1s. 2 2s. 2 2p. 6 3s. 2 3p. 6 3d. 10 4s. 2 4p. 5 .
Valence electrons are highlighted in bold. Refers to the family of p-elements. Since the largest main quantum number is 4th, and the number of electrons in the external energy level is 7, the bromine is located in the 4th period, the VIIIA group of the periodic table. The energy diagram for valence electrons has the form:
Germanium.
1s. 2 2s. 2 2p. 6 3s. 2 3p. 6 3d. 10 4s. 2 4p. 2 .
Valence electrons are highlighted in bold. Refers to the family of p-elements. Since the largest main quantum number is 4th, and the number of electrons in the external energy level is 4, Germanium is located in the 4th period, IVA group of periodic table. The energy diagram for valence electrons has the form:
Cobalt.
1s. 2 2s. 2 2p. 6 3s. 2 3p. 6 3d. 7 4s. 2 .
Valence electrons are highlighted in bold. Refers to the family of D-elements. Cobalt is located in the 4th period, the VIIB group of the periodic table. The energy diagram for valence electrons has the form:
Copper.
1s. 2 2s. 2 2p. 6 3s. 2 3p. 6 3d. 10 4s. 1 .
Valence electrons are highlighted in bold. Refers to the family of D-elements. Since the largest main quantum number is 4th, and the number of electrons in the external energy level is 1, the copper is located in the 4th period, I in the periodic table group. Energy diagram for valence electrons has the form.
chemical element, SN
Alternative descriptionsMetal protecting other metals from corrosion
Metal from which a resistant soldier was made in the Andersen fairy tale
Metal, which in excess can be mined from the surface of cans
Metal used as solder
Soft Dake Silver-White Metal
Soft metal used for soldering
One of the seven metals that Persians wore from the evil
Silver-white metal, soft and plastic
Soldier metal (fabulous)
Chemical Element, Soft Silver-White Metal
Latin "Stannum" (Stannum)
Metal for tinning
Cassiterid
Chemical element, metal
Metal, which caused the death of the expedition of Robert Scott to the South Pole
Silver droplet on the soldering iron
Metal for Ludiller
Soft Metal Rings Almanzora
Mixture of salts of this metal - "yellow composition" - has long been used as a dye for wool
What metal make a "white tin"?
The Latin name of this metal is translated as "solid", although it is one of the most soft and low-melting
Metal solder
Translate from Latin word "clan"
Foundation Stani
Material for persistent soldiers
Metal, "Stannum"
Heavy and soft metal
Lady metal
Soldiers, Metal
After India.
Metal for soldiers
Fragile frost metal
Soft metal
Twist lead
After India with Mendeleev
Metal, SN.
Coating cans
Component Cassiterita
Metal for persistent soldiers
Flesh of the toy army
Metal for soldering
. SN for Chemist
Metal Ludilleovikov
Cassiteritis is this whose ore?
Soldier metal (fairy tale.)
Metal Rings Almanzora
Latin "Stannum"
What makes "white tin"?
Droplet on a soldering iron
Metal as part of solders
Between India and antimony
Protective coating of tin
Metal, "Picky Chuma"
Mendeleev appointed it 60th
Soft and lightweight metal
Antimony predecessor in the table
Metal for spoons and soldiers
India successor in table
In the table he after India
Mendeleev determined it sixties
Following India in the table
Metal number sixty
Foil metal
Mendeleev appointed it sixties
Sixtieth Count Mendeleev
Metal wedding roses
Mendeleev prescribed it sixties
Metal as part of the Pewer
Metal for solder
Chemical element for soldiers
Antimony Final Table
In the table it is before antimony
Before antimony in the table
Metal soldering
Silver metal
. "Soft-fat" metal
Metal
Between India and antimony in the table
Fiftieth element
Going behind India in the table
SN in the table
Metal for soldier
Metal, killed Scott
Material for uniform buttons
Fiftieth metal in the table
To antimony in the table
The foundation of the medal for the fourth place for the US Championship Participants in figure skating
Fat India in Table
Material for soldiers
After India in the table
India follower
Metal with SN symbol
Metal toy soldiers
Chemical element called SN
Chemical element at a number of fifty
India follower in table
Chemical element, soft maquetty silver-white metal
Name of chemical element
. "SN" for chemist
. "Soft-fat" metal
What metal make "white tin"
What makes "white tin"
Cassiteritis is someone
Latin "Stannum"
The Latin name of this metal is translated as "solid", although it is one of the most soft and elbow
Mendeleev appointed it 60th in the table
Metal, "Picky Chuma"
Metal, "Stannum"
Translate from the Latin word "Stannum"
Latin "Stannum" (Stannum)
Mixture of salts of this metal - "yellow composition" - has long been used as a dye for wool
Cf. Kruzzzz (metal) ash-silver, white lead, very soft, lightweight, light weight, more comfortable for soldering and for casting simple small vessels; Star. Lead, from where the proverb: the word tin, uncessly. Pour tin, a saccine fortune. Only at the well done and the golden that the junk button! Tin mug or tin And the tin is m. Tin ore, cchedan, solder. Tin, tin m. Mixing, working tin dishes. Tin, Tin M. church. Tinsel, casting tin into water, for gadagna, predictions. Tin eyes, muddy and soulless; Tin eye, with lover. Tin m. Zap. pencil
Chemical. Element by "Surname" SN
What is the chemical element SN?
