Nitrogen compounds. Oxygen compounds of nitrogen Nitric acid. HNO3

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= N 2 O + Cu=

Nitrogen oxide (III) N 2 O 3 – nitrogen oxide (III) is a dark blue liquid, thermally unstable, boiling point = 3.5 0C, that is, it exists in a liquid state only when cooled, under normal conditions it turns into gaseous state. An acidic oxide that reacts with water to form nitrous acid. N 2 O 3 = N 2 O 3 + H 2 O =

Nitric acid. HNO 3 Nitric acid is a colorless hygroscopic liquid, has a pungent odor, “smoke” in air, is indefinitely soluble in water, boiling point = C. Solutions of nitric acid are stored in a dark glass jar, i.e. it decomposes in light: 4HNO 3 = 4NO 2 +2H 2 O+O 2

Slide 1

NITROGEN compounds Material for repetition and preparation for the GIA Chemistry teacher of the Municipal Educational Institution “Gymnasium No. 1” Saratova Shishkina I.Yu.

Slide 2

Nitrogen forms several strong compounds with hydrogen, the most important of which is ammonia. The electronic formula of the ammonia molecule is: Preparation of ammonia. In the laboratory: 2NH4Cl + Ca (OH)2 = CaCl2 + 2NH3 + 2H2O In industry: N2 + 3H2 2NH3 + 92 kJ

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Chemical properties 1. Ammonia is a strong reducing agent. 3Cu+2O + 2N-3H3 = 3Cu0 + N20 + 3H2O 2N-3 – 6e = N 2 Cu2+ + 2e = Cu 3 4NH3 + 3O2 = 2N2 + 6H2O In the presence of a catalyst, chromium (III) oxide, the reaction proceeds with the formation of nitrogen oxide (II) and water: Cr2O3 4NH3 + 5O2 = 4NO + 6H2O Reduction of metals from their oxides:

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Ammonia interacts with potassium permanganate: NH3 + KMnO4 = N2 + H2O + MnO2 +KOH Interaction with halogens: 2NH3 + 3Br2 = 6HBr + N2 2NH3 + 3Cl2 = 6HCl + N2 Adding ammonia changes the color of the solution:

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2. formation of ammonium salts. Reactions with the formation of donor-acceptor bonds. NH3 + H2O NH3 . H2O NH4+ + OH- NH4OH NH4+ + OH- H NH3 + H+Cl- [ H N H ]+ Cl- H

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ammonium salts Ammonium salts are obtained by reacting ammonia or its aqueous solutions with acids. NH3 + HNO3 = NH4NO3 NH3H2O + HNO3 = NH4NO3 + H2O Ammonium salts react with solutions of alkalis, acids and other salts: (NH4)Cl + NaOH = NaCl + H2O + NH3 CONC. 2NH4Cl + H2SO4 = (NH4)2SO4 + 2HCl (NH4)2SO4 + BaCl2 = 2NH4Cl + BaSO4

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All ammonium salts decompose when heated. (NH4)2CO3 = 2NH3 + H2O CO2 NH4NO2 = 2H2O + N2 NH4Cl NH3 + HCl (NH4)2Cr2O7 = Cr2O3 + 4H2O + N2 salts of volatile acids salts of oxidizing acids

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Qualitative reaction to ammonium ion. NH4+ + OH- H2O + NH3 A very important property of ammonium salts is their interaction with alkali solutions

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Nitrogen oxides. Nitrogen forms six oxygen compounds. oxidation states +1 N2O +2 NO +3 N2O3 +4 NO2, N2O4 +5 N2O5

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N2O Preparation: NH4NO = N2O +2H2O Chemical properties: 1. decomposition by heating 2N2+1O = 2N20+O2 2. with hydrogen N2+1O +H2 = N20 +H2O non-salting +1

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N2O3 +3 Chemical properties: NO2 + NO N2O3 Preparation: ALL properties of acid oxides. acid oxide

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N2O5 +5 Preparation: 1. 2NO2 + O3 = N2O5 + O2 2. 2HNO3 + P2O5 = 2HPO3 + N2O5 Chemical properties: 1. easily decomposes 2N2O5 = 4NO2 + O2 2. strong oxidizing agent acid oxide

