What is the oxidation state of F in HOF? Explain how it is possible.

Compound:

Hypofluorous acid (HOF)
We determine oxidation states by applying standard rules:

• Oxygen usually = -2 (except in peroxides or with fluorine).
• Hydrogen = +1.
• Fluorine is the most electronegative element; it usually = -1.

Oxidation State Calculation:
Let oxidation state of F = x
(+1 from H) + (-2 from O) + (x from F) = 0
1 – 2 + x = 0 → x = +1

So, fluorine in HOF has an oxidation state of +1.

Why is this unusual?

• Normally, fluorine is always -1 because of its highest electronegativity.
• But in HOF, oxygen is even less stable in a positive oxidation state, so fluorine is forced into +1 oxidation state.

Key Takeaways:

• Oxidation state of F in HOF = +1.
• Exception to the fluorine always -1 rule due to relative electronegativity and bonding.
• Important concept in inorganic chemistry exceptions.