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Chemical formula. K 2 TeO 3 Appearance white crystals, powder Hazards GHS labelling: ... Potassium tellurite, K 2 TeO 3, is an inorganic potassium-tellurium compound. [1]
Potassium telluride is an inorganic compound with a chemical formula K 2 Te. It is formed from potassium and tellurium, making it a telluride. [2] Potassium telluride is a white powder. Like rubidium telluride and caesium telluride, it can be used as an ultraviolet detector in space.
In aqueous solution tellurate ions are 6 coordinate. In neutral conditions the pentahydrogen orthotellurate ion, H 5 TeO − 6, is the most common; in basic conditions, the tetrahydrogen orthotellurate ion, H 4 TeO 2− 6, and in acid conditions, orthotelluric acid, Te(OH) 6 or H 6 TeO 6 is formed. [8]
A tellurite tellurate is a chemical compound or salt that contains tellurite and tellurate anions [TeO 3] 2-[TeO 4] 2-. These are mixed anion compounds , meaning the compounds are cations that contain one or more anions.
Tellurite is a oxyanion of tellurium with the formula TeO 2− 3.It is the ion of tellurous acid, and is chemically related to tellurium dioxide (TeO 2), whose mineral appearance also bears the name tellurite.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
When tellurium is treated with concentrated sulfuric acid, the result is a red solution of the Zintl ion, Te 2+ 4. [17] The oxidation of tellurium by AsF 5 in liquid SO 2 produces the same square planar cation, in addition to the trigonal prismatic, yellow-orange Te 4+ 6: [5]
If this convention is used, then the values are in the same range as monovalent ions, e.g. 59.5 S cm 2 mol −1 for 1 / 2 Ca 2+ and 80.0 S cm 2 mol −1 for 1 / 2 SO 2− 4. [4] From the ionic molar conductivities of cations and anions, effective ionic radii can be calculated using the concept of Stokes radius.