Ozone is an extremely powerful oxidizing agent. It is — p Block Elements Chemistry Question

💡 Solution & Explanation

I notice the question is incomplete — the options aren't provided, so I cannot identify what option A states. However, here's the key reasoning about ozone as an oxidizing agent: **Why Ozone is a Powerful Oxidizer:** 1. **High reduction potential**: Ozone ($O_3$) has a standard reduction potential of ~+2.07 V, among the highest of common oxidizing agents. 2. **Unstable structure**: The bent $O_3$ molecule is thermodynamically unstable and readily decomposes: $$O_3 \rightarrow O_2 + [O]$$ releasing atomic oxygen $[O]$, which is extremely reactive. 3. **Mechanism**: Ozone oxidizes substances by either: - Direct addition across double bonds - Accepting electrons (getting reduced to $O_2$ or $O^{2-}$) 4. **Strength ranking**: Among common oxidizers: $O_3 > Cl_2 > Br_2 > I_2$ **To verify option A**, please provide the complete options. Common correct statements about ozone include: - "...unstable and decomposes easily" - "...more powerful than chlorine" - "...used for disinfection/sterilization" - "...forms atomic oxygen"