Nitrogen: position in P.S.E., atomic structure, occurrence in nature, preparation and properties. Application of nitrogen. Presentation "use of nitrogen" Presentation on the topic of obtaining and using nitrogen

Repeat and consolidate knowledge about the structure of the atom and molecule of nitrogen. Study the physical and chemical properties of nitrogen. Reveal the role of nitrogen in nature.

“There is no life without nitrogen, for it is an indispensable component of proteins.” D.N. Pryanishnikov

K. Scheele and G. Cavendish obtained nitrogen in 1772. D. Rutherford described the preparation and properties in 1787. Lavoisier proposed the name nitrogen - “lifeless” (and - no, zoe - life). Numerous names: unclean gas, suffocating gas, spoiled air, flammable air, saltpeter, putrefactive agent, deadly gas, nitrogen, etc.

Natural form Earth's shell Salts of ammonium and nitric acid Lithosphere, hydrosphere Nitrogen Atmosphere Nitrogen and ammonia from volcanoes Lithosphere Compounds in some types of fuel (oil, coal) Lithosphere Nucleic acids, protein substances Biosphere

2nd period, 5th group, main subgroup Contains 5 electrons on the outer energy level +7)) 2 5 Oxidizing agent N 0 + 3e -  N -3 * Make up formulas for compounds of N with Li, Ca, Al. Reducing agent N 0 –1,2,3,4,5e -  N +1 ,N +2 ,N +3 ,N +4 ,N +5 * Make up the formulas of the oxides 3 1 2 4

N N N  N BOND: -COVALENT NON-POLAR -TRINARY -STRONG MOLECULE: -VERY STABLE -LOW REACTIVITY 1 3 4 2

Colorless, odorless and tasteless gas. Poorly soluble in water. Slightly lighter than air, density 1.2506 kg/m3 Tº pl.= -210 º C Tº boil.= -196 º C Does not support respiration and combustion

Oxidizing N 2 0 2N -3 When heated with other metals (Ca, Al, Fe) At room tº only with Li * At high tº, p, kat (Fe, Al, K oxides) with H 2 Reductive N 2 0 2N +2 * At tº electric arc (3000 - 4000 º C) with O 2

Application Production of ammonia and nitric acid. Creation of an inert atmosphere in metallurgy. Production of nitrogen fertilizers. Production of explosives. Liquid nitrogen in medicine. Saturation of steel surface to increase strength

Preparation In industry - from liquid air In the laboratory - by decomposition of unstable nitrogen compounds

1 m 2 o 3 l 4 e 5 k 6 u 7 l 8 a Securing new material

Reflection (work in pairs) Name of the topic - one noun Description of the topic - two adjectives Description of the action - two verbs + gerunds (or three verbs) Attitude to the topic - four words The essence of the topic - one word.

Paragraph No. 23, report sheet, exercise 5 work tetra Write a story on the topic: “The Journey of Nitrogen in Nature” Answer the questions: How can you prove experimentally that there is nitrogen in the air? To transport vegetables and fruits over long distances, refrigerators are used, in which liquid NITROGEN is used as a refrigerant. What properties is this based on?

HISTORY OF THE DISCOVERY 1772 K. Scheele and G. Cavendish obtained nitrogen D. Rutherford described the preparation and properties 1787 Lavoisier proposed the name nitrogen - “lifeless” (but no, zoe - life) Numerous names: unclean gas, suffocating gas, septon, spoiled air, disturbed air, saltpeter, putrefactive agent, deadly gas, nitrogen, etc.

Occurrence in nature: 1) in a free state in the atmosphere (78%), 2) in a bound state (see table) Natural form Earth's shell Salts of ammonium and nitric acid Lithosphere, hydrosphere Nitrogen Atmosphere Nitrogen and ammonia of volcanoes Lithosphere Compounds in some types of fuel ( oil, coal) Lithosphere Nucleic acids, protein substances Biosphere

Here is what famous scientists wrote about Nitrogen: F. Engels - “Life is the way of existence of protein bodies on Earth” D. Rutherford - “Suffocating Air” K. Scheele - “Bad Air” A. Lavoisier - “Lifeless Air” D.I. . Pryanishnikov - “There is no life without nitrogen, for it is the most important component of the protein molecule.”

