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Chemical elements of the main subgroup IA of group of the periodic system of elements of D. I. Mendeleev: Li, Na, K, Rb, Cs, Fr. The name comes from hydroxides of alkali metals, called caustic alkalis. Atoms of alkali metals have 1 s-electron on the outer shell, and 2 s- and 6 p-electrons on the previous shell (except for Li). Characterized by low melting temperatures, low densities; soft, cut with a knife. The oxidation state of alkali metals in compounds is always +1. These metals are chemically very active - they are quickly oxidized by atmospheric oxygen, react violently with water, forming alkalis MeOH (where Me is a metal); activity increases from Li to Fr.
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Lithium (lat. - lithium), Li-chemical element of the first group, A-subgroup of the periodic system of D.I. Mendeleev, belongs to the alkali metals, serial number 3, atomic mass is 6.939; under normal conditions, a silvery-white, lightweight metal. Natural lithium consists of two isotopes with mass numbers 6 and 7. An interesting detail: the cost of lithium isotopes is not at all proportional to their abundance. At the beginning of this decade in the United States, relatively pure lithium-7 was almost 10 times more expensive than very high-purity lithium-6. Two more lithium isotopes have been obtained artificially. Their lifetime is extremely short: lithium-8 has a half-life of 0.841 seconds, and lithium-9 has a half-life of 0.168 seconds.
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Lithium is a typical element of the earth's crust, a relatively rare element (content 3.2×10-3% by mass), it accumulates in the most recent products of magma differentiation - pegmatites. There is little lithium in the mantle - in ultramafic rocks it is only 5 × 10-3% (in basic rocks 1.5 × 10-3%, in intermediate rocks - 2 × 10-3%, in acidic rocks 4 × 10-3%). The proximity of the ionic radii of Li+, Fe2+ and Mg2+ allows lithium to enter the lattices of magnesium-iron silicates - pyroxenes and amphiboles. In granitoids it is contained as an isomorphic impurity in micas. Only 28 independent lithium minerals (silicates, phosphates, etc.) are known in pegmatites and in the biosphere. They are all rare. In the biosphere, lithium migrates relatively weakly, its role in living matter is less than that of other alkali metals. It is easily extracted from waters by clays; there is relatively little of it in the World Ocean (1.5×10-5%).
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Potassium (Kalium) Potassium is a chemical element of group I of the periodic system of Mendeleev; atomic number 19, atomic mass 39.098; silver-white, very light, soft and fusible metal. The element consists of two stable isotopes - 39K (93.08%), 41K (6.91%) and one weakly radioactive 40K (0.01%) with a half-life of 1.32×109 years.
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Occurrence in nature Potassium is a common element: the content in the lithosphere is 2.50% by mass. In magmatic processes, potassium, like sodium, accumulates in acidic magmas, from which granites and other rocks crystallize (average potassium content 3.34%). Potassium is found in feldspars and micas. Basic and ultrabasic rocks rich in iron and magnesium are low in potassium. On the earth's surface, potassium, unlike sodium, migrates weakly. When rocks weather, potassium partially passes into water, but from there it is quickly captured by organisms and absorbed by clays, so river waters are poor in potassium and much less of it enters the ocean than sodium. In the ocean, potassium is absorbed by organisms and bottom silts (for example, it is part of glauconite); Therefore, ocean waters contain only 0.038% potassium - 25 times less than sodium.
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In nature, it is the ninth most abundant element (sixth among metals), found only in the form of compounds. It is part of many minerals, rocks, and salt layers. The third most abundant metal in natural waters: 1 liter of sea water contains 0.38 g of K+ ions. Potassium cations are well adsorbed by soil and are difficult to wash out with natural waters. A vital element for all organisms. K+ ions are always found inside cells (unlike Na+ ions). The human body contains about 175 g of potassium, the daily requirement is about 4 g. The lack of potassium in the soil is compensated by applying potassium fertilizers - potassium chloride KCl, potassium sulfate K2SO4 and plant ash.
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Interesting facts WHAT IS POTASSIUM CYANIDE NEEDED FOR? For extracting gold and silver from ores. For galvanic gilding and silvering of base metals. For obtaining many organic substances. For nitriding steel - this gives its surface greater strength. Unfortunately, this much-needed substance is extremely poisonous. And KCN looks quite harmless: small white crystals with a brownish or gray tint.
