Nitrogen - also known as N in the periodic table (also known as the first letter in the abbreviationNPK on numerous fertilizer packages).
Before examining in detail the role and forms of nitrogen in fertilizers, we need to recall that it belongs to the group MACROelements . This is a category of elements vital for absolutely all plants, which, in addition to nitrogen, includes phosphorus P and potassium K. MICROElements (iron, sulfur, zinc, manganese and others) also play an important role, but they are needed in dosages hundreds of times less than macroelements (hence and the name "micro"). Nitrogen, like phosphorus and potassium, is directly involved in the formation of basic plant tissues and is responsible for developmental phases (growth, vegetation, flowering, fruiting) and growth rate.
Why does a plant need nitrogen?
If an artist wanted to draw a picture of a fragrant garden from the elements of the periodic table, then instead of green foliage, stems and young shoots there would be the letter N - nitrogen. It is this volatile gas that participates through various compounds in the formation of chlorophyll - the same protein that takes part in photosynthesis and plant respiration. If there is enough nitrogen, the foliage has a rich emerald color, which, coupled with good watering, can become glossy. As soon as nitrogen becomes scarce, the plant turns pale to a stunted yellow color, and new shoots grow slowly or practically stop growing. 
ON THE PICTURE: The difference between plants that received nitrogen during cultivation and those that grew on poor soils is obvious
It is also generally accepted that phosphorus is responsible for fruiting, and it is its presence that will affect the yield. This is true, but mostly in terms of the quality of the crop. Nitrogen will be responsible for the quantity. The more vegetative mass the plant gains, the more flower buds will appear on the stems or in the axils. In some plants, nitrogen directly affects the formation of flower buds, especially in dioecious plants with female and male flowers (hemp, willow, lemongrass, sea buckthorn and many others).
How to understand that a plant lacks nitrogen?
The first sign of nitrogen deficiency is stunted, yellowish, even pale yellow, foliage color. Yellowing begins from the edges of the leaf towards the center. At the same time, the leaf blade becomes thinner and becomes soft, even if watering is observed. Very similar symptoms are observed with a lack of sulfur (S), but in the case of nitrogen, the lower leaves turn yellow first. In advanced cases, they dry out and fall off - the plant “pulls” all the nutrients from them to give to the upper shoots or fruits, if any. With a lack of sulfur, leaf fall from below is not observed.
There can usually be two reasons for the shortage: either they forgot to feed the plant (when and how to feed it - below) or the soil is highly acidified, and the acidic reaction of the environment disrupts the absorption of nitrogen. Also, in an acidic environment, a lack of nitrogen can mimic chlorosis - a lack of iron or magnesium. However, in this case this is not important - the soil requires drastic replacement or renewal.
What kind of nitrogen is sold in stores and which one is better?
For every gardener, this question is perhaps the most important. However, let’s first figure out what kind of nitrogen actually exists? Without this, it will be difficult to understand what is written on the package.
Ammonia or ammonium nitrogen (NH 4)
This nitrogen is also called organic nitrogen. There really is a lot of it in the organic remains of decaying matter, like manure or fallen leaves. Plants love ammonium very much, since it easily penetrates into the roots and can be converted into amino acids, which will form the leaves and shoots of the plant. However, there is a significant drawback: despite all the resistance mechanisms, ammonium can penetrate the plant cell and have a toxic effect on it.
In nature, an overdose of ammonium is quite rare, because it is quite quickly “converted” by bacteria to nitrates NO 3 (nitrification process) and further to nitrites (NO 2) and up to pure nitrogen, which quickly evaporates from the soil. In a garden or vegetable garden, ammonia nitrogen also quickly leaves the soil, unless the owner of the site applies clean, fresh manure in large quantities. In this case, the so-called “burning” the roots or the entire plant. In indoor conditions, organic nitrogen should be used to a minimum, because It is quite difficult to control the required dosage.
