I want to know about xenon(atomic #54). Please tell me the IMPORTANT USES and some 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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Huge order. Let's see how far it can be served.\n\n1. Monoatomic negative ions: take the element name (sometimes shortened) and add "-ide" (as in hydride, nitride, oxide, sulphide, phosphide, chloride...)\nPositive ions: element-name, charge (if several charges are possible), ion (sodium ion, iron II ion...)\n\n2. Polyatomic ions:\nComplexes with various ligands list the ligands and the central ion/atom.\nOxygen as ligands has its own nomenclature, depending on oxidation state. E.g. Sulphate, sulphite, perchlorate, chlorate, chlorite, hypochlorite...\n\n3. Binary molecular compounds: Halogen, oxygen and sulphur compounds usually have the correspondent "-ide" as if you had ionic compounds. Usually the more electropositive element is used as center.\n\n4. Acids: Oxygen acids have a similar nomenclature to oxygen ions.
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This may help: http://en.wikipedia.org/wiki/Bohr_atom
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I'm going to cheat a little bit in both cases by just referring back to the nearest noble gas.  That itself may be acceptable for your purposes (it's how most chemists list them because things past that point are usually of no interest)... if you need, I'll pass on the underlying noble gas configuations too.\n\n13:  [Ne] 3s2 3p1\n33:  [Ar] 4s2 3d10 4p3\n\nBasically, the electrons usually fill up the shells just as you see the elements arranged on the periodic table.  Group 1 and 2 (the two columns on the left) are the s shell, and the number of the s shell is indicated by the row number.  Group 13 through 18 (the six columns on the right) are the p shell; its number is also the same as the row number.  The middle stretch are d orbitals, and they're so expensive energetically that the ones on each row are orbitals from one shell down.  That chart is handy for all kinds of things!\n\nHope that helps!
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check this site out\n\nhttp://www.chemicalelements.com/elements/al.html
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You can ask atomic research agency. they are using this type of software.
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i can give you this much. but i find you lazy not to find this website if u dont already have it &#92;=)\n\nhttp://education.jlab.org/itselemental/ele037.html\n\nand more...\n\nhttp://chemistry.about.com/library/blrb.htm\n\nhttp://www.portlandschools.org/CTS/GrantsProjects/~driscc/elements/rubidium/rubidium.html\n\nhttp://www.scipeeps.com/Sci-Chemistry_Topics_Pr_-_R/Rubidium.html\n\n\ngood luck on your chemistry project. im working on one too. im doing Argon. got all my info. =)
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Technetium is a chemical element that has the symbol Tc and the atomic number 43. Pronounced tek-nee-s(h)ee-um, the chemical properties of this silvery grey, radioactive, crystalline transition metal are intermediate between rhenium and manganese. Its short-lived isotope Tc-99m is used in nuclear medicine for a wide variety of diagnostic tests. Tc-99 is used as a gamma ray-free source of beta particles, and its pertechnetate ion (TcO4-) could find use as an anodic corrosion inhibitor for steel.\n\nDmitri Mendeleev predicted many of the properties of element 43, which he called ekamanganese, well before its actual discovery (see Mendeleev's predicted elements). In 1937 its isotope Tc-97 became the first element to be artificially produced, hence its name (from the Greek τεχνητος, meaning "artificial"). Most technetium produced on Earth is a by-product of fission of uranium-235 in nuclear reactors and is extracted from nuclear fuel rods. No isotope of technetium has a half-life longer than 4.2 million years (Tc-98), so its detection in red giants in 1952 helped bolster the theory that stars can produce heavier elements. On earth, technetium occurs naturally only in uranium ores as a product of spontaneous fission; the quantities are minute but have been measured.\n\nNotable characteristics\nTechnetium is a silvery-grey radioactive metal with an appearance similar to platinum. However, it is commonly obtained as a grey powder. Its position in the periodic table is between rhenium and manganese and as predicted by the periodic law its properties are intermediate between those two elements. This element is unusual among the lighter elements because it has no stable isotopes and is therefore extremely rare on Earth.\n\nThe metal form of technetium slowly tarnishes in moist air. Its oxides are TcO2 and Tc2O7. Under oxidizing conditions technetium (VII) will exist as the pertechnetate ion, TcO4-. Common oxidation states of technetium include 0, +2, +4, +5, +6 and +7. When in powder form technetium will burn in oxygen. It dissolves in aqua regia, nitric acid, and concentrated sulfuric acid, but it is not soluble in hydrochloric acid. It has characteristic spectral lines at 363 nm, 403 nm, 410 nm, 426 nm, 430 nm, and 485 nm.\n\nThe metal form is slightly paramagnetic, meaning its magnetic dipoles align with external magnetic fields even though technetium is not normally magnetic. The crystal structure of the metal is hexagonal close-packed. Pure metallic single-crystal technetium becomes a type II superconductor at 7.46 K; irregular crystals and trace impurities raise this temperature to 11.2 K for 99.9% pure technetium powder. Below this temperature technetium has a very high magnetic penetration depth, the largest among the elements apart from niobium.