1. Introduction to Chemistry
Chapter 1

2. Branches of Chemistry Chemistry Organic Chemistry Inorganic Chemistry
The study of matter and changes it undergoes
Organic Chemistry
Carbon containing chemicals
Pharmaceuticals (drugs), plastics
Inorganic Chemistry
Matter with no Carbon
Minerals, metals and non-metals

3. Branches of Chemistry Physical Chemistry Analytical Chemistry
Behavior and change of matter and energy (chemistry and physics combined)
Reaction Rates, reaction mechanisms (how fast reactions take place and how to speed them up)
Analytical Chemistry
Composition of substance
Food nutrients, quality control, FDA
Biochemistry
Processes of living organisms
Metabolism, fermentation

4. Scientific Method
The scientific method is an organized set of investigation procedures.
6 common steps
State the problem
Gather information
Forming a hypothesis
Testing the hypothesis
Analyzing the data
Drawing a conclusion

5. Scientific Method (Step 1,2,3)
1.State the Problem(Questions)
2.Make Observation – do research
Visual Observations
Existing Knowledge
3.Create a Hypothesis
Tentative explanation, a testable statement or prediction
DOES NOT need to be a question

6. Scientific Method (Step 4)
4.Experiments
Set of controlled observations
Tests one variable at a time
Independent Variable- Plan to change
Dependent Variable- Value changes in response to independent variable
Control Group- Standard for comparison
Experimental Group – Where one changes the independent variable.

7. Scientific Method (Step 5,6)
5.Data: Graphs, Tables, Lists, etc.
Collect data
Qualitative Data- describes a property w/out measurements, uses senses (ex. Color)
Quantitative data – data collected using measurements (ex. Volume)
6.Conclusion
Judgment based on information; Responds to purpose; Analysis of results

8. Scientific Theory
Explanation supported by many, many experiments can be modified, lead to new conclusions
Examples of Theories:

9. Scientific Law No exceptions to laws, in any experiment
Example of Laws:

10. Law of Conservation of Mass
Total amount of matter in the universe remains constant
Matter can’t be created nor destroyed
Total amount b/4 reaction= total amount after reaction
Ex. Balancing equations

11. PbI demo

12. Law of Conservation of Energy
Energy can’t be created nor destroyed
Total amount remains constant
Can transform into different types of energy
Ex. Match: potential chemical energy into heat, light, sound, kinetic

13. Research Scientific Research Chance discoveries
Pure Research: seeks for knowledge itself
Applied Research:To solve specific problem (disease research)
Chance discoveries
Botox

14. Matter Anything that has mass and takes up space. Examples of matter:
Examples of non-matter:

15. a. Inertia
Resistance to change in motion or resistance to change in direction or rate

16. b. Mass Amount of matter in an object Measure of the inertia
Does NOT change from place to place
Measure with a balance

17. Measure of the force of gravity between 2 objects
c. Weight
Measure of the force of gravity between 2 objects
Weight= mass X gravity
Changes with location
Measure with scale

18. Property possessed by matter, ability to do work
2. Energy
Property possessed by matter, ability to do work
We are interested in the energy changes that take place

19. Types of Energy
Potential- energy due to the objects position, also stored energy (ex. Battery- chemical potential energy)
Kinetic- energy of motion
Radiant- energy that goes in all directions (light, x-rays, UV), transferred by electromagnetic waves
Other- heat, sound, nuclear, electric

20. Models
Visual, verbal, and/or mathematical explanations of how things occur.
Where have you seen models before?

21. Lab Equipment

22. Lab Equipment