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Mercury chloride halides

Two metal halides have been found to react with olefins by what appears to be insertion reaction. Palladium chloride and mercury chloride both will add to olefins. The palladium alkyls canot be isolated, but they go on to products which can be accounted for by an initial addition. [Pg.209]

Sulfur also reacts with fluoroalkyl mercurials and fluoroalkyl iodides to give fluorothioacyl halides. In the case of the reaction with mercurials, the halide formed is determined by substitution on the carbon attached to mercury. For example, bis(perfluoroethyl)mercury gives trifluorothioacetyl fluoride and bis-(l,l-dichloro-2,2,2-trifluoroethyl)mereury gives trifluorothioacetyl chloride. [Pg.89]

In the presence of proton and/or Lewis acid and strong nucleophiles bicyclo[3.2.0]heptan-6-ones are converted to 3-substituted cycloheptanones (Table 15). Bicyclo[3.2.0]heptan-6-ones rearrange to give 3-iodocycloheptanones on treatment with iodotrimethylsilane. Zinc(II) iodide or mercury(II) halides as catalysts enhance the rate and the selectivity of the reaction.31 If a second, enolizable carbonyl group is present, an intramolecular alkylation may follow the ring enlargement under these reaction conditions.32 Consecutive treatment with tributyltin hydride/ 2,2 -azobisisobutyronitrile affords reduced, iodo-free cycloheptanones, whilst treatment with l,8-diazabicyclo[5.4.0]undecene yields cycloheptenones.33 Similarly, benzenethiol adds to the central bond of bicyclo[3.2.0]heptan-6-ones in the presence of zinc(II) chloride and hydrochloric acid under anhydrous conditions to form 3-(phenylsulfanyl)cycloheptanones.34... [Pg.565]

Metal Halides. Reacts explosively or violently with the following calcium bromide iron(III) bromide or chloride iron(II) bromide or iodide cobalt(II) chloride silver fluoride all four mercury(II) halides copper(I) chloride, bromide or iodide copper(II) chloride and bromide ammonium tetrachlorocuprate zinc and cadmium chlorides, bromides, and iodides aluminum fluoride, chloride, and bromide thallium bromide tin(II) or (IV) chloride tin(IV) iodide arsenic trichloride and triiodide antimony and bismuth trichlorides, tribromides, and triiodides vanadium(V) chloride chromium(IV) chloride manganese(II) and iron(II) chlorides and nickel chloride, bromide, and iodide.17,22"25... [Pg.485]

Anodic limits on mercury. Mercury is readily oxidized, particularly in the presence of anions that precipitate or complex mercury or mercury ) ions, such as the halides, cyanide, thiosulfate, hydroxide, or thiocyanate. For this reason, mercury is seldom used to study anodic processes except for those subtances that are easily oxidized, for example, Cr(II), Cu(I), and Fe(II). Under carefully controlled conditions, mercury can be coated with a thin layer of mercury chloride such that it does not interfere with electron transfer in the oxidation of a number of organic compounds, particularly amines.66... [Pg.209]

Unsymmetrical phenylpentafluorophenyl and methylpentafluorophenyl compounds are obtained from the appropriate mercury(ll) halide [45], or by decarboxylation procedures [69], and these mixed derivatives are particularly susceptible to attack. Nevertheless, bis(pentafluorophenyl)mercury is very resistant to acid cleavage for example, it can be recrystallised from concentrated sulphuric acid, but the well-known ligand-exchange process, e.g. with mercury(ll) chloride, occurs very rapidly and presumably by a four-centre process [45] (Figure 10.23). [Pg.375]

Nitroselenenylation of alkenes141-149 is performed in a mixture of acetonitrile/tetrahydro-furan (compared to the nitromercuration reaction, this allows application to alkenes that may be insoluble in water) by the addition of phenylselenenyl halides, mercury(ii) chloride, and silver nitrite. Mercury chloride is necessary to significantly or completely suppress the formation of -hydroxy selenides due to the ambident character of the nitrite anion. [Pg.687]

The reaction is specific in that the allyl group retains its configuration in the course of transfer. Thus reactions of metallic mercury with an asymmetrically substituted 7r-allylpalladium chloride (for example, crotyl-palladium chloride) might equally afford both cis- and /raMr-2-butenyl-mercury chloride isomers, as well as the 1-butenyl compound. Hence generally three compounds could be expected in the reaction. However, it has been found 161) that essentially the reaction yields only trans-crotylmercury chloride (based on infrared spectra). In the case of 1-phenyl-77-allylpalladium chloride and l-acetyl-2-methyl-7r-allylpalladium chloride, again only the respective y-substituted /raw-allylmercury halides have been found. Since such conditions do not allow the allyl rearrangement 162), formation of the /ra r-allylmercury derivatives is evidence that the... [Pg.376]

Aryl tellurium halides react with aliphatic and aromatic Grignard reagents, with ethenyl magnesium halides , with ethynyl magnesium bromide with dimethyl and diethyl cadmium , with 2-(diphenylphosphino)-phenyl lithium, and with phenyl mercury chloride to produce aryl organo telluriums (p. 416). [Pg.250]

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" . [Pg.694]

