1. The Characteristics of Matter

2. States of Matter Solid: Liquid: Gas: Plasma:

3. States of Matter Solid: definite volume & shape, hard to compress, dense Liquid: Gas: Plasma:

4. States of Matter Solid: definite volume & shape, hard to compress, dense Liquid: definite volume, takes shape of container, hard to compress, somewhat dense Gas: Plasma:

5. States of Matter Solid: definite volume & shape, hard to compress, dense Liquid: definite volume, takes shape of container, hard to compress, somewhat dense Gas: indefinite volume, fills container, easy to compress, not dense Plasma:

6. States of Matter Solid: definite volume & shape, hard to compress, dense Liquid: definite volume, takes shape of container, hard to compress, somewhat dense Gas: indefinite volume, fills container, easy to compress, not dense Plasma: like gas but ionized (with + or – charge)

7. Phase Changes (Changes of State) Solid  liquid: Liquid  solid: Liquid  gas: Gas  liquid: Solid  gas: Gas  solid: Gas  plasma: Plasma  gas:

8. Phase Changes (Changes of State) Solid  liquid: melting Liquid  solid: freezing (solidification) Liquid  gas: boiling (evaporation) Gas  liquid: condensation Solid  gas: sublimation Gas  solid: deposition Gas  plasma: ionization Plasma  gas: recombination

9. Phase Changes (Changes of State)

10. Phase Changes in Water Boiling point of water = Melting point of water = Freezing point of water =

11. Phase Changes in Water Boiling point of water = 373.15K Melting point of water = 273.15K Freezing point of water = 273.15K

12. Phase Changes in Water Boiling point of water = 373.15K Melting point of water = 273.15K Freezing point of water = 273.15K Notice that these are the same? They are interchangeable

13. The Kinetic Molecular Theory Particles are always moving The more energy they have, the faster they move Heat is the measure of total kinetic energy Temperature is the average kinetic energy of all the molecules

14. The Kinetic Molecular Theory Solid particles: closely packed (dense), low energy and little space to move so they vibrate in place Liquids particles: more space and more energetic so they can flow (slide past each other) Gas particles: lots of space, most energetic and move freely within a container

16. Physical and Chemical Changes in Matter

17. Physical Properties vs. Chemical Properties Properties that can be found without a chemical reaction (without creating a new substance) E.g. density, colour, hardness, malleability, ductility, lustre, viscosity, melting point, boiling point Describe the ability of a substance to undergo chemical reactions and change into new substances E.g. H 2 can burn in air to produce H 2 O; H 2 combines with Cl 2 to form HCl

18. Physical Change Change in the shape or state of a substance No new substances formed (same chemicals) Reactants are the same as products Generally possible and easy to reverse E.g. changes in state (liquid water  ice), changes in shape or volume

19. Physical Change

20. Chemical Change A change where new substances are formed Reactants are different from the products Difficult or impossible to reverse Often include changes in physical properties E.g. cooking an egg, burning a match

21. Chemical Change

22. Homework Read Hebden p.44-52 HW check on p.44 #13 and p.52 #33, 35-41, 44