how many electrons take part in redox reaction: Cl2 -> ClO3^-
To determine the number of electrons taking part in a redox reaction, you need to analyze the change in oxidation numbers of the elements involved.
In the given reaction:
Cl2 -> ClO3^-
The oxidation state of chlorine (Cl) in Cl2 is 0 since it exists as a diatomic element. The oxidation state of oxygen (O) in ClO3^- is -2, and since there are three oxygen atoms, the total oxidation state for oxygen is -6. The overall charge of ClO3^- is -1, which means the oxidation state of chlorine is +5.
Now, we need to find the change in oxidation state. Chlorine goes from an oxidation state of 0 in Cl2 to +5 in ClO3^-. So, the change is +5 - 0 = +5.
To balance the equation in terms of electrons, the change in oxidation state must be equal to the number of electrons transferred.
Therefore, in this redox reaction, 5 electrons are taking part.
To determine the number of electrons involved in a redox reaction, we need to compare the oxidation states of the elements involved before and after the reaction.
In the reaction Cl2 -> ClO3^-, chlorine (Cl) is going from an oxidation state of 0 in Cl2 to +5 in ClO3^-.
To balance the oxidation state change, we can assign x electrons to each Cl atom participating in the reaction. Since Cl starts with an oxidation state of 0 and ends with an oxidation state of +5, it gains 5 electrons.
Therefore, the number of electrons taking part in this redox reaction is 5.