Application of hydrogen presentation. Presentation on the topic "hydrogen". Chemical bond - covalent

Presentation for the lesson

"Hydrogen and its properties"

8th grade

Chaplygina Iraida Ivanovna

"NO SCIENCE NEEDS EXPERIMENT TO THE EXTENT OF CHEMISTRY"

(MICHAEL FARADEY)

Mystery

You already met me

I am a space wanderer

Elements progenitor

And a brave leader

I am an oxygen lover

Together with him I give water.

Station "OBTAINING HYDROGEN"

Station "OBTAINING HYDROGEN"

Answer option number 1

• Hydrogen is in the first group. Ordinal number 1, valency is 1.

• H, H2

The molecular weight is 2, the atomic weight is 1;

Molar mass 2g/mol

Answer option number 2

Station "OBTAINING HYDROGEN"

Station "OBTAINING HYDROGEN"

Station "OBTAINING HYDROGEN"

ZnCl2+H2

Test

• This substance is a gas;
• Gas, colorless, odorless, slightly soluble in water;
• The most common element in space;
• The most abundant chemical element in the earth's crust;
• A chemical element that is part of water;
• A molecule is made up of two atoms;
• What substances are oxygen and hydrogen made from?

A) zinc and hydrochloric acid, potassium and water; decomposition of water;

B) potassium permanganate was heated; hydrogen peroxide, water decomposition.

Determine and write out the numbers of only true statements

Hydrogen

Oxygen

note

Homework

Exercise 1-2, p.76

Mini-message "Application of hydrogen"

PUZZLES

• 1. A GUEST FROM SPACE HAS COME,

I FOUND A SHELTER IN THE AIR.

• 2. WHAT CHEMICAL ELEMENTS DO

WHAT OTHER SUBSTANCES CAN BIRTH.

Hydrogen has redox amphotericity with a predominance of reducing properties. Under normal conditions, hydrogen reacts only with fluorine, with some other substances? when heated

View document content
"Voprosy_k_slaydam"

Slide Questions Application

1. Name the first element of the "Periodic Table of Chemical Elements

DI. Mendeleev "(slides - No. 1, No. 4)

2. By whom and in what century was hydrogen discovered? (slide number 5)

3. Why was element #1 called hydrogen? (slide number 6)

4. Where and in what form (free or bound) does hydrogen occur in nature?

(slide number 7)

5. How is the hydrogen atom arranged? (slide number 8)

6. What are the isotopes of hydrogen known to you (slide number 9)

7. Which of them are the most common on Earth? (slide number 10)

8. What do you know about heavy water? (slide number 11)

9. Why is the hydrogen molecule diatomic? (slide number 12)

10. What are the valence capabilities of hydrogen? (slide number 13)

11. List the physical properties of hydrogen known to you (slide No. 14)

12. What mixture is called explosive gas? (slide number 15)

13. In what cases is hydrogen checked for purity and how it is carried out

practically? (slide number 16)

14. On what physical properties of hydrogen are the methods of collecting it based?

(slide number 17)

15. How is hydrogen produced in the laboratory? (slide number 18)

16. How is hydrogen produced in industry? (slide number 19)

17. How to explain the dual location of hydrogen in the "Periodic system

chemical elements D.I. Mendeleev" - inI -a andVII -and subgroups?

(slide number 20,21)

18. Under what conditions is hydrogen chemically active? (slide number 22)

19. Give examples where hydrogen acts as a reducing agent

(slide number 23, 24)

20. Give examples where hydrogen acts as an oxidizing agent (slide number 25)

21.Where is hydrogen used or could it be used in the future? (slide number 26)

View presentation content
"Prezentatsia"

1 . First element

2. Henry Cavendish

3. Antoine Lavoisier

4. Spreading hydrogen in nature

5. Structure atom hydrogen

6. isotopes hydrogen

7. isotopes hydrogen on the ground

8. Some regular and heavy water constants

9. Molecule hydrogen

10. Valence possibilities of hydrogen

11. Physical properties

12. Rattlesnake gas

(continuation should – cm . next slide)

13. Examination hydrogen on the purity

14. Ways picking up hydrogen

15. Receipt in laboratories

16. Receipt in industry

17 . Hydrogen in periodical table

18 . Oxidatively - restorative

amphotericity

19 . Chemical properties hydrogen

20 . Recovery properties hydrogen

21 . Recovery copper from oxide copper( II)

hydrogen

22. Oxidative properties hydrogen

23 . Application hydrogen

24 . Appendix "Questions for slides"

25 . Appendix "Questions for slides"

(continuation)

