What is the oxidation state of Mn in the given reaction involving MnF\(_3\) and Mn\(_2\)O\(_3\)?
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To determine the oxidation state of a transition metal in a compound, balance the charges of the ions in the compound based on known oxidation states of the other elements.
Step 1: Understanding the Compounds.
The compound \( \text{MnF}_3 \) contains manganese in the +3 oxidation state (since fluoride is typically -1). Similarly, \( \text{Mn}_2\text{O}_3 \) has manganese in the +3 oxidation state, as oxygen is -2.
Step 2: Analyzing the Options.
- (A) Mn in +2 is incorrect for this reaction.
- (B) Mn in +3 is the correct answer because both \( \text{MnF}_3 \) and \( \text{Mn}_2\text{O}_3 \) have Mn in the +3 oxidation state.
- (C) Mn in +4 is not correct for this reaction.
- (D) Mn in +5 is also incorrect.
Step 3: Conclusion.
The correct answer is (B) Oxidation state of Mn is +3.
