Redox Reactions

Cl2 + Co 2--> Cl- + Co2+

species oxidized?
species reduced?
oxidizing agent?
reducing agent?

As the reaction proceeds, electrons are transferred from?

Co

Cl
Cl
Co
Co
Cl

Loss of electrons is oxidization.

Gain of electrons is reduction.
The substance oxidized is the reducing agent.
The substance reduced is the oxidizing agent.

To determine the species oxidized, reduced, oxidizing agent, and reducing agent, we need to compare the oxidation states of the elements before and after the reaction.

In the given redox reaction:

Cl2 + Co --> Cl- + Co2+

The oxidation state of chlorine (Cl) changes from 0 to -1, so it is reduced. Hence, chlorine is the species reduced.

The oxidation state of cobalt (Co) changes from 0 to +2, so it is oxidized. Therefore, cobalt is the species oxidized.

The reducing agent is the species that is oxidized, so cobalt (Co) is the reducing agent.

The oxidizing agent is the species that is reduced, so chlorine (Cl) is the oxidizing agent.

As the reaction proceeds, electrons are transferred from cobalt (Co) to chlorine (Cl).

To determine the species being oxidized and reduced in a redox reaction, as well as identifying the oxidizing and reducing agents, we can consider the changes in oxidation states of the elements involved.

In the given reaction: Cl2 + Co2+ -> Cl- + Co2+

1. Species oxidized: The species that undergoes an increase in its oxidation state is the one being oxidized. In this case, the chlorine (Cl2) goes from an oxidation state of 0 (elemental form) to -1 (as chloride ion, Cl-). Therefore, chlorine is being oxidized.

2. Species reduced: The species that undergoes a decrease in its oxidation state is the one being reduced. In this case, cobalt (Co2+) goes from an oxidation state of +2 to +2 (there is no change in the oxidation state). Therefore, cobalt is not being reduced, and there is no reduction happening in this reaction.

3. Oxidizing agent: The oxidizing agent is the species that causes the oxidation to occur. It accepts electrons from the species being oxidized. In this reaction, since chlorine is being oxidized, the chlorine molecule (Cl2) is acting as the oxidizing agent.

4. Reducing agent: The reducing agent is the species that causes the reduction to occur. It donates electrons to the species being reduced. In this reaction, since there is no reduction happening, there is no reducing agent involved.

5. As the reaction proceeds, electrons are transferred from the species being oxidized to the oxidizing agent. In this case, electrons are transferred from the chlorine molecule (Cl2) to the chlorid