Manganese oxalate

Manganese oxalate
Names
	Other names Manganese(II) oxalate, Manganese(2+) oxalate, Lindbergite
Identifiers
CAS Number	640-67-5 ;
3D model (JSmol)	Interactive image;
ChemSpider	62705;
ECHA InfoCard	100.010.335
EC Number	211-367-3;
PubChem CID	69499;
UNII	A8PK5I86G8 ;
CompTox Dashboard (EPA)	DTXSID90894218 ;
	InChI InChI=1S/C2H2O4.Mn/c3-1(4)2(5)6;/h(H,3,4)(H,5,6);/q;+2/p-2 Key: RGVLTEMOWXGQOS-UHFFFAOYSA-L;
	SMILES C(=O)(C(=O)[O-])[O-].[Mn+2];
Properties
Chemical formula	C2MnO4
Molar mass	142.956 g·mol−1
Appearance	Light pink crystals
Density	2.43
Solubility in water	insoluble
Solubility product (Ksp)	1.7×10−7
Hazards
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H302, H312
Precautionary statements	P264, P270, P280, P301+P312, P302+P352, P312, P322, P330, P363, P501
Related compounds
Related compounds	Magnesium oxalate; Strontium oxalate; Barium oxalate; Iron(II) oxalate; Iron(III) oxalate; Praseodymium oxalate
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Manganese oxalate is a chemical compound, a salt of manganese and oxalic acid with the chemical formula MnC
₂O
₄.^[2]^[3] The compound creates light pink crystals, does not dissolve in water, and forms crystalline hydrates.^[4] It occurs naturally as the mineral Lindbergite.^[5]

Synthesis

Exchange reaction between sodium oxalate and manganese chloride:

{\mathsf {MnCl_{2}+Na_{2}C_{2}O_{4}+2H_{2}O\ {\xrightarrow {}}\ MnC_{2}O_{4}\cdot 2H_{2}O\downarrow +2NaCl}}

Physical properties

Manganese oxalate forms light pink crystals.

It does not dissolve in water, p K_sp= 6.8.

Forms crystalline hydrates of the composition MnC₂O₄•n H₂O, where n = 2 and 3.^[6]

Crystalline hydrate of the composition MnC₂O₄•2H₂O forms light pink crystals of the orthorhombic system, space group P2₁2₁2₁, cell parameters a = 0.6262 nm, b = 1.3585 nm, c = 0.6091 nm, Z = 4, melts in its own crystallization water at 100°C.^[7]^[8]

Chemical properties

Decomposes on heating:

{\mathsf {MnC_{2}O_{4}\ {\xrightarrow {215^{o}C}}\ MnO+CO\uparrow +CO_{2}\uparrow }}

Application

Manganese oxalate is used as an auxiliary siccative.
Manganese oxalate precursor is used to synthesize single phase nanoparticles of various manganese oxides, such as MnO, Mn
₂O
₃, and Mn
₃O
₄.^[9]

References

^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
^ Lunge, Georg (1924). Lunge and Keane's Technical Methods of Chemical Analysis. 2d Ed., Edited by Charles A. Keane ...and P.C.L. Thorne. Gurney and Jackson. p. 61. Retrieved 5 August 2021.
^ Young, Philena Anne (1928). The Volumetric Determination of Vanadium and Chromium in Special Alloy Steels: Ceric Sulfate as a Volumetric Oxidizing Agent. Mack Printing Company. p. 74. Retrieved 5 August 2021.
^ Donkova, B.; Mehandjiev, D. (2004). "Mechanism of decomposition of manganese(II) oxalate dihydrate and manganese(II) oxalate trihydrate". Thermochimica Acta. 421 (1–2): 141–149. Bibcode:2004TcAc..421..141D. doi:10.1016/j.tca.2004.04.001. ISSN 0040-6031. Retrieved 5 August 2021.
^ Atencio, Daniel; Coutinho, José M.V.; Graeser, Stefan; Matioli, Paulo A.; Menezes Filho, Luiz A.D. (2004). "Lindbergite, a new Mn oxalate dihydrate from Boca Rica mine, Galiléia, Minas Gerais, Brazil, and other occurrences". American Mineralogist. 89 (7): 1087–1091. Bibcode:2004AmMin..89.1087A. doi:10.2138/am-2004-0721. ISSN 1945-3027. S2CID 100604132. Retrieved 1 December 2021.
^ Nedyalkova, Miroslava; Antonov, Vladislav (1 January 2018). "Manganese oxalates - structure-based Insights". Open Chemistry. 16 (1): 1176–1183. doi:10.1515/chem-2018-0123. ISSN 2391-5420. S2CID 104343447.
^ Puzan, Anna N.; Baumer, Vyacheslav N.; Lisovytskiy, Dmytro V.; Mateychenko, Pavel V. (1 April 2018). "Structure disordering and thermal decomposition of manganese oxalate dihydrate, MnC2O4·2H2O". Journal of Solid State Chemistry. 260: 87–94. Bibcode:2018JSSCh.260...87P. doi:10.1016/j.jssc.2018.01.022. ISSN 0022-4596. Retrieved 5 August 2021.
^ Donkova, Borjana; Avdeev, Georgi (1 August 2015). "Synthesis and decomposition mechanism of γ-MnC2O4·2H2O rods under non-isothermal and isothermal conditions". Journal of Thermal Analysis and Calorimetry. 121 (2): 567–577. doi:10.1007/s10973-015-4590-4. ISSN 1588-2926. S2CID 97032400. Retrieved 5 August 2021.
^ Ahmad, Tokeer; Ramanujachary, Kandalam V.; Lofland, Samuel E.; Ganguli, Ashok K. (24 November 2004). "Nanorods of manganese oxalate: a single source precursor to different manganese oxide nanoparticles (MnO, Mn2O3, Mn3O4)". Journal of Materials Chemistry. 14 (23): 3406–3410. doi:10.1039/B409010A. ISSN 1364-5501. Retrieved 5 August 2021.

