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alkaline earth metals

Position in the periodic table. In the periodic system, they are in the main subgroup of group II. They are strong reducing agents, they give 2 ē, in all compounds they show an oxidation state of +2. General configuration of external energy level nS ² Mg +12 2 ē , 8 ē , 2 ē Ca +20 2 ē , 8 ē , 8 ē , 2 ē Sr +38 2 ē , 8 ē , 18 ē , 8 ē , 2 ē Ba +56 2 ē , 8 ē , 18 ē , 18 ē , 8 ē , 2 ē

Position in the periodic table Be Mg Ca Sr Ba Ra Reducing properties are enhanced

Atomic structure +4)) +12))) +20)))) +38))))) +56)))))) Be Mg Ca Sr Ba 2 2 2 2 2

Physical properties of alkaline earth metals Alkaline earth metals are silvery-white, solid substances. Compared with alkali metals, they have higher t°pl. and t ° boiling., ionization potentials, densities and hardness. Beryllium (Be) very solid material and is able to leave scratches on the glass; the hardness of other elements of the subgroup decreases, and barium is close in hardness to lead

Physical properties of alkaline earth metals. Values ​​Be Mg Ca Sr Ba Ra Ρ g/cm 1.85 1.737 1.54 2.63 3.6 6 T pl. ° according to C 1287 648 842 768 727 969

Physical properties flame color þ t melting 1.74 g / cm 3 651 C 0 1.54 g / cm 3 851 C 0 2.63 g / cm 3 770 C 0 3.76 g / cm 3 710 C 0 Mg Ca Sr Ba

Occurrence in nature Beryllium: 3BeO Al2O3 6SiO2 – beryl Magnesium: MgCO3 – magnesite Calcium: CaCO3 MgCO3 – dolomite KCl MgSO4 3H2O – kainite KCl MgCl2 6H2O – carnallite CaCO3 – calcite (limestone, marble, chalk) Ca3(PO4)2 – apatite, phosphorite CaSO4 2H2O - gypsum CaSO4 - anhydrite CaF2 - fluorspar (fluorite) Strontium: SrSO4 - celestite SrCO3 - strontianite Barium: BaSO4 - barite BaCO3 - witherite

Chemical properties With simple substances (non-metals) 2Me 0 + O 2 → 2Me +2 O -2 - oxide Me 0 + H 2 → Me +2 H 2 - hydride Me 0 + Cl 0 2 → Me +2 Cl 2 - chloride Me 0 + S 0 → Me +2 S -2 - sulfide 2. With complex substances Me 0 + 2HCl → Me +2 Cl 2 + H 2 Me 0 + 2HOH → Me +2 (OH) 2 + H 2

Compounds of alkaline earth metals Oxides of alkaline earth metals - MeO, are basic in nature, easily react with oxides of non-metals to form the corresponding salts.

BaSO 4 Due to its insolubility and ability to delay x-rays, it is used in x-ray diagnostics - barite porridge.

Ca 3 (PO 4) 2 Included in phosphorites and apatites, as well as in bones and teeth. The body of an adult contains 1 kg of Ca in the form of calcium phosphate.

CaCO 3 Calcium carbonate is one of the most common compounds on Earth. It contains rocks - chalk, marble, limestone.

CaSO 4 ∙ 2H 2 O Occurs in nature in the form of the mineral gypsum, which is a crystalline hydrate. It is used in construction, in medicine for applying plaster bandages, for making casts.

MgCO 3 is widely used in the production of glass, cement, bricks, as well as in metallurgy to convert waste rock into slag.

Ca (OH) 2 Calcium hydroxide or slaked lime with sand and water is called lime mortar and is widely used in construction. When heated, it decomposes into oxide and water.

Topic: Alkaline earth metal compounds Lesson Objectives: - knowledge-based common properties metals and their compounds (oxides and hydroxides), characterize the properties of oxides and hydroxides of alkaline earth metals; generalize, establish the relationship between the structure and properties of substances, reason logically. Epigraph to the lesson The only way leading to knowledge is activity. B. Show

I game five minutes. Identify the metal 1. That metal is used for metallothermy - the recovery of rare metals from their ores. 2. The sulfate of this element, known as bitter or Epsom salt, is used in medicine as a laxative. 3. Sea salt has a bitter taste due to the presence of cations of this metal in it. 4. The burning of this metal is accompanied by a blinding flash, so it was previously used in photography. 5. In its atom at the outer level there are two electrons, all electrons are placed on three energy levels.

