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Two crystalline forms are known, both being very similar to the corresponding potassium sulfate. Orthorhombic β-K 2 CrO 4 is the common form, but it converts to an α-form above 66 °C. [1] These structures are complex, although the chromate ion adopts the typical tetrahedral geometry. [2]
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2 CrO 2− 4 + 2 H + ⇌ Cr 2 O 2− 7 + H 2 O. The predominance diagram shows that the position of the equilibrium depends on both pH and the analytical concentration of chromium. [notes 1] The chromate ion is the predominant species in alkaline solutions, but dichromate can become the predominant ion in acidic solutions.
Potassium dichromate, K 2 Cr 2 O 7, is a common inorganic chemical reagent, most commonly used as an oxidizing agent in various laboratory and industrial applications. As with all hexavalent chromium compounds, it is acutely and chronically harmful to health.
Structure of an octahedral metal aquo complex. Chromium(II) ion in aqueous solution. Most aquo complexes are mono-nuclear, with the general formula [M(H 2 O) 6] n+, with n = 2 or 3; they have an octahedral structure. The water molecules function as Lewis bases, donating a pair of electrons to the metal ion and forming a dative covalent bond ...
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It is very insoluble in water, but is soluble in acids: 2 BaCrO 4 + 2 H + → 2 Ba 2+ + Cr 2 O 7 2− + H 2 O K sp = [Ba 2+][CrO 4 2−] = 2.1 × 10 −10. It can react with barium hydroxide in the presence of sodium azide to create barium chromate(V). The reaction releases oxygen and water.