The oxygen compound is nitrogen. Oxygen nitrogen compounds - Knowledge hypermarket

Summary of the lesson on the topic: " Oxygen compounds  nitrogen. " Grade 9

The purpose of the lesson: to study the properties of nitrogen oxides.

Tasks:

educational: consider nitrogen oxides, and by their example, repeat the classification and basic properties of oxides;

educational: the formation of a scientific picture of the world;

developing: the development of logical thinking, the ability to work with additional literature, the ability to generalize and systematize.

During the classes.

Organizing time.

Repetition of the material studied.

Several students work on the cards, with the rest conducted a frontal survey on the previous topic.

Didactic card number 1

a) Write the formulas of the following substances: ammonia, ammonia, ammonia

Qualitative reaction to the ammonium cation;

The interaction of ammonium sulfate with barium chloride.

Didactic card number 2

a) Write the formulas of the following substances: ammonium dichromate, ammonia, ammonium sulfate.

b) Write the following reaction equations:

The interaction of ammonium chloride with silver nitrate;

The interaction of ammonium carbonate with hydrochloric acid.

Front-end survey:

1) What is “ammonia”? What is it used for?

2) What properties of ammonia underlie its use in refrigeration?

3) How should ammonia be collected? Why? How can ammonia be recognized?

5) What is ammonia? What is it used for?

6) What is the use of carbonate and ammonium bicarbonate?

3. Actualization of knowledge.

Arrange the degree of oxidation in nitrogen oxides:

N 2 O NO N 2 O 3 NO 2 N 2 O 5

The study of new material.

The teacher informs the topic, purpose and lesson plan.

Plan:

Classification of nitrogen oxides.

Post student on the topic: "The history of the discovery of nitric oxide (I)."

Physical properties of nitrogen oxides (independent work with the text of the textbook).

Chemical properties, production and use of nitrogen oxides, (teacher’s story and explanation).

Classification of nitrogen oxides. Students together with the teacher fill out the diagram.

ABOUT nitrogen oxides

Non-salt-forming Salt-forming

N 2 O NO N 2 O 3 → HNO 2

do not interact with acids, N 2 O 5 → HNO 3

nor with alkalis and do not form salts NO 2 → HNO 2 and HNO 3

Student's message subject: "The history of the discovery of nitric oxide (I)».

Laughing gas.

An American chemist in 1800 studied the interaction of sulfur with a heated solution of sodium nitrite NaNO 2 in formamide HCONH 2. Suddenly, a violent reaction began with the release of gas with a faint pleasant smell. Woodhouse suddenly felt hilarious, and he started dancing, singing songs. The next day, returning to the laboratory, he discovered in the flask where the experiment was going on, sodium thiosulfate crystals Na 2 S 2 O 3. Almost at that time, the English chemist Humphrey Devi carried out the thermal decomposition of ammonium nitrate NH 4 NO 3. As he later recalled, the assistant leaned too close to the installation and several times inhaled the gas with a pleasant smell coming out of the retort. Suddenly the assistant burst out with a gratuitous laugh, and then fell in the corner of the room and immediately fell asleep.

Scientists obtained the same gas - nitric oxide (I) N 2 O.

Oxide formula

Physical properties

Chemical properties

Preparation and use

N 2 O

colorless incombustible with a pleasant sweetish and.

2N 2 O → 2N 2 + O 2

NH 4 NO 3 → N 2 O + 2H 2 O

Low concentrations of nitrous oxide cause lung(hence the name “laughing gas”). When inhaling clean gas, intoxication and drowsiness develop rapidly. Nitrous oxide has a weak narcotic activity, and therefore in medicine it is used in high concentrations.

colorless gas, poorly soluble in water.

2NO + O 2 → 2NO 2

4 NH 3 + 5O 2 → 4NO + 6H 2 O

Obtaining NO is one of the stages of receipt.

NO 2

A poisonous gas, red-brown in color, with a characteristic pungent odor or yellowish liquid. Fox's tail.

