7439-89-6

Usage

Chemical Description

Iron is a metallic element used in many industries, including construction and manufacturing.

Uses

Used in Construction and Manufacturing Industry:
Iron is used as a primary material for carbon steels, which are alloys of iron containing carbon in varying proportions, usually up to 1.7% carbon. Other metals such as nickel and chromium are also incorporated into carbon steels to produce low-alloy steels, classified as stainless steel, tool steels, and heat-resistant steels. These steels are extensively used in various construction and manufacturing applications due to their strength and durability.
Used in Catalyst Industry:
Iron is used as an industrial catalyst in catalyst compositions in the Haber process for the synthesis of ammonia, and in the Fischer-Tropsch process for producing synthetic gasoline. These processes are essential for the production of fertilizers and liquid fuels, respectively.
Used in Pharmaceutical, Pesticide, and Powder Metallurgy Industries:
Iron is used as a reducing agent, as well as for iron salt manufacturing and in the electronics industry. It is also used in powder metallurgy products, all kinds of mechanical parts and components products, cemented carbide products, etc.
Used in Food Industry:
Iron is a mineral used in food fortification that is necessary for the prevention of anemia. It is used for fortification in flour, baked goods, pasta, and cereal products. Iron sources for fortification include ferric ammonium sulfate, chloride, fructose, glycerophosphate, nitrate, phosphate, pyrophosphate, and ferrous ammonium sulfate, citrate, sulfate, and sodium iron EDTA.
Used in Magnet Industry:
One of the most useful characteristics of iron is its natural magnetism, which can also be introduced into iron products by electrical induction. Magnets of all sizes and shapes are used in motors, atom smashers, CT scanners, and TV and computer screens, among other applications. Super magnets can be formed by adding other elements to high-quality iron.
Used in Nutritional Supplements:
Iron is used as a nutritional supplement (iron fortifier) for casting or as a reducing agent. It is an essential trace mineral that we need about 10 to 18 milligrams of each day to maintain proper health. Iron deficiency may cause anemia, weakness, fatigue, headaches, and shortness of breath, while excess iron in the diet can cause liver damage, although this is a rare condition.

History

Iron has been known to mankind from early civilization. In fact, a period of history, the “iron age,” is named for the widespread use of this metal. For almost a thousand years, it remained as the single most-used metal, and its use in mechanization made the industrial revolution possible. Iron, after oxygen, silicon and aluminum, is the fourth most abundant element in the earth’s crust. It is the prime constituent of earth’s core along with nickel. Its abundance in the crust is 5.63%. Its concentration in the seawater is about 0.002mg/L. The principal ores of iron are hematite, Fe2O3; pyrite, Fe2S2; ilmenite, FeTiO3; magnetite, Fe3O4; siderite, Fe2CO3; and limonite [FeO(OH)]. It also is found in a number of minerals, such as corundum, as an impurity. It also is found in meteorites. Iron occurs in every mammalian cell and is vital for life processes. It is bound to various proteins and found in blood and tissues. The iron-porphyrin or heme proteins include hemoglobin, myoglobin and various heme enzymes, such as cytochromes and peroxidases. Also, it occurs in non heme compounds, such as ferritin, siderophilin, and hemosiderin. Hemoglobin, found in the red blood cells, is responsible for transport of oxygen to the tissue cells and constitutes about two-thirds (mass) of all iron present in the human body. An adult human may contain about 4 to 6 grams of iron.

History

Iron is a relatively abundant element in the universe. It is found in the sun and many types of stars in considerable quantity. It has been suggested that the iron we have here on Earth may have originated in a supernova. Iron is a very difficult element to produce in ordinary nuclear reactions, such as would take place in the sun. Iron is found native as a principal component of a class of iron–nickel meteorites known as siderites, and is a minor constituent of the other two classes of meteorites. The core of the Earth, 2150 miles in radius, is thought to be largely composed of iron with about 10% occluded hydrogen. The metal is the fourth most abundant element, by weight, making up the crust of the Earth. The most common ore is hematite (Fe2O3). Magnetite (Fe3O4) is frequently seen as black sands along beaches and banks of streams. Lodestone is another form of magnetite. Taconite is becoming increasingly important as a commercial ore. Iron is a vital constituent of plant and animal life, and appears in hemoglobin. The pure metal is not often encountered in commerce, but is usually alloyed with carbon or other metals. The pure metal is very reactive chemically, and rapidly corrodes, especially in moist air or at elevated temperatures. It has four allotropic forms,or ferrites, known as α, β, γ, and δ, with transition points at 700, 928, and 1530°C. The α form is magnetic, but when transformed into the β form, the magnetism disappears although the lattice remains unchanged. The relations of these forms are peculiar. Pig iron is an alloy containing about 3% carbon with varying amounts of S, Si, Mn, and P. It is hard, brittle, fairly fusible, and is used to produce other alloys, including steel. Wrought iron contains only a few tenths of a percent of carbon, is tough, malleable, less fusible, and usually has a “fibrous” structure. Carbon steel is an alloy of iron with carbon, with small amounts of Mn, S, P, and Si. Alloy steels are carbon steels with other additives such as nickel, chromium, vanadium, etc. Iron is the cheapest and most abundant, useful, and important of all metals. Natural iron contains four isotopes. Twenty-six other isotopes and isomers, all radioactive, are now recognized.

