HISTORICAL BACKGROUND Ammonia was first obtained in its pure form in 1774 by the English chemist Joseph Priestley. In 1784, the French chemist Claude Louis Berthollet decomposed ammonia into elements using an electric discharge and thus established the composition of this gas, which in 1787 received the official name "ammoniac" - from the Latin name for ammonia - sal ammoniac; this salt was obtained near the temple of the god Amun in Egypt. Joseph Priestley Claude Louis Berthollet

HISTORICAL SUMMARY This name is still preserved in most Western European languages ​​(German Ammoniak, English ammonia, French ammoniaque); the abbreviated name "ammonia" that we use was introduced in 1801 by the Russian chemist Yakov Dmitrievich Zakharov, who first developed the system of Russian chemical nomenclature. Oasis of Ammon in North Africa Remains of the Temple of Ammon

The pungent smell of ammonia has been known to man since prehistoric times, since this gas is formed in significant quantities during the decay, decomposition and dry distillation of organic compounds containing nitrogen, such as urea or proteins. It is possible that in the early stages of the Earth's evolution there was quite a lot of ammonia in its atmosphere. Even now, however, minute amounts of this gas can always be found in the air and in rainwater, since it is continuously formed during the decomposition of animal and vegetable proteins. On some planets solar system the situation is different: astronomers believe that a significant part of the masses of Jupiter and Saturn falls on solid ammonia. HISTORY REFERENCE

STRUCTURE OF THE AMMONIA MOLECULE Nitrogen is a more electronegative element than hydrogen, therefore, when a bond is formed N-H common electron pairs "shift" to the nitrogen atom. Each N-H bond becomes polar, so the ammonia molecule as a whole is polar. Another thing is clear from the electronic formula: the nitrogen atom has a free (lone) pair of electrons. This further increases the polarity of the ammonia molecule and determines many of the properties of ammonia.

PHYSICAL PROPERTIES OF AMMONIA colorless gas has a pungent odor pungent taste 1.7 times lighter than air at T = -33.4 0 C liquefies at T = - 77.7 0 C solidifies dissolves in alcohols, benzene, acetone is highly soluble in water ( in 1 V of water - 700 V of ammonia) Solubility of ammonia in water H2OH2O NH3

PHYSIOLOGICAL EFFECTS ON THE HUMAN BODY According to the physiological effect on the body, it belongs to the group of substances with an asphyxiant and neurotropic effect, capable of causing toxic pulmonary edema and severe injury in case of inhalation damage. nervous system. Ammonia vapor strongly irritates the mucous membranes of the eyes and respiratory organs, as well as the skin. This is what we perceive as a pungent smell. Ammonia vapors cause profuse lacrimation, pain in the eyes, chemical burns of the conjunctiva and cornea, loss of vision, coughing fits, redness and itching of the skin. When liquefied ammonia and its solutions come into contact with the skin, a burning sensation occurs, a chemical burn with blisters and ulcerations is possible. In addition, liquefied ammonia absorbs heat during evaporation, and frostbite of varying degrees occurs when it comes into contact with the skin.

CHEMICAL PROPERTIES OF AMMONIA (associated with changes in nitrogen oxidation state) 1. Decomposition of ammonia: ? N -3 H 3 + \u003d N? H Combustion of ammonia: ? N-3H? O 2 0 = ? N? H 2 O -2 + Q 3. Catalytic oxidation of ammonia: ? N-3H? O 2 0 = ? N+2O+? H 2 O -2 + Q Combustion of ammonia in oxygen Task: draw up an electronic balance, indicate the oxidizing agent / reducing agent, the process of oxidation / reducing agent NH 4 Cl, Ca (OH) 2 KMnO 4 O2O2 NH3

CHECK YOURSELF! 1) 2 N -3 H 3 + \u003d N H N e \u003d N oxidation / reducing agent 3 2H + + 2e \u003d H 2 0 - reduction / oxidizing agent 2) 4 N -3 H O 2 0 \u003d 2 N H 2 O -2 + Q 2 2N e \u003d N oxidation / reducing agent 3 O e \u003d 2O -2 - reduction / oxidizing agent 3) 4 N -3 H O 2 0 \u003d 4 N +2 O + 6 H 2 O -2 + Q 4 N e \u003d N +2 - oxidation / reducing agent 5 О e \u003d 2О -2 - reduction / oxidizing agent

