Step 1: Understanding the Concept:
The empirical formula gives the simplest whole-number ratio of atoms. The oxidation state of the central atom is then found using known states of the other atoms. Step 2: Key Formula or Approach:
Divide both numbers in the ratio by the smallest one to find whole numbers. Step 3: Detailed Explanation:
1. Given ratio Xe : F = 0.4 : 2.4.
2. Divide by 0.4: Xe = \(\frac{0.4}{0.4} = 1\), F = \(\frac{2.4}{0.4} = 6\).
3. The formula is XeF$_6$.
4. Fluorine always has an oxidation state of -1.
5. Let Xe be \(x\). In a neutral molecule: \(x + 6(-1) = 0 \implies x = +6\). Step 4: Final Answer:
The oxidation number of Xe is +6.