NO 2 + H 2 O → HNO 2 + HNO 3

4NO 2 + H 2 O + O 2 → 4HNO 3

2NO 2 + 2NaOH → NaNO 3 + NaNO 2 + H 2 O

2Cu (NO 3) 2 → 2CuO + 4NO 2 + O 2

In productionand, as an oxidizing agent in a liquidand composite explosives.Highly toxic. It irritates the respiratory tract, in high concentrations causesNO + NO 2 = N 2 O 3

Used in the laboratory to obtain nitrous acid and its salts. Highly toxic. The effect on the body is comparable with fuming nitric acid, causes severe skin burns.

N 2 O 5

colorless, very volatile crystals. Extremely unstable.

N 2 O 5 + H 2 O = 2HNO 3

N 2 O 5 + CaO = Ca (NO 3) 2

N 2 O 5 + 2 NaOH = 2NaNO 3

2NO 2 + O 3 = N 2 O 5 + O 2

N 2 O 5 is toxic.

4. Fastening. Exercise 6

5. Reflection, summing up. Ratings.

6. Homework §26.

Oxygen nitrogen compounds serve as a vivid example of how the qualities of bodies change when their quantitative composition changes. The first is a gas, the second, at ordinary temperatures, is a solid crystalline solid.
  Oxygen compounds of nitrogen exist for all its positive oxidation states from 1 to V. Nitrogenous acid H2N2O2 and its salts - hyponitrite - are very unstable when heated, have weak oxidizing and reducing properties.
  Oxygen compound of nitrogen, where it exhibits the highest valence - N2Os, nitrogen pentoxide, nitrogen anhydride.
  Oxygen nitrogen compounds serve as vivid examples of how the qualities of bodies change as their quantitative composition changes. The first is a gas, the second, at ordinary temperatures, is a solid crystalline solid.
  Oxygen compounds of nitrogen (PG, U) in an acidic environment oxidize HoS, PHg, RI in solution to form water-soluble compounds.
  Consider the oxygen compounds of nitrogen.
  The ability of the oxygen compounds of nitrogen NO2X to complexate and nitrate reactions should be determined by both electrophilicity and the coordination unsaturation of the nitrogen atom. With the same coordination number, the activity is determined by electrophilicity, with the free nitronium cation ONO being the most active. Solvation greatly reduces its activity. The decrease in the selectivity of the entering nitrogroup into the nucleus with an increase in the temperature of Titov is explained by a decrease in the solvation of the nitronium cation.
The chemistry of oxygen compounds of nitrogen and phosphorus has already been considered; We now turn to the consideration of the elements of subgroups A and B. The chemistry of the oxygen compounds of vanadium, the least electropositive of all the elements of subgroup A, is in many ways similar to the chemistry of phosphorus. Since these two elements have the same coordination numbers with respect to oxygen, their oxo compounds with the same formula have similar structures and are often isomorphic to each other, and also isomorphic to the corresponding arsenic compounds. For example, dodecahydrates Na3PO4, Na3AsO4, Na3VO4, and Pb3 (PO4) C1, Pb5 (AsOJCl and Pb5 (VO4) Cl) complex salts are isomorphic. Vanadium is widely distributed in nature; it is commonly found with phosphorus in the form of vanadium (large deposits of the rare mineral patronite VSB are also a very important source of vanadium), and niobium and tantalum are commonly found together with other transition or rare earth metals. Ortho -, meta - and pyrovanadates are known, but the degree of stability of these compounds in aqueous solutions is inverse to the stability of the corresponding phosphorus s.
  Oxygen compounds of nitrogen include all oxides of nitrogen, nitric and nitrous acids, and their salts.
  In oxygen compounds of nitrogen per nitrogen atom accounts for from 0 5 to 3 oxygen atoms. Depending on the conditions, the nitrogen atom can attach or lose some or all of the oxygen atoms.
  Like all oxygen compounds of nitrogen, its oxide is an endothermic compound, and oxygen is retained in it leprotochno. Therefore, hydrogen, coal, kerosene and other combustible substances burn in it as well as in pure oxygen, with a flame with a wide bluish halo.
  Like all oxygen compounds of nitrogen, its oxide is - the compound is endothermic, the oxygen in it is held weakly. Therefore, hydrogen, coal, kerosene and other combustible substances; burn in it as well as in pure oxygen, flame, with a wide bluish halo.
  Oxides and oxygen compounds of nitrogen of different degrees of oxidation are obtained by oxidation of ammonia first to nitric oxide (catalytic process), which is then easily oxidized by atmospheric oxygen to nitric acid.
  Ammonium ion scheme. Of all the oxygen compounds of nitrogen in nature, salts of nitric acid, the so-called saltpeter, are the most common; NaNOs deposits in Chile are especially famous.

