Iron compounds naming

Up to now, two types of iron compounds have been studied with ENDOR, namely heme compounds (hemoproteins and some heme model compounds) and iron-sulfur proteins. For comprehensive summaries of the corresponding EPR work, the reader is referred to the literature234-2371. 

Synonym Neatsfoot Oil Necatorina Nechexane Neutral Ahhonium Pluoride Neutral Anhydrous Calcium Hypochlorite Neutral Lead Acetate Neutral Nicotine Sulfate Neutral Potassium Chromate Neutral Sodium Chromatetanhydrous Neutral Verdigris Nickel Acetate Nickel Acetate Tetrahyorate Nickel Ammonium Sulfate Nickel Ammonium Sulfate Hexahydrate Nickel Bromide Nickel Bromide Trihydrate Nickel Carbonyl Nickel Chloride Nickel Chloride Nickel Cyanide Nickel Iiu Fluoborate Nickel Fluoroborate Solution Nickel Fluoroborate Nickel Formate Nickel Formate Dihyorate Nickel Nitrate Nickel Nitrate Hexahydrate Nickel Sulfate Nickel Tetracarbokyl Nickelous Acetate Nickelous Sulfate Nicotine Nicotine Sulfate Nifos Nitralin Nitram O-Nitraniline P-Nitraniline Nitric Acid Nitric Acid, Aluminum Salt Nitric Acid, Iron (111) Salt Compound Name Oil Neatsfoot Carbon Tetrachloride Neohexane Ammonium Fluoride Calcium Hypochlorite Lead Acetate Nicotine Sulfate Potassium Chromate Sodium Chromate Copper Acetate Nickel Acetate Nickel Acetate Nickel Ammonium Sulfate Nickel Ammonium Sulfate Nickel Bromide Nickel Bromide Nickel Carbonyl Nickel Chloride Nickel Chloride Nickel Cyanide Nickel Fluoroborate Nickel Fluoroborate Nickel Fluoroborate Nickel Formate Nickel Formate Nickel Nitrate Nickel Nitrate Nickel Sulfate Nickel Carbonyl Nickel Acetate Nickel Sulfate Nicotine Nicotine Sulfate Tetraethyl Pyrophosphate Nitralin Ammonium Nitrate 2-Nitroaniline 4-Nitroaniline Nitric Acid Aluminum Nitrate Ferric Nitrate... 

In chemical experiments, the most commonly used iron compound is the iron sulfate (ferrous sulfate, FeSOj-THjO) — also called green vitriol and copperas. Don t let the last name mislead you— it has nothing to do with copper but conies from an old French word, coupe rose. 

Sedimentary rocks with the highest arsenic concentrations largely consist of materials that readily sorb or contain arsenic, such as organic matter, iron (oxy)(hydr)oxides, clay minerals, and sulfide compounds. Arsenian pyrite and arsenic-sorbing organic matter are especially common in coals and shales. Ironstones and iron formations are mainly composed of hematite and other iron (oxy)(hydr)oxides that readily sorb or coprecipitate arsenic. Iron compounds also occur as cements in some sandstones. Although almost any type of sedimentary rock could contain arsenic-rich minerals precipitated by subsurface fluids (Section 3.6.4), many sandstones and carbonates consist almost entirely of minerals that by themselves retain very little arsenic namely, quartz in sandstones and dolomite and calcite in limestones. 

The iron compounds have been known for several centuries and valued as pigments. The name Prussian (Berlin) blue is given to the compound formed from a solution of a ferric salt and a ferrocyanide, while that obtained from a ferrous salt and a ferricyanide has been known as Turnbull s blue. It appears from Mbssbauer studies that both of these compounds are (hydrated) Fe4 [Pe (CN)6]3. with high-spin Fe and low-spin Fe in the ratio 4 3. There is also a soluble Prussian blue with the composition KFe[Fe(CN)6] which is also a ferrocyanide. Most, if not all, of the compounds we are discussing are hydrated we consider the water of hydration later. 

Name some common minerals that contain iron. Write the chemical formula for the iron compound in each. What is the oxidation number of iron in each substance ... 

Systematic names are easier and less ambiguous than common names. Whenever possible, we will use this system of nomenclature. The older, common names (-ous, -ic) are less specific furthermore, they often use the Latin names of the elements (for example, iron compounds use/err-, from ferrum, the Latin word for iron). 