IMPORTANT : on fertilizer packages for indoor plants ammonia nitrogen is extremely rarely indicated by the formula (NH 4) or formulation. As a rule, an organic form is used: some kind of extract (for example, algae extract) or a liquid form of pure organic fertilizer (“vermicompost”), or a gel-like mass (“sapropel” - bottom sludge), etc.
For the garden the mineral form is used - ammonium sulfate (NH 4) 2 SO 4. The big advantage of this fertilizer is that it also contains sulfur. Together with nitrogen, it participates in the synthesis of important amino acids, including essential ones. Ammonium sulfate is part of the popular today brand of fertilizer “Aquarin” (numbers 6 and 7 are suitable for gardening). This fertilizer contains approximately 25% ammonium and 75% nitrate nitrogen.
Nitrate nitrogen (NO3)
If the plant tries to immediately put organic nitrogen into use without wasting energy, then nitrate the picture is completely opposite. Almost any crop greedily stores nitrates in tissues in quantities sometimes exceeding permissible limits! And the reason for this is the high mobility of nitrogen in the biosphere. Today, a cow plops down a cake, and bacteria (and a little later, insects) immediately attack it, converting nitrogen from organic to mineral form NO 3 . But this form does not stay long: what the plants did not have time to take away is already converted by other bacteria to the nitrite NO 2 form, and then to nitrogen. Plus nitrate - harmless to the plant. Minus - the need for light and heat, thanks to which nitrate in the leaves is reduced to ammonium (more precisely, various amines NH 2) and then to amino acids and proteins. As a result: in unfavorable conditions, the plant will tend to accumulate nitrates in order to use them when the situation improves.
In room conditions nitrate nitrogen is the real solution. It is indicated by the formula on the packaging NO 3 and is accompanied by the corresponding text. Dosages are calculated in advance for periods of rest and active growth. It's impossible to make a mistake.
In the garden
nitrate nitrogen is used straightaway
after the start of sap flow (which corresponds to a soil temperature of about +15°C). It is important not to miss this moment and provide the plant with an element from which new shoots and leaves will begin to be built in the very next few days. They stop using nitrogen fertilizers in July, or rather, immediately after the end of the growing season (trees and shrubs slow down, fruiting begins). In winter, the garden is sent without nitrogen fertilizing or done in late autumn, before frosts, and the organic form, which will stay in the soil longer. Also, do not forget that winters have recently become warmer, which does not have the best effect on the retention of nitrogen in the soil.
In everyday life, nitrate nitrogen is known as saltpeter , of which the most popular in Russia is potassium (or “potassium”) nitrate. This form of nitrate nitrogen is suitable for both garden and indoor plants. Provides easily digestible nitrogen and potassium.
Amide nitrogen CO(NH 2) 2, urea or simply urea
A rich, biogenic (that is, also obtained organically) fertilizer that can contain up to 46% nitrogen. For use in the ground, it has recently been rarely used, because ubiquitous “urease” bacteria quickly convert precious urea into ammonium carbonate, better known in the food industry as a leavening agent. In Soviet times, fields were “fertilized” with this “baking powder” until nitrogen losses were realized. Today, urea is used in spray solutions. Of course, its best use is in fields and large gardens. It is rarely used in private practice, therefore it is practically not found on the shelves of ordinary stores.
Urea is an excellent remedy against scab and some other pathogenic fungi.
Summarize
- Nitrogen is one of the most important elements that a plant constantly needs for healthy growth and development.
- In indoor culture, nitrogen fertilizers are added during the period of active growth. A month and a half before dormancy, nitrogen nutrition is stopped so as not to cause excessive growth and disruption of the dormant period.
- In gardening and vegetable crops, nitrogen is added in the spring, as soon as the temperature warms up to +15°C (the roots begin to absorb moisture). End of application period: mid-summer; early August - only in case of cold spring/summer.
- In room culture, it is necessary to use nitrate nitrogen: NO 3 will be written on the package, perhaps only the word “nitrate” will appear.
