lithium oxalate
{{Chembox
| ImageFile = Lithium oxalate.svg
| ImageSize = 200px
| ImageAlt =
| IUPACName = Lithium oxalate
| OtherNames = {{ubl|Dilithium oxalate|di-Lithium oxalate{{cite web |title=553-91-3 {{!}} Sigma-Aldrich |url=https://www.sigmaaldrich.com/RU/ru/search/553-91-3?focus=products&page=1&perPage=30&sort=relevance&term=553-91-3&type=cas_number |publisher=Sigma Aldrich |access-date=15 June 2021}}|Oxalic acid dilithium salt{{cite web |title=di-Lithium oxalate |url=https://www.merckmillipore.com/RU/ru/product/di-Lithium-oxalate,MDA_CHEM-822085?ReferrerURL=https%3A%2F%2Fwww.google.ru%2F |publisher=Merck Millipore |access-date=15 June 2021}}}}
|Section1={{Chembox Identifiers
| CASNo = 553-91-3
| CASNo_Ref = {{cascite|correct|CAS}}
| ChemSpiderID = 61669
| UNII_Ref = {{fdacite|changed|FDA}}
| UNII = K737OT0E73
| EINECS = 209-054-1
| PubChem = 68383
| SMILES = [Li+].[Li+].[O-]C(=O)C([O-])=O
| StdInChI = 1S/C2H2O4-C.2Li/c3-1(4)2(5)6;;/h(H,3,4)(H,5,6);;/q;2*+1/p-2
| StdInChIKey = YNQRWVCLAIUHHI-UHFFFAOYSA-L
}}
|Section2={{Chembox Properties
| Formula = {{chem2|Li2C2O4}}
| Li=2|C=2|O=4
| Appearance = Colorless crystalline solid
| Density = 2.12 g/cm3
| MeltingPtC =
| BoilingPtC =
| Solubility = 6.6 g per 100 g of water}}
|Section7={{Chembox Hazards
| MainHazards =
| GHSPictograms = {{GHS07}}
| GHSSignalWord = WARNING
| HPhrases = {{H-phrases|302|312}}
| PPhrases = {{P-phrases|264|270|280|301+312|302+352|312|322|330|363|501}}
| FlashPtC =
| AutoignitionPt = }}
|Section9={{Chembox Related
| OtherCompounds = {{ubl|Sodium oxalate|Potassium oxalate|Beryllium oxalate|Magnesium oxalate|Calcium oxalate|Strontium oxalate|Barium oxalate}}
}}
}}
Lithium oxalate is an organic compound with the chemical formula {{chem2|Li2C2O4}}. It is a salt of lithium metal and oxalic acid.{{cite journal |last1=Beagley |first1=B. |last2=Small |first2=R. W. H. |title=The structure of lithium oxalate |url=https://scripts.iucr.org/cgi-bin/paper?a04249 |journal=Acta Crystallographica |access-date=15 June 2021 |pages=783–788 |language=en |doi=10.1107/S0365110X64002079 |date=1964-06-10|volume=17 |issue=6 |doi-access=free}}{{cite journal |last1=Solchenbach |first1=Sophie |last2=Wetjen |first2=Morten |last3=Pritzl |first3=Daniel |last4=Schwenke |first4=K. Uta |last5=Gasteiger |first5=Hubert A. |title=Lithium Oxalate as Capacity and Cycle-Life Enhancer in LNMO/Graphite and LNMO/SiG Full Cells |journal=Journal of the Electrochemical Society |pages=A512–A524 |language=en |doi=10.1149/2.0611803jes |date=2018|volume=165 |issue=3 |s2cid=104199908 |doi-access=free}} It consists of lithium cations {{chem2|Li+}} and oxalate anions {{chem2|C2O4(2−)}}. Lithium oxalate is soluble in water and converts to lithium oxide when heated.{{cite web |title=Lithium Oxalate |url=https://www.emdmillipore.com/CA/en/product/di-Lithium-oxalate,MDA_CHEM-822085 |publisher=Millipore-Sigma |access-date=10 Feb 2022 |language=en}}
Synthesis
One of the methods of synthesis is the reaction of direct neutralization of oxalic acid with lithium hydroxide:
:{{chem2|2 LiOH + H2C2O4 → Li2C2O4 + 2 H2O}}
Properties
The compound crystallizes in the monoclinic system, cell parameters a = 3.400 Å, b = 5.156 Å, c = 9.055 Å, β = 95.60°, Z = 4.
Lithium oxalate decomposes when heated at {{cvt|410-500|C|F K}}:
:{{chem2|Li2C2O4 → Li2CO3 + CO}}
Applications
In pyrotechnics, the compound is used to color the flame red.{{cite conference |last1=Koch |first1=Ernst-Christian |title=Is it possible to Obtain a Deep Red Pyrotechnic Flame Based on Lithium? |url=https://www.researchgate.net/publication/268211790 |access-date=15 June 2021 |doi=10.13140/2.1.1657.0567 |date=2009|conference= 36th International Pyrotechnics Seminar}}
References
{{Reflist}}
{{Lithium compounds}}
{{Oxalates}}