1. Due to the high chemical activity, this metal is not suitable for the manufacture of products. 2. The body of an adult contains more than 1 kg of this element in the form of phosphate. 3. This metal was first obtained by G. Davy in 1808. 4. Compounds of this element are widely used, for example, in construction. Chalk, marble, limestone is its carbonate. 5. In its atom at the outer level there are two electrons, all electrons are placed on four energy levels.

Continue the statement 1. Calcium differs in physical properties from alkali metals a) color b) density c) hardness d) melting point 2. Reacts with calcium a) CI 2, P, Si b) C, CI 2, S c) O 2 , H 2, Fe 3. Hydrogen can be obtained by the interaction of calcium with a) HCI b) CO2 c) H 2 O d) NaOH e) H 2 SO4 4. Calcium has electrons distributed over energy levels a) 2.8.8.3 b ) 2,8,8,1 c) 2,8,8,2 5. Calcium exhibits properties a) oxidizing b) reducing c) oxidizing and reducing

CaCO 3 - calcium carbonate - one of the most common compounds on Earth. Minerals containing it are known, such as marble, chalk, limestone. The most important of these minerals is limestone, without which not a single building can do, and secondly, it is a raw material for obtaining other materials: cement, slaked and quicklime, glass, etc. There are large deposits of limestone and chalk in our region. Therefore, in the Belgorod region there are many factories for the production of cement and industrial chalk.

MARBLE (from the Greek marmaros, a shiny stone), a crystalline granular metamorphic carbonate rock, a product of limestone recrystallization, less often dolomite. Due to the close adhesion of calcite grains to each other, the rock is well polished. In engineering and construction, marble is called any carbonate rock, satisfactorily amenable to polishing - limestone, dolomite or marble. The metamorphism of pure limestone leads to the formation of marble, since the only possible change in calcite at high pressures and temperatures is its recrystallization. The color of marble is usually light, but the presence of even a fraction of a percent of impurities - silicates, iron oxides and graphite - leads to the coloration of the rock in different colors and shades, including yellow, brown, red, green and even black; there are also colorful, multi-colored marbles.

Limestones LIMESTONE, sedimentary rock, consisting mainly of calcite, rarely of aragonite; often with an admixture of dolomite, clay and sand particles. Limestones often contain remains of calcareous skeletons of fossil organisms. Used in metallurgy (fluxes), construction, chemical industry, etc.

MgCO 3 - magnesium carbonate, is necessary in the production of cement, glass, bricks, as well as in metallurgy to transfer waste rock, that is, not containing metal compounds, into slag. CaSO 4 - calcium sulfate, occurs in nature in the form of the mineral gypsum CaSO 4 * 2H 2 O, which is a crystalline hydrate. It is used in construction, medicine for applying fixed plaster bandages, for making casts. For this, semi-aqueous gypsum 2CaSO 4 - alabaster is used.

MgSO 4 - magnesium sulfate, known as bitter, or Epsom salt, used in medicine as a laxative. Contained in sea water and gives it a bitter taste Ca 3 (PO 4) 2 - calcium phosphate, is part of phosphorites (rock) and apatite (mineral), as well as bones and teeth. The body of an adult contains more than 1 kg of calcium in the form of Ca 3 (PO 4) 2.

Coded dictation 1. Oxides exhibit basic properties, except for beryllium. (1) 2. All oxides of the main subgroup of group II are active in reaction with water. (0) 3. Calcium oxides are called quicklime in engineering. (1) 4. Calcium hydroxide solution - lime water is used to detect carbon dioxide. (1) 5. Barium carbonate is the main constituent of minerals: chalk, marble, limestone. (0) Students peer-check their work.