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Cesium Cesium was discovered relatively recently, in 1860, in the mineral waters of famous healing springs in the Black Forest (Baden-Baden, etc.). In a short historical period, it has gone through a brilliant path - from a rare, unknown chemical element to a strategic metal. He belongs to the working family of alkali metals, and the blue blood of the last of his kind flows in his veins... However, this does not in the least prevent him from communicating with other elements, and even if they are not so famous, he willingly enters into contacts with them and establishes strong communications. Currently, he works simultaneously in several industries: in electronics and automation, in radar and cinema, in nuclear reactors and on spaceships...”
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Cesium is known to have been the first element discovered by spectral analysis. Scientists, however, had the opportunity to become familiar with this element even before Robert Bunsen and Gustav Kirchhoff created a new research method. In 1846, the German chemist Plattner, analyzing the mineral pollucite, discovered that the sum of its known components was only 93%, but was unable to accurately determine what other element (or elements) was included in this mineral. Only in 1864, after the discovery of Bunsen, the Italian Pisani found cesium in pollucite and established that it was the compounds of this element that Plattner could not identify.
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Interesting Facts Cesium and Pressure All alkali metals change greatly when exposed to high pressure. But it is cesium that reacts to it most uniquely and sharply. At a pressure of 100 thousand atm. its volume decreases almost three times - more than that of other alkali metals. In addition, it was under high pressure conditions that two new modifications of elemental cesium were discovered. The electrical resistance of all alkali metals increases with increasing pressure; In cesium this property is especially pronounced.
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Francium Among the elements at the end of the periodic table D.I. Mendeleev, there are those about which non-specialists have heard and know a lot, but there are also those about which even a chemist can tell little. The former include, for example, radon (No. 86) and radium (No. 88). Among the second is their neighbor in the periodic table, element No. 87 - francium. Francium is interesting for two reasons: firstly, it is the heaviest and most active alkali metal; secondly, francium can be considered the most unstable of the first hundred elements of the periodic table. The longest-lived isotope of francium, 223Fr, has a half-life of only 22 minutes. Such a rare combination in one element of high chemical activity with low nuclear stability determined the difficulties in the discovery and study of this element.
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Occurrence in nature In addition to 223Fr, several isotopes of element No. 87 are now known. But only 223Fr exists in nature in any noticeable quantities. Using the law of radioactive decay, it can be calculated that a gram of natural uranium contains 4·10–18 g of 223Fr. This means that about 500 g of France-223 is in radioactive equilibrium with the entire mass of earthly uranium. There are two more isotopes of element No. 87 in vanishingly small quantities on Earth - 224Fr (a member of the radioactive thorium family) and 221Fr. Naturally, it is almost impossible to find an element on Earth whose global reserves do not reach a kilogram. Therefore, all studies of francium and its few compounds were performed on artificial products.
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Interesting facts Sodium on a submarine Sodium melts at 98°C, but boils only at 883°C. Consequently, the temperature range of the liquid state of this element is quite large. That is why (and also due to the small neutron capture cross section) sodium began to be used in nuclear energy as a coolant. In particular, American nuclear submarines are equipped with power plants with sodium circuits. The heat generated in the reactor heats the liquid sodium, which circulates between the reactor and the steam generator. In a steam generator, sodium, when cooled, evaporates water, and the resulting high-pressure steam rotates a steam turbine. For the same purposes, an alloy of sodium and potassium is used.
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Inorganic photosynthesis Typically, the oxidation of sodium produces an oxide of the composition Na2O. However, if sodium is burned in dry air at elevated temperatures, then instead of oxide, peroxide N2O2 is formed. This substance easily gives up its “extra” oxygen atom and therefore has strong oxidizing properties. At one time, sodium peroxide was widely used to bleach straw hats. Now the proportion of straw hats in the use of sodium peroxide is negligible; The main quantities of it are used for bleaching paper and for air regeneration in submarines. When sodium peroxide interacts with carbon dioxide, the process opposite to respiration occurs: 2Na2O2 + 2CO2 → 2Na2CO3 + O2, i.e. Carbon dioxide is bound and oxygen is released. Just like a green leaf!
