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| Atomic symbol: Xe |
| Atomic number: 54 |
| Atomic weight: 131.30 |
| Atomic volume: 37.3 cm3/mol |
| Density: 0.00588 g/cm3 |
| Period Number: 5 |
| Group number: 18 |
| Group name: Noble Gas |
| Element classification: Non-metal |
| Phase at room temperature: Gas |
| Melting Point: 161.3 K |
| Boiling point: 165 K |
| Heat of fusion: 2.297 kJ/mol |
| Heat of vaporization: 12.636 kJ/mol |
| Ionization Energy: 12.130 eV |
| 1st ionization energy: 1170.4 kJ/mole |
| 2nd ionization energy: 2046.4 kJ/mole |
| 3rd ionization energy: 3097.2 kJ/mole |
| Electronegativity: 2.6 |
| Electron affinity: kJ/mole |
| Specific heat: 0.158 J/gK |
| Heat atomization: 0 kJ/mole atoms |
| Shells: 2,8,18,18,8 |
| Electron Shell Configuration: [Kr] 4d10 5s2 5p6 |
| Minimum oxidation number: 0 |
| Maximum oxidation number: 8 |
| Minimum common oxidation number: 0 |
| Maximum common oxidation no: 6 |
Appearance & Characteristics |
| Structure:: fcc: face-centered cubic |
| Color: colorless |
| Hardness: mohs |
| Toxicity: no |
| Characteristics: unreactive |
| Uses: UV-laser, hi intens lamps |
| Reaction with air: none |
| Reaction with 6M HCl: none |
| Reaction with 15M HNO3: none |
| Reaction with 6M NaOH: none |
| Number of isotopes: 9 |
| Oxide(s): XeO3 XeO4 |
| Hydride(s): none |
| Chloride(s): none |
| Atomic Radius: 131 pm |
| Ionic radius (1- ion): pm |
| Ionic radius (1+ ion): pm |
| Ionic radius (2- ion): pm |
| Ionic radius (2+ ion): pm |
| Ionic radius (3+ ion): pm |
| Thermal conductivity: 0.01 J/m-sec-deg |
| Electrical conductivity: 0 1/mohm-cm |
| Polarizability: 4 A^3 |
| Source: Air |
| Relative abundance solar system: 0.672 log |
| Abundance earth's crust: -4.5 log |
| Estimated crustal abundance: 3×10-5 milligrams per kilogram |
| Estimated oceanic abundance: 5×10-5 milligrams per liter |
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| (Gr. xenon, stranger) Discovered in 1898 by Ramsay and Travers in residue left after evaporating liquid air. Xenon is a member of the so-called noble or "inert" gases. It is present in the atmosphere to the extent of about one part in twenty million. Xenon is present in the Martian atmosphere to the extent of 0.08 ppm. the element is found in the gases evolved from certain mineral springs, and is commercially obtained by extraction from liquid air. |
| The gas is used in making electron tubes, stoboscopic lamps, bactericidal lamps, and lamps used to excite ruby lasers that generate coherent light. Xenon is used in the nuclear energy field in bubble chambers, probes, and other applications where a high molecular weight is of value. The perxenates are used in analytical chemistry as oxidizing agents. 133Xe and 135Xe are produced by neutron irradiation in air cooled nuclear reactors. 133Xe has useful applications as a radioisotope. The element is available in sealed glass containers of gas at standard pressure. Xenon is not toxic, but its compounds are highly toxic because of their strong oxidizing characteristics. |
| Natural xenon is composed of nine stable isotopes. In addition to these, 20 unstable isotopes have been characterized. Before 1962, it had generally been assumed that xenon and other noble gases were unable to form compounds. Evidence has been mounting in the past few years that xenon, as well as other members of zero valance elements, do form compounds. Among the "compounds" of xenon now reported are sodium perxenate, xenon deuterate, xenon hydrate, difluoride, tetrafluoride, and hexafluoride. Xenon trioxide, which is highly explosive, has been prepared. More than 80 xenon compounds have been made with xenon chemically bonded to fluorine and oxygen. Some xenon compounds are colored. Metallic xenon has been produced, using several hundred kilobars of pressure. Xenon in a vacuum tube produces a beautiful blue glow when excited by an electrical discharge. |
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