What is the boiling point of iron

Pure iron (99.97%), purified by electrolysis

Iron

- a malleable silver-white metal with high chemical reactivity: iron quickly corrodes at high temperatures or high humidity in the air. Iron burns in pure oxygen, and in a finely dispersed state it spontaneously ignites in air. Denoted by the symbol Fe (Latin Ferrum). One of the most common metals in the earth's crust (second place after aluminum).

Two modifications of the iron crystal lattice

Several polymorphic modifications have been established for iron, of which the high-temperature modification - γ-Fe (above 906°) forms a lattice of a face-centered cube of the Cu type (a = 3.63), and the low-temperature modification - the α-Fe lattice of a centered cube of the α-Fe type (a = 2.86). Depending on the heating temperature, iron can be found in three modifications, characterized by different crystal lattice structures:

In the temperature range from the lowest to 910 ° C - a-ferrite (alpha ferrite), which has a crystal lattice structure in the form of a centered cube;
In the temperature range from 910 to 1390°C - austenite, the crystal lattice of which has the structure of a face-centered cube;
In the temperature range from 1390 to 1535 ° C (melting point) - d-ferrite (delta ferrite). The crystal lattice of d-ferrite is the same as that of a-ferrite. The only difference between them is the different (larger for d-ferrite) distances between the atoms.

When liquid iron is cooled, primary crystals (crystallization centers) appear simultaneously at many points in the cooled volume. With subsequent cooling, new crystalline cells are built around each center until the entire supply of liquid metal is exhausted. The result is a granular structure of the metal. Each grain has a crystal lattice with a certain direction of its axes. With subsequent cooling of solid iron, during the transitions of d-ferrite to austenite and austenite to a-ferrite, new crystallization centers may appear with a corresponding change in grain size

In its pure form under normal conditions it is a solid. It has a silver-gray color and a pronounced metallic luster. The mechanical properties of iron include its level of hardness on the Mohs scale. It is equal to four (average). Iron has good electrical and thermal conductivity. The last feature can be felt by touching an iron object in a cold room. Because this material conducts heat quickly, it removes most of it from your skin in a short period of time, which is why you feel cold. If you touch, for example, wood, you will notice that its thermal conductivity is much lower. The physical properties of iron include its melting and boiling points. The first is 1539 degrees Celsius, the second is 2860 degrees Celsius. We can conclude that the characteristic properties of iron are good ductility and fusibility. But that's not all. Also, the physical properties of iron include its ferromagnetism. What it is? Iron, whose magnetic properties we can observe in practical examples every day, is the only metal that has such a unique distinctive feature. This is explained by the fact that this material is capable of magnetization under the influence of a magnetic field. And after the end of the action of the latter, the iron, the magnetic properties of which have just been formed, remains a magnet for a long time. This phenomenon can be explained by the fact that in the structure of this metal there are many free electrons that are able to move.

RESERVES AND PRODUCTION

Iron is one of the most common elements in the solar system, especially on the terrestrial planets, in particular on Earth. A significant part of the iron of the terrestrial planets is located in the cores of the planets, where its content is estimated to be about 90%. The iron content in the earth's crust is 5%, and in the mantle about 12%.

Iron is quite widespread in the earth's crust - it accounts for about 4.1% of the mass of the earth's crust (4th place among all elements, 2nd among metals). In the mantle and earth's crust, iron is concentrated mainly in silicates, while its content is significant in basic and ultrabasic rocks, and low in acidic and intermediate rocks. A large number of ores and minerals containing iron are known. Of greatest practical importance are red iron ore (hematite, Fe2O3; contains up to 70% Fe), magnetic iron ore (magnetite, FeFe2O4, Fe3O4; contains 72.4% Fe), brown iron ore or limonite (goethite and hydrogoethite, respectively FeOOH and FeOOH nH2O ). Goethite and hydrogoethite are most often found in weathering crusts, forming so-called “iron hats”, the thickness of which reaches several hundred meters. They can also be of sedimentary origin, falling out of colloidal solutions in lakes or coastal areas of the seas. In this case, oolitic, or legume, iron ores are formed. Vivianite Fe3(PO4)2·8H2O is often found in them, forming black elongated crystals and radial aggregates. The iron content in sea water is 1·10−5 -1·10−8% In industry, iron is obtained from iron ore, mainly from hematite (Fe2O3) and magnetite (FeO·Fe2O3). There are various ways to extract iron from ores. The most common is the domain process. The first stage of production is the reduction of iron with carbon in a blast furnace at a temperature of 2000 °C. In a blast furnace, carbon in the form of coke, iron ore in the form of agglomerate or pellets, and flux (such as limestone) are fed from above, and are met by a stream of forced hot air from below. In addition to the blast furnace process, the process of direct iron production is common. In this case, pre-crushed ore is mixed with special clay, forming pellets. The pellets are fired and treated in a shaft furnace with hot methane conversion products, which contain hydrogen. Hydrogen easily reduces iron without contaminating the iron with impurities such as sulfur and phosphorus, which are common impurities in coal. Iron is obtained in solid form and is subsequently melted in electric furnaces. Chemically pure iron is obtained by electrolysis of solutions of its salts.

