Final answer:
The question pertains to a redox reaction where BrO- is oxidized to BrO3- and Fe3+ is reduced to Fe2+. Examples demonstrate the concept of redox reactions, with a focus on changes in oxidation numbers and electron transfer to ensure electrical neutrality in balanced reactions.
Step-by-step explanation:
The student's question is about a redox reaction where BrO- is oxidized to BrO3- and Fe3+ is reduced to Fe2+. In redox reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). The provided examples describe different redox reactions, including the oxidation of iron (Fe) and the reduction of chlorine (Cl2) and bromine (Br). Each reaction is characterized by changes in the oxidation number of elements involved, indicating the loss or gain of electrons.
For instance, in the reaction 4 Fe + 3 O2 → 2 Fe2O3, iron (Fe) is going from an oxidation state of 0 to +3, thus it is oxidized, and oxygen (O) is going from an oxidation state of 0 to -2, thus it is reduced. Similarly, in the reaction Zn(s) → Zn2+(aq) + 2 e-, zinc (Zn) is acting as the reductant because it is losing electrons. It's important to balance redox reactions so that the number of electrons lost is equal to the number of electrons gained, ensuring that the overall reaction is electrically neutral.