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Nitrogen and its compounds

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For the first time nitrogen was studied by Daniel Rutherford. After D. Belk discovered the reaction of the interaction of carbon dioxide with lime water, Rutherford investigated the changes in the composition of the air, after it lived and killed the living entity (in closed volume). After carbon dioxide was absorbed by alkali, the rest of the gas does not support combustion, and living beings instantly died. At about the same time, nitrogen was isolated from the air by chemists G. Cavendish and K. shale, both of them, unlike D. Rutherford realized that nitrogen is only part of the aria component. Cavendish wrote: "I converted ordinary air from one vessel through hot coals into another, then through fresh burning coal – into the next vessel, absorbing each time the formed fixed air (carbon dioxide) with lump lime. The specific gravity of the obtained gas was only slightly different from the specific gravity of ordinary air: nitrogen is slightly lighter than air from both gases. It extinguishes the flame and makes ordinary air unable to excite combustion, as well as fixed air (CO2), but to a lesser extent" History of Nitrogen

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K.Shelle G.Kavendish D.Rezerford

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Symbol:N Atomic nuber:7 Atomic mass:14 Electron conf: 2s2 2p3 Melting point:-210.1°C Boiling point:-195.8°C Density:1.25*10-³ Ionization energy:1402.3kj Atomic radius:75pm Common oxid.state:between -3;+5 Color: colorless Physical state at 25°C:gas Origin and meaning of name:nitron genes-nitrate former Earth's crust abundences:210*10-³

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Physical properties of nitrogen Under normal conditions, nitrogen-colorless gas, tasteless and odorless, absolutely harmless, a little lighter than air, little soluble in water. Melting point -210 °C, boiling point -196 °C.Nitrogen gas consists of diatomic molecules. A triple bond is realized between atoms in the molecule, as a result of which the nitrogen molecule is extremely strong, the energy of chemical bond is 945 kJ/mol. Even at 3000 °C, the degree of decomposition of the nitrogen molecule into atoms reaches only 0.1 %.The structure of solid nitrogen is constructed from diatomic molecules bound by weak forces of intermolecular interaction.

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 Chemical properties of nitrogen Due to the presence of a strong triple bond, molecular nitrogen is inactive, and nitrogen compounds are thermally unstable and relatively easily decompose when heated to form free nitrogen. Interaction with metals: Under normal conditions, molecular nitrogen reacts only with some strong reducing agents, such as lithium:  6Li + N2 = 2li3n.  For the formation of magnesium nitride from simple substances requires heating up to 300°C:  3Mg + N2 = Mg3N2. Nitrides of active metals are ionic compounds that are hydrolyzed with water to form ammonia. Interaction with oxygen. Only under the influence of electric discharge nitrogen reacts with oxygen:  O2 + N2 = 2NO.  Hydrogen interaction with. The reaction with hydrogen takes place at a temperature of about 400 ° C and a pressure of 200 ATM in the presence of a catalyst-iron:  3H2 + N2 = 2NH3.  Interaction with other non-metals.At high temperatures reacts with other nonmetals, such as boron:  2B + N2 = 2BN Nitrogen does not react directly with Halogens and sulfur, but the halides and sulfides can be obtained by indirect means. Nitrogen does not interact with water, acids and alkalis.

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Nitrogen-Production and application In the laboratory nitrogen can be easily obtained by heating concentrated ammonium nitrite:  NH4NO2 N2 + 2H2O.  The technical method of producing nitrogen based on a pre- separation of liquid air which is then subjected to distillation. Free nitrogen is used in many industries: as an inert environment in various chemical and metallurgical processes, to fill in space in a mercury thermometer, when pumping flammable liquids, etc. Liquid nitrogen finds application in various refrigeration systems. It is stored and transported in steel Dewar vessels, compressed nitrogen - in cylinders. Many nitrogen compounds are widely used. The production of fixed nitrogen began to develop intensively after the 1st world war and has now reached enormous proportions.

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 The presence in the nature. In nature, nitrogen is in free form and in the form of compounds. Free nitrogen is the main component of air (78% by volume). Inorganic nitrogen compounds are found in small quantities except for a large field of sodium nitrate in Chile. The soil contains small amounts of nitrogen in the form of salts of nitric acid.

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