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Sodium and gold By the time sodium was discovered, alchemy was no longer in favor, and the idea of turning sodium into gold did not excite the minds of natural scientists. However, now a lot of sodium is consumed to obtain gold. “Gold ore” is treated with a solution of sodium cyanide (and it is obtained from elemental sodium). In this case, gold is converted into a soluble complex compound, from which it is isolated with the help of zinc. Gold miners are among the main consumers of element No. 11. On an industrial scale, sodium cyanide is produced by the reaction of sodium, ammonia and coke at a temperature of about 800°C.
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Sodium in water Every schoolchild knows what happens if you throw a piece of sodium into water. More precisely, not into water, but onto water, because sodium is lighter than water. The heat released when sodium reacts with water is enough to melt the sodium. And now a sodium ball runs through the water, driven by the released hydrogen. However, the reaction of sodium with water is not only dangerous fun; on the contrary, it is often useful. Sodium reliably removes traces of water from transformer oils, alcohols, ethers and other organic substances, and using sodium amalgam (i.e. an alloy of sodium with mercury) you can quickly determine the moisture content in many compounds. Amalgam reacts with water much more calmly than sodium itself. To determine moisture content, a certain amount of sodium amalgam is added to a sample of organic matter and the moisture content is determined by the volume of hydrogen released.
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Rubidium is a metal that can be called chemically touchy. Upon contact with air, it spontaneously ignites and burns with a bright pinkish-violet flame. It explodes with water and also reacts violently on contact with fluorine, chlorine, bromine, iodine, and sulfur. As a true touch-me-not, rubidium must be protected from external influences. For this purpose, it is placed in vessels filled with dry kerosene... Rubidium is heavier than kerosene (density of rubidium 1.5) and does not react with it. Rubidium is a radioactive element and slowly releases a stream of electrons to become strontium. The most remarkable property of rubidium is its peculiar sensitivity to light. Under the influence of light rays, rubidium becomes a source of electric current. With the cessation of light irradiation, the current also disappears. R. reacts with water explosively, and hydrogen is released and a solution of R. hydroxide, RbOH, is formed.
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Interesting facts Rubidium has not ignored many representatives of the plant world: traces of it are found in seaweed and tobacco, in tea leaves and coffee beans, in sugar cane and beets, in grapes and some types of citrus fruits. Why was it called rubidium? Rubidus – Latin for “red”. It would seem that this name is more suitable for copper than for rubidium, which is very ordinary in color. But let's not rush to conclusions. This name was given to element No. 37 by its discoverers Kirchhoff and Bunsen. More than a hundred years ago, while studying various minerals with a spectroscope, they noticed that one of the lepidolite samples sent from Rosen (Saxony) gave special lines in the dark red region of the spectrum. These lines have not been found in the spectra of any known substance. Soon, similar dark red lines were discovered in the spectrum of sediment obtained after the evaporation of healing waters from the mineral springs of the Black Forest. It was natural to assume that these lines belonged to some new, previously unknown element. So in 1861 rubidium was discovered
Galtseva O.N. Chemistry teacher MBOU "Anninskaya Secondary School with UIOP"
Lesson topic: MetalsIA-groups of the Periodic Table and the simple substances they form
The purpose of the lesson: To develop the cognitive interest of students and intensify their cognitive activity when studying elementsIA-groups, their physical and chemical properties.
Planned learning outcomes .
Subject.Knowledge of the features of the electronic structure of alkali metal atoms, their physical and chemical properties; the ability to express knowledge of chemical properties through the preparation of appropriate equations of chemical reactions; ability to observe and describe chemical experiments.
Metasubject.The ability to define concepts, generalize, establish analogies, classify, independently select grounds and criteria for classification, establish cause-and-effect relationships, build logical reasoning, and draw conclusions.
Personal.Formation of a holistic worldview corresponding to the modern level of development of science.
Basic Concepts: alkali metals, atomic structure, type of crystal lattice, oxides, peroxides.
