Please tell me about XENON!!! -the importance and the characteristics?
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I Hope this Helps.  XENON \n\n\n\n[General | States | Energies | Oxidation & Electrons] \n[Appearance & Characteristics | Reactions | Other Forms] \n[Radius | Conductivity | Abundance | History]\n\n\nGeneral\nName Xenon  Symbol Xe  \nAtomic number 54  Atomic weight 131.30  \nDensity @ 293 K 0.00588 g/cm3  Atomic volume 37.3 cm3/mol  \nGroup Noble Gas  Discovered 1898  \n\nBack to the top\nStates\nState (s, l, g) g  \nMelting point 161.3 K  Boiling point 165 K  \nHeat of fusion 2.297 kJ/mol  Heat of vaporization 12.636 kJ/mol  \n\nBack to the top \n\nEnergies\n1st ionization energy 1170.4 kJ/mole  Electronegativity 2.6  \n2nd ionization energy 2046.4 kJ/mole  Electron affinity kJ/mole  \n3rd ionization energy 3097.2 kJ/mole  Specific heat 0.158 J/gK  \nHeat atomization 0 kJ/mole atoms  \n\nBack to the top\nOxidation & Electrons\nShells 2,8,18,18,8  Electron configuration [Kr] 4d10 5s2 5p6  \nMinimum oxidation number 0  Maximum oxidation number 8  \nMinimum common oxidation number 0  Maximum common oxidation number 6  \n\nBack to the top \n\nAppearance & Characteristics\nStructure fcc: face-centered cubic  Color colorless  \nUses UV-laser, hi intens lamps  Toxicity no  \nHardness mohs  Characteristics unreactive  \n\nBack to the top\nReactions\nReaction with air none  Reaction with 6M HCl none  \nReaction with 6M HCl none  Reaction with 15M HNO3 none  \nReaction with 6M NaOH none  \n\nBack to the top \n\nOther Forms\nNumber of isotopes 9  Hydride(s) none  \nOxide(s) XeO3 XeO4  Chloride(s) none  \n\nBack to the top\nRadius\nIonic radius (2- ion) pm  Ionic radius (1- ion) pm  \nAtomic radius 131 pm  Ionic radius (1+ ion) pm  \nIonic radius (2+ ion) pm  Ionic radius (3+ ion) pm  \n\nBack to the top \n\nConductivity\nThermal conductivity 0.01 J/m-sec-deg  Electrical conductivity 0 1/mohm-cm  \nPolarizability 4 A^3  \n\nBack to the top\nAbundance\nSource Air  Rel. abund. solar system 0.672 log  \nAbundance earth's crust -4.5 log  Cost, pure 120 $/100g  \nCost, bulk $/100g  \n\nBack to the top \n\nHistory: \n\n\n(Gr. xenon, stranger) Discovered by Ramsay and Travers in 1898 in the residue left after evaporating liquid air components. 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. 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. The gas is used in making electron tubes, stroboscopic lamps, bactericidal lamps, and lamps used to excite ruby lasers for generating 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 compo
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Something very close to it already exists:  Ion drive.  This uses charged xenon particles as its propellant.  The acceleration is very low, but it is much more efficient than chemical rockets.  NASA has already put it to practical use with their Deep Space 1 probe, and will use it again with their Helium 3 probe.\n\nOf course, that's still a mass-reaction drive.  A rather exotic one, but still...\n\nOne way of using light for propulsion is with a "solar sail," which The Planetary Society tried to test with its Cosmos-1 mission.  Unfortunately, the probe was lost in a launch failure.  They want to try again, though; you might want to write to them about your idea.
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Phase - gas \nDensity  (0 °C, 101.325 kPa)\n9.73 g/L \nMelting point  202 K\n(-71 °C, -96 °F) \nBoiling point 211.3 K\n(-61.7 °C, -79.1 °F) \nCritical point 377 K, 6.28 MPa \nHeat of fusion 3.247 kJ·mol−1 \nHeat of vaporization 18.10 kJ·mol−1 \nHeat capacity (25 °C) 20.786 J·mol−1·K−1 \nVapor pressure P/Pa 1 10 100 1 k 10 k 100 k \nat T/K 110 121 134 152 176 211 \n \nAtomic properties \nCrystal structure cubic face centered \nOxidation states 0 \nElectronegativity no data (Pauling scale) \nIonization energies 1st: 1037 kJ/mol \nAtomic radius (calc.) 120 pm \nCovalent radius 145 pm \nMiscellaneous \nMagnetic ordering non-magnetic \nThermal conductivity (300 K) 3.61 mW·m−1·K−1 \nCAS registry number 10043-92-2 \nSelected isotopes \nIsotopes of radon iso NA half-life DM DE (MeV) DP \n211Rn syn 14.6 h Epsilon 2.892 211At \nAlpha 5.965 207Po \n222Rn 100% 3.824 d Alpha 5.590 218Po \n \n\n\nthis is what wikipedia had to say. hope it helps!