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BERYLIUM, MAGNESIUM AND ALKALINE EARTH METALS

What we learn ... 18.04.17 The position of metals in the Periodic system Change of properties in the group History of the name Finding in nature Physical properties Chemical properties Fixing Literature

04/18/17 Beryllium, magnesium and alkaline earth metals are in group IIA Maximum oxidation state +2 External energy level structure ns 2 Valence - I I

18.04.17 Ra Ba Sr Ca М g Ве Change in the properties of the group In the series of metals: The radius of the atom increases The reduction properties (the ability to donate electrons) The strength of the metal-metal chemical bond decreases

04/18/17 "If you do not know the names, the knowledge of things will die" Carl Linnaeus

DISCOVERY OF METALS Magnesium and calcium were first obtained by the English chemist and physicist G. Davy in 1808. Magnesium from white magnesia. The name of the mineral gave the name of the element. The name of the element calcium comes from lat. The words kals, which means "lime, soft stone". 04/18/17 Humphry Davy (1778 - 1829)

Magnesium rock - magnesite. Found in nature As active metals, they occur in nature only in the form of compounds Calcium rocks - limestone, marble, chalk.

04/18/17 Alkali metals are light, soft and fusible, silvery, strontium has a golden hue. Strontium - malleable Physical properties Beryllium - light grey, hard, brittle Magnesium - relatively soft, ductile, malleable Calcium - hard and ductile

04/18/17 Chemical properties 1. Metals interact with almost all non-metals: 2Me 0 + O 2 0 \u003d 2Me +2 O -2 (oxide) Me 0 + H 2 0 \u003d Me + 2 H 2 -1 (hydride) Me 0 + Cl 2 0 \u003d M e + 2 Cl 2 -1 (chloride) Me 0 + S 0 \u003d M e + 2 S -2 (sulfide) 3Me 0 + N 2 0 \u003d M e 3 + 2 N 2 - 3 (nitride)

04/18/17 Chemical properties 2. Beryllium does not react with water, magnesium reacts slowly, other metals react with water, forming alkalis and reducing water to hydrogen: Me 0 + 2H 2 O \u003d Me + 2 (OH) 2 + H 2  3 • Magnesium reacts with acids. Me 0 + 2H Cl = Me +2 Cl 2 + H 2  4. Magnesium and calcium react with oxides. 2 M g 0 + Ti O 2 \u003d 2 M g + 2 O + Ti

Check yourself (work with the table of D.I. Mendeleev) Compare the atoms of the elements by putting signs or = instead of *: a) nuclear charge: Be * Ba; M g * Al ; Ca*K; b) number of electron layers: Be * Ba; M g * Al ; Ca*K; c) the number of electrons in the outer level: Be * Ba; M g * Al ; Ca*K; d) atomic radius: Be * Ba; M g * Al ; Ca*K; e) reducing properties: Be * Ba; M g * Al ; Ca*K. 04/18/17

04/18/17 Complete the schemes for the interaction of alkali metals with non-metals with general formulas and names of the reaction products. Write down specific reaction equations, placing the coefficients in them by the method electronic balance. a) M + H 2 c) M + C1 2 Example: ___________________ Example: b) M + S d) M + N 2 Example: _______________________________ Example: ___________________________ Complete the reaction equations. How does the rate of reactions located in the sequence indicated by the arrow change? a) Ca + H 2 O → ………………………. b) Sr + H 2 O →………………………. c) Ba + H 2 O→……………………….. Explain on what factor the reaction rate of the interaction of alkali metals with water depends ……………………….. Name the reaction products. Describe how to prove their education. ……………………… .................................. ... Test yourself

Municipal Autonomous General Educational Institution

« secondary school No. 24, Syktyvkar

PLAN - LESSON SUMMARY

TOPIC: Alkaline earth metals

Completed by: Malakhaeva Anna Lvovna

SYKTYVKAR, 2015

The purpose of the lesson:

study physical, Chemical properties alkaline earth metals;

Learn about the use of alkaline earth metals and their compounds.

lesson type - learning new material.

Critical Thinking Technology

Forms of organization learning activities - frontal, steam room, individual.

Teaching methods :

Partially search;

Interdisciplinary conversation.

learning techniques :

independent / pair / individual work of students.

Tasks

I Tutorials:

Describe the physical properties of alkaline earth metals;

Acquaintance with the features of the chemical properties and areas of application of alkaline earth metals.

II Developing:

Development and generalization of students' knowledge about the practical use of alkaline earth metals;

III Educational :

Equipment:

Multimedia projector

for demonstration experiments: magnesium, hydrochloric acid, spoons for burning substances, matches, flasks filled with oxygen, test tubes;

instruction card "Application of alkaline earth metals and their compounds"

Literature for the teacher:

Kuznetsova N.E., Titova I.M., Gara N.N., Zhegin A.Yu. Chemistry: Grade 9: Textbook for students of educational institutions / Ed. N.E. Kuznetsova. – M.: Ventana-Graf, 2008.

