What must occur for ionic compounds to be solvated in water?

For ionic compounds to be solvated in water, the breaking of ionic bonds is essential. In ionic compounds, the ions are held together by strong electrostatic forces of attraction between positively charged cations and negatively charged anions. When ionic compounds are introduced to water, the polar nature of water molecules plays a crucial role. Water molecules surround the individual ions, leading to the disruption of these ionic bonds.

This process involves the attraction between the dipole of water molecules and the charged ions. The partially negative oxygen atoms of water are attracted to the positively charged cations, while the partially positive hydrogen atoms are attracted to the negatively charged anions. As these interactions occur, the ionic bonds are effectively broken, allowing the ions to separate and disperse throughout the solution, achieving solvation.

The other options do not accurately reflect the necessary processes for solvation in this context. Breaking of covalent bonds is not relevant here, as ionic compounds do not involve covalent bonds in their solid state. The formation of new ionic bonds does not apply since the soluble ions are becoming dispersed rather than forming new compounds. The increasing concentration is a consequence of the solvation process, but it does not describe what must occur for the ionic compounds to dissolve in water.