Purpose:

The purpose of this lab exercise is to construct a table of relative strengths of oxidizing and reducing agents. By completing this exercise, you will see how more extensive tables of relative strengths of oxidizing and reducing agents have been developed.

Procedure:
Using the results from the three tables below, prepare a single table of relative strengths of oxidizing and reducing agents

Table 1. Reactions of metals and nonmetals with solution of ions

I2(aq) Cu2+(aq) Ag+(aq) Br2(aq)
I-(aq) X X T T
Cu(s) T X T T
Ag(s) X X X T
Br-(aq) X X X X

Table 2.Reaction of metals and solutions of ions
Ag+(aq) Pb2+(aq) Cu2+(aq) Zn2+(aq)
Ag(s)X X X X
Pb(s)T X T X
Cu(s)T X X X
Zn(s)T T T X

Table 3. Reactions of nonmetals with solutions of ions
Br-(aq) Cl-(aq) I-(aq)
Br2(aq) X X T
Cl2(aq) T X T
I2(aq) X X X

Legend:
T = evidence redox reaction occured
X = no evidence of redox reaction

*Please note

For table 1 I2(aq), Cu2+(aq), Ag+(aq) and Br2(aq) are supposed to be shifted to the right since they are horizontal.
I-(aq), Cu(s), Ag(s) and Br-(aq) are vertical.

For table 2
Ag+(aq), Pb2+(aq), Cu2+(aq) and Zn2+(aq) are supposed to be shifted to the right since they are horizontal.
Ag(s), Pb(s), Cu(s) and Zn(s) are vertical.

For table 3
Br-(aq), Cl-(aq) and I-(aq) are supposed to be shifted to the right since they are horizontal.
Br2(aq), Cl2(aq) and I2(aq) are vertical.

To prepare a single table of relative strengths of oxidizing and reducing agents, we will combine the information from the three tables provided.

Table of Relative Strengths of Oxidizing and Reducing Agents:

I2(aq) Cu2+(aq) Ag+(aq) Br2(aq) I-(aq) Cu(s) Ag(s) Br-(aq)
I2(aq) X X X X T X X X
Cu2+(aq) X X X X X X X X
Ag+(aq) T X X X X X X X
Br2(aq) T T T X X X T X
I-(aq) T T T X X T X X
Cu(s) X T X X X X X X
Ag(s) X T X T X X X X
Br-(aq) X X X X X X X X
Pb2+(aq) X X X X X X X X
Zn2+(aq) X X X X X X X X
Pb(s) X T X X X T X X
Zn(s) X X X X X T X X
Cl-(aq) X X X X X X X X
Cl2(aq) X X X X X X X X

Legend:
T = evidence of a redox reaction occurring
X = no evidence of a redox reaction

Explanation:
To construct the table, we aligned the corresponding compounds and ions from each of the three tables. In each cell, we indicated whether there was evidence of a redox reaction occurring or not.

For example, in the cell where I2(aq) and Ag+(aq) intersect, we can see from Table 1 that there is evidence of a redox reaction occurring. Similarly, in the cell where Cu2+(aq) and Cu(s) intersect, there is evidence of a redox reaction occurring.

In some cases, there is no evidence of a redox reaction occurring, as indicated by the X. For example, in the cell where Ag+(aq) and Pb2+(aq) intersect, there is no evidence of a redox reaction occurring.

By combining the information from the three tables, we can create a comprehensive table that shows the relative strengths of oxidizing and reducing agents based on the observed redox reactions.

To prepare a single table of relative strengths of oxidizing and reducing agents, we can combine the information from the three given tables.

First, let's label the columns of the table as "Oxidizing Agents" and the rows as "Reducing Agents".

Now, let's fill in the table using the information from the three tables provided.

Starting with Table 1, we can see that in the row of I-(aq), there is evidence of a redox reaction with Cu2+(aq), Ag+(aq), and Br2(aq). Therefore, we can label these as "T" (evidence of redox reaction) in the corresponding cells of the table.

Moving on to the rows of Cu(s) and Ag(s), we can see that there is evidence of a redox reaction with Cu2+(aq) and Br2(aq). So we'll label these cells as "T" as well.

Finally, for the row of Br-(aq), there is evidence of a redox reaction with Br2(aq). Thus, we'll label this cell as "T".

Now, let's incorporate the information from Table 2.

Looking at the row of Ag(s), we can see that there is no evidence of a redox reaction with any of the listed oxidizing agents. Hence, we'll label these cells as "X" (no evidence of redox reaction).

For the row of Pb(s), there is evidence of a redox reaction with Ag+(aq) and Cu2+(aq). So we'll label these cells as "T".

Moving on to the row of Cu(s), we can see that there is evidence of a redox reaction with Cu2+(aq). Thus, we'll label this cell as "T".

Finally, for the row of Zn(s), there is evidence of a redox reaction with all the listed oxidizing agents. Therefore, we'll label these cells as "T".

Now, let's incorporate the information from Table 3.

In the row of Br-(aq), there is evidence of a redox reaction with Cl2(aq) and I2(aq). Hence, we'll label these cells as "T".

For the row of Cl-(aq), there is evidence of a redox reaction with Br2(aq) and I2(aq). So we'll label these cells as "T".

Lastly, in the row of I-(aq), there is no evidence of a redox reaction with any of the listed oxidizing agents. Therefore, we'll label these cells as "X".

After incorporating all the information, we have completed the single table of relative strengths of oxidizing and reducing agents based on the given data.