[crc-1] John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.

[2] Lunge, Georg (1924). Lunge and Keane's Technical Methods of Chemical Analysis. 2d Ed., Edited by Charles A. Keane ...and P.C.L. Thorne. Gurney and Jackson. p. 61. Retrieved 5 August 2021.

[3] Young, Philena Anne (1928). The Volumetric Determination of Vanadium and Chromium in Special Alloy Steels: Ceric Sulfate as a Volumetric Oxidizing Agent. Mack Printing Company. p. 74. Retrieved 5 August 2021.

[4] Donkova, B.; Mehandjiev, D. (2004). "Mechanism of decomposition of manganese(II) oxalate dihydrate and manganese(II) oxalate trihydrate". Thermochimica Acta. 421 (1–2): 141–149. Bibcode:2004TcAc..421..141D. doi:10.1016/j.tca.2004.04.001. ISSN 0040-6031. Retrieved 5 August 2021.

[5] Atencio, Daniel; Coutinho, José M.V.; Graeser, Stefan; Matioli, Paulo A.; Menezes Filho, Luiz A.D. (2004). "Lindbergite, a new Mn oxalate dihydrate from Boca Rica mine, Galiléia, Minas Gerais, Brazil, and other occurrences". American Mineralogist. 89 (7): 1087–1091. Bibcode:2004AmMin..89.1087A. doi:10.2138/am-2004-0721. ISSN 1945-3027. S2CID 100604132. Retrieved 1 December 2021.

[6] Nedyalkova, Miroslava; Antonov, Vladislav (1 January 2018). "Manganese oxalates - structure-based Insights". Open Chemistry. 16 (1): 1176–1183. doi:10.1515/chem-2018-0123. ISSN 2391-5420. S2CID 104343447.

[7] Puzan, Anna N.; Baumer, Vyacheslav N.; Lisovytskiy, Dmytro V.; Mateychenko, Pavel V. (1 April 2018). "Structure disordering and thermal decomposition of manganese oxalate dihydrate, MnC2O4·2H2O". Journal of Solid State Chemistry. 260: 87–94. Bibcode:2018JSSCh.260...87P. doi:10.1016/j.jssc.2018.01.022. ISSN 0022-4596. Retrieved 5 August 2021.

[8] Donkova, Borjana; Avdeev, Georgi (1 August 2015). "Synthesis and decomposition mechanism of γ-MnC2O4·2H2O rods under non-isothermal and isothermal conditions". Journal of Thermal Analysis and Calorimetry. 121 (2): 567–577. doi:10.1007/s10973-015-4590-4. ISSN 1588-2926. S2CID 97032400. Retrieved 5 August 2021.

[9] Ahmad, Tokeer; Ramanujachary, Kandalam V.; Lofland, Samuel E.; Ganguli, Ashok K. (24 November 2004). "Nanorods of manganese oxalate: a single source precursor to different manganese oxide nanoparticles (MnO, Mn2O3, Mn3O4)". Journal of Materials Chemistry. 14 (23): 3406–3410. doi:10.1039/B409010A. ISSN 1364-5501. Retrieved 5 August 2021.

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v t e Manganese compounds
Manganese(−I)	MnH(CO)₅
Manganese(0)	Mn₂(CO)₁₀
Manganese(I)	(C₅H₄CH₃)Mn(CO)₃ Mn(CO)₅Br Na₅Mn(CN)₆
Manganese(II)	MnC₂O₄ MnO Mn₃(PO₄)₂ MnS MnSe MnTe Mn(NO₃)₂ MnCO₃ MnCl₂ MnSO₄ MnF₂ MnBr₂ MnI₂ MnTiO₃ MnMoO₄ Mn(CH₃COO)₂ Mn(OH)₂ MnSe₂ Mn(ClO₃)₂ Mn(ClO₄)₂ Mn(C₅H₅)₂ Mn(C₃H₅O₃)₂ C ₂₄H ₄₈MnO ₄ C ₃₆H ₇₀MnO ₄
Manganese(II,III)	Mn₃O₄
Manganese(II,IV)	Mn₅O₈
Manganese(III)	MnCl₃ Mn₂O₃ MnF₃ K₆Mn₂O₆ MnAs MnPO₄ Mn(CH₃COO)₃
Manganese(IV)	MnS₂ MnCl₄ MnO₂ MnF₄ MnSi MnGe
Manganese(V)	K₃MnO₄ MnF₅ (predicted)
Manganese(VI)	H₂MnO₄ MnO₃ Na₂MnO₄ K₂MnO₄ BaMnO₄ MnO₂F₂ (predicted)
Manganese(VII)	Mn₂O₇ KMnO₄ MnO₃F

Synthesis

Physical properties

Chemical properties

Application

See also

References