Question

What is the simplest formula for iron $(II)$ sulfide?

Answer 1

Hint : We know that to answer this question, we must firstly recall the concept of empirical formula. It is the simplest whole number ratio of the number of atoms present in the molecule. Sulfide is an Anion of nitrogen. It gains electrons in order to attain the configuration of a noble gas, which means it gains three electrons.

Complete Step By Step Answer:
The elemental constituents of a compound define its chemical identity, and chemical formulas are the most appropriate way of representing this elemental makeup. When a compound’s formula is not known to us, measuring the mass of each of its constituent elements is obviously the first step in the process of determining the formula experimentally.
Atoms, by default, have the same number of protons as electrons, resulting in a balance between positive and negative charged particles. Because it gains three electrons, there are more electrons than protons, so it has a charge of $-2.$
The molecule iron $(II)$ sulfide is an ionic molecule between the metal Iron and the non-metal sulfur. In an ionic molecule the formula is determined by balancing the charges on the ions.
For this case the Roman numeral (III) tells us the iron has a charge of $+3~or~F{{e}^{+3}}.$ The element sulfur has a charge of $-2~or~{{S}^{-2}}$
To balance these ion charges it takes two $+3~$ iron ions to balance three $-2$ sulfide ions. The molecule formula is $F{{e}_{2}}{{S}_{3}}.$
Therefore, the simplest formula for iron $(II)$ sulfide is $F{{e}_{2}}{{S}_{3}}.$

Note :
We should remember that with regard to deriving empirical formulas; we must consider examples in which a compound’s percent composition is available rather than the absolute masses of the compound’s constituent elements. This will make our calculations much easier.