Content analysis

Accurately weigh approximately 200 mg of the sample and transfer it into a 300 ml Erlenmeyer flask, add 50 ml of a dilute sulfuric acid solution (TS-241). Use a plug containing a Bunsen valve (the production method is to insert a glass tube connected with a short segment of rubber tube to the plug. The side of the rubber tube has a long slit while the other side is inserted of a glass rod so that the gas can escape and the air can’t enter). The solution was heated on a steam bath to dissolve the iron. After cooling, dilute with 50 ml of freshly boiled and cooled water. Add 2 drops of the test solution (TS-162) to 0.1 mol/L Apply cerium sulfate titration to until the red color becomes light blue color. Each ml of 0.1mol/L of high cerium sulfate are equivalent to 5.585 mg of iron (Fe). The method is the same as that of "reduced iron (01219)”.

Production Methods

Most iron produced today is from its oxide minerals, hematite and magnetite. The process involves reducing mineral iron with carbon in a blast furIRON 411nace. There are several types of blast furnaces which vary in design and dimensions. The overall processes, however, are more or less the same. One such process is outlined below: The mixture of ore, coke and limestone is fed into the blast furnace from the top. The materials are preheated to about 200°C in the top most zone. Hematite is partially reduced to magnetite and then to FeO by the ascending stream of carbon monoxide formed at the bottom and mid zones of the furnace resulting from high temperature oxidation of carbon. The ferrous oxide FeO formed at the top zone is reduced to metallic iron at about 700°C in the mid zone by carbon monoxide. A hot air blast at 900°C passes through the entire furnace for a very short time (usually for a few seconds). This prevents any gassolid reaction product from reaching equilibrium. In the temperature zone 700 to 1,200°C ferrous oxide is completely reduced to iron metal by carbon monoxide. Also, more CO is formed by oxidation of carbon by carbon dioxide. Further down the furnace at higher temperatures, around 1,500°C, iron melts, dripping down into the bottom. Also, in this temperature zone acidic silica particles react with basic calcium oxide produced from the decomposition of limestone, producing calcium silicate. The molten waste calcium silicate also drips down into the bottom. In the hottest zone of the blast furnace, between 1,500 to 2,000°C, some carbon dissolves into the molten iron. Also at these temperatures any remaining silicates and phosphates are reduced to silicon and phosphorus, and dissolve into the molten iron. Additionally, other tract metals such as manganese dissolve into the molten iron. The impure iron melt containing about 3 to 4% carbon is called “pig iron”. At the bottom, the molten waste slag floats over the impure pig iron melt that is heavier than the slag melt and immiscible with it. Pig iron is separated from the slag and purified for making different types of steel. Chemical reactions and processes occurring in various temperature zones of blast furnace are summarized below: Pig iron produced in the blast furnace is purified and converted to steel in a separate furnace, known as a basic-oxygen furnace. Jets of pure oxygen gas at high pressure are blown over and through the pig iron melt. Metal impurities are converted into oxides. Part of the dissolved carbon in the impure iron melt is converted into carbon dioxide gas. Formation of SiO2, CO2, and other metal oxides are exothermic reactions that raise the temperature to sustain the melt. A lime flux (CaO) also is added into the melt, which converts silica into calcium silicate, CaSiO3, and phosphorus into calcium phosphate, Ca3(PO4)2, forming a molten slag immiscible with molten steel. The lighter molten slag is decanted from the heavier molten steel.

Production Methods

Iron ore reserves are found worldwide. Areas with more than 1 billion metric tons of reserves include Australia, China, Brazil, Canada, the United States, Venezuela, South Africa, India, the former Soviet Union, Gabon, France, Spain, Sweden, and Algeria. The ore exists in varying grades, ranging from 20 to 70% iron content. North America has been fortunate in its ore deposits. There are commercially usable quantities in 22 U.S. states and in six Canadian provinces. In the United States the most abundant supplies, discovered in the early 1890s, are located in the Lake Superior region around the Mesabi Range. Other large deposits are found in Alabama, Utah, Texas, California, Pennsylvania, and New York. These deposits, particularly the Mesabi Range reserves, seemed inexhaustible in the 1930s when an average of 30 million tons of ore was produced annually from that one range. The tremendous demand for iron ore duringWorldWar II virtually tripled the output of the Mesabi Range and severely depleted its deposits of high-grade ore. The major domestic (U.S.) production is nowfrom crude iron ore, mainly taconite, a low-grade ore composed chiefly of hematite [FeO(OH) ·H2O] and silica found in the Great Lakes region.

Mining

China pyrrhotite-type sulfur pyrite mine has less of mining hills resources. Take the MinXi mine in the DaTian City, Fujian Province and Zhangjiagou mine in Dandong City, Liaoning Province as the representatives; both of them are underground mining mines. The former applies the Housing pile mining method while the later one uses the section mining method. The pit mining process is the same as the method of "phosphate rock." Beneficiation methods include flotation process and flotation-magnetic combined process.

Toxicity

Iron Powder: GRAS (FDA, § 184.1375, 2000); Inhalation of dust can cause pneumoconiosis. Operation personnel should wear overall, wear dust masks and other labor insurance products. Production equipment should be closed, the workshop should be well-ventilated. Be sure to pay attention to dust protection.

Isotopes

There are 30 isotopes of iron ranging from Fe-45 to Fe-72. The following arethe four stable isotopes with the percentage of their contribution to the element’s naturalexistence on Earth: Fe-54 = 5.845%, Fe-56 = 91.72%, Fe-57 = 2.2%, and Fe-58 =0.28%. It might be noted that Fe-54 is radioactive but is considered stable because ithas such a long half-life (3.1×10+22 years). The other isotopes are radioactive and areproduced artificially. Their half-lives range from 150 nanoseconds to 1×105 years.

