What group is Hydrogen found in on the Periodic Table?
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Hydrogen is generally accepted as a member of group I or IA, but it is also accepted as having no group.  Allow me to explain.  \n\nHydrogen can be classified as a member of group I because like all of the other elements in group I, it has exactly one valence electron (one electron on its outermost electron shell, in the case of hydrogen, the only shell). Valence shell counts and electron configurations are the basis of the periodic table. \n\nHowever, hydrogen is very unique and exhibits far different chemical properties from any other element in group I or any other group.  For example, hydrogen is a non-metal, it exists in a diatomic state in nature, it can form compounds with both metals and non-metals, and does not form salt compounds with non-metals. For these reasons, sometimes periodic tables will not have hydrogen in group I.  Instead, some periodic tables will put hydrogen in a small box by itself above the rest of the periodic table, totally separated from the rest of the periodic table.  The little box for hydrogen in these periodic talbes is usually pretty close to the middle to represent the fact that it exhibits properties on both sides of the periodic table.  \n\nIn conclusion, either "no group" or group I or IA is acceptable to answer the homework question.
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http://www.webelements.com/webelements/elements/text/H/key.html\nhttp://periodic.lanl.gov/elements/1.html\nhttp://www.chemicalelements.com/elements/h.html\nhttp://education.jlab.org/itselemental/ele001.html
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Hydrogen gas molecules, H2
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Investigate the origins of the periodic table.
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in the universe hydrogen, on earth it is iron
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First you need to look up the element on a periodic table of elements.  I am sure you have one laying around somewhere =P\nAnyway, then look in the square that contains your element for a number either in the upper left corner or in some cases directly above it.  That is the number of protons in the atom.  Then you also know the number of electrons which is exactly the same as the number of protons.  To figure out neutrons, look for another number on in the square that isnt in the left corner or above the element.  This is the atomic mass.  Take the atomic mass and subtract the number of protons to get the number of neutrons
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Most Common Element\nHydrogen is the most common element in both the Universe and the Solar System. Over 90% of the Universe is comprised of hydrogen. -----Iron is the most common element on Earth,----- accounting for 36% of its mass.
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Common elements that exist as diatomic molecules are H, N, O, F, Cl, Br, and I.\n\nSo these elements are most commonly found in nature as H2, N2, O2, F2, Cl2, Br2, and I2.
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It's all the elements in the d-block of the periodic table. Basically, the group starting from column three to column twelve. These transition metals commonly have many oxidation states and have either partially filled d-orbitals or full d-orbitals (like mercury). They also form complex ions quite readily.\n\nIf all of that doesn't make sense, just remember it's the metals in that "lowered" part in the middle.
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Hydrogen is a very dangerous compound, especially under pressure or concentrated.  When burned, hydrogen creates a violent exposion with oxygen that produces water.  Furthermore, hydrogen is a main part the most acidic compounds known to man such as hydrocloric acid.
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Anything from the periodic table is pure. these are all basic elements that can't be broken down into other elements. examples: hydrogen, nitrogen, iron, zinc and gold.\nclick here for the table: http://www.chem.qmul.ac.uk/iupac/AtWt/table.html
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Group 1-alkali metals Group 2- alkaline earth metals Groups 3-12-transition metals Group 17-Halogens Group 18- Noble gasses
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CO2 and H2SO4\n\n"metal" belongs to group IA, IIA, and B\n\nNa is IA\nK is IA
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it's vital in organisms. hydrogens make up the three most important types of molecules to human beings: carbohydrates, proteins, and fats.\n\nthey are trying to develop cars that run on hydrogen fuel.
