Gold-mercury compounds

Mercury is used in the manufacture of thermometers, barometers and switchgear, and in the production of amalgams with copper, tin, silver and gold, and of solders. A major use in the chemical industry is in the production of a host of mercury compounds and in mercury cells for the generation of chlorine. Mercury has a significant vapour pressure at ambient temperature and is a cumulative poison. 

Ammonia is capable of reacting with some heavy metal compounds (silver, gold, mercury) to produce materials, some of uncertain constitution, which may explode violently when dry. 

The low-potential responses are detected on Hg. Solid electrodes like glassy carbon, gold or platinum show no response in this range. This implies that oxidation of the mercury electrode takes place as well. Indeed, the second DPP waves observed at +0.68 up to +0.72 V correspond to oxidation of mercury compounds such as Ph2Hg. The... 

This class of compounds showing explosive instability deals with heavy metals bonded to elements other than nitrogen and contains the separately treated groups GOLD COMPOUNDS LEAD SALTS OF NITRO COMPOUNDS LITHIUM PERALKYLURANATES MERCURY COMPOUNDS METAL ACETYLIDES METAL FULMINATES METAL OXALATES PLATINUM COMPOUNDS PRECIOUS METAL DERIVATIVES SILVER COMPOUNDS... 

The reaction of [PPN][Au2 CH2P(S)Ph2 2] with HgCl2, followed by T1PF6 treatment, resulted in a rearrangement of the Au-C bonds and compound 6 was isolated. It is an isomer of compound 5 in the cation of which both gold and mercury are linearly coordinated by a carbon and a sulfur atom. The isomers 5 and 6 do not interconvert under reflux inTHF [36]. The transannular gold-mercury distance in the cation of 6 [2.989(1) A] is about 0.1 A shortest than in the cations containing the... 

The development of the second class of compounds with gold-mercury bonds, that is, Hg-containing, Au-rich clusters, was mainly the contribution of Pignolet and coworkers [41-43]. Such compounds were generally obtained by addition of mercury... 

As mentioned in Chapter II, many metallic arsenides are found in Nature. Arsenic combines directly with most metals to form stable compounds, those of the heavy metals being the most stable. The latter may be obtained by allowing an aqueous solution of a salt of the appropriate metal to drop into an atmosphere of arsine, air being completely absent, and the vessel continually shaken.1 Precipitation by passing arsine into the salt solution is not satisfactory as, in the case of copper, silver, gold, mercury and lead, a secondary reaction with the excess of metallic ions occurs ... 

Cr(II) may be used to carry out all the reactions of Ti(III), but usually under milder conditions. Applications of Cr(II) as a reductant have been reviewed. The applications include Sn(IV) chloride in the presence of catalysts such as Sb(V) or Bi(III), Sb(V) in 20% HCl at elevated temperatures, Cu(II), silver, gold, mercury, bismuth, iron, cobalt, molybdenum, tungsten, uranium, dichromate, vanadate, titanium, thallium, hydrogen peroxide, oxygen in water and gases, as well as organic compounds such as azo, nitro, and nitroso compounds and quinones. Excess Cr(II) in sulfuric acid solution reduces nitrate to ammonium ion. The reduction is catalyzed by Ti(IV), which is rapidly reduced to Ti(III). 

Aqueous solutions of triorgano telluronium halides formed precipitates when mixed with aqueous solutions of copper(II) chloride zinc(II) chloride , gold(III) chloride ", mercury(II) halides " , and tin(II) chloride. Analytical data are only available for the mercury compounds. These data indicate that equimolar amounts of the telluronium halide and the mercury halide combine. The reactions can also be carried out in ethanol" . 

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