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Boron

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Boron Basic information
Boron Chemical Properties
  • Melting point:2300°C
  • Boiling point:2550°C
  • Density 2.34 g/mL at 25 °C(lit.)
  • storage temp. Storage temperature: no restrictions.
  • solubility H2O: soluble
  • form pieces
  • color Dark gray
  • Specific Gravity2.34~2.37
  • Resistivity1.5E12 μΩ-cm, 20 °C
  • Water Solubility insoluble H2O [MER06]
  • Merck 13,1333
  • Stability:Stable. Substances to be avoided include strong oxidizing agents and strong acids. May decompose on exposure to air - store under nitrogen. Highly flammable.
  • InChIKeyUORVGPXVDQYIDP-UHFFFAOYSA-N
  • CAS DataBase Reference7440-42-8(CAS DataBase Reference)
  • NIST Chemistry ReferenceBoron(7440-42-8)
  • EPA Substance Registry SystemBoron(7440-42-8)
Safety Information
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Boron Usage And Synthesis
  • DescriptionBoron was discovered by Sir Humphry Davy and J.L. Gay-Lussac in 1808. It is a trivalent non-metallic element that occurs abundantly in the evaporite ores borax and ulexite. Boron is never found as a free element on Earth. Boron appears as charcoal-grey pieces or black powder or as crystalline; is a very hard, black material with a high melting point; and exists in many polymorphs. Boron has several forms, and the most common one is amorphous boron, a dark powder, non-reactive to oxygen, water, acids, and alkalis. It reacts with metals to form borides. Boron is an essential plant micronutrient. Sodium borate is used in biochemical and chemical laboratories to make buffers. Boric acid is produced mainly from borate minerals by the reaction with sulphuric acid. Boric acid is an important compound used in textile products. The most economically important compound of boron is sodium tetraborate decahydrate or borax, used for insulating fibreglass and sodium perborate bleach. Compounds of boron are used in organic synthesis, in the manufacture of a particular type of glasses, and as wood preservatives. Boron filaments are used for advanced aerospace structures, due to their high strength and light weight.
  • Chemical Propertiescharcoal-grey pieces or black powder
  • Chemical PropertiesIn 1808, Sir Humphry Davy and J. L. Gay-Lussac discovered boron. It is a trivalent, nonmetallic element that occurs abundantly in the evaporite ores, borax and ulexite. Boron is never found as a free element on Earth. Boron as a crystalline is a very hard, black material with a high melting point, and exists in many polymorphs. Boron has several forms, the most common form being amorphous boron, a dark powder, non-reactive to oxygen, water, acids, and alkalis. It reacts with metals to form borides. Boron is an essential plant micronutrient. Sodium borate is used in biochemical and chemical laboratories to make buffers. Boric acid is produced mainly from borate minerals by the reaction with sulfuric acid. Boric acid is an important compound used in textile products. Compounds of boron are used in organic synthesis, in the manufacture of special types of glasses, and as wood preservatives. Boron fi laments are used for advanced aerospace structures owing to their high strength and light weight. It is used as an antiseptic for minor burns or cuts and is sometimes used in dressings. Boric acid was fi rst registered in the United States in 1948 as an insecticide for control of cockroaches, termites, fi re ants, fl eas, silverfi sh, and many other insects. It acts as a stomach poison affecting the insects’ metabolism, and the dry powder is abrasive to the insects’ exoskeleton. Boric acid is generally considered to be safe for use in household kitchens to control cockroaches and ants. The important use of metallic boron is as boron fi ber. Borate-containing minerals are mined and processed to produce borates for several industrial uses, i.e., glass and ceramics, soaps and detergents, fi re retardants and pesticides. The fi bers are used to reinforce the fuselage of fi ghter aircraft, e.g., the B-1 bomber. The fi bers are produced by vapor deposition of boron on a tungsten fi lament. Pyrex is a brand name for glassware, introduced by Corning Incorporated in 1915. Originally, Pyrex was made from thermal shock-resistant borosilicate glass. The common borate compounds include boric acid, sodium tetraborates (Borax), and boron oxide
  • Chemical PropertiesBoron is a yellow or brownish-black powder and may be either crystalline or amorphous. It does not occur free in nature and is found in the minerals borax, colemanite, boronatrocalcite, and boracite.
