y 2) do not point toward neighboring atoms in the lattice, and therefore are not involved in metallic bonding. This happens because the orbitals of those two electrons (d z 2 and d x 2 −. Magnetite īelow its Curie point of 770 ☌ (1,420 ☏ 1,040 K), α-iron changes from paramagnetic to ferromagnetic: the spins of the two unpaired electrons in each atom generally align with the spins of its neighbors, creating an overall magnetic field.
Magnetization curves of 9 ferromagnetic materials, showing saturation. The inner core of the Earth is generally presumed to consist of an iron- nickel alloy with ε (or β) structure.
(Confusingly, the term "β-iron" is sometimes also used to refer to α-iron above its Curie point, when it changes from being ferromagnetic to paramagnetic, even though its crystal structure has not changed. It is supposed to have an orthorhombic or a double hcp structure. Some controversial experimental evidence exists for a stable β phase at pressures above 50 GPa and temperatures of at least 1500 K.
The higher-temperature γ-phase also changes into ε-iron, but does so at higher pressure. Above approximately 10 GPa and temperatures of a few hundred kelvin or less, α-iron changes into another hexagonal close-packed (hcp) structure, which is also known as ε-iron. The physical properties of iron at very high pressures and temperatures have also been studied extensively, because of their relevance to theories about the cores of the Earth and other planets. At 912 ☌ and below, the crystal structure again becomes the bcc α-iron allotrope. As it cools further to 1394 ☌, it changes to its γ-iron allotrope, a face-centered cubic (fcc) crystal structure, or austenite. As molten iron cools past its freezing point of 1538 ☌, it crystallizes into its δ allotrope, which has a body-centered cubic (bcc) crystal structure. The first three forms are observed at ordinary pressures. pressure for α iron at room temperatureĪt least four allotropes of iron (differing atom arrangements in the solid) are known, conventionally denoted α, γ, δ, and ε. Iron also forms many coordination compounds some of them, such as ferrocene, ferrioxalate, and Prussian blue have substantial industrial, medical, or research applications. Iron forms compounds in a wide range of oxidation states, −2 to +7. Iron shares many properties of other transition metals, including the other group 8 elements, ruthenium and osmium. Ĭhemically, the most common oxidation states of iron are iron(II) and iron(III). Iron is also the metal at the active site of many important redox enzymes dealing with cellular respiration and oxidation and reduction in plants and animals. To maintain the necessary levels, human iron metabolism requires a minimum of iron in the diet. These two proteins play essential roles in vertebrate metabolism, respectively oxygen transport by blood and oxygen storage in muscles. The body of an adult human contains about 4 grams (0.005% body weight) of iron, mostly in hemoglobin and myoglobin. electrolytic iron) are more resistant to corrosion. Unlike the oxides of some other metals that form passivating layers, rust occupies more volume than the metal and thus flakes off, exposing more fresh surfaces for corrosion. Iron reacts readily with oxygen and water to produce brown-to-black hydrated iron oxides, commonly known as rust. Pristine and smooth pure iron surfaces are a mirror-like silvery-gray. The iron and steel industry is thus very important economically, and iron is the cheapest metal, with a price of a few dollars per kilogram or pound. In the modern world, iron alloys, such as steel, stainless steel, cast iron and special steels, are by far the most common industrial metals, due to their mechanical properties and low cost.
That event is considered the transition from the Bronze Age to the Iron Age. Humans started to master that process in Eurasia during the 2nd millennium BCE and the use of iron tools and weapons began to displace copper alloys-in some regions, only around 1200 BCE. It is the fourth most common element in the Earth's crust, being mainly deposited by meteorites in its metallic state, with its ores also being found there.Įxtracting usable metal from iron ores requires kilns or furnaces capable of reaching 1,500 ☌ (2,730 ☏) or higher, about 500 ☌ (932 ☏) higher than that required to smelt copper. It is, by mass, the most common element on Earth, just ahead of oxygen (32.1% and 30.1%, respectively), forming much of Earth's outer and inner core.
#Iron charge series#
It is a metal that belongs to the first transition series and group 8 of the periodic table. Iron is a chemical element with the symbol Fe (from Latin ferrum 'iron') and atomic number 26.
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