What is irrediam copper?
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After looking it up on the internet, it looks like a scam.  Try looking up Iridium Copper and see for yourself.
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Equation becomes CuCl2 + 2KI --> CuI2 + 2KCI\n\nProducts are Cuprous Iodide and Potassium Chloride
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copper most easily interact with oxygen than the other metals\ncoins are made of
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Hydrogen peroxide can oxidize copper metal on the surface of the penny by displacing it as copper(II) ions.  See link for detail explanation.
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A di-electric union sold in plumbing stores. Example if you have iron pipe and you want to join to copper. Any good plumber could tell you at the hardware store.
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8-hydroxyquinoline is a complexing ligand used for the extraction of transition metal ions. Commonly used for complexation of nickel, copper, etc. It also has use as a fungicide and antibacterial agent.\n\nIf you omit this material from the experiment, you will fail to extract the nickel from solution.
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Cu2S + 12HNO3 -> Cu(NO3)2 + CuSO4 + 10NO2 + 6H2O\n\nThere you go.
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1) Fe(s) +Cu^2+(aq) --> Fe^2+(aq) + Cu(s)  Single replacement, redox reaction where iron is oxidized and copper is reduced\n\n2) 2Al(s)+(3/2)O2(g)-->Al2O3(s)\nredox reaction, oxygen is reduced (neutral to -2) and aluminum is oxidized (neutral to +3)
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Gold AU\nSilver AG\nLead PB\nCarbon C\nNickle NI\nIridium IR\nZR Zirconium\nCU copper\nLi Lithium
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It's an iron oxide and it forms in an oxidising environment. Rich deposits may be the result of weathering, or precipitation out of oxygen-rich surface water or oxygen-rich water in hydrothermal veins.\n\nAs to why it is sometimes red and sometimes metallic-grey I'd say it is probably due to the size of the crystals. When it is ground up fine, it is always red. The smaller grains scatter red light.
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like the 1st guy said, u need the coordination number. if the no. of ligands is 6 (as copper has a tendency to form octahedral complexes) its Cu(NH3)6
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copper metal is listed as "very unreactive".  This means it is relatively stable as a metal, and relatively unstable as an ion.\n\nMagnesium metal "reacts with acids" so it is more stable in ionic form than copper,and less stable as pure metal.\n\nThe goal of nature is to go from an net unstable form to a more stable form.  (This is called reducing the free energy, or delta G of a system).\n\nIn order to use the activity series:\n\nany metal below a given metal is less stable in ionic form and more stable as a pure metal.\n\nThis means that a pure metal can reduce the ions of any metals below it.\n\nFor example, aluminum metal can reduce manganese ions, zinc ions, and so on because they are below it.\n\nAluminum metal cannot reduce magnesium ions, calcium ions, and other metals above it.\n\nI hope you can get it now.  Ok I am sure what I typed is correct now.  Good luck!\n\nhttp://en.wikipedia.org/wiki/Activity_series
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Cu.\nIt is a transition metal with ions of Cu+ and Cu2+.
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it's either copper or iron.  i don't remem ber exactly which one.
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The net ionic equation is:\n\nFe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s)
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(NH4)2S.  Cu2S is dark in color.
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KCl + Cu(Cr2O7)\n\nDichromate has 2 Chromium +6s to counter the 7 oxygen -2s.  +2 + -2 = 0\n\nPotassium Chlorite and Copper Dichromate