- In horticultural culture, as a rule, ready-made brands of fertilizers are used, in which nitrate and ammonium forms of nitrogen are mixed. Both are indicated on the packaging with the formulas ammonium sulfate and potassium nitrate (most often).
- If you come across urea (carbamide), use it to spray plants. The period of use is similar to other forms of nitrogen.
Nitrogen is a chemical element with atomic number 7. It is an odorless, tasteless and colorless gas.
Thus, a person does not feel the presence of nitrogen in the earth’s atmosphere, while it consists of 78 percent of this substance. Nitrogen is one of the most common substances on our planet. You can often hear that without nitrogen there would be no food, and this is true. After all, the protein compounds that make up all living things necessarily contain nitrogen.
Nitrogen in nature
Nitrogen is found in the atmosphere in the form of molecules consisting of two atoms. In addition to the atmosphere, nitrogen is found in the Earth's mantle and in the humus layer of the soil. The main source of nitrogen for industrial production is minerals.
However, in recent decades, when mineral reserves began to deplete, an urgent need arose to separate nitrogen from the air on an industrial scale. This problem has now been solved, and huge volumes of nitrogen for industrial needs are extracted from the atmosphere.
The role of nitrogen in biology, the nitrogen cycle
On Earth, nitrogen undergoes a number of transformations in which both biotic (life-related) and abiotic factors are involved. Nitrogen enters plants from the atmosphere and soil, not directly, but through microorganisms. Nitrogen-fixing bacteria retain and process nitrogen, converting it into a form that can be easily absorbed by plants. In the plant body, nitrogen is converted into complex compounds, in particular proteins.
Through the food chain, these substances enter the bodies of herbivores and then predators. After the death of all living things, nitrogen returns to the soil, where it undergoes decomposition (ammonification and denitrification). Nitrogen is fixed in the soil, minerals, water, enters the atmosphere, and the circle repeats.
Application of nitrogen
After the discovery of nitrogen (this happened in the 18th century), the properties of the substance itself, its compounds, and the possibility of using it on the farm were well studied. Since the reserves of nitrogen on our planet are huge, this element has become extremely actively used. 
Pure nitrogen is used in liquid or gaseous form. Liquid nitrogen has a temperature of minus 196 degrees Celsius and is used in the following areas:
— in medicine. Liquid nitrogen is a refrigerant in cryotherapy procedures, that is, cold treatment. Flash freezing is used to remove various tumors. Tissue samples and living cells (in particular, sperm and eggs) are stored in liquid nitrogen. Low temperature allows the biomaterial to be preserved for a long time, and then thawed and used.
The possibility of storing entire living organisms in liquid nitrogen, and, if necessary, defrosting them without any harm, was expressed by science fiction writers. However, in reality it has not yet been possible to master this technology;
— in the food industry Liquid nitrogen is used when bottling liquids to create an inert environment in the container.
In general, nitrogen is used in areas where a gaseous environment without oxygen is required, e.g.
— in fire fighting. Nitrogen displaces oxygen, without which combustion processes are not supported and the fire goes out.
Nitrogen gas has found application in the following industries:
— food production. Nitrogen is used as an inert gas medium to maintain the freshness of packaged products;
— in the oil industry and mining. Pipelines and tanks are purged with nitrogen, it is injected into mines to form an explosion-proof gas environment;
— in aircraft manufacturing The chassis tires are inflated with nitrogen.
All of the above applies to the use of pure nitrogen, but do not forget that this element is the starting material for the production of a mass of various compounds:
- ammonia. An extremely sought-after substance containing nitrogen. Ammonia is used in the production of fertilizers, polymers, soda, and nitric acid. It is itself used in medicine, in the manufacture of refrigeration equipment;
— nitrogen fertilizers;
- explosives;
- dyes, etc. 
Nitrogen is not only one of the most common chemical elements, but also a very necessary component used in many branches of human activity.
