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21.09.2023

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Oxygen

Position of oxygen in p.s. Electronic structure. 2nd period, 2nd row, 6-A group The ancestor of the main subgroup of the 6th group. “Chalcogens” - giving birth to ores (O, S, Se, Te, Po) O 8 15.9994 2s 2 2p 4 Oxygen

Distribution of oxygen in nature. Oxygen is the most abundant element on our planet.

Oxygen accounts for approximately half of the total mass of the earth's crust. In soils, groundwater, river and sea waters, oxygen acts as a real geochemical dictator.

Physical properties of oxygen. Gas without color, smell and taste; In the liquid state it has a light blue color, in the solid state it is blue; Oxygen gas is more soluble in water than nitrogen and hydrogen.

Chemical properties of oxygen. A strong oxidizing agent, it interacts with almost all elements, forming oxides. Oxidation state −2. As a rule, the oxidation reaction proceeds with the release of heat and accelerates with increasing temperature. Example of reactions occurring at room temperature: 4K + O2 → 2K2O 2Sr + O2 → 2SrO Oxidizes compounds that contain elements with less than the maximum oxidation state: 2NO + O2 → 2NO2 Oxidizes most organic compounds: CH3CH2OH + 3O2 → 2CO2 + 3H2O Oxygen does not oxidize Au and Pt, halogens and inert gases. Reacts with other non-metals, forming oxides: S+O2 →SO2 C+O2 →CO2 Actively interacts with alkali and alkaline earth metals to form oxides and peroxides: 2Na+O2 →Na2O2 Reacts with other metals when heated, releasing a large amount of heat and light: 2 Mg+O2 →2MgO

Obtaining oxygen in the laboratory. Most often, oxygen is obtained by heating substances (which contain oxygen in bound form) such as potassium permanganate (potassium permanganate), potassium chlorate (Berthollet salt), potassium nitrate (saltpeter), hydrogen peroxide: 2 KMnO 4 = K 2 MnO 4 + MnO 2 + O 2 potassium permanganate heating potassium manganate manganese dioxide oxygen 2 KClO 3 = 2 KCl + 3 O 2 potassium chlorate heating potassium chloride oxygen

2 KNO 3 = 2 KNO 2 + O 2 potassium nitrate heating potassium nitrite oxygen 2 H 2 O 2 = 2 H 2 O + O 2 hydrogen peroxide catalyst oxygen

Oxygen collection by water and air displacement methods

Oxygen cycle in nature.

Photosynthesis

Discovery of oxygen. He obtained oxygen in many ways: by calcining mercuric oxide (as Priestley and Lavoisier did), heating mercury carbonate and silver carbonate, etc. Undoubtedly, Scheele was the first (1772) to “hold in his hands” pure oxygen.

Scheele manuscript page

Joseph Priestley (Joseph Priestley, 1733-1804) 2 HgO = 2 Hg + O 2 mercuric oxide heating mercury oxygen

Antoine Lavoisier (Lavoisier, Antoine Laurent, 1743-1794) Repeating Priestley's experiments, Lavoisier concluded that atmospheric air consists of a mixture of “vital” (oxygen) and “suffocating” (nitrogen) air and explained the combustion process by combining substances with oxygen. Early in 1775, Lavoisier reported that the gas obtained by heating red oxide of mercury was “air as such, unchanged (except that) ... it is purer, more respirationable.”

Use of oxygen.

Thank you for your attention!

Where did the oxygen come from?

The nature of this chemical element was discovered 3 times, the last one was the famous French chemist Antoine Laurent Lavoisier, who studied oxygen as a component in combustion.

For more than 2 years he studied all the reactions of interaction between various elements, which gave him the opportunity to claim the “life gas” released during the combustion of nitrogen, and thus he discovered a new element - oxygen.

Now everyone knows that this element is vital for all living things; its chemical structure is closely related to almost every element known today (with the exception of inert gases).

As part of the atmosphere of our planet, oxygen arrives in a free (not bound) state.

