Final answer:
To create empirical formulas for binary ionic compounds with the given ions, balance the total positive and negative charges. Example compounds include FeCl2 (iron(II) chloride), FeS (iron(II) sulfide), NiCl4 (nickel(IV) chloride), and NiS2 (nickel(IV) sulfide).
Step-by-step explanation:
To write the empirical formulas for binary ionic compounds using the ions Fe2+, Ni4+, Cl−, and S2−, we must ensure that the total positive charge balances the total negative charge, resulting in an electrically neutral compound.
- For the pair Fe2+ and Cl−, we'll need two Cl− ions to balance the charge of one Fe2+ ion, giving us the formula FeCl2.
- Next, for Fe2+ and S2−, since both ions have charges of ±2, just one of each ion is needed, leading to the formula FeS.
- With Ni4+ and Cl−, four Cl− ions are required to balance the four positive charges of Ni4+, resulting in the formula NiCl4.
- Lastly, for Ni4+ and S2−, two S2− ions are necessary to balance the Ni4+ charge, giving us the formula NiS2.
These are the empirical formulas for four binary ionic compounds consisting of the provided ions. This process of creating formulas is foundational in the study of chemical compounds.