Alkali metals are s-elements. On the outer electron layer, each of them has one electron (ns1). The atomic radii increase from top to bottom in the subgroup, the ionization energy decreases, and the reduction activity, as well as the ability to donate valence electrons from the outer layer, increases.

The metals under consideration are very active, therefore they are not found in nature in a free state. They can be found in the form of compounds, in the composition of minerals ( table salt NaCl, sylvinite NaCl∙KCl, Glauber's salt NaSO4∙10H2O and others) or in the form of ions in sea ​​water.

Physical properties of alkali metals

All alkali metals are silvery white under normal conditions. crystalline substances with high thermal and electrical conductivity. They have body-centered cubic packing (BCP). The densities, boiling and melting points of group I metals are relatively low. From top to bottom in the subgroup, densities increase and melting points decrease.

Obtaining alkali metals

Alkali metals are usually obtained by electrolysis of molten salts (usually chlorides) or alkalis. During the electrolysis of a NaCl melt, for example, pure sodium is released at the cathode, and gaseous chlorine is released at the anode: 2NaCl (melt) \u003d 2Na + Cl2.

Chemical properties of alkali metals

In terms of chemical properties, lithium, sodium, potassium, rubidium, cesium and francium are the most active metals and one of the strongest reducing agents. In reactions, they easily donate electrons from the outer layer, turning into positively charged ions. In compounds formed by alkali metals, ionic bonds predominate.

When interacting alkali metals with oxygen, peroxides are formed as the main product, and oxides as a by-product:

4Na+O2=2Na2O (sodium oxide).

With halogens they give halides, with sulfur - sulfides, with hydrogen - hydrides:

2Na+Cl2=2NaCl (sodium chloride),

2Na+S=Na2S (sodium sulfide),

2Na+H2=2NaH (sodium hydride).

Sodium hydride is an unstable compound. It decomposes with water, giving alkali and free hydrogen:

NaH+H2O=NaOH+H2.

Free hydrogen is also formed when alkali metals themselves interact with water:

2Na+2H2O=2NaOH+H2.

These metals also react with dilute acids, displacing hydrogen from them:

2Na+2HCl=2NaCl+H2.

Alkali metals react with organic halides by the Wurtz reaction.

“Lithium is the lightest metal; he has specific gravity 0.59, as a result of which it floats even on oil; melts at about 185°, but does not volatilize in red-hot heat. It resembles sodium in color and, like sodium, has a yellow tint.

D. I. Mendeleev. Fundamentals of chemistry.

When in 1817 the 25-year-old Swedish chemist Johan August Arfvedson (1792-1841) isolated a new “flammable alkali of a hitherto unknown nature” from the mineral petalite (it was lithium hydroxide), his teacher, the famous Swedish chemist Jens Jakob Berzelius (1779-1848), proposed to call it lithion, from the Greek. lithos - stone.

This alkali, in contrast to the already known sodium and potassium, was first discovered in the "kingdom" of stones. In 1818, the English chemist Humphrey Davy (1778-1829) obtained from "lithion" new metal which he named lithium. The same Greek root is in the words "lithosphere", "lithography" (an impression from a stone mold), etc.

Lithium is the lightest of the solids: its density is only 0.53 g/cm3 (half that of water). Lithium is obtained by electrolysis of a melt of lithium chloride. A rare property of metallic lithium is the reaction with nitrogen under normal conditions to form lithium nitride.

Lithium is increasingly used in the production of lithium-ion batteries. As a result, the world production of lithium in 2012 amounted to 37 thousand tons - five times more than in 2005.

Lithium compounds are used in the glass and ceramic industries. Lithium hydroxide - absorber of excess carbon dioxide in cabins spaceships and submarines. Lithium carbonate is used in psychiatry to treat certain disorders. The average human contains less than 1 mg of lithium.

Sodium

“The production of metallic sodium is one of the most important discoveries in chemistry, not only because the concept of simple bodies has thereby expanded and become more correct, but especially because in sodium Chemical properties, only weakly expressed in other well-known metals.