Using the example of oxygen compounds of nitrogen, one can demonstrate the formation of complex atoms of double, triple, and higher orders, which Dalton does.
Which of the five oxygen compounds of nitrogen have acidic properties.
  Of the oxygen compounds of nitrogen present in the atmosphere, the pollutants are nitric oxide, nitrogen dioxide and nitric acid. They are mainly formed as a result of the decomposition of nitrogen-containing substances by soil bacteria. Every year around the world, 50 - 10 7 tons of nitric oxide of natural origin enter the atmosphere, while as a result of human activity, only 5 - 10 7 tons of oxide and nitrogen dioxide.
  Quantum-chemical characteristics for oxygen nitrogen compounds obtained by the CPAP method are given.
  The oxygen compounds of nitrogen that we have examined so far can all be obtained from nitric oxide and are converted into it, and therefore nitrogen oxide is in close connection with them. The transition of nitric oxide in the presence of oxygen to higher oxidation states and back serves in practice as a means for the transfer of atmospheric oxygen to substances capable of oxidation. Having nitric oxide, it is easy to convert it, with the help of air and water oxygen, to nitric acid, to N2O3 and NO2, and with the help of them to oxidize the body. This oxidative action again produces nitric oxide; it can be transferred again to nitric acid, and so on, without end, if only there would be oxygen in the air and water.
  From the point of view of thermodynamics, all oxygen compounds of nitrogen can be reduced to hydrazine by many reducing agents.
  Oxidation-reduction reactions are very typical for oxygen compounds of nitrogen and phosphorus.
  Nitric acid and nitrates are the most important oxygen compounds of nitrogen. In the concentrated state, nitric acid has strong oxidizing properties and extreme care should be taken when working with it.
  The reactions of reduction of some oxygen compounds of nitrogen and arsenic compounds are of analytical importance. Appropriate methods are widely included in the practice of a number of laboratories. Among the phosphorus compounds there are also those that could be reduced by the divalent chromium ion, but the reactions have not been studied.
  Below are the most widely used in industry oxygen compounds of nitrogen.
Influence of the coefficient of excess air in the furnace on the loss of heat from chemical underburning when burning natural gas. | The effect of excess air in the furnace on the content of S03 in the combustion products. When burning fuel oil in furnaces of energy steam generators, toxic oxygen nitrogen compounds are formed. The amount of nitrogen oxides formed is strongly influenced by excess air and the temperature of the process. The higher they are, the more nitrogen oxides.
  Similarly, Dalton determines the structure of ammonia, oxygen compounds of nitrogen, sulfur and carbon and other substances. In all these cases, he concludes, weights are expressed in hydrogen atoms, each of which is denoted by a unit.
  The elucidation of the electronic structure and characteristics of chemical bonds in oxygen compounds of nitrogen presents considerable difficulties. The fact is that some molecules of nitrogen oxides, for example NO, NO2, have an odd number of valence electrons, therefore, there always remains one electron that cannot form an electron pair. Thus, the theory of electron pairs is insufficient and requires either its further development or the development of a new approach to solving the problems of chemical bonding, the foundations of which are laid in quantum chemistry.
  The elucidation of the electronic structure and characteristics of chemical bonds in oxygen compounds of nitrogen presents considerable difficulties. The fact is that some molecules of nitrogen oxides, for example N0, N02, have an odd number of valence electrons, therefore, there is always one electron left that cannot form an electron pair. Thus, the theory of electron pairs is insufficient and requires either its further development or the development of a new approach to solving the problems of chemical bonding, the foundations of which are laid in quantum chemistry.

