Nitrogen - what is this substance? Types and properties of nitrogen. Who discovered nitrogen and when? How the element nitrogen was discovered

Nitrogen (English Nitrogen, French Azote, German Stickstoff) was discovered almost simultaneously by several researchers. Cavendish obtained nitrogen from the air (1772), passing the latter through hot coal, and then through an alkali solution to absorb carbon dioxide. Cavendish did not give a special name to the new gas, referring to it as mephitic air (lat. - mephitis - suffocating or harmful evaporation of the earth). Officially, the discovery of nitrogen is usually attributed to Rutherford, who published in 1772 his dissertation "On fixed air, otherwise called suffocating", where some of the chemical properties of nitrogen were first described. In the same years, Scheele received nitrogen from atmospheric air in the same way as Cavendish. He called the new gas spoiled air (Verdorbene Luft). Priestley (1775) called nitrogen phlogisticated air (Air phlogisticated). Lavoisier in 1776-1777 studied in detail the composition of atmospheric air and found that 4/5 of its volume consists of asphyxiating gas (Air mofette).
Lavoisier proposed to name the element "nitrogen" from the negative Greek prefix "a" and the word for life "zoe", emphasizing its inability to sustain respiration. In 1790, the name "nitrogen" (nitrogene - "forming saltpeter") was proposed for nitrogen, which later became the basis for the international name of the element (Nitrogenium) and the symbol for nitrogen - N.

Being in nature, getting:

Nitrogen occurs in nature mainly in the free state. In air, its volume fraction is 78.09%, and its mass fraction is 75.6%. Nitrogen compounds are found in small amounts in soils. Nitrogen is a constituent of proteins and many natural organic compounds. The total nitrogen content in the earth's crust is 0.01%.
The atmosphere contains about 4 quadrillion (4 10 15) tons of nitrogen, and about 20 trillion (20 10 12) tons in the oceans. An insignificant part of this amount - about 100 billion tons - is annually bound and included in the composition of living organisms. Of these 100 billion tons of bound nitrogen, only 4 billion tons are found in the tissues of plants and animals - the rest accumulates in decomposing microorganisms and eventually returns to the atmosphere.
In technology, nitrogen is obtained from the air. To obtain nitrogen, the air is transferred to a liquid state, and then nitrogen is separated from less volatile oxygen by evaporation (t bale N 2 \u003d -195.8 ° С, t bale O 2 \u003d -183 ° С)
Under laboratory conditions, pure nitrogen can be obtained by decomposing ammonium nitrite or by mixing solutions of ammonium chloride and sodium nitrite when heated:
NH 4 NO 2 N 2 + 2H 2 O; NH 4 Cl + NaNO 2 NaCl + N 2 + 2H 2 O.

Physical properties:

Natural nitrogen consists of two isotopes: 14 N and 15 N. Under normal conditions, nitrogen is a colorless, odorless and tasteless gas, slightly lighter than air, poorly soluble in water (15.4 ml of nitrogen dissolves in 1 liter of water, oxygen - 31 ml ). At -195.8°C, nitrogen turns into a colorless liquid, and at -210.0°C, into a white solid. In the solid state, it exists in the form of two polymorphic modifications: below -237.54 ° C, a stable form with a cubic lattice, above - with a hexagonal one.
The binding energy of atoms in a nitrogen molecule is very high and amounts to 941.6 kJ/mol. The distance between the centers of atoms in a molecule is 0.110 nm. The N 2 molecule is diamagnetic. This indicates that the bond between the nitrogen atoms is triple.
Density of gaseous nitrogen at 0°C 1.25046 g/dm 3

Chemical properties:

Under normal conditions, nitrogen is a chemically inactive substance due to a strong covalent bond. Under normal conditions, it reacts only with lithium, forming a nitride: 6Li + N 2 = 2Li 3 N
With an increase in temperature, the activity of molecular nitrogen increases, while it can be both an oxidizing agent (with hydrogen, metals) and a reducing agent (with oxygen, fluorine). When heated, at elevated pressure and in the presence of a catalyst, nitrogen reacts with hydrogen to form ammonia: N 2 + 3H 2 = 2NH 3
Nitrogen combines with oxygen only in an electric arc to form nitric oxide (II): N 2 + O 2 \u003d 2NO
In an electric discharge, a reaction with fluorine is also possible: N 2 + 3F 2 \u003d 2NF 3

