Fluorine reacts with ice and results in the change: H2O(s) + F2(g) ? HF(g) + HOF(g) Justify that this reaction is a redox reaction. ?

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This is a disproportionation reaction which is a special type of redox reaction. In this F is oxidised as well as reduced.
Oxidation: F2 → H-
reduction: H2O → HOF

In this case,F2 is reduced to HF and oxidised to HOF. Therefore, it is a redox reaction. HOF is unstable and decomposes to form O2 and HF.2HOF➡2HF+OFIndian this reaction, F of HOF is reduced while O of HOF is oxidised. Therefore, it is a redox reaction but not a disproportionatin reaction. If oxygen of HOF disproportionates, then oxygen must show three oxidation state. If we assume that oxidation state of O is zero in HOF, then it`s oxidation state decreases to -2. HOF is reduced to H2O and increases to +2 if HOF gets oxidised to OF2.Therefore, the possible reaction is-2HOF➡H2O+OF2