Shatalov M.A., Kuznetsova N.E. Teaching chemistry. Solution of integrative educational problems: 8-9 grades: Toolkit. – M.: Ventana-Graf, 2006.

Kuznetsova N.E., Shatalov M.A. Teaching chemistry based on interdisciplinary integration: 8-9 cells: educational method. Benefit. -M.: Ventana-Graf, 2006.

G.O. Astvatsaturov Technology of lesson goal-setting. - Volgograd: Teacher, 2009.

Materials of the workshop "Development of competency-oriented tasks for academic subjects» ANO "Center for Youth Development", Yekaterinburg.

During the classes

I Organizing time

Teacher greeting. Ready for the lesson. What do you see in the pictures. What unites them?(Slide 1). Metals.

II Actualization of knowledge

Let's remember everything we know about metals (“I know”). Metals are located in the lower left part of the PS, have a metallic luster, conduct well electricity, and also studied the properties of alkali metals(Slide 2). What haven't we learned yet? Supposed to be alkaline earth metals and a subgroup of aluminum. So what is the topic of today's lesson? alkaline earth metals (Slide 3). So what do we want to know? Physical properties, chemical properties and applications (Slide 4). The purpose of our lesson will be: 1. To study the physical, chemical properties of alkaline earth metals; 2. Learn about the use of alkaline earth metals (Slide 5).

Physical properties of alkaline metals. What physical properties do you think the alkaline earth metals will have?Assume: metallic luster, softness (similar to alkaline), low density. You have an instruction card on the tables. Read the text. What do they have in common? They are silver in color, and all are soft, except for beryllium.(Slide 6).

What determines the chemical properties of alkaline earth metals? The presence of 2 electrons in the outer energy level. What do you think the alkaline earth metals will react with? They can assume: with water, acids, oxygen.

Chemical properties of alkaline metals.

Let's look at the chemical properties. To do this, we will divide into three groups (by columns). Open §51 p.237. Column I will record the chemical properties with oxygen and with halogen using magnesium as an example. 2 Me + O 2 = 2 MeO (oxide),2Mg + O 2 = 2Mgo . Let's see how magnesium burns (demonstration experiment: combustion of magnesium (student shows)). Me + Hal 2 = MeHal 2 ( halides), Mg+Cl 2 = MgCl 2 .

II column - with sulfur and with nitrogen using calcium as an example. Me+S = MeS( sulfide), Sr+S =SrS; Me+N 2 = Me 2 N 3 ( nitride), Sr + N 2 = Sr 2 N 3 . III column - with hydrogen and with water using calcium as an example. Me + H 2 = MeH 2 (hydride),Ca + H 2 = Ca H 2 ; Me + 2H 2 O =M e(Oh ) 2 + H 2 , Ca + 2H 2 O =Ca (Oh ) 2 + H 2 .

Still SHCHZ metals will interact with acids. Let's see how magnesium will interact with hydrochloric acid (demonstration experience: the interaction of magnesium with acid (student shows)). Attention to the slide! Me + acids = salt +H 2 (Slide 7). What products are formed as a result of the reaction? Magnesium chloride and hydrogen is released.Mg + 2HCl = MgCl 2 + H 2.

Finding alkaline earth metals in nature and compounds of alkaline earth metals. Where do you think pure alkaline earth metals can be found in nature? Nowhere, because in its pure form, they are not found due to their high chemical activity. There are papers on your tables. Scan the text with your eyes (15 seconds). Now I am showing you a picture, and you, using the text that is on your tables, will tell you where this metal is found and used. Answer using the text on the tables(Slides 8-9).

III Consolidation

Today we have studied alkaline earth metals. What did you learn about them? Did you achieve the goal you set at the beginning of the lesson? Yes, we have, we have learned their physical and chemical properties, their presence in nature and their application(Slide 10). And now "Fill in the blanks!" (Slide 11). Homework. §51; prepare about the history of the discovery of alkaline earth metals according to options: I option - Be , II option - mg , III option - Ca , IV option - Sr , V option - Ba , VI option - Ra (Slide 12).

