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Potassium ferrioxalate contains the iron(III) complex [Fe(C 2 O 4) 3] 3−. In chemistry, iron(III) or ferric refers to the element iron in its +3 oxidation state. Ferric chloride is an alternative name for iron(III) chloride (FeCl 3). The adjective ferrous is used instead for iron(II) salts, containing the cation Fe 2+.
Iron(III) oxide is a product of the oxidation of iron. It can be prepared in the laboratory by electrolyzing a solution of sodium bicarbonate, an inert electrolyte, with an iron anode: 4 Fe + 3 O 2 + 2 H 2 O → 4 FeO(OH) The resulting hydrated iron(III) oxide, written here as FeO(OH), dehydrates around 200 °C. [18] [19] 2 FeO(OH) → Fe 2 O 3 ...
Iron(II) is oxidized by hydrogen peroxide to iron(III), forming a hydroxyl radical and a hydroxide ion in the process. This is the Fenton reaction . Iron(III) is then reduced back to iron(II) by another molecule of hydrogen peroxide, forming a hydroperoxyl radical and a proton .
The iron compounds produced on the largest scale in industry are iron(II) sulfate (FeSO 4 ·7H 2 O) and iron(III) chloride (FeCl 3). The former is one of the most readily available sources of iron(II), but is less stable to aerial oxidation than Mohr's salt ((NH 4) 2 Fe(SO 4) 2 ·6H 2 O). Iron(II) compounds tend to be oxidized to iron(III ...
Thiocyanate is a common test for the presence of iron(III) as it forms the blood-red [Fe(SCN)(H 2 O) 5] 2+. Like manganese(II), most iron(III) complexes are high-spin, the exceptions being those with ligands that are high in the spectrochemical series such as cyanide. An example of a low-spin iron(III) complex is [Fe(CN) 6] 3−.
Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO 3) 3. (H 2 O) n. Most common is the nonahydrate Fe(NO 3) 3. (H 2 O) 9. The hydrates are all pale colored, water-soluble paramagnetic salts.
Iron oxides feature as ferrous or ferric or both. They adopt octahedral or tetrahedral coordination geometry. Only a few oxides are significant at the earth's surface, particularly wüstite, magnetite, and hematite. Oxides of Fe II. FeO: iron(II) oxide, wüstite; Mixed oxides of Fe II and Fe III. Fe 3 O 4: Iron(II,III) oxide, magnetite; Fe 4 O ...
The iron is low spin and easily reduced to the related ferrocyanide ion [Fe(CN) 6] 4−, which is a ferrous (Fe 2+) derivative. This redox couple is reversible and entails no making or breaking of Fe–C bonds: [Fe(CN) 6] 3− + e − ⇌ [Fe(CN) 6] 4−. This redox couple is a standard in electrochemistry.