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Hmm, kinda hard to help you here, since we can't see all your options for the first two.  The ellipses (. . .) indicate that you have more in your message than is being displayed.  Perhaps if you retyped them, it would be easier for us to help.\n\nHere's what I *can* help with:\n\nHalogens:Reactive as Noble Gas:STABLE\n(the halogens are very reactive gases, while the noble gases are extremely stable, almost to the point of being inert)\n\nOxygen:molecule as chloride:ION\nOxygen gas is a molecule, while chloride is the ionic form of chlorine\n\nRatio:subscript as oxidation number:CHARGE\nthe ratio of components in a mixture is denoted by the subscripts, as the oxidation number of an atom is denoted by its ionic charge
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Here's a great website with pictures of the various nobel gases in lamps so you can see their glows and describe them yourself.\n\nhttp://www.assumption.edu/users/bniece/Spectra/Complete.html
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I don't know if you're saying they don't last as long as the manufacturer says they should or just that they don't last long, but: the xenon bulbs use a lot of power, about 5 watts compared to the LED's 1 watt. Lithium battery lifetime is given as 2 hours with xenon bulb. See the ref. for the specs.
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The noble gasses are inert because they all have full electron orbitals, but the heavier noble gasses have so many electron shells that it is possible to strip some of the outer electrons off to get a reaction. Neon is going to be really tough to get a a reaction out of, but Xenon, a much heavier noble gas, will form compounds with Flourine under the right conditions. I'm thinking it's XeF4, but I can't recall exactly.\n\nLasers don't exactly require chemical reactions, as far as I know, so a Helium Neon laser could contain the two gasses unreacted with each other.
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helium neon argon krypton xenon radon\nyou probably do not need to know ununoctium because it was just discovered, is radioactive, and radioactively decays in a few seconds.
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Atoms favor complete valence shell fulfillment and charge neutrality above all.  Since potassium has a positive center that requires 1 electron above the more stable electron orbital fulfillment, it does not require much energy to release the electron.  Since our environment consists of O2, it will react to it because a more stable configuration than the O=O configuration is the K2O.  Why?  Oxygen's center does not have enough electrons to complete the p orbital shell.  Therefore, it is not satisfied.  Thus, oxygen will share 2 electrons with another oxygen to form O2 until it has an opportunity to take 2 K electrons that potassium does not want.  Therefore, Oxygen is a lot happier than it was with another Oxygen atom who wanted the 2 electrons.  Potassium is a lot happier getting rid of the electron that it did not want.  But wait?  Why are they stuck together?  Because despited wanted to shape their electron clouds at the most ideals shapes possible, the nucleus still requires an equal amount of electrons closeby to be happy.  Thus, the only way to achieve this is to stick around Oxygen who's slightly negative.\n\nThe same could be said between Potassium and any halide, but not Potassium and any of the noble gases.  Noble gases are really happy to be complete because their electron configurations are at an ideal state - completely fulfilled.  To strip an electron would require a really high amount of energy.\n\nThus, the reasons why K likes most stuff that aren't satisfied, but not all.
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it is a noble gas, but just because something isnt solid doesnt meanits a nonmetal. metals all become gasses at high temperature. the metals are on the left side of the periodic tabl and the non metals arre on the right. xenon is all the way on the right so its a non metal.\n\nhttp://en.wikipedia.org/wiki/Periodic_table#Standard_periodic_table
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From the early 1960's compounds have been made, but only xenon compounds are stable and usually combined with oxygen and fluorine, which, not surprisingly, are the more reactive non-metals.
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They are inert and so don't react with other elements/compounds.  Often used in situations where oxidation would occur if oxygen was present.\n\nExample:  Xenon is car head lights.  Get very hot and the filaments would oxidise (burn up) if oxygen was present.
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do you mean information on gases like chlorine etc?\n\nwhat specific information do you require?\n\na good resource for information is wikipedia
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Noble Gases:  He, Ar, Ne, Xe\nHalogens:  F2, Cl2, Br2, I2, At2\nOthers:  N2, O2
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http://hyperphysics.phy-astr.gsu.edu/hbase/nucene/bomb.html\nhttp://hydrogen.kiwiki.homeip.net/\nhttp://whyfiles.org/186ed_teller/3.html
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d)Argon: 1s2 2s2 2p6 3s2 3p6\ne)Could be carbon, silicon, germanium, tin, or lead.  It's not specific enough.  And there is no such thing as an "elemen." Please treat chemistry with enough respect just type a "t" at the end of a word.  \nCarbon: 1s2 2s2 2p2\nSilicon: 1s2 2s2 2p6 3s2 3p2\nGermanium:  1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2\nTin: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d6 5s2 4d10 5p2 \nLead: \n1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d6 5s2 4d10 5p6 6s2 4f14 5d10 6p2
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Under ordinary conditions xenon will not react.  Under very low temperatures and very high pressure it can be forced to react with oxygen and fluorine forming xenon trioxide (XeO3) and xenon tetrafluoride (XeF4).  These compounds are extremely unstable and will decompose into their elements easily and explosively.