1. Slope Rise = y 2 -y 1 = m 2 -m 1 = mass Run x 2 -x 1 v 2 -v 1 volume Pick 2 points. Write the coordinates (x 1,y 1 )(x 2,y 2 ) Calculate the density Do this on your graph.

2. Computer Graphing Excel A- x axis,Time B- Y axis, volume of Na2S2O3 Highlight all 2columns Insert X,Y scatter middle chart left column Chart layout first box Title (include your name), label both axis right click, move chart, New sheet Unshade background Print 2 to lexchem

3. More Dimensional Analysis 1.Convert 45 miles/hour to: in/sec 2.Convert 14.6 Kg/L to: dg/mL

4. Observing Card Trick Zooley Always make at least 4 observations: state of matter (solid,liquid,gas) color clarity odor

5. Energy Capacity to do work or produce heat

6. Measuring Energy Calorie the amount of heat needed to raise the temperature of 1 gram of water 1 o C. 1000 cal.=1 Kcal=1 Calorie (food) Joule 1 cal.=4.184 J

7. Practice 1.A student uses 30 J of energy putting books on a shelf. How many calories is this? 2.The energy content of a bag of potato chips is 350 Calories How many J is this?

8. Energy Types Nuclear Chemical Electrical Solar Thermal Mechanical

9. Law of Conservation of Energy Energy is neither created nor destroyed (its converted from one form to another)

10. Energy Conversion Hair dryer

11. Temperature Amount of hotness or coldness Temperature is not heat C= K-273 ( Celsius is smaller so subtract) K= C+ 273

12. Pure Matter Elements cannot be broken down by chemical processes Compound Chemical combination of elements (share or transfer of electrons)

13. Changes in Matter Physical changes Involve no change in composition P hysical properties: Boiling/melting point, density, color, odor, ductile Chemical changes Involves a change in composition Heat change Color change Gas evolved Precipitate formed Chemical properties: combustion, reactivity

14. Lab: Physical/Chemical Changes Title Purpose: To determine physical and chemical changes as indicators for a chemical reaction Safety: Data table:

15. Law of Conservation of Matter Matter is neither created nor destroyed, it is conserved (not in nuclear reactions)

16. Matter Anything that has mass and volume do not copy in notebook DensityPressureContainer Solid High not affectedown shape Liquid High not affected takes shape Gas low affectedfills Plasma low affected fills

17. Mixtures (Not pure substances physical combination) Homogeneous (solution) 1 phase visible Heterogeneous 2 or more phases visible

18. Separation of Mixtures Homogeneous: Distillation Crystallization Chromatography Heterogeneous: Filtration

19. Practice Physical/Chemical Processes 2.3 RR 2.4 RR 2.5 RR

20. Types of Energy Kinetic energy of motion Potential stored energy

21. Lab: Separation of Mixture Title Partner, date Goal: To separate a mixture of salt and sand and to determine the percent sand and salt Write your own specific step by step procedure Make your own data table Show percent calculations and percent error Specific error analysis

22. Pre-lab quiz - Fractional distillation 1.State 1 safety hazard to remember with ethyl alcohol (ethanol) 2.What will be recorded periodically through the distillation? 3.List 2 physical properties observed or recorded 4.State 1 safety hazard to remember about the flask at the end. 5.What observation/measurement will indicate to change beakers to collect each fraction?