chemical task

8/2/2019 Chemical Task

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CHEMICAL TASK

IRON

BY:

DIMAS GUNTUR . A . (07)

ERDIANSYAH (08)

FELA FITRIN (11)


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PREFACE

All praise to Allah, and for it give, we can to make a checimal task about

IRON with fluent and nothing a hindrance.

In this book, we will to explaining about IRON which is the one of the

element in the world.

Says to finish, Wasallamualaikum Wr.Wb.

Malang, November 2011

Writer


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CONTENTS


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Iron is a chemical element with the symbol Fe (from Latin:ferrum) and atomic number 26. It isa metal in the first transition series. It is the most common element (by mass) forming the planetEarth as a whole, forming much of Earth's outer and inner core. It is the fourth most common

element in the Earth's crust. Iron's very common presence in rocky planets like Earth is due to its

abundant production as a result of fusion in high-mass stars, where the production ofnickel-56

(which decays to iron) is the last nuclear fusion reaction that is exothermic. This allowsradioactive nickel to become the last element to be produced before collapse of a supernova

leads to events that scatters this precursor radionuclide of iron into space.

Like other Group 8 elements, iron exists in a wide range ofoxidation states, 2 to + 6, although

+2 and +3 are the most common. Elemental iron occurs in meteoroids and other low oxygenenvironments, but is reactive to oxygen and water. Fresh iron surfaces appear lustrous silvery-

gray, but oxidize in normal air to give iron oxides, also known as rust. Unlike many other metals

which form passivating oxide layers, iron oxides occupy more volume than iron metal, and thus

iron oxides flake off and expose fresh surfaces for corrosion.

Iron metal has been used since ancient times, though lower-melting copper alloys were used firstin history. Pure iron is soft (softer than aluminium), but is unobtainable by smelting. Thematerial is significantly hardened and strengthened by impurities from the smelting process, such

as carbon. A certain proportion of carbon (between 0.2% and 2.1%) produces steel, which may

be up to 1000 times harder than pure iron. Crude iron metal is produced in blast furnaces, whereore is reduced by coke to cast iron, which has a high carbon content. Further refinement with

oxygen reduces the carbon content to the correct proportion to make steel. Steels and low carbon

iron alloys with other metals (alloy steels) are by far the most common metals in industrial use,

due to their great range of desirable properties.

Iron chemical compounds, which include ferrous and ferric compounds, have many uses. Iron

oxide mixed with aluminium powder can be ignited to create a thermite reaction, used in weldingand purifying ores. It forms binary compounds with the halogens and the chalcogens. Among its

organometallic compounds, ferrocene was the first sandwich compound discovered.

Iron plays an important role in biology, forming complexes with molecular oxygen in

hemoglobin and myoglobin; these two compounds are common oxygen transport proteins in