Origin of Name

The name “iron” or “iren” is Anglo-Saxon, and the symbol for iron (Fe) is from ferrum, the Latin word for iron.

Characteristics

Iron is the only metal that can be tempered (hardened by heating, then quenching in wateror oil). Iron can become too hard and develop stresses and fractures. This can be corrected byannealing, a process that heats the iron again and then holds it at that temperature until thestresses are eliminated. Iron is a good conductor of electricity and heat. It is easily magnetized,but its magnetic properties are lost at high temperatures. Iron has four allotropic states. Thealpha form exists at room temperatures, while the other three allotropic forms exist at varyinghigher temperatures.Iron is the most important construction metal. It can be alloyed with many other metals tomake a great variety of specialty products. Its most important alloy is steel.An interesting characteristic of iron is that it is the heaviest element that can be formed byfusion of hydrogen in the sun and similar stars. Hydrogen nuclei can be “squeezed” in the sunto form all the elements with atomic numbers below cobalt (27Co), which includes iron. Itrequires the excess fusion energy of supernovas (exploding stars) to form elements with protonnumbers greater than iron (26Fe).

Preparation

Most iron produced today is from its oxide minerals, hematite and magnetite. The process involves reducing mineral iron with carbon in a blast furnace. There are several types of blast furnaces which vary in design anddimensions. The overall processes, however, are more or less the same. Onesuch process is outlined below: The mixture of ore, coke and limestone is fed into the blast furnace from thetop. The materials are preheated to about 200°C in the top most zone.Hematite is partially reduced to magnetite and then to FeO by the ascendingstream of carbon monoxide formed at the bottom and mid zones of the furnaceresulting from high temperature oxidation of carbon. The ferrous oxide FeOformed at the top zone is reduced to metallic iron at about 700°C in the midzone by carbon monoxide. A hot air blast at 900°C passes through the entirefurnace for a very short time (usually for a few seconds). This prevents any gassolid reaction product from reaching equilibrium. In the temperature zone 700to 1,200°C ferrous oxide is completely reduced to iron metal by carbon monox-ide. Also, more CO is formed by oxidation of carbon by carbon dioxide. Furtherdown the furnace at higher temperatures, around 1,500°C, iron melts, drippingdown into the bottom. Also, in this temperature zone acidic silica particlesreact with basic calcium oxide produced from the decomposition of limestone,producing calcium silicate. The molten waste calcium silicate also drips downinto the bottom. In the hottest zone of the blast furnace, between 1,500 to2,000°C, some carbon dissolves into the molten iron. Also at these temperatures any remaining silicates and phosphates are reduced to silicon and phosphorus, and dissolve into the molten iron. Additionally, other tract metals suchas manganese dissolve into the molten iron. The impure iron melt containingabout 3 to 4% carbon is called “pig iron”. At the bottom, the molten waste slagfloats over the impure pig iron melt that is heavier than the slag melt andimmiscible with it. Pig iron is separated from the slag and purified for makingdifferent types of steel. Chemical reactions and processes occurring in varioustemperature zones of blast furnace are summarized below: Pig iron produced in the blast furnace is purified and converted to steel ina separate furnace, known as a basic-oxygen furnace. Jets of pure oxygen gasat high pressure are blown over and through the pig iron melt. Metal impurities are converted into oxides. Part of the dissolved carbon in the impure ironmelt is converted into carbon dioxide gas. Formation of SiO2, CO2,and othermetal oxides are exothermic reactions that raise the temperature to sustainthe melt. A lime flux (CaO) also is added into the melt, which converts silicainto calcium silicate, CaSiO3,and phosphorus into calcium phosphate,Ca3(PO4)2,forming a molten slag immiscible with molten steel. The lightermolten slag is decanted from the heavier molten steel.

Air & Water Reactions

Highly flammable. May react with water to give off hydrogen, a flammable gas. The heat from this reaction may ignite the hydrogen.

Reactivity Profile

Iron is pyrophoric [Bretherick, 1979 p. 170-1]. A strong reducing agent and therefore incompatible with oxidizing agents. Burns in chlorine gas [Mellor 2, Supp. 1:380 1956]. Reacts with fluorine with incandescence [Mellor 13:314, 315, 1946-1947].

Hazard

Iron dust from most iron compounds is harmful if inhaled and toxic if ingested. Iron dustand powder (even filings) are flammable and can explode if exposed to an open flame. Asmentioned, excessive iron in the diet may cause liver damage.

Health Hazard

Fire may produce irritating and/or toxic gases. Contact may cause burns to skin and eyes. Contact with molten substance may cause severe burns to skin and eyes. Runoff from fire control may cause pollution.

Fire Hazard

Flammable/combustible material. May be ignited by friction, heat, sparks or flames. Some may burn rapidly with flare burning effect. Powders, dusts, shavings, borings, turnings or cuttings may explode or burn with explosive violence. Substance may be transported in a molten form at a temperature that may be above its flash point. May re-ignite after fire is extinguished.

Biochem/physiol Actions

Carbonyl iron has a role as an absorber of microwave radiation. Carbonyl iron also exhibits shielding properties because of the low density and the connectivity among the fillers it provide. It is used in industries and in the synthesis of nitro-group-containing pharmaceutical ingredients.

Environmental Fate

Iron occurs rarely by itself in nature due to the ease with which it forms compounds, especially in oxidation reactions. Many iron compounds are water soluble, leading to potentially high concentrations in water, especially in seawater. Iron is a necessary component of all life and it is therefore taken up readily by organisms from all sources.

Purification Methods

Clean it in conc HCl, rinse in de-ionised water, then reagent grade acetone and dry it under vacuum.