HENRY CAVENDISH

First convinced , what

under the action of acids

for some metals

formed" COMBUSTIBLE GAS » , which, mixed with air

spirit when set on fire

explodes

1731 - 1810

Antoine Laurent Lavoisier

First installed , that hydrogen, when burned, forms water , and called him

Hydrogenium-

"giving birth to water"

2 H 2 + O 2 = 2H 2 ABOUT

1743 - 1794

The structure of the hydrogen atom

hydrogen atom

is made up of a nucleus

and one electron

Electronic

atom configuration

1 s 1

HYDROGEN ISOTOPS

Isotopes are varieties of one

atom , having in the core :

1 . the same number of protons

( and therefore the same nuclear charge) ;

2. different number of neutrons

( and therefore a different size BUT r )

H( 1 H) - protium D ( 2 H) - deuterium T ( 3 H) – tritium

H (1r + + 0 n 0 ) + 1 e - BUT rH = 1

n D (1r + + 1n 0 ) + 1 e - BUT rD = 2

T (1r + + 2n 0 ) + 1 e - BUT r T = 3

AND ZOTOPES HYDROGEN ON THE W EMLE

In natural compounds

deuterium and protium on average

1: 5 500 (according to the number of atoms)

T lithium – radioactive isotope ,

received art c tvenno

SOME CONSTANTS OF ORDINARY AND HEAVY WATER

Constants

Plain water H 2 ABOUT

M r

heavy water D 2 ABOUT

ρ at 25 0 FROM , kg/m 3

0, 9971

t kip , 0 C

t frozen , 0 C

1 ,1042

10 1 , 4

t Max . tight , 0 C

3, 8

11, 6

HYDROGEN MOLECULE

H 2 – diatomic

Chemical bond - covalent

non-polar

H – H

H++ H → H:H

VALENCE CAPABILITIES OF HYDROGEN Electronic configuration of an atom : 1 s 1

Hydrogen valence : 1 Oxidation states : - 1 0 +1

Degrees

oxidation

hydrogen

with non-metals

In simple

substance

Examples

with metals

HF H 2 About NH 3 CH 4

Chemical

connection between

atoms

covalent

polar

H 2

covalent

non-polar

NaN CaN 2

Ionic

colorless gas

Without smell

Almost insoluble in water (1: 50)

Density - 0 ,0899 kg/m 3

IN 14 ,5 times lighter than air

At -252 , 8 0 Hydrogen is liquefied

2 n 2 + about 2 = 2 n 2 about

2 V : 1V

• If hydrogen is pure , then he burns quietly , with characteristic

sound "p-groin"

• If hydrogen contains impurities air , then it burns with an explosion

displacement method

water

displacement method

air

in industry

BUT . by electrolysis water and water

solutions of alkalis and salts

2H 2 O= 2 H 2 + O 2

2N A CL+2H 2 O=H 2 +CL 2 + 2N A Oh

B . By passing water vapor over

hot coal

C + H 2 O = CO + H 2

IN . Methane conversion (when heating )

FROM H 4 + H 2 O = CO + 3 H 2

Oxidatively – restorative

amphotericity of hydrogen

H 0 e → H +1

H 0 + e → H –1

• Hydrogen has a redox amphotericity with a predominance of reducing properties

• Under normal conditions hydrogen only reacts with fluorine , with some other substances ▬ when heated

A. WITH NON-METALS

2H 2 + FROM l 2 = 2H Cl

2H 2 + ABOUT 2 = 2H 2 ABOUT

H 2 +S = H 2 S

B. C METAL OXIDES

H 2 + C AND O = C AND + H 2 ABOUT

copper oxide (II)

CuO + H 2 = C + H 2 ABOUT

2. OXIDATIVE PROPERTIES

Interaction hydrogen

with active metals

H 2 + 2 LI = 2 LI H

H 2 + Ca = CaH 2

• For the industrial synthesis of many substances

(of hydrochloric acid , ammonia , methanol, etc. .)

• Recovery of rare metals from their oxides

(tungsten , molybdenum, etc. .)

• Hydrogenation of organic compounds

(for the purpose of obtaining , for example , solid fats

from vegetable oils ; artificial

liquid fuel from coal, etc. .)

• For welding and cutting metals

(hydrogen - oxygen flame)

• As a gaseous and liquid fuel - H 2
• As a fusion fuel - isotopes B .

(to be used already in our century)

Grade 9

Teacher: Smirnova Ekaterina Sergeevna

Lesson topic: Hydrogen.

The purpose of the lesson: to activate and systematize knowledge about being in nature. physical properties. Chemical properties of hydrogen:
reactions with non-metals and metals. Reactions of hydrogen with metal oxides. Obtaining hydrogen in the laboratory and industry.
The use of hydrogen.(slide 2)

Lesson type: the assimilation of new knowledge, skills, and their creative application in practice.