Chemical. Element by "Surname" SN
Tin (lat. Stannum; denotes symbol Sn) - element of the main subgroup of the fourth group, the fifth period of the periodic system of chemical elements D. I. Mendeleev, with atomic number 50. Refers to a group of light metals. Under normal conditions, a simply substance is plastic, a macked and low-melting brilliant silver-white metal. Tin forms two allotropic modifications: below 13.2 ° C is a resistant α-tin (gray tin) with a diamond type cubic lattice, above 13.2 ° C resistant β-tin (white tin) with a tetragonal crystal grille.
History
Tin was known to a person already in the IV millennium BC. e. This metal was lowered and roads, as it is rarely found among Roman and Greek antiquities. The tin is mentioned in the Bible, the fourth book Moses. Tin is (along with copper) one of the components of bronze (see the history of copper and bronze), invented at the end or middle of the 3rd millennium BC. e .. Since the bronze was the most durable of the metals and alloys known at that time, the tin was the "strategic metal" during the entire "bronze age", more than 2,000 years (very approximately: 35-11th century BC. er).
origin of name
The Latin name Stannum, associated with the Sanskrit word, meaning "resistant, durable", originally applied to the lead and silver alloy, and later to another, imitating its alloy containing about 67% tin; To the IV century, this word began to call the tin.
The word tin - general Slavonic, having conformity in the Baltic languages \u200b\u200b(cf. Lit. Alavas, Alvas - "Tin", Prusska. Alwis - "Lead"). It is a suffix formation from the root of OL- (Wed. Old Womennenec ELO - "Yellow", Lat. Albus - "White", etc.), so the metal is called color.
Production
In the process of production, the rudonal breed (cassiteritis) is exposed to crushing to the size of particles on average ~ 10 mm, in industrial mills, after which the cassiterite due to its relatively high density and mass is separated from the empty breed by the vibration and gravitational method on the processing tables. In addition, the flotation method of enrichment / cleaning ore is applied. The resulting concentrate of tin ore is smelted in the furnaces. In the process of smelting is restored to a free state by applying in the restoration of charcoal, the layers of which are stacked alternately with the layers of ore.
Application
1. Tin is used mainly as a safe, non-toxic, corrosion-resistant coating in pure form or in alloys with other metals. The main industrial applications of tin - in white tin (tinted iron) for the manufacture of food packaging, in soldiers for electronics, in house pipelines, in bearing alloys and in coatings made of tin and its alloys. The most important alloy of tin - bronze (with copper). Another famous alloy - Puteter - used for the manufacture of dishes. Recently, interest in the use of metal is reborn, since it is the most "environmental" among heavy non-ferrous metals. Used to create superconducting wires based on the NB 3 SN intermetallic compound.
2. The intermetallic compounds of tin and zirconium have high melting temperatures (up to 2000 ° C) and oxidation resistance when heating in air and have a number of applications.
3. Tin is an essential alloying component upon receipt of titanium structural alloys.
4. Tin dioxide is a very effective abrasive material used with the "finishing" of the optical glass surface.
5. A mixture of tin salts - "yellow composition" - previously used as a dye for wool.
6. Tin is also used in the chemical sources of current as an anode material, for example: a manganese-tin element, oxide-mercury-tin item. Perspectively use tin in a lead-tin battery; For example, with an equal voltage, compared with the lead battery, a lead-tin battery has 2.5 times greater capacity and 5 times greater energy capacity per unit volume, its internal resistance is significantly lower.
Light colored metal, simple inorganic substance. The Mendeleev table denotes SN, Stannum (Stannum). Translated from Latin this means "durable, persistent." Initially, this word was called the fusion of lead and silver, and only much later they began to call the pure tin. The word "Tin" has Slavic roots and denotes "white".
Metal refers to scattered elements, and not the most common on Earth. In nature, it is found in the form of various minerals. The most important for industrial production: Cassithiterita - Tin Stone, and Stannin - Tin Chered. Ore from ores, usually contain no more than 0.1 percent of this substance.
