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Iron
*** Shopping-Tip: Iron
{{otheruses}}
{{Elementbox_header | number=26 | symbol=Fe | name=iron | left=
manganese .html">cobalt
_above=- | below=ruthenium|Ru | color1=#ffc0c0 | color2=black }}
{{Elementbox_series |
transition metals }}
{{Elementbox_groupperiodblock | group=8 | period=4 | block=d }}
{{Elementbox_appearance_img | Fe,26| lustrous metallic
with a grayish tinge }}
{{Elementbox_atomicmass_gpm |
1 E-26 kg 55.845List of elements by atomic mass (2) }}
{{Elementbox_econfig | [
argon Ar] 3d
6 4s
2 }}
{{Elementbox_epershell | 2, 8, 14, 2 }}
{{Elementbox_section_physicalprop | color1=#ffc0c0 | color2=black }}
{{Elementbox_phase |
solid }}
{{Elementbox_density_gpcm3nrt | 7.86 }}
{{Elementbox_densityliq_gpcm3mp | 6.98 }}
{{Elementbox_meltingpoint | k=1811 | c=1538 | f=2800 }}
{{Elementbox_boilingpoint | k=3134 | c=2861 | f=5182 }}
{{Elementbox_heatfusion_kjpmol | 13.81 }}
{{Elementbox_heatvaporiz_kjpmol | 340 }}
{{Elementbox_heatcapacity_jpmolkat25 | 25.10 }}
{{Elementbox_vaporpressure_katpa | 1728 | 1890 | 2091 | 2346 | 2679 | 3132 | comment= }}
{{Elementbox_section_atomicprop | color1=#ffc0c0 | color2=black }}
{{Elementbox_crystalstruct |
Body-centered cubicexcept between temperatures
1185 K and 1667 K when
it is a
face-centered cubic}}
{{Elementbox_oxistates | 2, '''3''', 4, 6
(
amphoteric oxide) }}
{{Elementbox_electroneg_pauling | 1.83 }}
{{Elementbox_ionizationenergies4 | 762.5 | 1561.9 | 2957 }}
{{Elementbox_atomicradius_pm |
1 E-10 m 140 }}
{{Elementbox_atomicradiuscalc_pm |
1 E-10 m 156 }}
{{Elementbox_covalentradius_pm |
1 E-10 m 125 }}
{{Elementbox_section_miscellaneous | color1=#ffc0c0 | color2=black }}
{{Elementbox_magnetic |
ferromagnetism ferromagnetic }}
{{Elementbox_eresist_ohmmat20 | 96.1 n}}
{{Elementbox_thermalcond_wpmkat300k | 80.4 }}
{{Elementbox_thermalexpansion_umpmkat25 | 11.8 }}
{{Elementbox_speedofsound_rodmpsatrt | (electrolytic)
5120 }}
{{Elementbox_youngsmodulus_gpa | 211 }}
{{Elementbox_shearmodulus_gpa | 82 }}
{{Elementbox_bulkmodulus_gpa | 170 }}
{{Elementbox_poissonratio | 0.29 }}
{{Elementbox_mohshardness | 4.0 }}
{{Elementbox_vickershardness_mpa | 608 }}
{{Elementbox_brinellhardness_mpa | 490 }}
{{Elementbox_cas_number | 7439-89-6 }}
{{Elementbox_isotopes_begin | isotopesof=iron | color1=#ffc0c0 | color2=black }}
{{Elementbox_isotopes_decay | mn=54 | sym=Fe | na=5.8% | hl=>3.1×10
22year y | dm=2ε capture |de=? | pn=54 | ps=
chromium Cr }}
{{Elementbox_isotopes_decay | mn=55 | sym=Fe | na=
synthetic radioisotope syn | hl=2.73 y | dm=ε capture | de=0.231 | pn=55 | ps=
manganese Mn }}
{{Elementbox_isotopes_stable | mn=56 | sym=Fe | na=91.72% | n=30 }}
{{Elementbox_isotopes_stable | mn=57 | sym=Fe | na=2.2% | n=31 }}
{{Elementbox_isotopes_stable | mn=58 | sym=Fe | na=0.28% | n=32 }}
{{Elementbox_isotopes_decay | mn=59 | sym=Fe | na=
synthetic radioisotope syn | hl=44.503 d | dm=
Beta decay β | de=1.565 | pn=59 | ps=
cobalt Co }}
{{Elementbox_isotopes_decay | mn=60 | sym=Fe | na=
synthetic radioisotope syn | hl=1.5E6 y | dm=
Beta decay β- | de=3.978 | pn=60 | ps=
cobalt Co }}
{{Elementbox_isotopes_end}}
{{Elementbox_footer | color1=#ffc0c0 | color2=black }}
'''Iron''' is a
chemical element with the symbol '''Fe''' (
Latin L.: Ferrum) and
atomic number 26. Iron is a
Group 8 element group 8 and
Period 4 element period 4 metal. Iron is notable for being the final element produced by
stellar nucleosynthesis, and thus the heaviest element which does not require a
supernova or similarly cataclysmic event for its formation. It is therefore the most abundant heavy metal in the universe.
