Atomic weight of the element: 26.98
Atomic volume: (cubic centimeters/mole)
10.0
Type of the element: Metal
Atomic number: 13
Symbol of the element: Al
Chinese name of the element: Aluminum
Concentration of the element in the sun. Content of the element in seawater: (ppm)
60
Content of the element in seawater: (ppm)
Pacific Ocean surface 0.00013
Element's English name: Aluminum
Relative atomic mass: 26.98
Content of the element in the Earth's crust: (ppm)
82000<
Number of protons in the nucleus: 13
Number of electrons outside the nucleus: 13
Nuclear electric nucleus number: 13
Oxidation state:
Main Al+3
Other Al0, Al+1
Proton mass: 2.1749E-26
Relative mass of protons: 13.091
Period: 3
Group number: IIIA
Molar mass: 27
Hydride: AlH3
Oxide: Al2O3
Highest valence oxide chemical formula: Al2O3
Density: 2.702
Melting point: 660.37
Boiling point: 2467.0
Flammability: 550 degrees Celsius
Thermal conductivity: W/(m-K)
237
Chemical bonding energy: (kJ /mol)
Al-H 285
Al-C 225
Al-O 585
Al-F 665
Al-Cl 498
Al-Al 200
Rate of propagation of sound in it: (m/S)
5000
Ionization energy (kJ/ mol)
M - M+ 577.4
M+ - M2+ 1816.6 <
M2+ - M3+ 2744.6
M3+ - M4+ 11575
M4+ - M5+ 14839
M5+ - M6+ 18376
M6+ - M7+ 23293
M7+ - M8+ 27457
M8+ - M9+ 31857
M8+ - M9+
M3+ - M2+ 1816.6
M9+ - M10+ 38459
Mohs hardness: 2.75
Peripheral electron arrangement: 3s2 3p1
Externally arranged electrons in the nucleus: 2,8,3
Crystalline structure: the crystal cell is a face-centered cubic cell, each cell contains 4 metal atoms.
Cell parameters:
a = 404.95 pm
b = 404.95 pm
c = 404.95 pm
alpha = 90°
beta = 90°
gamma = 90°
colour and state: silvery-white metal
atomic radius: 1.82
Common valence: +3
Discovered by: ?rsted, Wyler
Discovered in: 1825 Denmark
Elemental origin: the most abundant metal in the earth's crust, at more than 7%
Elemental use: can be used as structural material for airplanes, vehicles, ships, ships, rockets. Pure aluminum can be made of ultra-high voltage cables. Aluminum for daily utensils is often called "steel fine", "steel species"
Industrial production: electrolysis of a mixture of molten alumina and cryolite
Laboratory production: electrolysis of molten aluminum chloride
Other compounds: AlCl3-aluminum chloride NaAlO2-sodium meta-aluminate Al(OH)3-aluminum hydroxide
Extended description: bluish, silvery-white, trivalent metallic element, malleable, ductile and capable of making a [loud] sound, known for its lightness, good electrical and thermal conductivity, high reflectivity and resistance to oxidation.
Discovered by:
Discovery date:
Discovery process:
In 1827, Weiler of Germany made aluminum by ****heating potassium and anhydrous aluminum chloride.
Elemental description:
Silver-white lustrous metal, density 2.702 g/cm3, melting point 660.37 °C, boiling point 2467 °C. Composition ± 3. Has good thermal conductivity, electrical conductivity, and ductility, ionization energy 5.986 eV, although it is called active metal, but in the air its surface will form a dense oxide film, so that it can not continue to act with oxygen, water. At high temperatures can react with oxygen, releasing a large amount of heat, with this high reaction heat, aluminum can be replaced from other oxides in the metal (aluminum heat method). For example: 8Al + 3Fe3O4 = 4Al2O3 + 9Fe + 795 kcal, at high temperatures, aluminum also reacts with non-metals, can also be dissolved in acid or alkali to release hydrogen. It has no effect on water, sulfide, concentrated sulfuric acid, acetic acid of any concentration, and all organic acids.