NITROGEN, N (lat. Nitrogenium * a. nitrogen; n. Stickstoff; f. azote, nitrogene; i. nitrogeno), is a chemical element of group V of the Mendeleev periodic system, atomic number 7, atomic mass 14.0067. Discovered in 1772 by the English explorer D. Rutherford.
Properties of nitrogen
Under normal conditions, nitrogen is a colorless and odorless gas. Natural nitrogen consists of two stable isotopes: 14 N (99.635%) and 15 N (0.365%). The nitrogen molecule is diatomic; the atoms are connected by a covalent triple bond NN. The diameter of the nitrogen molecule, determined by various methods, is 3.15-3.53 A. The nitrogen molecule is very stable - the dissociation energy is 942.9 kJ/mol.
Molecular nitrogen
Molecular nitrogen constants: f melting - 209.86°C, f boiling - 195.8°C; The density of gaseous nitrogen is 1.25 kg/m3, liquid nitrogen - 808 kg/m3.
Characteristics of nitrogen
In the solid state, nitrogen exists in two modifications: cubic a-form with a density of 1026.5 kg/m3 and hexagonal b-form with a density of 879.2 kg/m3. Heat of fusion 25.5 kJ/kg, heat of evaporation 200 kJ/kg. Surface tension of liquid nitrogen in contact with air 8.5.10 -3 N/m; dielectric constant 1.000538. Solubility of nitrogen in water (cm 3 per 100 ml of H 2 O): 2.33 (0°C), 1.42 (25°C) and 1.32 (60°C). The outer electron shell of the nitrogen atom consists of 5 electrons. The oxidation states of nitrogen vary from 5 (in N 2 O 5) to -3 (in NH 3).
Nitrogen compound
Under normal conditions, nitrogen can react with transition metal compounds (Ti, V, Mo, etc.), forming complexes or being reduced to form ammonia and hydrazine. Nitrogen interacts with active metals such as when heated to relatively low temperatures. Nitrogen reacts with most other elements at high temperatures and in the presence of catalysts. Nitrogen compounds with: N 2 O, NO, N 2 O 5 have been well studied. Nitrogen combines with C only at high temperatures and in the presence of catalysts; this produces ammonia NH 3 . Nitrogen does not directly interact with halogens; therefore, all nitrogen halides are obtained only indirectly, for example, nitrogen fluoride NF 3 - by interaction with ammonia. Nitrogen does not combine directly with sulfur either. When hot water reacts with nitrogen, cyanogen (CN) 2 is formed. When ordinary nitrogen is exposed to electric discharges, as well as during electric discharges in the air, active nitrogen can be formed, which is a mixture of nitrogen molecules and atoms with an increased energy reserve. Active nitrogen interacts very energetically with oxygen, hydrogen, vapor, and some metals.
Nitrogen is one of the most common elements on Earth, and the bulk of it (about 4.10 15 tons) is concentrated in a free state in. Every year, volcanic activity releases 2.10 6 tons of nitrogen into the atmosphere. A small part of nitrogen is concentrated in (average content in the lithosphere 1.9.10 -3%). Natural nitrogen compounds are ammonium chloride and various nitrates (saltpeter). Nitrogen nitrides can only form at high temperatures and pressures, which appears to have been the case in the earliest stages of Earth's development. Large accumulations of saltpeter are found only in dry desert climates (, etc.). Small amounts of fixed nitrogen are found in (1-2.5%) and (0.02-1.5%), as well as in the waters of rivers, seas and oceans. Nitrogen accumulates in soils (0.1%) and living organisms (0.3%). Nitrogen is part of protein molecules and many natural organic compounds.
Nitrogen cycle in nature
In nature, there is a nitrogen cycle, which includes a cycle of molecular atmospheric nitrogen in the biosphere, a cycle in the atmosphere of chemically bound nitrogen, a cycle of surface nitrogen buried with organic matter in the lithosphere with its return back to the atmosphere. Nitrogen for industry was previously extracted entirely from natural saltpeter deposits, the number of which is very limited in the world. Particularly large deposits of nitrogen in the form of sodium nitrate are found in Chile; saltpeter production in some years amounted to more than 3 million tons.