Notable characteristics
Iron is the most abundant metal on
Earth, and is believed to be the tenth most abundant
chemical element element in the
universe. Iron is also the second most abundant (by mass, 34.6%) element making up the Earth; the concentration of iron in the various layers of the Earth ranges from high at the inner core to about 5% in the outer crust; it is possible the Earth's inner core consists of a single iron
crystal although it is more likely to be a mixture of iron and
nickel; the large amount of iron in the Earth is thought to contribute to its
Earth's magnetic field magnetic field.
Iron is a
metal extracted from iron ore, and is hardly ever found in the free (elemental) state. In order to obtain elemental iron, the impurities must be removed by chemical
reduction (chemistry) reduction. Iron is used in the production of
steel, which is not an element but an
alloy, a solution of different metals (and some non-metals, particularly
carbon).
Nuclei of iron have some of the highest binding energies per nucleon, surpassed only by the
nickel isotope 62Ni. The universally most abundant of the highly stable nucleides is, however,
56Fe. This is formed by nuclear fusion in the stars. Although a further tiny energy gain could be extracted by synthesizing
62Ni, conditions in stars are not right for this process to be favoured. When a very large star contracts at the end of its life, internal pressure and temperature rise, allowing the star to produce progressively heavier elements, despite these being less stable than the elements around mass number 60 (the "iron group"). This leads to a
supernova.
Some cosmological models with an open universe predict that there will be a phase where as a result of slow fusion and fission reactions, everything will become iron.
Applications
Iron is the most used of all the metals, comprising 95 percent of all the metal tonnage produced worldwide. Its combination of low cost and high strength make it indispensable, especially in applications like
automobiles, the
hull (ship) hulls of large
ships, and structural components for
buildings.
Steel is the best known alloy of iron, and some of the forms that iron takes include:
*
Pig iron has 4% – 5% carbon and contains varying amounts of contaminants such as
sulfur,
silicon and
phosphorus. Its only significance is that of an intermediate step on the way from
iron ore to
cast iron and
steel.
*
Cast iron contains 2% – 4.0%
carbon , 1% – 6%
silicon , and small amounts of
manganese. Contaminants present in pig iron that negatively affect the material properties, such as sulfur and phosphorus, have been reduced to an acceptable level. It has a melting point in the range of 1420–1470 K, which is lower than either of its two main components, and makes it the first product to be melted when carbon and iron are heated together. Its mechanical properties vary greatly, dependent upon the form
carbon takes in the alloy. 'White' cast irons contain their carbon in the form of
cementite, or iron carbide. This hard, brittle compound dominates the mechanical properties of white cast irons, rendering them hard, but unresistant to shock. The broken surface of a white cast iron is full of fine facets of the broken carbide, a very pale, silvery, shiny material, hence the appellation. In
grey iron, the carbon exists free as fine flakes of
graphite , and also, renders the material brittle due to the stress-raising nature of the sharp edged flakes of graphite. A newer variant of grey iron, referred to as
ductile iron is specially treated with trace amounts of
magnesium to alter the shape of graphite to sheroids, or nodules, vastly increasing the toughness and strength of the material.
*
Carbon steel contains between 0.4% and 1.5%
carbon, with small amounts of
manganese,
sulfur,
phosphorus, and
silicon.
*
Wrought iron contains less than 0.2% carbon. It is a tough, malleable product, not as fusible as pig iron. It has a very small amount of carbon, a few tenths of a percent. If honed to an edge, it loses it quickly. Wrought iron is characterised, especially in old samples, by the presence of fine 'stringers' or filaments of
slag entrapped in the metal.
