What is the correct formula for iron (II) sulfide? FeS FeS FeS Fe2S3
The Correct Answer and Explanation is:
The correct formula for iron (II) sulfide is FeS.
Explanation:
- Iron (II) sulfide refers to a compound formed between iron in the +2 oxidation state (Fe²⁺) and sulfur in the -2 oxidation state (S²⁻).
- The charge of iron in iron (II) sulfide is +2, which is denoted by the Roman numeral II in the name. This means each iron ion carries a +2 charge.
- The charge on the sulfur ion (S²⁻) is -2. To balance the charges, one Fe²⁺ ion combines with one S²⁻ ion, forming a neutral compound.
- The formula is derived by ensuring that the total positive charge equals the total negative charge. Since both the iron and sulfur ions have charges of 2 (but opposite in sign), the simplest ratio is 1:1. Hence, the formula for iron (II) sulfide is FeS.
- The other options, Fe2S3, refer to iron (III) sulfide, where iron is in the +3 oxidation state (Fe³⁺), which is different from iron (II). In Fe2S3, two Fe³⁺ ions combine with three S²⁻ ions to form a neutral compound, which is a different compound entirely.
Thus, the correct formula for iron (II) sulfide is FeS, where the iron ion is in its +2 oxidation state.