D. I. Mendeleev. Fundamentals of chemistry.

Russian name "sodium" (it is also in Swedish and German) comes from the word "natron": this is how the ancient Egyptians called dry soda, which was used in the mummification process. In the XVIII century, the name "natron" was assigned to the "mineral alkali" - caustic soda. Now soda lime is called a mixture of caustic soda and calcium oxide (in English soda lime), and sodium in English (and in many other languages ​​- sodium). The word "soda" comes from the Latin name of the plant hodgepodge (sodanum). It's coastal sea ​​plant, whose ash was used in the manufacture of glass in ancient times. This ash contains sodium carbonate, which is called soda. And now soda is the most important component of the charge for the production of most glass, including window glass.


Halite is the main mineral of sodium

The first person to see what metallic sodium looks like was G. Davy, who isolated the new metal by electrolysis. He also proposed the name of the new element - sodium.

Sodium is a very active metal; it quickly oxidizes in air, becoming covered with a thick crust of reaction products with oxygen and water vapor. A lecture experience is known: if a small piece of sodium is thrown into water, it will begin to react with it, releasing hydrogen. A lot of heat is released in the reaction, which melts the sodium, and its ball runs along the surface. Water cools the sodium and prevents the hydrogen from flaring up, but if the piece of sodium is large, a fire and even an explosion is possible.

Sodium metal is widely used in various syntheses as a reducing agent and also as a desiccant for non-aqueous liquids. It is present in high-capacity sodium-sulphur batteries. A low-melting alloy of sodium and potassium, liquid at room temperature, works as a coolant that removes excess thermal energy from nuclear reactors. Everyone knows the yellow color of the flame in the presence of sodium: this is how the flame of a gas burner is colored if the smallest drop of salty soup gets into it. Sodium vapor glows yellow in economical gas-discharge lamps that illuminate the streets.

For centuries, salt has been the only way to preserve food. Long-distance sea voyages would be impossible without table salt, round the world expeditions and great geographical discoveries. The history of Russia knows a grand uprising, called the Salt Riot, which began in 1648 and swept across the country. One of the reasons for the uprising is the increase in the tax on salt.

Once upon a time, hundreds of thousands of tons of sodium were produced per year: it was used to produce tetraethyl lead, which increases the octane number of gasoline. The ban on leaded gasoline in many countries has led to a decline in sodium production. Now the world production of sodium is about 100 thousand tons per year.

The mineral halite (sodium chloride) forms huge deposits rock salt. Only in Russia, its reserves amount to tens of billions of tons. Halite usually contains up to 8% other salts, mainly magnesium and calcium. More than 280 million tons of sodium chloride are mined annually, this is one of the largest productions. Sometime in large quantities Sodium nitrate was mined in Chile, hence its name - Chilean nitrate.

Other sodium salts, of which many are currently known, are also used. One of the most famous is sodium sulfate. If this salt contains water, it is called Glauber's. Huge amounts of it are formed during the evaporation of water in the Kara-Bogaz-Gol Bay of the Caspian Sea (Turkmenistan), as well as in some salt lakes. Currently, sodium sulfate solutions are used as a heat accumulator in devices that store solar energy, in the production of glass, paper, and fabrics.

Salt

Sodium is a vital element. Sodium ions are found mainly in the extracellular fluid and are involved in the mechanism of muscle contractions (a lack of sodium causes convulsions), in maintaining water-salt balance (sodium ions retain water in the body) and acid-base balance (maintaining a constant blood pH value). Produced from sodium chloride in the stomach hydrochloric acid, without which it is impossible to digest food. The content of sodium in the body of an average person is about 100 g. Sodium enters the body mainly in the form of table salt, its daily dose is 3-6 g. A single dose of more than 30 g is life-threatening.

Potassium

In Arabic, al-qili is ash, and also something calcined. They also began to call the product obtained from the ashes of plants, i.e. potassium carbonate. In sunflower ash, potassium is more than 30%. Without the Arabic article, this word in Russian turned into "potassium". In addition to Russian and Latin (kalium), this term has been preserved in many European languages: German, Dutch, Danish, Norwegian, Swedish (with Latin ending-um), in Greek (κάλιο), as well as in a number of Slavic languages: Serbian (Kalijum), Macedonian (Kalium), Slovenian (kalij).

Potassium is one of the most abundant elements in earth's crust. Its main minerals are sylvin (potassium chloride), sylvinite (mixed potassium and sodium chloride) and carnallite (mixed potassium and magnesium chloride). Silvin, as well as potassium nitrate (potassium, it is also Indian nitrate) in huge quantities used as potash fertilizers. Together with nitrogen and phosphorus, potassium is one of the three most important elements for plant nutrition.