*
Alloy steels contain varying amounts of carbon as well as other metals, such as
chromium,
vanadium,
molybdenum,
nickel,
tungsten, etc. They are used for structural purposes, as their alloy content raises their cost and necessitates justification of their use. Recent developments in ferrous metallurgy have produced a growing range of microalloyed steels, also termed 'HSLA' or high-strength, low alloy steels, containing tiny additions to produce high strengths and often spectacular toughness at minimal cost.
*
Iron(III) oxides are used in the production of
magnetic storage in computers. They are often mixed with other compounds, and retain their magnetic properties in solution.
History
The first signs of use of iron come from the
Sumerians and the
Egyptians, where around 4000 BC, a few items, such as the tips of spears, daggers and ornaments, were being fashioned from iron recovered from
meteorites. Because meteorites fall from the sky some linguists have conjectured that the English word ''iron'' (OE ''Ä«sern''), which has cognates in many northern and western European languages, derives from the
Etruscan language Etruscan ''aisar'' which means "the gods". Even if this is not the case, the word is likely a loan into pre-
Proto-Germanic from
Celtic languages Celtic or
Italic languages Italic (Krahe
Indogermanische Forschungen IF 46:184f. compares
Old Irish,
Illyrian,
Venetic and
Messapic forms).
By 3500 BC to 2000 BC, increasing numbers of smelted iron objects (distinguishable from meteoric iron by the lack of nickel in the product) appear in
Mesopotamia,
Anatolia, and
Egypt. However, their use appears to be ceremonial, and iron was an expensive metal, more expensive than
gold. In the
Iliad, weaponry is mostly
bronze, but iron ingots are used for trade. Some resources (see the reference ''What Caused the Iron Age?'' below) suggest that iron was being created then as a by-product of
copper refining, as
sponge iron, and was not reproducible by the metallurgy of the time. By 1600 BC to 1200 BC, iron was used increasingly in the Middle East, but did not supplant the dominant use of
bronze.
Image:Axe of iron from Swedish Iron Age, found at Gotland, Sweden.jpg thumb|left|250px|Axe of iron from Swedish Iron Age, found at Gotland, Sweden.
In the period from the 12th to 10th century BC, there was a rapid transition in the Middle East from bronze to iron tools and weapons. The critical factor in this transition does not appear to be the sudden onset of a superior ironworking technology, but instead the disruption of the supply of
tin. This period of transition, which occurred at different times in different parts of the world, is the ushering in of an age of civilization called the
Iron Age.
Image:Mars symbol.png right|50px|Symbol of Iron
The common
alchemical symbol for iron, the metal of weapons, was that of
Mars (god) Mars, the god of war.
Concurrent with the transition from bronze to iron was the discovery of ''carburization'', which was the process of adding carbon to the irons of the time. Iron was recovered as sponge iron, a mix of iron and slag with some carbon and/or carbide, which was then repeatedly hammered and folded over to free the mass of slag and oxidise out carbon content, so creating the product wrought iron. Wrought iron was very low in carbon content and was not easily hardened by quenching. The people of the Middle East found that a much harder product could be created by the long term heating of a wrought iron object in a bed of
charcoal, which was then quenched in water or oil. The resulting product, which had a surface of
steel, was harder and less brittle than the bronze it began to replace.
In China the first irons used were also meteoric iron, with archeological evidence for items made of wrought iron appearing in the northwest, near Xinjiang, in the 8th century BC. These items were made of wrought iron, created by the same processes used in the Middle East and Europe, and were thought to be imported by non-Chinese people.
In the later years of the
Zhou Dynasty (ca 550 BC), a new iron manufacturing capability began because of a highly developed
kiln technology. Producing
blast furnace blast furnaces capable of temperatures exceeding 1300 K, the Chinese developed the manufacture of
cast iron cast, or
pig iron.
Iron was used in India as early as 250 BCE. The famous iron pillar in the
Qutb complex in
Delhi is made of very pure iron (98%) and has not rusted or eroded till this day.
Image:Maramec Iron Works furnace a.jpg Missouri.html" title="Meaning of thumb thumb|right|250px|This blast furnace in eastern [[Missouri consumed up to 11,000 tons of ore and 16,000
Wood fuel#Firewood cords of wood annually from 1827 to 1891..html" title="Meaning of right|250px|This blast furnace in eastern [[Missouri">thumb|right|250px|This blast furnace in eastern [[Missouri consumed up to 11,000 tons of ore and 16,000
Wood fuel#Firewood cords of wood annually from 1827 to 1891.">right|250px|This blast furnace in eastern [[Missouri">thumb|right|250px|This blast furnace in eastern [[Missouri consumed up to 11,000 tons of ore and 16,000
Wood fuel#Firewood cords of wood annually from 1827 to 1891.
