過マンガン酸、(化合物)過マンガン酸塩　　

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a dark purple salt of permanganic acid; in water solution it is used as a disinfectant and antiseptic

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過マンガン酸塩

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2016/05/10 01:46:35」(JST)

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A permanganate is the general name for a chemical compound containing the manganate(VII) ion, (MnO−
4). Because manganese is in the +7 oxidation state, the permanganate(VII) ion is a strong oxidizing agent. The ion has tetrahedral geometry.^[1] Permanganate solutions are purple in color and are stable in neutral or slightly alkaline media. The exact chemical reaction is dependent upon the organic contaminants present and the oxidant utilized. For example, trichloroethene (C₂HCl₃) is oxidized by sodium permanganate to form carbon dioxide (CO₂), manganese dioxide (MnO₂), sodium ions (Na⁺), hydronium ions (H⁺), and chloride ions (Cl⁻).^[2]

In an acidic solution, permanganate(VII) is reduced to the colourless +2 oxidation state of the manganese(II) (Mn²⁺) ion.

8 H+
+ MnO−
4 + 5 e⁻ → Mn²⁺ + 4 H₂O

In a strongly basic solution, permanganate(VII) is reduced to the green +6 oxidation state of the manganate ion, MnO2−
4.

MnO−
4 + e⁻ → MnO2−
4

In a neutral medium, however, it gets reduced to the brown +4 oxidation state of manganese dioxide MnO₂.

2 H₂O + MnO−
4 + 3 e⁻ → MnO₂ + 4 OH⁻

Production

Permanganates can be produced by oxidation of manganese compounds such as manganese chloride or manganese sulfate by strong oxidizing agents, for instance, sodium hypochlorite or lead dioxide:

2 MnCl₂ + 5 NaClO + 6 NaOH → 2 NaMnO₄ + 9 NaCl + 3 H₂O

2 MnSO₄ + 5 PbO₂ + 3 H₂SO₄ → 2 HMnO₄ + 5 PbSO₄ + 2 H₂O

It may also be produced by the disproportionation of manganates, with manganese dioxide as a side-product:

3 Na₂MnO₄ + 2 H₂O → 2 NaMnO₄ + MnO₂ + 4 NaOH

They are produced commercially by electrolysis or air oxidation of alkaline solutions of manganate salts (MnO2−
4).^[3]

A series of potassium permanganate solutions with varying concentration, increasing to the right.

Properties

Absorption spectrum of an aqueous solution of potassium permanganate, showing a vibronic progression

Permanganates(VII) are salts of permanganic acid. They have a deep purple colour, due to a charge transfer transition. Permanganate(VII) is a strong oxidizer, and similar to perchlorate. It is therefore in common use in qualitative analysis that involves redox reactions (permanganometry). According to theory, permanganate is strong enough to oxidize water, but this doesn't actually happen to any extent. Besides this, it is stable.

It is a useful reagent, though with organic compounds, not very selective.

Manganates(VII) are not very stable thermally. For instance, potassium permanganate decomposes at 230 °C to potassium manganate and manganese dioxide, releasing oxygen gas:

2 KMnO₄ → K₂MnO₄ + MnO₂ + O₂

A permanganate can oxidize an amine to a nitro compound,^[4]^[5] an alcohol to a ketone,^[6] an aldehyde to a carboxylic acid,^[7]^[8] a terminal alkene to a carboxylic acid,^[9] oxalic acid to carbon dioxide,^[10] and an alkene to a diol.^[11] This list is not exhaustive.

In alkene oxidations one intermediate is a cyclic Mn(V) species:

Compounds

Ammonium permanganate, NH₄MnO₄
Calcium permanganate, Ca(MnO₄)₂
Potassium permanganate, KMnO₄
Sodium permanganate, NaMnO₄
Silver permanganate, AgMnO₄