In the binary ionic compounds considered earlier (Type I), the metal present forms only a single type of cation. That is, sodium forms only Na, calcium forms only Ca, and so on. However, as we will see in more detail later in the text, there are many metals that form more than one type of positive ion and thus form more than one type of ionic compound with a given anion. For example, the compound FeCl2 contains Fe ions, and the compound FeCl3 contains Fe ions. In a case such as this, the charge on the metal ion must be specified. The systematic names for these two iron compounds are iron(ll) chloride and iron(lll) chloride, respectively, where the Roman numeral indicates the charge of the cation. 

Albomycins, natural siderophores and antibiotics first isolated from Streptomyces griseus and named grisein in 1947. Some years later, another microbial iron-transport compound, named albomycin, was isolated from Streptomyces subtropicus which had the same structure as grisein. In 1982, the structure of the albomycins was firmly established. The linear tripeptide built of N -acetyl-N -hydroxy-L-omithine is the hexadentate, octahedral ligand for ferric ion responsible for intraceUular transport of iron. The albomycins are used for treatment of iron metabolism disorders [G. Benz et al., Angew. Chem. Int. Ed. 1982, 21, 527 G. Benz, Liebigs Ann. Chem. 1984, 1408]. 

You w3l nodoe that die compounds of iron are named ironfil) sulphate and irondll) sulphate to show which of its valencies iron is using in the compound. This is always done with tbe compounds of elements of variable valency. For valency and oxidation number, see Chapter 8, p. 72. 

As mentioned, in the older naming system, the metal that contains the lower number of outer-shell electrons ends with the sufBx ous. The metal that contains the higher number of outer-shell electrons ends with the sufQx ic. For example, iron has the possibility of two or three electrons in the outer shell. When iron II is used in a compound, the name for the iron is ferrous therefore, a salt compound containing iron II and chlorine would be called ferrous chloride. In this case, the ous indicates two electrons in the outer shell of the iron. In order to use this system, you must first know the possible numbers of outer-shell electrons to determine which is the higher and which is the lower number of electrons in the outer shell. For example, mercury can have one or two, copper one or two, iron two or three, etc. If iron III were used in a compound, the name would end in ic therefore, the iron 111 name would he ferric. If iron 111 were combined with chlorine, the name of the salt compound would be ferric chloride. 

A good example is bauxite, an ore named after Les Baux, in France, where it is found. But converting bauxite into pure aluminum is quite an involved process. Bauxite s reddish color is due mostly to iron compounds, which must be removed in order to obtain pure alumina, the white powder that is the key to isolating aluminum. No commercially viable method to convert bauxite to aluminum existed until the late 1800s, when... 

Analogous complexes of iron(ll), namely [Fe(QP)(H20)2l, 6, and [Fe(pQP)(H20)2l, 7, have been isolated as perchlorate salts and characterized with X-ray crystallography. The quaterpyridine unit in compound 7 is twisted about the two central pyridyl rings while those In 6 are almost coplanar. This feature may partly explain the smaller stability of 7 in aqueous solutions. 

For this treatment both pyro- and hydrometallurgical processes are available, the latter being the most frequently used and comprising leaching and iron precipitation steps. The processes are named after the precipitated iron compound. 

In 1876, Henry J.H. Fenton publicly announced that the use of a mixture of H2O2 and Fe " (thereafter so-called Fenton s reagent) allowed the destruction of an organic compound, namely, tartaric acid [1], Such discovery triggered an intense research to elucidate the mechanistic fundamentals and propose different variants and applications of the Fenton process. The possible formation of Fe(IV) as an active Fenton intermediate, as well as the modeling of the real structure of the iron aqua complexes, is still the subject of discussion [2, 3]. However, at present, it is quite well established that the classical Fenton s reaction (1) involves the production of highly oxidative hydroxyl radicals ( OH) in the bulk as the main reactive species, and its optimum pH value is 2.8-3.0 [1] ... 

Although there are three types of active sites in non-heme iron proteins, namely containing one, two, and four iron atoms per center, in the discussion above only tetrameric Fe-S species have been considered. This topic has been treated with some detail because these compounds meet properly the concept of cluster and are therefore clearly within the scope of this book. That is not the case for the di-iron species which form the 2Fe-2S active sites in the ferredoxins nor for the mononuclear center in the rubredoxins. However, in order to get a better understanding of the chemistry of the iron-sulfur proteins, an overview of the chemistry of the 2Fe-2S analogues is also outlined in this Section. 

Table 4. Model NACs compound names, one-electron reduction potentials ( EJO, carbon-normalized second-order rate constants (Icnom) for the reaction with Hyde County NOM, second-order rate constants for the reaction with an iron porphyrin (kpep), and apparent zero-order rate constants for reduction in an aquifer column under ferrogenic conditions (k bs)...

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