In the production of sulfuric acid by the nitrous method, oxygen nitrogen compounds play a crucial role. In § 2, the essence of the process of obtaining sulfuric acid using oxides of nitrogen was briefly described.
  In this method of obtaining sulfuric acid, oxygen nitrogen compounds play a crucial role. Chapter 1 summarized the essence of the process of obtaining sulfuric acid using oxides of nitrogen.
When the mixture is distilled in vacuum, unchanged formaldehyde, oxygen nitrogen compounds, formic acid and methyl alcohol are distilled; A few drops of an oily brown liquid with a caramel smell (polymerized trioxymethylene [(CH20) 3] 2, obtained by Renard during the electrolysis of glycerin acidified with sulfuric acid) and a few very spreadable ammonium nitrate crystals remain in the flask.
  Further, Dalton determines in the same way the structure of ammonia and oxygen compounds of nitrogen and carbon.
  Kinetics of thermal decomposition of oxygen compounds. In tab. VI, 1 shows the kinetic data on the decomposition of oxygen compounds of nitrogen and halogens.
  Thus, this experience conclusively proves that the reduction of oxygen compounds of nitrogen, or, equivalently, the reduction of nitric acid with formaldehyde, leads to the formation of formaldoxime. It should, however, be noted that the yield of formaldoxime is extremely low, partly because it very easily evaporates with the ether ester pairs as already noted by Schole.
  In tab. VI, 1 shows the kinetic data on the decomposition of oxygen compounds of nitrogen and halogens.
  When considering the properties of fluorinated compounds, it is appropriate to draw an analogy with the properties of oxygen nitrogen compounds, since the latter have been studied in detail and have found wide application.
  Only relatively recently it became clear that nitric oxide is directly oxidized to dioxide, bypassing the intermediate oxygen compounds of nitrogen, the existence of which had previously been assumed.
  If we express these relations in percentages, then we will not be able to reveal any natural connection between the composition of all oxygen compounds of nitrogen.
  We now apply these concepts to ammonia, as a hydrogenous compound, in order to see its relation to oxygen compounds of nitrogen.
  Associated nitrogen is contained in the air in the form of ammonia (formed during the decomposition of nitrogen-containing organic compounds) and traces of oxygen nitrogen compounds (NO2 and DR -) - Ammonia derivatives (for example, ammonium salts) and salts of nitric acid are found in the earth's crust. The good solubility of these compounds explains the absence of significant accumulations in the crust. In a bound form, nitrogen is also found in black coal (from 1 to 2 5 wt.
Associated nitrogen is contained in the air in the form of ammonia (formed during the decomposition of nitrogen-containing organic compounds) and traces of oxygen nitrogen compounds (NO. Ammonia derivatives (for example, ammonium salts) are found in the earth's crust. Nitric acid salts. Good solubility of these compounds explains the absence of significant their accumulations in the earth's crust. In a bound form, nitrogen is also found in black coal (from 1 to 2 5 wt.

Ensure that the reagents used for analysis do not contain oxygen compounds of nitrogen at all and that rubber and glass tubes used are not contaminated with oxygen compounds of nitrogen.

Laboratory - practical lesson number 21

Topic 2.1.3. Main subgroup of the V group

The topic of the lesson is “Properties of compounds of oxidized nitrogen, phosphorus and its compounds”.

Objectives of the lesson:

· Improve knowledge of the properties of oxygen-containing compounds of nitrogen and phosphorus by performing exercises on the compilation of reaction equations proving

Chemical properties of oxygen-containing compounds of nitrogen and phosphorus;

Features of the interaction of nitric acid with metals

Thermal decomposition of nitrates.

· To get skills

Perform qualitative reactions to nitrate -, nitrite -, phosphate - ions.

· Improve the skills of formulating the equations of redox reactions

Theoretical part:

I Oxygen nitrogen compounds.

1. Nitrous acid.Nitrous acid is weak, unstable, exists only in solution. When interacting with alkalies, it forms salts - nitrites.