Properties of tin
Light soft plastic metal silver-white color. It has three structural modifications, it moves from the state of α-tin (gray tin) in β-tin (white tin) at a temperature of +13.2 ° C, and into the state of γ-tin at t +161 ° C. Modifications are very much different in their properties. α-tin - gray powder, which belongs to semiconductors, β-tin ("Normal Tin" at room temperature) - silver fork metal, γ-tin - white fragile metal.
In chemical reactions, Tin manifests polymorphism, that is, acidic and outfit properties. The reagent is quite inert in air and in water, as it is quickly covered with a solid oxide film that protects it from corrosion.
Tin easily enters the reaction with non-metals, with difficulty - with concentrated sulfur and hydrochloric acid; With these acids in the diluted state does not interact. With concentrated and dilute nitric acid reacts, but in different ways. In one case, tin acid is obtained, in the other - tin nitrate. Alkalis reacts only when heated. Oxygen forms two oxide, with a degree of oxidation 2 and 4. It is the basis of a whole class of tin-organ compounds.
Impact on the human body
Tin is considered safe for a person, it is in our body and every day we get it in the minimum quantities with food. His role in the functioning of the body has not yet been studied.
Tin pairs and its aerosol particles are dangerous, since with long and regular inhalation it can cause lung diseases; Poisonous are also organic compounds of tin, so it is necessary to work with it and its connections in the means of protection.
Such a tin compound as tin hydrogen, SNH 4, can cause severe poisoning when eating very old canned foods, in which organic acids have reacted with a tin layer on the walls of the cans (tin from which canning cans are made - this is a thin iron sheet, covered with two sides by tin). Poisoning with tin hydrogen may even be fatal. Its symptoms include cramps and a sense of equilibrium loss.
With a decrease in air temperature below 0 ° C, the white tin goes into a modification of a gray tin. In this case, the volume of substance increases by almost a quarter, the tin product cracks and turns into a gray powder. This phenomenon began to call "tin chum."
Some historians believe that the "tin plague" served as one of the reasons for the defeat of the Napoleon's army in Russia, since he turned the buttons on the clothes of French soldiers and belts for belts in powder, and thus had a demoralizing effect on the army.
But the real historical fact: the expedition of the English polar explorer Robert Scott ended in a tragically, including because all their fuel resulted out of the tall tanks, they lost their motorcycles, and did not have enough effort.
Application
Most of the solid is used in metallurgy for 
production of various alloys. These alloys go to the manufacture of bearings, foils for packing, white food tin, bronze, soldering, wires, timeline fonts.
- Tin in the form of foil (Stanol) in demand in the production of capacitors, dishes, art products, organ pipes.
- used to doping structural titanium alloys; To apply anti-corrosion coatings on iron and other metal products (s).
- The zirconium alloy has high refractory and resistance to corrosion.
- tin oxide (II) - is used as an abrasive when processing optical glasses.
- It is part of materials used for the manufacture of batteries.
- in the production of paints "under gold", dyes for wool.
- Artificial radioisotopes of tin are used as a source of γ-radiation in spectroscopic research methods in biology, chemistry, material science.
- Two-rod two-chip (tin salt) is used in analytical chemistry, in the textile industry for dyeing, in the chimprom for organic synthesis and production of polymers, in oil refining - for discoloration of oils, in the glass industry - for glass processing.
- Tin Borfluorian is used for the manufacture of tin, bronze, other necessary industry alloys; for tinning; lamination.
: Nashville - Opatsky. A source: t. XXIA (1897): Nashville - Opatsky, s. 889-893 () Other sources: Bean: MESS
Tin (Chem.; Lat. Stannum; Franz. Etain, it. Zinn; Chemical designation SN.) - Belongs to the number of metals known to humanity with deep antiquity. Egyptians knew him for 3000-4000 years before R. Kh. And he was stated in the Bible. In Nature, O. is mainly in the form of an oxygen compound SNO 2 - tin stone (see), less commonly occurs in the form of sulfur O. in a compound with sulfur iron or copper. O. has silver-white color, but darker silver. It is a bit of hard lead and very hard - when rolling gives extremely thin sheets, but the wire is easily rushing. In ordinary conditions, it has a clear crystal structure. When flexing the chopstick O., a characteristic sound is heard, which is explained by the gaps in the crystalline mass. Well-formed crystals O. It is easy to obtain, decomposing a weak current, for example, a solution of O. chloride in water (see below); It is easier for them, if on a strong solution of O. chloride, acidified with hydrochloric acid, pour water cautiously (so that it is not mixed with the solution) and immerse the tin plate here - the crystals of the separating fluid will begin to grow on it. As the crystals form, the plate in the lower part will be dissolved. Crystals seem to belong to the correct system. O. melts at 228 ° -232 °, and before that (about 100 °) becomes fragile, boils from 1460 ° to 1600 ° according to various