  • Physical propertiesBoron has only three electrons in its outer shell, which makes it more metal than nonmetal.Nonmetals have four or more electrons in their valence shell. Even so, boron is somewhatrelated to metalloids and also to nonmetals in period 2.
    It is never found in its free, pure form in nature. Although less reactive than the metalswith fewer electrons in their outer orbits, boron is usually compounded with oxygen andsodium, along with water, and in this compound, it is referred to as borax. It is also found asa hard, brittle, dark-brown substance with a metallic luster, as an amorphous powder, or asshiny-black crystals.
    Its melting point is 2,079°C, its boiling point is 2,550°C, and its density is 2.37 g/cm3.
  • IsotopesThere are a total of 13 isotopes of boron, two of which are stable. The stableisotope B-10 provides 19.85% of the element’s abundance as found in the Earth’s crust,and the isotope B-11 provides 80.2% of boron’s abundance on Earth.
  • Origin of NameIt is named after the Arabic word bawraq, which means “white borax.”
  • OccurrenceBoron is the 38th most abundant element on Earth. It makes up about 0.001% of theEarth’s crust, or 10 parts per million, which is about the same abundance as lead. It is notfound as a free element in nature but rather in the mineral borax, which is a compound ofhydrated sodium, hydrogen, and water. Borax is found in salty lakes, dry lake-beds, or alkalisoils. Other naturally occurring compounds are either red crystalline or less dense, dark-brownor black powder.
    Boron is also found in kernite, colemanite, and ulexite ores, and is mined in many countries,including the western United States.
  • CharacteristicsBoron is a semimetal, sometimes classed as a metallic or metalloid or even as a nonmetal.It resembles carbon more closely than aluminum. Although it is extremely hard in its purified form—almost as hard asdiamonds—it is more brittle than diamonds, thus limiting its usefulness. It is an excellentconductor of electricity at high temperatures, but acts as an insulator at lower temperatures.
  • HistoryBoron compounds have been known for thousands of years, but Boron was not discovered until 1808 by Sir Humphry Davy and by Gay-Lussac and Thenard. The element is not found free in nature, but occurs as orthoboric acid usually in certain volcanic spring waters and as borates in borax and colemanite. Ulexite, another boron mineral, is interesting as it is nature’s own version of “fiber optics.” Important sources of boron are the ores rasorite (kernite) and tincal (borax ore). Both of these ores are found in the Mojave Desert. Tincal is the most important source of boron from the Mojave. Extensive borax deposits are also found in Turkey. Boron exists naturally as 19.9% 10B isotope and 80.1% 11B isotope. Ten other isotopes of boron are known. High-purity crystalline boron may be prepared by the vapor phase reduction of boron trichloride or tribromide with hydrogen on 4-6 The Elements electrically heated filaments. The impure, or amorphous, boron, a brownish-black powder, can be obtained by heating the trioxide with magnesium powder. Boron of 99.9999% purity has been produced and is available commercially. Elemental boron has an energy band gap of 1.50 to 1.56 eV, which is higher than that of either silicon or germanium. It has interesting optical characteristics, transmitting portions of the infrared, and is a poor conductor of electricity at room temperature, but a good conductor at high temperature. Amorphous boron is used in pyrotechnic flares to provide a distinctive green color, and in rockets as an igniter. By far the most commercially important boron compound in terms of dollar sales is Na2B4O7 · 5H2O. This pentahydrate is used in very large quantities in the manufacture of insulation fiberglass and sodium perborate bleach. Boric acid is also an important boron compound with major markets in textile fiberglass and in cellulose insulation as a flame retardant. Next in order of importance is borax (Na2B4O7 · 10H2O) which is used principally in laundry products. Use of borax as a mild antiseptic is minor in terms of dollars and tons. Boron compounds are also extensively used in the manufacture of borosilicate glasses. The isotope boron-10 is used as a control for nuclear reactors, as a shield for nuclear radiation, and in instruments used for detecting neutrons. Boron nitride has remarkable properties and can be used to make a material as hard as diamond. The nitride also behaves like an electrical insulator but conducts heat like a metal. It also has lubricating properties similar to graphite. The hydrides are easily oxidized with considerable energy liberation, and have been studied for use as rocket fuels. Demand is increasing for boron filaments, a high-strength, lightweight material chiefly employed for advanced aerospace structures. Boron is similar to carbon in that it has a capacity to form stable covalently bonded molecular networks. Carboranes, metalloboranes, phosphacarboranes, and other families comprise thousands of compounds. Crystalline boron (99.5%) costs about $6/g. Amorphous boron (94–96%) costs about $1.50/g. Elemental boron and the borates are not considered to be toxic, and they do not require special care in handling. However, some of the more exotic boron hydrogen compounds are definitely toxic and do require care.
