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It may be formed by the salt metathesis reaction of potassium chromate and iron(III) nitrate, which gives potassium nitrate as byproduct. 2 Fe(NO 3) 3 + 3 K 2 CrO 4 → Fe 2 (CrO 4)3 + 6 KNO 3. It also can be formed by the oxidation by air of iron and chromium oxides in a basic environment: 4 Fe 2 O 3 + 6 Cr 2 O 3 + 9 O 2 → 4 Fe 2 (CrO 4) 3
When Fe 2 O 3 ·H 2 O is heated, it loses its water of hydration. Further heating at 1670 K converts Fe 2 O 3 to black Fe 3 O 4 (Fe II Fe III 2 O 4), which is known as the mineral magnetite. Fe(O)OH is soluble in acids, giving [Fe(H 2 O) 6] 3+. In concentrated aqueous alkali, Fe 2 O 3 gives [Fe(OH) 6] 3−. [12]
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+. The word ferric is derived from the Latin word ferrum, meaning "iron". Although often abbreviated as Fe 3+, that naked ion does not exist
Iron shows the characteristic chemical properties of the transition metals, namely the ability to form variable oxidation states differing by steps of one and a very large coordination and organometallic chemistry: indeed, it was the discovery of an iron compound, ferrocene, that revolutionalized the latter field in the 1950s. [1]
Its importance lies in its ability to mediate electron transfer. In the ferrous state (Fe 2+), iron acts as an electron donor, while in the ferric state (Fe 3+) it acts as an acceptor. Thus, iron plays a vital role in the catalysis of enzymatic reactions that involve electron transfer (reduction and oxidation, redox).
The first stage of Fenton's reaction (oxidation of Fe 3+ with hydrogen peroxide) is used in Haber–Weiss reaction; Fenton's reagent can be used in organic synthesis reactions: e.g. hydroxylation of arenes via a free radical substitution; Conversion of benzene into phenol by using Fenton's reagent; Oxidation of barbituric acid into alloxan.
When metallic iron (oxidation state 0) is placed in a solution of hydrochloric acid, iron(II) chloride is formed, with release of hydrogen gas, by the reaction Fe 0 + 2 H + → Fe 2+ + H 2. 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.
In the absence of EDTA or similar chelating agents, ferric ions form insoluble solids and are thus not bioavailable. [1] Together with pentetic acid (DTPA), EDTA is widely used for sequestering metal ions. Otherwise these metal ions catalyze the decomposition of hydrogen peroxide, which is used to bleach pulp in papermaking. Several million ...