Oxygen compounds of nitrogen - Hypermarket of knowledge. I Oxygen compounds of nitrogen
With degrees of oxidation +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 - nitric acid HNO3. Nitric oxide (IV) N02, when dissolved in water, simultaneously forms two acids - HNO2 and HNO3.
If it dissolves in water in the presence of excess oxygen, only nitric acid is obtained
4N02 + 02 + 2H20 = 4HNO3
Nitric oxide (IV) NO2 is a brown, very toxic gas. It is easily obtained by oxidation of colorless non-salt-forming nitric oxide (P) by atmospheric oxygen:
Contents of the lesson summary of the lesson support framework presentation of the lesson accelerative methods interactive technologies Practice tasks and exercises self-examination workshops, trainings, cases, quests homework discussion topics rhetorical questions from students Illustrations audio, video and multimedia photos, pictures graphics, tables, schemes humor, anecdotes, jokes, comics parables, sayings, crossword puzzles, quotes Additions abstracts articles of the chip for the curious cheat sheets textbooks basic and additional terms of the dictionary other Improvement of textbooks and lessons correction of errors in the textbook updating the fragment in the textbook elements of innovation in the lesson of replacing obsolete knowledge with new Only for teachers perfect lessons a calendar plan for the year, the methodological recommendations of the discussion program Integrated lessonsLaboratory and practical lesson № 21
Topic 2.1.3. The main subgroup of Group V
The topic of the lesson is "Properties of compounds of oxidized nitrogen, phosphorus and its compounds".
Objectives of the lesson:
· To improve the knowledge of the properties of oxygen-containing nitrogen and phosphorus compounds by performing exercises on the formulation 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
Performance of qualitative reactions on nitrate -, nitrite -, phosphate - ions.
· To improve the skills of drawing up the equations of redox reactions
I Theoretical part:
I Oxygen compounds of nitrogen.
1. Nitrous acid.Nitrous acid is weak, unstable, exists only in solution. When interacting with alkalis, it forms salt-nitrite.
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 oxidation-reduction 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
oxidizer
The reaction with KI in an acid medium is widely used in analytical chemistry for the detection of the NO 2 nitrite ion (the liberated iodine forms a blue-colored compound with starch).
Most salts of nitrous acid are poisonous.
The greatest use is made of sodium nitrite NaNO 2, which is widely used in the production of organic dyes, medicinal substances, in analytical chemistry. In medical practice it is used as a vasodilator for angina pectoris, and also as an antidote for cyanide poisoning.
The toxicity of nitrites when used in large quantities is due to the fact that the body produces free nitrous acid. Then, oxygen hemoglobin is converted into methemoglobin, the formation of which creates conditions for oxygen starvation of tissues, since such blood is unable to carry oxygen. Death from paralysis of the respiratory center may occur.
2. Nitric acid exhibits both the typical properties of strong inorganic acids due to the presence of 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 + CaCO 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 oxidant, since 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 reacts with reducing agents, hydrogen, as a rule, is not released. There is a reduction of nitrogen to oxidation states
from +4 to -3, depending on the reaction conditions, the acid concentration and the reducing properties of the co-reactant.
The lower the acid concentration and the more pronounced the reducing properties of the co-agent, the deeper the nitric acid is reduced. In the interaction of inactive metals with concentrated nitric acid, as a rule, NO 2:
Ag + 2NNO 3 (conc) = AgNO 3 + NO 2 + H 2 O.
In the interaction of inactive metals with dilute nitric acid, as a rule, nitric oxide (II) is formed:
3Cu + 8HNO 3 (razb) = 3Cu (NO 3) 2 + 2NO + 4H 2 O.
When nitric acid reacts with active metals, a mixture of several products of recovery is usually formed, although one of them may predominate. For example, in the interaction of zinc with nitric acid, the reduction product changes with decreasing acid concentration:
Concentrated nitric acid passivates iron, chromium, aluminum and some other metals, so it is transported by rail in steel and aluminum tanks.
With non-metals, a very concentrated (more than 60%) nitric acid reacts, 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 HCl is called royal vodka, since it dissolves the "king of metals" - gold. The total equation of this reaction
Au + HNO 3 + 4HCl = H [AuCI 4] + NO + 2H 2 O.
Being monobasic, nitric acid forms one row of salts - nitrates. All of them are highly soluble in water, more stable than nitric acid, and therefore hardly possess oxidizing properties in aqueous solutions. However, when acid solutions are acidified, the properties of nitrates as oxidants are enhanced.
Page 1
Oxygen nitrogen compounds serve as a vivid example of how the qualities of bodies change with a change in their quantitative composition. The first is gas, the second, at ordinary temperature, is a solid crystalline body.