The most important connections:

Nitrogen is able to form chemical compounds, being in all oxidation states from +5 to -3. Nitrogen forms compounds in positive oxidation states with fluorine and oxygen, and in oxidation states greater than +3, nitrogen can only be found in compounds with oxygen.
Ammonia, NH 3 - a colorless gas with a pungent odor, readily soluble in water ("ammonia"). Ammonia has basic properties, interacts with water, hydrogen halides, acids:
NH 3 + H 2 O NH 3 * H 2 O NH 4 + + OH - ; NH 3 + HCl = NH 4 Cl
One of the typical ligands in complex compounds: Cu(OH) 2 + 4NH 3 = (OH) 2 (violet, p-rim)
Reductant: 2NH 3 + 3CuO 3Cu + N 2 + 3H 2 O.
Hydrazine- N 2 H 4 (hydrogen pernitride), ...
Hydroxylamine- NH2OH, ...
Nitric oxide(I), N 2 O (nitrous oxide, laughing gas). ...
Nitric oxide(II), NO is a colorless gas, odorless, slightly soluble in water, non-salt-forming. In the laboratory, they are obtained by reacting copper and dilute nitric acid:
3Cu + 8HNO 3 \u003d 3Cu (NO 3) 2 + 2NO + 4H 2 O.
In industry, it is obtained by catalytic oxidation of ammonia in the production of nitric acid:
4NH 3 + 5O 2 4NO + 6 H 2 O
Easily oxidized to nitric oxide (IV): 2NO + O 2 = 2NO 2
Nitric oxide(III), ??? ...
...
Nitrous acid, ??? ...
...
Nitrites, ??? ...
...
Nitric oxide(IV), NO 2 - a poisonous brown gas, has a characteristic odor, dissolves well in water, while giving two acids, nitrous and nitric: H 2 O + NO 2 \u003d HNO 2 + HNO 3
Upon cooling, it turns into a colorless dimer: 2NO 2 N 2 O 4
Nitric oxide(V), ??? ...
...
Nitric acid, HNO 3 - colorless liquid with a pungent odor, t bp = 83°C. Strong acid, salts - nitrates. One of the strongest oxidizing agents, which is due to the presence of a nitrogen atom in the composition of the acid residue in the highest oxidation state N +5. When nitric acid interacts with metals, it is not hydrogen that is released as the main product, but various reduction products of the nitrate ion:
Cu + 4HNO 3 (conc) = Cu(NO 3) 2 + 2NO 2 + 2H 2 O;
4Mg + 10HNO 3 (intelligent) = 4Mg (NO 3) 2 + NH 4 NO 3 + 5H 2 O.
Nitrates, ??? ...
...

Application:

It is widely used to create an inert environment - filling electric incandescent lamps and free space in mercury thermometers, when pumping liquids, in the food industry as a packaging gas. They nitride the surface of steel products, iron nitrides are formed in the surface layer, which give the steel greater hardness. Liquid nitrogen is often used for deep cooling of various substances.
Nitrogen is important for the life of plants and animals, since it is part of protein substances. Nitrogen is used in large quantities to produce ammonia. Nitrogen compounds are used in the production of mineral fertilizers, explosives and in many industries.

L.V. Cherkashin
KhF Tyumen State University, gr. 542(I)

Sources:
- G.P. Khomchenko. A manual on chemistry for university students. M., New wave, 2002.
- A.S. Egorov, Chemistry. Allowance-tutor for entering universities. Rostov-on-Don, Phoenix, 2003.
- Discovery of the elements and the origin of their names /