Element Source:
Aluminum exists in various rocks or ores in the form of chemical compounds, such as feldspar, mica, kaolin, bauxite, alum, and so on. There are oxides of aluminum produced by fusion electrolysis with cryolite (Na3AlF6)****.
Elemental Uses:
Aluminum can replace metal from other oxides (Aluminum Heat Method). Its alloys are light and tough, and are used as structural materials in the manufacture of airplanes, rockets, and automobiles. Pure aluminum is used in large quantities in cables. It is widely used to make everyday utensils.
Elemental supporting information:
Aluminum in the earth's crust in the distribution of the amount of all the chemical elements after oxygen and silicon, accounting for the third, in all the metal elements in the first place. However, due to the strong oxidizing power of aluminum, it is not easy to be reduced, thus it was discovered late.
After the Italian physicist Volt created the battery in 1800, the British chemist David David and the Swedish chemist Betsy Rius tried to use electric current to separate aluminum from alumina-vanadium soil during 1808-1810, but were unsuccessful. Betsy Rius, however, gave the unobtainable metal the name alumien, from the Latin alumen. The term was used in medieval Europe as a general term for the astringent alum, a mordant used in dyeing cotton fabrics. It is from this that the later Latin name for aluminum, aluminium, and the symbol for the element, Al, derive.
In 1825, the Danish chemist Osder published his experiments on the production of aluminum, and in 1827, the German chemist Wüller repeated Osder's experiments and continued to improve the method of producing aluminum.
In 1854, the German chemist Devereux used sodium instead of potassium to reduce aluminum chloride, producing ingots of metallic aluminum.
Element symbol: Al English name: Aluminum Chinese name: aluminum
Relative atomic mass: 26.9815 Common valence: +3 Electronegativity: 1.61
Peripheral electron arrangement: 3s2 3p1 Extranuclear electron arrangement: 2,8,3
Isotopes and radioactivity: Al-26[730000y] * Al-27 Al-28[2.3m]
Electron affinity and energy: 48 KJ-mol-1
First ionization energy: 577.6 KJ-mol-1 Second ionization energy: 1817 KJ-mol-1 Third ionization energy: 2745 KJ-mol-1
Monominal density: 2.702 g/cm3 Monomers Melting point: 660.37 °C Boiling point of monomer: 2467 °C
Atomic radius: 1.82 angstroms Ionic radius: 0.51(+3) angstroms ***Valence radius: 1.18 angstroms
Common compounds: Al2O3 AlCl3 Al2S3 NaAlO2 Al2(SO4)3 Al(OH)3
Aluminum,Atomic number 13,atomic weight 26.981539. 182525 26.981539. In 1825 the Danish scientist Auster used anhydrous aluminum trichloride to act with potassium amalgam and evaporated the mercury to obtain aluminum; in 1854 Devereux used sodium metal to reduce the molten salts of sodium chloride and aluminum chloride to produce metallic aluminum, which was displayed at the Paris Exposition in 1855; in 1886 Hall and Eyre invented the molten-salt method of aluminum production by electrolysis of alumina and cryolite, respectively, to make aluminum a metal that could be metal for practical use. Aluminum is found in the earth's crust in 8 percent of the earth's surface, second only to oxygen and silicon. It is widely distributed in rocks, soil, animals and plants.
Aluminum is a silver-white light metal, melting point 660.37 ° C, boiling point 2467 ° C, density 2.702 g / cm? Aluminum is face-centered cubic structure, has good electrical and thermal conductivity; pure aluminum is softer.
Aluminum is an active metal, the surface of aluminum in dry air immediately form a dense oxide film about 50 ? thick, so that the aluminum will not be further oxidation and water resistance; but aluminum powder mixed with the air is extremely flammable; molten aluminum can react violently with water; high temperature can be many metal oxides are reduced to the corresponding metal; aluminum is amphoteric, that is, easily soluble in strong bases, but also soluble in dilute acids.
Aluminum has a wide range of applications.
Copper
Element name: copper
Element symbol: Cu
Element atomic weight: 63.55
Element type: metal element
Element content in the sun: (ppm)
0.7
Crystal structure: the cell is face-centered cubic cell, each cell contains 4 metal atoms.