Presumably, according to scientists, there was practically no oxygen on the young, newly created planet Earth. It began to be created through the development of the life activity of photosynthetic organisms.

The main part of the surface consisted of gases that can now be found during a volcanic explosion (water vapor, carbon monoxide, hydrogen sulfide, etc.).

The process of creating an atmosphere began with the development of prokaryotes, which, under the influence of sunlight, absorbed oxygen from carbon dioxide, and in return they released oxygen as a by-product of the reaction.

Since prokaryotes did not need constant free oxygen for respiration, but used anaerobic oxygen, oxygen accumulated in the atmosphere itself and entered into mutual reactions with elements on the surface of the still young planet.

Practical meaning of oxygen

Up to 65% of a person's body weight is oxygen. This is approximately 40 kg for an adult. It is the most common oxidizing agent on the planet.

Oxygen is found in:

● composition of rocks of the earth's crust

● the world's oceans (as part of the water molecule itself and dissolved in gaseous form)

● Atmosphere (free form and in the composition of other gases)

It is important for the human body as an element of redox processes.

Thanks to the presence of oxygen in our body, we can process fats, carbohydrates, and proteins to extract the necessary useful energy for human needs.

Oxygen is widely used in medicine as a source of pure substance for the resuscitation of seriously ill patients. It is administered through a special oxygen machine and mask.

The use of oxygen is also developed in:

● automotive industry for plasma cutting as an additional gas;

● chemical industry, as the main oxidizer of many processes;

● glass industry to improve combustion quality;

● the field of metallurgy for air enrichment or air replacement;

As can be seen from the list, oxygen is an integral component of the normal functioning of all life on the planet.

Antoine Laurent LAVOISIER () () Investigated oxygen and created the oxygen theory of combustion, which replaced the phlogiston theory. He studied oxygen and created the oxygen theory of combustion, which replaced the phlogiston theory.

Oxygen is the most common element on Earth In the air 21% (by volume), In the air 21% (by volume), in the earth's crust 49% (by mass), in the earth's crust 49% (by mass), in the hydrosphere 89% ( by mass), in the hydrosphere 89% (by mass), in living organisms up to 65% of mass. in living organisms up to 65% of the mass.

Physical properties Physical state - gas under normal conditions. At very low temperatures (-183°C) it turns into a liquid aggregate state (blue liquid), and at even lower temperatures (-219°C) it becomes solid (blue snow crystals). The physical state is gas under normal conditions. At very low temperatures (-183°C) it turns into a liquid aggregate state (blue liquid), and at even lower temperatures (-219°C) it becomes solid (blue snow crystals). Color – colorless. Color – colorless. Smell - odorless. Smell - odorless. Solubility in water - poorly soluble. Solubility in water - poorly soluble. Heavier than air (M air = 29 g/mol, and M O 2 = 32 g/mol. Heavier than air (M air = 29 g/mol, and M O 2 = 32 g/mol.

Chemical properties Oxygen is a very strong oxidizing agent! It oxidizes many substances already at room temperature (slow oxidation) and even more so when the substance is heated or burned (fast oxidation). Oxygen is a very strong oxidizing agent! It oxidizes many substances already at room temperature (slow oxidation) and even more so when the substance is heated or burned (fast oxidation). In reactions with all elements (except fluorine), oxygen is always an OXIDIZING agent. In reactions with all elements (except fluorine), oxygen is always an OXIDIZING agent.

Reactions with metals As a result of the reaction, an oxide of this metal is formed. For example, aluminum is oxidized by oxygen according to the equation: As a result of the reaction, the oxide of this metal is formed. For example, aluminum is oxidized by oxygen according to the equation: t° 4Al + 3O 2 2Al 2 O 3 t° 4Al + 3O 2 2Al 2 O 3 Another example. When a red-hot iron wire is lowered into a bottle of oxygen, the wire burns, spraying out sheaves of sparks - hot particles of iron scale Fe 3 O 4: t° 3Fe + 2O 2 Fe 3 O 4 t° 3Fe + 2O 2 Fe 3 O 4

