1. Exam Review Know the parts of the periodic table. (Group names)
Know the prefixes.

2. Midterm Review

3. 1. Scientific Method State the problem Gather information
Form a hypothesis
Test the hypothesis
Analyze the data
Draw conclusions
Hypothesis supported or not supported

4. 2 & 3. Hypothesis
Possible explanation for a problem using what you know and what you have observed
Through observations

5. 4. Written Hypothesis
If (independent variable), then (dependent variable).
Ex. If I study for this test, then I will make a good grade.

6. 5. Laboratory apparatuses
Balances
Test tubes
Graduated cylinders
Flasks
Bunsen burner
Pipettes, etc.
thermometers
See laboratory apparatus lab.

7. 6. Laboratory procedures
See lab manual

8. 7. Precision and Accuracy
Precision: How close your measurements are to each other
Accuracy: How close a measurement is to being correct

9. 8. Laboratory tools
See lab manual

10. 9. Tools for specified data
Volume: graduated cylinder
Length: ruler
Mass: balance

11. 10. Parts of an experiment
Independent Variable: This is what will change within your experiment and will affect the dependent variable

12. 11. How do you create an experiment?
Make observations
Collect data
Research
Form a hypothesis
Choose your variables
Constants & controls

13. 12. Graphs
Line Graph
Circle Graph
Bar Graph

14. 13. Formulas needed for specific investigations
Dependent on investigation
Volume (l X w X h)
Density (d=m/v)

15. 14. Technology
Computers
Laboratory equipment

16. 15. cost, time and materials in cost of products
Ex. More time it takes to make something, cost increases.

17. 16. Science & Technology Technology: applied science to help people
Technology doesn’t always follow science
Both have steps

18. 17. Safety procedures
See lab safety manual

19. 18. Classification of Matter
Physical Properties
Chemical Properties

20. 19. Types of Mixtures Homogeneous (solutions) Heterogeneous Colloids
Suspension

21. 20. Chemical Properties
Characteristic of a substance that indicates whether it can undergo a chemical change.
Flammability, light sensitivity

22. 21. Physical Properties
Anything you can observe without changing the identify of something
Appearance: shape, color, size, density, melting point, boiling point
Behavior : ex. magnetism

23. 22. Density
Mass per unit volume of a material
D = m/v

24. 23. States of Matter
Solids
Liquids
Gases
Plasma

25. 24. State changes
Solid  Liquid  Gases  Plasma Particles are arranged closely in solids  as heat is added they start moving faster and spread apart  gases The faster particles move, the more energy involved K inetic Theory

26. 25. Archimede’s, Bernoulli’s and Pascal’s Principles
Archimide’s: Buoyancy (buoyant force and weight)
Bernoulli’s: as velocity of a fluid increases, the pressure decreases
Ex. Airplane technology, roofs lifted during tornadoes
Pascal’s: Pressure applied to a fluid is transmitted throughout the fluid
Ex. Toothpaste tube

27. 26. Charles’ and Boyle’s Laws
Charles: The volume of a gas increases with increasing temperature.
Pressure stays constant here
Gas expands as it is heated
Ex. Hot air balloon
Boyles: if you decrease volume of a container of gas, the pressure of the gas will increase
Temperature stays constant here

28. 27. Kinetic Theory All matter is composed of small particles
These particles are in constant, random motion
If you increase the temperature, particles move faster.
If you decrease the temperature, particles move slower.

29. 28. Subatomic Particles Nucleus Protons: Positive Neutrons: Neutral
Electron Cloud
Electrons : negative

30. 29 & 30. How do subatomic particles affect properties of an atom?
Nucleus: gives atom its mass
Mass number = protons + neutrons
Protons: (atomic number)
Identity
Electrons: give the atom its chemical properties
Ionic and Covalent Bonding

31. Ex. Carbon-12 & Carbon-14 are both isotopes of Carbon
31. Compare/contrast atoms of elements which exist as stable or unstable isotopes.
Isotopes: atoms of the same element with different numbers of neutrons.
Ex. Carbon-12 & Carbon-14 are both isotopes of Carbon
Carbon – 12 is stable