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Aqueous solutions of iron(III) chloride are also produced industrially from a number of iron precursors, including iron oxides: Fe 2 O 3 + 6 HCl + 9 H 2 O → 2 FeCl 3 (H 2 O) 6. In complementary route, iron metal can be oxidized by hydrochloric acid followed by chlorination: [10] Fe + 2 HCl → FeCl 2 + H 2 FeCl 2 + 0.5 Cl 2 + 6 H 2 O → FeCl ...
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Tetrachloroferrate is the polyatomic ion having chemical formula FeCl − 4.The metallate can be formed when ferric chloride (FeCl 3) abstracts a chloride ion from various other chloride salts. [1]
Potassium hexacyanidoferrate(II) is produced industrially from hydrogen cyanide, iron(II) chloride, and calcium hydroxide, the combination of which affords Ca 2 [Fe(CN) 6]·11H 2 O.
Iron(II) chloride, also known as ferrous chloride, is the chemical compound of formula FeCl 2.It is a paramagnetic solid with a high melting point. The compound is white, but typical samples are often off-white.
The number and type of ligands bound to iron(II) determine how these electrons arrange themselves. With the so-called "strong field ligands" such as cyanide , the six electrons pair up. Thus ferrocyanide ( [Fe(CN) 6 ] 4− has no unpaired electrons, meaning it is a low-spin complex.
Fe(acac) 3 has been examined as a precatalyst and reagent in organic chemistry, although the active iron-containing species is usually unidentified in these processes. In one instance, Fe(acac) 3 was shown to promote cross-coupling a diene to an olefin. [5]
The formation of Fe(III)-EDTA (FeY) − can be described as follows: FeSO 4 ∙7H 2 O + K 2 H 2 Y + 1/4 O 2 → K[FeY(H 2 O)]. H 2 O + KHSO 4 + 5.5 H 2 O (1) [8]. Iron chelate has also been used as a bait in the chemical control of slugs, snails and slaters in agriculture in Australia and New Zealand.