The chemical reactivity of elements varies over immense range.Some, like sodium or fluorine are so reactive that they never foundin the free or uncombined state in nature. Others, like xenon orplatinum, are nearly inert and can react with other elements onlyunder special conditions.

The reactivity of an element is related to its tendency to loseor gain electrons; that is to be oxidized or reduced. In principleit is possible to arrange nearly all elements into a single seriesin order of their reactivities. A series of this kind indicateswhich free elements are capable of displacing other elements fromtheir compounds.

A generalized single replacement reaction is represented by theequation:

A(s) + BC(aq) ? B(s) + AC(aq)

Element A is the more active element and replaces element B fromthe compound BC. But if element B is more active than element A, noreaction will occur.

Consider two equations below:

2 Al(s) + 3 CuCl₂(aq) ? 3 Cu(s) + 2AlCl₃(aq) (1)

Cu(s) + AlCl₃(aq) ? Noreaction (2)

The reaction of aluminum with copper (II) chloride - equation(1) - is classified as a single replacement reaction becausealuminum “replaces” copper ions in copper (II) chloride. Reactionrepresented by equation (2) does not occur. A more activemetal always replaces the ion of a less activemetal.

Objectives:

To observe the results of a variety of single replacementreactions and become familiar with some signs of thisreactions.

To predict the products for each reaction which occur andpractice writing and balancing chemical equations.

To place elements involved in reaction in order of theiractivities – construct activity series.

Procedure:

Click on the link below or copy and paste it to yourbrowser.

http://intro.chem.okstate.edu/1515F01/Laboratory/ActivityofMetals/home.html

Click start. Click Activity 1. Follow instruction on the screento proceed with your experiment. Once a metal is removed from thesolution record your observation in data table 1. Determine whichmetal is more active and document it in data table 2.

Data:

Table 1 – write down your observation, note ifreaction occur or not.

	Metal
Aqueous solution	Mg	Cu	Zn	Ag
Mg(NO3)2	No reaction	No reaction	No reaction	No reaction
Cu(NO3)2	There was a reaction. Turned partially dark grey	No reaction	No reaction	No reaction
Zn(NO3)2	There was a reaction. Turned partially orange	No reaction	There was a reaction. Turned partially orange	No reaction
AgNO3	There was a reaction. Turned partially light grey	There was a reaction. Turned partially light grey	There was a reaction. Turned partially light grey	No reaction

Table 2 – based on your observation determinewhich of the two metals in each reaction is more active.

	Metal
More active
Less active

Table 3 – predict the products if reactionoccur, write and balance chemical equation.

Reaction	Equation
1
2
3
4
5
6

Results:

Place your four metals in order of activity, the most activefirst.

Post lab questions:

Complete activity 2, 3 and 4, using the same link.

Answer the following questions:

• Which of the metals reacted with the most solutions?

• Which of the metals reacted with the fewest solutions?

• If you want add Pb to your activity series, where it would beon the list? Why?

• Which of the solution used in your activity 1 would you expectto Fe react with? (refer to attached activity series).

Activity series.
lithium	Li	These metals displace hydrogen from water Ca(s) + 2H2O(l)?Ca(OH)2 + H2 (g) These elements are very reactive and react readily to form compounds
potassium	K
barium	Ba
calcium	Ca
sodium	Na
		These metals displace hydrogen from acids Zn(s) + HCl(aq)? ZnCl2 +H2(g)
magnesium	Mg
aluminum	A
zinc	Zn
chromium	Cr
iron	Fe
cadmium	Cd
nickel	Ni
tin	Sn
lead	Pb
hydrogen	H
copper	Cu	These metals do not displace hydrogen from acids or water These elements are more stable, and form compounds less readilythan do those higher in the table.
silver	Ag
mercury	Hg
platinum	Pt
gold	Au
least active