Pure Iron

Pure Iron

Iron is a chemical element with symbol Fe (from Latin word Ferrum). Its atomic number is 26 and atomic mass is 55.85. It has a melting point of 1538 deg C and boiling point of 2862 deg C. It is a metal in the first transition series. It is by mass the most common element on the earth, forming much of earth’s outer and inner core. It is the fourth most common element and the second most common metal in the earth crust. Steels contain over 95 % Fe.

Pure iron is a common metal but it is mostly confused with other metals such as steel and wrought iron. All these metals vary in composition. The carbon content of pure iron makes it unique and different from the other metals and ferrous alloys. The carbon content in pure iron is always less than 0.008 %. Wrought iron has a higher carbon content of up to 0.5 %. This shows how less the impurities are in the pure iron.

Pure iron is silvery white colored metal and is extremely lustrous. Its most important property is that it is very soft. It is easy to work and shape and it is just soft enough to cut through (with quite a bit of difficulty) using a knife. Pure iron can be hammered into sheets and drawn into wires. It conducts heat and electricity and is very easy to magnetize. Its other properties include easy corrosion in the presence of moist air and high temperatures.

Pure iron has got valencies +2 and +3. Compounds of iron with valency +2 are known as ferrous compounds while the compounds of iron with valency +3 are known as ferric compounds.

Metallurgy of pure iron

The metallurgical nature of solid pure iron can be studied from the experiment as described here. A bar of pure iron (e.g., 25 mm in diameter) is sectioned to form a thin disk in the shape of a quarter. A face of the disk is now polished on polishing wheels, starting first with a coarse grit polish and proceeding in steps with ever finer grits until the face has the appearance of a shiny mirror. The shiny disk is now immersed for around 20 to 30 seconds in a mixture of 2 % to 5 % nitric acid (HNO3) with methyl alcohol, a mixture often called nital (‘nit’ for the acid and ‘al’ for the alcohol). This process of etching causes the shiny surface to become a dull color. If the sample is now viewed in an optical microscope at a magnification of 100 ×, it is found to have the appearance as shown in Fig 1.

The individual regions, such as those numbered 1 to 5, are called iron grains, and the boundaries between them, such as that between grains 4 and 5 highlighted with an arrow, are called grain boundaries. The average size of the grains is quite small. In the figure at the 100× magnification, a length of 200 microns (1 micron is 0.001 mm and is also known as micrometer) is shown by the arrow so labeled. The average grain diameter for this sample has been measured to be 125 microns. Although a small number, this grain size is much larger than the grain size of most commercial irons. For a comparison, the thickness of aluminum foil and the diameter of a hair are both approximately 50 microns.

Microstructure of pure iron

Fig 1 Microstructure of pure iron showing grains, grain boundary and crystal structure

In pure iron the basic building blocks are the individual atoms of iron (Fe) atoms. The grains shown in Fig 1 are called crystals and they are made up of atoms, all of the atoms are uniformly arranged in layers. As shown in Fig 1, if lines are drawn connecting the centres of the atoms, a three-dimensional array of little cubes stacked together to fill space is generated. In iron at room temperature, the cubes have an atom at each of the eight corners and one atom right in the middle of the cube. This crystal structure is called a body-centered cubic (bcc) structure, and the geometric arrangement of atoms is often called a bcc lattice. In the Fig 1, the crystal lattice can be envisioned as three sets of intersecting planes of atoms, with each plane set parallel to one face of the cube.

Iron with a bcc structure is called ferrite. Another name for ferrite is alpha iron. The nature of a grain boundary is shown in Fig 1. The boundary is a planar interface, generally curved, along which two grains of different orientation intersect. The ‘A’ planes in grain 4 make a much steeper angle with the horizontal than do the ‘A’ planes of grain 3. If grain 4 is rotated clockwise to cause its ‘A’ planes to line up with the ‘A’ planes of grain 3, then the grain boundary gets removed and the two grains become one larger grain.

Upon heating pure Iron experiences two changes in crystal structure. The first change occurs when the iron is heated to 912 deg C. At this temperature the crystal structure changes spontaneously from bcc to a new structure called face-centered cubic (fcc). This structure is also shown in Fig 1, where it is seen that the atoms lie on the corners of a cube as well as one atom at each of the six faces of the cube. Like the low temperature bcc structure, this structure is called either austenite or gamma iron.

When the ferritic iron is heated to 912 deg C, the old set of ferrite grains changes (transforms) into a new set of austenite grains. As the ferrite grain structure reaches the transformation temperature, there are initially the formations of a new set of very small austenite grains forming on the old ferrite grain boundaries, and then the growth of these grains take place until all the old ferrite grains disappear. Two important effects occur when ferrite changes to austenite. These are given below.