Other examples of reactions with non-metals The combustion of sulfur in oxygen with the formation of sulfur dioxide SO 2: t° S + O 2 SO 2 t° S + O 2 SO 2 The combustion of coal in oxygen with the formation of carbon dioxide: The combustion of coal in oxygen with the formation of carbon dioxide: t° C + O 2 CO 2 t° C + O 2 CO 2

Reactions with certain complex substances In this case, oxides of the elements that make up the molecule of the complex substance are formed. In this case, oxides of the elements that make up the molecule of the complex substance are formed. For example, when roasting copper (II) sulfide For example, when firing copper (II) sulfide t° 2CuS + 3O 2 2CuO + 2SO 2 t° 2CuS + 3O 2 2CuO + 2SO 2 two oxides are formed: copper (II) oxide and sulfur oxide ( IV). Two oxides are formed: copper (II) oxide and sulfur (IV) oxide. When sulfides are roasted, sulfur oxide is always formed, the valence of sulfur in which is equal to IV. When sulfides are roasted, sulfur oxide is always formed, the valence of sulfur in which is equal to IV. Another example is the combustion of methane CH 4. Since this molecule consists of atoms of the elements carbon C and hydrogen H, this means that two oxides are formed: carbon monoxide (IV) CO 2 and hydrogen oxide, that is, water - H 2 O: t° CH 4 + 2O 2 CO 2 + 2H 2 O t° CH 4 + 2O 2 CO 2 + 2H 2 O

The chemical interaction of a substance with oxygen is called an oxidation reaction. Oxidation reactions accompanied by the release of heat and light are called combustion reactions. Combustion reactions of substances are examples of rapid oxidation, but rotting, rusting, etc. these are examples of slow oxidation of substances with oxygen. Combustion reactions of substances are examples of rapid oxidation, but rotting, rusting, etc. these are examples of slow oxidation of substances with oxygen

Production of oxygen (laboratory methods) decomposition of water by electric current, decomposition of water by electric current, decomposition of hydrogen peroxide H 2 O 2 under the action of the MnO 2 catalyst, decomposition of hydrogen peroxide H 2 O 2 under the action of the MnO 2 catalyst, decomposition of potassium permanganate KMnO 4 when heated. decomposition of potassium permanganate KMnO 4 when heated.

Oxygen production (industrial method) In industry, to obtain pure oxygen, liquid air distillation is used, based on different boiling temperatures of air components. The air is cooled to approximately -200°C and then slowly heated. When the temperature reaches - 183°C, oxygen evaporates from the liquid air; the remaining components of liquefied air at this temperature remain in a liquid aggregate state. In industry, to obtain pure oxygen, liquid air distillation is used, based on different boiling temperatures of air components. The air is cooled to approximately -200°C and then slowly heated. When the temperature reaches - 183°C, oxygen evaporates from the liquid air; the remaining components of liquefied air at this temperature remain in a liquid aggregate state.

The use of oxygen in construction and mechanical engineering in construction and mechanical engineering - for oxygen-acetylene gas welding and gas cutting of metals - for oxygen-acetylene gas welding and gas cutting of metals - for spraying and surfacing of metals in oil production in oil production - when pumping into the reservoir to increase displacement energy in metallurgy and mining industry in metallurgy and the mining industry - in convective steel production, oxygen blasting in blast furnaces, extraction of gold and ores, production of ferroalloys, smelting of nickel, zinc, lead, zirconium and other non-ferrous metals - in convective steel production, oxygen blasting in blast furnaces , extraction of gold and ores, production of ferroalloys, smelting of nickel, zinc, lead, zirconium and other non-ferrous metals - during direct reduction of iron - during direct reduction of iron - during fire cleaning in foundries - during fire cleaning in foundries - during fire drilling of solids breeds

