Lab: Creating a Redox Table
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 solutions of ions.
I 2(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. Reactions 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)
Br 2(aq)
X
X
T
Cl 2(aq)
T
X
T
I 2(aq)
X
X
X
Legend:
T = evidence redox reaction occurred
X = no evidence of redox reaction
Sorry.... the tables not supposed to turn out liek that. Can anyone show me how the table can be improved?
Table 1: 4 vertical columns, 4 horizontal columns (on top)
Table 2: 4 vertical columns, 4 horizontal columns (on top)
Table 3: 3 vertical columns, 3 horizontal columns (on top)
Would it be possible if I scanned the table and sent it through as a jpg image?
These boards have a problem with spacing, as you have just proved to yourself. I don't think you can scan an image into the page. We can't draw structures of compounds, either, but sometimes we can use ingenuity and rearrange them so we can draw them. I have seen them done this way and that might be something to play with; for example,
Column 1...Column 2... Column3...Column 4
I2(aq).....Cu^+2(aq)...Ag^+(aq)..Br2(aq)
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 create a single table of relative strengths of oxidizing and reducing agents, we need to analyze the results from the three given tables.
Start by examining Table 1, which shows the reactions of metals and nonmetals with solutions of ions. The legend tells us that "T" represents evidence of a redox reaction and "X" indicates no evidence of a redox reaction.
Looking at the first row, we see that when Iodine (I2(aq)) reacts with various ions, there is evidence of a redox reaction (T) when it reacts with Br-(aq) and Cu2+(aq), but no evidence (X) when it reacts with Ag+(aq).
Similarly, for Copper (Cu), there is evidence of a redox reaction (T) when it reacts with I-(aq) and Ag+(aq), but no evidence (X) when it reacts with Cu2+(aq).
Lastly, for Silver (Ag), there is evidence of a redox reaction (T) only when it reacts with I-(aq).
Now, move on to Table 2, which shows the reactions of metals and solutions of ions. Again, refer to the legend: "T" represents evidence of a redox reaction and "X" indicates no evidence of a redox reaction.
Analyzing the first row, we can see that Silver (Ag) shows no evidence (X) of a redox reaction when it reacts with any of the ions listed.
Pb(s) shows evidence of a redox reaction (T) when it reacts with Ag+(aq) and Cu2+(aq), but no evidence (X) when it reacts with Pb2+(aq).
Cu(s) shows evidence of a redox reaction (T) when it reacts with Ag+(aq), but no evidence (X) when it reacts with Cu2+(aq).
Lastly, Zinc (Zn) shows evidence of a redox reaction (T) when it reacts with Ag+(aq), Pb2+(aq), and Cu2+(aq).
Moving to Table 3, which shows the reactions of nonmetals with solutions of ions. Again, refer to the legend: "T" represents evidence of a redox reaction and "X" indicates no evidence of a redox reaction.
Analyzing the first row, we can see that Iodine (I2(aq)) shows evidence of a redox reaction (T) only when it reacts with Br-(aq).
Chlorine (Cl2(aq)) shows evidence of a redox reaction (T) when it reacts with Br-(aq) and I-(aq), but no evidence (X) when it reacts with Cl-(aq).
Finally, Bromine (Br2(aq)) shows evidence of a redox reaction (T) only when it reacts with I-(aq).
Combining the information from all three tables, we can create a single table of relative strengths of oxidizing and reducing agents:
```
Cu2+ Ag+ Br2 Cl- I-
I2(aq) Reaction: X X T X X
Cu(s) Reaction: T T T X X
Ag(s) Reaction: X X X X T
Br-(aq) Reaction: X X X T X
------------------------------------------------------------------
Ag+ Reaction (Table 2): X X X X X
Pb2+ Reaction (Table 2): X X T X X
Cu2+ Reaction (Table 2): X X X X X
Zn2+ Reaction (Table 2): X X X X X
------------------------------------------------------------------
Br2(aq) Reaction (Table 3): X X T X X
Cl2(aq) Reaction (Table 3): X X X T X
I2(aq) Reaction (Table 3): X X X X X
```
This table summarizes the relative strengths of oxidizing and reducing agents based on the results from the three given tables. Remember, "X" indicates no evidence of a redox reaction, and "T" represents evidence of a redox reaction.