Rank the following metals by ease of oxidation from hardest to easiest?
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Copper, Iron, Chromium, Aluminium
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copper, silver, aluminum, lead, magnesium, platinum and tungsten
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Because most metals are susceptible to oxidation, having low electronegativities, prefering to be in a cationic form vs. the neutral element.  Only metals such as gold, which is resistant to oxidation, will be found pure in nature.
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Zinc Oxide\n\nGood source on the properties of Zinc Oxide:\nhttp://www.chemicalland21.com/industrialchem/inorganic/ZINC%20OXIDE.htm
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AlthoughO2 is a strong oxidizing agent, its oxidizing reactions are usually slow kinetically. Many flammable materials will exist in the presence of air until a flame or spark starts the reaction. The very electronegative nonmetals are poor reducing agents. \n\nF2 will oxidize all metals and most other substances. It must be stored in either nickel or copper containers because the fluorides of these metals form a film passivating the metal surface. \n\nFor more please visit:\nhttp://www.wou.edu/las/physci/ch412/nonmetal.htm
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the answer is (a)\nThe element Ti has an oxidation number of +4\n\nRemember this...\n1) oxidation number of Oxygen is -2 (there is some exceptions)\n2) oxidation number of Hydrogen is +1 (there is some exceptions)\n3) oxidation nember of Fluorine is ALWAYS -1 because it is the most electronegative element\n4) oxidation number of a compound (without charge on it) is 0\n5) oxidation nember of an ion or an ionic compound is equal to the charge number it carries...\n\nHere i'll only explain (a) for you and you should try to calculate the other 3 elements to confirm to answer...\n\nlet x be the oxidation number of Ti\nhence\nx + (-2)2 = 0\nx - 4 = 0 \nx = +4
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easiest = english\nhardest = latin
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Just in general\n\nAlkali Earth Metals- Pretty reactive they are found in many compounds\n\nBoron group- Low reactivity\n\nCarbon group- More reactive then boron group but still pretty low\n\nNitrogen group- More reactive then Carbon group\n\nOxygen group- Very reactive oxygen has an unually high affinty for electrons relative to where it is on the periodic table\n\nHalogen group- Even more reactive than oxygen th&#92;ey have very hi\naffinity for electrons\n\nNoble gases- Basically inert, they have a full outer orbital of electrons and will only react in rare cases such as with flourine
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1 Aluminum (III) Oxide\n\n2 Iron (II) Sulfide\n\n3 Silver (I) Nitrate\n\n4 Tin (IV) Nitrate\n\n5 Carbon Monoxide\n\n6 Magnesium Sulfide\n\n7 Lead (II) Oxide\n\n9(8?) Sulfur Hexafluoride\n\n10 Mercury (I) Chloride
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Pure silver is nearly white, lustrous, soft, very ductile, malleable, it is an excellent conductor of heat and electricity. It is not a chemically active metal, but it is attacked by nitric acid (forming the nitrate) and by hot concentrated sulfuric acid. It has the highest electrical conductivity of all metals, but its greater cost has prevented it from being widely used for electrical purposes.\n\nSilver is almost always monovalent in its compounds, but an oxide, a fluoride, and a sulfide of divalent silver are known. It does not oxidize in air but reacts with the hydrogen sulfide present in the air, forming silver sulfide (tarnish). This is why silver objects need regular cleaning. Silver is stable in water.\n\nProperties\n----------\nAtomic number 47\nAtomic mass 107.87 g.mol -1\nElectronegativity according to Pauling 1.9\nMelting point 962 °C\nBoiling point 2212 °C\nVanderwaals radius 0.144 nm\nIonic radius 0.126 nm\nIsotopes 11\nElectronic shell [ Kr ] 4d10 5s1\nEnergy of first ionization 758 kJ.mol -1\nEnergy of second ionization 2061 kJ.mol -1\nDiscovered by The ancients\n\nDensity of solid [/kg m-3]: 10490  \nMolar volume [/cm3]: 10.27  \nVelocity of sound [/m s-1]: 2600  \n\nElastic properties\nYoungs modulus [/GPa]: 83  \nRigidity modulus [/GPa]: 30  \nBulk modulus [/GPa]: 100  \nPoissons ratio [no units]: 0.37  \n\nHardnesses\nMineral hardness [no units]: 2.5  \nBrinell hardness [/MN m-2]: 24.5  \nVickers hardness [/MN m-2]: 251  \n\nElectrical properties\nElectrical resistivity [/10-8 Ω m; or mΩ cm]: 1.6  \n\nReflectivity [/%]: 97
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Depends on the application you have for the copper. You can shield it from oxygen and other corrosive agents using a protective atmosphere.\n\nAt 500°C exposed to atmospheric oxygen you will want a solid metal with a stable passivizing surface or too noble to react. Titanium or platinum will probably be overkill, stainless steel may discolour.\n\nOr you might be thinking about a sacrificial anode, leaving the copper intact but dissolving the connected material (e.g. zinc or magnesium).
