| Classification: | Heavy Metal |
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| Transport Package: | Packed in Wooden Cases/Iron Drums |
| Specification: | Rod, plate, pipe and wire |
| Trademark: | taixie |
| Origin: | China |
| Samples: |
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| Customization: |
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Product name: X - ray beryllium window, beryllium sheet
Grade: HIP-56 HP-56(B-1,B-2)
Purity Purity: 98% 99% 99.69% 99.9%
Technical parameters
The tensile strength is reduced to ≥320Mpa, the yield strength is reduced to 0.2≥220Mpa, the elongation is δ≥2%, and the elastic modulus is ≥300000Mpa. Beryllium has a small atomic weight, a high neutron float cross section and a high X-ray perspectivity.
Beryllium is the second major group element of the second period, with atomic number of 4 and element symbol Be. Beryllium is a kind of grayish alkali earth metal belonging to the hexagonal crystal system, hard and malleable. Beryllium and its compounds are highly toxic. Beryllium dissolves in both acid and lye, and is an amphoteric metal. Beryllium is mainly used in atomic reactor materials, aerospace engineering materials, various alloys, X-ray transmission Windows, etc. [3]
On October 27, 2017, beryllium was included in the list of Group 1 carcinogens published by the International Agency for Research on Cancer (IARC) of the World Health Organization (WHO).
Chinese name Beryllium [7] Foreign name Beryllium
BerylliumatomCAS login number 7440-41-7 [7] EINECS login number 231-150-7 [7] Melting point 1278 ºC [7] boiling point 2970 ºC [7] Water soluble insoluble water density 1.85g /cm³ outside View gray metal should be used for nuclear reactor materials, aerospace engineering materials, all kinds of alloys, X-ray transmission window and other safety description S53; S45 Hazard symbol T+ Hazard Description R49 Discovery Human Volkland element symbol Be Atomic weight 9.0121831 Atomic number 4 cycle second Group II Group A Region s electron configuration 1s22s2 Electronegativity 1.57 (Pauling scale) atomic radius 112pm Element Type Alkali Earth metals
directory
1 A brief history of discovery
2 Mineral Deposit Distribution
3 Physical and Chemical properties
4 isotope
5 Chemical Properties
▪ Anomalous properties of beryllium
▪ Product
▪ Comparison of properties of beryllium aluminum
▪ Toxicity
6 Application Fields
A brief history of discovery
In 1798, the French chemist Vauquelin Niclas Louis (1763~1829) discovered beryllium during the chemical analysis of beryl and emeralds. However, elemental beryllium was obtained thirty years later in 1828 by the German chemist Friedrich Woler (1800-1882) by reducing molten beryllium chloride with potassium metal.
Clapprote had analyzed greenstone from Peru, but he couldn't find beryllium. Bergman had also analyzed greenstone and concluded that it was a silicate of aluminum and calcium. At the end of the 18th century, chemist Vaucland, at the request of the French mineralogist Ayuyi, carried out a chemical analysis of chlorite and beryl. He found that the two were chemically identical, and discovered that they contained a new element called Glucinium, from the Greek glykys, meaning sweet, because the salts of beryllium are sweet. Vaucland presented his discovery of the new element to the French Academy of Sciences on February 15, 1798. Since yttrium's salts were also sweet, Weiler later named them Beryllium, after beryl, the main beryllium ore.
Mineral distribution editor broadcast
More than 30 beryllium-bearing minerals are known, but until 1968 only beryl was of industrial value. Beryl is a beryllium aluminosilicate with the general formula Be3Al2(SiO3)6, which theoretically contains nearly 14% BeO. In fact, the BeO content is generally 9-13%. Mainly produced in Brazil, Argentina, India, South Africa and so on. China's Xinjiang, Jiangxi and other places also produce. In 1968, beryllium was made from hydrated silica beryllium. The theoretical content of beryllium oxide in hydrous beryllium is 39~42%, but the industrial minerals are highly dispersed, the content of beryllium oxide is only 1.7~2.5%, mainly produced in the United States. [1]
Physical and chemical properties edited broadcast
Beryllium is a steel-gray metal light metal. Beryllium is harder than its Cousins, and unlike calcium, strontium, and barium, can be cut with a knife.
Specific heat capacity: 1.82J/gK
Heat of evaporation: 292.4KJ/mol
Heat of melting: 12.2KJ/mol
Conductivity: 0.313×106/cm
Thermal conductivity: 2.01 W/(cm·K)
Mohs hardness: 5.5
Atomic radius: 112 pm
Covalent radius: 90 pm
Vapor pressure: 4180Pa
Chemical properties
Beryllium, like lithium, forms a protective oxide layer in the air, so it is stable even when red hot in the air. Insoluble in cold water, slightly soluble in hot water, soluble in dilute hydrochloric acid, dilute sulfuric acid and potassium hydroxide solution and release hydrogen. Beryllium metal has significant corrosion resistance to sodium metal without oxygen even at higher temperatures.Beryllium has a +2 valence and can form polymers and a class of covalent compounds with significant thermal stability. [1]
Anomalous properties of beryllium
The valence shell structure of Be atom is 2s2, its atomic radius is 89pm, the ion radius of Be2+ is 31pm, and the electronegativity of Be is 1.57. Beryllium, due to its small atomic and ionic radii and relatively high electronegativity, tends to form covalent bonds rather than ionic compounds like other elements in its family. Beryllium, therefore, often exhibits anomalous properties that differ from other elements in its family.