Sylvin is one of the main potassium minerals (along with sylvinite and carnallite).

The element's English name is potassium, as is Russian name potassium carbonate (potash), borrowed from the languages ​​of the Germanic group; in English, German and Dutch ash is ash, pot is a pot, i.e. potash is “ash from a pot”. Previously, potassium carbonate was obtained by evaporating the extract from the ash in vats; it was used to make soap. Potassium soap, unlike sodium soap, is liquid. From the Arabic name for ash came the name of alkali in many European languages: English. and goll. alkali, German Alkali, French and ital. alcali etc. The same root is present in the word "alkaloids" i.e. "like alkalis").

Potassium was the first element discovered by G. Davy (he also received lithium, barium, calcium, strontium, magnesium and boron for the first time). Davy electrolyzed a wet lump of potassium hydroxide. At the same time, according to Davy, “small balls with a strong metallic sheen appeared on its surface, outwardly no different from mercury. Some of them, immediately after their formation, burned out with an explosion and with the appearance of a bright flame, while others did not burn out, but only dimmed, and their surface was covered with a white film. Potassium is a very active metal. His small piece, brought into the water, explodes.

Potassium is an important bioelement, the human body contains from 160 to 250 g of potassium, more than sodium. Potassium ions are involved in the passage of nerve impulses. Fruits and vegetables contain a lot of potassium.

Potassium hydroxide is used to make soap. It serves as an electrolyte in alkaline batteries - iron-nickel, nickel-metal hydride. Previously, potassium nitrate (potassium nitrate) was consumed in large quantities for the production of black powder; now it is used as a fertilizer.

Natural potassium contains 0.0117% of the long-lived radionuclide 40K with a half-life of 1.26 billion years. This explains the fact that potassium-40 "survived" to our time from the moment of its synthesis in nuclear reactions in stars. However, since the formation of the Earth 4.5 billion years ago, the content of 40K on the planet has decreased by 12.5 times due to its decay! A human body weighing 70 kg contains approximately 20 mg 40K, or 3 x 1020 atoms, of which more than 5000 atoms decay every second! It is possible that such "internal" irradiation (enhanced by the decay of carbon-14) was one of the causes of mutations in the course of the evolution of wildlife. World production metal potassium is small: about 200 tons per year.

rubidium and cesium

Rubidium and cesium are the first chemical elements, discovered with the help of spectral analysis. This method was developed by German scientists and friends - the physicist Gustav Robert Kirchhoff (1824-1887) and the chemist Robert Wilhelm Bunsen (1811-1899), who worked at the University of Heidelberg. With this extremely sensitive method, they analyzed all the substances they came across in the hope of finding something new. And in the early 1860s. discovered two new elements. This happened when they analyzed the dry residue obtained by evaporating water from the mineral springs of the Bad Dürkheim resort, 30 km from Heidelberg. In the spectrum of this substance, in addition to the lines of sodium, potassium and lithium already known to them, Kirchhoff and Bunsen noticed two weak blue lines. They realized that these lines belong to an unknown chemical element that is present in water in very small quantities. According to the light of the spectral lines, a new element

Continuing their research, Kirchhoff and Bunsen discovered in the aluminosilicate mineral lepido (lithium mica) sent to them from Saxony, one more element, in the spectrum of which dark red lines stood out. It was called rubidium: from lat. rubidus - red. The same element was found in mineral water, from where the chemist Bunsen managed to isolate it. It is worth mentioning that 44 tons had to be processed to obtain a few grams of rubidium salt. mineral water and over 180 kg of lepidolite.

Cesium crystals can be stored in a sealed ampoule.

And as in late XIX century, in no less titanic work on the isolation of radium salt, radioactivity served as a "compass" for Marie Curie, and a spectroscope was a similar "compass" for Kirchhoff and Bunsen.

Rubidium and cesium are typical alkali metals. This was confirmed when the chemist Bunsen, by reducing the salt of rubidium, obtained this element in the form of a metal. More active cesium was obtained in pure form only in 1881 by the Swedish chemist Carl Theodor Setterberg (1853-1941) by electrolysis of molten cesium cyanide. Cesium is one of the most fusible metals. In its pure form, it has a golden color. But it is not easy to obtain pure cesium: in air it instantly ignites spontaneously. Pure rubidium melts at only 39.3 °C, cesium - 10 degrees lower, and on a very hot summer day, samples of these metals in ampoules become liquid.