Methods for obtaining metal

There are several ways to get iron:

Direct methods. This is the production of sponge iron in shaft and tunnel furnaces. Production of iron dough in rotary kilns. It is possible to obtain iron in fluidized bed reactors and the chemical-thermal method.
The blast furnace process is a common method. Iron ore and flux are reduced by carbon from coke, resulting in cast iron. If necessary, impurities (phosphorus, sulfur) and excess carbon are removed from cast iron in open-hearth furnaces or converters. Alloy steel is produced in electric furnaces (ESF).
Chemically pure iron can be obtained from a solution of its salts using electrolysis.

ORIGIN

Origin telluric (terrestrial) iron is rarely found in basalt lavas (Uifak, Disko Island, off the western coast of Greenland, near Kassel, Germany). At both locations, pyrrhotite (Fe1-xS) and cohenite (Fe3C) are associated with it, which is explained by both the reduction by carbon (including from the host rocks) and the decomposition of carbonyl complexes such as Fe(CO)n. In microscopic grains, it has more than once been established in altered (serpentinized) ultrabasic rocks, also in paragenesis with pyrrhotite, sometimes with magnetite, due to which it arises during reduction reactions. Very rarely found in the oxidation zone of ore deposits, during the formation of swamp ores. Findings have been recorded in sedimentary rocks associated with the reduction of iron compounds with hydrogen and hydrocarbons. Almost pure iron was found in lunar soil, which is associated with both meteorite falls and magmatic processes. Finally, two classes of meteorites - stony-iron and iron - contain natural iron alloys as a rock-forming component.

Chemical composition

Telluric iron contains impurities of nickel (Ni) 0.6-2%, cobalt (Co) up to 0.3%, copper (Cu) up to 0.4%, platinum (Pt) up to 0.1%, carbon. Native iron usually contains Ni in solid solution. The composition of individual varieties has not been precisely established; the analyzes are mostly old, performed on material not verified by mineragraphic and x-ray studies. Minor admixtures of Co, Cu, S, C, Mn, P, Pt, As, Ge have been identified, partly associated, apparently, with a mechanical admixture of cohenite; the presence of gas inclusions (CO and CO2) was noted.

Varieties

Ferrite (Vernadsky, 1912) is the purest, almost Ni-free native iron. Awaruite - awaruite (Skei, 1885) 6 -(Ni, Fe). Native nickel-iron with a high Ni content (Ni: Fe from 4: 1 to 2: 1). Hardness. 5. Density 8.1. It resembles polyxene in luster and color. In reflected light, pure white or light cream, isotropic, highly reflective. Named for its location in Avarua Bay (New Zealand), where it is associated with gold, platinum, cassiterite, chromite, and magnetite. It is found as a secondary mineral in peridotites that have undergone serpentinization, serpentinites, trachytes, and quartz porphyries. Varieties of nickel-iron of terrestrial origin close to or identical to awaruite, found in placers and in serpentinized peridotites, are described under the names: josephinite (Melville, 1892), souesite-souesite (Hofman, 1905), octibbehite (Taylor, 1905). 1857), catarinite - satarinite (Damur, 1877). Under the name bobrovkite (Vysotsky, 1913), nickel-iron (iron-nickel) is described, found in the form of fine-scaled grains together with platinum (polyxene) in the placers of M. Bobrovka (Ural). Contains Ni 71.93, Fe 28.07, as well as Co, Mn.

