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Goal 1 Notes

Goal 1 Notes. Physical Science By Nancy Booth. Physical Science. I. Applied Science vs. Pure Science II. Technology III. What is Physical Science? IV. Problems vs. exercises A. Problem solving 1. Known 2. Unknown 3. No set way to find answer. B. Critical Thinking

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Goal 1 Notes

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  1. Goal 1 Notes Physical Science By Nancy Booth

  2. Physical Science I. Applied Science vs. Pure Science II. Technology III. What is Physical Science? IV. Problems vs. exercises A. Problem solving 1. Known 2. Unknown 3. No set way to find answer

  3. B. Critical Thinking C. Scientific Method 1. Observation 2. Purpose: Question 3. Hypothesis: Proposed answer 4. Experiment 5. Data 6. Data analysis 7. Conclusion

  4. V. Hypothesis vs. theory vs. law VI. The Experiment A. Control B. Constant C. Independent variable - manipulated variable D. Dependent variable - responding variable

  5. VII. SI - International System of Units A. Base unit for some measurements 1. Distance - meter 2. Mass - kilogram 3. Time - second 4. Temperature - Kelvin scale • Absolute zero - lowest temperature • Kelvin temperature = Celsius temperature + 273 B. Based on 10’s C. Derived units - combine base units D. Standards

  6. VIII. Metric Conversions A. Set-up ratios and cross multiple. Then solve. Ex.: 20 liters = _____ milliliters 1 liter = 1000 milliliters

  7. B. Factor-Label Method Ex.: 20 liters = _____ milliliters 1 liter = 1000 milliliters

  8. C. Small Unit Large Unit (divide) ÷ Large Unit Small Unit (multiply) × 20 L = _______ ml 300 mg = _______ g

  9. D. Use a number line King Henry Died Monday Drinking Chocolate Milk

  10. E. Use stair steps as a guide

  11. IX. Graphs A. Line graphs - trend or pattern over time 1. y-axis - dependent variable 2. x-axis - independent variable B. Bar graph - Comparison of numbers 1. Bars don’t touch 2. Numbers must be on one axis

  12. C. Circle graph or Pie graph - Parts of a whole 1. Parts must add to 100% 2. Numbers for parts do not have to equal 100, but when converted to a % the total of all parts equals 100%

  13. Bar Graph • 1st Period: 10 – 9th; 2 – 10th; 3 – 11th; and 4 – 12th. • 2nd Period: 8 – 9th; 6 – 10th; 10 – 11th; and 2 – 12th. • 4th Period: 0 – 9th; 12 – 10th; 9 – 11th; and 8 – 12th.

  14. Pie Graph • Use the data from the bar graph to create a pie graph with slices for 9th, 10th, 11th, and 12th.

  15. Line Graph Time Distance 0 sec 0 m 10 sec 20 m 30 sec 50 m 60 sec 90 m 70 sec 100 m 80 sec 120 m 100 sec 150 m

  16. X. Density Density refers to how compacted a material is. Units D = density mg/ml, g/cm3, kg/l m = mass kg, g, mg V = volume ml, l, cm3, dm3

  17. Example 1: What is the density of a 20 g object that has a volume of 5 cm3? D = ? m = 20 g V = 5 cm3 D = 20 g / 5 cm3 = 4 g/cm3

  18. Example 2: What is the volume of 20 g of gold? (Density of gold is 19.3 g/cm3) D = 19.3 g/cm3 m = 20 g V = ? V = 20 g / (19.3 g/cm3) = 1.04 cm3

  19. Example 3: What is the mass of 30 cm3 of quartz? (Density of quartz is 2.6 g/cm3) D = 2.6 g/cm3 m = ? V = 30 cm3 m = V D m = (30 cm3)(2.6 g/cm3) = 78 g

  20. Flash Card - Density

  21. Density Practice Problems 1. What is the density of an object that is 30 cm3 and has a mass of 99 g?

  22. 2. What is the volume of 69 g of a liquid that has a density of 1.3 g/cm3?

  23. 3. What is the mass of 650 cm3 of gold? (Gold has a density of 19.3 g/cm3)

  24. 4. Determine the density of 45 g of a solid that is 5 cm by 4 cm by 6 cm? (NOTE: Volume of a rectangular solid is V = w h l)

  25. 5. Determine the volume of 65 g of mercury. The density of mercury is 13.6 g/cm3.

