A. (1997), "Thermal Decomposition and Pyrohydrolysis of Manganese Tetrafluoride", Russ. J. Inorg. Chem. , 42 (11): 1646– 49 . ^ a b Adelhelm, M.; Jacob, E. (1991), "MnF 4 : preparation and properties", J. Fluorine Chem. , 54 ( 1– 3): 21, doi : 10.1016/S0022-1139(00)83531-9 . ^ Ehlert, T. C.; Hsia, M. (1972), "Mass spectrometric and thermochemical studies of the manganese fluorides", J. Fluorine Chem. , 2 (1): 33– 51, Bibcode : 1972JFluC...2...33E , doi : 10.1016/S0022-1139(00)83113-9 . ^ Cox, J. D.; Wagman, D. D.; Medvedev, V. A. (1989), CODATA Key Values for Thermodynamics , New York: Hemisphere, ISBN   0891167587 . ^ Žemva, B.; Zupan, J.; Slivnik, J. (1971). "On the XeMnF 6 synthesis" . Journal of Inorganic and Nuclear Chemistry . 33 (11): 3953– 3955. doi : 10.1016/0022-1902(71)80305-6 . ^ a b Motaln, Klemen; Gurung, Kshitij; Brázda, Petr; Kokalj, Anton; Radan, Kristian; Dragomir, Mirela; Žemva, Boris; Palatinus, Lukáš; Lozinšek, Matic (2024-09-25). "Reactive Noble-Gas Compounds Explored by 3D Electron Diffraction: XeF 2 –MnF 4 Adducts and a Facile Sample Handling Procedure" . ACS Central Science . 10 (9): 1733– 1741. doi : 10.1021/acscentsci.4c00815 . ISSN   2374-7943 . PMC   11428288 . PMID   39345812 . ^ Weinland, R. F.; Lauenstein, O. (1899), "Über Fluormanganite", Z. Anorg. Allg. Chem. , 20 : 40, doi : 10.1002/zaac.620200106 . ^ Hoppe, Rudolf; Blinne, Klaus (1957), "Hexafluoromanganate IV der Elemente Ba, Sr, Ca und Mg", Z. Anorg. Allg. Chem. , 291 ( 5– 6): 269– 75, Bibcode : 1957ZAACh.291..269H , doi : 10.1002/zaac.19572910507 . ^ a b Hoppe, Rudolf; Liebe, Werner; Dähne, Wolfgang (1961), "Über Fluoromanganate der Alkalimetalle", Z. Anorg. Allg. Chem. , 307 ( 5– 6): 276– 89, Bibcode : 1961ZAACh.307..276H , doi : 10.1002/zaac.19613070507 . ^ Bode, Hans; Jenssen, H.; Bandte, F. (1953), "Über eine neue Darstellung des Kalium-hexafluoromanganats(IV)", Angew. Chem. , 65 (11): 304, Bibcode : 1953AngCh..65..304B , doi : 10.1002/ange.19530651108 . ^ a b Chaudhuri, M. K.; Das, J. C.; Dasgupta, H. S. (1981), "Reactions of KMnO 4 —A novel method of preparation of pentafluoromanganate(IV)[MnF 5 ] − ", J. Inorg. Nucl. Chem. , 43 (1): 85– 87, doi : 10.1016/0022-1902(81)80440-X . ^ Hofmann, B.; Hoppe, R. (1979), "Zur Kenntnis des (NH 4 ) 3 SiF 7 -Typs. Neue Metallfluoride