Nitrogen is a gas that is slightly soluble in water and has no color, smell or taste. In its free form, nitrogen can be used in various industries. Let's take a closer look at those industries that use nitrogen.
Metallurgy
- During annealing, sintering with powder metal.
- With neutral hardening, hard soldering.
- During cyanidation (nitrogen is necessary to protect ferrous and non-ferrous metals).
- Nitrogen also plays an important role in the operation of the blast furnace charging device and the fire metal stripping machine.
- At coke production.
Chemistry, gas, oil
- Nitrogen gas is used during well development. It is used to reduce the water level in wells. This method is very promising; it is characterized by reliability, as well as ease of control and regulation of the process over a wide range of pressures and flow rates. With the help of gaseous nitrogen, deep wells are quickly emptied, a quick and sharp, or a slow and gradual decrease in pressure in the well. Nitrogen provides drainage of the formation and replenishment of compressed gas, which is necessary for the flow of liquid.
- Nitrogen is used to create an inert environment in various containers during unloading and loading operations. Nitrogen is also used when extinguishing fires, during testing and purging of pipelines.
- Nitrogen in its pure form is used for the synthesis of ammonia, in the production of nitrogen-type fertilizers, as well as in the processing of associated gases and methane conversion.
- Nitrogen is used to reduce deposits in petroleum refineries, to process high octane components and to increase the productivity of petroleum crackers.
Firefighting
- Nitrogen has inert properties, due to which it is possible to displace oxygen and prevent oxidation reactions. Combustion is, in essence, rapid oxidation, due to the presence of oxygen in the atmosphere and a combustion source, which can be a spark, an electric arc, or simply a chemical reaction with a large amount of heat generated. By using nitrogen, this situation can be avoided. If the nitrogen concentration in the environment is 90%, then fire will not occur.
- Both stationary nitrogen plants and mobile nitrogen production stations can effectively prevent fire. With their help, a fire can also be successfully extinguished.
Medicine
- In research in laboratories, for hospital analyses.
Mining industry
- In coal mines, nitrogen is also needed for firefighting.
Pharmaceuticals
- Nitrogen is used to package, transport and displace oxygen from a variety of product tanks.
Food industry
- Nitrogen is necessary for handling, storage, packaging of food products (especially cheeses and fatty products, which are very quickly oxidized by oxygen), to increase their shelf life, as well as to preserve the taste of these products.
- A mixture of nitrogen and carbon dioxide helps stop bacteria from multiplying.
- Nitrogen, creating an inert environment, helps protect food from harmful insects.
- Nitrogen acts as a diluent to create a gas mixture.
Pulp and paper industry
- Nitrogen is used in cathode beam processes on paper, cardboard, and even some wood items to polymerize varnish coatings. This method allows to reduce the cost of photoinitiators, as well as reduce the emission of volatile compounds and improve the quality of processing.
Nitrogen
NITROGEN-A; m.[French azote from Greek. an- - not-, without- and zōtikos - giving life]. Chemical element (N), a colorless and odorless gas that does not support respiration or combustion (it makes up the bulk of the air by volume and mass, and is one of the main elements of plant nutrition).
◁ Nitrogen, oh, oh. A-th acid. A fertilizers. Nitrogenous, oh, oh. A-th acid.
nitrogen(lat. Nitrogenium), chemical element of group V of the periodic table. Name from Greek. a... is a negative prefix, and zōē is life (does not support breathing and combustion). Free nitrogen consists of 2-atomic molecules (N 2); colorless and odorless gas; density 1.25 g/l, t pl –210ºC, t kip –195.8ºC. Chemically very inert, but reacts with complex compounds of transition metals. The main component of air (78.09% of the volume), the separation of which produces industrial nitrogen (more than 3/4 goes to the synthesis of ammonia). Used as an inert medium for many technological processes; liquid nitrogen is a refrigerant. Nitrogen is one of the main biogenic elements that is part of proteins and nucleic acids.
