Potassium chlorochromate

In this article we will explore Potassium chlorochromate, a topic that has caught the attention of experts and enthusiasts alike. Potassium chlorochromate is a concept that has been the subject of debate and analysis in various fields, from science to popular culture. Throughout history, Potassium chlorochromate has played a crucial role in people's lives, influencing the way we think, act, and relate to the world around us. Through a multidisciplinary approach, we will examine the different perspectives on Potassium chlorochromate, highlighting its most relevant and controversial aspects. Additionally, we will explore how Potassium chlorochromate has evolved over time, and what its relevance is today. Get ready to enter the fascinating world of Potassium chlorochromate!

Potassium chlorochromate
Names
Other names
Potassium trioxochlorochromate,[1][2][3] Peligot's salt, Péligot's salt
Identifiers
3D model (JSmol)
ECHA InfoCard 100.036.506 Edit this at Wikidata
  • InChI=1S/ClH.Cr.K.3O/h1H;;;;;/q;;+1;;;/p-1
    Key: PEBPTQFCMJWPGZ-UHFFFAOYSA-M
  • O=(=O)=O..
Properties
KCrO3Cl
Molar mass 174,5472 g/mol
Appearance orange solid
Density 2.5228 g/cm3
Soluble[vague]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Highly toxic, corrosive, carcinogenic
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).

Potassium chlorochromate is an inorganic compound with the formula KCrO3Cl.[4] It is the potassium salt of chlorochromate, −. 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.

Structure and synthesis

Potassium 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

Although 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 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

Potassium 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

  1. ^ Synonyms Of Chemicals. Csudh.edu (2003-09-16). Retrieved on 2011-06-01.
  2. ^ Merck & Co (1930). Merck's index: an encyclopedia for the chemist, pharmacist and physician. Merck & Co. Retrieved 1 June 2011.
  3. ^ Arthur Rose; Elizabeth Rose (1966). The Condensed chemical dictionary. Reinhold. Retrieved 1 June 2011.
  4. ^ Norm Stanley Colorful Chromium Compounds, 23 August 2002
  5. ^ 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)
  6. ^ U. Kolitsch (2002). "Redetermination of potassium chlorochromate, KCrO3Cl". Acta Crystallogr. E58 (11): i105 – i107. doi:10.1107/S1600536802019396.
  7. ^ 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.
  8. ^ 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.
  9. ^ 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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