Question

Observe the following reaction: \[ {H}_2{O}(s) + {F}_2(g) \rightarrow {HF}(g) + {HOF}(g) \] In this reaction, identify the correct redox changes.

• A. Hydrogen is reduced and fluorine is oxidized
• B. Oxygen is reduced and fluorine is oxidized
• C. Oxygen is oxidized and fluorine is reduced
• D. Hydrogen is oxidized and fluorine is reduced

Hint:

Always check for changes in oxidation states to accurately identify reductions and oxidations in a redox reaction.

Answer 1

The Correct Option is C

Step 1: Determine the initial oxidation states. In \({H}_2{O}\), hydrogen has an oxidation state of +1, and oxygen has -2. In \({F}_2\), fluorine is 0 because it is a diatomic molecule. 
Step 2: Determine the final oxidation states. In \({HF}\), hydrogen remains at +1, and fluorine is -1. In \({HOF}\), hydrogen is +1, oxygen is -2 (like in water), and fluorine is -1. 
Step 3: Analyze the changes in oxidation states. Hydrogen's oxidation state does not change (+1 in all compounds). Fluorine's oxidation state changes from 0 in \({F}_2\) to -1 in \({HF}\) and \({HOF}\), indicating reduction. Oxygen's oxidation state does not change in this reaction. 
Step 4: Conclusion. Since fluorine's oxidation state decreases, it is reduced. Oxygen and hydrogen do not undergo any redox changes in terms of oxidation states in this particular reaction.