The world production of metallic rubidium is small - about 3 tons per year. Rubidium-87 is used in medicine: its atoms are absorbed by blood cells, and by the emission of fast electrons by them, with the help of special equipment, “bottlenecks” in the blood vessels can be seen. Rubidium is used in solar cells.

Gustav Kirchhoff (left) and Robert Bunsen discovered rubidium using a spectroscope. In the spectrum of lepidolite, they found dark red lines and gave the name to the new element - rubidium.

The body of a middle-aged person contains approximately 0.7 g of rubidium, and cesium - only 0.04 mg.

Electronic transitions in cesium atoms are used in extremely accurate "atomic clocks". All over the world there are now more than 70 such most accurate clocks - time standards: the error is less than a second in 100 million years. A cesium clock has a unit of time - a second.

It was proposed to use cesium ions to accelerate the rocket using an electric jet engine. In it, ions are accelerated in a strong electrostatic field and ejected through a nozzle.

Electrical rocket engines with low thrust, they are able to work for a long time and fly long distances.

France

This element was discovered (by its radioactivity) in 1939 by Marguerite Perey (1909-1975), an employee of the Radium Institute in Paris, and she named it in honor of her homeland in 1946.

Francium is a neighbor of cesium in the Periodic Table of the Elements. D. I. Mendeleev called the then undiscovered element - ekacesium. This last and heaviest alkali metal is strikingly different from all others in its group. Firstly, no one has ever seen and will not see even the smallest piece of France. Secondly, francium does not have such physical properties as density, melting point and boiling point. So the term "heaviest metal" can only be attributed to its atoms, but not to a simple substance. And all because francium is an artificially obtained highly radioactive element, its longest-lived isotope 223 Fr has a half-life of only 22 minutes. And to study physical properties substance, you need to have it in the form of at least the smallest piece. But for France it is impossible.

Marguerite Perey is the first woman elected (in 1962) to the French Academy of Sciences.

Francium is obtained artificially. And as it fuses, its atoms rapidly decay. Moreover, the more accumulated atoms, the more of them decays per unit time. So, in order to simply keep the number of francium atoms constant, they must be synthesized at a rate no less than the rate of their decay. During the synthesis of francium in Dubna by irradiating uranium with a powerful beam of protons, about a million atoms of this element were produced every second. At this rate of synthesis, the rate of decay of the sample becomes equal to the rate of its formation when the number of its atoms is equal to two billion. This is a completely negligible amount of substance, it is not even visible under a microscope.

In addition, these atoms are not assembled into a piece of metal, but are distributed over the surface of the uranium target. So it is not surprising that in everything the globe at any moment there will be no more than two or three tens of grams of francium scattered singly in radioactive rocks.

Alkali metals - common name elements of the 1st group of the periodic system of chemical elements. Its composition is lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), francium (Fr), and the hypothetical element ununenium (Uue). The name of the group comes from the name of soluble sodium and potassium hydroxides, which have the reaction and taste of alkali. Consider common features structures of atoms of elements, properties, production and use of simple substances.

Outdated and new group numbering

According to the outdated numbering system, alkali metals, occupying the leftmost vertical column of the periodic table, belong to I-A group. In 1989, the International Chemical Union (IUPAC) proposed a different option (long-period) as the main one. Alkali metals, in accordance with the new classification and continuous numbering, belong to the 1st group. The representative of the 2nd period, lithium, opens this set, and the radioactive element of the 7th period, francium, completes it. All metals of the 1st group have one s-electron in the outer shell of atoms, which they easily give up (recover).

The structure of alkali metal atoms

The elements of the 1st group are characterized by the presence of a second energy level, which repeats the structure of the previous inert gas. Lithium has 2 electrons on the penultimate layer, the rest have 8 electrons each. IN chemical reactions atoms easily donate an external s-electron, acquiring an energetically favorable configuration of a noble gas. Elements of the 1st group have small values ​​of ionization energy and electronegativity (EO). They easily form singly charged positive ions. In the transition from lithium to francium, the number of protons and electrons, the radius of the atom, increases. Rubidium, cesium and francium donate an outer electron more easily than the elements that precede them in the group. Consequently, in the group from top to bottom, the restorative capacity increases.

