1. Advanced Physical Science 1 st Semester Exam Review December ~ 2009

2. Know #2: SI units of measurement  Mass – grams (g)  Volume – milliliters (mL)  Density – grams per cubic cm (g/cm³)  Distance – meters (m)  Speed – meters per second (m/s)  Velocity - meters per second South (m/s South)  Acceleration – m/s² South  Force – Newtons (N)

3. #3: Three types of scientific models  Physical  Mathematical  Conceptual

4. #4 Examples of physical properties of matter  Solubility  State of matter (solid, liquid, gas)  Density  Ductility  Malleability  Thermal conductivity  Shape, texture, etc.  Odor  Color  Back Back

5. #5 Viscosity and an example  Physical property of a liquid which is its level of resistance to flow  High viscosity – stronger attraction of molecules, flow is slower  Honey has a high viscosity compared to water

6. #6: The states of matter…  Solid – Definite shape, definite volume  Liquid – Definite volume, no definite shape  Gas – No definite shape or volume  Plasma – (gas) No definite shape of volume

7. #6 Continued – Changes of State  Liquid to gas – evaporation  Gas to liquid – condensation  Solid to liquid – melting (endothermic)  Liquid to solid – freezing (exothermic)  Sublimation – solid to gas

8. #7: What sublimation is  Solid becoming a gas without going through the liquid state.  Example – Dry Ice

9. # 8: Properties of metals…  Hard  Shinny  Malleable – can be pounded, pressed  Ductile – can be pulled into wire  Good conductors of heat

10. #9: Properties of non- metals…  Dull  Not malleable/ductile  Poor conductors

11. #10: The parts of an atom and their charges  Protons – positive, in nucleus  Neutrons – no charge, in nucleus  Electrons – negative charge, move in all directions at various levels around the nucleus

12. #11: How the periodic table is arranged…  By increasing atomic number from left to right  Family / groups in columns  Periods in horizontal rows

13. #13: Reference point…  Place or object used for comparison to determine if something is in motion

14. #14: Balanced, unbalanced forces and net force  Balanced – forces acting on an object are equal; no movement/ motion  Unbalanced – forces acting on an object are not equal; results in motion  Net force – Combination of all forces acting on an object  Force can be a push or a pull

15. #15: Examples of Acceleration and what would not be an example  Speeding up – or slowing down  Changing direction  Spinning around  Orbiting NOT Examples:  Going in one direction at a steady rate  Not moving at all

16. #16 - 17: Know examples of exothermic and endothermic reactions  Exothermic – Heat leaving. Liquid to solid – freezing; Or vapor cooling to liquid - Condensation  Endothermic – Heat coming in. Solid to liquid – melting; Or liquid to gas - evaporation

17. Understand 1: The Scientific Method  Ask question or state problem  Gather info  Form a hypothesis  Test the hypothesis  Observe  Analyze  Draw a conclusion

18. Scientific Method, continued  Independent variable – The one you’re testing; the one that’s changing  Dependent variable – the one that changes as a result of the experiment; what you’re measuring.

19. #2: The difference between scientific law and theory  Scientific Theory - Explains / an explanation based on hypothesis and observations  Scientific Law – Summarizes/ a summary of many results; Will predict or tell what will happen every time.

20. #4: Examples of chemical properties and what they mean  Flammability – ability to burn  Reactivity– Ability to chemically combine

21. #5: The difference between a physical and chemical property  Physical property – can be observed or measured without changing identity See slide #4 under “Know”slide #4 under “Know”  Chemical property – ability to change into a new substance

22. # 6: Difference between mass and weight  Mass is the amount of matter in an object  Weight is the measure of gravitational force on an object

23. #7: The particles in solids, liquids and gases  In solids they vibrate in place ( strong attractions of particles)  Liquids – Are close but slide past one another  Gases – Move apart independently and randomly

24. #8: The difference between compounds and mixtures  Compounds – a chemical combination of elements  Mixtures – combination of 2+ substances not chemically combined  Compound examples – H 2 O, CO 2  Mixture examples – dirt, pizza, salad, blood, oil & vinegar

25. #9: Difference between elements and compounds  Elements are pure substances that can’t be broken down by physical or chemical means (particle – atom)  Compounds are pure substances made of 2+ elements combined chemically (particle – molecule)

26. Difference between solvent and solute  The solvent is the substance in which the solute is dissolved.  Salt water- Water is the solvent, salt is the solute

27. # 11: Difference between metals, non-metals and metalloids  Metals are shiny, malleable, ductile and good conductors of heat  Non-metals are dull and poor conductors  Metalloids are semi-conductors; properties of both

28. #12: Difference between mass number and atomic number  Atomic number is the # of protons in an atom  Mass number is the sum of protons and neutrons  Atomic mass is how much mass is contained in all the particles of an atom. On the Periodic Table it is the average mass of the isotopes.

29. # 13: Motion vs. Speed  Motion is an object’s change of position relative to a reference point  Speed is the distance traveled over the time it takes to get there; D/T

30. #14: Speed vs. Velocity  Speed is D/T (m/s)  Velocity is D/T in a certain direction - North, South, East, West (m/s East)  When you know speed and direction, you can determine velocity  Acceleration is the change in velocity over time (m/s ² South) V 2 – V 1 T 2 - T 1

31. #15: Static vs. Kinetic friction  Static friction – friction that does not allow movement  Kinetic friction – friction that allows movement  Static – Trying to move a ton of concrete blocks  Kinetic – Sliding a book

32. #1 Be able to…  A pure substance is the smallest sample of matter where there is only one type of particle (an atom or molecule).  Elements and compounds are both considered the smallest samples of matter and are pure substances  A single element or a single compound (elements combined chemically) have definite physical and chemical properties.

33. #2: Be able to….  Compounds are elements combined chemically; They are pure substances; Require chemical reactions to separate. Example – H 2 O  Mixtures are substances mixed together, but that aren’t combined chemically. NOT pure substances; Physically separated. - Example – Salad, Salt water solution.

34. #3: Be able to….  Acceleration is the change in velocity over the time to make the change.

35. #4: Be able to….  Compounds are the chemically combined atoms of elements whose smallest particle is a molecule

36. #5: Be able to…  By spinning around, orbiting or changing direction

37. #6 & 7: Be able to…  Exothermic – heat out. For example, freezing  Endothermic – heat in. For example, melting

38. #8: Be able to calculate…  Density – M/V – 1 st you have to calculate volume – L x W x H (or by water displacement cm³), then divide mass by your answer  Speed – D/T  Acceleration – V 2 – V 1 T 2 - T 1  Net Force 5 N East and 8 N West Net Force = 3 N West