vertebrates. Iron is also the metal used at the active site of many important redox enzymesdealing with cellular respiration and oxidation and reduction in plants and animals.
http://en.wikipedia.org/wiki/Chemical_elementhttp://en.wikipedia.org/wiki/Latin_languagehttp://en.wikipedia.org/wiki/Atomic_numberhttp://en.wikipedia.org/wiki/Metalhttp://en.wikipedia.org/wiki/First_transition_serieshttp://en.wikipedia.org/wiki/Outer_corehttp://en.wikipedia.org/wiki/Inner_corehttp://en.wikipedia.org/wiki/Abundance_of_elements_in_Earth%27s_crusthttp://en.wikipedia.org/wiki/Nickel-56http://en.wikipedia.org/wiki/Nuclear_fusion_reactionhttp://en.wikipedia.org/wiki/Exothermichttp://en.wikipedia.org/wiki/Type_II_supernovahttp://en.wikipedia.org/wiki/Precursor_%28chemistry%29http://en.wikipedia.org/wiki/Radionuclidehttp://en.wikipedia.org/wiki/Group_8_elementhttp://en.wikipedia.org/wiki/Oxidation_statehttp://en.wikipedia.org/wiki/Oxidation_statehttp://en.wikipedia.org/wiki/Meteoroidhttp://en.wikipedia.org/wiki/Iron_oxidehttp://en.wikipedia.org/wiki/Rusthttp://en.wikipedia.org/wiki/Aluminiumhttp://en.wikipedia.org/wiki/Carbonhttp://en.wikipedia.org/wiki/Steelhttp://en.wikipedia.org/wiki/Blast_furnacehttp://en.wikipedia.org/wiki/Coke_%28fuel%29http://en.wikipedia.org/wiki/Cast_ironhttp://en.wikipedia.org/wiki/Alloyhttp://en.wikipedia.org/wiki/Alloy_steelhttp://en.wikipedia.org/wiki/Thermitehttp://en.wikipedia.org/wiki/Halogenshttp://en.wikipedia.org/wiki/Chalcogenshttp://en.wikipedia.org/wiki/Ferrocenehttp://en.wikipedia.org/wiki/Sandwich_compoundhttp://en.wikipedia.org/wiki/Hemoglobinhttp://en.wikipedia.org/wiki/Myoglobinhttp://en.wikipedia.org/wiki/Oxygen_transporthttp://en.wikipedia.org/wiki/Redoxhttp://en.wikipedia.org/wiki/Cellular_respirationhttp://en.wikipedia.org/wiki/Cellular_respirationhttp://en.wikipedia.org/wiki/Redoxhttp://en.wikipedia.org/wiki/Oxygen_transporthttp://en.wikipedia.org/wiki/Myoglobinhttp://en.wikipedia.org/wiki/Hemoglobinhttp://en.wikipedia.org/wiki/Sandwich_compoundhttp://en.wikipedia.org/wiki/Ferrocenehttp://en.wikipedia.org/wiki/Chalcogenshttp://en.wikipedia.org/wiki/Halogenshttp://en.wikipedia.org/wiki/Thermitehttp://en.wikipedia.org/wiki/Alloy_steelhttp://en.wikipedia.org/wiki/Alloyhttp://en.wikipedia.org/wiki/Cast_ironhttp://en.wikipedia.org/wiki/Coke_%28fuel%29http://en.wikipedia.org/wiki/Blast_furnacehttp://en.wikipedia.org/wiki/Steelhttp://en.wikipedia.org/wiki/Carbonhttp://en.wikipedia.org/wiki/Aluminiumhttp://en.wikipedia.org/wiki/Rusthttp://en.wikipedia.org/wiki/Iron_oxidehttp://en.wikipedia.org/wiki/Meteoroidhttp://en.wikipedia.org/wiki/Oxidation_statehttp://en.wikipedia.org/wiki/Group_8_elementhttp://en.wikipedia.org/wiki/Radionuclidehttp://en.wikipedia.org/wiki/Precursor_%28chemistry%29http://en.wikipedia.org/wiki/Type_II_supernovahttp://en.wikipedia.org/wiki/Exothermichttp://en.wikipedia.org/wiki/Nuclear_fusion_reactionhttp://en.wikipedia.org/wiki/Nickel-56http://en.wikipedia.org/wiki/Abundance_of_elements_in_Earth%27s_crusthttp://en.wikipedia.org/wiki/Inner_corehttp://en.wikipedia.org/wiki/Outer_corehttp://en.wikipedia.org/wiki/First_transition_serieshttp://en.wikipedia.org/wiki/Metalhttp://en.wikipedia.org/wiki/Atomic_numberhttp://en.wikipedia.org/wiki/Latin_languagehttp://en.wikipedia.org/wiki/Chemical_element


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Besi adalah unsur kimia dengan simbol Fe (dari bahasa Latin: zat besi) dan nomor atom 26. Ini

adalah logam dalam seri transisi pertama. Ini adalah elemen yang paling umum (massa)

membentuk planet Bumi secara keseluruhan, banyak membentuk inti bumi luar dan dalam. Ini

adalah elemen yang paling umum keempat dalam kerak bumi. Kehadiran besi sangat umum diplanet berbatu seperti Bumi adalah karena produksi berlimpah sebagai hasil dari fusi di bintang-

bintang bermassa tinggi, dimana produksi nikel-56 (yang meluruh menjadi zat besi) adalah

reaksi fusi nuklir yang terakhir eksotermik. Hal ini memungkinkan nikel radioaktif untukmenjadi elemen terakhir yang diproduksi sebelum runtuhnya supernova mengarah ke peristiwa

yang menyebarkan ini prekursor radionuklida dari besi ke ruang angkasa.

Seperti Kelompok lainnya 8 unsur, zat besi ada di berbagai negara oksidasi, -2 ke + 6, meskipun

+2 dan +3 adalah yang paling umum. Unsur besi terjadi pada meteoroid dan lingkungan oksigen

rendah, tetapi reaktif terhadap oksigen dan air. Permukaan besi berkilau keperakan muncul segar

abu-abu, namun teroksidasi di udara normal untuk memberikan oksida besi, juga dikenal sebagai

karat. Tidak seperti logam lain yang membentuk lapisan oksida pasivator, oksida besi menempativolume lebih dari logam besi, dan dengan demikian besi oksida mengelupas off dan mengekspos

permukaan segar untuk korosi.