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Nitric acid. Preparation of nitric acid: KNO3 + H2SO4 = HNO3 + KHSO4 In the laboratory, with low heating: In industry, the process of producing nitric acid can be divided into three stages: 1. Oxidation of ammonia on a platinum catalyst to NO: 4NH3 + 5O2 = 4NO + 6H2O 2. Oxidation air oxygen NO to NO2: 2NO + O2 = 2NO2 3. Absorption of NO2 by water in the presence of excess oxygen: 4NO2 + 2H2O + O2 = 4HNO3

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HNO3 diluted concentrated alkali and alkaline earth Fe, Su heavy metals NH4NO NH3 NO alkali and alkaline earth heavy metals N2O NO2 Fe Cr Au Al Pt passivates does not interact

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Dilute nitric acid. Concentrated nitric acid. Ag + 2HNO3 = AgNO3 + NO2 H2O 3Ag + 4HNO3 = 3AgNO3 + NO + 2H2O 4Zn + 10HNO3 (very dilute) = 4Zn(NO3)2 + NH4NO3 + 3H2O

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Nitric acid reacts with many non-metals, oxidizing them to the corresponding acids: 3P + 5HNO3 + H2O = 3H3PO4 + 5NO C + 4HNO3 = CO2 + H2O + 4NO2

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Nitrates are salts of nitric acid, obtained by the action of acid on metals, their oxides and hydroxides. Nitrate is a salt of nitric acid and alkali metals. NaNO3 – sodium nitrate KNO3 – potassium nitrate NH4NO3 – ammonium nitrate Ca(NO3)2 – calcium nitrate Properties: ALL are soluble in water.

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When heated, nitrates decompose with the release of oxygen (O2) t MeNO3 MeNO2 + O2 t MeNO3 MeO + NO2 + O2 t MeNO3 Me + NO2 + O2 to Mg from Mg to Pb after Cu

Slide 21

Nitrate is used as fertilizer. KNO3 is used to prepare black powder.

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1 Ammonia under normal conditions is... 1) a colorless, odorless gas 2) a brown, pungent-smelling gas 3) a colorless, pungent-smelling gas 4) a colorless liquid Tests: 2 Does not interact with concentrated nitric acid... 1) Hg 2) Al 3) Cu 4) Zn 3 In industry, nitric acid is obtained by the reaction: 1) NaNO3(K) + H2SO4(K) = NaHSO4 + HNO3 2) Ba(NO3)2 + H2SO4 = BaSO4 + 2HNO3 3) 4NO2 + O2 + 2H2O = 4HNO3 4) N2O5 + H2O = 2HNO3 4 Ammonium salts react with alkalis, since in this case... 1) a weak base is formed, ammonium hydroxide 2) ammonia gas is released 3) a new salt is formed 4) a weak base is formed and a gas is released 5 Coefficient in front of the salt formula in the reaction equation Mg + HNO3 NO + … + H2O is equal to... 1)3 2)4 3)6 4)8 6 When silver nitrate was added to a solution of some mineral fertilizer, a white precipitate formed. This fertilizer... 1) calcium nitrate 2) potassium nitrate 3) ammonium nitrate 4) sylvinite 7 is the weakest of the acids, the formula of which is HNO3 2) H2SiO3 3) H2SO3 4) H3PO4 8 nitric acid corresponds to the oxide... 1) N2O 2) NO 3) NO2 4)N2O5 9 of the listed chemical elements has the greatest electronegativity in compounds: 1) Be 2)B 3) S 4)N 10 complete the phrase “saltpeter is …” I option