(1) Beryllium is easy to form a dense protective film on its surface and does not react with water, while other metals in the same group, such as magnesium, calcium, strontium and barium, react with water easily.
(2) Beryllium hydroxide is amphoteric, while the hydroxides of other elements in the same group are moderately or strongly basic.
(3) Beryllium salts hydrolyze strongly to form tetrahedral ions [Be(H2O)2]2+. The strong Be-O bond weakens the O-H bond, so that the hydrated beryllium ion has a tendency to lose protons:
Beryllium salts are therefore acidic in pure water. The salts of other elements in the same group (except magnesium) have no hydrolysis. [2]
Product of products
1. Beryllium oxide
When beryllium is burned in oxygen, or when carbonates, nitrates and hydroxides of beryllium are heated and decomposed, white beryllium oxide BeO can be obtained. With a melting point of 2803K, BEO is insoluble in water or ethanol, and can be used as a high temperature resistant material. BeO is covalent and has a 44 zinc sulfide (sphalerite) structure. BeO is insoluble in water, but soluble in beryllium salts from acids and in beryllium salts from bases. BeO is an amphoteric oxide.
2. Beryllium hydroxide
Beryllium hydroxide is a white solid with low solubility in water. It is an amphoteric hydroxide that dissolves in acids to form Be2+ and in bases to form [Be(OH)4]2-.
3. Beryllium hydride
Be cannot be directly combined with H2 to form beryllium hydride, but beryllium hydride can be produced by reducing beryllium chloride with lithium aluminum hydride.
Beryllium hydride is a covalent compound with a structure similar to that of eborane, forming a hydrogen bridge bond between the two Be atoms.
Each Be atom is bonded to four H atoms, and each H atom makes two bonds. Since the Be atom has only 2 valence electrons, there are not enough electrons in the hydrogenated beryllium to form a normal electron pair bond (that is, two electrons shared between two atoms), and hydrogenated beryllium is an electron-deficient compound. Thus, in the Be-H-Be bridge bond, a "banana-shaped" three-center two-electron bond is formed. This is a cluster compound.
4. Beryllium chloride
Beryllium chloride is a covalent compound that absorbs moisture in air and smokes due to hydrolysis:
BeCl2+H2O=BeO+2HCl
Beryllium chloride sublimates and conducts no current. Anhydrous beryllium chloride is the polymeric type (BeCl
5. Beryllium sulfide
Beryllium sulfide (BeS) is an off-white powder with a relative density of 2.36. It can be obtained by the reaction of beryllium chloride and anhydrous hydrogen sulfide.
6. Beryllium carbide
Beryllium carbide (Be2C) is a yellow-red solid that decomposes in contact with water. It is obtained by the reaction of beryllium powder and high quality graphite powder. [2]
7. Beryllium complexes
Since beryllium is an electron-deficient atom, its halide is a Lewis acid that readily forms complexes or admixtures with electron pair donors. Therefore beryllium can form many complexes.
In 1923, the American physical chemist Lewis put forward the theory of acid-base electron that any substance that can accept electron pairs is called an acid, and any substance that can give electron pairs is called a base. An acid is an electron docking acceptor and a base is an electron pair donor.
Beryllium also produces a number of stable chelates. For example, evaporation of beryllium hydroxide with acetic acid yields basic beryllium acetate Be4O(CH3COO)6. This is a covalent compound in which four Be atoms surround a central O atom and six Ac- acetate roots are arranged along the six edges of the tetrahedron. The complex is covalent and can be distilled for the purification of beryllium.
In other chelates of beryllium, such as beryllium oxalate salts, naphthol complexes, and acetyl acetone complexes, beryllium atoms are tetrahedrally surrounded in these chelates. Beryllium compounds are extremely toxic due to their high solubility and the ease with which they form complexes. [1]
Comparison of properties of beryllium aluminum
In the periodic table, beryllium and group IIIA aluminum are located diagonally, and their properties are very similar.
1. Standard electrode potential is similar: both are active metals.
2. They are all oxygen-loving elements. The metal surface is easy to form an oxide protective film, and they are able to be passivated by thick HNO.