Besi logam telah digunakan sejak zaman kuno, meskipun lebih rendah-lebur paduan tembaga

digunakan pertama dalam sejarah. Besi murni yang lunak (lembut dari aluminium), tapi tak dpt

diperoleh dengan peleburan. Materi yang signifikan mengeras dan diperkuat dengan kotoran dariproses peleburan, seperti karbon. Sebagian tertentu dari karbon (antara 0,2% dan 2,1%)

memproduksi baja, yang mungkin sampai 1000 kali lebih keras dari besi murni. Logam besi

mentah yang diproduksi di tanur tiup, dimana bijih dikurangi dengan kokas untuk melemparkanbesi, yang memiliki kandungan karbon tinggi. Perbaikan lebih lanjut dengan oksigen mengurangi

kandungan karbon dengan proporsi yang benar untuk membuat baja. Baja dan paduan besikarbon rendah dengan logam lain (baja paduan) yang jauh logam yang paling umum digunakan

industri, karena berbagai besar mereka sifat yang diinginkan.

Senyawa kimia besi, yang meliputi senyawa besi dan besi, memiliki banyak kegunaan. Besi

oksida dicampur dengan bubuk aluminium dapat dinyalakan untuk menciptakan reaksi termit,yang digunakan dalam pengelasan dan bijih memurnikan. Ini membentuk senyawa biner dengan

halogen dan chalcogens. Diantara senyawa organologam nya, ferrocene adalah senyawa

sandwich yang pertama kali ditemukan.

Besi memainkan peran penting dalam biologi, membentuk kompleks dengan molekul oksigen di

hemoglobin dan mioglobin, dua senyawa adalah protein transportasi umum oksigen dalamvertebrata. Besi juga merupakan logam yang digunakan pada situs aktif enzim banyak redokspenting berurusan dengan respirasi seluler dan oksidasi dan reduksi pada tumbuhan dan hewan.


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Contents

[hide]

1 Characteristics
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o 1.1 Mechanical propertieso 1.2 Phase diagram and allotropeso 1.3 Isotopeso 1.4 Nucleosynthesiso 1.5 Occurrence

1.5.1 Planetary occurrence 1.5.2 In-use stocks in society

2 Chemistry and compoundso 2.1 Binary compoundso 2.2 Coordination and organometallic compounds

3 Historyo 3.1 Wrought irono 3.2 Cast irono 3.3 Steelo 3.4 Foundations of modern chemistryo 3.5 Recent discoveries

4 Industrial productiono 4.1 Blast furnaceo 4.2 Direct iron reductiono 4.3 Further processes

5 Applicationso 5.1 Metallurgicalo 5.2 Of compounds

6 Biological roleo 6.1 Bioinorganic compoundso 6.2 Health and dieto 6.3 Uptake and storageo

6.4 Regulation of uptakeo 6.5 Permeable reactive barriers

7 Precautions 8 See also 9 References 10 Books 11 External links

Characteristics

Mechanical properties

Characteristic values oftensile strength(TS) andBrinell hardness(BH) of different forms of

iron.[1][2]

MaterialTS

(MPa)

BH

(Brinell)

Iron whiskers 11000
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Ausformed (hardened) steel 2930 8501200

Martensitic steel 2070 600

Bainitic steel 1380 400

Pearlitic steel 1200 350

Cold-worked iron 690 200Small-grain iron 340 100

Carbon-containing iron 140 40

Pure, single-crystal iron 10 3

Mechanical properties of iron and its alloys are evaluated using a variety of tests, such as the

Brinell test,Rockwell test, ortensile strengthtests, among others; the results on iron are so

consistent that iron is often used to calibrate measurements or to relate the results of one test toanother.[2][3]Those measurements reveal that mechanical properties of iron crucially depend on

purity: Purest research-purpose single crystals of iron are softer than aluminium. Addition of

only 10parts per millionof carbon doubles their strength.[1]

The hardness increases rapidly with

carbon content up to 0.2% and saturates at ~0.6%.[4]The purest industrially produced iron (about99.99% purity) has a hardness of 2030 Brinell.

[5]

Phase diagram and allotropes

Main article:Allotropes of iron

Iron represents an example ofallotropyin a metal. There are at least four allotropic forms of

iron, known as , , , and ; at very high pressures, some controversial experimental evidence

exists for a phase stable at very high pressures and temperatures.[6]

Low-pressurephase diagramof pure iron

As molten iron cools down it crystallizes at 1538 C into its allotrope, which has abody-centered cubic(bcc) crystal structure. As it cools further itscrystal structurechanges toface-

centered cubic(fcc) at 1394 C, when it is known as -iron, oraustenite. At 912 C the crystal

structure again becomes bcc as -iron, orferrite, is formed, and at 770 C (theCurie point, Tc)

iron becomesmagnetic. As the iron passes through the Curie temperature there is no change in
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crystalline structure, but there is a change in "domain structure", where each domain contains

iron atoms with a particular electronic spin. In unmagnetized iron, all the electronic spins of theatoms within one domain are in the same direction; the neighboring domains point in various

directions and thus cancel out. In magnetized iron, the electronic spins of all the domains are

aligned, so that the magnetic effects of neighboring domains reinforce each other. Although each

domain contains billions of atoms, they are very small, about 10 micrometres across .