Instructional card "Physical properties, application and finding of alkaline earth metals and their compounds"

Beryllium- solid metal of light gray color. It occurs in nature in the form of minerals: beryl, chrysoberyl and their varieties: emerald, aquamarine, alexandrite - known as precious stones. Beryllium and its water-soluble compounds are highly toxic (poisonous). Even a negligibly small admixture of it in the air leads to serious illnesses. It finds wide application in technology. Added to copper, it greatly increases its hardness, strength, chemical resistance, and makes it look like steel. The main consumer of beryllium is nuclear power. The need for it is growing every year.

Magnesium - soft, silvery-white metal. B It was first obtained by Devi in ​​1808 from white magnesia (magnesite MgCO 3) - a mineral found near the Greek city of Magnesia. By the name of the mineral, they gave the name to a simple substance and a chemical element. Magnesium sulfate (one of the common magnesium salts) is also called bitter salt - it gives sea water a bitter taste. This magnesium salt is used as a laxative. Alloys with magnesium are stronger, harder, easily polished, processed and used in the automotive industry, aviation, and rocket technology.

Calcium - soft silvery white. It ranks fifth in terms of prevalence. It was also first obtained by Devi in ​​1808. The name of the element comes from the Latin word "cals", which means "lime, soft stone". It occurs in the form of calcite (calcite forms deposits of chalk, marble, limestone), as well as in the form of the mineral gypsum, which is a crystalline hydrate. It is used in construction, in medicine for applying plaster bandages, for making casts. Calcium is also found in human bones and teeth.

Strontium- soft, malleable and plastic silver-gold color. It is less common in the form of the mineral celestine, which means "heavenly" in Latin - strontium sulfate, formed by pink-red, pale blue crystals. It (strontium) got its name from the name of the Scottish village of Strontian, near which a rare mineral strontianite SrCO 3 was found at the end of the 18th century. The main areas of application of strontium and its chemical compounds are the radio-electronic industry, pyrotechnics, metallurgy

Barium- soft silver-white metal. It occurs in the form of barite BaSO 4 (“baris” - heavy from Latin). It is used for the manufacture of radio lamps, in leather business (to remove wool), in sugar production, for making photographic paper, smelting special windows. BaSO 4 due to its insolubility and ability to delay x-rays is used in x-ray diagnostics - barite porridge.

Radium- Shiny silver-gold metal.

Used for making luminous colors constant glow (for marking the dials of aviation and marine instruments, special watches and other instruments).

Fill in the blanks!

Ca + ... = 2CaO

… + … = Be 3 N 2

Mg + ... = MgSO 4 + ...

Lesson type: learning new material.

Type of lesson: combined lesson

Lesson objectives:

Tutorials: the formation of students' knowledge about alkaline earth elements as typical metals, the concept of the relationship between the structure of atoms and properties (physical and chemical).

Developing: development of research skills, the ability to extract information from various sources, compare, generalize, draw conclusions.

Educators: education of sustainable interest in the subject, education of such moral qualities as accuracy, discipline, independence, responsible attitude to the task assigned.

Methods: problematic, search, laboratory work, independent work students.

Equipment: computer, safety table, disk “Virtual laboratory in chemistry”, presentation .

During the classes

1. Organizational moment.

2. Introductory word of the teacher.

We are studying the section, metals, and you know that metals are of great importance in the life of a modern person. In previous lessons, we got acquainted with the elements of group I of the main subgroup - alkali metals. Today we are starting to study the metals of group II of the main subgroup - alkaline earth metals. In order to learn the material of the lesson, we need to remember the most important questions discussed in previous lessons.

3. Actualization of knowledge.

Conversation.

Where are the alkali metals in the periodic system of D.I. Mendeleev?

Student:

In the periodic system, alkali metals are located in group I of the main subgroup, on the outer level 1 electron, which alkali metals easily give away, therefore, in all compounds they exhibit an oxidation state of +1. With an increase in the size of atoms from lithium to francium, the ionization energy of atoms decreases and, as a rule, their chemical activity increases.

Teacher:

Physical properties of alkali metals?

Student:

All alkali metals are silvery-white in color with slight tints, light, soft and fusible. Their hardness and melting point naturally decrease from lithium to cesium.