The use of oxygen in medicine in medicine - in oxypressure chambers - in oxypressure chambers - when filling oxygen masks, pillows, etc. - when refilling oxygen masks, pillows, etc. - in wards with a special microclimate - in wards with a special microclimate - for the production of oxygen cocktails - for the production of oxygen cocktails - when growing microorganisms - when growing microorganisms in ecology in ecology - when purifying drinking water - when purifying drinking water - when recycling metals - during recycling of metals - when blowing wastewater with oxygen - when blowing wastewater with oxygen - when neutralizing chemically active waste in treatment plants in incinerators - when neutralizing chemically active waste in treatment plants in incinerators

The use of oxygen in the chemical industry in the chemical industry - in the production of acetylene, cellulose, methyl alcohol, ammonia, nitric and sulfuric acid - in the production of acetylene, cellulose, methyl alcohol, ammonia, nitric and sulfuric acid - in the catalytic conversion of natural gas (in the production of synthetic ammonia) - for catalytic conversion of natural gas (in the production of synthetic ammonia) - for high-temperature conversion of methane - for high-temperature conversion of methane in the energy sector in the energy industry - for gasification of solid fuels - for gasification of solid fuels - for air enrichment for domestic and industrial boilers - for enrichment air for domestic and industrial boilers - for compressing a water-coal mixture - for compressing a water-coal mixture

The use of oxygen in military equipment in military equipment - in pressure chambers - in pressure chambers - for operating diesel engines under water - for operating diesel engines under water - as a fuel oxidizer for rocket engines - as a fuel oxidizer for rocket engines in agriculture in agriculture - for enriching the aquatic environment with oxygen in fishing - for enriching the aquatic environment with oxygen in fishing - for the production of oxygen cocktails - for the production of oxygen cocktails - for weight gain for animals - for weight gain for animals

OZONE Allotropic modification of oxygen Ozone O 3 is a blue gas with a pungent odor. Anyone who has paid attention to how the air smells after a thunderstorm or near a source of electrical discharge knows the smell of this gas very well. Ozone O3 is a blue gas with a pungent odor. Anyone who has paid attention to how the air smells after a thunderstorm or near a source of electrical discharge knows the smell of this gas very well. In nature, ozone is formed under the influence of ultraviolet radiation from the Sun, and is also obtained from electrical discharges in the atmosphere: In nature, ozone is formed under the influence of ultraviolet radiation from the Sun, and is also obtained from electrical discharges in the atmosphere:

Ozone is a very strong oxidizing agent, so it is used to disinfect drinking water. An explosion occurs upon contact with most oxidizable substances. Ozone is formed in the Earth's atmosphere at an altitude of 25 km under the influence of solar radiation; it absorbs dangerous radiation from the Sun. However, in the Earth's ozone "umbrella", which is only about 30 meters thick, "holes" appear every now and then. More and more gases that are “harmful” to ozone are entering the air, such as nitrogen monoxide NO or those substances that are used to fill refrigeration units and aerosol cans. Even the partial disappearance of the ozone layer above the Earth threatens the death of all living things... However, in the ozone “umbrella” of the Earth, which is only about 30 meters thick, “holes” appear every now and then. More and more gases that are “harmful” to ozone are entering the air, such as nitrogen monoxide NO or those substances that are used to fill refrigeration units and aerosol cans. Even a partial disappearance of the ozone layer above the Earth threatens the death of all living things...

Slide presentation

Slide text: Presentation prepared by Roxana Smirnova, 9th grade student of the Lyceum of Otradnoye

Slide text: Oxygen as an element. 1. The element oxygen is in group VI, main subgroup, period II, serial number No. 8, 2. Atomic structure: P11 = 8; n01 = 8; ē = 8 valency II, oxidation state -2 (rarely +2; +1; -1). 3. Part of oxides, bases, salts, acids, organic substances, including living organisms - up to 65% by weight.

