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This article is about iron the metal. For the tool called iron, see ironing.
A chunk of iron

Iron (Fe) is the second most common metal on Earth, and the most widely-used metal. It is element 26, a transition metal in Group 8. Its symbol is Fe, from the Latin word for iron, ferrum. Its atomic number is 26 and its mass number is 55.85.

It is used a lot because it is very strong and cheap. Iron is the main ingredient used to make steel. Raw iron is attracted to magnets, but it is not actually a magnet, however it can be used to make an electromagnet.


Iron(III) oxide
Iron(II) oxide
Iron(II) sulfate
Iron(III) chloride

Physical properties

Iron is a grey, silvery metal. It is magnetic. It is easy to mine and make, which is why it is so useful. Pure iron is soft and very malleable(elastic) and is able to stretch a lot, while steel (iron mixed with a little carbon) is stronger and does not stretch as much as iron.

Chemical properties

Iron is reactive. It reacts with most acids like sulfuric acid. It makes ferrous sulfate when reacted with sulfuric acid. This reaction with sulfuric acid is used to clean metal.

Iron reacts with air and water to make rust. When the rust flakes off, more iron is exposed allowing more iron to rust. Eventually, the whole piece of iron is rusted away. Other metals like aluminum do not rust away. Iron can be alloyed with chromium and carbon to make stainless steel, which does not rust under most conditions.

Iron powder can react with sulfur to make iron(II) sulfide, a hard black solid. Iron also reacts with the halogens to make iron(III) halides, like iron(III) chloride. Iron reacts with the hydrohalic acids to make iron(II) halides like iron(II) chloride.

Chemical compounds

Iron makes chemical compounds with other elements. Normally the other element oxidizes iron. Sometimes two electrons are taken and sometimes three. Compounds where iron has two electrons taken are called ferrous compounds. Compounds where iron has three electrons taken are called ferric compounds. Ferrous compounds have iron in its +2 oxidation state. Ferric compounds have iron in its +3 oxidation state. Iron compounds can be black, brown, yellow, green, or purple.

Ferrous compounds are weak reducing agents. Many of them are green or blue. The most common ferrous compound is ferrous sulfate.

Ferric compounds are oxidizing agents. Many of them are brown. The most common ferric compound is ferric oxide, the same thing as rust. One reason why iron rusts is because ferric oxide is an oxidizing agent. It oxidizes iron, rusting it even under paint. That is why if there is a small scratch in the paint, the whole thing can rust.

Iron(II) compounds

Compounds in the +2 oxidation state are weak reducing agents. They are normally light colored. They react with oxygen in air. They are also known as ferrous compounds.

Mixed oxidation state

These compounds are rare; only one is common. They are found in the ground.

Iron(III) compounds

Compounds in the +3 oxidation state are normally brown. They are oxidizing agents. The are corrosive. They are also known as ferric compounds.

Iron in the ground

Iron metal is almost never found in native form in nature. Some Meteorites contain iron in the form of rare minerals. Normally iron is found as hematite ore in the ground. Iron can be easily extracted from the ore in a blast furnace.

Iron is present in meat. Iron is also found in hemoglobin in red blood cells.

Making iron

Blast furnace

Iron is made in large factories called ironworks by reducing hematite with carbon (coke). This happens in large containers called blast furnaces. The blast furnace is filled with iron ore, coke and limestone. A very hot blast of air is blown in, where it causes the coke to burn. The extreme heat makes the carbon react with iron ore, taking off the oxygen from iron oxides, and making carbon dioxide. The carbon dioxide is a gas and it leaves the mix. There is some sand in with the iron. The limestone, which is made of calcium carbonate, turns into calcium oxide and carbon dioxide when the limestone is very hot. The calcium oxide reacts with the sand to make a liquid called a slag. The slag is drained, leaving only the iron. The reaction will leave pure liquid iron in the blast furnace, where it can be shaped and hardened after cooling down. Almost all ironworks are today part of steel mills, and almost all iron is made into steel.

There are many ways to work iron. Iron can be hardened by heating a piece of metal and splashing it into cold water. It can be softened by heating it and allowing it to slowly cool. It can also be stamped by a heavy press. It can be pulled into wires. It can be rolled to make sheet metal.

In the United States, much of the iron was taken from the ground in Minnesota and then sent by ship to Indiana and Michigan where it was made into steel.


As a metal

A bridge made out of iron

Iron is used more than any other metal. It is strong and cheap. It is used to make buildings, bridges, nails, screws, pipes, girders, and towers.

Iron is not very reactive, so it is both easy and cheap to extract from ores. It is very strong once made into steel, and is used to reinforce concrete.

There are different types of iron. Cast iron is iron made by the way described above in the article. It is hard and brittle. It is used to make things like storm drain covers, manhole covers, and engine blocks (the main part of an engine).

Steel is the most common form of iron. Steels come in several forms. Mild steel is steel with a low percentage of carbon. It is soft and easily bent, but it does not crack easily. It is used for nails and wires. Carbon steel is harder but more brittle. It is used in tools. There are many other types of steel. Stainless steel because of the chromium content is rust resistant and nickel-iron alloys are very tolerant of high temperatures. Other steels can be very hard, depending on the alloys added.

Wrought iron is easily shaped and used to make fences and chains.

Very pure iron is soft, and can rust(oxidize) easily. It is also fairly reactive.

As compounds

Iron compounds are used for several things. Iron(II) chloride is used to make water clean. Iron(III) chloride is also used. Iron(II) sulfate is used to reduce chromates in cement. Some iron compounds are used in vitamins.

Use in food

Our bodies need iron to help oxygen get to our muscles, because the molecule is at the heart of some essential macromolecules in our bodies such as hemoglobin cause the heart to work better. Many cereals have some added iron (the element metal iron).[1][2] It is added to cereal in the form of tiny metal filings. It is even possible to see the slivers sometimes by taking an extremely strong magnet and putting it into the box. The magnet will attract these pieces of iron. Eating these small metal shavings are not harmful to our body.[3]

Iron is most available to the body when added to amino acids – iron in this form is ten to fifteen times more digestible than than it is as an element.[4] Iron is also found in meat, for example steak. Iron provided by diet supplements is in the form of a chemical, such as a sulphate, which is cheap and is absorbed well. The body will not take up more iron than it needs, and it usually needs very little. The iron in red blood cells is recycled by a system which breaks down old cells. Loss of blood by injury or parasite infection may be more serious.[5]


Iron is toxic when large amounts are swallowed. It can damage the body. When too many vitamins that have iron in them are eaten, people get sick. There are chemicals that doctors have that can react with iron and stop it from poisoning people.

Related pages


  1. "Testing the Fortitude of Iron in Cereals". United States Department of Agriculture. Retrieved 2010-01-29.
  2. Adams, Cecil. Return of the Straight Dope. New York: Ballantine Books, 1994
  3. Felton, Bruce. One of a Kind. New York: William Morrow and Co., 1992
  4. Pineda O, Ashmead HD (2001). "Effectiveness of treatment of iron-deficiency anemia in infants and young children with ferrous bis-glycinate chelate". Nutrition 17 (5): 381–4. doi:10.1016/S0899-9007(01)00519-6 . PMID 11377130 .
  5. Andrews N.C. 2000. Disorders of iron metabolism. New England Journal of Medicine. Related correspondence, published in NEJM 342:1293-1294.