2. Kinetic Theory  3 Basic “assumptions” All matter is composed of small particles [molecules, atoms and ions] The particles are in constant, random motion. The particles are colliding with each other and the wall of their container.

3. Why is kinetic theory important?  Solubility: The Ability to Dissolve  Dissolving The process of combining a solid and a liquid into a solution.

4. Is a PHYSICAL change… No new products are formed. The ID of the substances never changes.

5. Two parts to a solution  Solvent: The medium that does the dissolving.  Solute: The substance being dissolved. For example: Salt Water ○ Which is which?

7. Dissolving example  Ex salt and Water The salt is composed of billions of NaCl particles. The water is composed of individual water molecules.  The salt particles are pulled apart by the water molecules and become distributed throughout the water.  The water removes layers of salt until the solid appears gone.

9. Factors that can affect solubility  Surface Area (particle size)  Agitation  Temperature

10. Sugar Cube lab!  Lets start dissolving!

11. Effects of particle size  The smaller the size of the solute, the faster they dissolve.  The smaller the size, the more surface area comes in contact with the solvent causing the dissolving to occur faster.

12. Stirring or Agitation Effects  The more a solution is stirred or agitated, the faster the rate of dissolving for a solid in a liquid  Stirring or agitation causes the molecules to collide and breakdown into solution faster.

13. Effects of Temperature  The higher the temperature, the faster the solute will dissolve  At higher temperatures more of the solvent molecules moving faster and colliding with the solute particles.  The collisions breakdown the solute, causing it to dissolve faster.