APPLICATION

Iron ring

Iron is one of the most used metals, accounting for up to 95% of global metallurgical production. Iron is the main component of steels and cast irons - the most important structural materials. Iron can be part of alloys based on other metals - for example, nickel. Magnetic iron oxide (magnetite) is an important material in the production of long-term computer memory devices: hard drives, floppy disks, etc. Ultrafine magnetite powder is used in many black and white laser printers mixed with polymer granules as a toner. This uses both the black color of the magnetite and its ability to stick to the magnetized transfer roller. The unique ferromagnetic properties of a number of iron-based alloys contribute to their widespread use in electrical engineering for magnetic cores of transformers and electric motors. Iron(III) chloride (ferric chloride) is used in amateur radio practice for etching printed circuit boards. Ferrous sulfate heptate (ferrous sulfate) mixed with copper sulfate is used to combat harmful fungi in gardening and construction. Iron is used as an anode in iron-nickel batteries and iron-air batteries. Aqueous solutions of ferrous and ferric chlorides, as well as its sulfates, are used as coagulants in the purification processes of natural and waste water in the water treatment of industrial enterprises.

Melting point table for metals

Each metal or alloy has unique properties, including its melting point. In this case, the object passes from one state to another, in a particular case, it becomes liquid from solid. To melt it, you need to apply heat to it and heat it until the desired temperature is reached. At the moment when the desired temperature point of a given alloy is reached, it may still remain in a solid state. As exposure continues, it begins to melt.

Mercury has the lowest melting point - it melts even at -39 °C, tungsten has the highest - 3422 °C. For alloys (steel and others) it is extremely difficult to determine the exact figure. It all depends on the ratio of the components in them. For alloys it is written as a numerical interval.

Metal alloys

To design products from alloys, their properties are first studied. To study, the metals being studied are melted in small containers in different ratios to each other. Based on the results, graphs are built.

The lower axis represents the concentration of component A with component B. The vertical axis is temperature. Here the values of the maximum temperature are noted when all the metal is in a molten state.

When cooled, one of the components begins to form crystals. In a liquid state, eutectic is an ideal compound of metals in an alloy.

Metallurgists identify a special ratio of components at which the melting point is minimal. When making alloys, they try to select the amount of substances used in order to obtain a eutectoid alloy. Its mechanical properties are the best possible. Crystal lattices form ideal face-centered positions of atoms.

The crystallization process is studied by studying the hardening of samples upon cooling. They build special graphs where they observe how the cooling rate changes. Ready-made diagrams are available for different alloys. By marking the start and end points of crystallization, the composition of the alloy is determined.

How the process works

Elements, whatever they are: gold, iron, cast iron, steel or any other, melt approximately the same. This occurs due to external or internal heating. External heating is carried out in a thermal furnace. For internal applications, resistive heating is used, passing an electric current or induction heating in a high-frequency electromagnetic field . The impact is approximately the same.

When heating occurs , the amplitude of thermal vibrations of molecules increases. Structural lattice defects appear , accompanied by the rupture of interatomic bonds. The period of lattice destruction and accumulation of defects is called melting.

Depending on the degree at which metals melt, they are divided into:

low-melting - up to 600 °C: lead, zinc, tin;
medium-melting - from 600 °C to 1600 °C: gold, copper, aluminum, cast iron, iron and most of all elements and compounds;
refractory - from 1600 °C: chromium, tungsten, molybdenum, titanium.

Depending on what the maximum degree is, the melting apparatus is selected. It should be stronger the stronger the heating.

The second important value is the boiling degree. This is the parameter at which liquids begin to boil. As a rule, it is twice the melting point. These values are directly proportional to each other and are usually given at normal pressure.

If the pressure increases, the amount of melting also increases. If the pressure decreases, then it decreases.

Characteristics table

Metals and alloys are an indispensable basis for forging , foundry, jewelry and many other areas of production. Whatever the craftsman does ( gold jewelry , cast iron fences, steel knives or copper bracelets) , in order to work correctly, he needs to know the temperatures at which this or that element melts.