sources. Coefficient Expans: Lin. between 0 ° and 100 ° \u003d 0.00002193 (Calvert-Johnson), cube. - V \u003d V o (L + 0.000061 t. + 0,0000000789t. 2) (Mattisen); The proportion of forged o. \u003d 7.3, crystalline \u003d 7.18. Heat capacity 0.05623 (Rheno). Thermal conductivity 14.5-15.4 (for silver \u003d 100). Electrical conductivity \u003d 11.45 at 21 ° (mattisen) (for silver \u003d 100). Interesting action on O. Low temperature. In Siberia, it was noted that gray spots appear in large frosts on the tin dishes, which are gradually growing. In these places, O. is done brittle, it is easily defined. Frieche cooled O. up to -35 ° and showed that the crystalline structure changes and the connectedness between its particles changes and is lost. When heated (freichest to 35 °), this O. goes into ordinary. The proportion of the changed O. \u003d 5.952 (Frichsh), so that the change of state is accompanied by a large increase in volume; The heat capacity was found 0.0545 (Rheno) - also less than for ordinary O. at ordinary temperature O. Almost does not change in dry or wet air; solutions of salts and very weak acids actually act on it; Thanks to this, it is used to prevent other metals (see the mezzani). When heated O. gives SNO 2 oxide; Couples are burning with a white flame. Strong hydrochloric acid, especially when heated, is easily dissolved by O. with the release of hydrogen and the formation of the chloride O. SNCl 2; The dissolution is better in the presence of platinum due to the formation of a galvanic pair. Sulfuric acid also dissolves O., while, depending on the acid fortress, heating, etc., an acid is decking: sulfur gas, hydrogen sulfide, sulfur, but hydrogen is obtained. Nitric acid is very strong on O. Does not operate, weaker, such as specific weight 1.4, energetically oxidizes it: nitrogen oxides are isolated and insoluble methaologic acid is formed; If nitric acid is weak and the action occurs slowly and in the cold, then O. goes into the solution - a nitric acid salt forms O., ammonia and hydroxylamine. Chlorine, bromine, iodine directly connected with O., with metals it gives alloys. When influencing O. decomposes water. Atomic weight O. about 118 (Meyer-Ceibert is considered to be 117.37; Van der Plaats - 118.07, etc.). In the periodic system of elements O. is placed in the IV group, in an odd row, together with silicon, Germany and lead. Like them, it gives mainly two rows of compounds of the SNX 2 and SNX 4 type; Here, the SNO also has the character of a weak base and SNO 2 oxide 2 -Character of weak acid. For O., compounds and intermediate types are known, Sn 2 x 6, A with oxygen O. also gives SNO 3.
Skill O. SNO is obtained from tin zaki hydrate, which, in turn, is obtained in the form of a white amorphous sediment when decomposing alkalis or their carbonic salts of O. SNCl 2 chloride. Cauccisi hydrate O. When heating or boiling with water, it highlights very easily water and goes into a black amorphous SNO powder. OK O. It is easily obtained in a crystalline form, when such a decomposition of the oxide hydrate occurs in the presence of alkalis (but not ammonia), weak acids, such as hydrochloric, acetic, some salts, such as the ammonia. Tin crooked hydrate is easily dissolved in alkalis Na (HO) and K (HO); From such solutions, due to the smaller SNO solubility in alkali, the dark shiny SNO crystals are allocated with a specific weight of up to 6.7. The speed of dehydration of the hydrate depends on the concentration of alkali and temperature. In very concentrated solutions or at boiling, a further reaction occurs: the separation of metal O. and the formation of oxide O. SNO 2, which gives salt alkali, for example SNO + KHO \u003d SN + K 2 SNO 3 + H 2 O. Obtaining crystalline Zakisi O. Under the action of weak hydrochloric acid, the hydrate is explained (Ditte) in such a way that a certain amount of O. SNCl 2 chloride is formed (determined by the degree of dissociation of it); It gives the chlorock O. and the last, decomposing water, gives SNO. Also acts ammonia. Zaku O. - especially in amorphous form it is easily oxidized into oxide; heated in the air burns; When influencing without access, the metal is distinguished by metallic O. and also goes into oxide: 2SnO \u003d Sn + SnO 2. Gyrat Zakisi O. has a different composition, depending on the drying. Indicate the existence of Sn (HO) 2 + H 2 O, 3SNO + 2N 2 O and so on. It is mentioned above. Zaku O. dissolves in alkalis, forming low-strength compounds; At the same time, it forms salt with acid acids and has the character of a weak base. Salts of Zakisi O. Malproof, are easily decomposed by water, moving to the main. Nitric acid easily dissolves the water hydrate about.; Dissolving it at 0 ° and then cooling up to -20 °, crystals are obtained, resembling the type of bertolet salt of the composition Sn (NO 3) 2 + 20H 2 O. When the solutions evaporates, a thick mass is obtained, which begins to decompose with the release of nitrogen oxides and the formation of the main salts. They decompose with water, when heated to 100 ° exploded. With sulfuric acid Zaku O. gives SNSO 4; It is also obtained by dissolving the hydrate B H 2 SO 4, crystallizes without water in the form of needles, it highlights sulfur gas during heating. Basic salts are also known. Salts of Zakisi O. Easily give double salts with alkali metal salts, for example, dual sulphate SNSO 4 k 2 SO 4 or 2SNSO 4 K 2 SO 4, etc.