J. Priestley, although he received oxygen, he did not understand its role in the processes of metal calcination. As a supporter of the doctrine of phlogiston, he was deeply mistaken, taking for air, from which oxide HgO took away phlogiston (as it should have been according to Stahl's system), turning into metal. But during this process, not all of the “air” is deprived of phlogiston, part of it remains in the compound. This part of the "phlogisticated air" (nitrogen), which firmly holds phlogiston, was also known to J. Priestley. In 1772, he conducted a series of experiments that culminated in the discovery of "phlogisticated air"1. Records were found in the archive of G. Cavendish after his death, from which it is clear that even before 1772 he knew about the existence of nitrogen. Passing ordinary air over hot coal and absorbing the resulting carbon dioxide, G. Cavendish received a “type of air”, which was somewhat lighter than ordinary air and, like carbon dioxide, did not support combustion. He called it "mephitic (which in the old days meant the harmful "evaporations" of the Earth) air." The scientist did not publish this work. But in the same 1772, D. Rutherford's study "On the so-called fixed and mephitic air" (carried out under the direction of J. Black) became known. D. Rutherford isolated and described "spoiled air" () as air saturated with phlogiston.

In 1783, in the article "On a new eudiometer", G. Cavendish answered two questions posed by himself: is atmospheric air constant in its composition? If yes, what is its composition? He made several thousand experiments and studied many air samples from the most diverse regions of England. G. Cavendish answered the first question positively. He then found that air contained 20.83% "combustible air" (oxygen) by volume. The share of “phlogisticated air” (nitrogen) accounted for 79.17%. The experiments of G. Cavendish were distinguished by high accuracy (according to modern data, 02-20.93%, N2-78.10%). The logical continuation of this research was G. Cavendish's article "Experiments on Air", published in 1784.

By the end of 1783, G. Cavendish completed his experiments and found that traces of nitric acid in water formed after the explosion of a mixture of hydrogen and oxygen appear because there was an admixture of nitrogen in oxygen. In 1785, passing electrical discharges through air, he found that pure nitrogen and oxygen give pure nitric acid (nitric oxide NO 2). So for the first time in laboratory conditions under the action of an electric discharge, a chemical interaction of the two main gases of the atmosphere was carried out. It took, however, a long period of development of chemistry, so that at the beginning of the 20th century. to carry out production from air on an industrial scale.

The interaction of nitrogen and oxygen when an electric discharge is passed through a mixture of these gases was first described by J. Priestley in the first volume of his book "Experiments and Observations on Different Types of Air" (1774). He found that the volume of air decreases in this case. A more thorough study of this phenomenon was carried out by G. Cavendish. Passing an electric spark for two weeks through a mixture of atmospheric air with oxygen in the presence (in this case, it is formed, which gives a mixture of potassium nitrate and potassium nitrite with caustic potash), after absorbing excess oxygen, he received an insignificant residue equal to about V120 of the taken air. However, he did not attach much importance to this observation.

Only after 110 years, D. Rayleigh established the difference in the densities of atmospheric nitrogen and nitrogen obtained by chemical means. Research by V. Ramsay and D. Rayleigh led to the discovery of argon and other inert gases in that very 1/120 part of the "phlogisticated air" that remained undecomposed in the experiments of Cavendish.

So, after the work of J. Black, K. Scheele, J. Priestley and G. Cavendish, it turned out that gases are diverse in nature. Their release or absorption during chemical processes served as the basis for explaining many transformations of substances. By the end of the XVIII century. in chemistry, the position was firmly established: without taking into account the mass of the gas, it is impossible to draw up balances of chemical reactions.

The history of chemistry has not yet known such a spectacular research work. For 20 years, it was possible to isolate about two dozen different gases and study their physical and chemical properties, as well as establish the qualitative and quantitative composition of atmospheric air.

Nitrogen is a well-known chemical element, which is denoted by the letter N. This element, perhaps, is the basis of inorganic chemistry, it begins to be studied in detail in the 8th grade. In this article, we will consider this chemical element, as well as its properties and types.

The history of the discovery of a chemical element

Nitrogen is an element that was first introduced by the famous French chemist Antoine Lavoisier. But many scientists are fighting for the title of the discoverer of nitrogen, among them Henry Cavendish, Karl Scheele, Daniel Rutherford.

As a result of the experiment, he was the first to single out a chemical element, but did not understand that he received a simple substance. He reported on his experience, which also did a number of studies. Probably, Priestley also managed to isolate this element, but the scientist could not understand what exactly he received, therefore he did not deserve the title of discoverer. Karl Scheele simultaneously conducted the same research, but did not come to the desired conclusion.

