* Oxidation: Sulfur in H₂S goes from an oxidation state of -2 to 0 in elemental sulfur (S). This is an increase in oxidation state, indicating oxidation.

* Reduction: Bromine in Br₂ goes from an oxidation state of 0 to -1 in HBr. This is a decrease in oxidation state, indicating reduction.

Explanation:

* H₂S: In H₂S, sulfur is in the -2 oxidation state (hydrogen is +1).

* Br₂: In Br₂, bromine is in the 0 oxidation state (elemental form).

* HBr: In HBr, bromine is in the -1 oxidation state (hydrogen is +1).

* S: Elemental sulfur has an oxidation state of 0.

Overall:

* Sulfur in H₂S loses electrons (oxidation) and is oxidized to elemental sulfur (S).

* Bromine in Br₂ gains electrons (reduction) and is reduced to bromide ions (Br-) in HBr.

Therefore, the reaction is a redox reaction because it involves the transfer of electrons between reactants.