  26. 6. If you have 33 ml of glue, how many grams do you have? (Glue has a density of 1.27 g/cm3)

  27. XI. Scientific Notation Shorthand method for writing very large and very small numbers by using powers of 10.

  28. XII. Rules for Scientific Notation A. Writing Numbers With Scientific Notation: 1. Move the decimal point so that only one number remains to the left of the decimal point. Ex.: In 36000 the decimal point will move to after the 3, giving 3.6

  29. 2. Count the number of places you moved the decimal point and use it as the exponent. Ex.: In 36000 the decimal point was moved 4 places to the left to give 3.6. • The exponent is negative if the decimal point is moved to the right. • The exponent is positive if the decimal point is moved to the left. 3. Write the number times 10 with the exponent of the number of places the decimal was moved. Ex.: 36000 is therefore 3.6 X 104

  30. B. Writing Numbers from Scientific Notation: 1. Write the number dropping the X 10. 2. Move the decimal point the number of places equal to the exponent that was on the X 10. Ÿ The decimal point is moved to the right if the exponent was positive. Ÿ The decimal point is moved to the left if the exponent was negative. Ex.: 7.9 X 106 becomes 7900000. 8.6 X 10-4 becomes .00086.

  31. C. Mathematical Operations using Scientific Notation: 1. Addition and Subtraction • Before numbers can be added or subtracted that are in scientific notation the must have the same exponent. 2. Multiplication • Multiply the first numbers and add the exponents. • Check the decimal in the new first number. Relocate the decimal as necessary and change the exponent as needed. 3. Division • Divide the first numbers and subtract the exponents. • Check the decimal in the new first number. Relocate the decimal as necessary and change the exponent as needed.

  32. XIII. Significant Figures Show the precision of an measurement. The more significant figures the more precise the measurement. The measurement show all the digits that are known plus a last one that is estimated.

  33. XIV. Rules for determining significant figures 1. All non-zero digits are significant. Ex.: 549 has 3 significant figures. 2. All zeroes between non-zero digits are significant. Ex.: 3005008 has 7 significant figures. 3. All zeroes to the right of a non-zero digit and to the left of an expressed decimal point are significant. Ex.: 5600. has 4 significant figures. 4. All zeroes after a non-zero digit and to the right of an expressed decimal point are significant. Ex.: 560.00 has 5 significant figures.

  34. 5. All zeroes after a non-zero digit and to the left of an unexpressed (assumed) decimal point are not significant. Ex.: 7600 has 2 significant figures. 6. All zeroes to the left of a non-zero digit and to the right of an expressed decimal point are not significant. Ex.: .00067 has 2 significant figures.

  35. 7. When multiplying and dividing number, count the number of significant figures in each number and round the final answer so that it has the same number of digit as the least significant number. Ex.: 54 X 768 = 42444 will be rounded to 2 significant figures or 42000 8. When adding and subtracting number, do the operation and round the answer to the same digit as the least significant number. Ex.: 56 + 34.980 - 6.7 = 84.28 will be rounded to the ones place or 84

  36. Practice Significant Figures and Scientific Notation Problems I. Convert the following numbers to scientific notation. 1. 76000 2. 876000000 3. .000823 4. .00732 5. .000000881 6. 7610320

  37. II. Change the following numbers to regular notation from scientific notation. 7. 6.7 x 107 8. 7.2 x 10-2 9. 8.6 x 104 10. 3.2 x 10-6 11. 8.1 x 10-5 12. 4.03 x 103

  38. III. How many significant figures do each of the following numbers have? 13. 7620 14. 326.6 15. 1.370 16. .0032 17. .0000302 18. 1.02030 19. .00012 20. 12000 21. 132000.0

  39. IV. Complete the following operations and record the answers with the correct number of significant figures. 22. 7.6 x 104 + 3.2 x 103 23. 9.3 x 10-2 x 8.2 x 10-5 24. 8.2 x 10-2 ¸ 2.5 x 10-6 25. 5.4 x 10-3 - 6.3 x 10-4 26. 326 x 67.30 27. 99.33 + 162 28. 600 + 170 29. 376.4 ¸ 2.2 30. 9443.56 - 6000

  40. 1. Test tube 2. Scoop 3. Forceps 4. Triple-beam balance 5. Funnel 6. Watch glass 7. Beaker 8. Dropper pipet 9. Utility clamp 10. Test tube rack 11. Tongs 12. Stopper 13. Ring stand 14. Graduated cylinder 15. Flask 16. Thermometer 17. Iron ring You need to know the following pieces of lab equipment. Make a study guide by drawing the following pieces found on page xxii in your lab manual:

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