In the same year, Daniel Rutherford managed not only to obtain nitrogen, but also to describe it, publish a dissertation and indicate the basic chemical properties of the element. But even Rutherford did not fully understand what he had received. However, it is he who is considered the discoverer, because he was closest to the solution.

Origin of the name nitrogen

From the Greek "nitrogen" is translated as "lifeless". It was Lavoisier who worked on the rules of nomenclature and decided to name the element that way. In the 18th century, all that was known about this element was that it did not support either breathing. Therefore, this name was adopted.

In Latin, nitrogen is called "nitrogenium", which means "giving birth to saltpeter". From the Latin language, the designation of nitrogen appeared - the letter N. But the name itself did not take root in many countries.

Element abundance

Nitrogen is perhaps one of the most common elements on our planet, it ranks fourth in abundance. The element is also found in the solar atmosphere, on the planets Uranus and Neptune. The atmospheres of Titan, Pluto and Triton are composed of nitrogen. In addition, the Earth's atmosphere consists of 78-79 percent of this chemical element.

Nitrogen plays an important biological role, because it is necessary for the existence of plants and animals. Even the human body contains 2 to 3 percent of this chemical element. It is part of chlorophyll, amino acids, proteins, nucleic acids.

A liquid nitrogen

Liquid nitrogen is a colorless transparent liquid, it is one of the states of aggregation of chemical nitrogen is widely used in industry, construction and medicine. It is used in the freezing of organic materials, cooling equipment, and in medicine for the removal of warts (aesthetic medicine).

Liquid nitrogen is non-toxic and non-explosive.

Molecular nitrogen

Molecular nitrogen is an element that is contained in the atmosphere of our planet and forms a large part of it. The formula of molecular nitrogen is N 2 . Such nitrogen reacts with other chemical elements or substances only at very high temperatures.

Physical properties

Under normal conditions, the chemical element nitrogen is odorless, colorless, and practically insoluble in water. Liquid nitrogen in its consistency resembles water, it is also transparent and colorless. Nitrogen has another state of aggregation, at temperatures below -210 degrees it turns into a solid, forms many large snow-white crystals. Absorbs oxygen from the air.

Chemical properties

Nitrogen belongs to the group of non-metals and adopts properties from other chemical elements from this group. Generally, non-metals are not good conductors of electricity. Nitrogen forms various oxides, such as NO (monoxide). NO or nitric oxide is a muscle relaxant (a substance that significantly relaxes the muscles and does not have any harm or other effects on the human body). Oxides containing more nitrogen atoms, such as N 2 O, are laughing gas, slightly sweet in taste, which is used in medicine as an anesthetic. However, NO 2 oxide has nothing to do with the first two, because it is a rather harmful exhaust gas that is contained in car exhausts and seriously pollutes the atmosphere.

Nitric acid, which is formed by hydrogen, nitrogen and three oxygen atoms, is a strong acid. It is widely used in the production of fertilizers, jewelry, organic synthesis, the military industry (the production of explosives and the synthesis of poisonous substances), the production of dyes, medicines, etc. Nitric acid is very harmful to the human body, leaving ulcers and chemical burns on the skin.

People mistakenly believe that carbon dioxide is nitrogen. In fact, due to its chemical properties, an element reacts with only a small number of elements under normal conditions. And carbon dioxide is carbon monoxide.

Application of a chemical element

Liquid nitrogen is used in medicine for cold treatment (cryotherapy), as well as in cooking as a refrigerant.

This element has also found wide application in industry. Nitrogen is a gas that is explosion and fire safe. In addition, it prevents rotting and oxidation. Now nitrogen is used in mines to create an explosion-proof environment. Gaseous nitrogen is used in petrochemistry.

In the chemical industry, it is very difficult to do without nitrogen. It is used for the synthesis of various substances and compounds, such as some fertilizers, ammonia, explosives, dyes. Now a large amount of nitrogen is used for the synthesis of ammonia.

In the food industry, this substance is registered as a food additive.

Mixture or pure substance?

Even the scientists of the first half of the 18th century, who managed to isolate the chemical element, thought that nitrogen was a mixture. But there is a big difference between these concepts.

