Understanding Oxidation States
* Oxidation state is a number assigned to an atom in a molecule or ion that represents its hypothetical charge if all bonds were 100% ionic.
* Rules:
* The oxidation state of a free element is always 0.
* The sum of oxidation states in a neutral molecule is 0.
* The sum of oxidation states in a polyatomic ion equals the charge of the ion.
* Fluorine (F) has an oxidation state of -1 in its compounds (except in F₂).
* Hydrogen (H) has an oxidation state of +1 in its compounds (except in metal hydrides, where it is -1).
Applying the Rules to HOF
1. Fluorine's oxidation state: Fluorine always has an oxidation state of -1, so F is -1 in HOF.
2. Hydrogen's oxidation state: Hydrogen is bonded to a more electronegative element (oxygen), so its oxidation state is +1.
3. Oxygen's oxidation state (let's call it "x"): Since the overall charge of HOF is 0, we can set up the equation:
(+1) + (x) + (-1) = 0
4. Solving for x:
x = 0
Therefore, the oxidation state of oxygen in HOF is 0.