To find out this parameter, you need to refer to the table. In the table you can also find the boiling degree.

Among the most commonly used elements in everyday life, the melting point indicators are as follows:

aluminum - 660 °C;
copper melting point - 1083 °C;
melting point of gold - 1063 °C;
silver - 960 °C;
tin - 232 °C. Tin is often used for soldering, since the temperature of a working soldering iron is exactly 250–400 degrees;
lead - 327 °C;
melting point of iron - 1539 °C;
the melting point of steel (an alloy of iron and carbon) is from 1300 °C to 1500 °C. It varies depending on the saturation of the steel with components;
melting point of cast iron (also an alloy of iron and carbon) - from 1100 °C to 1300 °C;
mercury - -38.9 °C.

As is clear from this part of the table, the most fusible metal is mercury, which at positive temperatures is already in a liquid state.

The boiling point of all these elements is almost twice, and sometimes even higher than the melting point. For example, for gold it is 2660 °C, for aluminum - 2519 °C , for iron - 2900 °C, for copper - 2580 °C, for mercury - 356.73 °C.

For alloys such as steel, cast iron and other metals, the calculation is approximately the same and depends on the ratio of components in the alloy.

The maximum boiling point of metals is rhenium - 5596 ° C. The highest boiling point is for the most refractory materials.

There are tables that also indicate the density of metals . The lightest metal is lithium, the heaviest is osmium. Osmium has a higher density than uranium and plutonium when viewed at room temperature. Light metals include: magnesium, aluminum, titanium. Heavy metals include most common metals: iron, copper, zinc, tin and many others. The last group is very heavy metals, these include: tungsten, gold, lead and others.

Another indicator found in the tables is the thermal conductivity of metals . Neptunium is the worst conductor of heat, and the best metal in terms of thermal conductivity is silver. Gold, steel, iron, cast iron and other elements are in the middle between these two extremes. Clear characteristics for each can be found in the required table.

B. Meteoric iron

Kamacite – Kamacite – nickel iron (6-9% Ni). The name kamacite comes from the Greek - beam, rod (Reichenbach, 1861),

A synonym for kamacite is beam iron, taenite is band iron (Reichenbach, 1861), edmonsonite (Flight, 1882). Plessite (Reichenbach, 1861) is a fine mixture of kamacite and taenite.

Taenite – Taenite – nickel-iron (up to 48% Ni), taenite – from Taivia - ribbon, strip (Reichenbach, 1861).

For taenite of the Fe2Ni composition, the following names have been proposed: nikdiferrite (Chirvinsky, 1928), orthotenite (Badhu, 1936) and chirvinite (Astapovich, 1950); a compound of this composition is established in the Fe-Ni system. Metakamacite is a metastable a-modification of pickled iron, and, in addition, a granular variety of plessite (Owen, 1940). Metatenite is taenite with an admixture of kamacite (Badhyo, 1936).

Native iron of cosmic origin makes up the mass of iron meteorites. Found in most stony meteorites. Forms:

a) a solid mass of a meteorite;

b) a spongy mass in which grains of olivine or other silicates are immersed;

c) grains and scales scattered throughout the meteorite;

d) separate crystalline individuals with numerous twin plates. Kamacite and taenite are always closely intergrown. Iron meteorites from the octahedrite group are characterized by systems of intersecting stripes, which are called Widmanstätten figures: individual stripes consist of kamacite with taenite rims, with plessite between the intersecting stripes. Widmanstätten figures arise as a result of the decomposition of a solid solution of γ-iron and nickel. In intergrowths of kamacite and taenite, the plane of the rhombic dodecahedron (110) of kamacite is parallel to the plane of the octahedron (111) of taenite, which is explained by their structural similarity.

Boiling point of iron in degrees

Iron is the first most important and widespread structural material. It has been known since ancient times, and its properties are such that when they learned to smelt iron in significant quantities, the metal replaced all other alloys. The age of iron has arrived and, judging by the scope of its application, this time will not end soon. This article will tell you what the specific density of iron is and what its melting point is in its pure form.