CHEMICAL PROPERTIES OF AMMONIA (associated with the features of the covalent polar bond in the ammonia molecule) 1) Interaction with water: .. NH3 + HOH NH 4 OH 2) Interaction with acids: .. NH3 + HCl NH 4 Cl Ammonium hydroxide or "ammonia chloride" Chloride ammonium or "ammonia", "smelling salt" Conclusion: ammonia has basic (alkaline) properties

AMMONIA PRODUCTION To obtain ammonia in the laboratory, the action of strong alkalis on ammonium salts is used: NH 4 Cl + NaOH \u003d NH 3 + NaCl + H 2 O. The industrial method for obtaining ammonia is based on the direct interaction of hydrogen and nitrogen: N 2 (g) + 3H 2 (d) 2NH 3 (g) + 45.9 kJ This is the so-called Haber process (German physicist, developed the physicochemical basis of the method). NH 4 Cl, Ca(OH) 2 NH3

AMMONIA APPLICATION Used for production nitrogen fertilizers(ammonium nitrate and sulfate, urea), explosives and polymers, nitric acid, soda (ammonia method) and other products of the chemical industry. Liquid ammonia is used as a solvent. In refrigeration, it is used as a refrigerant.

APPLICATION OF AMMONIA In medicine, a 10% solution of ammonia, often called ammonia, is used for fainting (to stimulate breathing), to stimulate vomiting, as well as external neuralgia, myositis, insect bites, and treatment of the surgeon's hands. To excite breathing and bring the patient out of fainting, a small piece of gauze or cotton wool moistened with ammonia is carefully brought to the patient's nose (for 0.5–1 s). The physiological effect of ammonia is due to the pungent smell of ammonia, which irritates specific receptors of the nasal mucosa and excites the respiratory and vasomotor centers of the brain, causing increased breathing and increased blood pressure.

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Ammonia

Tasks to repeat

• Carry out a chain of transformations:
• N 2 →Li 3 N→NH 3 →NO→NO 2 →HNO 3

• Determine the coefficients in the reaction equation using the electron balance method:
• Determine the coefficients in the reaction equation using the electron balance method:

• NH 3 + O 2 → NO + H 2 O
• NH 3 + O 2 → N 2 + H 2 O

This story took place during World War I.

The structure of ammonia

(NH 3 )

+7 N ))

+1 h)

Physical Properties

• Ammonia - this is colorless gas with sharp smell, 2 times lighter than air .

• Ammonia should not be inhaled for a long time, because. he poisonous.
• It liquefies easily.
• On contact with the skin, frostbite of varying degrees occurs.
• T pl = -78 0 FROM
• Highly soluble in water:

a) 25% solution - aqueous ammonia (ammonia water)

B) 10% solution - ammonia.

T kip = -33,5 0 FROM

Chemical properties

• According to the donor-acceptor mechanism:

A) Interaction with acids:

NH 3 + HCl \u003d NH 4 Cl

:NH 3 +□H + = NH 4 +

B) Interaction with water:

NH 3 + H 2 O ↔ NH 4 OH

ACCEPTOR

DONOR

Chemical properties

2) Interaction with metals:

2NH 3 + Na \u003d NaNH 2 + H 2

2NH 3 + O 2 \u003d 2H 2 O + N 2

2NH 3 + 3Br 2 \u003d 6HBr + N 2

Ammonia production

1) Industrial: synthesis from nitrogen and hydrogen:

N 2 + 3H 2 ↔2NH 3

2) Laboratory:

Ca (OH) 2 + NH 4 Cl \u003d CaCl 2 + NH 3 + 2H 2 O

Receipt

In the laboratory

NH 3

NH 4 Cl

Ca(OH) 2

Application

Production of nitrogen

In refrigeration

installations.