  • UsesIn nuclear chemistry as neutron absorber, in Ignitron rectifiers, in alloys, usually to harden other metals.
  • UsesBoron has found many uses and has become an important industrial chemical. Boron is used as an alloy metal, and when combined with other metals, it imparts exceptional strength to those metals at high temperatures. It is an excellent neutron absorber used to capture neutrons in nuclear reactors to prevent a runaway fission reaction. As the boron rods are lowered into the reactor, they control the rate of fission by absorbing excess neutrons. Boron is also used as an oxygen absorber in the production of copper and other metals, Boron finds uses in the cosmetics industry (talc powder), in soaps and adhesives, and as an environmentally safe insecticide. A small amount of boron is added as a dope to silicon transistor chips to facilitate or impede the flow of current over the chip. Boron has just three valence electrons; silicon atoms have four. This dearth of one electron in boron s outer shell allows it to act as a positive hole in the silicon chip that can be filled or left vacant, thus acting as a type of switch in transistors. Many of today s electronic devices depend on these types of doped-silicon semiconductors and transistors. Boron is also used to manufacture borosilicate glass and to form enamels that provide a protective coating for steel. It is also used as medication for relief of the symptoms of arthritis. Due to boron s unique structure and chemical properties, there are still more unusual compounds to be explored.
  • DefinitionA hard rather brittle metalloid element of group 3 (formerly IIIA) of the periodic table. It has the electronic structure 1s22s22p1. Boron is of low abundance (0.0003%) but the natural minerals occur in very concentrated forms as either borax (Na2B4O7.10H2O) or colemanite (Ca2B6O11). The element is obtained by conversion to boric acid followed by dehydration to B2O3 then reduction with magnesium. High-purity boron for semiconductor applications is obtained by conversion to boron trichloride, which can be purified by distillation, then reduction using hydrogen. Only small quantities of elemental boron are needed commercially; the vast majority of boron supplied by the industry is in the form of borax or boric acid.
    As boron has a small atom and has a relatively high ionization potential its compounds are predominantly covalent; the ion B3+ does not exist. Boron does not react directly with hydrogen to form boron hydrides (boranes) but the hydrolysis of magnesium boride does produce a range of boranes such as B4H10, B5H9, and B6H10. Thermal decomposition of these higher boranes produces, among other things, the simplest borane, B2H6 (diborane). The species BH3 is only a short-lived reaction intermediate.
    Finely divided boron burns in oxygen above 600°C to give the oxide, B2O3, an acidic oxide which will dissolve slowly in water to give boric acid (B(OH)3) and rapidly in alkalis to give borates such as Na2B4O7. A number of polymeric species with B–B and B–O links are known, e.g. a lower oxide (BO)x, and a polymeric acid (HBO2)n. Although the parent acid is weak, many salts containing borate anions are known but their stoichiometry gives little indication of their structure, many of which are cyclic or linear polymers. These contain both BO3 planar groups and BO4 tetrahedra. Boric acid and the borates give a range of glassy substances on heating; these contain cross-linked B–O–B chains and nets. In the molten state these materials react with metal ions to form borates, which on cooling give characteristic colors to the glass. See borax-bead test.