History of discovery

Everyone remembers the “Iron Age” from school. This is the period in history when man first learned to extract this metal from ore. The Iron Age spans the period from the 9th to the 7th century BC. This metal had a huge influence on the development of people of that time. According to its characteristics, it has replaced mixtures of non-ferrous metals. Tools, weapons, armor, materials for construction and much more were made from it. Gradually, blacksmiths began to mix it with other metals to create new materials. This is how new alloys appeared.

Composition and structure of iron

Iron is a typical metal, and it is chemically active. The substance reacts at normal temperature, and heating or increasing humidity significantly increases its reactivity. Iron corrodes in air, burns in an atmosphere of pure oxygen, and in the form of fine dust can ignite in air.

Pure iron is inherently malleable, but the metal is very rare in this form. In fact, iron means an alloy with small proportions of impurities - up to 0.8%, which is characterized by the softness and malleability of a pure substance. Alloys with carbon - steel, cast iron, stainless steel - are important for the national economy.

Iron is characterized by polymorphism: there are as many as 4 modifications, differing in structure and lattice parameters:

α-Fe – exists from zero to +769 C. It has a body-centered cubic lattice and is ferromagnetic, that is, it retains magnetization in the absence of an external magnetic field. +769 C – Curie point for metal;
from +769 to +917 C β-Fe appears. It differs from the α phase only in lattice parameters. Almost all physical properties are preserved with the exception of magnetic ones: iron becomes paramagnetic, that is, it loses the ability to magnetize and is drawn into a magnetic field. Metallurgy does not consider the β-phase as a separate modification. Since the transition does not affect significant physical characteristics;
in the range from 917 to 1394 C there is a γ-modification, which is characterized by a face-centered cubic lattice;
at temperatures above +1394 C, the δ phase appears, which is characterized by a body-centered cubic lattice.

STRUCTURE

Two modifications of the iron crystal lattice

Several polymorphic modifications have been established for iron, of which the high-temperature modification - γ-Fe (above 906°) forms a lattice of a face-centered cube of the Cu type (a0 = 3.63), and the low-temperature modification - the α-Fe lattice of a centered cube of the α-Fe type (a0 = 2.86). Depending on the heating temperature, iron can be found in three modifications, characterized by different crystal lattice structures:

In the temperature range from the lowest to 910°C - a-ferrite (alpha ferrite), which has a crystal lattice structure in the form of a centered cube;
In the temperature range from 910 to 1390°C - austenite, the crystal lattice of which has the structure of a face-centered cube;
In the temperature range from 1390 to 1535°C (melting point) - d-ferrite (delta ferrite). The crystal lattice of d-ferrite is the same as that of a-ferrite. The only difference between them is the different (larger for d-ferrite) distances between the atoms.

Properties and characteristics of metal

Iron is a fairly light, moderately refractory metal, silver-gray in color. Reacts easily with dilute acids and is therefore considered a medium activity element. In dry air, the metal is gradually covered with an oxide film, which prevents further reaction.

But at the slightest humidity, instead of a film, rust appears - loose and heterogeneous in composition. Rust does not prevent further corrosion of iron. However, the physical properties of the metal, and, most importantly, its alloys with carbon, are such that, despite the low corrosion resistance, the use of iron is more than justified.

Next, you will find out what the density of iron is (in kg per m3) in comparison, for example, with copper or aluminum.

Mass and density

The molecular weight of iron is 55.8, which indicates the relative lightness of the substance. What is the density of iron? This indicator is determined by the phase modification:

α-Fe – 7.87 g/cubic. cm at 20 C, and 7.67 g/cc. cm at 600 C;
The γ-phase has an even lower density - 7.59 g/cc at 1000C;
The density of the δ-phase is 7.409 g/cc.

With increasing temperature, the density of iron naturally decreases.

Now let's find out what the melting point of iron is in Celsius, comparing it, for example, with copper or cast iron.

Temperature Range

The metal is moderately refractory, which means a relatively low temperature of change in the state of aggregation:

Metals melt, as a rule, at a very high temperature, which can reach more than 3 thousand degrees. Although some of them can be melted at home, such as lead or tin. But mercury is melted at a temperature of minus 39 degrees. This cannot be achieved at home. Melting point is one of the important indicators of the production of not only the metal itself, but also its alloys. When smelting raw materials, specialists take into account other physical and chemical properties of the ore and metal.