Nitrous acid salts - nitrites - are quite resistant to heat. With the exception of AgNO 2, they are all readily soluble in water. Like nitrous acid itself, nitrites have redox duality:

5KNO 2 + 2KMnO 4 + 3H 2 SO 4 = 5KNOz + 2MnSO 4 + K 2 SO 4 + 3H 2 O

reducing agent

2KI + 2KNO 2 + 2H 2 SO 4 = I 2 + 2NO + 2K 2 SO 4 + 2H 2 O

oxidizing agent

The reaction with KI in an acidic environment is widely used in analytical chemistry for the detection of the nitrite ion NO 2 - (released free iodine forms a blue-colored compound with starch).

Most salts of nitrous acid are poisonous.

Sodium nitrite NaNO 2, which is widely used in the production of organic dyes, medicinal substances, in analytical chemistry, has the greatest application. In medical practice, used as a vasodilator in angina, as well as an antidote for cyanide poisoning.

The toxicity of nitrites when used in large quantities is due to the fact that free nitrous acid is formed in the body. Then, the conversion of blood oxyhemoglobin into methemoglobin occurs, the formation of which creates conditions for oxygen starvation of tissues, since such blood is not capable of carrying oxygen. Death from paralysis of the respiratory center can occur.

2. Nitric acid  It exhibits both the typical properties of strong inorganic acids due to the presence of a hydrogen cation in the solution, as well as the specific properties due to the oxidizing ability of the nitrate ion.

Nitric acid, as a strong inorganic acid, interacts with metal oxides, bases, salts:

2HNO 3 + CuO = Cu (NO 3) 2 + H 2 O;

2HNO 3 + Ba (OH) 2 = Ba (NO 3) 2 + 2H 2 O;

2HNO 3 + Ca CO 3 = Ca (NO 3) 2 + CO 2 + H 2 O;

2HNO 3 + Na 2 SiO 3 = 2NaNO 3 + H 2 SiO 3.

Nitric acid is a very strong oxidizing agent, as it contains a nitrogen atom in the maximum oxidation state (+5). It interacts with many simple and complex substances.

Nitric acid oxidizes almost all metals, except gold, platinum and platinum metals, as well as many non-metals and complex substances.

When heated, it decomposes:

4HNO 3 4NO 2 + 2H 2 O + O 2

When nitric acid interacts with reducing agents, hydrogen, as a rule, is not released. Nitrogen reduction to oxidation state occurs.

from +4 to -3, depending on the reaction conditions, the concentration of acid and the reducing properties of the coagent.

The lower the acid concentration and the more pronounced the reducing properties of the coagent, the deeper the reduction of nitric acid. When interacting inactive metals with concentrated nitric acid, as a rule, NO 2 is formed:

Ag + 2NNO 3 (conc) = AgNO 3 + NO 2 + H 2 O.

When inactive metals interact with dilute nitric acid, as a rule, nitric oxide (II) is formed:

3Cu + 8HNO 3 (dis) = 3Cu (NO 3) 2 + 2NO + 4H 2 O.

When nitric acid interacts with active metals, a mixture of several products of reduction is usually formed, although one of them may prevail. For example, when zinc interacts with nitric acid, the reduction product changes as the acid concentration decreases:

Concentrated nitric acid passivates iron, chromium, aluminum and some other metals, so it is transported by rail in steel and aluminum tanks.

A very concentrated (more than 60%) nitric acid reacts with non-metals, while it is reduced to NO 2 or NO:

6HNO 3 + S = H 2 SO 4 + 6NO 2 + 2H 2 O;

5HNO 3 + P = H 3 PO 4 + 5NO 2 + H 2 O;

2HNO 3 + S = H 2 SO 4 + 2NO;

5HNO 3 + 3P + 2H 2 O = 3H 3 PO 4 + 5NO

Concentrated nitric acid interacts with complex substances, oxidizing them.

A mixture of one volume of HNO 3 and three volumes of HCI is called royal vodka, since the “king of metals” - gold is dissolved in it. The total equation of this reaction

Au + HNO 3 + 4HCl = H [AuCl 4] + NO + 2H 2 O.

Being monobasic, nitric acid forms one series of salts - nitrates. All of them are well soluble in water, more stable than nitric acid, and therefore, in aqueous solutions, they almost do not possess oxidizing properties. However, when acidifying solutions, the properties of nitrates as oxidizing agents increase.

