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Chapter 2 – Measurements and Calculations

Chapter 2 – Measurements and Calculations. Evidence of Chemical Change. Evolution of a Gas (Bubbles, Odor) Formation of a Precipitate (Formation of Cloudiness in a Clear Solution, Solids Collecting at the Bottom or Top) Release of Energy (Heat, Light) Color Change. Scientific Method.

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Chapter 2 – Measurements and Calculations

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  1. Chapter 2 – Measurements and Calculations Honors Chemistry, Chapter 2 Page 1

  2. Evidence of Chemical Change Evolution of a Gas (Bubbles, Odor) Formation of a Precipitate (Formation of Cloudiness in a Clear Solution, Solids Collecting at the Bottom or Top) Release of Energy (Heat, Light) Color Change Honors Chemistry, Chapter 2 Page 2

  3. Scientific Method • Observing and Collecting Data • Qualitative (Bubbles Formed) • Quantitative (1 gram/liter of catalyst speeded the reaction by 25%) • Chemists Study Systems (Region Selected for Study) • Formulate Hypothesis • Generalization about Data • Testable Statement Honors Chemistry, Chapter 2 Page 3

  4. Scientific Method • Testing Hypothesis (Experimentation) • Supported, Retained • Not Supported, Discarded, Modified • Theorizing – Create a Model • Model: An Explanation of How Phenomena Occur and How Data or Events are Related. • Visual • Verbal • Mathematical Honors Chemistry, Chapter 2 Page 4

  5. JFHICW FH VHHVLBFND FL N ZGVHFIVLB, BTV NZZVNGNLPV CY JFHICW JFDD IC FL N PNLIFINBV. – VGFP HVRNGVFI. Honors Chemistry, Chapter 2 Page 5

  6. JFHICW FH VHHVLBFND FL N ZGVHFIVLB, BTV NZZVNGNLPV CY JFHICW JFDD IC FL N PNLIFINBV. – VGFP HVRNGVFI. (Wisdom is essential in a president, the appearance of wisdom will do in a candidate. – Eric Severeid) Honors Chemistry, Chapter 2 Page 6

  7. Chapter 2, Section 1 Review • What is the purpose of the scientific method? • Distinguish between qualitative and quantitative observations. • Describe the differences between hypothesis, theories, and models. Honors Chemistry, Chapter 2 Page 7

  8. Units of Measure Measurements Are Quantitative Information Quantity: Something That Has Size or Amount Honors Chemistry, Chapter 2 Page 8

  9. SI Measurement SI Units Are Defined in Terms of Standards of Measurement Seven Basic Units All Others Derived From Seven Basic Units Honors Chemistry, Chapter 2 Page 9

  10. SI Base Units Honors Chemistry, Chapter 2 Page 10

  11. SI Prefixes Honors Chemistry, Chapter 2 Page 11

  12. SI Prefixes Honors Chemistry, Chapter 2 Page 12

  13. Useful Conversion Factors • 1000 ml = 1 L • 1 cm3 = 1 ml • 1000 g = 1 kg • 1000 mg = 1 g • 1000 mg = 1 mg • 1000000 mg = 1 g • 1000 mmol = 1 mol Honors Chemistry, Chapter 2 Page 13

  14. Metric Prefixes

  15. Learning Check 1. 1000 m = 1 ___ a) mm b) km c) dm 2. 0.001 g = 1 ___ a) mg b) kg c) dg 3. 0.1 L = 1 ___ a) mL b) cL c) dL 4. 0.01 m = 1 ___ a) mm b) cm c) dm

  16. O—H distance = 9.4 x 10-11 m 9.4 x 10-9 cm 0.094 nm Units of Length • ? kilometer (km) = 500 meters (m) • 2.5 meter (m) = ? centimeters (cm) • 1 centimeter (cm) = ? millimeter (mm) • 1 nanometer (nm) = 1.0 x 10-9 meter

  17. Learning Check Select the unit you would use to measure 1. Your height a) millimeters b) meters c) kilometers 2. Your mass a) milligrams b) grams c) kilograms 3. The distance between two cities a) millimeters b) meters c) kilometers 4. The width of an artery a) millimeters b) meters c) kilometers

  18. Derived Units Area A m2 Volume V m3 Density D kg/m3 (=m/V) Molar Mass M kilograms/mol Concentration c mol/liter Molar Volume Vm m3/mol Energy E joule Honors Chemistry, Chapter 2 Page 18

  19. Helpful Hint m V D Relationship Between D, m, and V: Honors Chemistry, Chapter 2 Page 19

  20. PROBLEM:Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg in grams? In pounds?

  21. PROBLEM:Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg? First, note that1 cm3 = 1 mL Strategy 1. Use density to calc. mass (g) from volume. 2. Convert mass (g) to mass (lb) Need to know conversion factor = 454 g / 1 lb

  22. PROBLEM:Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg? 2. Convert mass (g) to mass (lb) 1. Convert volume to mass

  23. Learning Check Osmium is a very dense metal. What is its density in g/cm3 if 50.00 g of the metal occupies a volume of 2.22cm3? 1) 2.25 g/cm3 2) 22.5 g/cm3 3) 111 g/cm3

  24. Solution 2) Placing the mass and volume of the osmium metal into the density setup, we obtain D = mass = 50.00 g = volume 2.22 cm3 = 22.522522 g/cm3=22.5 g/cm3

  25. Volume Displacement A solid displaces a matching volume of water when the solid is placed in water. 33 mL 25 mL

  26. Learning Check What is the density (g/cm3) of 48 g of a metal if the metal raises the level of water in a graduated cylinder from 25 mL to 33 mL? 1) 0.2 g/ cm3 2) 6 g/m3 3) 252 g/cm3 33 mL 25 mL

  27. Learning Check K W V V K W W V K Which diagram represents the liquid layers in the cylinder? (K) Karo syrup (1.4 g/mL), (V) vegetable oil (0.91 g/mL,) (W) water (1.0 g/mL) 1) 2) 3)

  28. Learning Check The density of octane, a component of gasoline, is 0.702 g/mL. What is the mass, in kg, of 875 mL of octane? 1) 0.614 kg 2) 614 kg 3) 1.25 kg

  29. Learning Check If blood has a density of 1.05 g/mL, how many liters of blood are donated if 575 g of blood are given? 1) 0.548 L 2) 1.25 L 3) 1.83 L

  30. Conversion Factors Fractions in which the numerator and denominator are EQUAL quantities expressed in different units Example: 1 in. = 2.54 cm Factors: 1 in. and 2.54 cm 2.54 cm 1 in.

