1. MATTER AND CHANGE
CHAPTER 2

2. 2.1 PROPERTIES OF MATTER MATTER-anything that has mass and volume
Substance is matter that is uniform and has definite composition
PHYSICAL PROPERTY-quality or condition that can be observed or measured without changing the substance’s composition

3. STATES OF MATTER SOLIDS--fixed volume and shape
Atoms and molecules held tightly in a rigid structure, but vibrate slightly about fixed positions
LIQUIDS--fixed volume, but variable shape
Particles not held together in a rigid matter
Particles can slip and slide past one another—able to flow

4. STATES OF MATTER GASES--no fixed shape or volume
Can expand to fill any container they occupy.
Particles are not held to one another, and are free to move about

5. PHYSICAL CHANGES
A change which alters a given material without changing its composition
Examples of physical changes
Cutting, grinding, and bending a material

6. 2.2 MIXTURES
HOMOGENEOUS MIXTURE: contains substances that are uniformly distributed
All regions are identical in their composition and their properties
HETEROGENEOUS MIXTURE: contains substances that are not evenly distributed
Some regions have different properties from other regions

7. Phases
PHASES: any part of a system that has uniform composition and properties
Example:
Oil-vinegar dressing has two phases
How many phases do homogeneous mixtures have? Heterogeneous?

8. Methods of Separating Mixtures
Physical methods can be used to separate mixtures into the component parts
Techniques include:
Filtering
Chromatography
Distillation

10. Salt remains after all water is boiled off.

11. 2.3 ELEMENTS VS COMPOUNDS
SIMPLIEST BUILDING BLOCK OF MATTER
NO FURTHER SEPARATION POSSIBLE WHILE RETAINIING IDENTITY
COMBINATION OF TWO OR MORE SUBSTANCES
SEPARATED INTO SIMPLER SUBSTANCES BY CHEMICAL CHANGE

12. 2.4 CHEMICAL REACTIONS
CHEMICAL REACTION-one or more substances change into new substances
Reactants Products
Chemical property-the ability of a substance to undergo a chemical reaction
Fundamental law of chemistry
LAW OF CONSERVATION OF MASS

13. SCIENTIFIC MEASUREMENTS
CHAPTER 3

14. IMPORTANCE OF MEASUREMENT
Qualitative vs. quantitative measurement
ACCURACY: the extent to which it approaches the true value and is free from error
PRECISION: how close your results are for each trial
Percent Error = experimental value– true value x 100%
True value

15. Not precise, not accurate
Precise, but not accurate
Accurate and precise

16. International System of Units (SI)
Length = METER
Mass = KILOGRAM
Volume = LITER
Temperature = KELVIN
Amount of substance = mole

17. MASS VS. WEIGHT Weight depends on gravity, but mass doesn’t
Since gravity varies from place to place, weight also varies.
Mass is constant because it’s not determined by gravity.

18. Density All matter has a density Relationship between mass and volume
Means of identifying matter
D = m v

19. 3.5 TEMPERATURE
The temperature of a substance determines the direction of heat flow.
Heat energy moves from the object with a higher temperature to an object with a lower temperature.
Use two temperature scales.
Degrees Celsius
Kelvin C + 273=K