    Boron reacts with nitrogen on strong heating (1000°C) to give boron nitride, a slippery white solid with a layer structure similar to that of graphite, i.e., hexagonal rings of alternating B and N atoms. The material has an extremely high melting point and is thermally very stable but there is sufficient bond polarity in the B–N links to permit slow hydrolysis by water to give ammonia. There is also a ‘diamond-like’ form of B–N which is claimed to be even harder than diamond.
    Boron forms a range of compounds with elements that are less electronegative than itself, called borides. Borides such as ZrB2 and TiB2 are hard refractory substances, which are chemically inert and have remarkably high electrical conductivities. Borides have a wide range of stoichiometries, from M4B through to MB6, and can exist in close-packed arrays, chains, and two-dimensional nets. Natural boron consists of two isotopes, 10B (18.83%) and 11B (81.17%). These percentages are sufficiently high for their detection by splitting of infrared absorption or by n.m.r. spectroscopy. Both borax and boric acid are used as mild antiseptics and are not regarded as toxic; boron hydrides are however highly toxic.
  • Definitionboron: Symbol B. An element ofgroup 13 (formerly IIIB) of the periodictable; a.n. 5; r.a.m. 10.81; r.d.2.34–2.37 (amorphous); m.p. 2300°C;b.p. 2550°C. It forms two allotropes;amorphous boron is a brown powderbut metallic boron is black. Themetallic form is very hard (9.3 onMohs’ scale) and is a poor electrical conductor at room temperature. Atleast three crystalline forms are possible;two are rhombohedral and theother tetragonal. The element isnever found free in nature. It occursas orthoboric acid in volcanic springsin Tuscany, as borates in kernite(Na2B4O7.4H2O), and as colemanite(Ca2B6O11.5H2O) in California. Samplesusually contain isotopes in theratio of 19.78% boron–10 to 80.22%boron–11. Extraction is achieved byvapour-phase reduction of borontrichloride with hydrogen on electricallyheated filaments. Amorphousboron can be obtained by reducingthe trioxide with magnesium powder.Boron when heated reacts withoxygen, halogens, oxidizing acids,and hot alkalis. It is used in semiconductorsand in filaments for specializedaerospace applications.Amorphous boron is used in flares,giving a green coloration. The isotopeboron–10 is used in nuclear reactorcontrol rods and shields. Theelement was discovered in 1808 bySir Humphry Davy and by J. L. Gay-Lussac and L. J. Thenard.
  • DefinitionNonmetallic element of atomic number 5; group IIIA of the periodic table. Aw 10.81. Valence 3. Two stable isotopes: 11 (approximately 81%) and 10 (approximately 19%).
  • HazardVery toxic; industrial poison; causes depression of the circulation; persistent vomiting; diarrhea; shock and coma.
  • HazardPowdered or fine dust of elemental boron is explosive in air and toxic if inhaled. Several ofthe compounds of boron are very toxic if ingested or if they come in contact with the skin. Thisis particularly true of the boron compounds used for strong insecticides and herbicides.
  • Health HazardBoron has been studied extensively for its nutritional importance in animals and humans. There is a growing body of evidence that boron may be an essential element in animals and humans. Many nutritionists believe that people would benefi t from more boron and many popular multivitamins, such as centrum, in the diet. The adverse health effects of boron on humans is limited. However, ingestion/inhalation causes irritation to the mucous membrane and boron poisoning. Short-term exposures to boron in work areas are known to cause irritation of the eye, the upper respiratory tract, and the naso-pharynx, but the irritation disappears with the stoppage of further exposure. Ingestion of large amounts of boron (about 30 g of boric acid)over short periods of time is known to affect the stomach, intestines, liver, kidney, and brain and can eventually lead to death in exposed people.
  • Agricultural UsesBoron (B) is a non-metal occupying the first period and Group 13 (formerly, Ⅲ B) of the Periodic Table. Boron is essential for the growth of new cells. Its concentration in monocots and dicots varies between 6 to 18 ppm and 20 to 60 ppm, respectively. In most crops, the concentration of boron in mature leaf tissue is over 20 ppm.
