**Atoms, Elements, and Compounds: Predicting the Formula of Ionic Compounds** ### Exercise **Write the empirical formula for at least four ionic compounds that could be formed from the following ions:** - \( \text{Pb}^{4+} \) - \( \text{Fe}^{2+} \) - \( \text{MnO}_4^{-} \) - \( \text{SO}_4^{2-} \) **Answer:** 1. **Compound 1:** Lead(IV) Permanganate - Formula: \( \text{Pb(MnO}_4\text{)}_4 \) 2. **Compound 2:** Iron(II) Sulfate - Formula: \( \text{FeSO}_4 \) 3. **Compound 3:** Lead(IV) Sulfate - Formula: \( \text{Pb(SO}_4\text{)}_2 \) 4. **Compound 4:** Iron(II) Permanganate - Formula: \( \text{Fe(MnO}_4\text{)}_2 \) ### Instructions: To determine the empirical formulas, balance the charges of the cations and anions to ensure the overall charge of the compound is zero. For example: - For Lead(IV) Permanganate: \( \text{Pb}^{4+} \) and \( \text{MnO}_4^{-} \). Since lead has a charge of +4 and permanganate has a charge of -1, four permanganate ions are needed to balance one lead ion, resulting in \( \text{Pb(MnO}_4\text{)}_4 \). ### Additional Tools - You can use the provided diagram tool to practice writing the formulas below by clicking on the provided icons. #### Diagram Tool Explanation: - The tool includes options to clear your work (X), redo the last action (↻), and request help or additional information (?). This exercise helps reinforce the principles of charge balance in ionic compounds and develop a better understanding of empirical formula writing.

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