Notes Solubility1
- 1. Matter, Solutions, & Solubility
- 2. I. Phases of Matter The main differences in solids, liquids and gases is: how close their particles are, the speed of the particles & type of motion
- 3. B. kinetic molecular theory – particles of matter are in constant motion & the speed of the particles increases w/ increased temp
- 4. 1. In solids, the particles are very close together, touching each other and packed tightly enough that the particles cannot move at all except to rotate on their axes & vibrate.
- 5. a. SOLIDS - have definite shape and definite volume *usually HIGH density *expands only slightly when heated * almost incompressible because particles are packed very close together.
- 6. Crystalline - repeating geometric pattern covalent network metallic ionic covalent molecular Amorphous - no geometric pattern decreasing m.p.
- 7. Types of Solids Ionic (NaCl) Metallic
- 8. 2. In liquids , the particles touch each other constantly but can slide past each other as the liquid FLOWS. a. LIQUIDS – *have definite volume but not definite shape *usually SLIGHTLY less dense than solids
- 9. *expand more than solids when heated *almost incompressible; *takes the shape of its container *flows – viscosity refers to how quickly or slowly a fluid flows or changes shape
- 10. B. Liquid Properties Surface Tension attractive force between particles in a liquid that minimizes surface area
- 11. Liquid Properties Capillary Action attractive force between the surface of a liquid and the surface of a solid – paper towels! water mercury
- 12. 3. In gases , the particles are completely independent and do not touch each other continually. b. GASES - have no definite shape & no definite volume *very LOW density *expand greatly when heated
- 13. *highly compressible *take the shape of the container *flow *particles are completely independent and do not touch each other except when they bump into each other.
- 14. 4. phase changes a. melting/freezing – solid to liquid & liquid to solid b. boiling/condensating—liquid to gas gas to liquid c. sublimation/deposition—solid to gas & gas to solid
- 15. Liquids vs. Solids LIQUIDS Stronger than in gases Y high N slower than in gases SOLIDS Very strong N high N extremely slow IMF Strength Fluid Density Compressible Diffusion
- 16. Hydrogen Bonding Intermolecular forces of attraction between molecules Bonds exist within molecules Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 442
- 17. Water is an exception to the rule! Water becomes more dense as it gets colder UNTIL it reaches 4 C – it is MOST dense at 4 C. As it gets colder (3 C & lower) it expands & so gets less dense. That is why ice floats in water!