3. What is Matter?  Anything that takes up space (volume) and has mass.  Anything on EARTH.

4. Types of Matter  Homogeneous Matter that is made up of the same or alike particles.  SAME THROUGHOUT  Can’t see the particle  Heterogeneous Matter that is made up of different types of particles.  DIFFERENT THROUGHOUT  Can see the particles

5. Homogeneous Materials Kool aid Tea Clear sodas Rubbing alcohol Water Elements Compounds Acids

6. Heterogeneous Materials Cereal Salad Snack mix Kabobs Italian dressings Uncooked pizza M & M’s Skittles Vegetable soup Milk

7. Now it is your turn… you tell me: Homogeneous or Heterogeneous  Flat soda pop  Cherry vanilla ice cream  Sugar (C 2 H 3 O 2 )  Salt (NaCl)  City Air  Iron (Fe)  Beach Sand  Spaghetti Sauce

8. Mixtures vs. Pure Substances  MIXTURES Heterogeneous or Homogeneous Easily separated EXAMPLES Any Heterogeneous or homogeneous examples  PURE SUBSTANCES Homogeneous Hard to separate In it simplest form EXAMPLES Elements and compounds

9. Types of Pure Substances  Elements: Purest substance known that can’t be broken down Neon: Ne  Compounds: 2 or more elements chemically combined Water: H 2 O

10. Atoms are the counting units or quantity of the element.

11. Properties of Mixtures  Easily separated  Physically combined to easily separate.  Amounts vary when mixed  Changes only in physical appearance when dissolved.

12. Types of Mixtures  Heterogeneous Mixtures Suspensions Colloids  Homogeneous Mixtures Solutions

13. Solution  Homogeneous Mixture: Same throughout  Examples: Ice tea Sugar water Kool aid Sprite

14. Solutions and Its Properties  Particles are individual atoms, molecules, or ions (charged particles)  Clear  Can’t be filtered  Particles are evenly spread out  Can’t see the particles  Homogeneous

15. Parts of a Solution  Solute – Part being dissolved in the solvent. ex: Sugar, Hot Chocolate, Salt  Solvent – Part that does the dissolving. ex: Water – universal solvent

16. Aqueous vs. Tincture Solution  Aqueous – water is the solvent  Tincture – alcohol is the solvent

17. Combinations of Solutions SOLUTES 1. Solid 2. Solid 3. Solid SOLVENT Solid Liquid Gas EXAMPLES Alloy (pots) Sea water Soot in air 4. Liquid 5. Liquid 6. Liquid Solid Liquid gas Dental fillings Antifreeze Humid air 7. Gas 8. Gas 9. Gas Solid Liquid Gas Gas mask Sodas Air

18. Special Activities of Solutions Dissociation – splitting ions to form charges Ionization – gaining or losing electrons to form ions Electrolyte – Solution that produce electricity (Salt and Water) Non-electrolyte – solution that does not produce electricity (Sugar and Water)

19. Special Solutions  Miscible – when a liquid is dissolved into a liquid Example: Antifreeze, alcohol and water  Alloy – when a solid is dissolved into a solid Examples: Stainless steel pots and pans, bronze, brass, jewelry

20. Rates of Solutions (how to speed up a solution)  Stirring  Heating  Powdering- increasing the surface area

21. Solubility and Its Factors  Solubility – ability of a solute to dissolve into a solvent.  Factors that affect solubility of a gas in a solution Temperature – decreasing temperature Pressure – increasing pressure

22. Dilute vs. Concentrated  Dilute – weak solution “watered down”  Concentrated Strong solution

23. Levels of Solutions  Saturated – Holding as much solute at a given temperature  Supersaturated – UNSTABLE – more solute in the solvent at a high temp.

24. Colloid Properties  Heterogeneous Mixture  Can’t see particles  Particle size is larger than those in solutions  Scatters light – Tyndall Effect

25. Examples of Colloids  Fog- clouds  Smoke- smoke  Foam- whipped cream  Emulsion- mayonnaise  Sol- paints  Gel- butter

26. Suspension Properties  Heterogeneous Mixture  Can see the particles  Easily separated  EXAMPLES waste oil and water trail mix eggs cereals

27. Ways to Separate Mixtures  Filtering – Suspensions  Evaporation – Solution, Colloids, Suspensions  Distillation – Solutions, Colloids, Suspensions  Chromatography - Solutions

28. Physical Properties and Changes  Physical Properties  Characteristic you can observe without changing the substance  Examples: ○ Appearance: color, shape, … ○ Measurements: mass, length, volume… ○ Behavior: attracted by magnet, soluble… ○ Changes of State: melting point, boiling point…  Physical Changes  Change made to material that does not change the substances  Usually, the change can be reversed Examples: ○ Tearing, shredding crushing… ○ Boiling, melting, freezing… ○ Dissolving

29. Chemical Properties  Characteristic of a substance that undergoes a certain chemical change Examples: ○ Flammability or combustibility ○ Reactivity

30. Chemical Change  Change of one substance in a material to a different substance  Usually the change can’t be reversed  Signs of a chemical change: Smell Color Foaming or gas production Precipitate – solid forming when two items are mixed together Light or explosion (release of energy)  Examples: rusting, burning, …

31. Law of Conservation of Mass  Matter is neither created nor destroyed during a chemical change or physical change original mass = final mass