Write the balanced net ionic equations for the reactions of the halogens with copper metal. The halogens are oxidizing agents and the copper metal is a reducing agent.
a) Bromine (Br2)+copper metal (Cu)
b) Iodine (I2) + copper metal (Cu)
Based on your observations and knowledge of the redox potential series table with the diagonal rule:
a) Is copper metal an oxidizing agent or reducing agent?
b) Does it react with br2?
Does it react with I2?
Based on your observations and the diagonal rule place Cu on a halogen table in its proper location specifically with regards to Br2 and I2, making sure the pair is complete (ex. (Cu^2+----(Cu)).
Construct a single reduction potential series table by combining the 2 smaller tables from parts 2 and 3 based on your explanation from last part for the location (Cu^2+)----(Cu)
someone please help me with this or at least show an example very similar to this.
I assume you performed some experiment and you are to use your observations to help answers this question. What were your observations?
a) The balanced net ionic equation for the reaction between bromine (Br2) and copper metal (Cu) is:
2Br^- (aq) + Cu (s) → Cu^2+ (aq) + 2Br^- (aq)
b) The balanced net ionic equation for the reaction between iodine (I2) and copper metal (Cu) is:
I2 (aq) + 2Cu (s) → 2CuI (s)
a) Copper metal (Cu) is a reducing agent because it undergoes oxidation in these reactions, losing electrons to form Cu^2+.
b) Copper metal does react with Br2 to form Cu^2+ and 2Br^-, as shown in the balanced net ionic equation: 2Br^- (aq) + Cu (s) → Cu^2+ (aq) + 2Br^- (aq). Therefore, copper metal reacts with bromine.
Copper metal also reacts with I2 to form CuI, as shown in the balanced net ionic equation: I2 (aq) + 2Cu (s) → 2CuI (s). Therefore, copper metal reacts with iodine.
Based on the diagonal rule, copper (Cu^2+) is placed in the middle between bromine (Br^-) and iodine (I^-) on the halogen table, completing the pair:
(Br^-, Br2) ← Cu^2+ ((Cu)) → (I^-, I2)
To construct a single reduction potential series table, combine the halogen table and the copper table based on the explanation from the previous part:
F2 | Cl2 | (Br2) ← Cu^2+ ((Cu)) → (I2) | H2
The halogens are listed in order of increasing tendency to undergo reduction, and copper is in the middle as a transition element. H2 represents the reduction reaction with hydrogen.
To write the balanced net ionic equations for the reactions of the halogens with copper metal (Cu), we need to consider their redox reactions.
a) Bromine (Br2) + copper (Cu):
First, we need to determine the oxidation states of each element in the reaction. Bromine is diatomic and typically has an oxidation state of 0. Copper is in its elemental form, so its oxidation state is also 0.
To balance the equation, we can follow these steps:
1. Write the unbalanced equation: Br2 + Cu -> ?
2. Identify the reduction and oxidation half-reactions:
The halogens are oxidizing agents, meaning they tend to gain electrons (undergo reduction), while copper metal is a reducing agent, meaning it tends to lose electrons (undergo oxidation).
Br2 (reduction): Br2 + 2e- -> 2Br-
Cu (oxidation): Cu -> Cu2+ + 2e-
3. Balance the reduction and oxidation half-reactions:
Multiplying the reduction half-reaction by 2 and adding it to the oxidation half-reaction, we get:
2Br2 + Cu -> 2Br- + Cu2+
The balanced net ionic equation is: Br2 + Cu -> 2Br- + Cu2+.
b) Iodine (I2) + copper (Cu):
Following a similar process, we determine the oxidation states:
Iodine: 0
Copper: 0
1. Write the unbalanced equation: I2 + Cu -> ?
2. Identify the reduction and oxidation half-reactions:
I2 (reduction): I2 + 2e- -> 2I-
Cu (oxidation): Cu -> Cu2+ + 2e-
3. Balance the reduction and oxidation half-reactions:
Multiplying the reduction half-reaction by 2 and adding it to the oxidation half-reaction:
I2 + Cu -> 2I- + Cu2+
The balanced net ionic equation is: I2 + Cu -> 2I- + Cu2+.
a) Copper metal (Cu) is a reducing agent because it tends to lose electrons (undergo oxidation) in reactions.
b) Copper reacts with Br2 and I2, as shown in the balanced net ionic equations.
Based on the redox potential series table with the diagonal rule, we can determine the placement of Cu on a halogen table. The diagonal rule states that an element (in this case, Cu) lies on the same diagonal, below the elements it can reduce.
For Br2:
Br2 is higher in the redox potential series table than Cu. Therefore, Cu can reduce Br2.
For I2:
I2 is also higher in the redox potential series table than Cu. Therefore, Cu can reduce I2 as well.
The pair (Cu^2+----(Cu)) should be placed on the corresponding location on the halogen table.
To construct a single reduction potential series table, combining the information obtained from parts 2 (Br2) and 3 (I2), we would start with the highest oxidizing agent (highest up on the table) and move downward to the reducing agent (farthest down on the table).
Let's assume the original redox potential series table is as follows:
F2 > Cl2 > Br2 > I2
Inserting the pair (Cu^2+----(Cu)) based on the placement determined earlier, the revised table would be:
F2 > Cl2 > Br2 > Cu^2+----(Cu) > I2
Note: The exact values of the redox potential series would depend on the specific reference used. The above presentation is a simplified example for clarification purposes.