Aluminum is put into copper chloride and how can you tell what happens to them visually?
appropriate you're watching basically worry-unfastened atoms of rely. Protons are somewhat charged debris, the quantity of protons an atom has determines the form of atom itself. for example one proton is hydrogen, six protons is for carbon, etc. The neutrons are have not have been given any can charge in an atom, and help stabilize the atom. undergo in techniques like expenses repel eachother, neutrons carry the protons at the same time. They the two have basically approximately the comparable mass. finally electrons have a adverse can charge and bypass around atoms in unpredictable techniques. The closer the kind of electrons there are in an atom to protons, the greater impartial that's. An atom is impartial at the same time as there are 8 valence electrons indoors the outer shell distinctive than fir helium with basically 2. undergo in techniques, that's basically your undertaking-loose grade 9 stuff, now no longer the actual fact i understand.
This reaction occurs because Al is above Cu in the activity series.Al is oxidized and the copperis reduced. 2 Al^0(s) + 3Cu2+(aq) -- 2 Al3+(aq) + 3 Cu^0(s)
The aluminum metal appears to be turning into copper, but it is actually just removing the metallic copper from its compound state. The Aluminum is oxidized and loses e-, becoming Al 3+ and the copper ions are reduced (they accept those e-) to form solid copper precipitate. The aluminum ions and chloride ions remain in the solution. The reaction will only occur in water and occurs because the transfer of electrons from the aluminum to the copper results in a more stable system.
Aluminum will reduce copper ions (and be oxidized) when chloride ions are present. Otherwise aluminum metal will pretty much just sit there. The reason is the passivating layer of Al2O3 on the surface of any piece of aluminum. This metal oxide layer prevents the metal from actually reacting. But in the presence of chloride ion in water, Al2O3 will react, resulting in AlCl4^- and OH- ions. Al2O3(s) + 8Cl- + 3H2O(l) -- 2AlCl4^- + 6OH- This allows the aluminum metal to come into contact with copper ions resulting in the redox reaction: 2Al(s) + 3Cu2+ -- 2Al^3+ + 3Cu(s) There is a side reaction where aluminum metal reacts with water, and hydrogen gas is produced. 2Al(s) + 2H2O --2 AlOH^2+ + H2(g) When you actually observe the reaction, you will see copper metal being formed, aluminum metal dissolve and bubbles of hydrogen gas being given off. ============ Follow up ============= Because of the passivating effect of Al2O3 and the fact that Al2O3 dissolves in the presence of Cl- forming a new complex ion, AlCl4^-, Brian's answer leaves out a lot of the important chemistry.