Atomic volume: (cm3/mol)
7.1
Elemental content in seawater: (ppm)
Pacific Ocean surface 0.00008
Oxidation state:
Main Cu+2
Other Cu-1, Cu0, Cu+1, Cu+3. Cu+4
Cell parameters:
a = 361.49 pm
b = 361.49 pm
c = 361.49 pm
alpha = 90°
beta = 90°
gamma = 90°
Concentration in crust: (ppm)
50
Proton number: 29
Number of neutrons: 35
Atomic number: 29
Period to which it belongs: 3
Family to which it belongs: IB
Electronic layer distribution: 2-8-18-1
Moh's hardness: 3
Rate of sound propagation in it: (m/S)
3810
Density in general condition:8.9*10^3kg/m3
Discovered by:Discovery date:Discovery process:
Copper was found to exist in ancient times.
Elemental description
Metal with a purplish-red luster and a density of 8.92 g/cm3. melting point 1083.4±0.2 °C, boiling point 2567 °C. Common valency +1 and +2 (3-valent copper occurs only in a few unstable compounds). Ionization energy 7.726 eV. Copper is one of the earliest metals discovered by man and one of the best pure metals, slightly hard, extremely tough and resistant to wear. It also has good ductility. Thermal and electrical conductivity is good. Copper and some of its alloys have good corrosion resistance and are stable in dry air. But in the humid air in its surface can generate a layer of green alkaline copper carbonate [Cu2 (OH) 2CO3], which is called copper green. It is soluble in nitric acid and hot concentrated sulfuric acid, and slightly soluble in hydrochloric acid. It is easily eroded by alkali.
A Brief History of the Discovery of Copper
Copper is one of the metals that have been known since ancient times. It is generally believed that the first metal known to man was gold, followed by copper. Copper is very abundant in nature and is easy to process. Copper is the first metal used in human production, initially people only use the natural monomaterial copper that exists in nature, with a stone axe to cut it down, it can be hammered into a variety of artifacts. With the development of production, only the use of natural copper manufacturing tools are not enough to apply, the development of production prompted people to find a way to obtain copper from the copper ore. Copper-containing minerals are more common, most of them have bright and striking color, for example: golden yellow chalcopyrite CuFeS2, bright green malachite CuCO3Cu (OH) 2, dark blue lithic 2CuCO3Cu (OH) 2, etc., these ores in the air after the formation of copper oxide after roasting CuO, and then carbon reduction, you get the metal copper. Artifacts made of pure copper are too soft and easy to bend. It was discovered that by mixing tin into copper, a copper-tin alloy, bronze, could be made. Copper, COPPER, from Cuprum, is the ancient name of the island of Cyprus, famous for its copper production and long known to mankind. It and gold are the only two metals with colors other than gray, white and black. Alloys of copper and gold are used to make a variety of ornaments and utensils. The addition of zinc is brass; the addition of tin is bronze.
Elemental Sources
Chalcopyrite, chalcopyrite, chalcopyrite and malachite are important copper ores in nature. Copper is obtained by calcining sulfide ores and then fusing them with small amounts of silica and coke*** to obtain crude copper, which is then reduced to blister copper and finally electrolytically refined. A new method of extracting copper is being studied by crushing low-grade ore underground with atomic blasts, leaching it in situ with dilute sulfuric acid, then pumping the leach to the surface and precipitating the copper on iron filings.
Elemental uses
Copper is a non-ferrous metal with very close relationship with mankind, is widely used in electrical, light industry, machinery manufacturing, construction industry, defense industry and other fields, in China's consumption of non-ferrous metal materials, second only to aluminum.
Copper in the electrical and electronic industry is the most widely used, the largest amount, accounting for more than half of the total consumption. Used in a variety of cables and wires, motor and transformer winding resistance, switches and printed circuit boards.
In the manufacture of machinery and transport vehicles, used in the manufacture of industrial valves and fittings, instruments, plain bearings, molds, heat exchangers and pumps.
Widely used in the chemical industry in the manufacture of vacuums, distillation kettles, brewing kettles and so on.
