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Iron

Iron in Periodic Table

Iron (Fe), chemical element, silvery-white, lustrous, malleable, and ductile metal of Group 8 (VIIIB) of the periodic table, the most used and cheapest metal uses by the human civilization much later than copper, silver, and gold. In learning chemistry, the chemical element iron is included in the transition metals family due to the presence of incompletely d-orbitals in their atomic or ionic form.

The second most abundant metal, iron has chemical symbol Fe, atomic number 26, atomic weight 55.847, melting point 1538 °C, boiling point 2862 °C, density 7.874 gm/cm3, valence electron configuration [Ar] 3d6 4s2, and common oxidation number +2 and +3. The name iron comes from the old English while the symbol Fe comes from the Latin word Ferrum. Iron is the most magnetic substance among all elements and moderately chemically active metal in the earth’s environment. Iron occurs in nature by four stable isotopes like 54Fe (5.845 percent), 56Fe (91.754 percent), 57Fe (2.119 percent), and 58Fe (0.282 percent).

Iron (Fe), chemical element of Group 8 of periodic table with properties, uses of this cheapest metal for human civilization

History and Occurrence of Iron

Iron joined in the race of human civilization before copper, silver, and gold and was first used by our forefathers around 4000 B.C. The knowledge of extracting iron from its different types of ore developed in different countries at a long interval of time. In Egypt and Mesopotamia, the process was discovered about 2000 B.C. Early methods of heating ores with coal on windy sites yielded spongy metal shaped by prolonged hammering. The technique for making good quality metal was developed by using a furnace. In modern times, smelting furnaces have become well developed. Improvement of mechanical strength by making steel from iron ores was coming in the nineteenth century.

Iron is the second most abundant metal after aluminum and the fourth most abundant chemical element after oxygen, silicon, and aluminum in the earth’s crust occurring to an extent of more than 5 percent or 50,000 ppm. In the earth’s crust, the free metal is rare, terrestrial iron in basaltic rocks occurs in Greenland and carbonaceous sediments occurs in the United States (Missouri). About 0.5 percent of lunar soil consists of metallic iron, which means a vast quantity of Fe present on the moon’s surface.

Iron occurs mostly in oxide ores like red hematite (Fe2O3), brown hematite, or limonite (2F2O3, 3H2O), and magnetite (Fe2O3), other minerals included siderite (FeCO3), and pyrites (FeS2). Pyrites cannot be economical to produce Fe and hence pyrites are not considered an ore of Fe. The ores are found in different countries like China, Brazil, Australia, United States, and India, and 1000 million tonnes of iron are produced per year all over the world. The production of crude steel after 1996 over the world around 700 million tonnes.

Extraction

Iron is extracted through carbon reduction in a blast furnace. The ore, coke, and limestone (usually ratio 8:4:1) enter the top of the furnace while a blast of preheated air about 900 °C is brown through the holes near the bottom. The burning of coke produces heat near the base with the temperature near 2000 °C and fall gradually towards the top of the furnace (400 °C). Burning of carbon above 700 °C produces carbon monoxide which rises upward and reduces Fe2O3 and FeO. Some reduction is done by carbon. The limestone decomposes around 900 °C to give CaO which combines with silica to form slag (CaSiO3).

The molten slug and crude metal collect at the base of the blast furnace where they form separate layers and the slug floats on molten metal, preventing it from oxidation. These are drowned through separate holes and allowed to solidify in the sand mold to form pig or cast iron which contain impurities like carbon, silicon, phosphorus, sulfur, and manganese. When most of the impurities present in pig-Fe are removed, the pure commercial form of metal is formed, known as wrought iron.

Chemical Properties

Pure iron is chemically moderately active, silvery-white lustrous, malleable, ductile metal, and most magnetic substances among all periodic table elements. Iron has four allotropic crystal lattice like α-Fe (bcc ferromagnetic), β-Fe (bcc paramagnetic), γ-Fe (fcc paramagnetic), and δ-Fe (bcc paramagnetic). The finely divided metal is pyrophoric in the air at room temperature. Water can reacts above 500 °C liberating hydrogen and forming Fe2O3 and FeO.

In a heated finely divided state, iron reacts all the nonmetals (carbon, silicon, nitrogen, phosphorus, and hydrogen) to form solid metal-like compounds, Fe3C, Fe3Si, Fe3P, Fe4N, FeN, or binary ionic to covalent compounds like FeF3, FeCl3, FeS. The hard crystalline solid carbide Fe3C (cementite) is mainly responsible for the variation of properties of steel. In absence of oxygen, iron reacts with mineral acids (sulfuric acid, hydrochloric acid, or nitric acid) to give Fe(II) ion in solution.  Dilute alkali solutions and air-free water hardly attics Fe but hot concentrated alkali hydroxides attack it.

Chemistry and Compounds

In chemistry, iron has characteristic properties of transition metals with various oxidation states and various types of coordination and organometallic chemical compounds in different types of chemical bonding. +2 (ferrous) and +3 (ferric) oxidation states are the main oxidation states of iron to form a wide number of compounds in chemistry. In Fe (II), it forms simple compounds like oxides, halides (except iodine), and other salts, together with a large number of complex compounds. FeF3, FeCl3, and FeBr3 are the halides of Fe, formed by direct reaction of metals with respective halogens like fluorine, chlorine, and bromine.

Fe(II) is, in general, reducing in nature to form a large number of simple and complex compounds are quite stable in +2 state. The halides, nitrate, perchlorate, and sulfate are soluble in water but the hydroxide, carbonate, phosphate, and oxalate are sparingly soluble. It occurs in a higher oxidation state in purple potassium ferrate (KFeO4) with +6 oxidation state, obtained by oxidation of Fe(III) by hydrochloric acid.

Uses of Iron

Iron and steel are used mainly in the different types of structural units in modern civilization and civil engineering. There are different types of steel with different properties and uses, manufacture by alloyed iron with carbon and other chemical elements. Mild steel is most widely used in bridges, electricity pylons, bicycle chains, cutting tools, and rifle barrels. Iron is also used as a chemical catalyst in the Haber process for the production of ammonia, in small-scale production of hydrogen, it is used as a reducing agent.

Stainless steel is an important alloy of iron that contains at least 12 to 15 percent chromium and other metals such as nickel, molybdenum, titanium, and copper which resist corrosion and action of acids. It is widely used in architecture, bearings, cutlery, medicinal surgical instruments, and jewelry. Cast iron is another alloy that contains 3 to 5 percent carbon, widely used in pipes, valves, pumps, and the production of the magnet.

Biological Role of Iron

Iron is an essential non-toxic chemical element for all forms of life (plants and animals). A lot of iron ion is present in the hemoglobin of blood which carries oxygen from the lungs to the cell for the respiration of the body. The deficiency of iron in the human body causes anemia which is the most common neutralization disorder all over the world, in both developed and underdeveloped countries. Chronic blood loss, repeated pregnancy, and hookworm infarction may cause anemia in the human body. Anemia is characterized by a lower concentration of iron in hemoglobin of blood (<12mg/liter), causes retired growth, loss of appetite, sluggish metabolic activities, and dull or inactive attitude.