Ionic Solutions

e.g., NaCl in H2O

1. Ions that are less tightly held because of their position at a corner or an edge of the crystal are exposed to water molecules

2. Water molecules will collide with the NaCl until an ion breaks free

3. More water molecules then cluster around the ion, stabilizing it by ion dipole attractions

4. The water molecules attack the weak part of the crystal until it is dissolved

5. Ions in solution are said to be solvated (hydrated) they are surrounded and stabilized by an ordered shell of solvent (water) molecules

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