In the defense industry for the manufacture of bullets, shells, gun parts, etc., the production of 1 million rounds of ammunition, need to use 13-14 tons of copper.
In the construction industry, used to make all kinds of pipes, pipe fittings, decorative devices.
The following is the proportion of copper consumption in each industry to the total consumption of copper: Industry Proportion of copper consumption to total consumption
Electronics (including communications) 48%
Construction 24%
General engineering 12%
Transportation 7%
Other 9%
Applications of Copper Properties
Conductivity: 64%, Corrosion Resistance: 23%, Structural Strength: 12%, Decorative: 1%
Elemental Supporting Information
The largest natural copper obtained in nature weighs 420 tons. In ancient times, people found natural copper, cut it down with stone axes, and processed it into objects by hammering. Copper was then squeezed into the ranks of stone tools and gradually replaced them, ending the Neolithic period of human history.
In China, the Xia Dynasty, 4,000 years ago, already began to use red copper, or natural copper. It was characterized by wrought and hammered. nearly 20 pieces of copperware were excavated twice in 1957 and 1959 at the site of the Imperial Niangniang Terrace in Wuwei, Gansu Province, and analyzed to contain as much as 99.63 to 99.87 percent copper, which is pure copper.
Of course, the production of natural copper is, after all, rare. The development of production promoted people to find ways to obtain copper from copper ore. The total content of copper in the earth's crust is not large, not more than 0.01%, but the copper-containing minerals are more common, most of them have a variety of bright and striking colors, attracting people's attention. For example, bright green malachite CuCO3.Cu (OH) 2, dark blue litharge 2CuCO3.Cu (OH) 2 and so on. These ores are burned in air to give copper oxides, which are then reduced with carbon to give copper metal.
In 1933, in the excavation of Yinxu in Anyang County, Henan Province, malachite weighing 18.8 kg, charcoal lumps with a diameter of more than 1 inch, ceramic general's helmet used for refining copper, and cinders weighing 21.8 kg were found, which illustrates that more than 3,000 years ago, China's ancient laboring people obtained copper from copper ore.
But objects made from smelted copper were too soft, easily bent and quickly dulled. Then people discovered that tin could be mixed into copper to make a copper-tin alloy, bronze. Bronze was much easier to smelt and make than pure copper, and harder than pure copper (if the hardness of tin is set at 5, then the hardness of copper is 30, and the hardness of bronze is 100-150), and history calls this period the Bronze Age.
China's Warring States period of writings, "Zhou Li - Kao Gong Ji" summarizes the experience of smelting bronze, bronze casting of a variety of different objects using different ratios of copper and tin: "Gold has six Qi (formula). Six points of its gold (copper) and tin in one, called the bells and tripods of the Qi; five points of its gold and tin in one, called the axe catty of the Qi; four points of its gold and tin in one, called the halberd of the Qi; three points of its gold and tin in one, called the big edge of the Qi; five points of its gold and tin in two, called the cut to kill the vector (arrows) of the Qi; half of the gold and tin, called the identification of the (mirrors) flint (the use of mirrors to catch the light to take the fire) of the Qi." This shows that more than 3,000 years ago, China's working people have recognized that the use of different bronzes require different properties, used to cast bronze metal composition ratio should also be different.
Bronze because of the hard, easy to melt, can be very good casting molding, stable in the air, and therefore even in the Bronze Age after the Iron Age, but also did not lose its use value. For example, in about 280 BC, Europe in the Aegean Sea on the island of Rhodes on the port of Rhodes stands of bronze sun god, up to 46 meters high, finger height more than adults.
China's ancient working people more earliest use of natural copper compounds for wet refining of copper, which is the origin of wet technology, is an invention in the history of world chemistry. Western Han Dynasty "Huainanzi - Wanbi technology" recorded: Zengqing get iron is transformed into copper. Zengqing is copper sulfate. This method is expressed in modern chemical formula:
CuSO4+Fe=FeSO4+Cu
Western legend has it that the ancient Mediterranean island of CYPRUS is a copper-producing place, and thus it gets its Latin name CUPRUM and its elemental symbol, Cu. The English word COPPER, and the Latin word CUIVRE, are all originated from this.
