what are the other chemical properties of the element copper?
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Here is a centralized page of information, with several links along the left side for more information:\nhttp://www.webelements.com/webelements/elements/text/Cu/key.html
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An alloy,not being a chemical compound exhibits individual properties of the combined metals .In addition certain desirable properties are gained by the alloy .
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It is not due to the chemistry of copper or gold.\n\nIt is due to the electronic band structure. The two metals unusually have a band structure that causes them to absorb light at certain frequencies rather than reflecting it.
701182
It depends on what you mean by "properties."  Mass is determined by the number of protons & neutrons in the nucleus.  That also relates to melting point and boiling point, though other factors affect those, too.  But the CHEMICAL properties are determined by the electrons, and specifically, the electrons in the outer shell (and next to outer shell, for the transition elements).  It's those electrons that determine if an element is a metal or nonmetal, what elements it will form bonds with, how reactive it is, etc.
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Copper has a higher melting and boiling point and better electrical conductivity.\n\nIf you are a die caster, Zinc would be better because it can be easily pressure die-cast and hence better accuracy in the cast component with minimal metal removal for finishing.
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* Name: copper\n    * Symbol: Cu\n    * Atomic number: 29\n    * Atomic weight: 63.546 (3) r\n    * CAS Registry ID: 7440-50-8\n      \n      Standard state: solid at 298 K\n      Colour: copper, metallic\n      Classification: Metallic\n\n    * Group number: 11\n    * Group name: Coinage metal\n    * Period number: 4\n    * Block: d-block
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Copper is used as it has high conductence.\nWith high conductence we get accurate results.\nThis is one the reasons why copper is used in \ncolorimeters.
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http://www.chemicool.com/definition/element.html\nis this what you mean? \n\nI don't think that this is a physical property although for the life of me I can't see why it couldn't be.
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Copper Metal is a reddish-brown colour, but copper changes colour when it oxidizes.  Pennies are an excellent example of green copper.  New pennies are red, but as they get older and oxidize they start to turn black (copper Oxide CuO) and then green (copper carbonate Cu2CO3).  Copper can also be blue as in Copper sulfate CuSO4, copper hydroxide Cu(OH)2 and copper nitrate Cu(NO3)2.
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Silver  is a chemical element with the symbol Ag (Latin: argentum). A soft white lustrous transition metal, it has the highest electrical and thermal conductivity of any metal and occurs in minerals and in free form. This metal is used in coins, jewelry, tableware, photography, and in mirrors.\nSilver is a very ductile and malleable (slightly harder than gold) univalent coinage metal with a brilliant white metallic luster that can take a high degree of polish. It has the highest electrical conductivity of all metals, even higher than copper, but its greater cost and tarnishability has prevented it from being widely used in place of copper for electrical purposes.\n\nPure silver also has the highest thermal conductivity, whitest color, the highest optical reflectivity (although it is a poor reflector of ultraviolet light), and the lowest contact resistance of any metal. Silver halides are photosensitive and are remarkable for the effect of light upon them. This metal is stable in pure air and water, but does tarnish when it is exposed to ozone, hydrogen sulfide, or air containing sulfur. The most common oxidation state of silver is +1 (for example, silver nitrate; AgNO3); a few +2 (for example, silver(II) fluoride; AgF2) and +3 compounds (for example, silver(III) persulfate; Ag2(SO5)3) are also known.\n\nNobody and nothing formed an element.
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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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Copper (II) nitrate, Cu(NO3)2, is dark blue.\nBarium nitrate, Ba(NO3)2, is white.\nIron (III) nitrate, Fe(NO3)3, is purple-greenish.\nLead (II) nitrate, Pb(NO3)2, is clear or white.\n\nNot sure what the orange is, but it's not one of those.
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Do your own homework girl!\n\nNon-metals are the elements in groups 14-16 of the periodic table. Non-metals are not able to conduct electricity or heat very well. As opposed to metals, non-metallic elements are very brittle, and cannot be rolled into wires or pounded into sheets. The non-metals exist in two of the three states of matter at room temperature: gases (such as oxygen) and solids (such as carbon). The non-metals have no metallic luster, and do not reflect light. They have oxidation numbers of ±4, -3, and -2. \n\nThe Non-Metal elements are: \nHydrogen \nCarbon \nNitrogen \nOxygen \nPhosphorus \nSulfur \nSelenium
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Best ones are the metal elements with "spare" electrons.\nGold\nSilver\nLead\nCopper\nIron\nEtc.\nPS Pure water doesn't conduct electricity - it's the impurities or trace elements that do the conducting
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Copper is used as a conductor and as a easily maliable (formable) metal.  It is also naturally anti-bacterial.
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Try the following website if this may be useful :\n\nwww.conexindia.com/copper_casting_alloys_datachart_CDA/copper_casting_alloys
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CuCl2 + 2NH4OH --> Cu(OH)2 + 2NH4Cl\n\nCu(OH)2 (s) + 4NH3 (aq)     ----->     Cu(NH3)4^2+