The easy oxidizability of alkali metals leads to the fact that the elements of the 1st group exist in nature in the form of compounds of their singly charged cations. The content in the earth's crust of sodium - 2.0%, potassium - 1.1%. Other elements in it are in small quantities, for example, francium reserves - 340 g. Sodium chloride is dissolved in sea water, brine of salt lakes and estuaries, forms deposits of rock or common salt. Along with halite, sylvinite NaCl occurs. KCl and sylvin KCl. Feldspar is formed by potassium aluminosilicate K 2 . Sodium carbonate is dissolved in the water of a number of lakes, and the reserves of the element's sulfate are concentrated in the waters of the Caspian Sea (Kara-Bogaz-Gol). There are deposits of sodium nitrate in Chile (Chilean saltpeter). There are a limited number of naturally occurring lithium compounds. Rubidium and cesium are found as impurities in compounds of elements of the 1st group, and francium is found in the composition of uranium ores.

Alkali metal discovery sequence

The British chemist and physicist G. Davy in 1807 carried out the electrolysis of alkali melts, for the first time obtaining sodium and potassium in a free form. In 1817, the Swedish scientist Johann Arfvedson discovered the element lithium in minerals, and in 1825 G. Davy isolated the pure metal. Rubidium was first discovered in 1861 by R. Bunsen and G. Kirchhoff. German researchers analyzed the composition of aluminosilicates and obtained a red line in the spectrum corresponding to a new element. In 1939, an employee of the Paris Institute of Radioactivity, Marguerite Pere, established the existence of an isotope of francium. She also named the element in honor of her homeland. Ununennium (eca-francium) is the provisional name for a new type of atom with atomic number 119. The chemical symbol Uue is temporarily used. Researchers since 1985 have been trying to synthesize a new element, which will be the first in the 8th period, the seventh in the 1st group.

Physical properties of alkali metals

Almost all alkali metals are silvery white and have a metallic luster when freshly cut (cesium is golden yellow). In air, the luster fades, a gray film appears, on lithium it is greenish-black. This metal has the highest hardness among its neighbors in the group, but is inferior to talc, the softest mineral that opens the Mohs scale. Sodium and potassium are easily bent, they can be cut. Rubidium, cesium and francium in their pure form represent a pasty mass. The melting of alkali metals occurs at a relatively low temperature. For lithium, it reaches 180.54 °C. Sodium melts at 97.86°C, potassium at 63.51°C, rubidium at 39.32°C, and cesium at 28.44°C. The density of alkali metals is less than their related substances. Lithium floats in kerosene, rises to the surface of the water, potassium and sodium also float in it.

Crystal state

Crystallization of alkali metals occurs in the cubic syngony (body-centered). The atoms in its composition have a conduction band, on free levels which electrons can transfer. It is these active particles that carry out a special chemical bond- metal. Generality of the structure energy levels and the nature of the crystal lattices explain the similarity of the elements of the 1st group. In the transition from lithium to cesium, the masses of the elements' atoms increase, which leads to a regular increase in density, as well as to a change in other properties.

Chemical properties of alkali metals

The only external electron in alkali metal atoms is weakly attracted to the nucleus, so they are characterized by low ionization energy, negative or close to zero electron affinity. Elements of the 1st group, having reducing activity, are practically incapable of oxidizing. In the group from top to bottom, activity in chemical reactions increases:

Production and use of alkali metals

Metals belonging to the 1st group are produced in industry by electrolysis of melts of their halides and other natural compounds. When decomposed under the action electric current positive ions at the cathode gain electrons and are reduced to the free metal. The anion is oxidized at the opposite electrode.

During the electrolysis of hydroxide melts, OH particles are oxidized at the anode, oxygen is released and water is obtained. Another method is the thermal reduction of alkali metals from the melts of their salts with calcium. Simple substances and compounds of elements of the 1st group are of practical importance. Lithium serves as a raw material in nuclear power engineering and is used in rocket technology. In metallurgy, it is used to remove residuals of hydrogen, nitrogen, oxygen, and sulfur. Hydroxide supplement electrolyte in alkaline batteries.

Sodium is needed for nuclear energy, metallurgy, organic synthesis. Cesium and rubidium are used in the manufacture of solar cells. Hydroxides and salts, especially chlorides, nitrates, sulfates, carbonates of alkali metals, are widely used. Cations have biological activity, sodium and potassium ions are especially important for the human body.