References

^ Sukalyan Dash, Sabita Patel and Bijay K. Mishra (2009). "Oxidation by permanganate: synthetic and mechanistic aspects". Tetrahedron 65 (4): 707–739. doi:10.1016/j.tet.2008.10.038.
^ http://geocleanse.com/permanaganate.asp
^ Cotton, F. Albert; Wilkinson, Geoffrey; Carlos A. Murillo; Manfred Bochmann (1999). Advanced Inorganic Chemistry (6th ed.). New York: John Wiley & Sons, Inc. p. 770. ISBN 978-0471199571.
^ A. Calder, A. R. Forrester1, and S. P. Hepburn (1972). "2-methyl-2-nitrosopropane and its dimer". Org. Synth. 6: 803. ; Coll. Vol. 52, p. 77
^ Nathan Kornblum and Willard J. Jones (1963). "4-nitro-2,2,4-trimethylpentane". Org. Synth. 5: 845. ; Coll. Vol. 43, p. 87
^ J. W. Cornforth (1951). "Ethyl pyruvate". Org. Synth. 4: 467. ; Coll. Vol. 31, p. 59
^ R. L. Shriner and E. C. Kleiderer (1930). "Piperonylic acid". Org. Synth. 2: 538. ; Coll. Vol. 10, p. 82
^ John R. Ruhoff (1936). "n-heptanoic acid". Org. Synth. 2: 315. ; Coll. Vol. 16, p. 39
^ Donald G. Lee, Shannon E. Lamb, and Victor S. Chang (1981). "Carboxylic acids from the oxidation of terminal alkenes by permanganate: nonadecanoic acid". Org. Synth. 7: 397. ; Coll. Vol. 60, p. 11
^ Kovacs KA, Grof P, Burai L, Riedel M (2004). "Revising the Mechanism of the Permanganate/Oxalate Reaction". J. Phys. Chem. A 108 (50): 11026. doi:10.1021/jp047061u.
^ E. J. Witzemann, Wm. Lloyd Evans, Henry Hass, and E. F. Schroeder (1931). "dl-glyceraldehyde ethyl acetal". Org. Synth. 2: 307. ; Coll. Vol. 11, p. 52

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English Journal

Mathematical simulation of chlorinated ethene concentration rebound after in situ chemical oxidation.

Tressler A1, Uchrin C.
Journal of environmental science and health. Part A, Toxic/hazardous substances & environmental engineering.J Environ Sci Health A Tox Hazard Subst Environ Eng.2014 Jul 3;49(8):869-81. doi: 10.1080/10934529.2014.893790.
Permanganates have been used for in situ chemical oxidation (ISCO) projects since the 1990s. Unfortunately, there has been very little research performed on the phenomenon of concentration rebound after ISCO. Most research on ISCO has focused on demonstrating effectiveness, estimating kinetics, or q
PMID 24766588

Spatial and seasonal characteristics of river water chemistry in the Taizi River in Northeast China.

Bu H1, Meng W, Zhang Y.
Environmental monitoring and assessment.Environ Monit Assess.2014 Jun;186(6):3619-32. doi: 10.1007/s10661-014-3644-6. Epub 2014 Jan 30.
Anthropogenic activities have led to water quality deterioration in many parts of the world, especially in Northeast China. The current work investigated the spatiotemporal variations of water quality in the Taizi River by multivariate statistical analysis of data from the 67 sampling sites in the m
PMID 24477615

Modification of cyanobacterial bloom-derived biomass using potassium permanganate enhanced the removal of microcystins and adsorption capacity toward cadmium (II).

Shao J1, Gu JD2, Peng L3, Luo S3, Luo H3, Yan Z4, Wu G5.
Journal of hazardous materials.J Hazard Mater.2014 May 15;272:83-8. doi: 10.1016/j.jhazmat.2014.03.013. Epub 2014 Mar 18.
Cyanobacterial biomass shows high adsorption capacity toward heavy metal ions. However, the cyanotoxins in the cyanobacterial biomass inhibit its application in heavy metals removal. In order to safely and effectively remove Cd(II) from water using cyanobacterial bloom-derived biomass (CBDB), KMnO4
PMID 24681589

Japanese Journal

ケナフを材料とした弱酸性型陽イオン交換体の合成とその銅（II）及び白金族金属イオン吸着特性

分析化学 65(1), 33-38, 2016
NAID 130005124378

酸性過マンガン酸エッチングによるプラスチックめっきプロセス (小特集 REACH規制とSVHC(高懸念物質)リスト)

表面技術 = Journal of the Surface Finishing Society of Japan 66(5), 201-204, 2015-05
NAID 40020472958

Highly Sensitive Determination of Ethylenediaminetetraacetic Acid Using a Permanganate Chemiluminescence System Catalyzed by Gold Nanoparticles

Analytical Sciences 31(8), 751-756, 2015
NAID 130005092115

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リンク元	「過マンガン酸」「過マンガン酸塩」
拡張検索	「potassium permanganate」

「過マンガン酸」

Permanganate
Names
	Systematic IUPAC name Permanganate
Properties
Chemical formula	MnO−; 4
Molar mass	118.93 g·mol−1
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	Infobox references