A 3 MF 7 mit M = Si, Ti, Cr, Mn, Ni und A = Rb, Cs", Z. Anorg. Allg. Chem. , 458 (1): 151– 62, Bibcode : 1979ZAACh.458..151H , doi : 10.1002/zaac.19794580121 . ^ Verstraete, Reinert; Sijbom, Heleen F.; Joos, Jonas J.; Korthout, Katleen; Poelman, Dirk; Detavernier, Christophe; Smet, Philippe F. (2018), "Red Mn4+-Doped Fluoride Phosphors: Why Purity Matters" (PDF) , ACS Applied Materials & Interfaces , 10 (22): 18845– 18856, Bibcode : 2018AAMI...1018845V , doi : 10.1021/acsami.8b01269 , PMID   29750494 Further reading [ edit ] Gubkina, N. I.; Sokolov, Sergey V.; Krylov, E. I. (1966), "Fluorides of High Oxidising Power and Their Application to the Preparation of Organic Fluorine Compounds", Russ. Chem. Rev. , 35 (12): 930– 41, Bibcode : 1966RuCRv..35..930G , doi : 10.1070/RC1966v035n12ABEH001550 , S2CID   250817326 . Hoppe, R.; Müller, B.; Burgess, J.; Peacock, R. D.; Sherry, R. (1980), "The enthalpy of formation of manganese tetrafluoride", J. Fluorine Chem. , 16 (2): 189– 91, Bibcode : 1980JFluC..16..189H , doi : 10.1016/S0022-1139(00)82393-3 . v t e Manganese compounds Manganese(−I) MnH(CO) 5 Manganese(0) Mn 2 (CO) 10 Manganese(I) (C 5 H 4 CH 3 )Mn(CO) 3 Mn(CO) 5 Br Na 5 Mn(CN) 6 Manganese(II) MnC 2 O 4 MnO Mn 3 (PO 4 ) 2 MnS MnSe MnTe Mn(NO 3 ) 2 MnCO 3 MnCl 2 MnSO 4 MnF 2 MnBr 2 MnI 2 MnTiO 3 MnMoO 4 Mn(CH 3 COO) 2 Mn(OH) 2 MnS 2 MnSe 2 Mn(ClO 3 ) 2 Mn(ClO 4 ) 2 Mn(C 5 H 5 ) 2 Mn(C 3 H 5 O 3 ) 2 C 24 H 48 MnO 4 C 36 H 70 MnO 4 Manganese(II,III) Mn 3 O 4 Manganese(II,IV) Mn 5 O 8 Manganese(III) MnB MnCl 3 Mn 2 O 3 MnF 3 K 6 Mn 2 O 6 MnAs MnPO 4 Mn(CH 3 COO) 3 Manganese(IV) MnCl 4 MnO 2 MnF 4 MnSi MnGe Manganese(V) K 3 MnO 4 MnF 5 (hypothetical) Manganese(VI) H 2 MnO 4 MnO 3 Na 2 MnO 4 K 2 MnO 4 BaMnO 4 MnO 2 F 2 (hypothetical) Manganese(VII) Mn 2 O 7 KMnO 4 MnO 3 F v t e Salts and covalent derivatives of the fluoride ion HF ? HeF 2 LiF BeF 2 BF BF 3 B 2 F 4 +BO 3 CF 4 C x F y +CO 3 +C 2 O 4 NF 3 FN 3 N 2 F 2 NF N 2 F 4 NF 2 ? NF 5 +N +NO 3 OF 2 O 2 F 2 OF O 3 F 2 O 4 F 2 ?OF 4 F 2 Ne NaF MgF 2 AlF AlF 3 SiF 4 P 2 F 4 PF 3 PF 5 +PO 4 +HPO 3 S 2 F 2 SF 2 S 2 F 4 SF 3 SF 4 S 2 F 10 SF 6 +SO 4 ClF ClF 3 ClF 5 ? ArF 2 ? ArF 4 KF CaF CaF 2 ScF 3 TiF 2 TiF 3 TiF 4 VF 2 VF 3 VF 4 VF 5 CrF 2 CrF 3 CrF 4 CrF 5 ? CrF 6 MnF 2 MnF 3 MnF 4 ? MnF 5 FeF 2 FeF 3 FeF 4 CoF 2 CoF 3 