[7]

. Atpressures above approximately 10 GPa and temperatures of a few hundred kelvin or less, -iron

changes into ahexagonal close-packed(hcp) structure, which is also known as-iron; the higher-

temperature -phase also changes into -iron, but does so at higher pressure. The-phase, if itexists, would appear at pressures of at least 50 GPa and temperatures of at least 1500 K; it has

been thought to have an orthorhombic or a double hcp structure.[6]

Iron is of greatest importance when mixed with certain other metals and with carbon to form

steels. There are many types of steels, all with different properties, and an understanding of the

properties of theallotropes of ironis key to the manufacture of good quality steels.

-iron, also known as ferrite, is the most stable form of iron at normal temperatures. It is a fairlysoft metal that can dissolve only a small concentration of carbon (no more than 0.021% by massat 910 C).[8]

Above 912 C and up to 1400 C -iron undergoes aphase transitionfrom bcc to the fcc

configuration of -iron, also calledaustenite. This is similarly soft and metallic but can dissolve

considerably more carbon (as much as 2.04% by mass at 1146 C). This form of iron is used in

the type ofstainless steelused for making cutlery, and hospital and food-service equipment.[7]

The high-pressure phases of iron are important as endmember models for the solid parts of

planetary cores. Theinner coreof theEarthis generally assumed to consist essentially of an iron-

nickelalloywith (or ) structure.

The melting point of iron is experimentally well constrained for pressures up to approximately

50 GPa. For higher pressures, different studies placed the --liquidtriple pointat pressures

differing by tens of gigapascals and yielded differences of more than 1000 K for the melting

point. Generally speaking,molecular dynamicscomputer simulations of iron melting and shockwave experiments suggest higher melting points and a much steeper slope of the melting curve

than static experiments carried out indiamond anvil cells.[9]

Isotopes

Main article:Isotopes of iron

Naturally occurring iron consists of four stableisotopes: 5.845% of54Fe, 91.754% of56Fe,2.119% of

57Fe and 0.282% of

58Fe. Of these stable isotopes, only

57Fe has a nuclearspin(1/2).

Thenuclide54

Fe is predicted to undergodouble beta decay, but this process had never beenobserved experimentally for these nuclei, and only the lower limit on the half-life was

established: t1/2>3.11022

years.
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60Fe is anextinct radionuclideof longhalf-life(2.6 million years).

[10]It is not found on Earth, but

its ultimate decay product is forms part of the natural abundance of the stable nuclide nickel-60.

Much of the past work on measuring the isotopic composition of Fe has focused on determining60

Fe variations due to processes accompanyingnucleosynthesis(i.e.,meteoritestudies) and ore

formation. In the last decade however, advances inmass spectrometrytechnology have allowedthe detection and quantification of minute, naturally occurring variations in the ratios of the

stable isotopesof iron. Much of this work has been driven by theEarthandplanetary sciencecommunities, although applications to biological and industrial systems are beginning to

emerge.[11]

The most abundant iron isotope 56Fe is of particular interest to nuclear scientists as it represents

the most common endpoint of nucleosynthesis. It is often cited, falsely, as the isotope of highest

binding energy, a distinction which actually belongs tonickel-62.[12]

Since56

Ni is easily

produced from lighter nuclei in thealpha processinnuclear reactionsin supernovae (seesiliconburning process), nickel-56 (14alpha particles) is the endpoint of fusion chains insideextremely

massive stars, since addition of another alpha particle would result in zinc-60, which requires agreat deal more energy. This nickel-56, which has a half-life of about 6 days, is therefore madein quantity in these stars, but soon decays by two successive positron emissions within supernova

decay products in thesupernova remnantgas cloud, first to radioactive cobalt-56, and then stable

iron-56. This last nuclide is therefore common in the universe, relative to other stablemetalsofapproximately the sameatomic weight.

In phases of the meteorites Semarkona and Chervony Kuta correlation between theconcentration of60Ni, thedaughter productof60Fe, and the abundance of the stable iron isotopes

could be found which is evidence for the existence of60Fe at the time offormation of the solar

system. Possibly the energy released by the decay of60

Fe contributed, together with the energy

released by decay of the radionuclide

26

Al, to the remelting anddifferentiationofasteroidsaftertheir formation 4.6 billion years ago[citation needed]. The abundance of60Ni present inextraterrestrial

material may also provide further insight into the origin of thesolar systemand its early history.