Forms of work: lecture, presentation demonstration.

Equipment: projector, textbook.

During the classes.

Organizing time: greeting, checking readiness for the lesson.

Checking homework.

Updating of basic knowledge.

Frontal conversation:

1. What do you know about hydrogen as a simple substance?

2. Find hydrogen in PS.

3. According to the position in the PS, what properties of hydrogen can you say?

Learning new material.

In the dissertation of M.V. Lomonosov "On metallic luster" in 1745. for the first time, the production of hydrogen by the action of an acid on iron and other metals was described, and a hypothesis was put forward that hydrogen (combustible vapor) is phlogiston.

(slide 3)

The hydrogen content in the earth's crust is 1% by weight and 17% of the total number of atoms.(slide 4)

Hydrogen is the lightest of all elements. It is part of the water that covers about ¾ of the earth's surface, the composition of many minerals and rocks, as well as all organic compounds. In freehydrogen is found in small quantities in the upper atmosphere and in some natural combustible gases.(slide 5)

Physical properties . Hydrogen under normal conditions is a colorless and odorless gas. It is 14.5 times lighter than air, slightly soluble in water (2 volumes of hydrogen dissolve in 100 volumes of water). At a temperature of -2530 C and atmospheric pressure turns into a liquid state, and at -2590 C solidifies. Due to its low molecular weight, it easily diffuses (passes) through porous partitions and even through a heated metal partition. At elevated temperatures, hydrogen is highly soluble in many metals (nickel, platinum, palladium). (slide 6)

Hydrogen exists in the form of three isotopes: protium - with a mass number of 1, deuterium - with a mass number of 2 and tritium - with a mass number of 3. The main part of natural hydrogen (99.98%) is protium.(slide 7)

Chemical properties.

The hydrogen atom has one electron. In the formation of chemical compounds, it almost always gives up an electron, acquiring a +1 charge. Due to the small charge of the nucleus, the hydrogen atom attracts electrons relatively weakly and can attach them only when another element easily gives them away. In this case, the hydrogen atom forms a stable two-electrode shell of the inert helium gas.(slide 8)

Interaction with alkali and alkaline earth metals.

Alkali and alkaline earth metals readily donate electrons to hydrogen. The reaction proceeds when metals are heated in a hydrogen atmosphere and is accompanied by the formation of salt-like compounds - hydrides.

2 Na + H2 = 2 NaH- sodium hydride

Ca + H2 = CaH2 - sodium hydride(slide 9)

Interaction with non-metals.

Hydrogen compounds are more characteristic, in which it exhibits a positive oxidation state, it interacts with almost all non-metals, and, depending on the activity of the non-metal, the reaction proceeds at different rates. So, hydrogen always interacts with fluorine with an explosion:

H2 + F 2 = 2 HF

It interacts more calmly with chlorine. Hydrogen burns well in an atmosphere of chlorine:

H2 + Cl = 2 HCl

(slide 10)

Obtaining hydrogen in the laboratory.

Under laboratory conditions, hydrogen is obtained:

1) the interaction of the metal with hydrochloric or dilute sulfuric acid (the reaction is carried out in the Kipp apparatus):

Zn + 2HCl → ZnCl2 + H2

2) interaction with metal alkalis, the hydroxide of which has amphoteric properties (aluminum, zinc):

2Al + 2NaOH + 6H2 O → 2Na + 3H2

Zn + 2KOH + 2H2 O→K2 + H2 ( slide 11)

3) water electrolysis. To increase the electrical conductivity of water, an electrolyte is added to it - alkali or alkali metal sulfate. Chlorides are less suitable for this purpose. Since when they decompose, chlorine is released at the anode.

Obtaining hydrogen in industry.

1) as a by-product in the production of chlorine and alkali metal hydroxides by electrolysis of solutions of their chlorides;

2) conversion (transformation) of carbon and water vapor. To do this, in special gas generators, as a result of the interaction of water vapor with hot carbon (coal), a mixture of hydrogen and carbon monoxide is obtained:

C+H2 O=CO+H2

The resulting gas mixture, together with water vapor, is passed over hot iron monoxide, which plays the role of a catalyst:

CO+H2 O= CO2 + H2 ,

And then - through water or an alkali solution to absorb CO2 ;

3) conversion of methane with water vapor, carbon dioxide or a mixture of water vapor and carbon dioxide:

CH4 + SO2 = 2CO + 2H2

CH4 + H2 O=CO+3H2

3CH4 + SO2 + 2H2 O=4CO+8H2

These processes proceed at a temperature of about 10000 C. They are catalyzed by nickel with the addition of oxides of magnesium, aluminum and other metals. (slide 12)

Application.