  • It needs heat energy to change the ferrite grains into austenite grains. Therefore, on heating, the iron temperature remains close to 912 deg C until all the ferrite grains are transformed.
  • The ferrite-to-austenite transformation is accompanied by a volume change. The density of austenite is 2 % higher than the ferrite, which means that the volume per atom of iron is less in austenite.

If the heating of iron is continued beyond 912 deg C, then the second change in the crystal structure occurs at 1394 deg C when the austenitic grains of iron reverts back to body-centered cubic (bcc) structure known as delta ferrite. On further heating pure iron melts at its melting temperature of 1538 deg C.

At 770 deg C known as the Curie point, iron becomes magnetic.  As the iron passes through the Curie temperature there is no change in crystalline structure, but there is a change in the ‘domain structure’, where each domain contains iron atoms with a particular electronic spin. In non-magnetized iron, all the electronic spins of the atoms within one domain are in the same direction, however, the neighboring domains point in various other directions and thus overall they cancel each other out. As a result, the iron is non-magnetized. In magnetized iron, the electronic spins of all the domains are aligned, so that the magnetic effects of neighboring domains reinforce each other.  When the structure of iron was being discovered in the late 19th century, the magnetic transition in iron occurring at 770 deg C caused scientists to theorize a structure of iron they called beta iron, which was later shown not to exist.

Although each domain contains billions of atoms, they are very small, about 10 microns across. At pressures above approximately 10 GPa (Giga Pascal) and temperatures of a few hundred kelvin or less, alpha iron changes into a hexagonal closed packed (hcp) structure, which is also known as eta iron. The higher temperature gamma phase also changes into eta iron, but does so at higher pressure.

Alpha iron is the most stable form of iron at normal temperatures. It is a fairly soft metal that can dissolve only a small concentration of carbon (no more than 0.021 % by mass at 910 deg C. Gamma iron is also soft and metallic but can dissolve considerably more carbon (as much as 2.04 % by mass at 1146 deg C).

Commercially produced pure iron

Pure iron is a term used to describe new iron produced in an electric arc furnace where temperatures sufficient to melt the iron can be achieved. The result, also known as ‘butter iron’ is typically around 99.8 % pure with an approximate carbon content of 0.005 % and manganese content of 0.005 %. There are also traceable amounts of a number of other elements some of which add certain properties or characteristics to the material and others which are of no significance.

Pure Iron, with a minimum Fe content of 99.85 %, without the addition of alloy elements was first developed in 1909 by the former American Rolling Mill Company (ARMCO).

The typical analysis of the commercially produced pure iron is given in Tab 1. The ultimate tensile strength (UTS) of commercially produced pure iron is between 230 to -370 N/sq mm which is similar to that of new high grade wrought iron.  There is little difference between the two materials other than the fact that pure iron does not contain any slag or laminations and has superior corrosion resistance.

Tab 1 Typical composition of commercial pure iron
Element %Element%
Tellurium0.001Hydrogen1.1 ppm


Commercial pure iron has many different characteristics which include (i) improved resistance to corrosion and oxidation, (ii) excellent magnetic properties, (iii) high chemical and metallurgical purity, (iv) excellent hot and cold forming capability, and (v) it is suitable for all types of welding.

Pure Iron is largely used in the production of relatively small volumes of special alloy steels, in the aviation, automotive, construction, petrochemical industries, and in the manufacture of magnets, gaskets, fuse wire, welding rods, lighting conductors and MRI (magnetic resonance imaging) scanners.

In France, pure Iron has become the preferred material for the restoration of wrought ironwork. More and more British blacksmiths are also choosing pure Iron for restoration, new build, and artwork.

Comparison of pure iron with wrought iron

Wrought iron has a higher carbon content of up to 0.5 % against less than 0.008 % carbon content of pure iron. The other attribute is the structure. The structure of pure iron is homogenous whereas the wrought iron has a laminated structure. This makes wrought iron a very suitable material for civil engineering projects such as the Eiffel Tower because it has longitudinal strength. One of the disadvantages of this laminated structure is the way in which it corrodes. Whereas a homogenous material like pure iron rusts from the outside, wrought iron has a tendency to form layers of rust between the laminations (crevice corrosion) which can eventually lead to the material literally blowing itself and its surroundings apart. Evidence of this can be seen in many of the old buildings where wrought iron fixings have split stonework apart necessitating expensive repairs and renewals. Also many old park railings and gates are suffering from the same syndrome. Though pure iron also forms rust only on its outer surfaces, it does not rust as readily as mild steel.  Pure iron is 22 % more corrosion resistant than wrought iron.

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