Peroxide of Iron

Pertartkate of Iron, by dissolving the freshly prepared hydrated peroxide of iron in solution of tartaric acid. Its solution is not precipitated by alkalies. 

Goldschmidt and Pauncz (1933) suggested that Fenton s reaction is a chain reaction involving the same reactive intermediates occurring during catalytic decomposition of H202 rather than via formation of peroxides of iron ... 

Ferric Oxide—Seti ioxide or peroxide of iron—Colcothar—Jewellefv rouge—Venetian red—Pe,0,—159.8—occurs In nature (see above) snd is formed when ferrous sulphate is strongly heated, as in the msnutecture of... 

Peroxide of Iron. Peroxide, or sesquioxido of iron, is a brownish-red powd, known as the red oxide or mst of iron in its hydrated form it is very soluble in acids, but less so when anhydrous. The salts of peroxide of iron have for the most part a radish-yellow color, and redden bine litmus paper. Cooky.)... 

Teats for the Solutions of the Salts of Peroxide of Iron. Sulphuretted hydrogen throws down a black precipitate from Saline solutious. 

Isomorphism.—In many instances two or more substances crystallize in forms identical with each other, and, in most cases, such substances resemble e.ach other in their chemical constitution. They are said to be isomorphous. This identity of crystalline form does not depend so much upon the nature of the elements themselves, as upon the structure of the molecule. Tlie protoxid and peroxid of iron do not crystallize in the same form, nor can they be substituted for each other in reactions without i-adically altering the properties of the resultant compound. On the other hand, all that class of salts known as alums are isomorphous. Not only are their crystals identical in shape, but a crystal of one alum, placed in a saturated solution of another, gro ws... 

Ferric Oxid—Sesquioxid or peroxid of iron—Colcothar—Jeweller s rouge—Venetian red—FejOa—159.8—occurs in nature (see above and is formed when ferrous sulfate is strongly heated, as in the manufacture of pyrosulfuric acid. It is a reddish, Amorphous solid, is a weak base, and is decomposed at a white heat into O and Pes04. 

The first is, that since, by definition, an atom is that which cannot be divided, there cannot be formed a compound of 1 atom, or equivalent of one element, and an atom (or any fractional number of atoms, as 1.J-, 2, c.) of another element. Should such proportions appear to exist, they must be so expressed as to get rid of fractions, otherwise they imply a contradiction in terms. Thus, for example, iron combines with oxygen in two proportions. In the first compound, or protoxide of iron, 28 parts (1 eq.) of iron are combined with 8 parts, or 1 eq.j of oxygen. We, therefore, assume this compound to contain 1 atom of each element, and express it in symbols by FeO. In the other oxide, or peroxide of iron, 28 parts, or 1 eq., of iron are found to be combined with 12 parts of oxygen. Now, 8 being 1 eq. of oxygen, 12 must be l - eq. But as it would be absurd to call this oxide a compound of 1 atom of iron and 1.J- atom of oxygen, we get rid of the fraction by doubling both numbers, and we represent the peroxide of iron by Fe O,. Here the proportion is still that of 1 to l.p, but the absurdity of... 

Anhydrous sulphuric acid is obtained by distilling dried basic persulphate of iron, F, O, SO, when the peroxide of iron is left, and the sulphuric acid distils over, condensing in the receiver (if kept dry) as a white ciystaHine solid, which gives off thick fumes in moist air, is converted into vapour at about 160°, and has so strong an afiinity for the elements of water, that when thrown into water it hisses as a red-hot iron would do, combining with the water and forming oil of vitriol. 

Syn. Sesquichloride of Iron Permuriate of Iron.—It is formed when chlorine gas is passed over iron heated to a temperature below redness, when it appears as red iridescent scales, volatile at a temperature little beyond 212 , and soluble in water, alchohol, and ether. A solution of the perchloride is easily obtained by dissolving peroxide of iron in hydrochloric acid Fe, 0, + 3HC1 = Fe, Cl, -t- 3 HO. When evaporated to the consistence of syrup, and cooled, it forms red crystals, which contain water of ciystallisation. When heated, they are partly decomposed, peroxide being formed, and hydrochloric acid passing off, in consequence of the action between perchloride of iron and water. As perchloride of iron is a volcanic product, it is probably in this way that the crystals of peroxide, found in volcanic districts, have been formed. Perchloride of iron is much used in medicine. 

It is formed by the action of hydrosulphuric acid (sulphuretted hydrogen) on peroxide of iron, at a heat not above 212°, as a yellowish grey powder or by adding perchloiide of iron to an excess of hydrosulphuret of ammonia, as a black powder, rapidly oxidised by exposure to the air. 

When moist hydrated peroxide of iron is mixed with a neutral solution of protochloride of tin, an exchange takes place, and a bulky precipitate of a grey colour is formed, which is a hydrate of sesquioxide of tin. Fe Oj -p 2 SnCl = Sn, 0,-1-2 FeCl. The sesquioxide is soluble in acids and in ammonia, the latter character distinguishing it from the protoxide. Its solution in hydrochloric add forms, with chloride of gold, the purple of Cassius and seems, indeed, better adapted for making it than the protoxide. 

The only known antidote to arsenious acid is the hydrated peroxide of iron, the ferrugo of the Edin. Pharmacopoeia, which should be given in the moist state mixed with water. When made for this purpose, the precipitated oxide should never be dried, but kept under water as when once dried, it is far less efficacious. It acts by combining with the arsenious acid. 

Sulphate of the peroxide of iron does not crystallise, but forms crystallisable double salts. Formula Fe 0, 3 SO, or, Fe, 3 SO,. 

Carbonate of protoxide of iron is formed when an alkaline carbonate is added to a solution of protosulphate of iron. It falls as a dirty white bulky precipitate, which rapidly becomes green, and then brown, losing carbonic acid, and attracting oxygen, till it passes into hydrated peroxide of iron. It may be... 

Incompatibilities and Reactivities Anhydrous chlorides of iron, tin, and aluminum peroxides of iron and aluminum alkali metal hydroxides iron strong acids, caustics peroxides [Note Polymerization may occur due to high temperatures or contamination with alkalis, aqueous acids, amines acidic alcohols ] ... 

Antidotes.—Moist hydrated peroxide of iron magnesia cold affusions inhalation of ammonia. 

Antidotes.—Fresh air affusions of cold water inhalation of ammonia or chlorine freshly precipitated hydrated peroxide of iron mixed with an alkaline carbonate. 

Synonyms.—Moist Ferric Hydrate Ferri Peroxidum Hydratum Moist Hydrated Peroxide of Iron. 

Mix the solution of persulphate of iron with a pint of the distilled water, and add this gradually to the solution of soda, stirring constantly and briskly. Let the mixture stand for two hours, stirring it occasionally, then put it on a calico filter, and, when the liquid has drained away, wash the precipitate (moist peroxide of iron) with distilled water until the filtrate ceases to give a precipitate with barium chloride, which shows that the precipitate is freed from sulphate. Lastly, enclose the precipitate, without drying it, in a stoppered bottle from which evaporation cannot take place. This preparation, when used, should be recently made. 

Hydrated Peroxide of Iron. .. 1 part. Confection of Eoses.3 parts. 

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