Hydrogen is a valuable raw material for the chemical industry. It is used to produce ammonia and synthetic methyl alcohol, for the hydrogenation of solid fuels and fats. A significant amount of hydrogen is used to produce various metals and non-metals (germanium, gallium, tungsten, molybdenum, etc.) in industry by reducing their oxides or halides. Using the high combustion temperature of hydrogen in oxygen, it is used for cutting and welding metal structures. (Slide 13)

Checking the assimilation of knowledge.

Choose the correct definition. Physical properties of hydrogen:

A) colorless and odorless gas.

B) it is 16.4 times lighter than air.

B) soluble in water.

2. Give the names of hydrogen isotopes:

1H -

2H -

3H -

3. Fill in the missing words.

The hydrogen atom has one _________. In the formation of chemical compounds, it almost always ______ electron, acquiring a charge of ___. Due to the ______ charge of the nucleus, the hydrogen atom attracts _______ relatively ______ and can only attach them when another element easily gives them away. In this case, ________ hydrogen forms a stable two-electrode shell ________ _________ _______.(slide 15)

Lesson results. Homework: study item 19, complete the tasks for the paragraph in writing in a notebook.

Someday the time will come - and this time is not far off - when the measure of value will not be gold, but energy. And then hydrogen isotopes will save mankind from impending energy starvation: in controlled thermonuclear processes, each liter of natural water will provide as much energy as 300 liters of gasoline now provide. D.I. Shcherbakov

1. Combustion reaction: When hydrogen reacts with oxygen, water is formed. Hydrogen without impurities burns quietly. 2 H 2 + O 2 \u003d 2 H 2 O to J (exothermic)

4. Interaction with oxides of inactive metals called powder metallurgy.

Conclusions: 1). Under normal conditions, molecular hydrogen interacts only with the most active substances - fluorine, sodium, calcium. 2). Hydrogen compounds with non-metals are mostly gases. The exception is water. 3). Chemical reactions with hydrogen usually proceed at elevated temperature, pressure, or in the presence of a catalyst. 4). Hydrogen burns, and oxygen supports combustion. five). Hydrogen in reactions with oxides of inactive metals is a reducing agent.

Tasks: 1. What mass of hydrogen is required for its interaction with 64 g of sulfur. 2. What volume of hydrogen will be spent on the reduction of copper (II) oxide if 13 g of copper is formed as a result of the reaction. 3. According to the thermochemical equation 2 H 2 + O 2 \u003d 2 H 2 O to J, calculate the amount of heat that will be released when 10 liters of hydrogen are burned.

Homework: §27, questions and 11 - in writing.

slide 1

Made by: Gonenko Asya

slide 2

HYDROGEN (lat. Hydrogenium), H, chemical element with atomic number 1, atomic mass 1.00794. The chemical symbol of hydrogen H is read in our country "ash" as the chemical element hydrogen. Natural hydrogen consists of a mixture of two stable nuclides with mass numbers 1.007825 (99.985% in the mixture) and 2.0140 (0.015%). In addition, in natural hydrogen there are always negligible amounts of the radioactive nuclide - tritium 3H (half-life T1 / 212.43 years). Since the nucleus of a hydrogen atom contains only 1 proton (there cannot be less protons in the nucleus of an atom), it is sometimes said that hydrogen forms the natural lower boundary of the periodic system of elements of D. I. Mendeleev (although the element hydrogen itself is located in the uppermost part tables). The element hydrogen is located in the first period of the periodic table. It belongs to both the 1st group (group IA of alkali metals) and the 7th group (group VIIA of halogens).

Chemical element

slide 3

Physical properties

Hydrogen is the lightest and most abundant element in the universe. Over 95% of all known chemicals contain hydrogen. The main sources of hydrogen on Earth are water, oil, natural. In space, it is the most common element: it makes up more than half the mass of the Sun and other stars. It is a colorless and odorless gas. 14.5 times lighter than air. Practically insoluble in water. It dissolves well with some metals.

slide 4

Interaction of hydrogen with metals

When heated, hydrogen can react with the most active metals: alkali, alkaline earth and aluminum, forming hydrides. Under normal conditions, these are solid salt-like substances, unstable to water and acid solutions, which decompose irreversibly.

slide 5

Interaction of hydrogen with non-metals

Hydrogen reacts with very many non-metals, and, depending on the activity of the non-metal, these reactions can proceed under various conditions. Hydrogen interacts most easily with fluorine, chlorine and oxygen.