CoF 4 NiF 2 NiF 3 NiF 4 CuF CuF 2 ? CuF 3 ZnF 2 GaF 2 GaF 3 GeF 2 GeF 4 AsF 3 AsF 5 Se 2 F 2 SeF 4 SeF 6 +SeO 3 BrF BrF 3 BrF 5 KrF 2 ? KrF 4 ? KrF 6 RbF SrF SrF 2 YF 3 ZrF 2 ZrF 3 ZrF 4 NbF 4 NbF 5 MoF 4 MoF 5 MoF 6 TcF 4 TcF 5 TcF 6 RuF 3 RuF 4 RuF 5 RuF 6 RhF 3 RhF 4 RhF 5 RhF 6 PdF 2 Pd[PdF 6 ] PdF 4 ? PdF 6 Ag 2 F AgF AgF 2 AgF 3 CdF 2 InF InF 3 SnF 2 SnF 4 SbF 3 SbF 5 TeF 4 ? Te 2 F 10 TeF 6 +TeO 3 IF IF 3 IF 5 IF 7 +IO 3 XeF 2 XeF 4 XeF 6 ? XeF 8 CsF BaF 2   LuF 3 HfF 4 TaF 5 WF 4 WF 5 WF 6 ReF 4 ReF 5 ReF 6 ReF 7 OsF 4 OsF 5 OsF 6 ? OsF 7 ? OsF 8 IrF 2 IrF 3 IrF 4 IrF 5 IrF 6 PtF 2 Pt[PtF 6 ] PtF 4 PtF 5 PtF 6 AuF AuF 3 Au 2 F 10 ? AuF 6 AuF 5 •F 2 Hg 2 F 2 HgF 2 ? HgF 4 TlF TlF 3 PbF 2 PbF 4 BiF 3 BiF 5 PoF 2 PoF 4 PoF 6 AtF ? AtF 3 ? AtF 5 RnF 2 ? RnF 4 ? RnF 6 FrF RaF 2   LrF 3 Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og ↓ LaF 3 CeF 3 CeF 4 PrF 3 PrF 4 NdF 2 NdF 3 NdF 4 PmF 3 SmF SmF 2 SmF 3 EuF 2 EuF 3 GdF 3 TbF 3 TbF 4 DyF 2 DyF 3 DyF 4 HoF 3 ErF 3 TmF 2 TmF 3 YbF 2 YbF 3 AcF 3 ThF 2 ThF 3 ThF 4 PaF 4 PaF 5 UF 3 UF 4 UF 5 UF 6 NpF 3 NpF 4 NpF 5 NpF 6 PuF 3 PuF 4 PuF 5 PuF 6 AmF 2 AmF 3 AmF 4 ? AmF 6 CmF 3 CmF 4  ? CmF 6 BkF 3 BkF 4 CfF 3 CfF 4 EsF 3 EsF 4 ? EsF 6 Fm MdF 3 No Retrieved from " https://en.wikipedia.org/w/index.php?title=Manganese(IV)_fluoride&oldid=1337652230 " Categories : Manganese(IV) compounds Fluorides Metal halides Fluorinating agents Hidden categories: CS1 maint: work parameter with ISBN Articles without EBI source Articles without KEGG source Articles without UNII source ECHA InfoCard ID from Wikidata Articles containing unverified chemical infoboxes Articles with short description Short description matches Wikidata This page was last edited on 10 February 2026, at 18:34  (UTC) . Text is available under the Creative Commons Attribution-ShareAlike 4.0 License ; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy . Wikipedia® is a registered trademark of the Wikimedia Foundation, Inc. , a non-profit organization. Privacy policy About Wikipedia Disclaimers Contact Wikipedia Legal & safety contacts Code of Conduct Developers Statistics Cookie statement Mobile view Search Search Toggle the table of contents Manganese(IV) fluoride 16 languages Add topic ## Source - url: https://en.wikipedia.org/wiki/Manganese(IV)_fluoride