Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
**Predicting the Formula of Ionic Compounds with Common Ions** **Task:** Write the empirical formula for at least four ionic compounds that could be formed from the following ions: - \( \text{PO}_4^{3-} \) - \( \text{Pb}^{4+} \) - \( \text{OH}^- \) - \( \text{Fe}^{3+} \) **Instructions:** - Use the provided text box to input your empirical formulas. - You can use the options to clear or reset your entries if needed. **Explanation:** In this exercise, you will practice predicting the empirical formulas of ionic compounds. The ions listed can combine to form neutral compounds. Consider the charge balance: the sum of the charges in the compound must be zero. Here are a few example combinations: 1. **Pb(OH)_4:** Formed by combining \( \text{Pb}^{4+} \) and \( \text{OH}^- \). 2. **FePO_4:** Formed by combining \( \text{Fe}^{3+} \) and \( \text{PO}_4^{3-} \). 3. **Pb_3(PO_4)_4:** Formed by combining \( \text{Pb}^{4+} \) and \( \text{PO}_4^{3-} \). 4. **Fe(OH)_3:** Formed by combining \( \text{Fe}^{3+} \) and \( \text{OH}^- \). Use these combinations to guide your answers and ensure the total charge contributes to a neutral compound.
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Transcribed Image Text:**Predicting the Formula of Ionic Compounds with Common Ions** **Task:** Write the empirical formula for at least four ionic compounds that could be formed from the following ions: - \( \text{PO}_4^{3-} \) - \( \text{Pb}^{4+} \) - \( \text{OH}^- \) - \( \text{Fe}^{3+} \) **Instructions:** - Use the provided text box to input your empirical formulas. - You can use the options to clear or reset your entries if needed. **Explanation:** In this exercise, you will practice predicting the empirical formulas of ionic compounds. The ions listed can combine to form neutral compounds. Consider the charge balance: the sum of the charges in the compound must be zero. Here are a few example combinations: 1. **Pb(OH)_4:** Formed by combining \( \text{Pb}^{4+} \) and \( \text{OH}^- \). 2. **FePO_4:** Formed by combining \( \text{Fe}^{3+} \) and \( \text{PO}_4^{3-} \). 3. **Pb_3(PO_4)_4:** Formed by combining \( \text{Pb}^{4+} \) and \( \text{PO}_4^{3-} \). 4. **Fe(OH)_3:** Formed by combining \( \text{Fe}^{3+} \) and \( \text{OH}^- \). Use these combinations to guide your answers and ensure the total charge contributes to a neutral compound.
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