Diselenium dichloride

Sulphur and selenium form the chlorides disulphur dichloride S2CI2 and diselenium dichloride Se2Cl2. They are made by the direct combination of the elements. Both are covalent, yellow liquids which are readily hydrolysed by water ... 

Diselenium dichloride acts as a solvent for selenium. Similarly disulphur dichloride is a solvent for sulphur and also many other covalent compounds, such as iodine. S Clj attacks rubber in such a way that sulphur atoms are introduced into the polymer chains of the rubber, so hardening it. This product is known as vulcanised rubber. The structure of these dichlorides is given below ... 

Powdered aluminium ignites in the vapour of arsenic trichloride or sulfur dichloride, and incandesces in phosphorus trichloride vapour [1], Above 80°C, aluminium reacts incandescently with diselenium dichloride [2], The powder ignites in contact with phosphorus pentachloride [3],... 

Potassium dioxide Diselenium dichloride Sodium Non-metal halides Sodium peroxide Non-metal halides... 

Diselenium dichloride and seleninyl chloride both explode on addition of potassium [1,3], while the metal ignites in contact with phosphorus trichloride vapour or liquid [2], Mixtures of potassium with sulfur dichloride or sulfur dibromide, phosphorus tribromide or phosphorus trichloride, and with phosgene are shock-sensitive, usually exploding violently on impact. Potassium also explodes violently on heating with disulfur dichloride, and with sulfur dichloride or seleninyl bromide without heating [3]. 

Diselenium dichloride Mellor, 1947, Vol. 10, 897 Interaction is very violent. 

Dehnicke, K. et al., Angew. Chem. (Int.), 1991, 30(5), 577 Made from diselenium dichloride and trimethylsilyl azide, the crystalline nitride explodes under a hammer blow, or on heating to 80°C. Can apparently be handled safely at room temperature. 

Violent interactions occur with diselenium dichloride or disulfur dichloride, the latter emitting light and heat [1]. The very exothermic reaction with phosphorus trichloride may accelerate to explosion [2],... 

Diethylaminosulfur trifluoride, 1684 Diphosphoryl chloride, 4168 Diselenium dichloride, 4115 Disulfur dibromide, 0282 Disulfur dichloride, 4114 Disulfuryl dichloride, 4103... 

Diselenium dichloride, 4109 Disulfur dibromide, 0281 Disulfur dichloride, 4108 Disulfuryl dichloride, 4097... 

Nonmetal Halides. Reacts explosively or forms shock-sensitive mixtures with diselenium dichloride and seleninyl chloride,31,32 PC13 vapor or liquid,33 sulfur dichloride or dibromide, and PBr3 and phosgene.32... 

Nonmetal Halides. Vigorous or explosive reactions occur with phosphorus tribromide on addition of drops of water,20 phosphorus trichloride, phosphorus pentachloride,21 diselenium dichloride,22 sulfur dichloride, boron tribromide, sulfur dibromide,17 seleninyl bromide,23 phosphoryl chloride, sulfinyl fluoride, silicon tetrachloride, and silicon tetrafluoride.24... 

The same products were obtained when diselenium dichloride was used in place of selenium dioxide1. 

Heating diary) ditellurium compounds in pyridine with selenium dioxide or diselenium dichloride led to the insertion of a selenium atom into the Te — Te bond and the oxidation of one or more of the chalcogen atoms in the bis[aryltelluro] selenides7. 

Sc4N4 is prepared by ammonolysis of selenium tetrahalides, diselenium dichloride,selenium di-oxide, or diethyl selenite. It is rather unstable and decomposes explosively on heating or by sudden impact. 

Diselenium dichloride, 863012, and seleninyl chloride, 8eOOl2, react with a lithium salt of silylated t-butylamine with elimination of LiOl and Me38i01 or of LiOl, Mc3 8i01, and (Mc38i)20, respectively, to form the cyclic compounds (t-Bu)2X28c6 (16), a hexaselenadiazocin, and (t-Bu)6X68c9... 

DOT CLASSIFICATION 5.1 Label Oxidizer SAFETY PROFILE Explosive reaction when heated with carbon, 2-aminophenol + tetrahydrofuran (at 65°C). Forms a friction-sensitive explosive mixture with hydrocarbons. Violent reaction with diselenium dichloride, ethanol, potassium-sodium alloy. May ignite on contact with organic compounds. Incandescent reaction with metals (e.g., arsenic, antimony, copper, potassium, tin, and zinc). When heated to decomposition it emits toxic fumes of K2O. See also PEROXIDES. 

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