Zinc perchlorate
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| ImageFile = Zinc(II) perchlorate.svg
| ImageSize = 150px
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| ImageFile1 = Zinc perchlorate hexahydrate.jpg
| ImageSize1 = 150px
| ImageName1 = Zinc perchlorate hexahydrate
| PIN =
| OtherNames = Zinc diperchlorate, zinc(II) perchlorate
|Section1={{Chembox Identifiers
| CASNo = 13637-61-1
| CASNo_Ref = {{cascite|correct|CAS}}
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| ChemSpiderID = 8374666
| DTXSID = 50890711
| EC_number = 237-122-0
| PubChem = 10199167
| UNII = 725JL07841
| StdInChI=1S/2ClHO4.Zn/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2
| StdInChIKey = RXBXBWBHKPGHIB-UHFFFAOYSA-L
| SMILES = [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Zn+2]
}}
|Section2={{Chembox Properties
| Formula = {{chem|Cl|2|O|8|Zn}}
| MolarMass = 261.826
| Appearance = colorless solid
| Density = 2.252 g/cm3
| MeltingPtC = 106
| BoilingPtC = 210
| Solubility = soluble}}
|Section3={{Chembox Hazards
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|Section6={{Chembox Related
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Zinc perchlorate is the inorganic compound with the chemical formula Zn(ClO4)2 which forms the hexahydrate.{{cite journal |last1=Kumar |first1=Raj |last2=Thilagavathi |first2=Ramasamy |last3=Gulhane |first3=Rajesh |last4=Chakraborti |first4=Asit K. |title=Zinc(II) perchlorate as a new and highly efficient catalyst for formation of aldehyde 1,1-diacetate at room temperature and under solvent-free conditions |journal=Journal of Molecular Catalysis A: Chemical |date=2 May 2006 |volume=250 |issue=1 |pages=226–231 |doi=10.1016/j.molcata.2006.01.063 |url=https://www.sciencedirect.com/science/article/abs/pii/S1381116906005164 |access-date=14 March 2023 |language=en |issn=1381-1169|url-access=subscription }}{{cite book |title=Advances in Inorganic Chemistry |date=5 December 1984 |publisher=Academic Press |isbn=978-0-08-057877-4 |page=283 |url=https://books.google.com/books?id=U-YOlLVuV1YC&dq=zinc(II)+Perchlorate&pg=PA283 |access-date=14 March 2023 |language=en}}
Synthesis
Zinc perchlorate can be prepared by dissolving zinc oxide or zinc carbonate in perchloric acid:{{cite journal |last1=Lin |first1=Lili |last2=Liu |first2=Xiaohua |last3=Feng |first3=Xiaoming |title=Zinc(II) Perchlorate Hexahydrate |journal=Encyclopedia of Reagents for Organic Synthesis |date=27 May 2014 |pages=1–5 |doi=10.1002/047084289X.rn01657 |isbn=9780470842898 |access-date=14 March 2023|url=https://onlinelibrary.wiley.com/doi/abs/10.1002/047084289X.rn01657|url-access=subscription }}
:{{chem2 | ZnO + 2 HClO4 -> Zn(ClO4)2 + H2O }}
:{{chem2 | ZnCO3 + 2 HClO4 -> Zn(ClO4)2 + H2O + CO2 }}
Chemical properties
The compound decomposes when heated to high temperatures and may explode if heated too strongly.
Like most other perchlorates such as copper perchlorate and lead perchlorate, zinc perchlorate is prone to deliquescence.
Zinc perchlorate can form complexes with ligands such as 8-aminoquinoline, tricarbohydrazide, and tetraphenylethylene tetratriazole.{{cite web |title=8-aminoquinoline zinc perchlorate metal complex, and preparation method and application thereof |url=https://patents.google.com/patent/CN103755633A/en |access-date=14 March 2023 |language=en |date=30 April 2014}}
Physical properties
The compound forms a hexahydrate {{chem|Zn|(|Cl|O|4|)|2}}·6{{chem|H|2|O}}.{{cite web |title=Zinc Perchlorate Hexahydrate |url=https://www.americanelements.com/zinc-perchlorate-hexahydrate-10025-64-6 |publisher=American Elements |access-date=14 March 2023 |language=en}}{{cite web |title=Zinc perchlorate hexahydrate |url=https://www.sigmaaldrich.com/RU/en/product/aldrich/401439 |publisher=Sigma Aldrich |access-date=14 March 2023}}
Zinc perchlorate forms a hygroscopic colorless solid, odorless, soluble in water and low-weight alcohols.
Uses
Zinc perchlorate is used as an oxidizing agent and catalyst.
References
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External links
{{Zinc compounds}}
{{Perchlorates}}