Which elements on the periodic table like to be oxidized and which like to be reduced?
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I love chemistry. =P Though I last did chemistry in 1999...hmm.\n\nAnyway, ignore the group 8 elements (inert gases)..you know why. =P\n\nAlright, Group 1 and Group 2 are the 'metals', and they carry one/2 extra electrons in their orbits, which they 'readily donate' (i.e. they are reduced), hence this makes them oxidising agents in nature! Hence, to answer your question, these Group 1, Group 2 (and some Group 3, e.g. Aluminium) like to be reduced. (reactivity decreases along from left to right of the groups)\n\nElements on the opposite end of the periodic table (group 6, 7, eg. CL, F.. and some group 5 (use the "step ladder" to determine, e.g. Asitine)) are your reducing agents, because they 'need' electrons (i.e. to be oxidised) in order to have a complete stable orbit (1s, 2s, 2d, 3s, 3d, 3f..) ..hence, to answer your question, these like to be oxidised.
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D. Mg, because it will oxidize instead of the iron.
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They usually are not defined that way, but you can have:\n\n1. Redox in base solutions\n2. Redox in acid solutions\n3. Single species where the same species (such as I2) is bothe the oxidizing and reducing agent.\n4. Non water based\n5. Molten (no solvent at all) other than the components\n6.spontaneous/non-spontaneous
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"Redox" metals have more than one oxidation state.  e.g. Fe2+/Fe3+ or Cu1+/Cu2+.  Zn and Ca only occur in biological systems in the 2+ state (therefore they cannot redox cycle).
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Huge order. Let's see how far it can be served.\n\n1. Monoatomic negative ions: take the element name (sometimes shortened) and add "-ide" (as in hydride, nitride, oxide, sulphide, phosphide, chloride...)\nPositive ions: element-name, charge (if several charges are possible), ion (sodium ion, iron II ion...)\n\n2. Polyatomic ions:\nComplexes with various ligands list the ligands and the central ion/atom.\nOxygen as ligands has its own nomenclature, depending on oxidation state. E.g. Sulphate, sulphite, perchlorate, chlorate, chlorite, hypochlorite...\n\n3. Binary molecular compounds: Halogen, oxygen and sulphur compounds usually have the correspondent "-ide" as if you had ionic compounds. Usually the more electropositive element is used as center.\n\n4. Acids: Oxygen acids have a similar nomenclature to oxygen ions.
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LHS:\nPb4+\nSn2+\nCl-\n\nRHS:\nPb2+\nSn4+\nCl-\n\nOxidation number of Pb in PbCl4 decreases = it is reduced = it oxidizes the other = it is the oxidizing agent
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reduced: 2H2O + 2e- ---> H2 + 2OH-\n\noxidized: 2I- ---> I2 +2e-
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Fe2O3+3CO--->2Fe+3CO2:  The Fe2O3 (oxidizing agent) is reduced to 2Fe, and the 3CO (reducing agent) is oxidized to form 3CO2.\n\nSnO2+C--->Sn+CO2:  The SnO2 (oxidizing agent) is reduced to form Sn, and the C (reducing agent) is oxidized to form CO2.\n\nRemember, oxidation means gaining oxygen (and losing electrons), and reduction means losing oxygen (and gaining electrons).
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An oxidation reaction.\n\nAn oxidation reaction is associated with the loss of electrons.  The lost electrons have to go somewhere and thus a reduction reaction, which is associated with the gaining of electrons, occurs accompanies it.
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Just answered it in your other post, but perhaps this: Oxidation-reduction is a chemical reaction in which an atom or ion loses electrons to another atom or ion.
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Boron, Carbon, Nitrogen, Oxygen
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copper most easily interact with oxygen than the other metals\ncoins are made of
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Molecular oxygen is an oxidizing agent. Every molecule that is oxidized, requires an oxidizing agent. Molecular chlorine might work but is so corrosive that the plant would die.
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Differs from element to element.\n\nLow oxidation states have colours like green, higher ones are bluish.
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The metal which is the furtherest to the right-hand top corner of the periodic table will be the most electronegative. Those who said fluorine didn't read the question properly because you are asked for a metal and fluorine, although the most electronegative 'element', is not a metal. In answering this question, I'm going to assume that the metalloids aren't included and not a subset of the cagetory of metals. The most electronegative metal would be aluminium (13). Have a look at the periodic table, it's the element which is closest to the top-right hand side but is still classified as a metal.
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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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Within each half-reaction, the charge on each side must be balanced, as well as the number of each element.\n\nFor the overall oxidation-reduction reaction, the charge on each side must be the same, as well as the number of each element, and no free electrons should be in the equation.