Determination of an Activity Series

 

The purpose of this lab was to determine the oxidation potential of different metals with small scale chemical reaction activity series (basically finding which is more active). The results concluded that the different metals tested (Mg, Zn, Fe, Cu) were not equally active; Magnesium was the most active with four total reactions and a reduction potential of -2.37V, Zinc came in second with three reactions and -0.76 V potential, and Iron (2.87 V) and Copper (0.34 V)  tied for third with 2 reactions. The most reactive to the least seemed to have a connection towards the charge of the reduction potential. The most active, Mg, had the lowest potential while the least active metals had the highest potentials. This is because the negatively charged potentials need electrons. All of these reactions were single replacement and redox reactions. Redox reactions, or oxidation reduction reactions, involve the transfer of electrons between atoms and a change in the oxidation state. A single replacement reaction is when one element is replaced by another. Single replacement reactions are also redox reactions because the transfer of electrons occur with the transfer of elements.