The correct answer is option 2 - water is oxidized to O2.

In the given chemical equation, fluorine (F2) reacts with water (H2O) to produce hydrogen ions (H+), fluoride ions (F-), and oxygen gas (O2). This reaction represents a redox (reduction-oxidation) reaction.

Option 1 is incorrect because fluorine is not oxidized to F, but rather it gains electrons by accepting electrons from water molecules. This is evident from the formation of fluoride ions (F-) in the reaction.

Option 2 is correct because water is being oxidized. This is indicated by the formation of oxygen gas (O2) as a product in the reaction.

Option 3 is incorrect because water is not reduced to H+. Instead, water molecules lose electrons and are broken down to form hydrogen ions (H+) as one of the products.

Option 4 is incorrect because the oxidation state of fluorine changes from 0 in F2 to -1 in F- ions. Therefore, the oxidation state of fluorine does change in this reaction.

In summary, the correct statement is that water is oxidized to produce oxygen gas (O2) in the reaction of fluorine with water.