Copper metal with silver ion My book states that $\ce{2AgNO3(aq) +Cu -&gt;Cu(NO3^-)2(aq) +2Ag(s)}$. In addition to the formula, it also shows the following image:



As in the image it shows the salmon colored copper atoms are donating an electron to the $\ce{Ag+}$ ions. In the 2nd picture on the page it shows the $\ce{Ag}$ atoms on top of the salmon colored copper atoms. I would assume that the $\ce{Cu}$ and $\ce{Ag}$ form somewhat of an ionic bond, is this correct to say? If that is the case, why does the formula not indicate a bond between the copper and silver instead the overall product is just copper nitrate plus silver. I would think it would be something like $\ce{CuAg}$?
Actually the copper and silver aren't bonded. The silver that precipitates is pure. Also, a bond between two metals could not be ionic. Ionic bonds are always been metals and non-metals. Looking at the picture again, I think what may have thrown you off is that it looks like the silver at the end is Ag+. However, the silver is actually Ag+ in the beginning of the reaction when it is in the silver nitrate. That's how it is bonded with the nitrate. When the copper donates an electron to the silver, the silver goes from having a +1 charge to having no charge. It becomes neutral, and hence it doesn't bond with the copper.