Final answer:
To predict the relative strengths of oxidizing agents, compare their reduction potentials; the one with the larger reduction potential is the stronger agent. Fluorine is the strongest oxidizing agent, followed by agents like permanganate and dichromate, based on their positions in the standard cell potential table.
Step-by-step explanation:
To predict the relative strengths of oxidizing agents, you can compare the reduction potentials of different substances. A larger reduction potential indicates a stronger oxidizing agent because it is more easily reduced. For instance, based on the standard cell potential table, fluorine (F₂) is the strongest oxidizing agent as it has the highest reduction potential, meaning it can oxidize any substance below it on the table.
To analyze a chemical reaction, break it down into a net ionic equation and then into half-reactions. The substance that gains electrons in the half-reaction is being reduced and acts as the oxidizing agent. Conversely, the substance that loses electrons is being oxidized and acts as the reducing agent. For example, in the reaction between arsenic and bromine, bromine is the oxidizing agent as it gains electrons.
- Fluorine (F₂)
- Permanganate (MnO₄¹⁻)
- Dichromate (Cr₂O⁷²⁻)