What are the characteristics of nonmetals (in the periodic table) ?
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http://chemistry.allinfoabout.com/features/nonmetals.html
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Here is one : http://en.wikipedia.org/wiki/Periodic_table
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You need to look at a Periodic Table. The farther to the left of the table an element is, the more metallic it is.
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nonmetals have much higher ionization energies than metals do. this is because non-metals have more protons in their nucleuses to attract their electrons with. metals do not have as many, as compared to the rows they are in, so the electrons will move away from the nucleus of the metal if given a little push.
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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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Solid or gaseous, depending on what the question means when refering to non-metals:  There are 11 gases total out of the entire table (6 are nobel gases) and only 2 liquids..mercury and bromine.  The true non-metals comprise only 7 elements, and only 3 of those (hydrogen, nitrogen, and oxygen) are gases.  If you takea  looser definition of non-metals, which includes the true nonmetals plus the halogens and noble gases, the the answer is gaseous.  From the wording of the question, I would think they were trying to get you to say gaseous.
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Magnesium is an element it does not "break down".
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I'm not really sure what you mean, but here's a good site to look at the periodic table.\n\nhttp://en.wikipedia.org/wiki/Periodic_table
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True: in the same set of conditions, minerals will be unique in their properties including electrical conduction, hardness, light reflection, ect. Minerals can be in different forms though, which you should always take into consideration.
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You need to know more than just the electron configuration.  There is contraction from left to right on the periodic table, plus additional periodic trends that must be considered.   \n\nEven more importantly, you need to define whether you are looking for the largest element IN ITS NATURAL  STATE (i.e. Cl2, Hg metal, etc) or AS THE ION.   Atomic and ionic radii differ.\n\nMore clarity is needed here.
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Together with the metals and nonmetals, the metalloids (in Greek metallon = metal and eidos = sort - also called semimetals) form one of the three categories of chemical elements as classified by ionization and bonding properties. They have properties intermediate between those of metals and nonmetals. There is no unique way of distinguishing a metalloid from a true metal but the most common is that metalloids are usually semiconductors rather than conductors.\n\nThe known metalloids (and their atomic symbols) are:\n\nBoron (B) \nSilicon (Si) \nGermanium (Ge) \nArsenic (As) \nAntimony (Sb) \nTellurium (Te) \nPolonium (Po) \nAstatine (At) \nIn the periodic table, metalloids occur along the diagonal line from boron to polonium. Elements to the upper right of this line are nonmetals; elements to the lower left are metals.\n\nSemi-metallic behaviour is not confined to the elements, but is also found in alloys and compounds. Mercury (II) telluride is one example.\n\nOne definition of semi-metallic behavior would be if the conduction band and valence band overlap. This is also true of metals, so semi-metals must additionally have a relatively low carrier density.
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The chlorine ion would be much larger because Mg is a metal and Cl is a nonmetal. When ionized, metals tend to lose electrons (and a stable octet) and become smaller. On the contrary, nonmetals gain electrons (and a stable octet) and become larger.
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A nonstoichiometric compound is anything in which the elements do not occur in proportions of whole numbers.  Usually these are solids which have some defect in their crystal lattice structure, meaning it is missing some ions.\n\nA common example is of the three biggies in the iron oxides.  Fe2O3 and Fe3O4 are typically stoichiometric... if you have 2 million Fe ions in your Fe2O3, you will have very near 3 million O ions.  FeO, on the other hand, is often slightly short of iron, and is written Fe(1-x)O, in which x is some small number.
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jtkeel is mostly right, except the structure of copper is not crystaline.  Al3K is right about the structure of copper, which is the basic structure of all metals and is what gives them their physical characteristics, like their malleability, conductivity and so forth.
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The question is not clear.  Are you asking what a crystal is?  Are you asking what the different crystal structures are?  Are you asking for the characteristics of crystals in general?
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I think ur referring to the chemical definitions.\n\nIn the periodic table, groups are the vertical columns having similar elements... ie. they have the same valencies leading to similar properties.. Example Group 1: has valency 1.. (Na, K etc)\n\nperiods are horizontal rows having elements with the same number of shells.. ie.. 1st period elements have only one shell (H and He - K shell).. 2nd period elements have 2 shells (K,L) and so on..\n\nLook up wikipedia for more info..
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Nobody knows the answer to this exept for Mendeleev himself, and he isn't talking. The first periodic table had 64 elements, although 3 or 4 of those were still purely theoretical. Since there were more than 50 in the first periodic table, you can't really discuss the first 50 added very well. Several models of organization were proposed, but there were around 60 known elements before it was deemed necessary to organize them. Only Mendeleev's used periodicity, and it is the closest to our modern periodic table.\n\nThe only 2 elements in my periodic table are:\n\nWOMANIUM (XX)\nPhysical properties: Generally soft and round in form. Boils at nothing and may freeze any time. Very bitter if not used well.\nChemical properties: Very active and highly unstable. Possesses strong affinity with gold, silver, platinum, and precious stones. Violent when left alone. Turns slightly green when placed next to a better specimen.\nUsage: An extremely good catalyst for dispersion of wealth.\nCaution: Highly explosive in inexperienced hands!\n\nMANIUM (XY)\nPhysical properties: Solid at room temperature but gets bent out of shape easily. Difficult to find a pure sample. Due to rust, aging samples are unable to conduct electricity as easily as young samples.\nChemical properties: Attempts to bond with XX any chance it can get. Also tends to form strong bonds with itself. Becomes explosive when mixed with Childrium for prolonged period of time.\nUsage: Possibly good methane source.\nCaution: In the absence of XX, this element rapidly decomposes and begins to smell.