What was the order in which the noble gases were discovered?
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Not sure you can get an exact ranking, because three were researched simultaneously:\n\nHelium was discovered on Earth in 1895 by Scottish chemist Sir William Ramsay, though some credit the discovery of helium (in the sun's spectrum) to Janssen and Lockyear in 1868. Ramsay discovered most of the remaining noble gases--argon in 1894 (with Lord Rayleigh) and krypton, neon, and xenon in 1898 (with Morris M. Travers). Radon was discovered in 1898 by Fredrich Ernst Dorn.
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A number of chemists contributed to the development of the periodic table during the 19th century; however, Mendeleyev Dmitry Ivanovich, a russian chemist,  is regarded as the primary discoverer. His version of the table was the first to accommodate all the known elements and also successfully predicted the existence of several elements that had not yet been discovered. These undiscovered elements included gallium, scandium, and germanium.\n\n\nDuring the writing of his book, Mendeleyev tried to classify the elements according to their chemical properties. In 1869 he published his first version of what became known as the periodic table, in which he demonstrated the periodic law. In 1871 he published an improved version of the periodic table, in which he left gaps for elements that were not yet known. His chart and theories gained increased acceptance when three predicted elements—gallium, germanium, and scandium—were subsequently discovered.
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Sir Hans Krebs discovered teh Kreb's cycle in cellular respiration. He used X-Rays of cells to see how cell respiration takes place
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The Periodic Table of the Elements, as developed by Mendeleev.
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the amount of electrons in an atom.\n\nif you're going to use noble gas configuration, you would use the noble gas and then continue the configurations.\n\nex. i want the configuration of... flourine (F)\nfor noble gas configuration i would say: (He) 2s 2 2p 6\n\nthe parenthasese is actually a bracket, and the numbers that are spaced should be in the upper righthand corner of the letter before it.
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You can find noble gasses as trace amounts in the air, and are produced through various forms of nucleosynthesis in stars and supernovae.\n\n*Helium is a fusion product of main sequence stars and a fusion fuel for some Red Giant Stars\n*Neon is a fusion product of some red giant stars and a fusion fuel for massive stars nearing the end of their lives\n*Argon is produced by the decay of Potasium, and is often used as an inert gas while welding tungsten.\n*Krypton is a fission product of uranium, and used to make a powerful, short lived laser source.\n*Xenon is often used in high powered lamps\n*Radon is a decay product of Radium, and is radioactive, there are no to many common uses of Radon.
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Noble gases are also called inert gases because they do not react chemically.  There the one in the last column of the table.  Their last electron layer is full (all 8 electrons --2 for helium-- are there) and that's why they don't (usually) form bonds.
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Helium, CO2, Hydrogen and various others.
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Chlorine (Gr. χλωρος, greenish yellow) was discovered in 1774 by Swedish chemist Carl Wilhelm Scheele, who mistakenly thought it contained oxygen. Chlorine was given its name in 1810 by Sir Humphry Davy, who insisted that it was in fact an element.\n\nChlorine gas was first used as a weapon against human beings in WWI on April 22nd, 1915.