If iron ores are heated with carbon to 1420–1470 K, a molten liquid is formed, an
alloy of about 96.5% iron and 3.5% carbon. This product is strong, can be cast into intricate shapes, but is too brittle to be worked, unless the product is ''decarburized'' to remove most of the carbon. The vast majority of Chinese iron manufacture, from the Zhou dynasty onward, was of cast iron. Iron, however, remained a pedestrian product, used by farmers for hundreds of years, and did not really affect the nobility of China until the
Qin dynasty (ca 221 BC).
Cast iron development lagged in Europe, as the smelters could only achieve temperatures of about 1000 K. Through a good portion of the Middle Ages, in Western Europe, iron was still being made by the working of sponge iron into wrought iron. Some of the earliest casting of iron in Europe occurred in
Sweden, in two sites, Lapphyttan and Vinarhyttan, between 1150 and 1350 AD. There are suggestions by scholars that the practice may have followed the
Mongols across
Russia to these sites, but there is no clear proof of this hypothesis. In any event, by the late fourteenth century, a market for cast iron goods began to form, as a demand developed for cast iron cannonballs.
Early iron
smelting (as the process is called) used
charcoal as both the heat source and the reducing agent. In 18th century England, wood supplies ran down and
coke (fuel) coke, a fossil fuel, was used as an alternative. This innovation by
Abraham Darby I Abraham Darby supplied the energy for the
Industrial Revolution.
Occurrence
Image:IronInRocksMakeRiverRed.jpg thumb|right|The red appearance of this water is due to iron in the rocks.
Iron is one of the most common elements on Earth, making up about 5% of the Earth's crust. Most of this iron is found in various
iron oxides, such as the minerals
hematite,
magnetite, and
taconite. The
earth's core is believed to consist largely of a metallic iron-
nickel alloy. About 5% of the
meteorites similarly consist of iron-nickel alloy. Although rare, these are the major form of natural metallic iron on the earth's surface.
Iron is also one of the least
reactive metals, and therefore, it is sometimes found pure in
nature.
''See also
:category:Iron minerals iron minerals.''
Extraction from ore
Image:Iron-Making.jpg thumb|270px|How Iron was extracted in the 19th Century
Industrially, iron is extracted from its
ores, principally
hematite (nominally Fe
2O
3) and
magnetite (Fe
3O
4) by a
carbothermic reaction (reduction with
carbon) in a
blast furnace at temperatures of about 2000°C. In a blast furnace, iron ore, carbon in the form of
coke (fuel) coke, and a ''flux'' such as
limestone are fed into the top of the furnace, while a blast of heated
Earth's atmosphere air is forced into the furnace at the bottom.
In the furnace, the
coke (fuel) coke reacts with
oxygen in the air blast to produce
carbon monoxide:
:6
carbon C + 3
oxygen O2 → 6
carbon monoxide CO
The carbon monoxide reduces the iron ore (in the
chemical equation below, hematite) to molten iron, becoming
carbon dioxide in the process:
:6
carbon monoxide CO + 2
hematite Fe2O3 → 4 Fe + 6
carbon dioxide CO2
The flux is present to melt impurities in the ore, principally
silicon dioxide sand and other
silicates. Common fluxes include limestone (principally
calcium carbonate) and dolomite (
magnesium carbonate). Other fluxes may be used depending on the impurities that need to be removed from the ore. In the heat of the furnace the limestone flux decomposes to
calcium oxide (quicklime):
:
calcium carbonate CaCO3 →
calcium oxide CaO +
carbon dioxide CO2
Then calcium oxide combines with silicon dioxide to form a ''slag''.
:
calcium oxide CaO +
silicon dioxide SiO2 →
wollastonite CaSiO3
The slag melts in the heat of the furnace, which silicon dioxide would not have. In the bottom of the furnace, the molten slag floats on top of the more dense liquid iron, and spouts in the side of the furnace may be opened to drain off either the iron or the slag. The iron, once cooled, is called
pig iron, while the slag can be used as a material in
road construction or to improve mineral-poor soils for
agriculture.