STRUCTURE AND PROPERTIES OF THE ATOM? period, ? group, ? subgroup Contains at the external energy level? electrons +7)) ? ? ? N 0 + 3e - N -3 * Make up formulas for the compounds of N with Li, Ca, Al. ? N 0 –1,2,3,4,5e - N +1,N +2,N +3,N +4,N +5 * Make up the formulas of the oxides

STRUCTURE AND PROPERTIES OF THE ATOM 2nd period, 5th group, main subgroup C contains 5 electrons on the outer energy level +7)) 2 5 Oxidizing agent N 0 + 3e - N -3 * Make up formulas for compounds of N with Li, Ca, Al. Reducing agent N 0 –1,2,3,4,5e - N +1,N +2,N +3,N +4,N +5 * Make up the formulas of the oxides

STRUCTURE OF THE MOLECULE N N N BOND: -COVALENT NON-POLAR -TRINARY -STRONG MOLECULE: -VERY STABLE -LOW REACTIVITY

CHEMICAL PROPERTIES Assignment: give a complete description of the reactions *; under what conditions (c, t, p) the equilibrium will shift to the right. Oxidizing N 2 0 2N -3 When heated with other metals (Ca, Al, Fe) At room tº only with Li * At high tº, p, kat (Fe, Al, K oxides) with H 2 Reductive N 2 0 2N +2 * At tº electric arc (ºС) with O 2

TEST YOURSELF N 2 +3H 2 2NH 3 +Q Reversible Compounds Exothermic Homogeneous Catalytic with N 2 and H 2 increase tº decrease p increase N 2 +O 2 2NO –Q Reversible Compounds Endothermic Homogeneous Non-catalytic with N 2 and O 2 increase tº increase p does not affect

Questions for self-control 1. Gas without color, taste and smell 2. The molecule is diatomic 3. The content in the air is 78% 4. In the laboratory it is obtained by the decomposition of KMnO 4 and H 2 O 2 5. In industry - from liquid air 6. Chemically inactive 7. Interacts with almost all simple substances 8. The processes of respiration and photosynthesis are associated with it 9. Is an integral part of proteins 10. Participates in the cycle of substances in nature

TEST YOURSELF O 2 1, 2, 4, 5, 7, 8, 10. “5” N 2 1, 2, 3, 5, 6, 9, 10. “5” 1-2 errors “4” 3-4 errors “3” 5 errors or more “2” Using information about nitrogen as an example, give arguments in favor of two points of view: 1. Nitrogen is “lifeless” 2. Nitrogen is the main element of life on Earth.

Application. Liquid nitrogen is used as a refrigerant and for cryotherapy. Industrial applications of nitrogen gas are due to its inert properties. Gaseous nitrogen is fire- and explosion-proof, prevents oxidation and rotting. In petrochemistry, nitrogen is used to purge tanks and pipelines, check the operation of pipelines under pressure, and increase the production of fields. In mining, nitrogen can be used to create an explosion-proof environment in mines and to expand rock layers. In electronics manufacturing, nitrogen is used to purge areas that do not allow the presence of oxidizing oxygen. In a process traditionally carried out using air, if oxidation or decay are negative factors, nitrogen can successfully replace air. An important area of application of nitrogen is its use for the further synthesis of a wide variety of compounds containing nitrogen, such as ammonia, nitrogen fertilizers, explosives, dyes, etc. Large quantities of nitrogen are used in coke production (“dry quenching of coke”) during unloading coke from coke oven batteries, as well as for “pressing” fuel in rockets from tanks to pumps or engines. In the food industry, nitrogen is registered as a food additive E941, as a gaseous medium for packaging and storage, a refrigerant, and liquid nitrogen is used when bottling oils and non-carbonated drinks to create excess pressure and an inert environment in soft containers. Content.

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Nitrogen

“Nitrogen oxide” - 4. Give examples of reactions that prove the acidic properties of nitric oxide (III). Nitric oxide (V). Several nitrogen oxides are known. +1 +2 +3 +4 +5. NO. N2O. All nitrogen oxides, except N2O, are toxic substances. Nitrogen is capable of exhibiting several oxidation states from -3 to +5. +3 +5 2NO2 + H2O = HNO2 + HNO3.

“Silicon and its compounds” - Characteristics plan: In nature, it occurs in the form of oxides, silicates and aluminosilicates. From top to bottom: Garnet. Study the properties of silicon. Analysis of lunar soil samples showed the presence of SiO2 in an amount of more than 40%. Lesson objectives: Application of silicon compounds. Give a general description of the element silicon. It is also found in plants and animals.