Oxygen compounds of nitrogen exist for all of its positive oxidation degrees from 1 to V. Azotnovatistaya acid H2N2O2 and its salts - giponitrite - are very unstable when heated, have weak oxidative and reducing properties.
The oxygen compound of nitrogen, where it exhibits a higher valence - N2Os, semi-pentoxide nitrogen, nitric anhydride.
Oxygen compounds of nitrogen serve as vivid examples of how the qualities of bodies change with a change in their quantitative composition. The first is gas, the second, at ordinary temperature, is a solid crystalline body.
Oxygen compounds of nitrogen (HY, Y) in an acidic medium oxidize HoS, PHg, RI in solution to form water-soluble compounds.
Let us consider the oxygen compounds of nitrogen.
The ability of oxygen compounds of nitrogen NO2X to complex formation and the nitration reaction should be determined both by the electrophilicity and the coordination unsaturation of the nitrogen atom. With the same coordination number, the activity is determined by electrophilicity, with the most active being the free nitronium cation ONO. Solvation greatly reduces its activity. The decrease in the selectivity of the entering nitro group into the nucleus with an increase in temperature is explained by Titov by the decrease in the solvation of the nitronium cation.
The chemistry of oxygen compounds of nitrogen and phosphorus has already been considered by us; Let us now turn to the consideration of the elements of the subgroups A and B. The chemistry of the oxygen compounds of vanadium, the least electropositive of all elements of subgroup A, is in many respects similar to the chemistry of phosphorus. Since these two elements have the same coordination numbers with respect to oxygen, their oxy compounds with the same formula have similar structures and are often isomorphic to one another, as well as isomorphous to the corresponding arsenic compounds. For example, dodecahydrates Na3PO4, Na3AsO4, Na3VO4, and complex salts of Pb3 (PO4) C1, Pb5 (AsOJCl and Pb5 (VO4) Cl are isomorphic.) Vanadium is widely distributed in nature, it is usually found together with phosphorus in the form of vanadium (large deposits of the rare mineral of the patronite VSB are also a very important source of vanadium), and niobium and tantalum are usually found together with other transition or rare earth metals .Ortho, meta and pirvanadates are known, but the stability of these compounds in aqueous solutions is inverse to the stability of the corresponding phosphorus s.
Oxygen compounds of nitrogen include all nitrogen oxides, nitric and nitrous acids and their salts.
In oxygen compounds of nitrogen one atom of nitrogen accounts for from 0 to 5 oxygen atoms. Depending on the conditions, the nitrogen atom can attach or lose part or all of the oxygen atoms.
Like all oxygen compounds of nitrogen, its nitrous oxide is an endothermic compound, and oxygen in it is held leprosy. Therefore, hydrogen, coal, kerosene and other combustible substances burn in it as well as in pure oxygen, a flame with a wide bluish aureole.
Like all oxygen compounds of nitrogen, its nitrous oxide is an endothermic compound, the oxygen in it is held unstably. Therefore, hydrogen, coal, kerosene and other combustible substances; burn in it as well as in pure oxygen, flame, with a wide bluish aura.
Oxides and oxygen compounds of nitrogen of different degrees of oxidation are obtained by oxidizing ammonia first to nitric oxide (catalytic process), which is then easily oxidized by air oxygen up to nitric acid.
A summary of the chemistry lesson in the 9th grade on the topic "Oxygen compounds of nitrogen" according to the educational and methodical complex of OSGabrielyan. The work aims to consider the oxidation-connecting properties of nitrogen ions on the example of oxygen compounds. The concept contains educational, developmental, educational and health-saving tasks.
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Oxygen compounds of nitrogen.
Oxides of nitrogen. Nitrogen forms six oxygen compounds. degree of oxidation + 1 N 2 O + 2 NO + 3 N 2 O 3 + 4 NO 2, N 2 O 4 + 5 N 2 O 5
Preparation: NH 4 NO = N 2 O + 2H 2 O Chemical properties: 1. Decomposition on heating 2 N 2 + 1 O = 2 N 2 O + O 2 2. With hydrogen N 2 + O + H 2 = N 2 0 + H 2 O non-salt +1 N 2 O nitric oxide (I), nitrous oxide or "merry gas", excitably acts on the human nervous system, used in medicine as an anesthetic. Physical properties: gas, without color and odor. It shows oxidizing properties, easily decomposes.
NO +2 Preparation: 1. In nature: N 2 + O 2 = 2NO 2. In industry: 4 NH 3 + 5O 2 = 4NO + 6H 2 O Chemical properties: 1. Easily oxidized: 2 N + 2 O + O 2 = 2N +4 O 2 2. oxidizer: 2 N +2 O + 2SO 2 = 2SO 3 + N 2 0 non-salt colorless gas, thermally stable, poorly soluble in water, practically instantly reacts with oxygen (at room temperature).
