Potassium chlorochromate is an inorganic compound with the formula KCrO3Cl.[4] It is the potassium salt of chlorochromate, [CrO3Cl]−. It is a water-soluble orange compound is used occasionally for oxidation of organic compounds. It is sometimes called Péligot's salt, in recognition of its discoverer Eugène-Melchior Péligot.
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3D model (JSmol)
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| ECHA InfoCard | 100.036.506 |
PubChem CID
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| Properties | |
| KCrO3Cl | |
| Molar mass | 174,5472 g/mol |
| Appearance | orange solid |
| Density | 2.5228 g/cm3 |
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Main hazards
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Highly toxic, corrosive, carcinogenic |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Structure and synthesis
editPotassium chlorochromate was originally prepared by treating potassium dichromate with hydrochloric acid. An improved route involves the reaction of chromyl chloride and potassium chromate:[5]
- K2CrO4 + CrO2Cl2 → 2KCrO3Cl
The salt consists of the tetrahedral chlorochromate anion. The average Cr=O bond length is 159 pm, and the Cr-Cl distance is 219 pm.[6]
Reactions
editAlthough air-stable, its aqueous solutions undergo hydrolysis in the presence of strong acids. With concentrated hydrochloric acid, it converts to chromyl chloride, which in turn reacts with water to form chromic acid and additional hydrochloric acid. When treated with 18-crown-6, it forms the lipophilic salt [K(18-crown-6)]CrO3Cl.[7]
Peligot's salt can oxidize benzyl alcohol, a reaction which can be catalyzed by acid.[8] A related salt, pyridinium chlorochromate, is more commonly used for this reaction.
Safety
editPotassium chlorochromate is toxic upon ingestion, and may cause irritation, chemical burns, and even ulceration on contact with the skin or eyes. .[9] Like other hexavalent chromium compounds, it is also carcinogenic and mutagenic.
References
edit- ^ Synonyms Of Chemicals. Csudh.edu (2003-09-16). Retrieved on 2011-06-01.
- ^ Merck & Co (1930). Merck's index: an encyclopedia for the chemist, pharmacist and physician. Merck & Co. Retrieved 1 June 2011.
- ^ Arthur Rose; Elizabeth Rose (1966). The Condensed chemical dictionary. Reinhold. Retrieved 1 June 2011.
- ^ Norm Stanley Colorful Chromium Compounds, 23 August 2002
- ^ Harry H. Sisler; Louis E. Marchi (2007). "Potassium Monochlorochromate". Inorganic Syntheses. Vol. 2. pp. 208–210. doi:10.1002/9780470132333.ch64. ISBN 9780470132333.
{{cite book}}:|journal=ignored (help) - ^ U. Kolitsch (2002). "Redetermination of potassium chlorochromate, KCrO3Cl". Acta Crystallogr. E58 (11): i105–i107. doi:10.1107/S1600536802019396.
- ^ Kotlyar, Sergei A.; Zubatyuk, Roman I.; Shishkin, Oleg V.; Chuprin, Gennady N.; Kiriyak, Andrey V.; Kamalov, Gerbert L. (2005). "(18-Crown-6)potassium chlorochromate". Acta Crystallographica E. 61 (2): m293–m295. doi:10.1107/S1600536805000085.
- ^ Özgün, B.; Pek, A. (1991). "Kinetics and mechanism of the oxidation of benzyl alcohol by potassium chlorochromate". Reaction Kinetics & Catalysis Letters. 43 (2): 589–594. doi:10.1007/BF02064733. S2CID 98721175.
- ^ Susan Shaw; Susan D. Shaw; Monona Rossol (1 September 1991). Overexposure: health hazards in photography. Allworth Communications, Inc. pp. 122–. ISBN 978-0-9607118-6-4. Retrieved 1 June 2011.
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