1. IB Chemistry A Watson/ Scheffler South Pointe High School

2. IB Chemistry Instructor : Mrs. Allyson Watson Email : AWatson@rock-hill.k12.sc.us 2

3. Your Name Address Telephone Number Email Hobbies: Goals: Class Information/ Expectations Form 3

4. Periods Information forms Safety contracts Class Policies Cornell Notes Brief overview of the course Chemical Hazards/Lab Safety Scientific Methods Assignments IB Chemistr y Agenda 4

5. IB Chemistry JUNIORS Assignments NEXT CLASS: Return signed the Safety Agreement and read thoroughly the chemical hazards/Lab Safety handout OTHER CLASS: Finish reading topic 1 in textbook 5

6. Expectations See expectation handouts for details Attendance Make Up Behavior Grading Cornell notes

7. Cornell Notes Divide the paper Documentation Record notes Review and Clarify Summarize Study

8. Introduction to Chemistry Chemistry The study of matter and its relationships The study of materials and how they interact The Central Science 8

9. Chemistry Topics Include Atomic Theory Periodic Table Bonding Formulas and Stoichiometry States of matter Calorimetry / Thermodynamics Solutions Kinetics Equilibrium Acids and Bases Oxidation Reduction 9

10. Is Chemistry Hard?? 10 Maybe! --- but you will develop skills that are valuable for the rest of your life!

11. Is Chemistry Hard?? Abstract Thinking Critical Thinking Analysis Logic Math Skills Well maybe but you will develop skills that are valuable for the rest of your life These include: 11

12. Is Chemistry Hard?? Abstract Thinking Critical Thinking Analysis Logic Math Skills Problem Solving Communication Time Management Hazards Management Well maybe but you will develop skills that are valuable for the rest of your life These include: 12

13. Is Chemistry Dangerous?? 13 Well maybe. sort of…..

14. Chemical Hazards Hazard Criteria  A Threshhold Limit value of less than 500 ppm  A Lethal dose (LD50) less than 500 mg per kg  Readily polymerizable  Flashpoint less than 140 o F  A strong oxidizer or reducing agent  Highly corrosive  Carcinogen, mutagen,or teratogen.  Radioactive  See the handout for more definitions and criteria for chemical hazards 14

15. Scientific Methods Always based on observation and experimentation Observable and reproducible evidence are required to support conclusions 15

16. Scientific Method Investigation process - Preliminary observations - Formulation of a hypothesis -Design experiments to test the hypothesis -Evaluate and interpret data -Draw appropriate conclusions 16

17. Hypothesis, Theory and Law A Hypothesis A Hypothesis is a tentative explanation or expected result based on past evidence and experience A Theory A Theory is an explanation of a phenomona based on the results of scientific experimentation. A Law A Law is a principle that can be observed repeatedly in the world over a long period of time 17

18. Scientific Methods The scientific method is not necessarily a chronological order that scientists always follow. But remember ……….. Scientific information is always based on evidence. The emphasis is always on information that we can gain from observations and experiments Scientific information is always based on evidence. The emphasis is always on information that we can gain from observations and experiments 18

19. Matter Has both volume and mass Exists in various states: Solid Liquid Gas Plasma 19

20. Forms of Matter Element Compound Mixture Homogeneous Heterogeneous 20

21. Elemental Composition of the Earth

22. Properties of Matter Physical - Chemical - Extensive - Intensive - Color Density Melting point How the substance reacts with other substances Depend on the amount of material Independent of the amount of material 22

23. Density Definition Formula Ratio of mass to volume D = Mass/ volume Density is an intensive property. It is constant for most solids and liquids, but it depends on the pressure and temperature for a gas 23

24. Physical and Chemical Changes Physical - Chemical - A change in state or shape. Affects the physical properties but retains the properties of the substance Undergoes a chemical reaction. A new substance is formed with new physical and chemical properties 24

25. Measurement Measurements in the laboratory will normally be made using the metric system and SI units where feasible 25

26. Temperature Scales KelvinCelsiusFahrenheit Boiling point of water. 373 K100 o C212 o F Freezing point of water. 273 K100 o C32 o F Absolute Zero. 0 K-273 o C-460 o F 26

27. Temperature Conversions Fahrenheit to Celsius o C = 5/9 ( o F - 32) Celsius to Fahrenheit o F = 9/5 o C + 32 Celsius to Kelvin K = o C +273 27

28. Problem Solving Density Formulas Density = Mass/volume D = m/V M = DV V = m/D Units Density = g/cm 3 Mass = grams or g Volume = cubic centimeters or cm 3 If you solve the formula correctly the units will match D = m/V = g/cm 3 M = DV = (g/cm 3 ) /(cm 3 ) = g V = m/D =(g)/(g/cm 3 ) = cm 3

29. Measurement Issues Uncertainty Accuracy Precision Error Significant Figures Scientific Notation 29