1. You are provided with two liquids, one is H₂O and the other is H₂O₂. Safety regulations now prohibit you from touching/tasting them so suggest chemical tests that could distinguish between them. Include the reagents and observations expected and show balanced equations for the reactions.


2. Use the MO diagram below to determine the bond order for the following species and predict whether the bond lengths shown are consistent with your values.
   

   O2+ = 112 pm O2 = 121 pm O2- = 128 pm O22- = 149 pm



3. With the aid of suitable equations describe how H₂O₂ can be produced industrially and on a small scale in the laboratory.


4. Write balanced half equations and the net ionic equation for:
   i) the oxidation of Fe²⁺ by H₂O₂ in acidic solution.
   ii) the reaction between KMnO₄ and H₂O₂ in acidic solution.
   iii) the reaction between acidified KBr and H₂O₂.


5. Describe two uses of D₂O, including the chief large scale use.


6. With the aid of equations, describe how ozone is produced and destroyed in the upper atmosphere.


7. How would you prepare ozone in the laboratory? What conditions and safety equipment would be needed?


8. What experiment/techniques could be used to distinguish between O₃ and O₂?


9. How does the O-O bond length in O₃ of 127.2 pm compare to the data above for O₂ species?

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