1. Observation - What is evidence?
Any observation of Natural Phenomena
Qualitative
Use your senses
Ex. Texture, color, smell, taste, sound
Quantitative
Measured values
Ex. Weight, volume, length, temperature
Measurements, Verifiable observations, etc.
Utilizing the Scientific Method, this is how we know what we know!

2. Organization of Matter
Continuous
Aristotle
Discontinuous
Democritus
( B.C.)
Dalton
(1808)
Joseph Gay-Lussac
(1805)

3. States of Matter Solid: high degree of interparticle
Water can be found in the solid, liquid, and vapor (gaseous) forms simultaneously.
Solid: high degree of interparticle
forces
Liquid: significant degree of interparticle
Gases: very low degree of interparticle

4. Changes of Matter
Physical: a change which does NOT alter the composition of a substance.
i.e.: cutting, breaking, tearing, phase
changes (melting, boiling), etc.
Chemical: a change which alters the composition of a substance.
i.e.: “rusting”, burning, “chemically
reacting”, etc.
The green color of the Statue of Liberty results from the reaction of copper with the components of air.

5. "Good" versus "Bad" Properties for a Chemical Substance

6. Properties & Changes of Matter

7. Organization of Matter

8. How could the appearance of each type of chemical change?
Outward physical appearance of naturally occurring elements
Hg As S
Bi I2 Mg
Mercury, sulfur, arsenic, bismuth, magnesium, iodine

9. Laws of Matter Law of Conservation of Mass Law of Definite Proportions
Amount of matter does not change during a physical or chemical reaction
Law of Definite Proportions
In samples of a chemical compound, the masses of the elements are always in the same ratio
Ex. H2O
Law of Multiple Proportions
Two or more elements may form more than one compound.
Ex. H2O and H2O2

10. Studying Matter - Chemistry
Requires a scientific approach
Scientific method
Nature of science
Requires use of a measurement system and tools for measuring
Requires displaying and explaining experimental results
Variables (dependent vs. independent) & controls

11. Metric System
Be able to measure/calculate mass, volume, distance, density & temperature

12. Measuring Length
The scale on a measuring device determines the magnitude of the uncertainty for the recorded measurement.
Include all certain digits plus one uncertain digit in your measurement!
significant (figures) digits (sd)

13. Volume/Space Liter (L) 1 L = 1 dm3 Milliliter (mL) 1 mL = 1 cm3 = 1 cc
Microliter (L) L = 1 mm3

14. Measuring Volume
Note the type of liquid
Indicate which kind of meniscus it is (concave or convex)
Concave: read the bottom of the meniscus (WATER)
Convex: read the top of the meniscus (MERCURY)
Include all certain digits plus one uncertain digit in your measurement! sd

15. Mass/Weight
A gram is defined as the mass of ml of water at 4˚C. Therefore, water has a density of 1 g/mL at 4˚ C.

16. Measuring Mass
Check that the scale is TARED prior to placing anything on it.
Include all certain digits plus one uncertain digit in your measurement! sd

17. Converting between Measurement Units

18. Conversions 453.6 graham crackers = 1 pound cake
2000 mockingbirds = 2 kilomockingbirds

19. Distance Conversion
It is experimentally determined that 1 inch equals 2.54 cm, or 1 cm equals inch