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They are all row three transitions metals.  So the point about 5 valence electrons is correct depending on the oxidation state of the atom.
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a) sulfur tetrafluoride\nb) molybdenum tetrachloride\nc) cobaltous sulfide or cobalt sulfide\nd) SnO\ne) ferric chloride\nf) CrO3\n\nComment: the above names are the ones you're most likely to encounter in industry or in a real-world laboratory.  Few chemists out here would call FeCl3 "iron three chloride"!\n\nOh, I know, your teacher probably expects "sulfur (IV) fluoride, molybdenum (IV) chloride, cobalt (II) sulfide, and iron (III) chloride..."
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Solid in room temp, but melts in your hand (slightly above room temp)\n\nAlloys quickly with most metals.\n\nYou can read more at the following:
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1) ZnNO2\n2) Co(HSO3)3\n3) HgF\n4) Al2(CO3)3\n5) CeC2O4\n6) BaClO\n7) SnBr2\n8) Mg(HSO3)2
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Most efficient? If you don't have a lab, then I would assume just doing your best at grinding off the top layer, and trying to melt the shreddings down into a >70% gold alloy. Since gold's melting point is OVER 1000 degrees Celsius, I suppose your best bet is to heat the grindings as much as possible, and then pounding them together into a single mass (like a black-smith...or 'gold-smith'). But you have to realize HOW LITTLE gold is actually on there. The layer is so thin...sometimes merely 2-3 micrometers. You're gonna get a lot of impurities, such as nickel and copper. Gold-plating is usually done on copper or silver; and in the case of copper, a thin layer of nickel is placed below the gold. And since the melting point of nickel isn't that far from that of gold, and copper's is almost EXACTLY that of gold's, you're gonna get a random mixture of crap. I imagine the process is more trouble than it's worth. I'd just go buy gold from alfa aesar or somewhere like that for cheap-as-free.
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Metal\n\nChemical properties\n\nMost metals are chemically unstable, reacting with oxygen in the air to form oxides over varying timescales (for example iron rusts over years and potassium burns in seconds). The alkali metals react quickest followed by the alkaline earth metals, found in the leftmost two groups of the periodic table. The transition metals take much longer to oxidise (such as iron, copper, zinc, nickel). Others, like palladium, platinum and gold, do not react with the atmosphere at all. Some metals form a barrier layer of oxide on their surface which cannot be penetrated by further oxygen molecules and thus retain their shiny appearance and good conductivity for many decades (like aluminium, some steels, and titanium). The oxides of metals are basic (as opposed to those of nonmetals, which are acidic), although this may be considered a rule of thumb, rather than an absolute condition.\n\nPainting or anodising metals are good ways to prevent their corrosion. However, a more reactive metal in the electrochemical series must be chosen for coating, especially when chipping of the coating is expected. Water and the two metals form an electrochemical cell, and if the coating is less reactive than the coatee, the coating actually promotes corrosion.\n\nPhysical properties\n\nTraditionally, metals have certain characteristic physical properties: they are usually shiny (they have "lustre"), have a high density, are ductile and malleable, usually have a high melting point, are usually hard, and conduct electricity and heat well. However this is mainly because the low density, soft, low melting point metals happen to be reactive, and we rarely encounter them in their elemental, metallic form. Metals conduct sound well, that is, they are sonorous.\n\nThe electrical and thermal conductivity of metals originate from the fact, that in the metallic bond the outer electrons of the metal atoms form a gas of nearly free electrons, moving as an electron gas in a background of positive charge formed by the ion cores. Good mathematical predictions for electrical conductivity, as well as the electrons' contribution to the heat capacity and heat conductivity of metals can be calculated from the free electron model, which does not take the detailed structure of the ion lattice into account.\n\nWhen considering the exact band structure and binding energy of a metal, it is necessary to take into account the positive potential caused by the specific arangement of the ion cores - which is periodic in crystals. The most important consequence of the periodic potential is the formation of a small band gap at the boundary of the brillouin zone. Mathematically, the potential of the ion cores is treated in the nearly-free electron model.\n\nNonmetal\n\nMost nonmetals are found at the upper right of the periodic table. The exception is hydrogen, which is usually placed at the upper left with the alkali metals, but behaves like a nonmetal under most conditions. Unlike metals, which are electrically conductive, nearly all nonmetals are either insulators or semiconductors. Graphite, an allotrope of carbon, is an example of a nonmetal that does conduct electricity. Nonmetals may form ionic bonds with metals by gaining electrons, or covalent bonds with other nonmetals. The oxides of nonmetals are acidic.\n\nThere are only eighteen known nonmetals, compared to over eighty metals, but nonmetals make up most of the earth, particularly in the outer layers. Organisms are composed almost entirely of nonmetals. Many nonmetals (hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine) are diatomic, and most of the rest are otherwise polyatomic.\n\nMetalloid\n\nTogether with the metals and nonmetals, the metalloids (in Greek metallon = metal and eidos = sort) form one of the three categories of chemical elements as classified by ionization and bonding properties. They have chemical properties intermediate between those of metals and no