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helium \n(He), chemical element, inert gas of Group 0 (noble gases) of the periodic table. The second lightest element (only hydrogen is lighter), helium is a colourless, odourless, and tasteless gas that becomes liquid at -268.9 C (-452 F). Only under increased pressure (approximately 25 atmospheres) does helium solidify.\nHelium was discovered in the gaseous atmosphere surrounding the Sun by the French astronomer Pierre Janssen, who detected a bright yellow line in the spectrum of the solar chromosphere during an eclipse in 1868; this line was initially assumed to represent the element sodium. That same year, the English astronomer Joseph Norman Lockyer observed a yellow line in the solar spectrum that did not correspond to the known D1 and D2 lines of sodium, and so he named it the D3 line. Lockyer concluded that the D3 line was caused by an element in the Sun that was unknown on Earth; he and the chemist Edward Frankland used the Greek word for sun, helios, in naming the element. The British chemist Sir William Ramsay discovered the existence of helium on Earth in 1895. Ramsay obtained a sample of the uranium-bearing mineral cleveite, and upon investigating the gas produced by heating the sample, he found that a unique bright-yellow line in its spectrum matched that of the D3 line observed in the spectrum of the Sun; the new element of helium was thus conclusively identified. In 1903 Ramsay and Frederick Soddy further determined that helium is a product of the spontaneous disintegration of radioactive substances. \n\nHelium constitutes about 23 percent of the mass of the universe and is thus second in abundance to hydrogen in the cosmos. Helium is concentrated in stars, where it is synthesized from hydrogen by nuclear fusion. Although helium occurs in the Earth's atmosphere only to the extent of 1 part in 200,000 (0.0005 percent), and small amounts occur in radioactive minerals, meteoric iron, and mineral springs, great volumes of helium are found as a component (up to 7.6 percent) in natural gases in the United States (especially in Texas, New Mexico, Kansas, Oklahoma, Arizona, and Utah). Smaller supplies have been discovered in Canada and South Africa and in the Sahara Desert.\n\nAlthough there are six known isotopes of helium, only two are stable: helium-3 (symbolized 3He) and helium-4 (symbolized 4He). The four other isotopes are all radioactive, decaying very rapidly into other substances. The helium that is present on Earth is not a primordial component of the Earth but has been generated by radioactive decay. Alpha particles, ejected from the nuclei of heavier radioactive substances, are nuclei of the isotope helium-4. Helium does not accumulate in large quantities in the atmosphere because Earth's gravity is not sufficient to prevent its gradual escape into space. The trace of the isotope helium-3 on Earth is attributable to the negative beta decay of the rare hydrogen-3 isotope (tritium). Helium-4 is by far the most plentiful of the stable isotopes: helium-4 atoms outnumber those of helium-3 about 700,000:1 in atmospheric helium and about 7,000,000:1 in certain helium-bearing minerals.\n\nHelium-4 is unique in having two liquid forms (see Figure A). The normal liquid form is called helium I and exists at temperatures from its boiling point of 4.21 K (-268.9 C) down to about 2.18 K (-271 C). Below 2.18 K, helium-4 undergoes superfluidity (i.e., its viscosity, or resistance to flow, nearly vanishes) and its thermal conductivity becomes more than 1,000 times greater than that of copper. This liquid form is called helium II to distinguish it from normal liquid helium I. By contrast, the less plentiful helium-3 forms three distinguishable liquid phases (see Figure B), of which two are superfluids. Superfluidity in helium-4 was discovered by the Russian physicist Pyotr Leonidovich Kapitsa in the mid-1930s, and the same phenomenon in helium-3 was first observed by Douglas D. Osheroff, David M. Lee, and Robert C.
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Investigate the origins of the periodic table.
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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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If by "naturally occuring" you mean present in nature in its elemental form, then the answer includes noble gases (Helium and Argon), noble metals (Gold and Platinum and maybe Copper), and some diatomic molecules (Oxygen, Nitrogen) as well as Sulfur (S_8) and Carbon (graphite and diamond).  Most of the metals are found as some kind of oxide (in ores) or in salts (sodium chloride).  The halogens are found in salts (sodium chloride). \n\nA lot of today's useful materials were never present in significant amounts in elemental form, for example: iron, aluminum, zinc.
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Rutherford and Bohr did much of the early theoretical work on the structure of the atom but the real breakthrough was in 1938 when the Austrian physicist Lise Meitner and the German chemist Otto Hahn bombarded uranium with neutrons and caused it to splinter into barium and krypton. \n\nShe coined the term "fission" for this process. borrowing a term from biology. When the Nobel Prize was awarded for this joint work over 30 years, after WW2, he was awarded it and she was omitted. Being female and Jewish had caused her career to be eclipsed by his.
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Noble gases are inactive\nhalogens are very active\nLast one, ionization energy decreases\nlanthanide and actinide are the bottom 2 periods
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He weighed the atomic mass of elements and arranged them from the lowest to the highest. Also, he put them into the same column if they have the same chemical properties. But he didn't known that the last group (noble gases) exists because they have no reactions with other substances. So his periodic table just had 7 columns (groups).
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He was a chemist who discovered guncotton and ozone.  I'm sure Wiki would have an entry on him, and maybe some actual refrences