Approximately 1100Mt (million tons) of iron ore was produced in the world
in 2000, with a gross market value of approximately 25 billion US dollars. While ore production occurs in 48 countries, the five largest producers were China, Brazil, Australia, Russia and India, accounting for 70% of world iron ore production. The 1100Mt of iron ore was used to produce approximately 572Mt of pig iron.
Compounds
Image:LightningVolt Iron Ore Pellets.jpg iron ore.html" title="Meaning of thumb thumb|right|250px|This heap of [[iron ore pellets will be used in
steel production..html" title="Meaning of right|250px|This heap of [[iron ore">thumb|right|250px|This heap of [[iron ore pellets will be used in
steel production.">right|250px|This heap of [[iron ore">thumb|right|250px|This heap of [[iron ore pellets will be used in
steel production.
Common
oxidation states of iron include:
* the '''Iron(-II)''' state, Fe
2- (e.g. Fe(CO)
42-,Fe(CO)
2(NO)
2.
* the '''Iron(-I)''' state, Fe
2(CO)
42-.
* the '''Iron(0)''' state, Fe(CO)
5, Fe(PF
3)
5.
* the '''Iron(I)''' state, [Fe(H
2O)
5NO]
2+.
* the '''Iron(II)''' state, Fe
2+, previously ''ferrous'' is very common.
* the '''Iron(III)''' state, Fe
3+, previously ''ferric'', is also very common, for example in
rust.
* the '''Iron(IV)''' state, Fe
4+, previously ''ferryl'', stabilized in some enzymes (e.g.
peroxidase peroxidases).
Note that despite the chemical formula, the iron in the common
pyrite is '''not''' in the +4 oxidation state; the sulfur is in the -1 oxidation state.
* the '''Iron(VI)''' state, Fe
6+ is also known, if rare, in
potassium ferrate.
Iron carbide Fe
3C is known as
cementite.
''See also
:category:Iron compounds Iron compounds.''
Isotopes
Naturally occurring iron consists of four
isotopes: 5.845% of radioactive
54Fe (half-life: >3.1E22 years), 91.754% of stable
56Fe, 2.119% of stable
57Fe and 0.282% of stable
58Fe.
60Fe is an extinct
radionuclide of long
half-life (1.5 million years). Much of the past work on measuring the isotopic composition of Fe has centered on determining
60Fe variations due to processes accompanying
nucleosynthesis (i.e.,
meteorite studies) and ore formation.
The isotope
56Fe is of particular interest to nuclear scientists. A common misconception is that this isotope represents the most stable nucleus possible, and that it thus would be impossible to perform fission or fusion on
56Fe and still liberate energy. This is not true, as both
62Ni and
58Fe are more stable.
In phases of the meteorites ''Semarkona'' and ''Chervony Kut'' a correlation between the concentration of
60Nickel Ni, the
daughter product of
60Fe, and the abundance of the stable iron isotopes could be found which is evidence for the existence of
60Fe at time formation of solar system. Possibly the energy released by the decay of
60Fe contributed, together with the energy released by decay of the radionuclide
26Aluminium Al, to the remelting and
planetary differentiation differentiation of
asteroids after their formation 4.6 billion years ago. The abundance of
60nickel Ni present in
extraterrestrial material may also provide further insight into the origin of the
solar system and its early history.
Of the stable isotopes, only
57Fe has a nuclear
spin (physics) spin (−1/2). For this reason,
57Fe has application as a spin isotope in chemistry and biochemistry.
Biological role
Iron is essential to all
organisms, except for a few
bacterium bacteria. It is mostly stably incorporated in the inside of
metalloproteins, because in exposed or in free form it causes production of
free radicals that are generally toxic to cells. To say that iron is free doesn't mean that it is free floating in the bodily fluids. Iron binds avidly to virtually all biomolecules so it will adhere nonspecifically to
cell membranes,
nucleic acids,
proteins etc.