Demonstrations: Periodic table of chemical elements D.I. Mendeleev, metals lithium and sodium, experiment on the interaction of lithium and sodium with water.
| Lesson steps | Teacher activities | Student activity |
| Updating knowledge | Slide number 2. Repetition of the general characteristics of metals on the questions “Remove the excess” | They comment on the slide and “remove unnecessary things” that are not related to metals. Repeat the general characteristics of metals |
| Learning new material | Slide number 3. Compilation of comparative characteristics of alkali metals, changes in the properties of metals in a group depending on the structure of atoms | Fill out the table yourself. Using the completed table, a comparative description of alkali metals is given. |
| Slide 4. Metals in nature. Questions: What groups are metals divided into according to their occurrence in nature? What group do alkali metals belong to? How can I get them? Teacher explanation about the electrolysis process using slide animation. | From the previous lesson they give information in what form metals are found in nature. They answer the question about what form alkali metals occur in nature and how they can be obtained. |
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| Slide 5. Physical properties of alkali metals. Questions: What is the crystal lattice of metals? What properties of metals depend on this type of crystal lattice? What properties of alkali metals can you assume? Demonstration of lithium and sodium. | Answer the teacher's questions based on information received about the general characteristics of metals. It is assumed what physical properties alkali metals have. |
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| Slide 6. Chemical properties of alkali metals. Demonstration of the chemical reaction of lithium and sodium with water. Questions: How to explain the phenomena occurring in a demonstration experiment? Why did sodium react faster than lithium? What other chemical properties do alkali metals have? | They assume what properties alkali metals may have based on the general properties of metals. Observe a demonstration chemical experiment of the interaction of lithium and sodium with water. They explain the chemical phenomenon taking place, answer questions posed by the teacher and complete the tasks described on the slide. Write down information about chemical properties in a notebook. |
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| Slide 7. Use of sodium and potassium compounds. The slide is interactive. Work is carried out selectively, in accordance with the remaining time. Working with trivial names of substances. | The picture determines in which area a particular connection is used. By clicking on the picture, a task appears that is completed together, one student at the board. Working with trivial names of substances. |
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| Consolidation | Slide 8. Test work. When completing this task, you must select the correct answer and left-click on it.. | Perform an interactive test. Discussion of test results. |
| Homework |
Sources of information used
Akhmetov M.A., Gara N.N. Chemistry: 9th grade teaching aid, M. Ventana-Graf, 2014
Kuznetsova N.E., Titova I.M., Gara N.N. Chemistry: 9th grade: textbook for students of general education institutions. - 5th ed., revised. - M. Ventana-Graf, 2013
Kuznetsova N.E., Gara N.N. Chemistry: programs: grades 8-11 - 2nd ed., revised. - M. Ventana-Graf, 2012
Rubidium 37Rb. Rubidium is a light and very soft (like wax), silvery-white metal. Discovered in 1861 by two previously unknown dark red lines in the spectrum by German scientists R. Bunsen and G. Kirchhoff. The color of these lines determined the name: translated from Latin “rubidos” - “dark red”. ".
Slide 12 from the presentation "Characteristics of alkali metals". The size of the archive with the presentation is 264 KB.Chemistry 9th grade
summary of other presentations“Halogens and human health” - Crossword puzzle “Halogens”. Fluorine. Biological role of bromine. Biological role of iodine. Bromine. Milk running onto the stove. Handkerchiefs. Biological role of chlorine. Iodine. Biological role of fluorine. Halogens and human health. Useful tips. Chlorine. After World War II. General characteristics of halogens. Faded colors. This is useful to know. Knowledge from the field of biology.
“Nitrogen and ammonia” - Qualitative reaction. Third wheel. Safety precautions. Nitrogen in ammonia. Nessler's reagent. "Yes or no". Pharaoh's Snake. Ammonia molecule. Oxidation state. Choose a formula. Ammonium salts. Mechanism. Assessment. Ammonia in water. Characteristic properties of the class of salts. Laboratory work. Assimilation. Decomposition of ammonium chloride. Volcano. Qualitative reactions. Nitrogen. Physical and chemical properties.
“Gaseous substances” - Application of carbon dioxide. Gaseous substances. Oxygen is obtained by the decomposition of potassium permanganate. Artificial pollution. Distance between atoms. Atmosphere. Oxygen. Coniferous forest killed by acid rain. Ethylene. Carbon dioxide. History of the origin and development of the atmosphere. Carbon dioxide does not support combustion. Laboratory methods for producing ethylene. Methods for recognizing carbon dioxide.
"Water" - Lime slaking. Interaction. Water molecules are highly resistant to heat. Water is a very common substance on Earth. C + H2O = H2 + CO. Chemical properties of water. Pure water is a colorless, transparent liquid. Water. Water in nature. Physical properties of water.
