1. Matter and Energy Objectives:  Distinguish between a mixture and a pure substance  Describe four common states of matter and how particles behave in each state

2. Building Blocks of Matter Atom – smallest unit of an element that maintains the properties of that element. Neutral charge Element – a pure substance made of only one kind of atom Compound – a substance that is made of the atoms from two or more elements that are chemically combined

3. Classification of Matter Pure substance – composed of one kind of atom or molecule has a fixed composition has the same physical and chemical properties throughout Mixture – a blend of two or more kinds of matter Can be physically separated. Methods include: centrifugation, distillation, filtration, and magnets.

4.  Heterogeneous – NOT uniform throughout and will show Tyndall Effect (scattering of light due to particles in a solution) o Suspension - Particles are suspended in a fluid that will settle out  Homogeneous – uniform in composition throughout o Solution - one or more substances (the solutes) dissolved in another substance (the solvent) o Colloid - Particles suspended in a liquid that do not settle out. Can also exhibit Tyndall Effect Mixtures

6. States of Matter

7. Solid Have a definite shape and volume Particles have strong attractive force, but still vibrate Two types Crystalline – orderly arrangement of atoms Amorphous – no particular order or arrangement of atoms

8. Liquid Have a definite volume but not a definite shape Particles move fast enough to overcome forces of attraction Surface tension – force between particles at the surface that cause spherical shapes

9. Gas Does NOT have definite volume or shape Particles moves fast enough to break away from each other

10. Plasma Does NOT have a definite shape or volume Particle are broken apart (electrons have been stripped off) Conduct electric current Examples?

11. Energy & Change of State Deposition

12. Changes of State Melting point – Temperature at which a solid changes to a liquid Freezing point – Temperature at which a liquid changes to a solid Boiling point – Temperature at which a liquid changes to a gas Condensation point – Temperature at which a gas changes to a liquid Same Temp. Same Temp.

13. Phase Transitions Melting: change of a solid to a liquid. Freezing: change a liquid to a solid. Vaporization: change of a liquid to a gas. Condensation: change of a gas to a liquid. Sublimation : Change of solid to gas Deposition: Change of a gas to a solid. H 2 O(s)  H 2 O(l) H 2 O(l)  H 2 O(s) H 2 O(l)  H 2 O(g) H 2 O(g)  H 2 O(l) H 2 O(s)  H 2 O(g) H 2 O(g)  H 2 O(s)

15. Phase changes by Name

20. Energy & Change of State Reactions/Changes can be: Endothermic – requires energy or Exothermic – produces energy

21. Water phase changes Temperature remains constant during a phase change. Energy

22. Which of the following is a physical change? 1. burning gasoline 2. cooking an egg 3. decomposing meat 4. evaporating water 5. rusting iron 1234567891011121314151617181920 21222324252627282930

23. Which of these is an element? 1. Water 2. Nitric acid 3. Wood 4. Silver 5. Brass 1234567891011121314151617181920 21222324252627282930

24. Which of the following is an incorrect description? 1. A homogeneous mixture. 2. A heterogeneous compound. 3. A solid element. 4. A mixture of solids. 5. A solution of gases.

25. This is the process shown by the arrow. 1. Melting 2. Freezing 3. Evaporation 4. Condensation 5. Sublimation 6. Deposition 1234567891011121314151617181920 21222324252627282930

26. This is the process shown by the arrow. 1. Melting 2. Freezing 3. Evaporation 4. Condensation 5. Sublimation 6. Deposition 1234567891011121314151617181920 21222324252627282930

27. This is the classification of glass. 1. Homogeneous mixture 2. Heterogeneous mixture 3. Element 4. Pure substance 5. Colloid 1234567891011121314151617181920 21222324252627282930