NITROGENNITROGEN (lat. Nitrogenium - giving rise to nitrate), N (read “en”), a chemical element of the second period of the VA group of the periodic table, atomic number 7, atomic mass 14.0067. In its free form, it is a colorless, odorless, and tasteless gas; it is poorly soluble in water. Consists of diatomic N 2 molecules with high strength. Refers to non-metals.
Natural nitrogen consists of stable nuclides (cm. NUCLIDE) 14 N (content in the mixture 99.635% by weight) and 15 N. Configuration of the outer electronic layer 2 s 2
2p 3
. The radius of the neutral nitrogen atom is 0.074 nm, the radius of the ions: N 3- - 0.132, N 3+ - 0.030 and N 5+ - 0.027 nm. The sequential ionization energies of the neutral nitrogen atom are, respectively, 14.53, 29.60, 47.45, 77.47 and 97.89 eV. According to the Pauling scale, the electronegativity of nitrogen is 3.05.
History of discovery
Discovered in 1772 by the Scottish scientist D. Rutherford in the composition of the combustion products of coal, sulfur and phosphorus as a gas unsuitable for breathing and combustion (“suffocating air”) and, unlike CO 2, not absorbed by an alkali solution. Soon the French chemist A.L. Lavoisier (cm. LAVOISIER Antoine Laurent) came to the conclusion that the “suffocating” gas is part of the atmospheric air, and proposed the name “azote” for it (from the Greek azoos - lifeless). In 1784, the English physicist and chemist G. Cavendish (cm. CAVENDISH Henry) established the presence of nitrogen in nitrate (hence the Latin name for nitrogen, proposed in 1790 by the French chemist J. Chantal).
Being in nature
In nature, free (molecular) nitrogen is part of the atmospheric air (in air 78.09% by volume and 75.6% by mass of nitrogen), and in bound form - in the composition of two nitrates: sodium NaNO 3 (found in Chile, hence name Chilean saltpeter (cm. CHILEAN SALTPETER)) and potassium KNO 3 (found in India, hence the name Indian saltpeter) - and a number of other compounds. Nitrogen ranks 17th in abundance in the earth's crust, accounting for 0.0019% of the earth's crust by mass. Despite its name, nitrogen is present in all living organisms (1-3% by dry weight), being the most important biogenic element (cm. BIOGENIC ELEMENTS). It is part of the molecules of proteins, nucleic acids, coenzymes, hemoglobin, chlorophyll and many other biologically active substances. Some so-called nitrogen-fixing microorganisms are able to assimilate molecular nitrogen from the air, converting it into compounds available for use by other organisms (see Nitrogen fixation (cm. NITROGEN FIXATION)). The transformation of nitrogen compounds in living cells is the most important part of metabolism in all organisms.
Receipt
In industry, nitrogen is obtained from the air. To do this, the air is first cooled, liquefied, and the liquid air is subjected to distillation. Nitrogen has a slightly lower boiling point (-195.8°C) than the other component of air, oxygen (-182.9°C), so when liquid air is gently heated, nitrogen evaporates first. Nitrogen gas is supplied to consumers in compressed form (150 atm. or 15 MPa) in black cylinders with a yellow “nitrogen” inscription. Store liquid nitrogen in Dewar flasks (cm. DEWARD VESSEL).
In the laboratory, pure (“chemical”) nitrogen is obtained by adding a saturated solution of ammonium chloride NH 4 Cl to solid sodium nitrite NaNO 2 when heated:
NaNO 2 + NH 4 Cl = NaCl + N 2 + 2H 2 O.
You can also heat solid ammonium nitrite:
NH 4 NO 2 = N 2 + 2H 2 O.