PROPERTIES

Iron ore

Iron and its properties

Iron is a chemical element that is number 26 on the periodic table. It is one of the most abundant elements in the entire solar system. According to research materials, the Earth's core contains approximately 79−85% of this substance . There is also a large amount of it in the earth's crust, but it is inferior to aluminum.

In its pure form, the metal is white with a slightly silvery tint. It is plastic, but the impurities present in it can determine its physical properties. Reacts to a magnet.

Iron is present in water. In river waters its concentration is approximately 2 mg/l of metal. In sea water its content can be a hundred or even a thousand times lower.

Iron oxide is the main form that is mined and found in nature. Iron oxide can be located in the uppermost part of the earth's crust and be a component of sedimentary formations.

An element in twenty-sixth place on the periodic table can have several oxidation states. It is they who determine its geochemical feature of being in a certain environment. In the Earth's core, the metal is present in a neutral form.

What is iron?

From an industrial point of view, iron is the main building material in the world. Its use is everywhere - from door handles to interplanetary rocket engines. The reason for this popularity is simple - the abundance and low cost of raw materials, because iron is in second place in terms of its share in the earth’s crust after aluminum. Symbolic designation of iron "Fe"? and its serial number according to Mendeleev is 26.

Important: do not confuse steel and iron - these are completely different terms. Iron is a pure chemical element, and steel is an alloy of ferum and carbon.

Sometimes iron in the industry is called a highly concentrated alloy with an impurity content of less than 0.7% of the total mass. In this case, the physical properties of the substance are almost not lost. Most iron-based alloys belong to the group of ferrous metals.

In its pure form, iron has good ductility, making it easy to forge but difficult to cast. The structure of the metal is 5 phases, each of which has its own crystal structure and lattice parameters. More details in the table below.

The physical properties of iron directly depend on the purity of the substance. In addition to useful alloying components, which have a positive effect on the properties of the metal, there are also negative elements that can worsen its characteristics. Examples of these could be sulfur and phosphorus, which reduce ductility, in return not providing the alloy with any of the positive properties.

Basic characteristics of iron:

variable density depending on the residence phase of the metal. The general range is from 7.4 to 7.9 grams/cubic centimeter;
The resistance of iron in its pure form is low. The tensile strength of ordinary technical iron is 299 MPa, but if we are talking about high-speed steel, then the tensile strength increases to a value of 2.7 GPa;
pure iron on the Mohs scale is rated at 4 points;
the conductivity of pure ferum is lower than that of aluminum/copper – 9.7*10^(-8);
metal can be forged, but in its pure form cannot be cast;
low toxicity, but not biologically inert.

The absorption of iron by the human body is only ½ of what is received, which makes the metal less dangerous for humans than other elements of the metal group. The main harm to the environment is not caused by iron in its pure form, but by waste during production - gases and slags released. More details about production, thermal characteristics and areas of application will be discussed below.

Mining

There are several ores containing iron. However, the following are mainly used as raw materials for iron production in industry:

magnesite ore;
goethite ore;
hematite ore.

And also the following types of ore are often found:

lellingitis;
siderite;
marcasite;
ilmenite;
is violent.

There is also a mineral called melanterite . It is used primarily in the pharmaceutical industry. It consists of green, fragile crystals with a glassy sheen. Medicines containing ferum are produced from it.

The main deposit of this metal is South America, namely Brazil.

Iron melting and required temperature

The melting point of a metal is the minimum temperature at which it changes from solid to liquid. At the same time, it remains practically unchanged in volume.

Metal can be produced from ore in various ways, but the most basic of them is blast furnace . In addition to blast furnace, iron smelting is also used by roasting crushed ore with an admixture of clay. From the resulting mixture, pellets are formed, which are processed in a furnace followed by reduction with hydrogen. Next, the iron is melted in an electric furnace.

The melting point of iron is very high. For a technically pure element it is +1539 °C. This substance contains an impurity - Sulfur, which can only be extracted in liquid form. Without impurities, pure material is obtained by electrolysis of metal salts.

