Question41) (Bonus Question) What is the strongest oxidizing agent of the following set: $\mathrm{FeO}_{2} \mathrm{Fe}_{2} \mathrm{O}_{3}$ . $\mathrm{Fe}_{3} \mathrm{O}_{4}$ , $\mathrm{FeO}_{4} 2-$ ? A) FeO B) $\mathrm{Fe}_{2} \mathrm{O}_{3}$ C) $\mathrm{eO}_{4}^{2-}$ D) $\mathrm{Fe}_{3} \mathrm{O}_{4}$ +2 $+3$ $+6$ $+2,+3$ $\left(\mathrm{FeO} \bullet \mathrm{Fe}_{2} \mathrm{O}_{3}\right.$

Studdy Solution
Compare the oxidation states:
- The highest oxidation state is $+6$ in $\mathrm{FeO}_{4}^{2-}$ .
Therefore, the strongest oxidizing agent is the compound with the highest oxidation state of iron.
The strongest oxidizing agent is:
$\boxed{\mathrm{FeO}_{4}^{2-}}$

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