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Write the empirical formula for at least four ionic compounds that could be formed from the following ions: co, Mno,, Fe*, NH

Write the empirical formula for at least four ionic compounds that could be formed from the following ions: co, Mno,, Fe*, NH

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Question:** Write the empirical formula for at least four ionic compounds that could be formed from the following ions: \[ \text{CO}_3^{2-}, \, \text{MnO}_4^{-}, \, \text{Fe}^{2+}, \, \text{NH}_4^{+} \] **Answer Box:** ``` ``` **Explanation:** You are given a set of ions with their charges: - Carbonate ion: \( \text{CO}_3^{2-} \) - Permanganate ion: \( \text{MnO}_4^{-} \) - Iron(II) ion: \( \text{Fe}^{2+} \) - Ammonium ion: \( \text{NH}_4^{+} \) Using these ions, you need to form ionic compounds by combining cations and anions in such a way that the total charge of the compound is zero. Below are four possible combinations: 1. **Iron(II) Carbonate:** - \( \text{Fe}^{2+} \) and \( \text{CO}_3^{2-} \) - Empirical Formula: \( \text{FeCO}_3 \) 2. **Iron(II) Permanganate:** - \( \text{Fe}^{2+} \) and \( 2\text{MnO}_4^{-} \) - Empirical Formula: \( \text{Fe(MnO}_4\text{)}_2 \) 3. **Ammonium Carbonate:** - \( 2\text{NH}_4^{+} \) and \( \text{CO}_3^{2-} \) - Empirical Formula: \( \text{(NH}_4\text{)}_2\text{CO}_3 \) 4. **Ammonium Permanganate:** - \( \text{NH}_4^{+} \) and \( \text{MnO}_4^{-} \) - Empirical Formula: \( \text{NH}_4\text{MnO}_4 \) Ensure to balance the charges properly to form neutral compounds when writing the empirical formula.
Transcribed Image Text:**Question:** Write the empirical formula for at least four ionic compounds that could be formed from the following ions: \[ \text{CO}_3^{2-}, \, \text{MnO}_4^{-}, \, \text{Fe}^{2+}, \, \text{NH}_4^{+} \] **Answer Box:** ``` ``` **Explanation:** You are given a set of ions with their charges: - Carbonate ion: \( \text{CO}_3^{2-} \) - Permanganate ion: \( \text{MnO}_4^{-} \) - Iron(II) ion: \( \text{Fe}^{2+} \) - Ammonium ion: \( \text{NH}_4^{+} \) Using these ions, you need to form ionic compounds by combining cations and anions in such a way that the total charge of the compound is zero. Below are four possible combinations: 1. **Iron(II) Carbonate:** - \( \text{Fe}^{2+} \) and \( \text{CO}_3^{2-} \) - Empirical Formula: \( \text{FeCO}_3 \) 2. **Iron(II) Permanganate:** - \( \text{Fe}^{2+} \) and \( 2\text{MnO}_4^{-} \) - Empirical Formula: \( \text{Fe(MnO}_4\text{)}_2 \) 3. **Ammonium Carbonate:** - \( 2\text{NH}_4^{+} \) and \( \text{CO}_3^{2-} \) - Empirical Formula: \( \text{(NH}_4\text{)}_2\text{CO}_3 \) 4. **Ammonium Permanganate:** - \( \text{NH}_4^{+} \) and \( \text{MnO}_4^{-} \) - Empirical Formula: \( \text{NH}_4\text{MnO}_4 \) Ensure to balance the charges properly to form neutral compounds when writing the empirical formula.
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