From single displacement reactions it is easy to see some metals are more reactive than others. For instance when iron combines with copper sulfate the iron "steals" the sulfate from the copper. This means if an activity series was created with the more reactive metal on top and the less reactive metal on bottom the result would be:

Iron Copper You will now perform a series of single displacements using metals and solutions containing metal ions. This will enable you to create your own reactivity series.

Reaction Plate Place a small amount CuSO 4 in 4 of the wells. Repeat the same step with solutions of Iron(II) chloride, zinc nitrate, aluminium nitrate, magnesium chloride

CuSO 4 FeCl 3 ZnNO 3 Al(NO 3 ) 2 MgCl 2

CuSO 4 FeCl 2 ZnNO 3 Al(NO 3 ) 2 MgCl 2 Place a small amount of Fe, Zn, Al, Mg, Cu in each of the wells but don’t place metals with solutions which are the same.

CuSO 4 FeCl 3 Zn(NO 3 ) 2 Al(NO 3 ) 3 MgCl 2 Fe Zn Al Mg Cu

Now observe the wells using a dissecting microscope to detect any evidence of chemical change. Construct an activity series based on the empirical evidence.

Fe Zn Al Mg Cu Zn Fe Al Mg Cu Cu Zn Fe Al Mg Mg Cu Zn Fe Al Al Mg Cu Zn Fe

Write a lab report. In the conclusion include balanced chemical equations for all observed single displacement reactions. There are more than 20 possible chemical reactions. For metals with multiple oxidation states write all possible reactions. If no reaction occurs write the reactants with an arrow and NR (no reaction) as the product. If Cu doesn’t react with MgCl 2 (aq) write: Cu + MgCl > NR follow this sequence:

CuSO 4 FeCl 3 Zn(NO 3 ) 2 Al(NO 3 ) 3 MgCl 2 Fe Zn Al Mg Cu

Products of Reactions x x x x x

x x x x x

Mg Al Zn Fe Cu