    Boron is one of the seven micronutrients needed by plants. It exists in soils as a (a) primary rock and mineral, (b) mass combined in soil organic matter or adsorbed on colloidal clay and hydrous oxide surfaces, and (c) borate ion in solution. It occurs as borosilicate to the extent of 20 to 200 ppm in most semi-precious minerals that contain 3 to 4 % boron.
    Borosilicate contains varying amounts of iron (Fe), aluminum (Al), manganese (Mn), calcium (Ca), lithium (Li) and sodium (Na). As boron is resistant to weathering, its release from the mineral is slow and, therefore, it cannot meet the need of prolonged and heavy cropping.
    Though boron is essential for plants, its requirements and tolerances vary widely from plant to plant. It is required during (a) active cell division, (b) pollen germination, flower formation, fruit and root development, material transportation and cation absorption, (c) new cell development in meristematic tissue, (d) synthesis of amino acids and proteins, (e) nodule formation in legumes, ( f ) translocation of sugars, (g) polymerization of phenolic compounds, and (h) regulation of carbohydrate metabolism. Although boron is required for the growth of agricultural crops, it is not necessary for algae, diatoms, animals, fungi and microorganisms.
    Fruits, vegetables, and field crops may suffer from boron deficiency. The first visual symptom is cessation of terminal bud growth, followed by the death of young leaves. Boron deficiency restricts flowering and fruit development, and the symptoms are (a) thickened, wilted or curled leaves, (b) thickened, cracked or water-soaked condition of petioles and stems, and (c) discoloration, cracking or rotting of fruits, tubers or roots. The breakdown of internal root tissues gives rise to darkened areas, referred to as black or brown heart.
    The total boron content in soil varies from region to region and soil to soil. In Indian soils, for instance, the total boron content ranges between 4 and 630 mg/kg soil, while the available boron varies from traces to 68 mg/kg soil. Irrigation of arid and semi-arid soils with boron-rich water causes toxicity in plants, which can be reduced with the addition of organic matter.
    Boron is available in soils as an organic fraction and is released on decomposition to be partly absorbed by plants and partly lost during leaching. In soil solution, boron is present as a non-ionized molecule (H3BO3) which is absorbed by plant roots and distributed with the transpiration stream. The soil texture, pH and the moisture affect the movement of boron in soils. Coarsetextured sandy soils are low in boron and crops in such soils require additional boron in the form of borax, whereas crops in fine-structured sandy soils do not respond to the added boron. Fine-textured soils retain added boron for longer periods than coarse-textured soils. Clays retain boron more effectively than sands. Plant uptake of boron from clayey soils is larger than that from sandy soils.
    The soil pH influences the availability of boron; the higher the pH, the lower the boron uptake and the greater the deficiency. Generally, for the same type of crop, the application rate of a fertilizer containing water-soluble boron is lesser for coarse soils than for fine-textured sandy soils. Apple, alfalfa, asparagus, beet, celery, sunflower are some of the crops requiring high levels of boron (more than 0.5 ppm), whereas carrots, cotton, lettuce, peanuts, peach, sweet potato, tobacco and tomato need only 0.10 to 0.15 ppm of boron. The requirement of barley, beans, citrus, corn, forage grasses, soybeans and strawberry is lower than 0.1 ppm of the available soil boron.
    Interaction of boron with nutrients plays a vital role in the efficiency of the use of boron. For instance, boron is particularly effective with phosphorus, potassium and micronutrients, whereas its efficiency suffers with sodium, calcium and magnesium. For a good crop, it is essential to have a correct calcium to boron ratio.
    Boron compounds that are used to overcome boron deficiency are borax, boric acid, borosilicate glass or frits, calcium borate (Colemanite) and magnesium borate (Boracite). All boron materials used as fertilizers are stable chemicals and create no storage problem. The various methods by which boron is applied to plants are by drilling, broadcasting and spraying.
    The presence of boron in a fertilizer has to be clearly stated on the bag.