Nuclei of iron atoms have some of the highest binding energies per nucleon, surpassed only by

thenickel isotope62

Ni. This is formed bynuclear fusionin stars. Although a further tiny energy

gain could be extracted by synthesizing62

Ni, conditions in stars are unsuitable for this process tobe favored. Elemental distribution on Earth greatly favors iron over nickel, and also presumably

in supernova element production.[13]

Iron-56is the heaviest stable isotope produced by the alpha process instellar nucleosynthesis;

elements heavier than iron and nickel require asupernovafor their formation. Iron is the most

abundant element in the core ofred giants, and is the most abundant metal iniron meteoritesandin the dense metalcores of planetssuch asEarth.

Nucleosynthesis

Iron is created by extremely large, extremely hot (over 2.5 billion kelvin) stars, through a process

called thesilicon burning process. It is the heaviest stable element to be produced in this manner.
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The process starts with the second largest stable nucleus created by silicon burning: calcium.

One stable nucleus of calcium fuses with one helium nucleus, creating unstable titanium. Beforethe titanium decays, it can fuse with another helium nucleus, creating unstable chromium. Before

the chromium decays, it can fuse with another helium nucleus, creating unstable iron. Before the

iron decays, it can fuse with another helium nucleus, creating unstable nickel-56. Any further

fusion of nickel-56 consumes energy instead of producing energy, so after the production ofnickel-56, the star does not produce the energy necessary to keep the core from collapsing.

Eventually, the nickel-56 decays to unstable cobalt-56 which, in turn decays to stableiron-56

When the core of the star collapses, it creates aSupernova. Supernovas also create additionalforms of stable iron via ther-process.

Occurrence

See also Category:Iron minerals.

Planetary occurrence

Iron meteoritesof similar composition of Earth's inner and outer core

Iron is the sixth mostabundant elementin theUniverse, formed as the final step of

nucleosynthesis, bysilicon fusingin massive stars. Metallic iron is rarely found on the surface of

the earth because it tends to oxidize, but its oxides are pervasive and represent the primary ores.While it makes up about 5% of theEarth's crust, both the Earth'sinnerandoutercore are

believed to consist largely of an iron-nickelalloy constituting 35% of the mass of the Earth as a

whole. Iron is consequently the most abundant element on Earth, but only the fourth mostabundant element in the Earth's crust.[14][15]Most of the iron in the crust is found combined with

oxygen asiron oxideminerals such ashematiteandmagnetite. Large deposits of iron are found

inbanded iron formations. These geological formations are a type of rock consisting of repeated

thin layers ofiron oxides, eithermagnetite(Fe3O4) orhematite(Fe2O3), alternating with bands ofiron-poorshaleandchert. The banded iron formations are common in the time between3,700

million years ago and1,800million years ago[16][17]

About 1 in 20meteoritesconsist of the unique iron-nickel mineralstaenite(3580% iron) and

kamacite(9095% iron). Although rare,iron meteoritesare the main form of natural metallic

iron on the Earth's surface.[18]

It was proven byMssbauer spectroscopythat the red color of the

surface ofMarsis derived from an iron oxide-richregolith.[19]
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In-use stocks in society

According to theInternational Resource Panel'sMetal Stocks in Society report, the global per

capita stock of iron in use in society is 2200kg. Much of this is in more-developed countries

(700014000kg per capita) rather than less-developed countries (2000kg per capita).

Chemistry and compounds

See also Category:Iron compounds.

Oxidation

stateRepresentative compound

2 Disodium tetracarbonylferrate(Collman's reagent)

1

0 Iron pentacarbonyl

1 Cyclopentadienyliron dicarbonyl dimer("Fp2")

2 Ferrous sulfate,ferrocene

3 Ferric chloride,ferrocenium tetrafluoroborate

4 Barium ferrate(IV)

5

6 Potassium ferrate

Iron forms compounds mainly in the +2 and +3oxidation states. Traditionally, iron(II)compounds are calledferrous, and iron(III) compoundsferric. Iron also occurs in higher

oxidation states, an example being the purplepotassium ferrate(K2FeO4) which contains iron inits +6 oxidation state. Iron(IV) is a common intermediate in many in biochemical oxidation

reactions.[20][21]Numerousorganometalliccompounds contain formal oxidation states of +1, 0,

1, or even 2. The oxidation states and other bonding properties are often assessed using thetechnique ofMssbauer spectroscopy.[22]There are also manymixed valence compoundsthat

contain both iron(II) and iron(III) centers, such asmagnetiteandPrussian blue

(Fe4(Fe[CN]6)3).[21]