Many animals incorporate iron into the
heme complex, an essential component of
cytochromes, which are proteins involved in
redox reactions (including but not limited to
cellular respiration), and of oxygen carrying proteins
hemoglobin and
myoglobin. Inorganic iron involved in redox reactions is also found in the
iron-sulfur clusters of many
enzymes, such as
nitrogenase (involved in the synthesis of
ammonia from
nitrogen and
hydrogen) and
hydrogenase. A class of
non-heme iron proteins is responsible for a wide range of functions within several life forms, such as
enzymes methane monooxygenase (oxidizes
methane to
methanol),
ribonucleotide reductase (reduces
ribose to
deoxyribose;
DNA replication DNA biosynthesis),
hemerythrins (
oxygen transport and fixation in
marine biology#other sea life marine invertebrates) and
purple acid phosphatase (
hydrolysis of
phosphate esters). When the body is fighting a bacterial
infection, the body sequesters iron inside of cells (mostly stored in the storage molecule
ferritin) so that it cannot be used by bacteria.
Iron distribution is heavily regulated in
mammals, as a defense against bacterial infection and also because of the potential biological toxicity of iron. The iron absorbed from the
duodenum binds to transferrin, and is carried by
blood to different
cell (biology) cells. There it gets by an as yet unknown mechanism incorporated into target proteins. [http://www.plosbiology.org/plosonline/?request=get-document&doi=10.1371%2Fjournal.pbio.0000079]. A lengthier article on the system of human iron regulation can be found in the article on
human iron metabolism.
Dietary sources
Good sources of dietary iron include
meat,
fish,
poultry,
lentils,
beans,
leaf vegetables,
tofu,
chickpeas,
black-eyed pea,
strawberry strawberries and
farina (food) farina.
Iron provided by
dietary supplements is often found as
Ferrous fumarate Iron (II) fumarate. The
Recommended Dietary Allowance RDA for iron varies considerably based on the age, gender, and source of dietary iron (
heme-based iron has higher
bioavailability)[http://www.iom.edu/Object.File/Master/7/294/0.pdf]. Also note the section below on
#Precautions precautions.
Metallic iron filings are added to some
breakfast cereals and listed in the ingredients as "reduced iron" ("reduced" referring to
redox chemistry). If the cereal is crushed, the iron filings can be separated with a magnet.
Precautions
Excessive iron is toxic to humans, because excess ferrous iron reacts with
peroxides in the body, producing
free radicals. Iron becomes toxic when it exceeds the amount of
transferrin needed to bind free iron. In excess, uncontrollable quantities of free radicals are produced.
human iron metabolism Iron uptake is tightly regulated by the human body, which has no physiologic means of excreting iron and regulates iron solely by regulating uptake. However, too much ingested iron can damage the cells of the
gastrointestinal tract directly, and may enter the bloodstream by damaging the cells that would otherwise regulate its entry. Once there, it causes damage to cells in the
heart,
liver and elsewhere. This can cause serious problems, including the potential of death from overdose, and long-term organ damage in survivors.
Humans experience iron toxicity above 20 milligrams of iron for every kilogram of weight, and 60 milligrams per kilogram is a lethal dose.[http://www.emedicine.com/emerg/topic285.htm] Over-consumption of iron, often the result of children eating large quantitities of
ferrous sulfate tablets intended for adult consumption, is the most common toxicological cause of death in children under six. The
Dietary Reference Intake DRI lists the Tolerable Upper Intake Level (UL) for adults as 45
milligram mg/day. For children under fourteen years old the UL is 40 mg/day.
If iron intake is excessive
iron overload disorders can sometimes result, such as
hemochromatosis. Iron overload disorders require a genetic inability to regulate iron uptake; however, many people have a genetic susceptibility to iron overload without realizing it and without knowing a family history of the problem. For this reason, people should not take iron supplements unless they suffer from
iron deficiency (medicine) iron deficiency and have consulted a doctor.
Blood donation Blood donors are at special risk of low iron levels and are often recommended to supplement their iron intake.
The medical management of iron toxicity is complex. One element of the medical approach is a specific
chelator chelating agent called deferoxamine, used to bind and expel excess iron from the body in case of iron toxicity.
References
-
Los Alamos National Laboratory — Iron
External links
{{wiktionarypar|iron}}
{{Commons|Iron}}
-
WebElements.com – Iron
-
It's Elemental – Iron
-
The Most Tightly Bound Nuclei
Category:Iron
Category:Chemical elements Iron
Category:Transition metals
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{{Link FA|eo}}
{{Link FA|pt}}
{{Link FA|ru}}
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zh:é“?
Iron Fe{{qif|test={{{1|}}}|then=
{{{1}}}}}
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Category:Chemical elements
Category:Transition metals
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*** Shopping-Tip: Iron