    Borax (Na2B4O7·10H2O) the most popular boroncontaining fertilizer. For most crops, 15 to 20 kg borax/ha is applied at the time of sowing or transplanting. As boron is readily leached out from the soil and the initial uptake of the plant is large, it is applied as a fused glass to reduce its solubility.
    Solubor, a commercial product, is a highly concentrated and completely soluble source of boron (20 %) like borax. It is preferred to borax and is applied as spray or dust directly to the foliage of fruit trees, vegetables and other crops. Colemanite, a naturally occurring calcium borate (Ca2B6O11·5H2O), is less soluble and is also superior to borax.
    Boron frits or borosilicate glass containing up to 6 % boron provide boron traces to plants. Borosilicate glass, due to its slow solubility, makes boron available for a longer time than borax. The finely ground form is more effective than the coarse variety.
    A dilute solution of boric acid and water is sprayed to be absorbed by the leaves.
  • Industrial usesBoron (symbol B) is a metallic element closelyresembling silicon. Boron has a specific gravityof 2.31, a melting point of about 2200°C, anda Knoop hardness of 2700 to 3200, equal to aMohs hardness of about 9.3. At 600°C, boronignites and burns with a brilliant green flame.Minute quantities of boron are used in steelsfor case hardening by the nitriding process toform a boron nitride, and in other steels toincrease hardenability, or depth of hardness. Inthese boron steels, as little as 0.003% is beneficial,forming an iron boride, but with largeramounts the steel becomes brittle and susceptibleto hot-short unless it contains titanium orsome other element to stabilize the carbon . Incast iron, boron inhibits graphitization and alsoserves as a deoxidizer. It is added to iron andsteel in the form of ferroboron.
    Boron compounds are employed for fluxesand deoxidizing agents in melting metals, andfor making special glasses. Boron, like siliconand carbon, has an immense capacity for formingcompounds, although it has a differentvalence. The boron atom appears to have a lenticularshape, and two boron atoms can make astrong electromagnetic bond, with the boronacting like carbon but with a double ring.
  • Industrial usesBoron has the atomic number 5 and the symbol B, and is a so-called metalloid. Boron compounds have been known for many centuries and especially used in the production of glass. At the beginning of the nineteenth century, it was recognised that boron is an essential micronutrient for plants. A deficiency of boron can lead to deformation in the vegetable growth such as hollow stems and hearts. Furthermore, the plant growth is reduced and fertility can be affected. In general, boron deficiency leads to qualitative and quantitative reduction in the production of the crop. Boron is typically available to plants as boric acid [B(OH)2] or borate [B(OH)4]-. The exact role of boron in plants is not understood, but there is evidence that it is involved in pectin cross-linking in primary cell walls, which is essential for normal growth and development of higher plants.
  • Potential ExposureBoron is used in metallurgy as a degasifying agent and is alloyed with aluminum, iron, and steel to increase hardness. It is also a neutron absorber in nuclear reactors. Boron is frequently encountered in a variety of chemical formulations including boric acid, various borate salts, borax, and boron soil supplements.
  • ShippingBoron powder or dust: UN3178 Flammable solid, inorganic, Hazard Class: 4.1; Labels: 4.1—Flammable solid.
  • IncompatibilitiesBoron dust may form explosive mixture in air. Contact with strong oxidizers may cause explosions. Violent reaction (possible explosion) with concentrated nitric acid, hydrogen iodide; silver fluoride. Boron is incompatible with ammonia, bromine tetrafluoride, cesium carbide, chlorine, fluorine, interhalogens, iodic acid, lead dioxide, nitric acid, nitrosyl fluoride, nitrous oxide, potassium nitrite, rubidium carbide. Reacts exothermically with metals at high temperature above 900° C.
  • Waste DisposalDispose of contents and container to an approved waste disposal plant. All federal, state, and local environmental regulations must be observed.
  • PrecautionsElemental boron is non-toxic and common boron compounds, such as borates and boric acid, have low toxicity (approximately similar to table salt with the lethal dose being 2–3 g/kg) and do not require special precautions while handling. Some of the more exotic boron hydrogen compounds, however, are toxic as well as highly flammable and do require special care when handling
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