“Nitrogen Lesson” - At the end of the lesson, students evaluate their activities in accordance with self-assessment criteria. 2. Operational and execution stage (15 min.). Methodological recommendations for studying the topic “Nitrogen as a simple substance.” 3. Reflective-evaluative stage (20 min.). Equipment and teaching material. It takes 2 hours to study the topic.

“Nitrogen and its compounds” - Nitrogen compounds. Radioactive isotopes of nitrogen with mass numbers 11, 12, 13, 16 and 17 are known. The oxidation states of nitrogen in compounds are: 3, ?2, ?1, +1, +2, +3, +4, +5. The amount of CuO is 2 times greater than calculated. There is another version. Municipal educational institution “Secondary school No. 6 with in-depth study of the French language.”

“Obtaining radioactive isotopes” - Radioactive isotopes in biology. The “labeled atoms” method has become one of the most effective. Radioactive isotopes are widely used in science, medicine and technology. Application of radioactive isotopes. Radioactive isotopes in archeology. Using nuclear reactions, isotopes of all chemical elements can be obtained.

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Symbol - N Atomic weight - 14.0067 Density - 0.808 (at -195.8°C) Melting point - -209.86 °C Boiling point - -195.82 °C Discovered - by D. Rutherford in 1772 Nitrogen and its compounds

Liquid nitrogen Liquid nitrogen is non-explosive and non-toxic. By evaporating, nitrogen cools the fire and displaces the oxygen necessary for combustion, so the fire stops. Since nitrogen, unlike water, foam or powder, simply evaporates and disappears, nitrogen fire extinguishing, along with carbon dioxide, is the most effective method of extinguishing fires from the point of view of preserving valuables. transparent liquid. Has a boiling point of − 195.75 ° C

Application of liquid nitrogen; for cooling various equipment and machinery; for cooling computer components during extreme overclocking

Application of liquid nitrogen Liquid nitrogen is used in cosmetology. for the treatment of vulgar, plantar and flat warts, papillomas, hypertrophic scars, vulgar acne, rosacea. In the food industry, nitrogen is registered as a food additive E941, as a gaseous medium for packaging and storage, a refrigerant, and liquid nitrogen is used when bottling oils and non-carbonated drinks to create excess pressure and an inert environment in soft containers.

Behavior of substances in liquid nitrogen Substances in liquid nitrogen become brittle

Burns with liquid nitrogen It is necessary to cool the affected areas of the body with water or cold objects, administer painkillers, and apply bandages made of sterile dressings or improvised materials to the wounds.

Caisson sickness Caisson sickness occurs when there is a rapid decrease in pressure (for example, when ascending from depth, leaving a caisson or pressure chamber, or ascending to a height). In this case, nitrogen gas, previously dissolved in the blood or tissues, forms gas bubbles in the blood vessels. Characteristic symptoms include pain or neurological impairment. Severe cases can be fatal.

Chemical properties of nitrogen Chemically, nitrogen is a fairly inert gas due to its strong covalent bond, while atomic nitrogen is chemically very active. Of the metals, free nitrogen reacts under normal conditions only with lithium, forming nitride: 6Li + N2 = 2Li3N With increasing temperature, the activity of molecular nitrogen increases. When nitrogen interacts with hydrogen under heating, elevated pressure and the presence of a catalyst, ammonia is formed: N2 + 3H2 = 2NH3 Nitrogen combines with oxygen only in an electric arc to form nitrogen oxide (II): N2 + O2 = 2NO

Nitrogen oxides Do not react with water and alkalis Nitric oxide(I) (N2O) Nitric oxide(II) (NO) Nitric oxide(III) (N2O3) Nitric oxide(IV) (NO2) Nitric oxide(V) (N2O5) 2NO2 + H2O = HNO3 + HNO2, 4NO2 + 2H2O + O2 = 4 HNO3.

Nitric acid The boiling point of nitric acid is +83 °C, the freezing point is –41 °C, i.e. under normal conditions it is a liquid. The pungent odor and the fact that it turns yellow during storage is explained by the fact that the concentrated acid is unstable and partially decomposes when exposed to light or heating. 4HNO3 = 2H2O + 4NO2 + O2.

Interaction with metals Concentrated nitric acid Me + HNO3(conc.) → salt + water + NO2 Noble metals (Au, Ru, Os, Rh, Ir, Pt), but a number of metals (Al, Ti, Cr) do not interact with concentrated nitric acid , Fe, Co, Ni) are passivated at low temperatures with concentrated nitric acid. The reaction is possible with increasing temperature Ag + 2HNO3(conc.) → AgNO3 + H2O + NO2.