Toxicity evaluation

In some adults, iron overload can be the result of a genetic defect (idiopathic hemochromatosis) that causes malfunction of the normal homeostasis mechanism and, in turn, excessive absorption of iron. Iron overload can also be caused by too many blood transfusions, which results in too much iron in the various iron-containing organs. Recently, it has been suggested that the presence of increased transferrin concentrations in males is associated with an increased number of heart attacks. This must be corroborated by further research. Excess iron can lead to diabetes mellitus, faulty liver functions, and endocrine disturbance. Iron is a catalyst for oxidative damage leading to lipid peroxidation. The latest hypotheses link peroxidation to heart disease, cancer, and accelerated aging. Iron is involved in the Fenton reaction, which catalyzes the formation of free radicals that cause excessive damage to cells and their components.

Structure and conformation

Two structural types of iron occur in the solid state. At room temperature iron has a body-centered cubic lattice (the a form). At about 910°C the a form is transformed into the γ allotrope which has a cubic close-packed structure. Around 1390°C a body-centred cubic lattice is reformed—the δ form. Thus the allotropy of iron is unusual in that it can exist with the same crystal form in two distinct temperature ranges which are separated by a range within which a different form is stable. The a and ? forms have similar lattice parameters— the differences between them being expected in view of thermal expansion which increases the size of the unit cell of the δallotrope.

InChI:InChI=1/Fe

Synthetic route

iron(III) oxide → iron (7439-89-6)

Conditions	Yield
With hydrogen In neat (no solvent) passing H2 over Fe2O3 at 350°C over period of 36 h, at 440°C 12 h or at 500°C in fast reaction;;	100%
With H2 In neat (no solvent) passing H2 over Fe2O3 at 350°C over period of 36 h, at 440°C 12 h or at 500°C in fast reaction;;	100%
With hydrogen In neat (no solvent) reduction of Fe2O3 at 600°C leads to formation of powdered Fe, at 1000°C formed Fe hardly fragile;;

goethite + hydrogen (1333-74-0) → iron (7439-89-6)

Conditions	Yield
In neat (no solvent) Isothermal heat treatment for 2 h at 400°C.;	100%

iron(II) chloride → iron (7439-89-6)

Conditions	Yield
With 2,3,5,6-tetramethyl-1,4-bis(trimethylsilyl)-1,4-diaza-2,5-cyclo-hexadiene In tetrahydrofuran at 20℃; for 6h; Inert atmosphere;	100%
With hydrogen In neat (no solvent) heated with H2 at approx. 350 °C; formation of pyrophoric Fe;;
With aluminium trichloride; 1-ethyl-3-methyl-1H-imidazol-3-ium chloride In melt Electrochem. Process; (He or Ar); dissoln. of FeCl2 in AlCl3/1-ethyl-3-methyimidazoline chloride ionic liquid (room temp.), chronoamperometric electrodeposition (tungsten electrode substrate, -0.35 V vs. Fe/Fe(II), 120 s, room temp.);

LaFe(1+) (111496-23-2) → La(1+) + iron (7439-89-6)

Conditions	Yield
In gas collision induced dissocn. reaction (argon) in a mass spectrometer; energy range 17-78 eV; total pressure: 4E-6 Torr; not isolated;	A 100% B 100%

iron(III) oxide → iron (7439-89-6)

Conditions	Yield
With water; lithium chloride In melt at 660℃; for 5h; Inert atmosphere; Electrolysis;	98.4%

iron pentacarbonyl (13463-40-6) + Cyclohepta-1,3-diene (876938-53-3) → tricarbonyl(η-3-cyclohepta-1,3-diene)iron (40674-86-0) + iron (7439-89-6)

Conditions	Yield
In dibutyl ether cycloheptadiene stirred in n-Bu2O while N2 bubbled through mixt. for 15h, Fe(CO)5 added, heated with stirring at 150°C for 44 h, cooled; filtered through Celite, evapd. in vac.;	A 93% B n/a

iron(III) chloride (7705-08-0) + lithium triethylborohydride (22560-16-3) → iron (7439-89-6)

Conditions	Yield
In tetrahydrofuran FeCl3 in THF was added dropwise to stirring soln. of 12 ml LiBEt3H in THF (1.0 M), held at const. temp. under N2 atm.; forms of particles dependon dropping rate (1 drop/10s, 1/s, 2/s), stirring rate (200, 400, 1600 rpm) and temp.(0 - 60°C); vac. filtration, washed THF/EtOH (1:1), dried in vac.;	90%

1-trimethylsilyl-μ3-S,S'-ethylenedithiolatohexacarbonyldiiron → iron sulfide + (CH3)3SiC2H3S8Fe7 + iron (7439-89-6) + 4-Trimethylsilanyl-[1,3]dithiolan-2-one + ethenyltrimethylsilane (754-05-2)

Conditions	Yield
In decane byproducts: CH2CH2, CH3CHCH2, CO; Ar atmosphere; decompn. (165°C, 13 h); further products; GLC, chromato-mass spectroscopy;	A n/a B n/a C n/a D 5% E 75%

(μ-dithio)bis(tricarbonyliron) (14243-23-3) + Fe3-μ-(o-C6H4CH2NPh)(CO)8 → iron sulfide + Fe2-μ-(o-C6H4CH2NPh)(CO)6 + Fe3(CO)9S2 + iron (7439-89-6)