Oxide O. SNO 2 is obtained in amorphous form when burning O. or oxidation of the molten O. in air, when calculating oxide hydrates O., etc. It represents a yellowish powder, hard-wave, specific weight 6,89-7,18; dissolves in alkalis when fusing and in strong sulfuric acid; The technique is used to produce dairy glass and elbow enamel. In nature, it is found in the form of crystals of tin stone (see), commonly painted iron traces, manganese, etc. Artificially crystals are obtained by influencing the amorphous SNO 2 in the jet of hydrogen chloride, when the water vapor is passed through the chlorine O. SNCl 4 when influencing, etc. Oxide O. has the character of little vigorous oxides, but acidic nature is more clear in it than the main one. It is responded with two acids, tin and methalo, rather sharply different among themselves, but capable of moving one to another, and two rows of salts. For SNO 2, it was necessary to expect a normal hydrate of SN (HO) 4; He is famous; It is also known, in addition, the SNO (HO) 2 hydrate (HO) 2 and many other intermediate between SNO 3 and normal hydrate. In this respect, O. great similarity with silicon; However, it is necessary to indicate in advance that the difference in the properties of tin acids does not depend on whether there is a hydrate with one water content or other; Their composition may be the same, and here it is probably the case of a real isomerism.
Tinic acid It turns out when decomposing a freshly prepared solution of chlorine O. SNCl 4 ammonia, alkalis, soda, chalk, coal-barium salt, etc., also directly when boiling SNCL 4 solutions 4 sufficient fortress; and with decomposition by acids with salts, such as tin-sodium Na 2 SNO 3. Methodic acid It turns out mainly under the action of a strong nitric acid on O., as well as from its salts. Both the same and the other acid has the appearance of white, loose mass, in an ordinary condition insoluble in water. Their distinction: 1) tin acid (in a wet state) is easily dissolved in nitric acid. Such a solution is lowly selected with tin acid in the form of pupils; when heated to 50 ° it is coagulated; If this clutch is treated with ammonia, it dissolves again in HNO 3. Methodic acid is not dissolved under these conditions. 2) tin acid is dissolved in sulfuric acid, even diluted, and does not stand out when boiling. Methodoic in weak H 2 SO 4 is not dissolved, and in a strong swelling; However, water is washed with acid. 3) Tinic acid dissolves in hydrochloric acid. Methalin insoluble; However, it is part of a part with hydrochloric acid. This compound is not soluble in HCl solutions, but soluble in clean water. 4) tin-soluble acid in Na (HO) and in excess of it; Metolay, both alkaline and acid solutions precipitated with an excess of Na (HO) in the form of a sodium salt, which is insoluble in the ridiculous sodra, but soluble in water. Methodoic acid goes into tin, for example, if it is handled by a strong hydrochloric acid and evaporate. The amount of aligned acid depends on the duration of treatment, the amount of hydrochloric acid, and so on.; If methalin acid is heated with a large amount of KHO or NaHO, a solid acid salt is formed. The transition of tin acid into methalo occurs, for example, if it is dried with an ordinary or elevated temperature, even when stored under water. Chlorine solution SNCL 4, if it is fresh, gives, as it said, tin acid; With a debt of storage, methaologic acid is obtained; When boiling with a lot of HCl, it also gives it. What explains the difference in tin acids, - exactly unknown; Some seize various polymers in them, for example, for tin acid hydrate SNO 2, a for methalo hydrate hydrate Sn 5 O 10; Other that they are formed by various hydrates, etc. Ordinary tin and methalo acid in water are insoluble, but soluble modifications are known for them, like soluble silicism. If the SNCl 4 solution is decomposed by caustically or to the tin-sodium salt add HCl and subjected to dialysis, then the student weight formed at the beginning, as salts are removed, it dissolves little. The last traces of alkali are removed by adding several drops of iodine solution. The resulting soluble tin acid during heating gives methalin acid. They have all the properties of soluble colloids, coincided from the insignificant increase of HCl and many salts, etc. Salts of tin acid (usually species m 2 SNO 3) for the most part well crystallized; Alkaline salts are soluble in water and are easily prepared by the dissolution of tin acid in alkalis. Salts of other metals are mostly insoluble and obtained by double decomposition with alkaline. Metalic acid salts are very poorly crystallized. Both those and other low-strength and easily decompose with the weak acids. For the technique, the tin-sodium and potassium salt are greater importance. Sodium salt Na 2 SNO 3 of the concentrated solutions is released from 3H 2 o in the form of rhombohedra, from the weak - from 10N 2 O. 67.4 parts of it dissolves at 0 °, at 20 ° - 61,3 parts; In alcohol insoluble. It has an application in a technique as a protrava (see Tinges). Potash salt K 2 SNO 3 + 3N 2 O is similar to sodium, which sometimes replaces. It is more soluble (in 100 parts of water at 10 ° 106.6 parts), oxide O. As the intermediate oxide also forms salts with acids. It is known to compound it with nitric acid, sulfur, phosphoric, arsenic, and so on. When dissolving tin acid in sulfur and evaporation, Sn (SO 4) 2 + 2H 2 O and basic, for example SO (HO) 2 SO 4, etc. similar to A nitric acid salt of tin oxide is also obtained. Acting on a strong solution of chloride O. SNCl 2 (with hydrochloric acid) barium peroxide WAO 2, the springs got a turbid liquid, which during dialysis gave handicoic acid H 2 O (SNO 3) 2. When heated above 100 ° it highlights oxygen.
