1. What is an allotrope? \n2. What are the two allotrope of oxygen? \n3. Where are they found? \n4. List three uses and properties of each allotrope of oxygen.
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http://en.wikipedia.org/wiki/Allotrope
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1)SO2, the sulfur, when it burns in air reacts with the O to form SO2. When Mg burns in air it reacts with the O and the N in the air and forms both MgO and Mg3O2. The product SO2 is a gas and MgO and Mg3O2 is a solid.\n\n2)It is ionic. Ionic bonds form between a + ion and a - ion. Na is + and F is -.\n\n3)P with O is covalent. Both elements are negative ions so they share. You need a + and a - to be ionic.\n\n4)No! Lots and lots of liquids. Some solids also.\n\n5)O and S are in the same groups because they both have 2 electrons in their outer shells. P and S are next to each other because they both have the same number of energy levels (3).\n\nGet an "A".
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to quote any help?: "frogs work ok, as long as they are not solid"... what the hell?!? how many semi solid frogs you come across lately??? you are not any help, any help?... where you from? another oxygen thief...
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oxygen is made by distilling liquid air. liquid air is regular air cooled to about -200 degrees.  it becomes a liquid.\n\nthe oxygen doesnt need cleaning,  the distillation process removes any impurities.\n\noxygen is put into the cylinders by a machine similar to a super heavyduty air compressor.  the oxygen in a full cylinder is at about 2000 psi.
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Okay... *takes breath*\nTo find out the redox thingies--yes, "thingies." You have to find the oxidation number of each substance in the equation. Oxygen is usually -2, pure elements is always 0, ionic substances is the same as its charge. Compare the oxidation numbers of each element from the product and the reaction; if the number increases, it has been oxidized; if the number decreases, it has been reduced.\n\n1) 2Na + S ----> Na2S   so....\nNa=0, S=0 ---> Na=1, S=-2 (just look at the period table to get the last two numbers)\nNa goes from 0 to 1, so it has been oxidized, and Na is also the oxidizing agent.\nS goes from 0 to -2, it has been reduced, S is the reducing agent.\n\n2) K=oxidized, oxidizing agent\nCl=reduced, reducing agent\n\n3) Al=oxi, oxi agent\nO2=red, red agent\n\n4) H=oxi, oxi agent\nCl=red, red agent\n\n5) N=oxi, oxi agent\nH=red, red agent\n\nOn all of them, the first element is oxidized as well as oxidizing agent; and the second is reduced, and the reduced agent.
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Carbon Dioxide means "Carbon and two (di) oxygens".  Which means it's CO2\n\nMost of the other ones you asked can be figured out the same way.\n\n"Mon" = 1\n"Di" = 2\n"Tri" = 3\n"Tetra" = 4\n\nYou're not doing yourself any favors by having everyone else tell you all the answers - you need to LEARN this stuff, not just copy and paste someone else's answers.
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BALANCED . . . \n\n2Sr + O2 ---> 2SrO\n\n. . . and solved . . .\n\nGet an "A".
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1.) 2Ni + O2 -->  2NiO  (since it's Nickel II and Oxygen has a charge of -2, but you always have to put oxygen in groups of 2)\n\n1.) 2H2O --> 2H2 +O2  (same with hydrogen)\n2.) 2Al2O3 (because Aluminum has a charge of +3) --> 4Al + 3O2\n3.) 2NaCl --> 2Na + Cl2 (basically the rest follow the same rules)\n4.) 2NH3 --> 3H2 + 2N\n5.) 2HgO --> 2Hg + O2
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Oxygen has a molecular mass of 16 amu.\nHydrogen has a molecular mass of 1 amu.\n\nIn water, the total mass is 18.\nH=2 and O=16\nThink of this almost like lowest common denominators in fractions.\nthe ratio is as follows:\nyou need 16 Hydrogens to equal the mass of one oxygen\nbut water has a pair of hydrogens. There are two hydrogens for every oxygen. \nThus the ratio is 8:1.\n\nIn Hydrogen peroxide:\nthere are two hydrogens for every two oxygens.\nSimply, there is one hydrogen per oxygen.\nOxygen weighs 16 times as much as hydrogen.\nTHe ratio is 16:1.
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See if this article has a diagram\n\nhttp://jchemed.chem.wisc.edu/Journal/Issues/1999/Apr/abs542.html
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Mercury(II) oxide decomposes into its elements when heated.\nThere is no way that you would know this unless you had been taught about thermal decomposition. So all you need to worry about is the correct formula of oxygen gas.\n\nTherefore 2HgO --> 2Hg + O2.
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Haven't had chem in a while but maybe it would help to write out all the individual symbols.  Your second example would look like\n\nHHHPOOOO + MgOOHH  = MgMgMgPPOOOOOOOO + HHO\n\nthen you can see that the left side needs three Mg so you'd need 3 of the Mg(OH)2 to balance.  The left side also needs two P so there needs to be two H3PO4 there.  This makes a total of 12 H on the left, so to balance that you need 6 H2O on the right.  This also gives 14 O on the right to balance the 14 O you'd now have on the left.  So\n2 H3PO4 + 3 Mg(OH)2 = Mg3(PO4)2 + 6 H2O
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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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1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 4.793 g x (12 / 44) = 1.307 g\nhydrogen: 2.452 g x (2 / 18) = 0.272 g\noxygen: 2.018 - 1.307 - .272 = 0.439 g\n\n2) convert to moles.\ncarbon: 1.569 / 12 = 0.109 mol\nhydrogen: 0.272 / 1 = 0.272 mol\noxygen: 0.439 / 16 = 0.0274 mol\n\n3) divide each molar amount by the lowest value to find small integers:\ncarbon: 0.109 / 0.0274 = 4\nhydrogen: 0.272  / 0.0274 = 10\noxygen: 0.0274 / 0.0274 = 1\n\nThe empirical formula of the substance is (C4H10O)n\nThe atomic masses add up to 74, which is also the molar mass of the compound. Therefore n=1 and we find C4H10O
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H\n |    \nC=O:  (You need 2 lone pairs on Oxygen)\n |   \nH\n\nIt doesnt get much better than that :)
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they are called allotropes.  An example is diamond, and graphite. Both are pure carbon, but the bonding structures are different.  another example is O2 (oxygen gas) and O3 (ozone gas). Both are pure oxygen but the molecules are different.
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Typical Oxygen is O2 and it shares 2 electrons with each other. If you need the charge it is -2 meaning it is looking to gain 2 electrons to be neutral.