Conditions	Yield
In n-heptane N2 atmosphere; stirring (70°C, 40 min); filtn., evapn., chromy. (silica gel);	A n/a B 66% C 25% D n/a

benzothiaferrole (12086-84-9) → 2-thiocoumarin (3986-98-9) + iron (7439-89-6) + Benzo[b]thiophene (95-15-8)

Conditions	Yield
flash vac. pyrolysis in a Pyrex tube connected with a cold trap (E-5 Torr, 285-315°C); coating of the hot zone by Fe, rinsing of trap with acetone, GC;	A <1 B n/a C 63%
With ceric ammonium nitrate In acetone addn. of (NH4)2Ce(NO3)6 to a stirred soln. of Fe-compound in acetone (5 min, air), stirring for 2 h; monitored by TLC (hexane), filtn. (Celite), dilution of filtrate with ether, filtn. and evapn. to dryness, GLC of white crystals in acetone, TLC (CH2Cl2/hexane=1:1), (1)H NMR, IR, elem. anal.;	A 35.5% B 36% C 4.4%

iron pentacarbonyl (13463-40-6) → iron (7439-89-6)

Conditions	Yield
In not given byproducts: CO; Sonication; soln. of Fe(CO)5 in diphenylmethane sonicated for 3 h under Ar at 30 °C to give iron nanoparticles; removed by centrifugation, washed with pentane, dried under vac., detd. by Moessbauer spectroscopy, XRD;	53%
In further solvent(s) under Ar; thermolysis of Fe(CO)5 using heterogeneous nucleation technique (Proc. Phys. Soc. A 1949, 62, 562); diluted 2 times with octyl ether; Fe(CO)5 added (100°C); heated (260°C); cooled; EtOH (3:1 volume ratio to octyl ether); collected with magnet;	40%
With cis-Octadecenoic acid In further solvent(s) under Ar; thermolysis of Fe(CO)5 using heterogeneous nucleation technique (Proc. Phys. Soc. A 1949, 62, 562); oleic acid:oleylamine 1:1 molar ratio; diluted 2 times with octyl ether; Fe(CO)5 added (100°C); heated (260°C); cooled; EtOH (3:1 volume ratio to octyl ether); collected with magnet;	40%

lithiumpentamethylcyclopentadiene + ethanethiol (75-08-1) + iron(II) chloride → bis(pentamethylcyclopentadienyl)iron(II) (12126-50-0) + [(η5-pentamethylcyclopentadienyl)Fe(II)(μ2-SEt)3Fe(III)(η5-pentamethylcyclopentadienyl)] + iron (7439-89-6)

Conditions	Yield
With n-BuLi In tetrahydrofuran; hexane under Ar; FeCl2 added at 0°C to stirred suspn. of (C5Me5)Li in THF; stirred (1 h); cooled to -78°C; suspn. prepared from n-BuLi inn-hexane and HSEt at 0°C added; 1 h at -78°C; warmed to r oom temp. with stirring overnight; evapd. to dryness; purified by column chromy. (neutral alumina, n-hexane); insol. solid washed with H2O (Fe); elem. anal.;	A 9% B 49% C 15%

(η4-1,3-butadiene)tris(triethylphosphine)iron(0) (107339-80-0) → bis(η4-1,3-butadiene)(triethylphosphino)iron(II) (103835-78-5) + iron (7439-89-6)

Conditions	Yield
In tetrahydrofuran under Ar at 5°C;	A 40% B 40%

iron(II) bromide dimethoxyethane adduct (99611-53-7) + potassium dimethylnopadienide (1421320-35-5) → [Fe(η5-dimethylnopadienyl)2] + iron (7439-89-6)

Conditions	Yield
In tetrahydrofuran; toluene at 20℃; for 4h; Inert atmosphere;	A 28% B n/a

Fe(CO)4(COCH2CH2O) → 1,3-DIOXOLANE (646-06-0) + iron (7439-89-6)

Conditions	Yield
With H2 In decalin High Pressure; 71.5 atm H2 at room temp., heated to 200°C and stirred for 24 h; pressure realesed, detn. by GC and GC-MS;	A 27% B n/a

iron pentacarbonyl (13463-40-6) → triiron dodecarbonyl (17685-52-8) + iron (7439-89-6)

Conditions	Yield
In n-heptane; decalin Sonication; 0°C (Ar); products identified IR, UV, mass spect., chromy.;	A 9.8% B n/a
In octane Sonication; 0°C (Ar); products identified IR, UV, mass spect., chromy.;	A 6.9% B n/a
In decalin Sonication; 0°C (Ar); 0.1 M Fe(CO)5; products identified IR, UV, mass spect., chromy.;	A 4.7% B n/a

iron pentacarbonyl (13463-40-6) + hydrogen (1333-74-0) → iron(II,III) oxide + iron(II) oxide (1345-25-1) + iron(III) oxide + cementite + iron (7439-89-6)

Conditions	Yield
In neat (no solvent, gas phase) mixt. of vapor of Fe(CO)5 and H2 decomposed by plasma-chemical decomposition on Al2O3; monitored by XRD;	A n/a B n/a C n/a D 1% E n/a

ferric nitrate (7782-61-8) → iron (7439-89-6)

Conditions	Yield
Stage #1: ferric nitrate at 450℃; for 8h; Stage #2: With hydrogen at 500℃; for 16h;
In neat (no solvent) 15 min at 900°C under atomic hydrogen atmosphere;
With hydrogen In methanol Fe/MCM-41 prepd. by impregnation of MCM-41 with methanolic soln. of Fe(NO3)3 with stirring for 24 h under N2; catalyst filtered, washed with methanol, dried at 373 K and calcined at 773 K; catalyst reduced in H2 above 773 K;

