Understanding Oxidation States
* Oxidation state is the hypothetical charge an atom would have if all its bonds were 100% ionic.
* Fluorine (F) always has an oxidation state of -1 in its compounds.
* Oxygen (O) usually has an oxidation state of -2, except in peroxides (where it's -1).
Applying the Rules
1. Assign oxidation states to F and O:
* There are four fluorine atoms (4 x -1 = -4)
* There is one oxygen atom (-2)
2. Let the oxidation state of Xe be 'x'.
3. Set up an equation:
* x + (-4) + (-2) = 0 (The sum of oxidation states in a neutral molecule is zero)
4. Solve for 'x':
* x - 6 = 0
* x = +6
Therefore, the oxidation state of Xe in XeOF₄ is +6.