Copper has a unique conductive properties, aluminum can not be replaced, in today's electronic industry and the development of household appliances in the era, this ancient metal has restored its youth. Copper wire is being widely used. Products from abroad, an ordinary family car electronic and electric accessories required copper wire up to 1 kilometer, the French high-speed train tracks per kilometer with 10 tons of copper, Boeing 747-200-type aircraft in the total weight of copper accounted for 2%.
Element name: silver
Element symbol: Ag
Element English name: Silver
Latin original name: Argentum
Chinese is the metal metal gold character initials, plus Burgundy character form sound.
Element type: metallic element
Atomic volume: (cubic centimeter/mole) 10.3
Color and state: silver-white metal
Mohs' hardness: 2.5
Sound propagation rate in which: (m/S) 2680
Content
Element content in the sun: ( ppm)
0.001
Element's content in seawater:(ppm)
Surface of the Pacific Ocean 0.0000001
Content in the Earth's crust:(ppm)
0.07
Relative atomic mass: 107.9
Atomic number: 47
Proton Number: 47
Molar mass: 108
Period: 5
Family: IB
Electron level arrangement: 2-8-18-18-1
Common valence: +1
Monomer: silver
Monomer symbol: Ag
Oxidation state:
Main Ag+1
Oxygenation state:
Main Ag+1
Oxidizing state. Main Ag+1
Other Ag0, Ag+2, Ag+3
Ionization energy (kJ /mol)
M - M+ 731
M+ - M2+ 2073
M2+ - M3+ 3361
M3+ - M4+ 5000
M4+ - M5+ 6700
M5+ - M6+ 8600
M6+ - M7+ 11200
M7+ - M8+ 13400
M8+ - M9+ 15600
M9+ - M10+ 18000
Physical properties
Density: 11.7 g/ cm3
Melting point: 961.93°C
Boiling point: 2213°C
Other Properties:Rich in ductility, it is a metal with good thermal and electrical conductivity. The first ionization energy 7.576 e-volt. Chemically stable, not reactive to water and atmospheric oxygen; soluble in dilute nitric acid, hot concentrated sulfuric acid and hydrochloric acid, molten alkali hydroxide.
Crystal structure: the crystal cell is face-centered cubic cell, each cell contains 4 metal atoms.
Crystalline cell parameters:
a = 408.53 pm
b = 408.53 pm
c = 408.53 pm
alpha = 90°
beta = 90°
gamma = 90°
Chemical properties:
Silver is one of the metals discovered in ancient times. Although silver exists in nature as a single substance, the vast majority of it exists in a chemically complex state.
Silver is highly malleable, so it can be crushed into a transparent foil only 0.00003 centimeters thick, and one gram of silver grains can be drawn into a filament about two kilometers long.
Silver's thermal and electrical conductivity in the metal among the top.
Silver characteristics of the oxidation number of +1, its chemical properties than the poor copper, room temperature, and even when heated, not with water and oxygen in the air, but for a long time in the air can become black, lose the silver-white luster, this is because of the silver and the air in the synthesis of H2S black Ag2S's sake. The chemical reaction equation is:
4Ag + H2S + O2 = 2Ag2S + 2H2O
Silver can not react with dilute hydrochloric acid or dilute sulfuric acid to give off hydrogen, but silver can be dissolved in nitric acid or hot concentrated sulfuric acid:
Heating
2Ag + 2H2SO4 (concentrated) ==== Ag2SO4 + SO2↑ + 2H2O
Silver in normal room air can be heated up by the heat of the air. p>
Silver reacts slowly with halogens at room temperature, and halides can be produced under heating conditions:
473K
2Ag + F2 ===== 2AgF dark brown
heating
2Ag + Cl2 ===== 2AgCl↓ white
heating
2Ag + Br2 == === 2AgBr↓ Yellow
Heating
2Ag + I2 ===== 2AgI↓ Orange
Silver has a strong affinity potential for sulfur, and when heated, it can be directly chemosynthesized with sulfur to Ag2S:
Heating
2Ag + S ==== Ag2S