C26H28Br2N4O4 → iron (7439-89-6)

Conditions	Yield
In tetrahydrofuran; methanol for 1h; Heating / reflux;

ammonium tris(bi(tetrazolato)amine)ferrate(III) → iron (7439-89-6)

Conditions	Yield
Heating / reflux;

potassium carbonate (584-08-7) + potassium ferrocyanide → potassium cyanate (590-28-3) + potassium cyanide + iron (7439-89-6)

Conditions	Yield
In melt at red heat; pression of KCN from iron sponge out;
In melt byproducts: N2; at red heat; extraction of KCN with H2O;
In melt at red heat; pression of KCN from iron sponge out;

ferrous(II) sulfate heptahydrate + ammonium chloride → iron (7439-89-6)

Conditions	Yield
In water Electrolysis; electrolysis of aq. soln. of FeSO4*7H2O and NH3 leads to precipitation of light grey iron on cathode;;

zinc ferrite → iron (7439-89-6) + zinc (7440-66-6)

Conditions	Yield
With H2 In neat (no solvent) sample heating in TG apparatus in 25% H2/He (50 ml/min) at 5 K/min up to800°C; TG;

iron(III) oxide → iron (7439-89-6)

Conditions	Yield
With hydrogen In neat (no solvent) Kinetics; byproducts: H2O; 300°C, carrier gas N2 or Ar + CH4 or CH4 + Ar + CO or air;
With hydrogen In gaseous matrix Kinetics; byproducts: H2O; sample redn. by 10% H2/Ar at 15 K/min up to 1000 K;
With hydrogen; gold In gaseous matrix Kinetics; byproducts: H2O; Au/Fe2O3 mixt. heating at 15 K/min in 10% H2/Ar (24 ml/min) up to 1260 K;
With hydrogen In gaseous matrix Kinetics; byproducts: H2O; sample heating at 15 K/min in 10% H2/Ar (24 ml/min) up to 1260 K;

iron oxide → iron (7439-89-6)

Conditions	Yield
In sodium hydroxide aq. NaOH; Electrolysis; in 50 wt % NaOH/water electrolyte at 110°C using Pt cylinder counter electrode and steel/adsorbed hematite as cathode; at -1.2 V vs. Hg/HgO;
With hydrogen hematite redn. at 500°C under hydrogen;

iron oxide + hydrogen (1333-74-0) → iron (7439-89-6)

Conditions	Yield
In neat (no solvent) Kinetics; reduced at 252.5-383°C under conditions without an external diffusion effect; TEM;

iron(II) metasilicate → iron (7439-89-6)

Conditions	Yield
In solid Electrolysis; electrolyzing molten FeSiO3 with addn. of either CaO or MgO leads to pptn. of Fe on cathode;;
In neat (no solvent) no redn. of feO to Fe in a stream of H at 850°C;;	0%
In neat (no solvent) no redn. of feO to Fe in a stream of H at 850°C;;	0%

sodium iron(III) pyrophosphate → iron (7439-89-6)

Conditions	Yield
In not given Electrolysis; electrolyzing soln. of NaFeP2O7 with bath potential 4 V;; contains Fe2O3 and pyrophosphorous acid;;

iron(II) chloride tetrahydrate → iron (7439-89-6)

Conditions	Yield
In water Electrolysis; electrolyzing soln. FeCl2*4H2O and NaCl (addn. of little HCl to clear soln.) at 50 to 70°C with current efficiency of 95 %;;
With ammonia In ethanol n-type Si(100) substrate coated with drop of soln. FeCl2*4H2O; dried; loaded on quartz boat into quartz tube reactor; heated under Ar; treated by NH3 with flow rate of 20 sccm for 1-10 min;
With sodium hydroxide In further solvent(s) heating FeCl2*4H2O and NaOH in propylene glycol; X-ray diffraction;

4,4-dimethyl-3-(2-nitrobenzyl)-2-oxazolidinone (907994-35-8) + iron (7439-89-6) → 4,4-dimethyl-3-(2-aminobenzyl)-2-oxazolidinone (907993-76-4)

Conditions	Yield
With ammonium chloride In ethanol; water	100%

5-methyl-3-(2-nitrobenzyl)-2-oxazolidinethione (907994-36-9) + iron (7439-89-6) → 5-methyl-3-(2-aminobenzyl)-2-oxazolidinethione (907993-79-7)

Conditions	Yield
With ammonium chloride In ethanol; water	100%

5-ethyl-3-(2-nitrobenzyl)-2-oxazolidinone (907994-37-0) + iron (7439-89-6) → 5-ethyl-3-(2-aminobenzyl)-2-oxazolidinone (907993-80-0)

Conditions	Yield
With ammonium chloride In ethanol; water	100%

5,5-dimethyl-3-(2-nitrobenzyl)thiazolidine-2-one (907994-43-8) + iron (7439-89-6) → 3-(2-aminobenzyl)-5,5-dimethylthiazolidine-2-one (907994-20-1)

Conditions	Yield
With ammonium chloride In ethanol; water	100%

3-hexyl-6-methyl-6-(3-nitrophenyl)-3-azabicyclo[3.1.0]hexan-2-one (280759-64-0) + iron (7439-89-6) → 6-(3-Aminophenyl)-3-hexyl-6-methyl-3-azabicyclo[3.1.0]hexan-2-one

Conditions	Yield
With calcium chloride In ethanol; water	100%

3-hexyl-6-isopropyl-6-(3-nitrophenyl)-3-azabicyclo[3.1.0]hexane + iron (7439-89-6) → 3-(3-hexyl-6-isopropyl-3-azabicyclo[3.1.0]hex-6-yl)aniline