Halogen compounds A. With Chlorine O. gives mainly SNCL 2 and SNCL 4. O. SNCl 2 chloride is formed when he is heated by O. in the HCl jet, when heated with a sulea or calm oil, and so on. SNCl 2 is a colorless substance, melting at 250 °, boils at 617-628 °. The density of a pair of V. Meyer up to 1113 ° indicates the existence of a mixture of SNCl 2 and Sn 2 Cl 4 in pairs, and with an increase in temperature, the number of the latter decreases. At high temperatures, a small decomposition occurs with chlorine is released. SNCl 2 is well soluble in water, which slightly decomposes it, with crystallization of such solutions, the SNCl 2 + 2n hydrate is obtained - in practice it is called the "tin salt" and is used in the dye for the dors. It is also obtained by direct dissolution of O. in hydrochloric acid; melts at 37.7 °. SNCl 2 solution has a high ability to react reactions and easily absorbs oxygen; nitric acid to chromium act oxidatively on it; Mercury, silver, gold salts are restored to them to metal, etc. SNCl 2 is capable of connecting with many substances. First of all, it gives a variety of chlorokises of the NSNCl 2 MSNO + QH 2 O. type. They are obtained by decomposition with water SNCL 2. In addition, SNCl 2 gives numerous double salts with chloride metals, for example SNCl 2 + 2NH 4 CL + H 2 O, SNCl 2 \u003d 2KCl + H 2 O, SNCl 2 BaCl + 4H 2 O and PR. Chlorn O. SNCL 4 is formed under the action of chlorine on the "Stanol" (the reaction is accompanied by a large heat release), when chlorine is compounded with SNCl 2, etc. It is a heavy colorless liquid of specific weight (0/4) 2.28, boils about 114 °, hardens About - 33 °. She smokes in the air (alchemists called Spiritus Fumans Libavii). SNCL 4 for many bodies serves as an excellent solvent. SNCl 4 can be considered as a complete chlorohydride Sn (HO) 4; With water, it eagerly connects and forms a range of SNCl 4 + 3N 2 O, SNCl 4 + 2 O, SNCl 4 + 2 O, SNCl 4 + 5H 2 O, etc. solutions, it is obtained under the action of royal vodka on O. with ethyl and amyl alcohol SNCL 4 Forms crystalline compounds. Like SNCl 2, Chlorine O. forms a series of chlorokises, which give that tin, then methaological acid. They can be considered as substitution products in various tin acids of water residues chlorine. SNCl 4 gives numerous double salts similar to what are indicated for SNCL 2. It is connected to PCL 5, nitrogen anhydride, cyanide hydrogen, ammonia, etc. with Bromo O. Gives SNBr 2 and SNBR 4; They are obtained similarly as indicated at SNCl 2 and SNCl 4. According to properties, they resemble SNCL 2 and SNCL 4. The same can be said about the iodide compounds O. SNI 2 and SNI 4, and the fluoride SNF 2 and SNF 4. Fluoride O. SNF 2 is obtained by dissolving in fluorine-hydrochloric acid SnO, A fluoride SNF 4 by dissolving SNO 2. When evaporation of SNF 4 solutions, it decomposes, but it gives excellent-formed double compounds K 2 SNF 6 + H 2 O, SNBAF 6 3N 2 O, etc., these salts are areomorphic with appropriate salts of silica hydrofluoric acid, and this gave the opportunity to establish the formula SiO 2 silica acids like tin acid SNO 2. There are also compounds of O., where chlorine and bromine, or chlorine and iodine, etc. are found at the same time, etc.