Classification of metals by melting point

Different metals can turn liquid at different temperatures. As a result, a certain classification is distinguished. They are divided as follows:

Low-fusibility elements are those elements that can become liquid even at temperatures below 600 degrees. These include zinc, tin, lead, etc. They can be melted even at home - you just need to heat them up using a stove or soldering iron. Such types have found application in technology and electronics. They are used to connect metal elements and move electric current. Tin melts at 232 degrees, and zinc at 419 degrees.
Medium-melting - elements that begin to melt at temperatures from six hundred to one thousand six hundred degrees. These elements are used mainly for building elements and metal structures, that is, when creating fittings, slabs and building blocks. This group includes: iron, copper, aluminum. The melting point of aluminum is relatively low and is 660 degrees. But iron begins to turn into a liquid state only at a temperature of 1539 degrees. It is one of the most common metals used in industry, especially in the automotive industry. However, iron is susceptible to corrosion, that is, rust, so it requires special surface treatment. It must be coated with paint or drying oil, and moisture must not be allowed to enter.
Refractory are materials that melt and become liquid at temperatures above 1600 degrees. This group includes tungsten, titanium, platinum, chromium, etc. They are used in the nuclear industry and for some machine parts. They can be used for melting other metals, making high-voltage wires or wire. Platinum can be melted at 1769 degrees, and tungsten at 3420 °C.

The only element that is in a liquid state under normal conditions is mercury. Its melting point is minus 39 degrees and its vapors are poisonous, so it is used only in laboratories and closed containers.

Boiling point is the temperature at which a liquid substance changes to a gaseous state.

Strength of metals

In addition to the ability to transition from a solid to a liquid state, one of the important properties of a material is its strength - the ability of a solid body to resist destruction and irreversible changes in shape. The main indicator of strength is the resistance that occurs when a pre-annealed workpiece breaks. The concept of strength does not apply to mercury because it is in a liquid state. The designation of strength is adopted in MPa - Mega Pascals.

There are the following strength groups of metals:

Fragile. Their resistance does not exceed 50MPa. These include tin, lead, soft-alkaline metals
Durable, 50−500 MPa. Copper, aluminum, iron, titanium. Materials of this group are the basis of many structural alloys.
High strength, over 500 MPa. For example, molybdenum and tungsten.

Metal strength table

Metal	Resistance, MPa
Copper	200−250
Silver	150
Tin	27
Gold	120
Lead	18
Zinc	120−140
Magnesium	120−200
Iron	200−300
Aluminum	120
Titanium	580

Physical characteristics, composition and features of iron metal

Composition and structure of iron

Iron is characterized by polymorphism: there are as many as 4 modifications, differing in structure and lattice parameters:

α-Fe – exists from zero to +769 C. It has a body-centered cubic lattice and is ferromagnetic, that is, it retains magnetization in the absence of an external magnetic field. +769 C – Curie point for metal;
from +769 to +917 C β-Fe appears. It differs from the α phase only in lattice parameters. Almost all physical properties are preserved with the exception of magnetic ones: iron becomes paramagnetic, that is, it loses the ability to magnetize and is drawn into a magnetic field. Metallurgy does not consider the β-phase as a separate modification. Since the transition does not affect significant physical characteristics;
in the range from 917 to 1394 C there is a γ-modification, which is characterized by a face-centered cubic lattice;
at temperatures above +1394 C, the δ phase appears, which is characterized by a body-centered cubic lattice.

The temperature of phase transitions changes noticeably when doped with the same carbon. Actually, the very ability of iron to form so many modifications serves as the basis for processing steel in different temperature conditions. Without such transitions, the metal would not have become so widespread.

Now it’s time for the properties of the metal iron.

This video tells about the structure of iron:

Crystallographic characteristics

Cubic system

Class hexoctahedral

Crystal structure of native iron – Body-centered cubic lattice (for low-temperature modification)

Form of being in nature

The appearance of crystals. Only microscopically small ferrite crystals are known.

Twins in native iron at (111) with a fusion plane (211), often repeated.

Aggregates.

Grains, scales, wire-like sticks, curved ribbons, impregnations in rocks, sometimes large continuous deposits weighing up to several tons (ferrite), often intergrown with cohenite.