The latter is used as the traditional "blue" inblueprints.[23]

Hydratediron(III) chloride, also known as ferric chloride
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The iron compounds produced on the largest scale in industry areiron(II) sulfate(FeSO47H2O)

andiron(III) chloride(FeCl3). The former is one of the most readily available sources of iron(II),but is less stable to aerial oxidation thanMohr's salt((NH4)2Fe(SO4)26H2O). Iron(II) compounds

tend to be oxidized to iron(III) compounds in the air.[21]

Unlike many other metals, iron does not form amalgams with mercury. As a result, mercury istraded in standardized 76 pound flasks (34 kg) made of iron.[24]

Binary compounds

Iron reacts with oxygen in the air to form variousoxide and hydroxide compounds; the mostcommon areiron(II,III) oxide(Fe3O4), andiron(III) oxide(Fe2O3).Iron(II) oxidealso exists,

though it is unstable at room temperature. These oxides are the principal ores for the production

of iron (seebloomeryand blast furnace). They are also used in the production offerrites, useful

magnetic storagemedia in computers, and pigments. The best known sulfide isiron pyrite(FeS2), also known as fool's gold owing to its golden luster .

[21]

The binary ferrous and ferric halides are well known, with the exception of ferric iodide. Theferrous halides typically arise from treating iron metal with the corresponding binary halogen

acid to give the corresponding hydrated salts.[21]

Fe + 2 HX FeX2 + H2

Iron reacts with fluorine, chlorine, and bromine to give the corresponding ferric halides,ferricchloridebeing the most common:

2 Fe + 3 X2 2 FeX3 (X = F, Cl, Br)

Coordination and organometallic compounds

See also:organoiron chemistry

Prussian blue

Several cyanide complexes are known. The most famous example isPrussian blue,(Fe4(Fe[CN]6)3).Potassium ferricyanideandpotassium ferrocyanideare also known; the

formation of Prussian blue upon reaction with iron(II) and iron(III) respectively forms the basisof a "wet" chemical test.[21]Prussian blue is also used as an antidote forthalliumand radioactive

caesiumpoisoning.[25][26]

Prussian blue can be used in laundry bluing to correct the yellowish tint

left by ferrous salts in water.[27]
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on%28II,III%29_oxidehttp://en.wikipedia.org/wiki/Iron_oxidehttp://d/TUGAS%20FELA/Iron.htm%23cite_note-23http://d/TUGAS%20FELA/Iron.htm%23cite_note-HollemanAF-20http://en.wikipedia.org/wiki/Mohr%27s_salthttp://en.wikipedia.org/wiki/Iron%28III%29_chloridehttp://en.wikipedia.org/wiki/Water_of_crystallizationhttp://en.wikipedia.org/wiki/Iron%28II%29_sulfate


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Ferrocene

Several carbonyl compounds of iron are known. The premier iron(0) compound is iron

pentacarbonyl, Fe(CO)5, which is used to producecarbonyl ironpowder, a highly reactive form

of metallic iron. Thermolysis of iron pentacarbonyl gives the trinuclear cluster,triirondodecacarbonyl. Collman's reagent,disodium tetracarbonylferrate, is a useful reagent for organic

chemistry; it contains iron in the 2 oxidation state.Cyclopentadienyliron dicarbonyl dimer

contains iron in the rare +1 oxidation state.[28]

Ferroceneis an extremely stable complex. The firstsandwich compound, it contains an iron(II)center with twocyclopentadienylligands bonded through all ten carbon atoms. This arrangement

was a shocking novelty when it was first discovered,[29]

but the discovery of ferrocene has led toa new branch of organometallic chemistry. Ferrocene itself can be used as the backbone of a

ligand, e.g.dppf. Ferrocene can itself be oxidized to theferroceniumcation (Fc+); the

ferrocene/ferrocenium couple is often used as a reference in electrochemistry.[30]

History

Main article:History of ferrous metallurgy

Wrought iron

The symbol for Mars has been used since antiquity to represent iron.
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TheDelhi iron pillaris an example of the iron extraction and processing methodologies of India.

The iron pillar at Delhi has withstood corrosion for the last 1600 years.