Slide text: Oxygen as an element. Oxygen is the most common element on our planet. By weight, it accounts for approximately half of the total mass of all elements of the earth's crust. Air composition: O2 – 20-21%; N2 – 78%; CO2 – 0.03%, the rest comes from inert gases, water vapor, and impurities. 4. In the earth's crust it is 49% by mass, in the hydrosphere - 89% by mass. 5. Composed of air (in the form of a simple substance) – 20-21% by volume. 6. Included in most minerals and rocks (sand, clay, etc.). Composed of air (in the form of a simple substance). 7. A vital element for all organisms, found in most organic substances, involved in many biochemical processes that ensure the development and functioning of life. 8. Oxygen was discovered in 1769-1771. Swedish chemist K.-V. Scheele

Slide text: Physical properties. Oxygen is a chemically active non-metal and is the lightest element from the group of chalcogens. The simple substance oxygen under normal conditions is a colorless, tasteless and odorless gas, the molecule of which consists of two oxygen atoms, for which reason it is also called dioxygen. Liquid oxygen is light blue in color, while solid oxygen is light blue crystals.

Slide text: Chemical properties. With non-metals C + O2 CO2 S + O2 SO2 2H2 + O2 2H2O With complex substances 4FeS2 + 11O2 2Fe2O3 + 8SO2 2H2S + 3O2 2SO2 + 2H2O CH4 + 2O2 CO2 + 2H2O With metals 2Mg + O2 2MgO 2Cu + O2 –t 2CuO Inter action of substances with oxygen is called oxidation. All elements react with oxygen except Au, Pt, He, Ne and Ar; in all reactions (except for the interaction with fluorine), oxygen is an oxidizing agent. 1. Unstable: O3 O2 + O 2. Strong oxidizing agent: 2KI + O3 + H2O 2KOH + I2 + O2 Discolors dyes, reflects UV rays, destroys microorganisms.

Slide text: Methods of obtaining. Industrial method (distillation of liquid air). Laboratory method (decomposition of some oxygen-containing substances) 2KClO3 –t ;MnO2 2KCl + 3O2 2H2O2 –MnO2 2H2O + O2

Slide text: Checking the collected oxygen. Obtaining 3O2 2O3 During a thunderstorm (in nature), (in the laboratory) in an ozonizer of potassium permanganate when heated: 2KMnO4 –t K2MnO4 + MnO2 + O2 The decomposition of this salt occurs when it is heated above 2000 C.

Slide text: Application of oxygen: It is widely used in medicine and industry. During high-altitude flights, pilots are provided with special oxygen devices. For many pulmonary and heart diseases, as well as during operations, oxygen is given to inhale from oxygen cushions. Submarines are supplied with oxygen in cylinders. The combustion of loose combustible material impregnated with liquid oxygen is accompanied by an explosion, which makes it possible to use oxygen in blasting operations. Liquid oxygen is used in jet engines, in autogenous welding and metal cutting, even under water.

Oxygen

journey

Lavoisier Antoine Laurent

French chemist. One of the founders of classical chemistry. Introduced strict quantitative research methods into chemistry. He laid the foundation for the refutation of the phlogiston theory. Got oxygen. He proved the complex composition of atmospheric air containing oxygen and “suffocating air” (nitrogen). He proved the complex composition of water, establishing that it consists of oxygen and hydrogen.

“Oxygen is the substance around which all earthly chemistry revolves.”

(J. Berzelius)

« Living organisms drink air in order to

to get oxygen."

(D.I. Mendeleev)

« The first duty of someone who wants to become healthy is to cleanse the air around him.”

(R.Roland)

What do you know about oxygen?

And what do you want to know about him?

The purpose of the lesson:

What scientists

worked

with oxygen?

Oxygen

What is it

catalyst?

History of discovery

Methods of obtaining

oxygen

Finding

in nature

Physical properties

The purpose of the lesson:

find out the value of oxygen
learn the history of the discovery of oxygen
learn the physical properties of oxygen
learn to characterize

oxygen as a chemical element and

like a simple substance

learn about being in nature
learn about obtaining oxygen.

"Historical and informational"

He is everywhere and everywhere: In the ground, in the air, in the water. He is in the morning dew, And in the blue sky.

general characteristics

Chemical sign - O

Serial number - 8

Chemical formula - O 2

Molar mass M (O 2) = 32 g/mol

Valence - II

Group - 6 A

Period - 2

Oxygen is the eighth in a row, If you take weight as a measure. If moderation is the place in life, the number must be changed.

