Fundamentals of chemistry: properties, application and production of nitrogen

Nitrogen is one of the most common elements on Earth - in the atmosphere its content exceeds 78%. The existence of such a large amount of nitrogen in the free state indicates its inertness and difficult interaction with other elements under normal conditions.

In a bound state, this substance can be found in organic and inorganic matter. Linked to carbon and oxygen, nitrogen is found in animal and plant proteins.

In itself, the name "nitrogen" was invented by Lavoisier, who in numerous experiments established the presence in the atmosphere of some inert substance. The scientist considered this substance lifeless - in Greek "azote".

Nitrogen cycle

Despite the inertness of nitrogen, in the nature there are constant processes of fixation or binding. For example, in the roots of legumes plants accumulate specific bacteria that fix nitrogen, processing it into nitrates.

In the atmosphere, this gas is oxidized during the lightning discharge. Then, nitrogen oxides dissolve in the sediments, forming an acid nitrogen and nitrogenous. With snow, rain, fog, nitrogen enters the soil, where it turns into nitrites or nitrates. Then, various plants use them to build protein. Animals feed on plants, and vegetable protein is processed into animal. When plants and animals are decomposed after death, all nitrogen compounds in their organisms are converted to ammonia. Bacteria destroy it up to the simplest elements, thus releasing again pure nitrogen and hydrogen. This is how the nitrogen cycle or the nitrogen cycle in nature occurs.

Chemical properties of nitrogen

Its main property under normal conditions is inertia, i.e. Minimal chemical activity. A nitrogen atom can form a bond with another nitrogen atom, which is quite unusual for chemical elements (except silicon and carbon only).

When heated, this element reacts with most metals. In this case, ionic, covalent or intermediate nitrides with a negatively charged nitrogen ion are formed.

In reaction with hydrogen, nitrogen forms sufficiently stable compounds - nitrogenous hydrocarbons, which are reminiscent of hydrocarbons. Such substances include ammonia, hydrazine and nitric acid.

Preparation and application of nitrogen

The compounds of this substance play an important role in industry and agriculture. The method of obtaining nitrogen in the form of a chemical element depends on the necessary degree of its purity. Most of the nitrogen is needed for the production of ammonia, but it allows a small amount of noble gases in it.

Obtaining nitrogen from the atmosphere

This is one of the most economical ways in which purified air is subsequently liquefied by cooling and expansion. The resulting liquid air is distilled through the fractions, slowly raising the temperature. In this process, noble gases are first released, followed by nitrogen. Only liquid oxygen remains .

This production of nitrogen allows many millions of tons of this substance to be produced every year. Nitrogen is used mainly for the subsequent production of ammonia, which, in turn, acts as a raw material for obtaining industrial and agricultural nitrogen-containing compounds.

A clean nitrogen atmosphere can also be used when a complete absence of oxygen is required.

Nitrogen production in the laboratory

In small quantities, this gas is obtained by oxidizing ammonium ions or ammonia. In particular, the ammonium ion can be oxidized with a nitrite ion.

The production of nitrogen in the process of decomposition

When heated, azides decompose, ammonia decomposes with copper oxide, nitrites decompose from reaction with urea or sulfamic acid - as a result of all these reactions, nitrogen is formed.