Teacher:

We will check the knowledge of the chemical properties of alkali metals in the form of a small test work on the options:

• Ioption: Write the reaction equations for the interaction of sodium with oxygen, chlorine, hydrogen, water. Specify the oxidizing agent and reducing agent.
• I option: Write the reaction equations for the interaction of lithium with oxygen, chlorine, hydrogen, water. Specify the oxidizing agent and reducing agent.
• I I I option: Write the reaction equations for the interaction of potassium with oxygen, chlorine, hydrogen, water. Specify the oxidizing agent and reducing agent.

Teacher: The topic of our lesson is “Alkaline earth metals”

Lesson objectives: Give general characteristics alkaline earth metals.

Consider their electronic structure, compare physical and chemical properties.

Learn about the most important compounds of these metals.

Determine the scope of these compounds.

Our lesson plan is written on the board, we will work according to the plan, look at the presentation.

1. The position of metals in the periodic system D.I. Mendeleev.
2. The structure of the alkali metal atom.
3. physical properties.
4. Chemical properties.
5. The use of alkaline earth metals.

Conversation.

Teacher:

Based on the previous knowledge, we will answer the following questions: next questions: To answer, we will use the periodic system of chemical elements of D.I. Mendeleev.

1. List the alkaline earth metals

Student:

These are magnesium, calcium, strontium, barium, radium.

Teacher:

2. Why are these metals called alkaline earth?

Student:

The origin of this name is due to the fact that their hydroxides are alkalis, and their oxides are similar in refractoriness to oxides of aluminum and iron, which were previously worn. common name"lands"

Teacher:

3. Location of alkaline earth metals in PSCE D.I. Mendeleev.

Student:

Group II is the main subgroup. Metals of group II of the main subgroup have 2 electrons at the external energy level, located at a smaller distance from the nucleus than alkali metals. Therefore, their reducing properties, although great, are still less than those of the elements of group I. Strengthening of the reducing properties is also observed during the transition from Mg to Ba, which is associated with an increase in the radii of their atoms; in all compounds, the oxidation state is +2.

Teacher: Physical properties of alkaline earth metals?

Student:

Metals of group II of the main subgroup are silvery-white substances that conduct heat and electric current well. Their density increases from Be to Ba, while the melting point, on the contrary, decreases. They are much harder than alkali metals. All, except beryllium, have the ability to color the flame in different colors.

Problem: How are alkaline earth metals found in nature?

Why do alkaline earth metals mostly exist in nature in the form of compounds?

Answer: In nature, alkaline earth metals are in the form of compounds, because they have high chemical activity, which in turn depends on the features of the electronic structure of atoms (the presence of two unpaired electrons at the external energy level)

Fizkultminutka - rest for the eyes.

Teacher:

Knowing the general physical properties, the activity of metals, assume the chemical properties of alkaline earth metals. What substances do alkali metals interact with?

Student:

Alkaline earth metals interact with both simple and complex substances. They actively interact with almost all non-metals (with halogens, hydrogen, forming hydrides). From complex substances with water - forming water-soluble bases - alkalis and with acids.

Teacher:

And now, in experiments, we will verify the correctness of our assumptions about the chemical properties of alkaline earth metals.

4. Laboratory work on the virtual laboratory.

Target: carry out reactions confirming the chemical properties of alkaline earth metals.

We repeat the safety rules for working with alkaline earth metals.

• work in a fume hood
• on a tray
• with dry hands
• take in small quantities

We work with the text that we read in the virtual laboratory.

Experience No. 1. Interaction of calcium with water.

Experience number 2. Combustion of magnesium, calcium, strontium, barium

Write down the reaction and observation equations in a notebook.

5. Summing up the lesson, grading.

5. Reflection.

What do you remember about the lesson, what did you like?

6. Homework.

§ 12 exercise 1(b) exercise 4

Literature.

1. Rudzitis G.E., Feldman F.G. Chemistry 9.- Moscow.: Education, 2001
2. Gabrielyan O.S. Chemistry 9.-Moscow.: Bustard, 2008
3. Gabrielyan O.S., Ostroumov I.G. Handbook of the teacher. Chemistry 9.-Moscow.: Bustard 2002
4. Gabrielyan O.S. Control and verification work. Chemistry 9.-Moscow.: Bustard, 2005.
5. Collection of the Virtual Laboratory. Educational electronic edition