Iron forms various oxide and hydroxide compounds; the most common are iron(II,III) oxide (Fe 3O 4), and iron(III) oxide (Fe 2O 3). Iron(II) oxide also exists, though it is unstable at room temperature. Despite their names, they are actually all non-stoichiometric compounds whose compositions may vary. [62] These oxides are the principal ores for the production of iron (see bloomery and blast furnace). They are also used in the production of ferrites, useful magnetic storage media in computers, and pigments. The best known sulfide is iron pyrite (FeS 2), also known as fool's gold owing to its golden luster. [58] It is not an iron(IV) compound, but is actually an iron(II) polysulfide containing Fe 2+ and S 2− Iron(III) chloride finds use in water purification and sewage treatment, in the dyeing of cloth, as a coloring agent in paints, as an additive in animal feed, and as an etchant for copper in the manufacture of printed circuit boards. [137] It can also be dissolved in alcohol to form tincture of iron, which is used as a medicine to stop bleeding in canaries. [138] Murakami, M.; Ohishi Y.; Hirao N.; Hirose K. (2012). "A perovskitic lower mantle inferred from high-pressure, high-temperature sound velocity data". Nature. 485 (7396): 90–94. Bibcode: 2012Natur.485...90M. doi: 10.1038/nature11004. PMID 22552097. S2CID 4387193.

Fe(−4), Ru(−4), and Os(−4) have been observed in metal-rich compounds containing octahedral complexes [MIn 6− xSn x]; Pt(−3) (as a dimeric anion [Pt–Pt] 6−), Cu(−2), Zn(−2), Ag(−2), Cd(−2), Au(−2), and Hg(−2) have been observed (as dimeric and monomeric anions; dimeric ions were initially reported to be [T–T] 2− for Zn, Cd, Hg, but later shown to be [T–T] 4− for all these elements) in La 2Pt 2In, La 2Cu 2In, Ca 5Au 3, Ca 5Ag 3, Ca 5Hg 3, Sr 5Cd 3, Ca 5Zn 3(structure (AE 2+) 5(T–T) 4−T 2−⋅4e −), Yb 3Ag 2, Ca 5Au 4, and Ca 3Hg 2; Au(–3) has been observed in ScAuSn and in other 18-electron half-Heusler compounds. See Changhoon Lee; Myung-Hwan Whangbo (2008). "Late transition metal anions acting as p-metal elements". Solid State Sciences. 10 (4): 444–449. Bibcode: 2008SSSci..10..444K. doi: 10.1016/j.solidstatesciences.2007.12.001. and Changhoon Lee; Myung-Hwan Whangbo; Jürgen Köhler (2010). "Analysis of Electronic Structures and Chemical Bonding of Metal-rich Compounds. 2. Presence of Dimer (T–T) 4– and Isolated T 2– Anions in the Polar Intermetallic Cr 5B 3-Type Compounds AE 5T 3 (AE = Ca, Sr; T = Au, Ag, Hg, Cd, Zn)". Zeitschrift für Anorganische und Allgemeine Chemie. 636 (1): 36–40. doi: 10.1002/zaac.200900421. The roses on the cover symbolize secrecy—a major theme of the series and fitting for the revelations of secrets in this installment. [7] Pernet-Fisher, J.; Day, J.M.D.; Howarth, G.H.; Ryabov, V.V.; Taylor, L.A. (2017). "Atmospheric outgassing and native-iron formation during carbonaceous sediment–basalt melt interactions". Earth and Planetary Science Letters. 460: 201–212. Bibcode: 2017E&PSL.460..201P. doi: 10.1016/j.epsl.2016.12.022.Wilkinson, G.; Rosenblum, M.; Whiting, M. C.; Woodward, R. B. (1952). "The Structure of Iron Bis-Cyclopentadienyl". J. Am. Chem. Soc. 74 (8): 2125–2126. doi: 10.1021/ja01128a527. Iron has four stable isotopes: 54Fe (5.845% of natural iron), 56Fe (91.754%), 57Fe (2.119%) and 58Fe (0.282%). Twenty-four artificial isotopes have also been created. Of these stable isotopes, only 57Fe has a nuclear spin (− 1⁄ 2). The nuclide 54Fe theoretically can undergo double electron capture to 54Cr, but the process has never been observed and only a lower limit on the half-life of 3.1×10 22 years has been established. [18] The chapter titles, like in The Infernal Devices, are all taken from poetry of the Victorian and Edwardian era that the characters would be familiar with.

