To determine if the given reaction is an oxidation-reduction (redox) reaction, we must analyze the changes in oxidation states of the elements involved.
In the reactants, we have:
- Si in SiBr4 has an oxidation state of 0 (elemental state).
- Br in SiBr4 has an oxidation state of -1.
- Ba is in elemental form, so its oxidation state is 0.
In the products:
- Si is in elemental form again, so its oxidation state is 0.
- In BaBr2, Ba has an oxidation state of +2 and Br has an oxidation state of -1.
Next, let’s identify any changes in oxidation states:
- Si starts at 0 and remains at 0 (no change).
- Br stays at -1 (no change).
- Ba starts at 0 and goes to +2 (it is oxidized).
Since Ba is oxidized, it loses electrons, making it the reducing agent. On the other hand, the Si is reduced from being part of SiBr4 (where it can be considered to hold a positive state due to its bond with Br) to elemental Si (0 oxidation state), even though there is no actual gain in electrons from the perspective of oxidation states after it debuted in the reactants.
In conclusion:
- This reaction is indeed an oxidation-reduction (redox) reaction.
- The oxidizing agent is SiBr4.
- The reducing agent is Ba.
- The substance being oxidized is Ba.
- The substance being reduced is Si.
In summary, the reaction involves the transfer of electrons, confirming its classification as a redox reaction.