Mercury(I) chloride
From Wikipedia, the free encyclopedia
| Mercury(I) chloride | |
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| IUPAC name | Dimercury dichloride |
| Other names | Mercurous chloride; calomel |
| Identifiers | |
| CAS number | [10112-91-1] |
| RTECS number | OV8750000 |
| Properties | |
| Molecular formula | Hg2Cl2 |
| Molar mass | 472.09 g/mol |
| Appearance | White solid |
| Density | 7.150 g/cm3, solid |
| Melting point |
383 °C (sublimes) |
| Solubility in water | 0.2 mg/100 mL |
| Hazards | |
| Main hazards | Harmful, dangerous for the environment |
| R-phrases | R22, R36/37/38, R50/53 |
| S-phrases | (S2), S13, S24/25 S46, S60, S61 |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions | Mercury(I) bromide, mercury(I) iodide |
| Other cations | Mercury(II) chloride |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Mercury(I) chloride is the chemical compound with the formula Hg2Cl2. Also known as calomel or mercurous chloride, this dense white or yellowish-white, odorless solid is the principal example of a mercury(I) compound. It is a component of reference electrodes in electrochemistry.[1][2]
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[edit] History
The name calomel is thought to come from the Greek καλος beautiful, and μελας black. This name (somewhat surprising for a white compound) is probably due to its characteristic disproportionation reaction with ammonia, which gives a spectacular black coloration due to the finely dispersed metallic mercury formed. It is also referred to as the mineral horn quicksilver or horn mercury. Calomel was taken internally and used as a laxative and disinfectant before the 20th century . It was also used by doctors in the 1700's in America, and during the revolution, to make patients regurgitate and release their body from "impurities". George Washington may have died prematurely at the age of 67 because his physicians treated a respiratory illness with bloodletting and calomel[3]
[edit] Properties
Mercury is unique among the group 12 metals for its ability to form the M-M bond so readily. Hg2Cl2 is a linear molecule. The crystal structure is shown below:
[edit] Preparation and reactions
Mercurous chloride forms by the reaction of elemental mercury and mercuric chloride:
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- Hg + HgCl2 → Hg2Cl2
It can be prepared via metathesis reaction involving aqueous mercury(I) nitrate using various chloride sources including NaCl or HCl.
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- 2HCl + Hg2(NO3)2 → Hg2Cl2 + 2HNO3
Ammonia causes Hg2Cl2 to disproportionate:
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- Hg2Cl2 + 2NH3 → Hg + Hg(NH2)Cl + NH4Cl
[edit] Calomel electrode
Mercurous chloride is employed extensively in electrochemistry, taking advantage of the ease of its oxidation and reduction reactions. The calomel electrode is a reference electrode, especially in older publications. Over the past 50 years, it has been superseded by the silver/silver chloride (Ag/AgCl) electrode. Although the mercury electrodes have been widely abandoned due to the dangerous nature of mercury, many chemists believe they are still more accurate and are not dangerous as long as they are handled properly. The differences in experimental potentials vary little from literature values. Other electrodes can vary by 70 to 100 millivolts.[citation needed]
[edit] Photochemistry
Mercurous chloride decomposes into mercury(II) chloride and elemental mercury upon exposure to UV light.
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- Hg2Cl2 → HgCl2 + Hg
The formation of Hg can be used to calculate the number of photons in the light beam, by the technique of actinometry. By utilizing a light reaction in the presence of mercury(II) chloride and ammonium oxalate mercurous chloride is produced.
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- 2HgCl2 + (NH4)2C2O4 + Light → Hg2Cl2(s) + 2[NH4+][Cl−] + 2CO2
This particular reaction was invented by J.M. Eder (hence the name Eder reaction) in 1880 and reinvestigated by W. E. Rosevaere in 1929 [4]
[edit] Related mercury(I) compounds
Mercury(I) bromide, Hg2Br2, a light yellow, whereas mercury(I) iodide, Hg2I2, is greenish in colour. Both are poorly soluble. Mercury(I) fluoride is unstable in the absence of a strong acid.
[edit] Safety considerations
Mercurous chloride is toxic, although due to its low solubility in water it is generally less dangerous than its mercuric chloride counterpart. It was used in medicine as a diuretic and purgative (laxative), e.g. from the early 1830s through the 1860s as a purgative in the U.S. These medicinal uses were discontinued.
It has also found uses in cosmetics as soaps and skin lightening creams, but these preparations are now illegal to manufacture or import in many countries including U.S., Canada, Japan and Europe. A study of workers involved in the production of these preparations, showed that the sodium salt of 2,3-dimercapto-1-propanesulfonic acid (DMPS) was effective in lowering the body burden of mercury and in decreasing the urinary mercury concentration to normal levels.[5]
[edit] References
- ^ Housecroft, Catherine E., Sharpe, Alan G. (2001). Inorganic Chemistry, 2nd edition, New York: Pearson/Prentice Hall, 696-697.
- ^ Skoog, Douglas A., F. James Holler and Timothy A. Nieman (1998). Principles of Instrumental Analysis, 5th Edition, Saunders College Pub., 253-271.
- ^ Vadakan, M.D., Vibul V. (Winter/Spring 2005). A Physician Looks At The Death of Washington. Early America Review. Archiving Early America. Retrieved on 2008-02-17.
- ^ W. E. Roseveare (1930). "The X-Ray Photochemical Reaction between Potassium Oxalate and Mercuric Chloride". J. Am. Chem. Soc. 52 (7): 2612 - 2619. doi:.
- ^ D. Gonzalez-Ramirez, M. Zuniga-Charles, A. Narro-Juarez, Y. Molina-Recio, K. M. Hurlbut, R. C. Dart and H. V. Aposhian (1998). "DMPS (2,3-Dimercaptopropane-1-sulfonate, Dimaval) Decreases the Body Burden of Mercury in Humans Exposed to Mercurous Chloride" (free full text). Journal of Pharmacology and Experimental Therapy 287 (1): 8-12.
