Why ionic compounds are not soluble in solvents like kerosene, petrol , benzene.?

Question

Answer

Because organic compounds are not able to ionising the molecules of ionic compounds

Answer

Water is a polar covalent compound. It decreases the electrostatic forces of attraction, resulting in free ions in aqueous solution. Hence, ionic compounds dissolve in water. Kerosene is a non-polar organic solvent and dissolves non-polar covalent compounds.

Answer

Because it doesn't contain free ions

Answer

Introduction:
Ionic compounds are composed of positive and negative ions held together by strong electrostatic forces of attraction. These compounds are typically soluble in polar solvents but are insoluble in nonpolar solvents such as kerosene, petrol, and benzene. This can be explained by considering the nature of these solvents and the forces involved in the dissolution process.

1. Polarity of solvents:
Kerosene, petrol, and benzene are nonpolar solvents. They consist of molecules with relatively equal sharing of electrons, resulting in a lack of partial charges. On the other hand, ionic compounds are composed of charged ions, either positive or negative, which are attracted to each other through electrostatic forces. The polar nature of the solvents prevents them from effectively interacting with the charged ions.

2. Ion-dipole interactions:
Ionic compounds dissolve in polar solvents due to ion-dipole interactions. In a polar solvent, the positive end of the solvent molecule is attracted to the negatively charged ion, and the negative end is attracted to the positively charged ion. These interactions weaken the forces holding the ions together and allow them to separate and disperse throughout the solvent.

3. Nonpolar solvents and ion-ion interactions:
Nonpolar solvents lack the necessary partial charges to effectively interact with the ions in the ionic compound. The strong electrostatic forces of attraction between the ions are not overcome by the weak interactions with the nonpolar solvent molecules.

4. Role of intermolecular forces:
In nonpolar solvents, the dominant intermolecular forces are London dispersion forces. These forces arise from temporary fluctuations in electron distribution within molecules, resulting in temporary dipoles. However, these forces are generally weaker than the ionic forces in the solid lattice of an ionic compound. Therefore, the attractive forces between the ions in the ionic compound outweigh the forces between the solvent molecules and prevent the dissolution of the compound.

Conclusion:
Ionic compounds are not soluble in solvents like kerosene, petrol, and benzene due to the lack of polarity in these solvents. The absence of partial charges in nonpolar solvents limits their ability to interact with the charged ions in the ionic compound. The dominant intermolecular forces in nonpolar solvents are not strong enough to overcome the strong electrostatic forces holding the ions together. Therefore, these solvents are unable to dissolve ionic compounds.

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