Iron catalysts are traditionally used in the Haber–Bosch process for the production of ammonia and the Fischer–Tropsch process for conversion of carbon monoxide to hydrocarbons for fuels and lubricants. [135] Powdered iron in an acidic medium is used in the Bechamp reduction, the conversion of nitrobenzene to aniline. [136] Iron compounds Iron provided by dietary supplements is often found as iron(II) fumarate, although iron(II) sulfate is cheaper and is absorbed equally well. [137] Elemental iron, or reduced iron, despite being absorbed at only one-third to two-thirds the efficiency (relative to iron sulfate), [157] is often added to foods such as breakfast cereals or enriched wheat flour. Iron is most available to the body when chelated to amino acids [158] and is also available for use as a common iron supplement. Glycine, the least expensive amino acid, is most often used to produce iron glycinate supplements. [159] Dietary recommendationsis an extinct radionuclide of long half-life (2.6million years). [19] It is not found on Earth, but its ultimate decay product is its granddaughter, the stable nuclide 60Ni. [18] Much of the past work on isotopic composition of iron has focused on the nucleosynthesis of 60Fe through studies of meteorites and ore formation. In the last decade, advances in mass spectrometry have allowed the detection and quantification of minute, naturally occurring variations in the ratios of the stable isotopes of iron. Much of this work is driven by the Earth and planetary science communities, although applications to biological and industrial systems are emerging. [20] a b Audi, Georges; Bersillon, Olivier; Blachot, Jean; Wapstra, Aaldert Hendrik (2003), "The N UBASE evaluation of nuclear and decay properties", Nuclear Physics A, 729: 3–128, Bibcode: 2003NuPhA.729....3A, doi: 10.1016/j.nuclphysa.2003.11.001 Some iron in the high-temperature lower region of the furnace reacts directly with the coke: [114] 2 Fe 2 O 3 + 3 C ⟶ 4 Fe + 3 CO 2 {\displaystyle {\ce {2Fe2O3 + 3C -> 4Fe + 3CO2}}}

Chamati, Gaminchev (2014). "Dynamic stability of Fe under high pressure". Journal of Physics. IOP Publishing. 558 (1): 012013. Bibcode: 2014JPhCS.558a2013G. doi: 10.1088/1742-6596/558/1/012013. Klein, Cornelis and Cornelius S. Hurlbut, Jr. (1985) Manual of Mineralogy, Wiley, 20th ed, pp. 278–79 ISBN 0-471-80580-7 Enghag, Per (8 January 2008). Encyclopedia of the Elements: Technical Data – History – Processing – Applications. John Wiley & Sons. pp.190–91. ISBN 978-3-527-61234-5. Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp.1282–86. ISBN 978-0-08-022057-4. .

THE BRIGHT WEB

Iron is by far the most reactive element in its group; it is pyrophoric when finely divided and dissolves easily in dilute acids, giving Fe 2+. However, it does not react with concentrated nitric acid and other oxidizing acids due to the formation of an impervious oxide layer, which can nevertheless react with hydrochloric acid. [7] High-purity iron, called electrolytic iron, is considered to be resistant to rust, due to its oxide layer. In the far future of the universe, assuming that proton decay does not occur, cold fusion occurring via quantum tunnelling would cause the light nuclei in ordinary matter to fuse into 56Fe nuclei. Fission and alpha-particle emission would then make heavy nuclei decay into iron, converting all stellar-mass objects to cold spheres of pure iron. [27] Origin and occurrence in nature Cosmogenesis In the absence of an external source of magnetic field, the atoms get spontaneously partitioned into magnetic domains, about 10micrometers across, [17] such that the atoms in each domain have parallel spins, but some domains have other orientations. Thus a macroscopic piece of iron will have a nearly zero overall magnetic field. Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi: 10.1088/1674-1137/abddae.

Siegfried Pohl, Ulrich Bierbach, Wolfgang Saak; "FeI3SC(NMe2)2, a Neutral Thiourea Complex of Iron(III) Iodide", Angewandte Chemie International Edition in English (1989) 28 (6), 776-777. https://doi.org/10.1002/anie.198907761 Iron(III) oxide mixed with aluminium powder can be ignited to create a thermite reaction, used in welding large iron parts (like rails) and purifying ores. Iron(III) oxide and oxyhydroxide are used as reddish and ocher pigments. Wagner, Donald B. (1993). Iron and Steel in Ancient China. Brill. pp.335–340. ISBN 978-90-04-09632-5.The European Food Safety Authority (EFSA) refers to the collective set of information as Dietary Reference Values, with Population Reference Intake (PRI) instead of RDA, and Average Requirement instead of EAR. AI and UL defined the same as in United States. For women the PRI is 13mg/day ages 15–17 years, 16mg/day for women ages 18 and up who are premenopausal and 11mg/day postmenopausal. For pregnancy and lactation, 16mg/day. For men the PRI is 11mg/day ages 15 and older. For children ages 1 to 14 the PRI increases from 7 to 11mg/day. The PRIs are higher than the U.S. RDAs, with the exception of pregnancy. [161] The EFSA reviewed the same safety question did not establish a UL. [162] Further information: Ancient iron production The symbol for Mars has been used since antiquity to represent iron. The iron pillar of Delhi is an example of the iron extraction and processing methodologies of early India.