With oxidation states of +1, +2, +3, +4, +5.

Oxides N20 and N0 are non-salt-forming (what does this mean?), And the remaining oxides are acidic: N2O3 corresponds to nitrous acid HN02, and N205 corresponds to nitric acid HNO3. Nitric oxide (IV) NO2, when dissolved in water, simultaneously forms two acids — HNO2 and HNO3.

If it dissolves in water in the presence of an excess of oxygen, only nitric acid is obtained.

4N02 + 02 + 2Н20 = 4НNO3

Nitric oxide (IV) NO2 is a brown, very poisonous gas. It is easily obtained by oxidation by air of colorless non-salt-forming nitric oxide (P):

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Page 1

Oxygen nitrogen compounds serve as a vivid example of how the qualities of bodies change when their quantitative composition changes. The first is a gas, the second, at ordinary temperatures, is a solid crystalline solid.

Oxygen compounds of nitrogen exist for all its positive oxidation states from 1 to V. Nitrogenous acid H2N2O2 and its salts - hyponitrite - are very unstable when heated, have weak oxidizing and reducing properties.

Oxygen compound of nitrogen, where it exhibits the highest valence - N2Os, nitrogen pentoxide, nitrogen anhydride.

Oxygen nitrogen compounds serve as vivid examples of how the qualities of bodies change as their quantitative composition changes. The first is a gas, the second, at ordinary temperatures, is a solid crystalline solid.

Oxygen compounds of nitrogen (PG, U) in an acidic environment oxidize HoS, PHg, RI in solution to form water-soluble compounds.

Consider the oxygen compounds of nitrogen.

The ability of the oxygen compounds of nitrogen NO2X to complexate and nitrate reactions should be determined by both electrophilicity and the coordination unsaturation of the nitrogen atom. With the same coordination number, the activity is determined by electrophilicity, with the free nitronium cation ONO being the most active. Solvation greatly reduces its activity. The decrease in the selectivity of the entering nitrogroup into the nucleus with an increase in the temperature of Titov is explained by a decrease in the solvation of the nitronium cation.

The chemistry of oxygen compounds of nitrogen and phosphorus has already been considered; We now turn to the consideration of the elements of subgroups A and B. The chemistry of the oxygen compounds of vanadium, the least electropositive of all the elements of subgroup A, is in many ways similar to the chemistry of phosphorus. Since these two elements have the same coordination numbers with respect to oxygen, their oxo compounds with the same formula have similar structures and are often isomorphic to each other, and also isomorphic to the corresponding arsenic compounds. For example, dodecahydrates Na3PO4, Na3AsO4, Na3VO4, and Pb3 (PO4) C1, Pb5 (AsOJCl and Pb5 (VO4) Cl) complex salts are isomorphic. Vanadium is widely distributed in nature; it is commonly found with phosphorus in the form of vanadium (large deposits of the rare mineral patronite VSB are also a very important source of vanadium), and niobium and tantalum are commonly found together with other transition or rare earth metals. Ortho -, meta - and pyrovanadates are known, but the degree of stability of these compounds in aqueous solutions is inverse to the stability of the corresponding phosphorus s.

Oxygen compounds of nitrogen include all oxides of nitrogen, nitric and nitrous acids, and their salts.

In oxygen compounds of nitrogen per nitrogen atom accounts for from 0 5 to 3 oxygen atoms. Depending on the conditions, the nitrogen atom can attach or lose some or all of the oxygen atoms.

Like all oxygen compounds of nitrogen, its oxide is an endothermic compound, and oxygen is retained in it leprotochno. Therefore, hydrogen, coal, kerosene and other combustible substances burn in it as well as in pure oxygen, with a flame with a wide bluish halo.

Like all oxygen compounds of nitrogen, its oxide is - the compound is endothermic, the oxygen in it is held weakly. Therefore, hydrogen, coal, kerosene and other combustible substances; burn in it as well as in pure oxygen, flame, with a wide bluish halo.

Oxides and oxygen compounds of nitrogen of different degrees of oxidation are obtained by oxidation of ammonia first to nitric oxide (catalytic process), which is then easily oxidized by atmospheric oxygen to nitric acid.