Chemistry studies the properties of metals and non-metals. Did you know that there are alkaline and non-alkaline metals? And we not only know, but we will also give you a list for successful preparation in the subject of chemistry. So, the list of alkali metals is already given in the periodic table of Mendeleev. There, all the metals of the main subgroup in the first group are alkaline.

These are lithium, potassium, sodium, cesium, rubidium and francium. Only these metals are called alkaline. And they are called so because if they interact with water, then alkalis are formed as a result.

There is another type of metal - it is alkaline earth. If you want a list of only alkali metals, then there are only 6 metals. If all metals, the hydroxides of which have alkaline properties, then four more elements will enter - calcium, strontium, barium and radium.

It is difficult to find all alkali metals in their pure form in nature - after all, they easily enter into compounds. In particular, these metals are found in the form of these compounds.

Properties of alkali metals

Alkali metals are excellent conductors of heat and are good conductors of electricity.

Alkali metals have low temperature melting

The density of metals increases with increasing number, but it becomes easier to melt them if the metals are at the bottom of the group.

Obtaining alkali metals

Usually alkali metals are obtained by electrolysis, however, two alkaline earth metals, strontium and barium, are obtained using the aluminothermic method.

Chemical properties

As we said, these metals are very active, they are also excellent reducing agents. They are found in the form of compounds in which the ionic bond will be the main one.

As a rule, they always form stable compounds. The main reactions and additional properties of alkali metals are given in the table:

So, now, using the list and table, as well as the periodic system of Mendeleev, you can tell a lot about alkali metals.

You can see what alkali metals look like. There is also a list and given bond reactions with water, sulfur, acids, salts and halogens.

Chem. elements (alkaline elements) that make up Ch. subgroup 1 group periodic. systems of elements, as well as the corresponding simple substances metals. Shch. m. include lithium Li (at. number 3), sodium Na (11), potassium K (19), rubidium Rb (37), tse ... Physical Encyclopedia

ALKALI METALS, monovalent metals that make up the first group of the periodic table: lithium, SODIUM, RUBIDIUM, CAESIUM and FRANCE. These are soft, silvery-white metals that quickly oxidize in air and react violently with water when ... ... Scientific and technical encyclopedic dictionary

alkali metals- ALKALI METALS: lithium Li, sodium Na, potassium K, rubidium Rb, cesium Cs, francium Fr. Soft metals, easy to cut (except Li), Rb, Cs and Fr almost pasty under ordinary conditions; Li is the lightest of all metals, Na and K are lighter than water. Chemically very... Illustrated Encyclopedic Dictionary

Chemical elements Li, Na, K, Rb, Cs, Fr. Name from alkali hydroxides of alkali metals ... Big encyclopedic Dictionary

ALKALI METALS- elements of group I of the periodic system: lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), francium (Fr); very soft, ductile, fusible and light, usually silvery white color; chemically very active; react violently with... Russian Encyclopedia on labor protection

alkali metals- Group, incl. Li, Na, K, Rb, Cs, Fr. Topics metallurgy in general EN alkali metals … Technical Translator's Handbook

SUB-GROUP IA. ALKALI METALS LITHIUM, SODIUM, POTASSIUM, RUBIDIUM, CESIUM, FRANCE Electronic structure alkali metals is characterized by the presence on the outer electron shell of one electron, relatively weakly associated with the nucleus. From each ... ... Collier Encyclopedia

Alkali metals Alkali metals. Metals of the first group Periodic system, namely: lithium, sodium, potassium, rubidium, cesium and francium. They form strictly alkaline hydroxides, hence their name. (Source: "Metals and Alloys. Handbook." Under ... ... Glossary of metallurgical terms

alkali metals Encyclopedic Dictionary of Metallurgy

ALKALI METALS- chemical elements Li, Na, K, Rb, Cs, Fr. So named because their hydroxides are the strongest alkalis. Chemically, alkali metals are the most active metals. Their activity increases from Li to Fr... Metallurgical Dictionary

Books

  • A set of tables. Chemistry. Metals (12 tables) , . Educational album of 12 sheets. Art. 5-8683-012 Alkali metals. Chemistry of alkali metals. Elements II A - groups. Hardness of water. Aluminum. The use of aluminium. Iron. Types of corrosion. Methods…