Editing Metallic bonding (section)

==Solubility and compound formation==
Metals are insoluble in water or organic solvents, unless they undergo a reaction with them. Typically, this is an oxidation reaction that robs the metal atoms of their itinerant electrons, destroying the metallic bonding. However metals are often readily soluble in each other while retaining the metallic character of their bonding. Gold, for example, dissolves easily in mercury, even at room temperature. Even in solid metals, the solubility can be extensive. If the structures of the two metals are the same, there can even be complete solid [[solubility]], as in the case of [[electrum]], an alloy of silver and gold. At times, however, two metals will form alloys with different structures than either of the two parents. One could call these materials [[Intermetallics|metal compounds]]. But, because materials with metallic bonding are typically not molecular, Dalton's [[Law of definite proportions|law of integral proportions]] is not valid; and often a range of stoichiometric ratios can be achieved. It is better to abandon such concepts as 'pure substance' or 'solute' in such cases and speak of [[phase (matter)|phase]]s instead. The study of such phases has traditionally been more the domain of [[metallurgy]] than of [[chemistry]], although the two fields overlap considerably.