Conditions	Yield
With calcium chloride In ethanol; dichloromethane; water	100%

3-hexyl-6-(3-nitrophenyl)-6-propyl-3-azabicyclo[3.1.0]hexane + iron (7439-89-6) → 3-(3-hexyl-6-propyl-3-azabicyclo[3.1.0]hex-6-yl)aniline

Conditions	Yield
With calcium chloride In ethanol; dichloromethane; water	100%

3-Hexyl-6-(3-nitrophenyl)-6-(2,2,2-trifluoroethyl)-3-azabicyclo[3.1.0]hexane-2,4-dione + iron (7439-89-6) → 3-Hexyl-6-(3-aminophenyl)-6-(2,2,2-trifluoroethyl)-3-azabicyclo[3.1.0]hexane-2,4-dione

Conditions	Yield
With calcium chloride In ethanol; dichloromethane; water	100%

hydrogenchloride (7647-01-0) + water (7732-18-5) + iron (7439-89-6) → iron(II) chloride tetrahydrate

Conditions	Yield
In water soln. of Fe in concd. HCl was refluxed; ppt. filtered off, washed with Et2O, dried in vac.;	100%
In hydrogenchloride evapn. a soln. of iron filings in dild. aq. HCl over iron filings until the hot soln. starts foaming; crystn. on cooling;; filtn.; crystn.; drying in a stream of dry air at 30-40°C;;
In hydrogenchloride evapn. a soln. of iron filings in dild. aq. HCl over iron filings until the hot soln. starts foaming; crystn. on cooling;; filtn.; crystn.; drying in a stream of dry air at 30-40°C;;
In water slight excess of 0.1 M hydrochloric acid added to iron powder, heated to dissolution; evapd.;
In hydrogenchloride iron powder and aq. HCl;

formic acid (64-18-6) + water (7732-18-5) + iron (7439-89-6) → iron(II) formate dihydrate

Conditions	Yield
at 250℃; for 16h; Inert atmosphere;	100%
In not given HCOOH was neutralized with Fe at 70-80°C; filtered, concd., cooled to room temp., recrystd. from water, dried in air;
Inert atmosphere;
Inert atmosphere;
In neat (no solvent) at 80℃;

5,10,15,20-tetraphenyl-21H,23H-porphine (917-23-7) + iron (7439-89-6) → 5,10,15,20-tetraphenyl porphyrin iron (16591-56-3)

Conditions	Yield
In toluene byproducts: H2; cocondensation of iron and toluene vapor at liq. nitrogen temp.; heating to -94.6°C; dropwise addn. of porphine soln. under nitrogen to the slurry (molar ratio Fe:porphine 4:1); gradually warming to 0°C, 1h; filtration; evapn. of filtrate;	100%
With Ag(111) In neat (no solvent) deposition of porphyrin deriv. onto silver by evapn. at 638 K, removing excess of porphyrin at 550 K, deposition of stoich. amount of iron; Buchner F., Schwald V., Cmanici K., Steinrueck H.-P., Marbach H. ChemPhysChem 2007, 8, 241-243; XPS and UPS;

iron (7439-89-6) + picrolonic acid (132-42-3) → iron picrolonate*H2O

Conditions	Yield
With HClO4 In water iron fillings dissolve in dilute HClO4, added aq. NaOH, resulting soln. added to aq. picrolonic acid at room temp.; ppt. filtered, washed with water, ethanol, ether, dried in vac. till constant weight, elem. anal.;	100%

lithium nitride + nitrogen (7727-37-9) + iron (7439-89-6) → Li2.7Fe0.3N

Conditions	Yield
In neat (no solvent) Li3N fused in pure iron vessel; sealed under 300 kPa of N2; heated at 850-1050°C for 12 h; thermally quenched; detd. by X-ray powder diffraction;	100%

uranium + selenium (7782-49-2) + iron (7439-89-6) → UFeSe3

Conditions	Yield
In melt (Ar glovebox) U, Fe and Se were placed in fused-silica ampoule, evacuated to about 1E-4 Torr, sealed, heated to 1173 K in 30 h, maintained at 1173 K for 2 days, cooled to 773 K in 6 days, maintained at 773 K for 2 days, cooled to 298 K over 6 h; washed with water and dried with acetone, XRD;	100%

1-(4-(7-(2-fluoro-4-nitrophenoxy)thieno[3,2-b]pyridin-2-yl)benzyl)pyrrolidin-2-one (1342835-29-3) + iron (7439-89-6) → 1-(4-(7-(4-amino-2-fluorophenoxy)thieno[3,2-b]pyridin-2-yl)benzyl)pyrrolidin-2-one (1342835-31-7)

Conditions	Yield
With ammonium chloride In water	100%

hydrogenchloride (7647-01-0) + iron (7439-89-6) → Fe(57)Cl2

Conditions	Yield
In water at 60℃; for 47h;	100%

zinc diacetate (557-34-6) + nickel diacetate (373-02-4, 14998-37-9, 33025-09-1, 94044-50-5, 98268-31-6) + oxalic acid (144-62-7) + iron (7439-89-6) → (x)Ni(2+)*(1-x)Zn(2+)*2Fe(2+)*3C2O4(2-)*99H2O