In medicine,

for soldering

Production

fertilizer

Production

explosive

Check of knowledge

1. What is the oxidation state of nitrogen in ammonium nitrate?

2. Write the chemical equations for the following transformations:

nitrogen→ammonia→ammonium chloride

3. Additional task: Determine the coefficients in the following diagram chemical reaction using the electronic balance method:

Cu + NH 3 → N 2 + Cu + H 2 O

Homework

• THE PURPOSE OF THE LESSON:
• study of the structure of the ammonia molecule, its physical and chemical properties;
• determination of the role of ammonia and its derivatives in human life, their application;

• From the history of chemical names.
• The structure of the ammonia molecule.
• Physical properties of ammonia. Action on the body. Rules for handling ammonia.
• Chemical properties of ammonia.
• Methods for obtaining ammonia in the laboratory and in industry.
• The use of ammonia in the areas of the national economy.
• Environmental problems associated with ammonia leakage.

God Amon in the form of a ram

8th century BC. (Museum of Meroe, Sudan)

The structure of the nitrogen atom looks like this: +7))

The electronic formula is: 1S22S22P3

Conclusion. The presence of an unshared electron pair on the nitrogen atom and the presence of three polar covalent bonds in the ammonia molecule will contribute to the fact that it will enter into reactions of the addition of the hydrogen proton H +, that is, react with water and with acid solutions that have hydrogen protons. The presence of a hydrogen bond in the ammonia molecule explains its dissolution in water, and the easy liquefaction of this gas.

Ammonia is a colorless gas

with a pungent odor

liquefies at -33.35 °С,

hardens at -77.7 °C.

at a pressure of 9 105 Pa, it liquefies already at room temperature,

highly soluble in water, at 20 °C 700 volumes of ammonia dissolve in 1 volume of water,

It also dissolves well in alcohols and acetone.

In addition, liquefied ammonia absorbs heat during evaporation,

on contact with the skin, frostbite of varying degrees occurs.

physical properties

Structure

with characteristic

lighter than air

Highly soluble in water

Molecular

crystalline

PHYSICAL PROPERTIES OF AMMONIA

1. Interaction with water. The effect of an aqueous solution of ammonia on indicators. 2. Interaction with acids 3. Oxidation:

• without catalyst;
• with catalyst;
4. With salts to form a complex compound

H2O in 1 liter will dissolve 700 liters of ammonia

The dissolution of ammonia in water and in acids is a chemical process based on the ability of ammonia molecules to bind hydrogen ions. The reason for this is the presence of a free electron pair at the nitrogen atom, which “pulls” a hydrogen proton from water and acid molecules. The dissolution of ammonia in water and in acids is a chemical process based on the ability of ammonia molecules to bind hydrogen ions. The reason for this is the presence of a free electron pair at the nitrogen atom, which “pulls” a hydrogen proton from water and acid molecules. NH3 + HCl → NH4Cl. ammonium chloride (ammonia) 2 NH3 + H2SO4 → (NH4) 2 SO4 ammonium sulfate 1. In the absence of a catalyst NH3 + O2 → N2 + H2O 4NH3 + 3O2 = 2N2 + 6H2O

• 1. In the absence of a catalyst NH3 + O2 → N2 + H2O 4NH3 + 3O2 = 2N2 + 6H2O
• 2. Combustion of ammonia WITH A CATALYST. In the combustion reaction, ammonia exhibits the reducing properties of ammonia
• NH3 + O2 → NO + H2O
• 4NH3 + 5O2 = 4NO + 6H2O

• Ammonia does not burn in air, but in pure oxygen or in the presence of a catalyst, ammonia oxidizes well, showing the properties of a reducing agent.

CuSO4 +2NaOH→Cu(OH)2+Na2SO4

4NH3+ Cu(OH)2→(OH)2

Receipt

In the laboratory

2NH4Cl + Ca(OH)2 = CaCl2 + 2NH3 + 2H2O

Application

Properties

contains

valuable to

plants element

Ammonia is a gas.

Ammonia has

Strong smell.

Interacts with

Oxygen.

reducing agent

evaporation

absorbed

quantity of heat.

So that the products do not disappear

• So that the products do not disappear
• Ammonia will help you
• And plants, of course.
• Ammonia is not the enemy at all.
• If fainting occurs -
• Can bring to life
• Get out of drunkenness
• Shine the windows.

APPLICATION OF AMMONIA AND ITS COMPOUNDS

Do not touch the spilled substance, it can cause a painful burn of the skin.