Interaction with metals Dilute nitric acid The product of reduction of nitric acid in a dilute solution depends on the activity of the metal involved in the reaction: Active metal 8 Al + 30HNO3(dil.) → 8 Al(NO3)3 + 9H2O + 3NH4NO3 Medium activity metal 10Cr + 36HNO3( dil.) → 10Cr(NO3)3 + 18H2O + 3N2 Low-active metal 3 Ag + 4HNO3(dil.) → 3 AgNO3 + 2H2O + NO

Preparation of nitric acid NaNO3 + H2SO4 = NaHSO4 + HNO3 4NH3 + 5O2 → 4NO + 6H2O (Conditions: catalyst – Pt, t = 500˚ C) 2NO + O2 → 2NO2 4 NO2 + O2 + 2 H2O ↔ 4HNO3

Application of nitric acid Production of nitrogen and complex fertilizers. Production of explosives. Production of dyes. Medicine production. Production of films, nitro-varnishes, nitro-enamels. Production of artificial fibers. As a component of a nitrating mixture for trawling metals in metallurgy.

Ammonia. Ammonia - NH3, hydrogen nitride, under normal conditions - a colorless gas with a sharp characteristic odor (the smell of ammonia). Ammonia is almost twice as light as air. The solubility of NH3 in water is extremely high - about 1200 volumes (at 0 °C) or 700 volumes (at 20 °C) per volume (Ammonia (in European languages its name sounds like “ammoniac”) owes its name to the Ammon oasis in North Africa, located at the crossroads of caravan routes. In hot climates, urea (NH2)2CO, contained in animal waste products, decomposes especially quickly. One of the products of decomposition is ammonia. According to other sources, ammonia got its name from the ancient Egyptian word amonian. This was the name of the people worshipers of the god Amon. During their ritual rites, they sniffed ammonia NH4Cl, which, when heated, evaporates ammonia.

Ammonia is dangerous In medicine, a 10% aqueous solution of ammonia is known as ammonia. The pungent odor of ammonia irritates specific receptors of the nasal mucosa and promotes excitation of the respiratory and vasomotor centers, therefore, in case of fainting or alcohol poisoning, the victim is allowed to inhale vapors of ammonia. Ammonia is dangerous if inhaled. In acute poisoning, ammonia affects the eyes and respiratory tract, and at high concentrations it can be fatal. Causes severe coughing, suffocation, and with a high concentration of vapors - agitation, delirium. Upon contact with skin - burning pain, swelling, burn with blisters. First aid: rinse eyes and face with water, put on a gas mask or a cotton-gauze bandage moistened with a 5% solution of citric acid, rinse exposed skin with plenty of water, immediately leave the source of infection. If ammonia gets into the stomach, drink several glasses of warm water with the addition of one teaspoon of table vinegar per glass of water and induce vomiting.

To produce ammonia, laboratories use the action of strong alkalis on ammonium salts: NH4Cl + NaOH = NH3 + NaCl + H2O (NH4)2SO4 + Ca (OH)2 = 2NH3 + CaSO4 + 2H2O The industrial method for producing ammonia is based on the direct interaction of hydrogen and nitrogen: N2( g) + 3H2(g) ↔ 2NH3(g) + 45.9 kJ Conditions: catalyst - porous iron temperature - 450 - 500 ˚ C pressure - 25 - 30 atm

Chemical properties of ammonia NH3 is a strong reducing agent. 1. Combustion of ammonia (when heated) 4NH3 + 3O2 → 2N2 + 6H20 2. Catalytic oxidation of ammonia (catalyst Pt – Rh, temperature) 4NH3 + 5O2 → 4NO + 6H2O

Interaction of ammonia with water and acids Both an aqueous solution of ammonia and ammonium salts contain a special ion - the ammonium cation NH4, which plays the role of a metal cation. It is obtained as a result of the fact that the nitrogen atom has a free (lone) electron pair, due to which another covalent bond is formed with the hydrogen cation passing to ammonia from acid or water molecules: This is a mechanism for the formation of a covalent bond that does not arise as a result sharing of unpaired electrons, and due to the free electron pair present in one of the atoms, it is called donor-acceptor. NH3 + HCl = NH4Cl 2NH3 + H2SO4 = (NH4)2SO4↓ NH3 + H20 NH4 + OH- If a few drops of phenolphthalein are added to an ammonia solution, it will turn crimson, i.e. it will show an alkaline environment:

