Final answer:
Iron (II) sulfide is composed of iron and sulfur atoms in a chemical formula of FeS, indicating a 1:1 ratio. It is important to know the stoichiometry for determining the exact amount of reactants and the mass of iron sulfide produced.
Step-by-step explanation:
The composition of iron (II) sulfide involves a combination of iron (Fe) and sulfur (S) atoms in a 1:1 ratio, represented by the chemical formula FeS. During the synthesis of iron sulfide, every atom of iron will react with a single atom of sulfur to form this compound. Understanding the stoichiometry of the reaction allows scientists and industrial professionals to calculate the necessary quantities of reactants and the expected mass of iron sulfide produced.
The empirical formula for iron (II) sulfide is simply FeS, and this represents one unit of the compound. It is important to note that iron in this compound loses two electrons, which can come from the s-orbital or as a combination of s- and d-orbitals, leading to the Fe(II) or ferrous state. The process of forming iron sulfide can be observed through a reaction involving iron filings and powdered sulfur when heated together.