“Characteristics of alkali metals” - Alkali metals. Sodium. Simple metals. Write down reaction equations. Lesson plan. Rubidium. Cesium. Franc. Natural compounds of alkali metals. Check yourself. Lithium. Regularities in the structure of alkali metal atoms. Potassium. Alkali metal compounds. General characteristics of the elements of the main subgroup of group I.
“The concept of metals” - Inorganic chemistry. Write an equation for the reaction. Which of these elements is redundant? Basic concepts. Find the picture. Find matches. Find all metals. Find the third extra substance. Answer the questions. Which of these metals does not react with water. Sodium oxide. Sodium hydroxide. Gypsum. Feldspars. What characteristics are suitable for aluminum. With which of these salts will zinc not react?
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Topic: Compounds of alkali metals Test on the topic: Alkali metals. Answers: 1- d 2 - c 3 - b 4 - c 5 - a 6 - d 7 - b 8 - a 9 - b 10 - c. Grading scale: no errors – “5”, 1.2 errors – “4”, 3.4 errors – “3”, more – “2” D/z § 11, ex. 1 (b) p.48. Alkali metals do not include: a) rubidium; c) potassium; b) cesium; d) copper. The electronic formula 1s2 2s2 2p6 3s2 3p6 4s1 corresponds to the element: a) lithium; c) potassium; b) sodium; d) copper. The atomic radius of elements of group I of the main subgroup with increasing nuclear charge: a) changes periodically; c) does not change; b) increases; d) decreases. Alkali metals exhibit very strong: a) oxidizing properties; c) restorative properties; b) amphoteric properties; d) neutral properties. In all their compounds, alkali metals exhibit an oxidation state: a) +1; c) +2; b) +3; d) +4. 6. The physical properties of alkali metals do not include: a) silvery-white; c) good electrical conductors; b) soft and light; d) refractory. 7. When elements of group I of the main subgroup interact with water, the following is formed: a) acid; c) oxide and hydrogen is released; b) alkali and hydrogen is released; d) salt. 8. When oxygen interacts with alkali metals, an oxide is formed only with: a) lithium; c) potassium; b) sodium; d) rubidium. 9. Alkali metals do not interact with: a) non-metals; c) water; b) acid solutions; d) concentrated acids. 10. Sodium and potassium are stored in kerosene or mineral oil because they: a) have a pungent odor; c) are easily oxidized in air; b) very light; d) strong oxidizing agents.
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2. Alkali metal hydroxides a) physical properties: b) chemical properties: Instructions Pour sodium hydroxide into a clean test tube, add a few drops of phenolphthalein. What are you observing? Add hydrochloric acid solution to the same test tube. What are you observing? Write down the reaction equation. Pour sodium hydroxide into a clean test tube and add copper sulfate solution. What are you observing? Write down the reaction equation. Carefully add sodium hydroxide to the test tube containing zinc hydroxide. What are you observing? Write down the reaction equation. Draw a conclusion about the chemical properties of alkali metal hydroxides.
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2. Alkali metal hydroxides c) application: Sodium hydroxide – NaOH – caustic soda, caustic soda, caustic. Potassium hydroxide - KOH - caustic potash. NaOH and KOH are caustic alkalis that corrode fabrics and paper
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3. Alkali metal salts baking soda potash table salt Glauber's salt crystalline soda Salt formula name application
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4. The importance of alkali metal compounds in the life of organisms Sodium and potassium ions play an important biological role: Na+ is the main extracellular ion, found in the blood and lymph, and K+ is the main intracellular ion. The ratio of the concentration of these ions regulates blood pressure in a living organism and ensures the movement of salt solutions from the roots to the leaves of plants. Potassium ions - support the functioning of the heart muscle, help with rheumatism, and improve intestinal function. Potassium compounds – eliminate swelling.
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An adult should consume 3.5 g of potassium ions per day with food. Task. 100g of dried apricots contains 2.034g of potassium. How many grams of dried apricots should you eat to get your daily requirement of potassium? Lesson summary: What physical and chemical properties are characteristic of oxides and hydroxides of alkali metals. Where are alkali metal hydroxides and salts used? Thank you for your work.