The monoaryl boric acids, RB(OH)2, arc usually isolated, as stated al >o x, l)y the action of water on the type RBXg, aitliough in certain cases this leads to the formation of the oxide RBO. The phenyl eom >ound has l)ecn obtained b " boiling with water the product of reaction from magnesium phenyl bromide and boron trifluoride. The most remarkable feature of the type RE(OH)2 is that the action of iiiercuric chloride upon them leads to the production of mercury aryl halides (RHgX). The anisyl and phenetyl compounds do not yield oxides when heated, or form salts, and tlie jS-naphthyl acid exists in two modifications. Dehydration of the acids in maw gives the oxides, RBO. [Pg.220]

Vibrational constants were estimated by analogy with the other mercuric halides and the mercurous halides. The bond length was estimated by assuming the mercurous bond to be 0.965 of the mercuric bond by analogy with the mercury chlorides. [Pg.1071]

Anhydrous lanthanide trihalides, particularly the trichlorides, are important reactants for the formation of a variety of lanthanide complexes, including organometallics. Routes for the syntheses of anhydrous lanthanide trihalides generally involve high temperature procedures or dehydration of the hydrated halides.The former are inconvenient and complex for small scale laboratory syntheses, while dehydration methods may also be complex and have limitations, for example, use of thionyl chloride. - Moreover, the products from these routes may require purification by vacuum sublimation at elevated temperatures. Redox transmetalation between lanthanide metals and mercury(II) halides was initially carried out at high temperatures. However, this reaction can be carried out in tetrahydrofuran (THF, solvent) to give complexes of lanthanide trihalides with the solvent. These products are equally as suitable as reactants for synthetic purposes as the uncomplexed... [Pg.136]

Other small-scale laboratory procedures have been developed for the direct synthesis of the more reactive THF adducts, avoiding inconvenient high temperature treatment [59-62]. For example, the preparation of LnCl3(thf)x from metal powder and hexachloroethane is facilitated by sonication [Eq. (1)] [59]. Additional metal-based synthetic routes include the redox transmetallation with mercury(II) halides [Eq. (2)] [60] and the reaction with trimethylsilyl chloride and anhydrous methanol [Eq. (3)] [61]. Ammonia has been employed as an alternative donating solvent in the synthesis of lanthanide alkoxides starting from lanthanide chlorides [63]. [Pg.12]

Halides of zinc, cadmium, and mercury are readily alkylated by aluminum alkyls (117, 303). All of the alkyl groups of the aluminum participate in the reaction with HgCl2. But the alkylation does not proceed beyond the formation of alkyl mercury chlorides, RHgCl, except in the presence of a complexing agent (e.g., NaCl). Then complete alkylation to the mercury dialkyl occurs. [Pg.310]

A-Alkylphenotellurazines form 1 1 molecular complexes with mercury(II) halides and with silver nitrate or silver perchlorate <85KGS757>. Bis(benzonitrile)palladium(II) chloride reacts to form a 2 1 adduct and rhodium carbonyls also complex with phenotellurazines <82D0K(266)1164>. [Pg.1012]

Human activities have resulted in the release of a wide variety of both inorganic and organic forms of mercury. The electrical industry, chloro-alkali industry, and the burning of fossil fuels (coal, petroleum, etc.) release elemental mercury into the atmosphere. Metallic mercury has also been released directly to fresh water by chloro-alkali plants, and both phenylmer-cuiy and methylmercury compounds have been released into fresh and sea water -phenylmercury by the wood paper-pulp industry, particularly in Sweden, and methyl-mercury by chemical manufacturers in Japan. Important mercury compounds which also may be released into the environment include mercury(II) oxide, mercury(II) sulfide (cinnabar), mercury chlorides, mer-cury(II) bromide, mercury(II) iodine, mer-cury(II) cyanide, mercury(II) thiocyanate, mercury(II) acetate, mercury nitrates, mercury sulfates, mercury(II) amidochloride monoalkyl- and monoarylmercury(II) halides, borates and nitrates dialkylmercury compounds like dimethylmercury, alkoxyal-kylmercury compounds or diphenylmercury (Simon and Wiihl-Couturier 2002) (for quantities involved, see Section 17.4). [Pg.945]

Mercury(I) halides have a similar trend, with Hg2p2 the most soluble and Hg2l2 the least soluble. However, LiF is by far the least soluble of the lithium halides its K p is 1.8 X 10 , but the other lithium halides are highly soluble in water. Similarly, Mgp2 and AIF3 are less soluble than the corresponding chlorides, bromides, and iodides. [Pg.201]


See other pages where Mercury chloride halides is mentioned: [Pg.438]    [Pg.353]    [Pg.940]    [Pg.438]    [Pg.979]    [Pg.1252]    [Pg.1252]    [Pg.556]    [Pg.2017]    [Pg.2588]    [Pg.2588]    [Pg.263]    [Pg.580]    [Pg.172]    [Pg.407]    [Pg.2016]    [Pg.2587]    [Pg.136]    [Pg.191]    [Pg.3]    [Pg.112]    [Pg.3006]    [Pg.17]    [Pg.89]   
See also in sourсe #XX -- [ Pg.17 ]




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Mercury halides

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