Physical and chemical properties
The density of gaseous nitrogen at 0 °C is 1.25046 g/dm 3, liquid nitrogen (at boiling point) is 0.808 kg/dm 3. Nitrogen gas at normal pressure at a temperature of –195.8 °C turns into a colorless liquid, and at a temperature of –210.0 °C into a white solid. In the solid state, it exists in the form of two polymorphic modifications: below –237.54 °C the form with a cubic lattice is stable, above – with a hexagonal lattice.
The critical temperature of nitrogen is –146.95 °C, the critical pressure is 3.9 MPa, the triple point lies at a temperature of –210.0 °C and a pressure of 125.03 hPa, from which it follows that nitrogen at room temperature is not at any, even very high pressure, cannot be turned into liquid.
The heat of evaporation of liquid nitrogen is 199.3 kJ/kg (at boiling point), the heat of fusion of nitrogen is 25.5 kJ/kg (at temperature –210 °C).
The binding energy of atoms in the N 2 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. This indicates that the bond between the nitrogen atoms is triple. The high strength of the N 2 molecule can be explained within the framework of the molecular orbital method. The energy scheme for filling the molecular orbitals in the N 2 molecule shows that only the bonding s- and p-orbitals in it are filled with electrons. The nitrogen molecule is non-magnetic (diamagnetic).
Due to the high strength of the N 2 molecule, the decomposition processes of various nitrogen compounds (including the notorious explosive RDX (cm. RDX)) when heated, impacted, etc. lead to the formation of N 2 molecules. Since the volume of the resulting gas is much greater than the volume of the original explosive, an explosion occurs.
Chemically, nitrogen is quite inert and at room temperature reacts only with the metal lithium (cm. LITHIUM) with the formation of solid lithium nitride Li 3 N. In compounds it exhibits various oxidation states (from –3 to +5). Forms ammonia with hydrogen (cm. AMMONIA) NH3. Hydrazine is obtained indirectly (not from simple substances) (cm. HYDRAZINE) N 2 H 4 and hydronitric acid HN 3. Salts of this acid are azides (cm. AZIDS). Lead azide Pb(N 3) 2 decomposes on impact, so it is used as a detonator, for example, in cartridge capsules.
Several nitrogen oxides are known (cm. NITROGEN OXIDES). Nitrogen does not react directly with halogens; NF 3 , NCl 3 , NBr 3 and NI 3 , as well as several oxyhalides (compounds that, in addition to nitrogen, contain both halogen and oxygen atoms, for example, NOF 3 ) are obtained indirectly.
Nitrogen halides are unstable and easily decompose when heated (some during storage) into simple substances. Thus, NI 3 precipitates when aqueous solutions of ammonia and iodine tincture are combined. Even with a slight shock, dry NI 3 explodes:
2NI 3 = N 2 + 3I 2.
Nitrogen does not react with sulfur, carbon, phosphorus, silicon and some other non-metals.
When heated, nitrogen reacts with magnesium and alkaline earth metals, resulting in salt-like nitrides of the general formula M 3 N 2, which decompose with water to form the corresponding hydroxides and ammonia, for example:
Ca 3 N 2 + 6H 2 O = 3Ca(OH) 2 + 2NH 3.
Alkali metal nitrides behave similarly. The interaction of nitrogen with transition metals leads to the formation of solid metal-like nitrides of various compositions. For example, when iron and nitrogen interact, iron nitrides of the composition Fe 2 N and Fe 4 N are formed. When nitrogen is heated with acetylene C 2 H 2, hydrogen cyanide HCN can be obtained.
Of the complex inorganic nitrogen compounds, nitric acid is the most important (cm. NITRIC ACID) HNO 3, its salts nitrates (cm. NITRATES), and nitrous acid HNO 2 and its salts nitrites (cm. NITRITES).
