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| Atomic symbol: Pt |
| Atomic number: 78 |
| Atomic weight: 195.09 |
| Atomic volume: 9.10 cm3/mol |
| Density: 21.45 g/cm3 |
| Period Number: 6 |
| Group number: 10 |
| Group name: Trans. Met. |
| Element classification: Metal |
| Phase at room temperature: Solid |
| Melting Point: 2045.2 K |
| Boiling point: 4443 K |
| Heat of fusion: 19.60 kJ/mol |
| Heat of vaporization: 510.0 kJ/mol |
| Ionization Energy: 9.0 eV |
| 1st ionization energy: 870 kJ/mole |
| 2nd ionization energy: 1791 kJ/mole |
| 3rd ionization energy: kJ/mole |
| Electronegativity: 2.28 |
| Electron affinity: 205.3 kJ/mole |
| Specific heat: 0.13 J/gK |
| Heat atomization: 565 kJ/mole atoms |
| Shells: 2,8,18,32,17,1 |
| Electron Shell Configuration: [Xe] 4f14 5d9 6s1 |
| Minimum oxidation number: 0 |
| Maximum oxidation number: 6 |
| Minimum common oxidation number: 0 |
| Maximum common oxidation no: 4 |
Appearance & Characteristics |
| Structure:: fcc: face-centered cubic |
| Color: silvery-white |
| Hardness: 4.3 mohs |
| Toxicity: ? |
| Characteristics: Inert, ductile |
| Uses: jewelry, catalysts |
| Reaction with air: none |
| Reaction with 6M HCl: none |
| Reaction with 15M HNO3: none |
| Reaction with 6M NaOH: none |
| Number of isotopes: 6 |
| Oxide(s): PtO2 |
| Hydride(s): none |
| Chloride(s): PtCl2 PtCl4 |
| Atomic Radius: 139 pm |
| Ionic radius (1- ion): pm |
| Ionic radius (1+ ion): pm |
| Ionic radius (2- ion): pm |
| Ionic radius (2+ ion): 94 pm |
| Ionic radius (3+ ion): pm |
| Thermal conductivity: 71.6 J/m-sec-deg |
| Electrical conductivity: 94.34 1/mohm-cm |
| Polarizability: 6.5 A^3 |
| Source: nickel ores (sulfides) |
| Relative abundance solar system: 0.127 log |
| Abundance earth's crust: -2.3 log |
| Estimated crustal abundance: 5×10-3 milligrams per kilogram |
| Estimated oceanic abundance: No Data Available |
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| (Sp. platina: silver) Discovered in South America by Ulloa in 1735 and by Wood in 1741. The metal was used by pre-Columbian Indians. |
Platinum occurs natively, accompanied by small quantities of iridium, osmium, palladium, ruthenium, and rhodium, all belonging to the same group of metals. These are found in the alluvial deposits of the Ural mountains, of Columbia, and of certain western American states. Sperrylite, occurring with the nickel-bearing deposits of Sudbury, Ontario, is the source of a considerable amount of metal.
The large production of nickel makes up for the fact that is only one part of the platinum metals in two million parts of ore.
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Platinum is a beautiful silvery-white metal, when pure, and is malleable and ductile. It has a coefficient of expansion almost equal to that of soda-lime-silica glass, and is therefore used to make sealed electrodes in glass systems. The metal does not oxidize in air at any temperature, but is corroded by halogens, cyanides, sulfur, and caustic alkalis.
It is insoluble in hydrochloric and nitric acid, but dissolves when they are mixed as aqua regia, forming chloroplatinic acid.
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The metal is extensively used in jewelry, wire, and vessels for laboratory use, and in many valuable instruments including therocouple elements. It is also used for electrical contacts, corrosion-resistant apparatus, and in dentistry.
Platinum-cobalt alloys have magnetic properties. One such alloy made of 76.7% Pt and 23.3% Co, by weight, is an extremely powerful magnet that offers a B-H (max) almost twice that of Alnico V. Platinum resistance wires are used for constructing high-temperature electric furnaces.
The metal is used for coating missile nose cones, jet engine fuel nozzles, etc., which must perform reliably at high temperatures for long periods of time. The metal, like palladium, absorbs large volumes of hydrogen, retaining it at ordinary temperatures but giving it up when heated.
In the finely divided state platinum is an excellent catalyst, having long been used in the contact process for producing sulfuric acid. It is also used as a catalyst in cracking petroleum products. Much interest exists in using platinum as a catalyst in fuel cells and in antipollution devices for automobiles.
Platinum anodes are extensively used in cathodic protection systems for large ships and ocean-going vessels, pipelines, steel piers, etc. Fine platinum wire will glow red hot when placed in the vapor of methyl alcohol. It acts here as a catalyst, converting the alcohol to formaldehyde. The phenomenon has been used commercially to produce cigarette lighters and hand warmers. Hydrogen and oxygen explode in the presence of platinum.
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