In the event of an ammonia leak, it is important to protect the skin and respiratory organs in the first place, and to avoid getting ammonia into the eyes.

In case of ammonia poisoning, you should not drink, but you need to drop albucid into your eyes or rinse your eyes with a solution of boric acid.

Drip warm sunflower, olive or peach oil into the nose, and wash the face, hands and generally affected areas of the body with a 2% solution of boric acid.

Control on the topic "Ammonia". What did you learn?

1 level

1) Ammonia ____________ dissolves in water.

2) Ammonia solution in water is called ___________ water or ___________ alcohol.

3) Under the action of ammonia, wet phenolphthalein paper changes its color to ________________.

4) When ammonia reacts with concentrated hydrochloric acid, a substance is formed in the form of puffs of white smoke, called _______________.

5) Ammonia in reactions exhibits ______________ properties ...

6) On what properties of ammonia are the methods of combating its leakage based?

7) On what properties of ammonia is its use in medicine, in refrigeration plants based?

2 level

1) The ammonia molecule has an unshared electron pair:

A. One B. Two C. Three D. Five

2) What substance is the reducing agent in the reaction

NH3 + O2  N2 + H2O

A. Ammonia B. Oxygen C. Nitrogen D. Water

3) Ammonia does not interact With:

A. Sulfuric acid B. Hydrochloric acid C. Sodium hydroxide D. Water

4) Set the match:

Nitrogen Properties Chemical Equations reactions

1. Reactions associated with the change A. NH3 + H2O ↔NH4OH

nitrogen oxidation states. B. 2NH3↔N2 + 3H2

2. Reactions associated with the formation of B. 4NH3 + 3O2 = 2N2 + 6H2O

covalent bond by donor-acceptor - G. NH3 + HCl = NH4Cl

nomu mechanism.

5) Write an equation for the chemical reaction of ammonia with nitric acid HNO3.

6) Why does ammonia-dyed phenolphthalein paper discolor over time? Write the appropriate reaction equations.

Ammonia

• Ammonia
• Gaseous
• Highly soluble
• Combustion reducing agent
• Salt forming ammonia
• Affecting mucous membranes
• Affects plants

N2NH3(NH4)2SO4NH4ClNH3

Make up a crossword puzzle with the keyword ammonia.

slide presentation

Slide text: Lesson topic: Ammonia “You can not love chemistry, but you cannot live without it today and tomorrow” O.M. Nefyodov

Slide text: Meet ammonia HNO3 production Medicine A product of protein metabolism in living organisms Fertilizer production Detergents Hair dye Coolant in refrigerators agriculture, chemistry, medicine, military affairs. And no less important, it is one of the products of protein metabolism in the body.

Slide text: History of the discovery of ammonia In the middle of the Libyan desert stood a temple dedicated to the god Amon Ra. In ancient times, Arab alchemists obtained colorless crystals from the Amon oasis, located near the temple. ground in mortars, heated - and received a caustic gas. At first it was called ammonia, and then the name was shortened to "ammonia". In the 18th century, ammonia was discovered by the English chemist Joseph Priestley. Today, ammonia is an extremely important raw material for the production of nitrogen-containing substances used in agriculture, chemistry, medicine, and military affairs. And no less important, it is one of the products of protein metabolism in the body.

Slide text: Production of ammonia (NH3) t NH4Cl+ Ca(OH)2 CaCl2+2NH3+2H2O Fe,t,p N2+ 3H2 2NH3+ Q

Slide text: Physical properties of ammonia NH3 NH3 ammonia is a gas: colorless, with a characteristic odor, lighter than air (collected in a vessel turned upside down) NH3 - TOXIC! Liquid ammonia causes severe skin burns; usually it is transported in steel cylinders (painted in yellow, have the inscription "Ammonia" in black) Ammonia - 3-10% ammonia solution Ammonia water - 18-25% ammonia solution Ammonia-air mixture is explosive!

