![]() Salts where chromium at an oxidation state of +3 acts as a cation display all typical properties of salts (most of them are soluble in water and hydrolyze – they decompose in water with the formation of chromium hydroxide Cr(OH)₃):Ĭhromium salts with an oxidation state of +3 can take part in oxidation-reduction reactions, for example in the following:ĢCrCl₃ + 3Zn + 4HCl = 2CrCl₂ + 3ZnCl₂ + 2H₂ (in the reaction between hydrochloric acid and zinc, atomic hydrogen is released, which reduces the chromium cation to the chromium cation). Chromium (II) oxideĬhromium (II) oxide is formed in the decomposition of chromium carbonyl (with heating):Ĭr(CO)₆ = CrO + 5CO + C. The reductive ability of Cr²⁺ salts is very high (in some cases these salts can even displace hydrogen from water). Hydrogen released in the course of reaction reduces Cr³⁺ to Cr²⁺. They are usually obtained by oxidation-reduction reactions from chromium (III). Salts of chromium (II) have a bluish color. The compounds are colored – chromium (II) oxide is black, and the hydroxide is yellow. Chromium in the oxidation state of +2Ĭhromium (II) oxide and hydroxide CrO and Cr(OH)₂ are compounds which display typical base properties. In compounds (which are brightly colored in the majority of cases), chromium displays several possible oxidation states - +2, +3, +4 (encountered quite rarely, chromium oxide CrO₂ is known), +6.
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