Answer: Undergoes disproportionation (one F atom is 0→-1 and the other is 0→+1 in HOF).
- A Undergoes disproportionation (one F atom is 0→-1 and the other is 0→+1 in HOF)
- B Is mainly reduced, with both fluorine atoms ending at the -1 oxidation state
- C Is mainly oxidised, with both fluorine atoms ending at a positive oxidation state
- D Does not change oxidation state throughout the reaction in typical laboratory settings
Correct answer: A. Undergoes disproportionation (one F atom is 0→-1 and the other is 0→+1 in HOF)
Explanation: One F₂ molecule gives HF (F = -1, reduced) and HOF (F = +1 in HOF; O is -2, H is +1, so F = +1, oxidised). This is disproportionation: F goes from 0 to both -1 and +1 simultaneously.
Electron transfer in a redox reaction: zinc loses electrons (oxidised, acts as reducing agent) and copper(II) ions gain those same electrons (reduced, acts as oxidising agent).
Concept context
Master electron transfer in chemistry: assign oxidation states, balance half-reactions, identify oxidising and reducing agents, and connect redox to everyday reactions.