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Option II 1 nitric acid is a strong acid, since it... 1) is completely dissociated in an aqueous solution 2) even dissolves silver 3) a strong oxidizing agent 4) highly soluble in water 6 Poorly soluble in water mineral fertilizer... 1) ammonium chloride 2) potassium nitrate 3) sylvinite 4) superphosphate 4 ammonium salts in relation to water... 1) highly soluble 2) poorly soluble 3) insoluble 4) there are soluble and insoluble 3 ammonia is produced in industry... 1) N2 + 3H2 2NH3 2) 4NO2 + O2 + 2H2O = 4HNO3 3) N2O5 + H2O = 2HNO3 4) NaNO3(K) + H2SO4(K) = NaHSO4 + HNO3 8 nitric acid corresponds to the oxide... 1) N2O 2) NO 3)NO2 4)N2O5 5 coefficient in front of the formula of the reducing agent in the reaction equation Zn + HNO3 N2O +... + H2O is equal to 1) 1 2) 2 3) 3 4) 4 2 the minimum degree of oxidation of nitrogen in the compound... 1) N2 2) NO 3) NO2 4) HNO3 7 the weakest of the acids, formula of which HNO3 2) H2SO4 3) H2CO3 4) H3SiO3 9 of the listed chemical elements has the greatest electronegativity in compounds: 1) B 2)P 3)N 4)F 10 complete the phrase “nitrates are …”

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1. Calculate the mass of ammonia required to produce 200 kg of nitric acid with a mass fraction of HNO3 of 60%. When calculating, keep in mind that the mass fraction of the final product yield during synthesis is 80%. Problems: 2. When sodium nitrate was heated, oxygen with a volume of 280 ml was formed (normal conditions). What mass of salt has undergone decomposition? 3. Calculate the mass of calcium(II) hydroxide, which can be neutralized with a 630 g solution of nitric acid, in which the mass fraction of HNO3 is 20% 4. By passing excess ammonia through a solution weighing 600 g with a mass fraction of nitric acid of 42%, ammonium nitrate is obtained weighing 300 g. Determine the mass fraction of ammonium nitrate yield. 5. A 75 g mixture of copper and copper (II) oxide was exposed to excess HNO3 (concentrated). In this case, a gas with a volume of 26.88 liters was formed (normal conditions). Determine the mass fraction of copper(II) oxide in the initial mixture. 6. Ammonia with a volume of 7.84 L (normal conditions) was subjected to catalytic oxidation and further conversion to nitric acid. As a result, a solution weighing 200 g was obtained. Assuming the yield of HNO3 to be 40%, determine its mass fraction in the resulting solution.

Nitric oxide (I) N2O

N2O – nitric oxide (I), nitrous oxide
or "laughing gas"
has a stimulating effect on
human nervous system,
used in medicine as
anesthetic.
Physical properties: gas, without
color and smell. Shows
oxidizing properties, easy
decomposes. Non-salt-forming
oxide.
2N2O=2N2 + O2

Nitric oxide (II)

NO – nitric oxide (I I)
colorless gas, thermal
stable, poorly soluble in
water, almost instantly
interacts with oxygen
(at room temperature).
Non-salt-forming oxide.
2NO+ O2= 2NO2

Nitric oxide (III)

N2O3 – nitrogen oxide (III) liquid
dark blue, thermal
unstable, boiling point = 3.5 0C, i.e.
exists in a liquid state
only when cooling, in normal
conditions turns into gaseous
state. Acid oxide, at
interaction with water is formed
nitrous acid.
N2O3 + H2O = 2HNO2

Nitric oxide (IV)

NO2 – nitrogen oxide (IV) or dioxide
nitrogen, brown gas, highly soluble
in water, completely reacts with it.
Is a strong oxidizing agent.
2NO2 + H2O = HNO2 + HNO3
Disproportionation reaction
Shows all properties
acid oxides

Nitric oxide (V)

N2O5 – oxide
nitrogen (V),
nitric
anhydride, white
hard
substance (tmelt=
410С). Shows
acidic
properties, is
very strong
oxidizing agent.
The product of the reaction between
acidic
oxide and water is
acid

Nitric acid. HNO3

Nitrogen
4HNO3=4NO2+2H2O+O2
acid
–
colorless
hygroscopic
liquid, has a sharp
smell,
"smoke"
on
air, unlimited
dissolves in water,
tboil= 82.6 0С. Solutions
nitric acid is stored
in a dark jar
glass,
T.
e.
she
decomposes in the light:

Compound. Structure. Properties.
HNO3
H-O-N
O
O
nitrogen oxidation state
nitrogen valence IV
+5
chemical bond
covalent polar