Iron objects of great age are much rarer than objects made of gold or silver due to the ease ofcorrosion of iron.[31]Beads made ofmeteoriciron in 3500 B.C. or earlier were found in Gerzah,

Egypt by G. A. Wainwright.[32]The beads contain 7.5% nickel, which is a signature of meteoric

origin since iron found in the Earth's crust has very little to no nickel content. Meteoric iron washighly regarded due to its origin in the heavens and was often used to forge weapons and tools or

whole specimens placed in churches.[32]Items that were likely made of iron by Egyptians date

from 2500 to 3000 BC.[31]

Iron had a distinct advantage over bronze in warfare implements. It

was much harder and more durable than bronze, although susceptible to rust. However, this iscontested.HittitologistTrevor Bryceargues that before advanced iron-working techniques were

developed inEuropeandIndia,cast-ironweapons used by earlyMesopotamianarmies had a

tendency to shatter in combat, due to their high carbon content.[33]

The first iron production started in theMiddle Bronze Agebut it took several centuries before

iron displaced bronze. Samples ofsmeltediron fromAsmar, Mesopotamia and Tall ChagarBazaar in northern Syria were made sometime between 2700 and 3000 BC.[34]TheHittites

appear to be the first to understand the production of iron from its ores and regard it highly in

their society.[27]

They began to smelt iron between 1500 and 1200 BC and the practice spread to

the rest of the Near East after their empire fell in 1180 BC.[34]

The subsequent period is called the

Iron Age. Iron smelting, and thus the Iron Age, reached Europe two hundred years later andarrived inZimbabwe, Africa by the 8th century.[34]

Artifacts from smelted iron occur inIndiafrom 1800 to 1200 BC,[35]and in theLevantfrom

about 1500 BC (suggesting smelting inAnatoliaor theCaucasus).[36][37]

TheBook of Genesis, fourth chapter, verse 22 contains the first mention of iron in theOld

Testamentof theBible; "Tubal-cain, an instructor of every artificer in brass and iron."[31]

Other
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A/Iron.htm%23cite_note-35http://d/TUGAS%20FELA/Iron.htm%23cite_note-35http://en.wikipedia.org/wiki/Caucasushttp://en.wikipedia.org/wiki/Anatoliahttp://en.wikipedia.org/wiki/Levanthttp://d/TUGAS%20FELA/Iron.htm%23cite_note-Tewari-34http://en.wikipedia.org/wiki/History_of_metallurgy_in_the_Indian_subcontinenthttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196832-33http://en.wikipedia.org/wiki/Zimbabwehttp://en.wikipedia.org/wiki/Iron_Agehttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196832-33http://d/TUGAS%20FELA/Iron.htm%23cite_note-Iron_2008-26http://en.wikipedia.org/wiki/Hittiteshttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196832-33http://en.wikipedia.org/wiki/Asmarhttp://en.wikipedia.org/wiki/Smeltinghttp://en.wikipedia.org/wiki/Middle_Bronze_Agehttp://d/TUGAS%20FELA/Iron.htm%23cite_note-32http://en.wikipedia.org/wiki/Mesopotamiahttp://en.wikipedia.org/wiki/Cast-ironhttp://en.wikipedia.org/wiki/Indiahttp://en.wikipedia.org/wiki/Europehttp://en.wikipedia.org/wiki/Trevor_Brycehttp://en.wikipedia.org/wiki/Hittiteshttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196829-30http://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196831-31http://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196831-31http://en.wikipedia.org/wiki/Meteorhttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196829-30http://en.wikipedia.org/wiki/Iron_pillar_of_Delhi


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verses allude to iron mining (Job 28:2), iron used as a stylus (Job 19:24), furnace (Deuteronomy

4:20), chariots (Joshua 17:16), nails (I Chron. 22:3), saws and axes (II Sam. 12:31), and cookingutensils (Ezekiel 4:3).[38]The metal is also mentioned in theNew Testament, for example in Acts

chapter 12 verse 10, "[Peter passed through] the iron gate that leadeth unto the city" of

Antioch.[39]

TheQuran referredto Iron 1400 years ago.

Iron working was introduced to Greecein the late 11th century BC.[40]

The spread of

ironworking in Central and Western Europe is associated withCelticexpansion. According toPliny the Elder, iron use was common in theRomanera.[32]The annual iron output of theRoman

Empireis estimated at 84,750t,[41]

while the similarly populous Han China produced around

5,000 t.[42]

During the Industrial Revolution in Britain,Henry Cortbegan refining iron frompig ironto

wrought iron(or bar iron) using innovative production systems. In 1783 he patented the puddling

processfor refining iron ore. It was later improved by others includingJoseph Hall.

Cast iron

Cast ironwas first produced inChinaabout 550 BC,[43]but was hardly in Europe until the

medieval period.[44][45]

During themedievalperiod, means were found in Europe of producing

wrought iron from cast iron (in this context known aspig iron) usingfinery forges. For all theseprocesses,charcoalwas required as fuel.

Coalbrookdale by Night, 1801. Blast furnaces light the iron making town ofCoalbrookdale.