Slide text: The structure of the ammonia molecule ▪ ▪ ▪ H * * * H H │ N ▪▪ The nitrogen atom, due to its three unpaired electrons, forms 3 covalent polar bonds with hydrogen atoms => the valency N is equal to III The unshared electron pair of the nitrogen atom is able to participate in the formation the fourth covalent bond with atoms having a vacant (free) orbital according to the donor-acceptor mechanism. The valency of N is IV Mechanism of donor-acceptor bond: H3N: + H+ = + ammonium ion

Slide text: Chemical properties of ammonia Reactions that occur with a change in the oxidation state of nitrogen NH3 is a strong reducing agent without changing the oxidation state of nitrogen NH3 is a weak base 1. ammonia is an unstable compound, decomposes when heated: 2NH3 N2 + 3H2 2. ammonia burns in oxygen: NH3 + O2 → N2 + H2O 3. oxidation of ammonia with air oxygen in the presence of a catalyst: NH3 + O2 NO + H2O Pt, Rh ammonia reacts with water: NH3 + H2O NH4OH NH4+ + OH− ammonium hydroxide ammonia reacts with acids: NH3 + HCl → NH4Cl ammonium chloride

Slide text: Good old ammonia, He is rich and he is poor, Rich in his unshared electrons, But only, that's the trouble, he's bored alone in solution. He is always ready to take a walk: There is acid, and here is water... Then, robbed to the skin, He cries: “Where are my belongings? What an iniquity: I have become an ammonium cation!”

1 slide

Lesson topic: Ammonia “You can not love chemistry, but you can’t live without it today and tomorrow” O.M. Nefyodov

2 slide

Meet ammonia HNO3 production Medicine Product of protein metabolism in living organisms Fertilizer production Detergents Hair dye Coolant in refrigerators And no less important, it is one of the products of protein metabolism in the body.

3 slide

The history of the discovery of ammonia In the middle of the Libyan desert stood a temple dedicated to the god Amon Ra. In ancient times, Arab alchemists obtained colorless crystals from the Amon oasis, located near the temple. ground in mortars, heated - and received a caustic gas. At first it was called ammonia, and then the name was shortened to "ammonia". In the 18th century, ammonia was discovered by the English chemist Joseph Priestley. Today, ammonia is an extremely important raw material for the production of nitrogen-containing substances used in agriculture, chemistry, medicine, and military affairs. And no less important, it is one of the products of protein metabolism in the body.

4 slide

5 slide

Physical properties of ammonia NH3 NH3 ammonia is a gas: colorless, with a characteristic odor, lighter than air (collected in a vessel turned upside down) NH3 - POISONOUS! Liquid ammonia causes severe skin burns; usually it is transported in steel cylinders (painted yellow, have the inscription "Ammonia" in black) Ammonia - 3-10% ammonia solution Ammonia water - 18 -25% ammonia solution The mixture of ammonia with air is explosive!

6 slide

The structure of the ammonia molecule ▪ ▪ ▪ Н * * *Н Н │ N ▪▪ The nitrogen atom, due to its three unpaired electrons, forms 3 covalent polar bonds with hydrogen atoms => valency N is equal to III The unshared electron pair of the nitrogen atom is able to participate in the formation of the fourth covalent bond with atoms having a vacant (free) orbital according to the donor-acceptor mechanism. The valency of N is IV Mechanism of donor-acceptor bond: H3N: + H+ = + ammonium ion

7 slide

Chemical properties of ammonia Reactions that occur with a change in the oxidation state of nitrogen NH3 is a strong reducing agent without changing the oxidation state of nitrogen NH3 is a weak base 1. ammonia is an unstable compound, decomposes when heated: 2NH3 N2 + 3H2 2. ammonia burns in oxygen: NH3 + O2 → N2 + H2O 3. oxidation of ammonia with atmospheric oxygen in the presence of a catalyst: NH3 + O2 NO + H2O Pt, Rh ammonia reacts with water: NH3 + H2O NH4OH NH4+ + OH− ammonium hydroxide ammonia reacts with acids: NH3 + HCl → NH4Cl ammonium chloride

8 slide

Good old ammonia, He is rich, and he is poor, Rich in his unshared electrons, But only, that's the trouble, he's bored alone in the solution. He is always ready to take a walk: There is acid, and here is water... Then, robbed to the skin, He cries: “Where are my belongings? What an iniquity: I have become an ammonium cation!”