| 词条 | Manganese(II,III) oxide |
| 释义 |
| Watchedfields = changed | verifiedrevid = 436384774 | ImageFile = | ImageSize = | IUPACName = manganese(II) dimanganese(III) oxide | OtherNames = Manganese tetroxide; Manganese oxide, Manganomanganic oxide, Trimanganese tetraoxide, Trimanganese tetroxide[1] |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|CAS}} | CASNo = 1317-35-7 | PubChem = 14825 | RTECS = OP0895000 | SMILES = [Mn]=O.O=[Mn]O[Mn]=O | StdInChI = 1S/3Mn.4O | StdInChIKey = GVNFAUMGUISVJW-UHFFFAOYSA-N}} |Section2={{Chembox Properties | Formula = Mn3O4 MnO.Mn2O3 | MolarMass = 228.812 g/mol | Appearance = brownish-black powder[1] | Density = 4.86 g/cm3 | MeltingPtC = 1567 | BoilingPtC = 2847 | Solubility = insoluble | SolubleOther = soluble in HCl | MagSus = +12,400·10−6 cm3/mol |Section3={{Chembox Hazards | MainHazards = | FlashPt = | AutoignitionPt = | IDLH = N.D.[1] | PEL = C 5 mg/m3[1] | REL = None established[1] }} |Section4={{Chembox Thermochemistry | DeltaHf = −1387 kJ·mol−1[2] | Entropy = 149 J·mol−1·K−1[2] }} }} Manganese(II,III) oxide is the chemical compound with formula Mn3O4. Manganese is present in two oxidation states +2 and +3 and the formula is sometimes written as MnO.Mn2O3. Mn3O4 is found in nature as the mineral hausmannite. PreparationMn3O4 formed when any manganese oxide is heated in air above 1000 °C.[3] Considerable research has centred on producing nanocrystalline Mn3O4 and various syntheses that involve oxidation of MnII or reduction of MnVI.[4][5][6] ReactionsMn3O4 has been found to act as a catalyst for a range of reactions e.g. the oxidation of methane and carbon monoxide;[7][8] the decomposition of NO,[9] the reduction of nitrobenzene[10] and the catalytic combustion of organic compounds.[11] StructureMn3O4 has the spinel structure, where the oxide ions are cubic close packed and the MnII occupy tetrahedral sites and the MnIII octahedral sites.[3] The structure is distorted due to the Jahn–Teller effect.[3] At room temperature Mn3O4 is paramagnetic, below 41-43 K, it is ferrimagnetic[12] although this has been reported as reducing in nanocrystalline samples to around 39 K.[13] UsesMn3O4 is sometimes used as a starting material in the production of soft ferrites e.g. manganese zinc ferrite,[14] and lithium manganese oxide, used in lithium batteries.[15] Manganese tetraoxide can also be used as a weighting agent while drilling reservoir sections in oil and gas wells. References1. ^1 2 3 4 {{PGCH|0381}} {{Manganese compounds}}{{Oxides}}{{oxygen compounds}}2. ^1 {{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 0-618-94690-X|page=A22}} 3. ^1 2 {{Greenwood&Earnshaw}} 4. ^Hausmannite Mn3O4 nanorods: synthesis, characterization and magnetic properties Jin Du et al. Nanotechnology, (2006),17 4923-4928, {{doi| 10.1088/0957-4484/17/19/024}} 5. ^One-step synthesis of Mn3O4 nanoparticles: Structural and magnetic study Vázquez-Olmos A., Redón R, Rodríguez-Gattorno G., Mata-Zamora M.E., Morales-Leal F, Fernández-Osorio A.L, Saniger J.M. Journal of Colloid and Interface Science, 291, 1, (2005), 175-180 {{doi|10.1016/j.jcis.2005.05.005}} 6. ^Use of Carbonaceous Polysaccharide Microspheres as Templates for Fabricating Metal Oxide Hollow Spheres Xiaoming Sun, Junfeng Liu, Yadong Li, Chemistry - A European Journal,(2005), 12, 7, 2039 – 2047, {{doi|10.1002/chem.200500660}} 7. ^The reduction and oxidation behaviour of manganese oxides Stobhe E.R, de Boer A.D., Geus J.W., Catalysis Today. (1999), 47, 161–167. {{doi|10.1016/S0920-5861(98)00296-X}} 8. ^An in situ XRD investigation of singly and doubly promoted manganese oxide methane coupling catalysts.Moggridge G.D, Rayment T, Lambert R.M. Journal of Catalysis, (1992), 134, 242–252, {{doi|10.1016/0021-9517(92)90225-7}} 9. ^NO Decomposition over Mn2O3 and Mn3O4. Yamashita T, Vannice A., Journal of Catalysis (1996),163, 158–168, {{doi|10.1006/jcat.1996.0315}} 10. ^Selective reduction of nitrobenzene to nitrosobenzene over different kinds of trimanganese tetroxide catalysts.Wang W.M., Yang Y.N., Zhang J.Y., Applied Catalysis A. (1995), 133, 1, 81–93 {{doi|10.1016/0926-860X(95)00186-7}} 11. ^Catalytic combustion of C3 hydrocarbons and oxygenates over Mn3O4. Baldi M, Finocchio E, Milella F, Busca G., Applied Catalysis B. (1998), 16, 1, 43–51, {{doi|10.1016/S0926-3373(97)00061-1}} 12. ^Magnetic Structure of Mn3O4 by Neutron Diffraction Boucher B., Buhl R., Perrin M., J. Appl. Phys. 42, 1615 (1971); {{doi|10.1063/1.1660364}} 13. ^Synthesis of superparamagnetic Mn3O4 nanocrystallites by ultrasonic irradiation I.K. Gopalakrishnan, N. Bagkar, R. Ganguly and S.K. Kulshreshtha Journal of Crystal Growth 280, 3-4, (2005), 436-441, {{doi|10.1016/j.jcrysgro.2005.03.060}} 14. ^Method of making manganese-zinc ferrite U.S Patent number: 4093688 (1978)Arthur Withop, Roger Emil Travagli 15. ^Process for preparing lithium manganese oxides,U.S Patent number: 6706443,(2004), Horst Krampitz, Gerhard Wohner 3 : Manganese compounds|Oxides|Mixed valence compounds |
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