Question

write the empirical formula for at least four ionic compounds that could be formed from the following ions: pb⁴⁺, so₄²⁻, ch₃co₂⁻, nh₄⁺

Explanation:

To form ionic compounds, we combine cations and anions such that the total positive charge equals the total negative charge.

Step 1: Combine \( \text{Pb}^{4+} \) and \( \text{SO}_4^{2-} \)

The charge of \( \text{Pb}^{4+} \) is +4 and \( \text{SO}_4^{2-} \) is -2. To balance the charges, we need 2 \( \text{SO}_4^{2-} \) ions for each \( \text{Pb}^{4+} \) ion. So the formula is \( \text{Pb(SO}_4\text{)}_2 \).

Step 2: Combine \( \text{Pb}^{4+} \) and \( \text{CH}_3\text{CO}_2^- \)

The charge of \( \text{Pb}^{4+} \) is +4 and \( \text{CH}_3\text{CO}_2^- \) is -1. We need 4 \( \text{CH}_3\text{CO}_2^- \) ions for each \( \text{Pb}^{4+} \) ion. The formula is \( \text{Pb(CH}_3\text{CO}_2\text{)}_4 \).

Step 3: Combine \( \text{NH}_4^+ \) and \( \text{SO}_4^{2-} \)

The charge of \( \text{NH}_4^+ \) is +1 and \( \text{SO}_4^{2-} \) is -2. We need 2 \( \text{NH}_4^+ \) ions for each \( \text{SO}_4^{2-} \) ion. The formula is \( (\text{NH}_4\text{)}_2\text{SO}_4 \).

Step 4: Combine \( \text{NH}_4^+ \) and \( \text{CH}_3\text{CO}_2^- \)

The charge of \( \text{NH}_4^+ \) is +1 and \( \text{CH}_3\text{CO}_2^- \) is -1. They combine in a 1:1 ratio. The formula is \( \text{NH}_4\text{CH}_3\text{CO}_2 \).

Answer:

\( \text{Pb(SO}_4\text{)}_2 \), \( \text{Pb(CH}_3\text{CO}_2\text{)}_4 \), \( (\text{NH}_4\text{)}_2\text{SO}_4 \), \( \text{NH}_4\text{CH}_3\text{CO}_2 \) (Other valid combinations are also possible, e.g., \( \text{Pb(CH}_3\text{CO}_2\text{)}_4 \) can be checked for charge balance: \( +4 + 4\times(-1) = 0 \), which is correct. Similarly, other compounds follow charge balance rules.)