N 2 O 3 +3 Chemical properties: NO 2 + NO N 2 O 3 Preparation: ALL properties of acidic oxides. acid oxide liquid is dark blue, thermally unstable, t boiling = 3.5 ° C, i.e., exists in the liquid state only upon cooling, under normal conditions it passes into a gaseous state. When reacting with water, nitrous acid forms.
NO 2 + 4 Preparation: 1. 2 NO + O 2 = 2NO 2 2. Cu + 4HNO 3 (k) = Cu (NO 3) 2 + 2NO 2 + 2H 2 O Chemical properties: 1. with water 2 NO 2 + H 2 O = HNO 3 + HNO 2 2. With alkalis 2NO 2 + 2NaOH = NaNO 3 + NaNO 2 + H 2 O 3. Dimerization of 2NO 2 N 2 O 4 is toxic nitrogen oxide (IV) or nitrogen dioxide, brown gas, good soluble in water, fully reacts with it. It is a strong oxidizing agent.
N 2 O 5 + 5 Preparation: 1. 2NO 2 + O 3 = N 2 O 5 + O 2 2. 2HNO 3 + P 2 O 5 = 2HPO 3 + N 2 O 5 Chemical properties: 1. It is easy to decompose 2N 2 O 5 = 4NO 2 + O 2 2. strong oxidizer acidic oxide nitric oxide (V), nitric anhydride, white solid (mp = 41 ° C). It shows acidic properties, it is a very strong oxidizer.
HNO 3 Composition. Structure. Properties. H O N O O - - degree of oxidation of nitrogen valence of nitrogen +5 IV chemical bond covalent polar Nitric acid - colorless hygroscopic liquid, with a sharp smell, "smoke" in the air, unlimitedly soluble in water. T melting point -41.59 ° C, boiling +82.6 ° C with partial decomposition. When stored in light, it decomposes into nitric oxide (IV), oxygen and water, acquiring a yellowish color: 4HNO 3 = 4NO 2 + O 2 + 2H 2 O Nitric acid is poisonous.
Nitric acid (HNO 3) Classification by: the presence of oxygen: basicity: solubility in water: volatility: degree of electrolytic dissociation: oxygen-containing monobasic soluble volatile strong
Production of nitric acid in industry NH 3 NO 2 HNO 3 4NH 3 + 5 O 2 = 4NO + 6H 2 O 2 NO + O 2 = 2NO 2 4 NO 2 + 2 H 2 O + O 2 = 4 HNO 3 Contact oxidation of ammonia to the oxide nitrogen (II): 2. Oxidation of nitric oxide (II) in nitric oxide (IV): 3. Adsorption (absorption) of nitric oxide (IV) by water with an excess of oxygen
In the laboratory, nitric acid is obtained by the action of concentrated sulfuric acid on nitrates with mild heating. NaNO 3 + H 2 SO 4 = NaHSO 4 + HNO 3
Chemical properties of nitric acid Nitric acid exhibits all the typical properties of acids. 1 . Properties of HNO 3 as electrolyte: 1 3 2 3 2) with basic and amphoteric oxides 3) with bases 1) Dissociation: HNO 3 = H + + NO 3 - 2HNO 3 + CuO = Cu (NO 3) 2 + H 2 O 6HNO 3 + Al 2 O 3 = 2Al (NO 3) 3 + 3H 2 O HNO 3 + NaOH = NaNO 3 + H2O 2HNO 3 + Zn (OH) 2 = Zn (NO 3) 2 + 2H 2 O 4) s salts of 2HNO 3 + Na 2 SiO 3 = H 2 SiO 3 ↓ + 2NaNO 3
2. Oxidizing properties: peculiarities of interaction with metals: (nitric acid never liberates hydrogen!) Me + HNO 3 = Me (NO 3) 2 + H 2 ↑ Metal Concentrated (\u003e 60%) Diluted (5-60%) Very dilute (
With metals standing in the row of strains to the left of hydrogen: With metals standing in the row of stresses to the right of hydrogen: Concentrated HNO 3 Dilute HNO 3 Chemical properties of nitric acid
2. Oxidizing properties 2) Features of interaction with nonmetals (S, P, C): 3) Interacts with organic substances (turpentine flashes): Chemical properties of nitric acid 3P + 5HNO 3 + H 2 O = 3H 3 PO 4 + 5NO C + 4HNO 3 = CO 2 + H 2 O + 4NO 2 5 HNO 3 + 3 P + 2 H 2 O → 3 H 3 PO 4 + 5 NO
Application of nitric acid 1 5 4 6 2 3 Production of nitrogen and complex fertilizers. Production of explosives Production of dyes Production of medicines Production of films, nitrocells, nitro-enamels Production of artificial fibers 7 As a component of a nitrating mixture for trawling metals in metallurgy
Nitrates - salts of nitric acid, are obtained by the action of acid on metals, their oxides and hydroxides. Saltpeter - salts of nitric acid and alkali metals. NaNO 3 - sodium nitrate KNO 3 - potassium nitrate NH 4 NO 3 - ammonium nitrate Ca (NO 3) 2 - calcium nitrate Properties: ALL are soluble in water.