  31. Learning Check Write conversion factors that relate each of the following pairs of units: 1. Liters and mL 2. Hours and minutes 3. Meters and kilometers

  32. How many minutes are in 2.5 hours? By using dimensional analysis / factor-label method, the UNITS ensure that you have the conversion right side up, and the UNITS are calculated as well as the numbers! Conversion factor 2.5 hr x 60 min = 150 min 1 hr cancel

  33. Factor Label Method 1 kg 1000 g 1 = --------------- or -------------- 1000 g 1 kg • Express 4.5 kg as grams • Begin by Expressing as a Fraction: 4.5 kg 1 • Identify Conversion Factor: 1 kg = 1000 grams • Express as a Fraction: Honors Chemistry, Chapter 2 Page 33

  34. Factor LabelContinued 4.5 kg 1000 g --------- x -------------- = 4500 g 1 1 kg Write Equation Including Proper Factor Cancel Units Multiply Numbers to Get Final Result Honors Chemistry, Chapter 2 Page 34

  35. Factor Label Steps • Express as a Fraction • Identify Conversion Factor • Express Conversion Factor as Two Fractions • Select Proper Factor (units in denom.) • Write Equation Including Proper Factor • Cancel Units • Multiply Numbers to Get Final Result Honors Chemistry, Chapter 2 Page 35

  36. Chapter 2, Section 2 Review • Distinguish between a quantity, a unit, and a measurement standard. • Name SI units for length, mass, time, volume, and density. • Distinguish between mass and weight. • Perform a density calculation. • Transform a statement of equality to a conversion factor (factor label method). Honors Chemistry, Chapter 2 Page 36

  37. Scientific Measurements Accuracy – The Closeness of Measurements to the Correct or Accepted Value Precision – The Closeness of a Set of Measurements Honors Chemistry, Chapter 2 Page 37

  38. Accuracy vs. Precision XX XX XX XX High Precision High Accuracy High Precision Low Accuracy Honors Chemistry, Chapter 2 Page 38

  39. Accuracy vs. Precision X X X X X X X X Low Precision Low Accuracy Low Precision High Accuracy (on average) Honors Chemistry, Chapter 2 Page 39

  40. Percent Error Valueaccepted - Valueexperimental %Error = --------------------------------------- Valueaccepted X 100 Honors Chemistry, Chapter 2 Page 40

  41. Significant Figures • | I I I I | I I I I | I I I I | I I I I | • 8 9 • 8.36 All the Digits Known With Certainty Plus One Final Digit Which is Somewhat Uncertain Honors Chemistry, Chapter 2 Page 41

  42. Rules for Significant Figures • Zeros Appearing Between Nonzero Digits are Significant • Zeros Appearing in Front of All Nonzero Digits are Not Significant • Zeros Appearing to the Right of the Decimal Point And at the End of the Number are Significant Honors Chemistry, Chapter 2 Page 42

  43. Rules for Significant Figures • 4. Zeros at the End of a Number but to the Left of the Decimal Point May or May Not be Significant. If a Zero Has Not Been Measured or Estimated but is Just a Placeholder, it is Not Significant. A Decimal Point Placed After Zeros Indicates They are Significant. Honors Chemistry, Chapter 2 Page 43

  44. Rules for Rounding If the Digit Following the Last Digit to be Retained is: > 5 Then Round Up < 5 Then Round Down 5 Followed by non Zero Digits Then Round Up Honors Chemistry, Chapter 2 Page 44

  45. Rules for Rounding If the Digit Following the Last Digit to be Retained is: 5 Followed by Non-Zero Digit(s), and Preceeded by an Odd Digit Round Up 5 Followed by Non-Zero Digit(s), and Preceeded by an Even Digit Leave Unchanged Honors Chemistry, Chapter 2 Page 45

  46. Significant Figures With Addition/Subraction When Adding or Subtracting Decimals, the Answer Must Have the Same Number of Digits to the Right of the Decimal Point as There are in the Measurement Having the Fewest Digits to the Right of the Decimal Point. Honors Chemistry, Chapter 2 Page 46

  47. Significant Figures With Multiplication/Division • When Multiplying or Dividing, the Answer Can Have no More Significant Figures Than are in the Measurement with the Fewest Number of Significant Figures. • (Conversion Factors Have Unlimited Digits of Accuracy.) Honors Chemistry, Chapter 2 Page 47

  48. Significant Figures • The numbers reported in a measurement are limited by the measuring tool • Significant figures in a measurement include the known digits plus one estimated digit

  49. Counting Significant Figures RULE 1. All non-zero digits in a measured number are significant. Only a zero could indicate that rounding occurred. Number of Significant Figures 38.15 cm 4 5.6 ft 2 65.6 lb ___ 122.55 m___

  50. Leading Zeros RULE 2. Leading zeros in decimal numbers are NOT significant. Number of Significant Figures 0.008 mm 1 0.0156 oz 3 0.0042 lb ____ 0.000262 mL ____

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