Activity Series of Metals
Introduction:
There are many ways to classify chemical reactions. Some might be classified as
acid –base, oxidation- reduction, or as synthesis or decomposition reactions. This
experiment will focus on single replacement reactions. In a single replacement reaction,
one element replaces another in a compound. When writing equations or predicting
products for these equations, it must be remembered that not all equations proceed as
written. For example, in the reaction between copper and silver Cu + AgNO3 → Ag +
Cu(NO3)2, the reaction proceeds as written. The reverse reactions, Ag + Cu(NO3)2 → Cu
AgNO3, however, does not occur.
Not all elements are equal in their ability to replace other elements. Metals, such
as sodium and potassium, are referred to as “active” metals. There metals can replace
hydrogen from water. K + H2O → KOH + H2. “Somewhat less active” metals, such as
aluminum, can’t displace hydrogen from water, but they can displace hydrogen from
acids such as a hydrochloric acid. Al + HCl → H2 + AlCl3. Some “less active” metals
will not displace hydrogen from HCl but will displace other metal ions in aqueous
solutions. The reaction Cu + AgNO3 → Ag + Cu(NO3)2, mentioned above, is an example
of such a reaction.
In order to predict products of single replacement reactions or to predict if they
will occur at all, a method is needed. An activity series allows one to make such
predictions. After observing or carrying out a series of reactions, you will construct an
activity series for some elements.
Purpose:
The purpose of this experiment is to construct an activity series fro tome metallic
elements.
Equipment/ Materials:
Metal samples: (Mg, Fe, Cu, Ca, Pb, Zn)
Solutions of the metals: Mg(NO3)2, FeSO4, Cu(NO3)2, Ca(NO3)2, Pb(NO3)2,
Zn(NO3)2
Test tubes/ test tube rack
Hot plate
24-well well plate
3 M HCl
Safety:
An apron and goggles should be worn in the lab.