Nitric acid (HNO3)
Classification
Nitric acid according to:
presence of oxygen:
oxygen-containing
basicity:
solubility in water:
monobasic
soluble
volatility:
volatile
degree of electrolytic dissociation:
strong

Production of nitric acid in industry
NH3
NO
NO2
1. Contact oxidation of ammonia to
nitric oxide (II):
4NH3+ 5O2 = 4NO + 6H2O
2. Oxidation of nitric oxide (II) into oxide
nitrogen(IV):
2NO+O2 = 2NO2
3. Adsorption (absorption) of oxide
nitrogen (IV) with water in excess of oxygen
4NO2 + 2H2O + O2 = 4HNO3
HNO3

In the laboratory, nitric acid is prepared by
concentrated sulfuric acid for nitrates at
low heat.
Write an equation for the reaction to produce nitric acid.
NaNO3 + H2SO4 = NaHSO4 + HNO3

1. Typical properties of acids
2. Interaction of nitric acid with metals
3. Interaction of nitric acid with non-metals

Chemical properties of nitric acid
Nitric acid exhibits all the typical properties of acids.
List the properties characteristic of acids.
Acids interact with basic and amphoteric
oxides, with bases, amphoteric hydroxides, with
salts.
Write down the reaction equations for nitric acid:
1 with copper (II) oxide, aluminum oxide;
2 with sodium hydroxide, zinc hydroxide;
3
with ammonium carbonate, sodium silicate.
Consider the reactions from a perspective. TED.
Give names to the resulting substances. Define the type
reactions.

1
2HNO3 + CuO = Cu(NO3)2 + H2O
2H+ + 2NO3– + CuO = Cu2+ + 2NO3– + H2O
2H+ + CuO = Cu2+ + H2O
6HNO3 + Al2O3 = 2Al(NO3)3 + 3H2O
6H+ + 6NO3– + Al2O3 = 2Al3+ + 6NO3– + 3H2O
6H+ + Al2O3 = 2Al3+ + 3H2O
2
HNO3 + NaOH = NaNO3 + H2O
H+ + NO3– + Na+ + OH– = Na+ + NO3– + H2O
H+ + OH– = H2O
2HNO3 + Zn(OH)2 = Zn(NO3)2 + 2H2O
2H+ + 2NO3– + Zn(OH)2 = Zn2+ +2NO3– + 2H2O
2H+ + Zn(OH)2 = Zn2+ + 2H2O

3
2HNO3 + (NH4)2CO3 = 2NH4NO3 + CO2 + H2O
2H+ + 2NO3– + 2NH4+ + CO22– = 2NH4+ +2NO3– + CO2 + H2O
2H+ + CO22– = CO2 + H2O
2HNO3 + Na2SiO3 = ↓H2SiO3 + 2NaNO3
2H+ + 2NO3– + 2Na+ + SiO32– = ↓H2SiO3 + 2Na+ + 2NO3–
2H+ + SiO32– = ↓H2SiO3
Active acids displace weak volatile or
insoluble acids from salt solutions.

Reaction of nitric acid with metals
How do metals react with acid solutions?
Metals,
standing
in the line of activity
to acid
hydrogen,
are crowding out
Peculiarities
interactions
nitrogen
with metals:
his
isodine
acids
Metals,
standing
after hydrogen
acids it
1. Neither
metal
never
doesn't highlight
from nitric acid
Not
are crowding out
those. don't interact
with acids,
Not
hydrogen.
Stand out
various connections
nitrogen:
dissolve
them. N2+1O, N20,
N+4O2, N+2вO,
N–3H3 (NH4NO3)
N–3H4+
N20
N2+1O
N+2O
N+4O2
acid concentration
metal activity
2. Metals upstream and downstream react with nitric acid.
after hydrogen in the activity series.
experience
experience
3. Nitric acid does not interact with Au, Pt
4. Concentrated nitric acid passivates metals:
Al, Fe, Be, Cr, Ni, Pb and others (due to the formation of dense
oxide film). When heated and when diluted with nitrogen
acids and metals dissolve in it.
experience

Write down the reaction equation for the interaction of concentrated
nitric acid with mercury. Consider the reaction from a perspective. OVR.
4HN+5O3 + Hg0 = Hg+2(NO3)2 + 2N+4O2 + 2H2O
N+5 + 1e → N+4 1 2
Hg0 – 2e → Hg+2 2 1
HNO3 (due to N+5) – oxidizing agent, reduction process;
Hg0 – reducing agent, oxidation process.

