Hydrate, bromine chlorine

Tin does not react directly with nitrogen, hydrogen, carbon dioxide, or gaseous ammonia. Sulfur dioxide, when moist, attacks tin. Chlorine, bromine, and iodine readily react with tin with fluorine, the action is slow at room temperature. The halogen acids attack tin, particularly when hot and concentrated. Hot sulfuric acid dissolves tin, especially in the presence of oxidizers. Although cold nitric acid attacks tin only slowly, hot concentrated nitric acid converts it to an insoluble hydrated stannic oxide. Sulfurous, chlorosulfuric, and pyrosulfiiric acids react rapidly with tin. Phosphoric acid dissolves tin less readily than the other mineral acids. Organic acids such as lactic, citric, tartaric, and oxaUc attack tin slowly in the presence of air or oxidizing substances. 

Bismuth pentafluoride is an active fluorinating agent. It reacts explosively with water to form ozone, oxygen difluoride, and a voluminous chocolate-brown precipitate, possibly a hydrated bismuth(V) oxyfluoride. A similar brown precipitate is observed when the white soHd compound bismuth oxytrifluoride [66172-91 -6] BiOF, is hydrolyzed. Upon standing, the chocolate-brown precipitate slowly undergoes reduction to yield a white bismuth(Ill) compound. At room temperature BiF reacts vigorously with iodine or sulfur above 50°C it converts paraffin oil to fluorocarbons at 150°C it fluorinates uranium tetrafluoride to uranium pentafluoride and at 180°C it converts Br2 to bromine trifluoride, BrF, and bromine pentafluoride, BrF, and chlorine to chlorine fluoride, GIF. It apparently does not react with dry oxygen. 

Aluminium powder ignites in chlorine without heating, and foil reacts vigorously with liquid bromine at 15°C, and incandesces on warming in the vapour [1], The metal and iodine react violently in the presence of water, either as liquid, vapour or that present in hydrated salts [2], Moistening a powdered mixture causes incandescence and will initiate a thermite mixture [3],... 

Flame retardants Antimony trioxide with chlorinated or brominated organics, hydrated alumina... 

Alkene and alkyne Bromination, acetic acid Chlorination, acetic acid Acid-catalyzed hydration, water... 

Reports of electrophilic substitution are scarce, but pyridazino[2,3-. ]quinoxaline-4,4-dicarboxylates reportedly undergo bromination and chlorination at C-3 with A -halosuccinimides in acetic acid (Scheme 29). Treatment of the product with hydrazine hydrate results in hydrolysis and mono-decarboxylation <2003JHC837>. 

Chlorine and bromine are fairly soluble in water iodine has a low solubility. Early determinations of the solubility of chlorine in water were made by J. L. Gay Lussac1 in 1839, by J. Pelouze in 1843, and by F. Sohonfeld in 1855. They noticed a maximum in the solubility curve in the vicinity of 10°, and at 100° the solubility is nil. Later determinations have been made by H. W. B. Roozeboom in 1885, and by L. W. Winkler in 1907. At temp, below 9 6°, chlorine forms a crystalline hydrate, C12.8H20 and this corresponds with the maximum in the solubility curve. The solubility curves of the gases chlorine and bromine 2 are indicated in Table III. 

H. W. B. Eoozeboom has measured the solubility of chlorine and bromine hydrates in water and expressed his results in terms of grams of chlorine per 100 grms. of soln. He found that 100 grms. of soln. contain 0 492 grm. of chlorine at —0 24°, at which temp, the solid phase present is a mixture of ice and chlorine hydrate, C12.8H20. Between 0° and 28 7° the solid phase is the hydrate alone, and the soln. has... 

F. Wohler 23 found that when chlorine hydrate in a sealed glass tube is exposed to sunlight, it forms two liquids, but does not decompose, since, after a summer s exposure, the two liquids re-form chlorine hydrate when winter returns. The same phenomena occur if the chlorine hydrate is warmed and cooled under similar conditions. A cone. soln. of chlorine water is far less prone to decomposition on exposure to sunlight than is a more dil. soln. J. M. Eder found the same to be the case with bromine water, but he also found that a cone. soln. of chlorine water lost 53 95 per cent, of chlorine while a dil. soln. lost 41 87 per cent, under similar conditions, but he does not state the concentration very exactly. A. Pedler further showed that soln. more cone, than one mols. of chlorine with 64 mol. of water had not decomposed perceptibly after a two months exposure to tropical sunlight, and with that increasing dilution, the action became progressively greater, as illustrated in Table VII. 

Triazine is resistant to electrophilic substitution. Chlorination requires vigorous conditions, and yields are low bromination is a more efficient process (Scheme 6). The reagents employed in the attempted sulfonation or nitration preferentially hydrolyze the ring (63AG(E)309). Recently, Korolev and Mal tseva have reported that 1,3,5-triazine is protonated and hydrated to form the cation shown in equation (2) (75ZOR2613). 

The period from 1810 to 1900 is characterized by efforts of direct composition measurements with inorganic hydrate formers, especially bromine, inorganics containing sulfur, chlorine, and phosphorus, and carbon dioxide. Other notable work listed in Table 1.2 was done by Cailletet and Bordet (1882), who first measured hydrates with mixtures of two components. Cailletet (1877) was also the first to measure a decrease in gas pressure when hydrates were formed in a closed chamber, using a precursor of an apparatus still in use at the Technical University of Delft, the Netherlands. 

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