Medievalblast furnaceswere about 10 feet (3.0 m) tall and made of fireproof brick; forced airwas usually provided by hand-operated bellows.[45]Modern blast furnaces have grown much

bigger.

In 1709,Abraham Darby Iestablished acoke-fired blast furnace to produce cast iron. Theensuing availability of inexpensive iron was one of the factors leading to the Industrial

Revolution. Toward the end of the 18th century, cast iron began to replace wrought iron for

certain purposes, because it was cheaper. Carbon content in iron wasn't implicated as the reasonfor the differences in properties of wrought iron, cast iron and steel until the 18th century.[34]

Since iron was becoming cheaper and more plentiful, it also became a major structural material

following the building of the innovativefirst iron bridgein 1778.
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iki/The_Iron_Bridgehttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196832-33http://en.wikipedia.org/wiki/Coke_%28fuel%29http://en.wikipedia.org/wiki/Abraham_Darby_Ihttp://d/TUGAS%20FELA/Iron.htm%23cite_note-ReferenceA-44http://en.wikipedia.org/wiki/Blast_furnaceshttp://en.wikipedia.org/wiki/Coalbrookdalehttp://en.wikipedia.org/wiki/Coalbrookdale_by_Nighthttp://en.wikipedia.org/wiki/Charcoalhttp://en.wikipedia.org/wiki/Finery_forgehttp://en.wikipedia.org/wiki/Pig_ironhttp://en.wikipedia.org/wiki/Medievalhttp://d/TUGAS%20FELA/Iron.htm%23cite_note-43http://d/TUGAS%20FELA/Iron.htm%23cite_note-43http://d/TUGAS%20FELA/Iron.htm%23cite_note-42http://en.wikipedia.org/wiki/Chinahttp://en.wikipedia.org/wiki/Cast_ironhttp://en.wikipedia.org/wiki/Joseph_Hall_%28metallurgist%29http://en.wikipedia.org/wiki/Puddling_%28metallurgy%29http://en.wikipedia.org/wiki/Puddling_%28metallurgy%29http://en.wikipedia.org/wiki/Wrought_ironhttp://en.wikipedia.org/wiki/Pig_ironhttp://en.wikipedia.org/wiki/Henry_Corthttp://d/TUGAS%20FELA/Iron.htm%23cite_note-41http://d/TUGAS%20FELA/Iron.htm%23cite_note-40http://en.wikipedia.org/wiki/Tonneshttp://en.wikipedia.org/wiki/Roman_Empirehttp://en.wikipedia.org/wiki/Roman_Empirehttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196831-31http://en.wikipedia.org/wiki/Ancient_Romehttp://en.wikipedia.org/wiki/Pliny_the_Elderhttp://en.wikipedia.org/wiki/Celtshttp://d/TUGAS%20FELA/Iron.htm%23cite_note-39http://en.wikipedia.org/wiki/Ancient_Greecehttp://en.wikipedia.org/wiki/Al-Hadid#Iron_in_the_Qur.27anhttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196830-38http://en.wikipedia.org/wiki/New_Testamenthttp://d/TUGAS%20FELA/Iron.htm%23cite_note-FOOTNOTEWeeks196829.E2.80.9330-37


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Steel

See also:Steelmaking

Steel (with smaller carbon content than pig iron but more than wrought iron) was first produced

in antiquity by using abloomery. Blacksmiths inLuristanin western Iran were making goodsteel by 1000 BC.

[34]Then improved versions,Wootz steelby India andDamascus steelby

China were developed around 300 B.C. and 500 A.D. respectively. These methods werespecialized, and so steel did not become a major commodity until the 1850s.[46]

New methods of producing it bycarburizingbars of iron in thecementation processweredevised in the 17th century AD. In theIndustrial Revolution, new methods of producing bar iron

without charcoal were devised and these were later applied to produce steel. In the late 1850s,

Henry Bessemerinvented a new steelmaking process, involving blowing air through molten pig

iron, to produce mild steel. This made steel much more economical, thereby leading to wroughtiron no longer being produced.[citation needed]

Foundations of modern chemistry

Antoine Lavoisierused the reaction of water steam with metallic iron inside an incandescent iron

tube to producehydrogenin his experiments leading to the demonstration of the mass

conservation. Anaerobic oxidation of iron at high temperature can be schematically representedby the following reactions:

Fe + H2O FeO + H2

2 Fe + 3 H2O Fe2O3 + 3 H2

3 Fe + 4 H2O Fe3O4 + 4 H2

Recent discoveries

discovery ofMssbauer effect many enzymes use iron in the catalytic center Nickel-56 is the natural end product

chemical task

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