Complete the reaction schemes:
1)
HNO3(conc.) + Cu → Cu(NO3)2 + … + H2O
2)
HNO3(dil.) + Cu → Cu(NO3)2 + … + H2O
Consider transformations in the light of OVR
1) 4HN+5O3(conc.) + Cu0 = Cu+2(NO3)2 + 2 N+4O2 + 2 H2O
oxidizer
reducing agent
N+5 + 1e → N+4 1 2
Cu0 – 2e → Cu+2 2 1
recovery
oxidation
2) 8 HN+5O3(conc.) + 3 Cu0 = 3Cu+2(NO3)2 + 2 N+2O + 4 H2O
oxidizer
reducing agent
N+5 + 3e → N+2 3 2
Cu0 – 2e → Cu+2 2 3
recovery
oxidation

Interaction of nitric acid with non-metals
Nitric acid as a strong oxidizing agent
Oxidizes non-metals to the corresponding acids.
Concentrated (more than 60%) nitric acid is reduced to
NO2, and if the acid concentration is (15 - 20%), then to NO.
Arrange the coefficients in the diagrams using the electronic balance method.
4 HNO3 + C → CO2 + 2 H2O + 4 NO2
N+5 + 1e → N+4 1 4
С0 – 4e → С+4 4 1
experience
HNO3 (due to N+5) – oxidizing agent, reduction potential
C – reducing agent, oxidation process
5 HNO3 + P → H3PO4 + 5 NO2 + H2O
experience
N+5 + 1e → N+4 1 5 HNO3 (due to N+5) – oxidizing agent, reduction process
P – reducing agent, oxidation process
P0 – 5e → P+5 5 1
5 HNO3 + 3 P + 2 H2O → 3 H3PO4 + 5 NO
N+5 + 3e → N+2 3 5 HNO3 (due to N+5) – oxidizing agent, reduction process
P0 – 5e → P+5 5 3 P – reducing agent, oxidation process

Application of nitric acid
1
Production of nitrogen and complex
fertilizers
2
Production of explosives
3
Dye production
4
Medicine production
5
Film production,
nitro varnishes, nitro enamels
6
Production
artificial fibers
7
As a nitrating component
mixtures, for trawling
metals in metallurgy

Nitric acid salts
What are the salts of nitric acid called?
nitrates
Nitrates K, Na, NH4+ are called nitrates
Make up formulas for the listed salts.
KNO3
NaNO3
NH4NO3
Nitrates – white crystalline
substances. Strong electrolytes, in
solutions completely dissociate
to ions. They enter into exchange reactions.
How can you determine the nitrate ion in solution?
Sulfuric acid is added to the salt (containing nitrate ion).
acid and copper. The mixture is slightly heated. Selection
brown gas (NO2) indicates the presence of nitrate ion.

Potassium nitrate (potassium nitrate)
Colorless crystals Significantly
less hygroscopic compared to
sodium, therefore it is widely used in pyrotechnics as an oxidizing agent.
When heated above 334.5ºС
melts above this temperature
decomposes releasing oxygen.
Sodium nitrate
Used as fertilizer; V
glass,
metalworking industry; for getting
explosives
substances
missile
fuels and pyrotechnic mixtures.

Ammonium nitrate
Crystalline
substance
white
colors. Melting point 169.6 °C,
when heated above this temperature
gradual
decomposition
substances, and at a temperature of 210°C
complete decomposition occurs.

When heated, nitrates decompose more completely, the more
to the right in the electrochemical series of voltages is metal,
forming salt.
Li K Ba Ca Na
Mg Al Mn Zn Cr Fe Co Sn Pb Cu
nitrite + O2
metal oxide + NO2 + O2
Ag Hg Au
Me + NO2 + O2
Write down the reaction equations for the decomposition of nitrate
sodium, lead nitrate, silver nitrate.
2NaNO3 = 2NaNO2 + O2
2Pb(NO3)2= 2PbO + 4NO2 + O2
2AgNO3 = 2Ag + 2NO2 + O2

Application of nitric acid.