Gas without color, taste, smell.
Heavier than air: 1 liter at N. u. weighs 1.43 g, and 1 liter of air - 1.29 g.
Poorly soluble in water (fish breathe oxygen dissolved in water; 5 liters of oxygen dissolve in 100 liters of water at a temperature of 0 degrees).
boiling t = – 182.9 degrees.
melting t = – 218.8 degrees.

2 HgO = 2 Hg + O 2
2 H 2 O 2 = 2 H 2 O + O 2 (cat. MnO 2)
2 KClO 3 = 2 KCl + 3 O 2 (cat. MnO 2)
2 H 2 O = 2 H 2 + O 2
2 KNO 3 = 2 KNO 2 + O 2

2 KMnO 4 = K 2 MnO 4 +MnO 2 + O 2

Catalysts are substances

which accelerate chemical reactions, but at the same time

are not spent.

An old Arab was dying. All his wealth consisted of 17 beautiful camels. Before his death, he announced his last will to his sons: “My eldest son, the support of the family, should receive half of the herd of camels, I leave the middle one a third, and the youngest one a ninth of the herd.” He said so and died...

The brothers, having buried their father, began to divide the inheritance. But 17 is not divisible by 2, 3, or 9.
The sage helped them by giving the brothers his camel. They ended up with 18 animals.
18: 2 = 9,
18: 3 = 6,
18: 9 = 2.
9+6+2 = 17!
The camel given to the scientist played the role of a catalyst.

Oxygen production in industry

Nitrogen boiling point -196ºС
The boiling point of oxygen is -183ºС
Air

Cooling to

Liquid oxygen and nitrogen gas

How can you separate a mixture of oxygen and nitrogen?

Oxygen

Option 1.

Chemical symbol of oxygen: a) N b) O c) K
The relative molecular mass of oxygen is: a) 16 b) 32 c) 48
a) lighter than air; b) poorly soluble in water;

c) does not support combustion.

4. The name "Oxygenium" was suggested by:

5. What substances does the chemical element oxygen form? a) only simple substances;

b) simple and complex substances;

c) only complex substances.

Answers: Option 1 – b, b, b, b, b.

Oxygen

Option 2.

Formula of oxygen molecule: a) O 2 b) O c) O 3
The relative atomic mass of oxygen is: a) 16 b) 32 c) 48
Oxygen has the following properties: a) heavier than air; b) highly soluble in water; c) does not support breathing.
Oxygen in water: a) slightly soluble; b) highly soluble;

c) does not dissolve at all.

5. In 1774, one scientist, after an experiment,

wrote: “But what struck me most was that

the candle burned in this air amazingly brilliant

flame..." It was: a) Priestley b) Lavoisier c) Scheele.

Answers: Option 2 – a, a, a, a, a.

Every year, as a result of photosynthesis, 3000 billion tons of oxygen enter the Earth's atmosphere.
The main suppliers of oxygen are tropical forests and ocean phytoplankton.
A person inhales approximately 750 liters of oxygen per day.
The complete passage of atmospheric oxygen through the biological cycle system takes 2000 years!

Homework

§18, 19, 20 (physical properties),

exercises 1 - 3 (page 59).

Write a fairy tale about the adventures of oxygen or an essay “What would I do to preserve clean air on planet Earth?”

Lesson #2

Oxygen

journey

in "The World of Amazing Substance".

"Experimental".

Chemical properties of oxygen.

I. Interaction with non-metals:

M.V. Lomonosov determined that oxygen oxidizes substances, i.e. enters into oxidation reactions.

sulfur burns in oxygen.

II. Interaction with metals.

Combustion of iron in oxygen.

Calcium combustion in oxygen.

3Fe + 2O 2 = Fe 3 ABOUT 4

2Ca+O 2 = 2CaO

What is combustion?
What common things were released as a result of combustion reactions?

What is formed as a result of all reactions?

Oxides.

There are different oxides Solid, liquid, gaseous. Called differently And the properties differ. But they are united in one thing They are collectively called oxides.