The number of ions formed on dissolving one molecule of \(\mathrm{FeSO}_{4}\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) are: (a) 3 (b) 4 (c) 5 (d) 6

Ion formation is a fundamental chemical process that occurs when atoms or molecules gain or lose electrons, resulting in charged particles known as ions. In the context of ionic compounds, such as FeSO₄(NH₄)₂SO₄ · 6H₂O, this process occurs when the compound dissolves in water.

During dissolution, the ionic components in the compound separate from one another and individual ions are formed. For instance, FeSO₄ dissociates into Fe²⁺ and SO₄^2- ions. Similarly, each NH₄ group forms NH₄⁺ ions. Considering that there are two NH₄ groups, this results in two NH₄⁺ ions. This ionization is crucial for the substance’s behavior in solution and affects properties such as conductivity and reactivity.

Ions can be either positively charged, termed cations (like Fe²⁺ and NH₄⁺), or negatively charged, referred to as anions (like SO₄^2-). The balance of total positive and negative charges in solution must be equal, thus maintaining electrical neutrality.

Molecular dissociation in solution refers to the separation of molecules into simpler components, typically ions, when a substance dissolves in a solvent. With ionic compounds, the process of molecular dissociation is critical for understanding how compounds interact in solution.

For example, the compound FeSO₄(NH₄)₂SO₄ · 6H₂O dissociates in water to form individual ions. Water's polar nature causes the ionic bonds holding the compound together to weaken, allowing each ion to separate and become surrounded by water molecules, a process known as hydration. The ions are then free to move independently within the solution, which can conduct electricity due to the presence of these free-moving charged particles.

The extent of dissociation can vary based on factors such as temperature, concentration, and the nature of both the ionic compound and the solvent. Understanding molecular dissociation is vital for studying chemical reactions in solution, as it dictates the availability of ions for reaction.

Stoichiometry of ionic compounds involves the quantitative relationships that govern the formation of ions when these compounds dissolve in solvents. It's a key component in solving chemical problems as it allows one to predict the amounts of reactants and products involved in chemical reactions.

When analyzing the dissociation of FeSO₄(NH₄)₂SO₄ · 6H₂O, stoichiometry helps us to understand that one molecule of this compound will produce five ions in total. Breaking this process down, we see the dissociation of one FeSO₄ into one Fe²⁺ ion and one SO₄^2- ion; two (NH₄)⁺ ions from the ammonium groups; and another SO₄^2- ion from the additional sulfate group.

Stoichiometry can be used to calculate reactant amounts for a desired product yield, to balance chemical equations, and to predict the outcomes of chemical reactions. Understanding stoichiometry is essential in fields ranging from pharmaceuticals to environmental science.