Ammonium salts enter into an exchange reaction with acids and salts: (NH4)2SO4 + Ba(NO3)2 → BaSO4 ↓ + 2NH4NO3 (NH4)2CO3 + 2HCl → 2NH4Cl + H2O + CO2 interact with alkali solutions to form ammonia - a qualitative reaction to the ion ammonium: NH4Cl + NaOH → NaCl + NH3 + H2O decompose when heated NH4Cl → NH3 + HCl NH4NO3 → N2O + 2 H2 O (NH4)2Cr2O7 → N2 + Cr2O3+ 4 H2 O

Nitrogen

and its connections

Unnoticeable in the atmosphere

And in reactions it is inert.

Can be beneficial

Serve in fertilizers...

Resides in the body

Plays a significant role...

We need him on the planet

To everyone, both adults and children...

What element are we talking about?

A Z O T

Being in nature

Nitrogen ranks 17th in abundance in the earth's crust, accounting for 0.0019% of the mass of the earth's crust

In bound form - mainly in the composition of two nitrates: sodium NaNO 3 (found in Chile, hence the name Chilean nitrate) and potassium KNO 3 (found in India, hence the name Indian saltpeter) and a number of other compounds.

In free form -

in the atmosphere

Five famous chemists of the 18th century. They gave a certain non-metal, which in the form of a simple substance is a gas and consists of diatomic molecules, five different names.

- “poisonous air”

- “dephlogisticated”

air"

- “spoiled air”

- "suffocating air"

- “lifeless air”

In 1772, a Scottish chemist

botanist and doctor Daniel Rutherford

In 1772, an English chemist

Joseph Priestley

In 1773, the Swedish chemist

pharmacist Karl Scheele

In 1774, an English chemist

Henry Cavendish

In 1776, a French chemist

Antoine Lavoisier

And it's all about nitrogen

Nitrogen forms strong diatomic N molecules 2 with short distance between cores

The molecule is diatomic and very strong

Structural formula N N

It contains a molecular lattice and a covalent

non-polar bond

Nitrogen is a colorless, odorless and tasteless gas.

Slightly soluble in water (2.5 volumes of nitrogen dissolve in 100 volumes of water).

It is lighter than air - 1 liter of nitrogen has a mass of 1.25 g.

At -196 C 0 nitrogen liquefies, and at -210 C 0 turns into a snow-like mass.

N 2

Nitrogen in compounds can manifest itself as

negative and positive CO.

Chemical properties of nitrogen

Nitrogen reacts with oxygen

(at electric arc temperature)

N 2 + O 2 =2NO

2. Nitrogen reacts with hydrogen (at a temperature of 300 0 C and pressure 20-30 MPa)

N 2 +3H 2 =2NH 3

3. At elevated temperatures, nitrogen reacts with certain metals

3Mg+N 2 =Mg 3 N 2

Production of nitrogen in industry :

Fractional distillation of liquid air

OJSC

"Nevinnomyssk Azot"

Plant for the production of nitrogen from liquid air

Obtaining nitrogen in the laboratory (decomposition of ammonium salts)

1. Decomposition of ammonium nitrite

N.H. 4 NO 2 =N 2 + 2H 2 O

2. Decomposition of ammonium dichromate

(NH 4 ) 2 Cr 2 O 7 =Cr 2 O 3 +N 2 +4H 2 O

Application

N 2

As a refrigerant

In cosmetology

For creating

inert

environment during experiments

For synthesis

ammonia

Application of nitrogen compounds

production of mineral fertilizers

production of explosives
production of medicinal products

Nitric oxide (I) N 2 O

N 2 O – nitric oxide (I), nitrous oxide or “laughing gas”, has a stimulating effect on the human nervous system, and is used in medicine as an anesthetic. Physical properties: gas, colorless and odorless. Exhibits oxidizing properties and easily decomposes. Non-salt-forming oxide.

2N 2 O=2N 2 + O 2

Nitric oxide (V)

N 2 O 5 – nitric oxide (V), nitric anhydride, white solid (mp. = 41 0 WITH). It exhibits acidic properties and is a very strong oxidizing agent.

The product of the reaction between an acidic

oxide and water is an acid

Nitric acid

One bond with oxygen is formed according to the donor-acceptor mechanism, but due to the proximity of the atoms in the molecule they become equivalent.