Conditions	Yield
In acetic acid heating of iron powder in a twofold excess of 1.5-2.0 M acetic acid under a N2 atmosphere; stirring; addn. of a soln. of Zn(2+) and Ni(2+) acetate; boilig; addn. of 3-5% excess 1 M oxalic acid; boiling for 1 h; filtration;; washing and drying at 100°C;;	99.8%
In acetic acid heating of iron powder in a twofold excess of 1.5-2.0 M acetic acid under a N2 atmosphere; stirring; addn. of a soln. of Zn(2+) and Ni(2+) acetate; boilig; addn. of 3-5% excess 1 M oxalic acid; boiling for 1 h;; frozen ppt. with liquid N2 (with total mother soln.) and then freeze dried;;

2,6-dichlorotoluene (118-69-4) + iron (7439-89-6) → 2,4-dichloro-3-methylbromobenzene (127049-87-0)

Conditions	Yield
With bromine; iodine In tetrachloromethane; (2S)-N-methyl-1-phenylpropan-2-amine hydrate	99.5%

3-allyl-6-methyl-6-(3-nitrophenyl)-3-azabicyclo[3.1.0]hexan-2-one + iron (7439-89-6) → 3-allyl-6-(3-aminophenyl)-6-methyl-3-azabicyclo[3.1.0]hexan-2-one

Conditions	Yield
With calcium chloride In methanol; ethanol; dichloromethane; water	99%

2,6-dibromo-4-nitro-pyridine 1-oxide (98027-81-7) + iron (7439-89-6) → 4-amino-2,6-dibromopyridine (39771-34-1)

Conditions	Yield
With acetic acid	99%

ferrous(II) sulfate heptahydrate + 2,2,4-trimethyl-4-[5-nitro-3-(3-phenylprop-2-ynyloxy)phenyl]-1,3-dioxolane (131341-02-1) + iron (7439-89-6) → 4-[5-amino-3-(3-phenylprop-2-ynyloxy)phenyl]-2,2,4-trimethyl-1,3-dioxolane

Conditions	Yield
With hydrogenchloride; triethylamine In methanol; water	99%

sodium bicarbonate water + 4-nitro-1-(4-trifluoromethoxyphenoxy)-2-trifluoromethylbenzene (875774-88-2) + iron (7439-89-6) → 4-(4-trifluoromethoxyphenoxy)-3-trifluoromethyl-aniline (875774-55-3)

Conditions	Yield
With hydrogenchloride In ethanol; water; ethyl acetate	99%

trifluorormethanesulfonic acid (1493-13-6) + iron (7439-89-6) + dimethyl sulfoxide (67-68-5) → iron(III) triflate - dimethylsulfoxide (1/6.2)

Conditions	Yield
With oxygen In dimethyl sulfoxide metal. Fe under O2 atm. treated with DMSO and triflic acid (3 equiv.) in3 portions, heated at 100°C for 24 h;	99%

picoline (108-89-4) + iron (7439-89-6) + thiourea (17356-08-0) → [4-methylpyridinium]2[Fe(isothiocyanate)4(4-methylpyridine)2]*2(4-methylpyridine)

Conditions	Yield
In further solvent(s) under Ar atm. using Schlenk techniques; metal powder, thiourea (excess),4-methylpyridine refluxed overnight; soln. refluxed for 4 ds; soln. coo led to room temp.; soln. layered (hexane); crystn.;	99%

trifluorormethanesulfonic acid (1493-13-6) + iron (7439-89-6) → iron(II) triflate

Conditions	Yield
In water stoich., Fe powder dissolved in aq. soln. of CF3SO3H by heating; ppt. filtered, dried (air), elem. anal.;	99%
In water metal compd. dissolved in aq. soln. of triflic acid; filtered, cocd., crystd., dried at 200°C for several h;
In water mixed, warmed in water;

6,6-Diphenylfulvene (2175-90-8) + iron (7439-89-6) → 1,1'-bis(diphenylmethyl)ferrocene

Conditions	Yield
In acetonitrile Electrolysis; iron anode, 0.1 M tetraethylammonium bromide base electrolyte, inert atmosphere, 40°C, current density 5 mA/cm*2; pptn. on water diln., collection (filtn.), dissoln. (acetone), repptn. on hexane addn., recrystn. (acetone);	99%
In dimethyl sulfoxide Electrolysis; iron anode, sodium bromide base electrolyte, inert atmosphere, 40°C, current density 5 mA/cm*2; pptn. on water diln., collection (filtn.), dissoln. (acetone), repptn. on hexane addn., recrystn. (acetone);	<80

Upstream product

• 7732-18-5 water 
• 7782-61-8 ferric nitrate 
• 7705-08-0 iron(III) chloride 
• 14362-44-8 iodide 
• 19229-76-6 iron(III) 
• 7440-31-5 tin 
• 7664-93-9 sulfuric acid 
• 15377-81-8 hexaaquairon(III) 
• 15969-58-1 titanium(II) 
• 16480-60-7 Fe₂Cl₆ 
• 47836-89-5 ferroin 
• 4119-52-2 iron(III) thiocyanate 
• 18475-84-8 iron(II) carbonyl dibromide 

Downstream Products

• 108-95-2 phenol 
• 92-52-4 biphenyl 
• 7722-84-1 dihydrogen peroxide 
• 10102-43-9 nitrogen(II) oxide 
• 22541-90-8 tin(II) 
• 7553-56-2 iodine 
• 19229-76-6 iron(III) 
• 4119-52-2 iron(II) thiocyanate 
• 10097-32-2 bromide 
• 16065-83-1 chromium (III) ion 
• 125920-89-0 {Fe(II)-(gallacetophenone phenylhydrazone)2(water)2} 
• 10097-32-2 bromine 
• 16397-91-4 manganese(II) 
• 7440-57-5 gold 

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