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Under certain conditions, H_{2}O_{2} can act as an oxidizing agent; under other conditions, as a reducing agent. A good theoretical explanation for this is that an atom within a compound can become more stable by either gaining OR losing electrons. Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a True b False

Answer :

Answer:

True

Explanation:

Not sure why but it's true.

The theoretical explanation given for the reason why H₂O₂ can act as an oxidizing agent and other times as a reducing agent is; True

We are told that under certain conditions, H₂O₂ can act as an oxidizing agent and under other conditions it can act as a reducing agent.

  • Now, an oxidizing agent is one that gains electrons and undergoes reduction in a chemical reaction while a reducing agent is one that loses electrons and undergoes oxidation in a chemical reaction.

       Now, an atom that loses electrons within a compound would become more stable if the loss of electrons means its' new valence shell has 8 electrons.

      Whereas, an atom that gains electrons within a compound would become more stable if the gain of electrons makes its' valence shell to fulfill the octet rule by having 8 electrons in its' outermost shell.

  • The oxygen atom in the given H₂O₂ (hydrogen peroxide), has an oxidation state of -1. Now, due to the fact that this -1 oxidation state lies between the more popular extremes of 0 and -2 oxygen oxidation states, it means that it can either act as an oxidizing agent or a reducing agent.

  • In conclusion, the theoretical explanation is true.

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