Sulfur connections O. Parallel SNO and SNO 2 O. gives gray SNS and SNS 2. One-tried tin SNS is obtained by the action of sulfur vapor to "Stanol", and a very energetic reaction with ignition occurs; When heating tin chips with gray; Since the reaction comes from the surface, the resulting mass is crushed and heated again with gray; For cleaning of sulfur traces or O., the product is made in a stream of hydrogen, SNS is also obtained by precipitating solutions of zaic compounds O. hydrogen sulfide and drying the resulting precipitate. When fusing a sediment with SNCl 2 and with further processing, the SNS is obtained in good crystals. In water, SNS is insoluble; water vapor when influencing decomposes it; amorphous, it is easily oxidized by nitric acid; Crystal, even at boiling, is very difficult. HCl gas decomposes it when heated; Saltic acid at ordinary temperature, depending on the concentration. Sulfur potassium dissolves little SNS at a weak concentration, with a greater (more than 20 parts of the salt by 100), the SNS transition is transition to SNS 2, which is connected to K 2 S, and O. It is distinguished by O. It is similar to the action of KHO on SNO. In a pure sulfur ammonium, SNS is not dissolved, but with multi-seiner incubates into the solution as connections corresponding to SNS 2. Alkali decompose it, for example, SNS + 2KHO \u003d SNO + K 2 S + H 2 O. When H 2 S is on neutral or weakly acidic solutions of o.Shur compounds, hydrochemical connections are obtained, when drying easily giving SNS. Soberous O. SNS 2 is obtained under the action of sulfur on O., if you do not give the reaction to go violently. Take usually 12 parts of O., 6 parts of mercury, 7 pieces of sulfur and 6 parts of the ammonia, put into a balloon and heated on a sand bath until white pairs stop standing out. Heating should be in moderation - not high and not weak, otherwise the SNS 2 color is bad. In the deposition of oxide salts O. hydrogen sulfide, in the presence of hydrochloric acid, a precipitate of hydrocarbon O., which, when drying, also gives SNS 2. Soberous O. in an anhydrous condition has a beautiful golden yellow color; It is the name of gravestone gold and goes for cheap gilding of a tree. SNS 2 during infection highlights sulfur. Chlorine when heated decomposes it, forming chloroserial compounds. When influencing in air goes into SNO 2. Soberous O., obtained during the precipitation with hydrogen sulfide dissolves in a strong hydrochloric acid when heated; On anhydrous nor salt, nor nitric acid act. It dissolves in royal vodka. Alkali caustic, carbon dioxide and sulfur dissolve SNS 2. Similarly, SNO 2 gives salts of the form M 2 SNO 3 and SNS 2 forms sulfosoli of the form M 2 SNS 3. Selenium and Tellur form similar compounds from O.
Metals O. gives numerous alloys, especially known alloys with copper (see Bronze). Many of them are wonderful in that they are melted at a very low temperature, for example, the Alloy d'Arc (2 parts of bismuth, 1 part of O. and 1 part of the lead), melts at 90 °; Rose alloy (8 pieces of bismuth. 3 parts Sn and 8 parts of lead) - at 95 °; Finally, Wood (15 pieces of bismuth, 4 parts Sn, 8 parts of lead, 3 pieces of cadmium) - at 68 °, etc., when analyzing O. is determined in the form of SNO 2.
Metallometallic connections O. (tin-organic or stannorganic compounds, stannalkyls) correspond to the types of SNX 2 and SNX 4, respectively, zakisi and oxide OU. And, moreover, another intermediate type Sn 2 x 6. As a form in the types of SNX 4 and SN 2 x 6, the counterparts of the corresponding compounds of carbon and silicon, compounds of O. detect the explicit differences due to the metal nature of this element, and in nature are approaching the real metallological compounds (see). In fact, there are no other bonds of the SN atom with carbon atoms, which is observed for silicon in its organic compounds, so that under the action of free halides instead of replacing hydrogen hydrocarbon residues, as is the case in silicon compounds, in the tin connections occurs The cleavage of the most residues, for example: Sn (CH 3) 4 + i 2 \u003d Sn (CH 3) 3 I + CH 3 I. The same, although more difficult, occurs even when heated with a strong hydrochloric acid, for example: Sn (C 2 H 5) 4 + HCl \u003d Sn (C 2 H 5) 3 Cl + C 2 H 6. Starnal buttons