When heated, nitrates decompose the fuller than the right in the electrochemical stress series is the metal forming the salt. Li K Ba Ca Na Mg Al Mn Zn Cr Fe Co Sn Pb Cu Ag Hg Au nitrite + O 2 metal oxide + NO 2 + O 2 Me + NO 2 + O 2 2NaNO 3 = 2NaNO 2 + O 2 2Pb (NO 3) 2 = 2PbO + 4NO 2 + O 2 2AgNO 3 = 2Ag + 2NO 2 + O 2
Nitrates are used as fertilizers. KNO 3 is used to prepare black powder.
Homework: § 26, exercise. 2.4 p. 121.
Abstract of the lesson on the topic: "Oxygen compounds of nitrogen". Grade 9
The purpose of the lesson is to study the properties of nitrogen oxides.
Tasks:
educational: to consider nitrogen oxides, and on their example to repeat the classification and the 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.
Repeat the studied material.
Several students work on cards, with the others conducted a front-line survey on the previous topic.
Didactic card number 1
a) Write the formulas for the following substances: ammonia, ammonia, ammonia
A qualitative reaction to the cation of ammonium;
Interaction of ammonium sulfate with barium chloride.
Didactic card number 2
a) Write the formulas for the following substances: ammonium dichromate, ammonia, ammonium sulfate.
b) Write the following reaction equations:
Interaction of ammonium chloride with silver nitrate;
Interaction of ammonium carbonate with hydrochloric acid.
Frontal survey:
1) What is "ammonia"? What is it used for?
2) What properties of ammonia are the basis of 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. Knowledge updating.
Arrange oxidation states in nitrogen oxides:
N 2 O NO 2 O 3 NO 2 N 2 O 5
Learning new material.
The teacher reports the topic, purpose and plan of the lesson.
Plan:
Classification of nitrogen oxides.
The student's message 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 application of nitrogen oxides, (story and explanation of the teacher).
Classification of nitrogen oxides. Students complete the scheme with the teacher.
ABOUT 
ksidy nitrogen
Nonsoluble Salts
N 2 O NO N 2 O 3 → HNO 2
do not interact with acids, N 2 O 5 → HNO 3
neither with alkalis nor form salts of NO 2 → HNO 2 and HNO 3
Student Report on the topic: "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 weak pleasant smell. Wodehouse suddenly became cheerful, and he started to dance, singing songs. The next day, returning to the laboratory, he found crystals of sodium thiosulfate Na 2 S 2 O 3 in the flask where the experiment was going on. Almost at the same time, the English chemist Gemfri Devi carried out the thermal decomposition of NH 4 NO 3 ammonium nitrate. As he recalled later, the assistant was too close to the installation and several times he inhaled a gas with a pleasant smell coming from the retort. Suddenly, the assistant burst into an unreasonable laugh, and then fell in the corner of the room and immediately fell asleep.
Scientists have received the same gas - nitric oxide (I) N 2 O.
The oxide formula
Physical properties
Chemical properties
Preparation and application
N 2 O
colorless incombustible with pleasant sweetish and.
2N 2 O → 2N 2 + O 2
NH 4 NO 3 → N 2 O + 2H 2 O
Small concentrations of nitrous oxide cause an easy(hence the name - "laughing gas"). When inhaled, pure gas rapidly develops intoxication and drowsiness. Nitrous oxide has a weak narcotic activity, in connection with which in medicine it is used in high concentrations.
colorless gas, poorly soluble in water.
2NO + O2 → 2NO2
4 NH 3 + 5O 2 → 4NO + 6H 2 O
The production of NO is one of the production steps.
NO 2
Poisonous gas, red-brown color, with a characteristic acute smell or a 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 oxidizer in a liquidand blended explosives.It is highly toxic. It irritates the respiratory tract, in high concentrations causesNO + NO 2 = N 2 O 3
It is used in the laboratory to produce nitrous acid and its salts. It is highly toxic. By action 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 = 2H N O 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.Zakreplenie. Ex.6
5. Reflection, summing up. Estimates.
6. Homework §26.
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