\n\n\nApplications\n\nNuclear medicine\nTc-99m ("m" indicates that this is a metastable nuclear isomer) is used in radioactive isotope medical tests, for example as a radioactive tracer that medical equipment can detect in the body. It is well suited to the role because it emits readily detectable 140 keV gamma rays, and it has a short half-life of 6.01 hours (meaning it has almost completely decayed to Tc-99 in 24 hours). In the book Technetium by Klaus Schwochau, 31 different radiopharmaceuticals based on Tc-99m are listed for imaging and functional studies of the brain, myocardium, thyroid, lungs, liver, gallbladder, kidneys, skeleton, blood and tumors.\n\nImmunoscintigraphy incorporates Tc-99m into a monoclonal antibody, an immune system protein capable of binding to cancer cells. A few hours after injection, medical equipment is used to detect the gamma rays emitted by the Tc-99m; higher concentrations indicate where the tumor is. This technique is particularly useful for detecting hard to find cancers, such as those affecting the intestine. These modified antibodies are sold by the German company Hoechst under the name Scintium.\n\nWhen Tc-99m is com
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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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Neon, Krypton, and Argon are non-reactive noble gases.  Passing an electric current through them will cause the electrons to enter excited states.  When the electrons drop back down to the ground state, they drop in energy by a characteristic amount--this characteristic amount corresponds to a wavelength of radiation (like a particular color of visible light).  If you want a beautiful orange color, use neon!  I don't know what color argon and krypton are, but they would probably be chosen based on the particular wavelength they emit.  (I think the process is called fluorescence).\n\nI don't know anything about the xenon application you mentioned.  If you want a really heavy, nonreactive gas though xenon has those properties.  Think about why you would need a heavy gas in that application.
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Nitrogen might be what you are looking for as it is a gas and is next to Oxygen in the periodic table so it has similar mass.\n\nBut as the person above has said, some kind of gaseous sulfur would have the closest properties to oxygen.
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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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The uses you have identified are using Helium because it is inert and will not chemicaly react with other elements, however, there are potential uses for Helium as fuel, contrary to the other answers. \n\nHelium 3 is considered to be an ideal potential fuel for fusion-reaction power plants. The energy equivalent of Helium 3 compared to steam coal (at $2.5/million BTU) is about $140 million per 100 kg. In other words, it is a quite valuable resource if we are eventually able to utilize fusion reactors. \n\nThe most interesting part of this is that the moon's surface rock contains helium of this light isotope in much higher concentrations than found on earth. It could become economical to obtain He 3 from the moon if we develop fusion reactors as an energy source.
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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.
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You proffered the example of XeF4.  Now the Lewis structure for XeF4 gives an expanded octet, viz: AX4E2, where A represents the central atom (Xe) in this example; X represents a shared pair of electrons; and E represents an unshared pair.  Thus for XeF4 we have 4 shared pairs and 2 unshared pairs, i.e. 6 pairs.  \n\nNow whatever the principal energy level(n), there is 1 s orbital; and for n=2 and higher, there are 3 p orbitals; and for n=3 and higher there are 5 d orbitals. For n=4 and higher there are 7 f orbitals.\n\nNow considering XeF4 hybridization, for the 6 pairs of electrons there will be 6 orbitals [each orbital holds a maximum of two electrons with opposite spin]. That means sp3d2 hybridization.  That is the one s orbital, the three p orbitals and two of the five d orbitals form six sp3d2 orbitals.  Of course, we are talking here about valence shell electrons.  How would these orbitals fill?  Well, electrons are added to orbitals such that electrons with the same spin are added until there are no more empty orbitals, then the orbitals with one electron fill (i.e. add a second electron) by acquiring an electron of opposite spin.\n\nThis gives XeF4 sp3d2 hybrid orbitals and an octahedron orientation. \n\nConsidering the Lewis structure for water, as another example, we obtain a AX2E2 form. Thus sp3 hydrid orbitals and a tetrahedron orientation. The 4 hybrid orbitals come from 1 s and 3 p atomic orbitals.
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94,240Pu ---> 40,93Zr + 54,144Xe + _3_ 0,1n\n\nThe first number is the proton number, the second is the nucleon number. Both of these must be conserved in fission. As the number of protons is already conserved, the difference in the nucleon number must come from free neutrons.
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Everything is here at this link:\nhttp://genchem.chem.wisc.edu/sstutorial/Text8/Tx84/tx84.html