It has a whole complex of constant properties, such as composition, physical and chemical properties. A mixture is a compound that contains two or more chemical elements.

Now we know that nitrogen is a pure substance, since it is a chemical element.

When studying chemistry, it is very important to understand that nitrogen is the basis of all chemistry. It forms various compounds that we all encounter, including laughing gas, brown gas, ammonia, and nitric acid. No wonder chemistry at school begins with the study of such a chemical element as nitrogen.

Publication date: 23.12.2018 15:32

The history of the discovery of nitrogen.

In 1772, D. Rutherford found that the air left under the cap where the mouse lived, after burning phosphorus in it, does not support combustion and respiration. He called this gas "poisonous air". In the same year, D. Priestley, having received "poisonous air" in a different way, called it "phlogistic air". In 1773, K. Scheele, a Swedish pharmacist from the city of Stralsund, established that air consists of two gases, and called the gas, which does not support combustion and breathing, "bad or spoiled air." In 1776, the famous French scientist A. Lavoisier, studying in detail "poisonous", "phlogisticated" and "bad" air, established an identity between them. And years later, as a member of the commission for the development of a new chemical nomenclature, he proposed calling this part of the air nitrogen (from the Greek words "a" - meaning negation, and "zoos" - life). The Latin name for nitrogen comes from the word "nitrogenium", which means "giving birth to saltpeter" ("saltpeter former"). This term was introduced into science in 1790 by J. Chaptal.

Finding in nature.

In the lithosphere, the average nitrogen content is 6*10 -3 wt. %. The main mass of nitrogen in silicates is in the chemically bound state in the form of NH 4 + , which isomorphically substituting the potassium ion in the silicate lattice. In addition, nitrogen minerals are also found in nature: ammonia (NH 4 C1), released from volcanoes in fairly large quantities, baddingtonite (NH 4 AlSi 3 O 8- * 0.5 H 2 O) is the only ammonium aluminosilicate found with zeolite water. In the most near-surface regions of the lithosphere, a number of minerals have been found, consisting mainly of nitrate salts. Among them is the well-known saltpeter (NaNO 3), large accumulations of which are characteristic of a dry desert climate (Chile, Central Asia). For a long time saltpeter was the main source of bound nitrogen. (Now the industrial synthesis of ammonia from atmospheric nitrogen and hydrogen is of primary importance.) Compared with silicate minerals, fossil organic matter is significantly enriched in nitrogen. Oil contains from 0.01 to 2% nitrogen, and coal - from 0.2 to 3%. As a rule, diamonds have a high nitrogen content (up to 0.2%).

In the hydrosphere, the average nitrogen content is 1.6-*10 -3 wt. %. The main part of this nitrogen is molecular nitrogen dissolved in water; chemically bound nitrogen, which is about 25 times less, is represented by nitrate and organic forms. In smaller quantities, the water contains ammonia and nitrite nitrogen. The concentration of bound nitrogen in the ocean is about 104 times less than in soils suitable for agricultural production.

Although the name nitrogen means "non-life-sustaining", it is actually an essential element for life. In plant organisms, it contains an average of 3%, in living organisms up to 10% of dry weight. Nitrogen accumulates in soils (on average 0.2 wt.%). In the protein of animals and humans, the average nitrogen content is 16%.

Between the atmosphere, the lithosphere and the biosphere there is a continuous exchange, with which the change of chemical forms of nitrogen is also associated. This exchange determines the nitrogen cycle in nature. The exchange of nitrogen between the atmosphere and the biosphere is called the biochemical nitrogen cycle. The main process of nitrogen movement in the biosphere is its transition from one chemical form to another in a closed cycle. The constant change of chemical forms of nitrogen is the source of life for many organisms ranging from microorganisms to highly organized forms of life. The reserves of bound nitrogen accumulated in the soil serve as a source of nutrition for higher plants, from where bound nitrogen can also enter animal organisms. Plants and animals, dying, give rise to organic nitrogen, located mainly in amino acids. In the process of ammonification of organic residues, the nitrogen of organic compounds passes into the ammonium (ammonia) form. The latter, with the help of microorganisms, passes into the nitrite form. In this case, about 70 kcal/mol is released. Another group of microorganisms completes the oxidation of ammonia to nitrate. The nitrate obtained in the process of nitrification is absorbed by plants, and the cycle of nitrogen movement in the biosphere is closed.