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GIVE ME TEN POINTS!!!  \n\nHERES UR GROUPS....\n\n\nGroup 0 Elements\nThe elements in this group have a full outer electronic shell and thus, the elements in this group have no tendency to lose, gain or share electrons. Thus, the elements in the group are chemically inert. \n\nAll the elements in this group are gaseous. Because of their chemical inertness, the elements in this group are called the Nobel Gases : \n\n\nHelium\nNeon\nArgon\nKrypton\nXenon\nRadon \n\n\n--------------------------------------------------------------------------------\n\nGroup I Elements\nThe elements in this group have one electron in their outer electronic shell. Thus, each element in this group has a tendency to lose a single electron, to form a singly charged positive ion, which has the stable electronic configuration of its neighbouring Nobel Gas element in the periodic table. \n\nThe elements in the group are chemically reactive. \n\nThe group is divided into two sub-groups. \n\nSub-Group Ia : The Alkali Metals\n\nLithium\nSodium\nPotassium\nRubidium\nCaesium\nFrancium\n\n\nSub-Group Ib : Transition Metal Elements\n\nCopper\nSilver\nGold\n\nHydrogen is included in this group because it has a single electron in its outer electronic shell. However, hydrogen has none of the metallic properties of the alkali metals. \n\n\n\n--------------------------------------------------------------------------------\n\nGroup II Elements\nThe elements in this group have two electrons in their outer electronic shell. Thus, each element in this group has a tendency to lose two electron, to form a doubly charged positive ion, which has the stable electronic configuration of its neighbouring Nobel Gas element in the periodic table. \n\nThe elements in the group are chemically reactive. \n\n\nSub-Group IIa : The Alkaline Earth Metals\n\nBeryllium\nMagnesium\nCalcium\nStrontium\nBarium\nRadium\n\n\nSub-Group IIb : Transition Metal Elements\n\nZinc\nCadmium\nMercury\n\n\n\n--------------------------------------------------------------------------------\n\nGroup III Elements\nThe elements in this group have three electrons in their outer-most electronic shell. The electronic configurations of the n th orbitals (i.e. outer-most orbitals) are ns2 np1. Thus, each element in this group has a tendency to lose three electron, to form a triply charged positive ion, which has the stable electronic configuration of its nearest neighbouring Nobel Gas element in the periodic table. \n\nThe elements in the group are chemically reactive. \n\n\nSub-Group IIIa : Transition Metal Elements\n\nScandium\nYttrium\nLanthanum\n\nThe following elements also have the same electronic configuration as lanthanum (i.e. 4s2 4p1) in their outer-most electronic orbitals, while the inner 3d orbitals are being filled, from going from element to element.\nCerium\nPraeseodymium\nNeodymium\nPromethium\nSamarium\nEuropium\nGadolinium\nTerbium\nDysprosium\nHolmium\nErbium\nThulium\nYtterbium\nLutecium\n\n\nThese are the transition elements, and are also called the Lanthanides. \n\nActinium\n\nThe following elements also have the same electronic configuration as actinium (i.e. 5s2 5p1) in their outer-most electronic orbitals, while the inner 4d orbitals are being filled, on going from element to element.\nNeptunium\nPlutonium\nAmericium\nCurium\nBerkelium\nThese are the inner transition elements, and are also called the Actinides. \n\n\nSub-Group IIIb : Main Group Elements\n\nBoron\nAluminium\nGallium\nIndium\nThallium\n\n\n\n--------------------------------------------------------------------------------\n\nGroup IV Elements\nThe elements in this group have four electrons in their outer electronic shell. Thus, each element in this group has a tendency to share these four electrons, to form covalent compounds, thereby gaining the stable electronic configuration of its neighbouring Nobel Gas element in the periodic table. \n\nThe elements in the group are chemically reactive. \n\nSub-Group IVa : Transition Me
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Hydrogen\nHelium\nLithium\nBeryllium\nBoron\nCarbon\nNitrogen\nOxygen\nFluorine\nNeon\nSodium\nMagnesium\nAluminum\nSilicon\nPhosphorus\nSulfur\nChlorine\nArgon\nPotassium\nCalcium\nScandium\nTitanium\nVanadium\nChromium\nManganese\nIron\nCobalt\nNickel\nCopper\nZinc\nGallium\nGermanium\nArsenic\nSelenium\nBromine\nKrypton\nRubidium\nStrontium\nYttrium\nZirconium\nNiobium\nMolybdenum\nTechnetium\nRuthenium\nRhodium\nPalladium\nSilver\nCadmium\nIndium\nTin\nAntimony\nTellurium\nIodine\nXenon\nCesium\nBarium\nLanthanum\nCerium\nPraseodymium\nNeodymium\nPromethium\nSamarium\nEuropium\nGadolinium\nTerbium\nDysprosium\nHolmium\nErbium\nThulium\nYtterbium\nLutetium\nHafnium\nTantalum\nTungsten\nRhenium\nOsmium\nIridium\nPlatinum\nGold\nMercury\nThallium\nLead\nBismuth\nPolonium\nAstatine\nRadon\nFrancium\nRadium\nActinium\nThorium\nProtactinium\nUranium\nNeptunium\nPlutonium\nAmericium\nCurium\nBerkelium\nCalifornium\nEinsteinium\nFermium\nMendelevium\nNobelium\nLawrencium\nRutherfordium\nDubnium\nSeaborgium\nBohrium\nHassium\nMeitnerium
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Selenium element is located in Group 6A of the periodic table. This in dicates that it has 6 electron in its valence or outermost shell. The Lewis dot structure of Selenium shoulde be written with Se surrounded by six dots. These six dots don't have to be an all four sides but if you do then that is the conventional way of doing it.