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The telluride ion is the anion Te 2− and its derivatives. It is analogous to the other chalcogenide anions, the lighter O 2−, S 2−, and Se 2−, and the heavier Po 2−. [1] In principle, Te 2− is formed by the two-e − reduction of tellurium. The redox potential is −1.14 V. [2] Te(s) + 2 e − ↔ Te 2−
Hydrogen telluride is the inorganic compound with the formula H 2 Te.A hydrogen chalcogenide and the simplest hydride of tellurium, it is a colorless gas.Although unstable in ambient air, the gas can exist long enough to be readily detected by the odour of rotting garlic at extremely low concentrations; or by the revolting odour of rotting leeks at somewhat higher concentrations.
TeO 2 + H 2 O 2 + 2 H 2 O → Te(OH) 6. Crystallization of telluric acid solutions below 10 °C gives telluric acid tetrahydrate Te(OH) 6 ·4H 2 O. [3] It is an oxidising agent, as shown by the electrode potential for the reaction below, although it is kinetically slow in its oxidations. [4] Te(OH) 6 + 2 H + + 2 e − ⇌ TeO 2 + 4 H 2 O, E o ...
Na 2 Te, like many related compounds with the formula M 2 X, adopts the antifluorite structure. Thus, in solid Na 2 Te each Te 2− ion is surrounded by eight Na + ions and each Na + ion is surrounded by four Te 2− ions. [3] Simple salts of the type M 2 X, where X is a monatomic anion, are not typically soluble in any solvent because they ...
Structure of tellurium tetrachloride, tetrabromide and tetraiodide. The +2 oxidation state is exhibited by the dihalides, TeCl 2, TeBr 2 and TeI 2.The dihalides have not been obtained in pure form, [3]: 274 although they are known decomposition products of the tetrahalides in organic solvents, and the derived tetrahalotellurates are well-characterized:
Tellurous acid is an inorganic compound with the formula H 2 TeO 3. It is the oxoacid of tellurium(IV). [2] This compound is not well characterized. An alternative way of writing its formula is (HO) 2 TeO. In principle, tellurous acid would form by treatment of tellurium dioxide with water, that is by hydrolysis.
One of Pauling's examples is olivine, M 2 SiO 4, where M is a mixture of Mg 2+ at some sites and Fe 2+ at others. The structure contains distinct SiO 4 tetrahedra which do not share any oxygens (at corners, edges or faces) with each other. The lower-valence Mg 2+ and Fe 2+ cations are surrounded by polyhedra which do share oxygens.
8 H 2 S n → 8 H 2 S + (n − 1) S 8. They also react with sulfite and cyanide to produce thiosulfate and thiocyanate respectively. [13] An alternative structural isomer of the trisulfide, in which the two hydrogen atoms are attached to the central sulfur of the three-sulfur chain rather than one on each end, has been examined computationally ...