Due to the small and highly electronegative nature of fluorine

Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For a molecule of fluorous acid, the atoms are arranged as HOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.)

What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed.

Express your answers as charges separated by comma. For example, a positive one charge would be written as +1.

Formal Charge for H, O, F, O =

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Dr. OWL answered 3 years ago

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Due to the small and highly electronegative nature of fluorine

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