3. Both are amphoteric metals. Hydroxides are also amphoteric.
4. Both oxide BeO and Al2O3 have high melting point and high hardness.
5. BeCl2 and AlCl3 are both electron-deficient covalent compounds that form polymeric molecules through bridging bonds.
6. Beryllium salt, aluminum salt are easy to hydrolysis, hydrolysis is acidic.
7. Beryllium carbide Be2C, like Al4C3, hydrolyzes to produce methane.
Although Be and Al share many similar chemical properties, the two have very different physiological effects in the human body. The human body can contain a moderate amount of aluminum, but not a tiny amount of beryllium, and inhaling a small amount of BeO can be fatal. [1]
The toxicity of
Beryllium compounds such as beryllium oxide, beryllium fluoride, beryllium chloride, beryllium sulfide, beryllium nitrate are more toxic, while beryllium metal is relatively less toxic. Beryllium is a systemic poison. The degree of toxicity depends on the entry route, the physicochemical properties of different beryllium compounds, and the species of experimental animal. Generally speaking, soluble beryllium is more toxic than insoluble beryllium. The toxicity of intravenous injection was the highest, followed by respiratory tract, and the least by oral and percutaneous injection. After beryllium enters the body, insoluble beryllium oxide is mainly stored in the lungs and can cause pneumonia. Soluble beryllium compounds are mainly stored in bone, liver, kidney and lymph nodes. They can interact with plasma proteins to form protein complexes, which can cause lesions of organs or tissues and lead to cancer. Beryllium is excreted from human tissues very slowly. Therefore, beryllium and its compounds should be handled with extreme caution. [2]
Application Field editor broadcast
As a new material, beryllium has been paid more and more attention. Beryllium is an indispensable precious material in atomic energy, rocket, missile, aviation, space navigation and metallurgical industry.
1. Among all the metals, beryllium has the strongest X-ray transmission ability and is known as metallic glass. Therefore, beryllium is an irreplaceable material for manufacturing the small window of X-ray tube.
2. Beryllium is the treasure of the atomic energy industry. In atomic reactors, beryllium is a neutron source that can provide a large number of neutron shells (hundreds of thousands of neutrons per second); Beryllium has a strong slowing effect on fast neutrons, which allows the fission reaction to continue continuously, so beryllium is the best neutron reducer in atomic reactors. In order to prevent neutrons from escaping the reactor and endangering workers, the reactor has to be surrounded by a neutron reflector to force those neutrons that try to escape back into the reactor. Beryllium oxide not only reflects neutrons back like a mirror reflects light, but also has a high melting point and is particularly resistant to high temperatures, making it the best material for neutron reflecting layers in reactors.
3. Beryllium is an excellent aerospace material. For every kilogram added to the weight of the satellite, the total weight of the launch vehicle will increase by about 500kg. The structural materials used to make rockets and satellites need to be light and strong. Beryllium is lighter than aluminum and titanium and four times stronger than steel. Beryllium has high heat absorption ability and stable mechanical properties.
4. In the metallurgical industry, the bronze containing 1% to 3.5% of beryllium is called beryllium bronze, which has better mechanical properties than steel, good corrosion resistance and high electrical conductivity. It is used to make gossaws in watches, high-speed bearings, submarine cables and so on.
5. Beryllium bronze containing a certain amount of nickel does not produce sparks when it is hit. With this wonderful property, it can be used to make chisels, hammers and drills specially used in petroleum and mining industries to prevent fire and explosion accidents. Beryllium bronze containing nickel is not attracted by magnets and can be used to make anti-magnetic parts.
Most of the industrial beryllium is used in the production of beryllium copper alloys in the form of beryllium oxide, a small part is used in the form of beryllium metal, and a small amount is used in beryllium oxide ceramics. Before 1940s, beryllium was used as X-ray window and neutron source, etc. From the mid-1940s to the early 1960s, it was mainly used in the field of atomic energy, such as the use of beryllium to make neutron proliferation as the reflection layer of test reactors, accelerators and nuclear weapons components. In 1956, beryllium gyro was used for the first time in inertial navigation system, thus opening up an important field of beryllium application. In the 1960s beryllium's primary use shifted to the aerospace and aerospace fields, where it was used to make parts for aircraft.
X - rays have a high permeability to beryllium. Beryllium is a neutron source material because it produces neutrons when its nucleus is struck or irradiated by neutrons, particles, deuterons, and gamma rays. The thermal neutron absorption cross section of beryllium atom is 0.009 target en.
▪ Holmium (67) ▪ Erbium (68) ▪ Thulium (69) ▪ Ytterbium (70) ▪ Lutetium (71)
actinide
▪ Actinide (89) ▪ Thorium (90) ▪ protactinium (91) ▪ Uranium (92) ▪ neptunium (93)
▪ Plutonium (94) ▪ Americium (95) ▪ Curium (96) ▪ berkelium (97) ▪ CF (98)
Forced were (99) forced the fermium (100) forced the mendelevium (101) forced the nobelium (102) forced the lawrencium (103).
Transition metal
▪ Scandium (21) ▪ Titanium (22) ▪ Vanadium (23) ▪ Chromium (24) ▪ Manganese (25)
▪ Iron (26) ▪ Cobalt (27) ▪ Nickel (28) ▪ Copper (29) ▪ Zinc (30)
▪ Yttrium (39) ▪ Zirconium (40) ▪ Niobium (41) ▪ Molybdenum (42) ▪ Technetium (43)
▪ Ruthenium (44) ▪ Rhodium (45) ▪ Palladium (46) ▪ Silver (47) ▪ Cadmium (48)
▪ Hafnium (72) ▪ Tantalum (73) ▪ Tungsten (74) ▪ Rhenium (75) ▪ osmium (76)
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