The main inorganic nitrogen compounds in soils are nitrate, ammonium, and nitrite, which is rare in natural conditions. The behavior of the first two components in the soil is completely different. If nitrate is a highly mobile compound, is not sorbed by soil minerals and remains in a state dissolved in water, then ammonium is easily chemisorbed by clay minerals, although this does not prevent it from being easily oxidized to nitrate under certain conditions. Such a difference in the mobility of nitrate and ammonium predetermines the sources of nitrogen nutrition for plants. From the energy standpoint, the ammonium form of nitrogen is more preferable, since the nitrogen valence in it is the same as the nitrogen valency in amino acids.

The nitrate form serves as the main source of nitrogen nutrition for vegetation due to its mobility, despite the need to spend additional energy associated with the reduction of nitrate by the plant.

Under the action of microorganisms, the reserves of chemically bound nitrogen not used by living matter are continuously converted into forms available for nitrogen nutrition of plants. Thus, ammonium fixed by clay minerals is oxidized to nitrates. Under certain conditions, in the absence of free oxygen and the presence of nitrate unused by living matter, the reduction of nitrogen to molecular nitrogen due to the process of denitrification can occur, with the latter leaving for the atmosphere.

The amounts of nitrogen removed from the biosphere by denitrifying bacteria are compensated by the processes of nitrogen fixation from the atmosphere by nitrogen-fixing bacteria. The latter are divided into two groups: living independently and living in symbiosis with higher plants or with insects. The first group of bacteria fixes approximately 10 kg/ha. Symbionts of higher plants fix much larger amounts of nitrogen. Thus, symbionts of legumes fix up to 350 kg/ha. With precipitation, nitrogen falls on the order of several kilograms per hectare.

In the balance of fixed nitrogen, artificially synthesized ammonia is becoming increasingly important, with its amount doubling every 6 years. In the near future, this may cause an imbalance between the processes of fixation and denitrification in the biosphere.

The sub-cycle of ammonia and nitrogen oxides circulation through the atmosphere should be noted, especially considering that this sub-cycle regulates the extent of the development of the biosphere. The sources of atmospheric ammonia are biochemical processes in the soil and, first of all, ammonification. Oxidized, ammonia gives the bulk of nitrogen oxides in the atmosphere. The nitrous oxide produced in the process of denitrification is responsible for the content of nitrogen oxides in the stratosphere, which catalytically destroy ozone, which protects the living matter of the biosphere from the harmful effects of hard ultraviolet radiation. Thus, in nature, certain limits were established for the development of the biosphere.

Human activity threatens to upset the established balance. Thus, the calculation showed that the amount of nitric oxide released during the planned flights of supersonic aircraft in the stratosphere will be comparable with its intake from natural sources. Thus, the cycle of movement of molecular nitrogen through the biosphere is completed. In this geochemical cycle, the very existence of the Earth's nitrogen atmosphere is determined by the rates of fixation and denitrification processes. With a sharp imbalance of these speeds, the nitrogen atmosphere of the Earth can disappear in just a few tens of millions of years.

In addition to the atmosphere, the biosphere determines the existence of another large reservoir of nitrogen nitrogen in the earth's crust. The lifetime of nitrogen in this cycle is about 1 billion years.

Isotopes of nitrogen.

Nitrogen is the only element on Earth whose most abundant nuclei are the odd-odd 14N isotope (7 protons, 7 neutrons). The content of 14 N and 15 N in the air is 99.634 and 0.366%, respectively.

In the upper layers of the atmosphere, under the action of neutrons from cosmic radiation, 14 N is converted into the radioactive isotope 14 C, on which the geochronological dating of geological samples containing "ancient" carbon is based.

At present, it is possible to obtain chemical compounds of nitrogen artificially enriched in the heavy isotope 15 N up to 99.9 atom.%. Samples enriched in 15 N are used in research in biochemistry, biology, medicine, chemistry and physical chemistry, physics, agriculture, technology and chemical engineering, analytical chemistry, etc.

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