Application
In industry, nitrogen gas is used mainly to produce ammonia (cm. AMMONIA). As a chemically inert gas, nitrogen is used to provide an inert environment in various chemical and metallurgical processes, when pumping flammable liquids. Liquid nitrogen is widely used as a refrigerant (cm. REFRIGERANT), it is used in medicine, especially in cosmetology. Nitrogen mineral fertilizers are important in maintaining soil fertility (cm. MINERAL FERTILIZERS).
encyclopedic Dictionary. 2009 .
Synonyms:See what “nitrogen” is in other dictionaries:
- (N) chemical element, gas, colorless, tasteless and odorless; makes up 4/5 (79%) air; beat weight 0.972; atomic weight 14; condenses into liquid at 140 °C. and pressure 200 atmospheres; constituent of many plant and animal substances. Dictionary… … Dictionary of foreign words of the Russian language
NITROGEN- NITROGEN, chemical. element, symbol N (French AZ), serial number 7, at. V. 14.008; boiling point 195.7°; 1 l A. at 0° and 760 mm pressure. weighs 1.2508 g [lat. Nitrogenium (“generating saltpeter”), German. Stickstoff (“suffocating… … Great Medical Encyclopedia
- (lat. Nitrogenium) N, chemical element of group V of the periodic system, atomic number 7, atomic mass 14.0067. The name is from the Greek a negative prefix and zoe life (does not support respiration or combustion). Free nitrogen consists of 2 atomic... ... Big Encyclopedic Dictionary
nitrogen- a m. azote m. Arab. 1787. Lexis.1. alchemist The first matter of metals is metallic mercury. Sl. 18. Paracelsus set off to the end of the world, offering everyone his Laudanum and his Azoth for a very reasonable price, for the healing of all possible... ... Historical Dictionary of Gallicisms of the Russian Language
- (Nitrogenium), N, chemical element of group V of the periodic system, atomic number 7, atomic mass 14.0067; gas, boiling point 195.80 shs. Nitrogen is the main component of air (78.09% by volume), is part of all living organisms (in the human body... ... Modern encyclopedia
Nitrogen- (Nitrogenium), N, chemical element of group V of the periodic system, atomic number 7, atomic mass 14.0067; gas, boiling point 195.80 °C. Nitrogen is the main component of air (78.09% by volume), is part of all living organisms (in the human body... ... Illustrated Encyclopedic Dictionary
- (chemical sign N, atomic weight 14) one of the chemical elements; colorless gas, odorless, tasteless; very little soluble in water. Its specific gravity is 0.972. Pictet in Geneva and Calhet in Paris succeeded in condensing nitrogen by subjecting it to high pressure... Encyclopedia of Brockhaus and Efron
N (lat. Nitrogenium * a. nitrogen; n. Stickstoff; f. azote, nitrogene; i. nitrogeno), chemical. element of group V is periodic. Mendeleev system, at.sci. 7, at. m. 14.0067. Opened in 1772 researcher D. Rutherford. Under normal conditions A.… … Geological encyclopedia
Male, chem. base, main element of saltpeter; saltpeter, saltpeter, saltpeter; it is also the main, in quantity, component of our air (nitrogen 79 volumes, oxygen 21). Nitrogenous, nitrogenous, nitrogenous, containing nitrogen. Chemists distinguish... Dahl's Explanatory Dictionary
Organogen, nitrogen Dictionary of Russian synonyms. nitrogen noun, number of synonyms: 8 gas (55) non-metal... Synonym dictionary
Nitrogen is a gas that extinguishes flames because it does not burn and does not support combustion. It is obtained by fractional distillation of liquid air and stored under pressure in steel cylinders. Nitrogen is used mainly for the production of ammonia and calcium cyanamide, and... ... Official terminology
Books
- Chemistry tests. Nitrogen and phosphorus. Carbon and silicon. Metals. Grade 9 (To the textbook by G. E. Rudzitis, F. G. Feldman “Chemistry. Grade 9”, Borovskikh T.. This manual fully complies with the federal state educational standard (second generation). The manual includes tests covering the topics of G.’s textbook. E. Rudzitisa, F. G.…