1. Iron (II) Chloride: The iron (II) ion has a charge of +2 and the chloride ion has a charge of -1. To balance the charges, we need two chloride ions for each iron (II) ion. So, the empirical formula is FeCl2.

2. Iron (II) Sulfide: The iron (II) ion has a charge of +2 and the sulfide ion has a charge of -2. The charges are already balanced, so we need one of each ion. The empirical formula is FeS.

3. Lead (IV) Chloride: The lead (IV) ion has a charge of +4 and the chloride ion has a charge of -1. To balance the charges, we need four chloride ions for each lead (IV) ion. So, the empirical formula is PbCl4.

4. Lead (IV) Sulfide: The lead (IV) ion has a charge of +4 and the sulfide ion has a charge of -2. To balance the charges, we need two sulfide ions for each lead (IV) ion. So, the empirical formula is PbS2.

Question

1. Iron (II) Chloride: The iron (II) ion has a charge of +2 and the chloride ion has a charge of -1. To balance the charges, we need two chloride ions for each iron (II) ion. So, the empirical formula is FeCl2.

2. Iron (II) Sulfide: The iron (II) ion has a charge of +2 and the sulfide ion has a charge of -2. The charges are already balanced, so we need one of each ion. The empirical formula is FeS.

3. Lead (IV) Chloride: The lead (IV) ion has a charge of +4 and the chloride ion has a charge of -1. To balance the charges, we need four chloride ions for each lead (IV) ion. So, the empirical formula is PbCl4.

4. Lead (IV) Sulfide: The lead (IV) ion has a charge of +4 and the sulfide ion has a charge of -2. To balance the charges, we need two sulfide ions for each lead (IV) ion. So, the empirical formula is PbS2.

Knowee AI · Accepted Answer

1. Iron (II) Chloride: The iron (II) ion has a charge of +2 and the chloride ion has a charge of -1. To balance the charges, we need two chloride ions for each iron (II) ion. So, the empirical formula is FeCl2.

2. Iron (II) Sulfide: The iron (II) ion has a charge of +2 and the sulfide ion has a charge of -2. The charges are already balanced, so we need one of each ion. The empirical formula is FeS.

3. Lead (IV) Chloride: The lead (IV) ion has a charge of +4 and the chloride ion has a charge of -1. To balance the charges, we need four chloride ions for each lead (IV) ion. So, the empirical formula is PbCl4.

4. Lead (IV) Sulfide: The lead (IV) ion has a charge of +4 and the sulfide ion has a charge of -2. To balance the charges, we need two sulfide ions for each lead (IV) ion. So, the empirical formula is PbS2.

Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions:Fe2+, Pb4+, Cl−, S2−

Question

Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions:

Solution

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