are formed under the action of iodide alkyls on O., taken in the form of a thin powder, or on the alloys of O. with sodium or zinc. Under action on pure O. or on O. with a small impurity of sodium, compounds with two hydrocarbon residues, the species Sn (R) 2 I 2, for example, Sn (C 2 H 5) 2 I 2 are preferably obtained. In the presence of a larger amount of sodium, the compounds Sn (R) 3 I and Sn (R) 4 are formed. The latter are very conveniently obtained by the action of cinorganic compounds on O. chloride, for example: 2SnCl 2 + 4ZN (C 2 H 5) 2 \u003d Sn (C 2 H 5) 4 + Sn + 4ZnCl (C 2 H 5). Acting with zincorganic compounds on the aforementioned iodide compounds, it is possible, by the way, to obtain stanabbles with different hydrocarbon radicals in composition, for example, Sn (C 2 H 5) 2 I 2 + Zn (CH 3) 2 \u003d Sn (C 2 H 5) 2 ( CH 3) 2 + ZNI 2. Stanntriethyl Sn 2 (C 2 H 5) 6 or (C 2 H 5) 3 Sn - Sn (C 2 H 5) 3 is obtained (similarly as a sodium) at SN (C 2 H 5) 3 I Equation: 2SN (C 2 H 5) 3 i + 2NA \u003d (C 2 H 5) 3 SN.SN (C 2 H 5) 3 + 2NAI; Standyethyl (Sn (C 2 H 5) 2) X - under the action of zinc on the compound Sn (C 2 H 5) 2 x 2 in an aqueous solution or, together with Sn 2 (C 2 H 5) 6, under the action of iodide ethyl Alloy O. with a large excess Na. Stantantraethyl, besides the above methods, it turns out even when heated to 150 ° Standiethyl: 2SN (C 2 H 5) 2 \u003d Sn (C 2 H 5) 4 + SN. Higher compounds O. SNR 4 is severe, colorless, with a weak ether smell of fluid, distinguishing without decomposition and insoluble in water. Stantanthramethyl Sn (CH 3) 4 boils at 78 °, specific gravity of 1.314 (0 °). Stantantraethyl Sn (C 2 H 5) 4 boils at 181 °, specific gravity 1,187 (23 °). Opened connections Sn (R) 3 I also liquid, colorless and volatile, have a sharp odor and even more specific weighing. Sn (CH 3) 3 boils at 170 °, specific gravity 2,143 (0 °). Sn (C 2 H 5) 3 I boils at 231 °, the specific gravity of 1.833 (22 °) is slightly soluble in water. Under the action of alkalis, they give hydrates of oxide Sn (R) 3 (OH), crystalline substances, volatile with water vapor, soluble in water with a strongly alkaline reaction and acids capable of forming salts. Sn (C 2 H 5) 3 (OH) boils at 272 ° and melted at 44. Of the corresponding salley (SN (CH 3) 3) SO 4 is easily soluble in water, Sn (C 2 H 5) 3 Cl is frozen on the cold oil shrill smell. Sn (C 2 H 5) 3 BR boils at 222-224 °, (Sn (C 2 H 5) 3) 2 SO 4 is difficult in water colorless prism soluble. In the distance of one-way compounds with sodium ethilat, derivatives that correspond to ether, for example, Sn (C 2 H 5) 3 (OC 2 H 5), boiling at 190-192 ° were obtained. Two-dyed compounds Sn (R) 2 I 2 crystal, soluble in water, especially in hot. Sn (CH 3) 2 I 2 - the prism of yellow, melted at 30 °, boiled at 228 °. Sn (C 2 H 5) 2 I 2 - colorless prisms, melt at 44.5 °, boiled at 245 °. With ammonia action they give white, amorphous, insoluble in water precipitation oxide Sn (CH 3) 2 O and Sn (C 2 H 5) 2 O, which with acids (salt, sulfur, acetic, etc.) are allowed soluble in water and well crystallizable salts, for example SN (CH 3) 2. CL 2 (40 ° melts, boils 188-190 °), Sn (C 2 H 5) Cl 2 (boils at 220 °), Sn (C 2 H 5) 2 .SO 4, SN (CH 3) 2 (C 2 H 3 O 2) 2. Stanntriethyl SN 2 (C 2 H 5) 6 represents a shrill smell liquid, specific gravity of 1,412 (0 °), boiling at 270 °, insoluble in water. The pair density is responsible for the written formula. As a substance of an intermediate type, Stanitriethyl easily passes into the highest-type compounds, connecting with halides, oxygen, as well as under the action of hydrochloric acid, and the connection between tin atoms occurs, for example: (C 2 H 5) 3 SN. Sn (C 2 H 5) 3 + i 2 \u003d Sn (C 2 H 5) 3 I + Sn (C 2 H 5) 3 I. Standyethyl (Sn (C 2 H 5) 2) X represents thick, severe, yellowish oil, insoluble in water, is quickly oxidized in air, forming Sn (C 2 H 5) 2 O, and with halides immediately connects, turning into the appropriate compounds of the highest Type. Compounds of O. with other radicals (C 3 H 7, C 4 H 9, C 5 H 11) were also obtained and studied by Kagur, Demars and Grimm. The study of the compounds described above belongs to Kahur, Frankland, Ladenburg, Lyovig, Bucton, Shtrekker, etc.
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