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Slide captions:
Metals C u, Au, Ag do not interact with water even when heated. Metals have electrical conductivity and thermal conductivity. Metals are characterized by a metallic crystal lattice. Metal atoms have 1-3 electrons in their outer level. Metal atoms have 1-3 electrons in their outer level. Metals are reducing and oxidizing agents. Metals are characterized by a metallic crystal lattice. Metals have electrical conductivity and thermal conductivity. When interacting with oxygen, metals accept electrons. All metals actively interact with acids. Metals C u, Au, Ag do not interact with water even when heated. Na, K belong to alkaline earth metals. Which statements are true:
Characterize Rb and C s according to its position in the Periodic System according to plan: a) position in the Periodic System; b) composition of the nucleus c) distribution of electrons across energy levels; d) degree of oxidation; e) formulas of oxide and hydroxide, their nature. Exercise 1
Alkali metals. Chemical properties. The most important compounds of alkali metals.
Alkali metals are good reducing agents. They interact with oxidizing agents: Nonmetals Water Acids
With oxygen Li + O 2 → Li 2 O lithium oxide Na + O 2 → Na 2 O 2 sodium peroxide Lithium, when burned in air, forms a basic oxide (the rest of the alkali metals form peroxides) Interaction with simple non-metallic substances
With halogens 2 Li + Cl 2 → 2 LiCl Lithium chloride 2 Na + Cl 2 → 2 NaCl Sodium chloride With sulfur 2 Li + S → Li 2 S lithium sulfide 2 Na + S → Na 2 S sodium sulfide With hydrogen Li + H 2 → LiH Na + H 2 → NaH
With water 2 Li + 2 H 2 O → 2 LiOH + H 2 Lithium hydroxide 2 Na + 2 H 2 O → 2 NaOH + H 2 Sodium hydroxide With acid solutions (equations are not usually written) 2Na + 2HCl → 2NaCl + H 2 2Li + 2HCl → 2LiCl + H 2 Interaction with complex substances
Me 2 O oxides are solids. They have pronounced basic properties: they interact with acidic oxides, water, and acids. MeOH hydroxides are white solids. Very hygroscopic. They dissolve well in water with the release of heat. They belong to alkalis. Interact with acids, acid oxides, salts, amphoteric oxides and hydroxides. The most important compounds of alkali metals
KOH – potassium hydroxide NaOH – sodium hydroxide LiOH – lithium hydroxide Alkali metal hydroxides What is the general formula of alkali metal hydroxides?
Alkali metal salts are solid crystalline substances of ionic structure. NaCl - rock salt Na 2 CO 3 - sodium carbonate NaHCO 3 - Sodium bicarbonate (baking soda) K 2 CO 3 - potassium carbonate (potash) Na 2 SO 4 10 H 2 O - crystalline sodium sulfate hydrate (Glauber's salt) NaNO 3 - saltpeter NaCl KCl – sylvinite Almost all sodium and potassium salts are soluble in water; Lithium sulfate, carbonate and fluoride are poorly soluble in water.
Melt electrolysis MeC l electric current Me + + C l - at the cathode: Me + + 1e Me 0 at the anode: C l - - 1e Cl 0 total process: 2Me Cl 2Me + Cl 2 Methods of production
What element are we talking about? They are usually stored in kerosene, and it runs on water, In nature, remember, from now on, It is not free anywhere, It is possible to open it in salts The flame turns yellow from it And you can get it from salt Just like Davy got it.
Write down the reaction equations for the interaction of potassium with oxygen, with bromine, with phosphorus, with water. Write an electron balance for these reactions. Task 2:
1.What new did you learn in class today, what did you learn? 2.What else would you like to know or study? 3.What did you like about the lesson and what didn’t you? 4.Your wishes to yourself, classmates, and teacher. Summarize:
§ 11, ex. 1,2,5 Homework
On the topic: methodological developments, presentations and notes
Lesson "Compounds of alkali metals."
Chemistry lesson in 9th grade using technology for developing critical thinking through reading and writing....
Presentation for the lesson: Compounds of alkali metals. Chemistry 9th grade.
1. The purpose of using the presentation “Compounds of alkali metals” in the lesson is to increase the motivation of students to study the properties of compounds of alkali metals and activate...
open lesson in 9th grade "Compounds of alkali metals"
The lesson was held in 9th grade. The topic of this lesson is the sixth in the “Metals” section. It was preceded by the study of alkali metals. Previously, the following topics were also studied: the position of metals in PSHE D.I. Mend...