Plastics
Dyes
Fertilizers
Explosives
Medicines

Summary of a chemistry lesson in the 9th grade on the topic "Oxygen compounds of nitrogen" according to the educational and methodological complex of O.S. Gabrielyan. The work aims to consider the oxidative-connective properties of nitrogen ions using the example of oxygen compounds. The abstract contains educational, developmental, educational and health-preserving tasks.

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Oxygen compounds of nitrogen.

Nitrogen oxides. Nitrogen forms six oxygen compounds. oxidation states + 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 when heating 2 N 2 +1 O = 2 N 2 0 + O 2 2. with hydrogen N 2 +1 O + H 2 = N 2 0 + H 2 O non-salt-forming +1 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.

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. oxidizing agent: 2 N +2 O + 2SO 2 = 2SO 3 +N 2 0 non-salt-forming colorless gas, thermally stable, poorly soluble in water, reacts almost instantly with oxygen (at room temperature).

N 2 O 3 +3 Chemical properties: NO 2 + NO N 2 O 3 Preparation: ALL properties of acid oxides. acid oxide is a dark blue liquid, thermally unstable, boiling point = 3.5 0C, i.e. it exists in a liquid state only when cooled, under normal conditions it turns into a gaseous state. When interacting with water, nitrous acid is formed.

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 2NO 2 N 2 O 4 toxic nitric oxide (IV) or nitrogen dioxide, brown gas, good soluble in water, completely reacts with 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. easily decomposes 2N 2 O 5 = 4NO 2 + O 2 2. strong oxidizing agent, acidic oxide, nitric oxide (V), nitric anhydride, white solid (melting point = 41 0 C). It exhibits acidic properties and is a very strong oxidizing agent.

HNO 3 Composition. Structure. Properties. H O N O O - - degree of oxidation of nitrogen nitrogen valence +5 IV chemical bond covalent polar Nitric acid is a colorless hygroscopic liquid, with a pungent odor, “smoke” in air, unlimitedly soluble in water. Melting point −41.59 °C, boiling point +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 according to: 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 NO 2 HNO 3 4NH 3 + 5O 2 = 4NO + 6H 2 O 2NO+O 2 = 2NO 2 4 NO 2 + 2 H 2 O + O 2 = 4 HNO 3 Contact oxidation of ammonia to oxide nitrogen (II): 2. Oxidation of nitric oxide (II) to nitric oxide (IV): 3. Adsorption (absorption) of nitric oxide (IV) by water in excess of oxygen

In the laboratory, nitric acid is prepared by reacting concentrated sulfuric acid with nitrates under low heat. 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 an 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 + H 2 O 2HNO 3 + Zn(OH) 2 = Zn(NO 3) 2 + 2H 2 O 4) s salts 2HNO 3 + Na 2 SiO 3 = H 2 SiO 3 ↓ + 2NaNO 3

2. Oxidizing properties: features of interaction with metals: (nitric acid never releases hydrogen!) Me + HNO 3 = Me(NO 3) 2 + H 2 ￪ Metal Concentrated (> 60%) Dilute (5-60%) Very diluted (

With metals in the voltage series to the left of hydrogen: With metals in the voltage series to the right of hydrogen: Concentrated HNO 3 Dilute HNO 3 Chemical properties of nitric acid

2. Oxidizing properties 2) Features of interaction with non-metals (S, P, C): 3) Interacts with organic substances (turpentine flares up): 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 drugs Production of films, nitro-varnishes, nitro-enamels Production of artificial fibers 7 As a component of a nitrating mixture, for trawling metals in metallurgy

Nitrates are salts of nitric acid, obtained by the action of acid on metals, their oxides and hydroxides. Nitrate is a salt 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 more completely the more to the right the metal forming the salt is in the electrochemical voltage series. 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

Nitrate is used as fertilizer. KNO 3 is used to prepare black powder.

Homework: § 26, ex. 2.4 p. 121.