How does water interact with ionic compounds when it acts as a solvent?

Water plays a significant role in the dissolution of ionic compounds due to its polar nature. In this context, when water acts as a solvent, it effectively shields the individual ions of the ionic compound through a process known as hydration. The water molecules surround the positive and negative ions, with the partially positive hydrogen atoms being attracted to the anions (negatively charged ions) and the partially negative oxygen atoms drawn to the cations (positively charged ions).

This interaction between water molecules and the ions reduces the electrostatic forces that hold the ionic compound together, facilitating the separation of the ions and allowing them to disperse into the solution. This is why many ionic compounds are soluble in water, as the hydration process stabilizes the ions in solution.

The other options do not accurately describe the interaction. Water does not form ionic bonds with the compounds because the nature of ionic interactions is different from the polar interactions in solvation. While chemical reactions can occur with some ionic compounds in water, this is not the standard scenario for all ionic substances and is not the primary function of water as a solvent. Additionally, while some ionic compounds may precipitate under certain conditions, this is not a general characteristic of how water interacts with them in the dissolution process. Thus, hydration