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CHEMISTRY SEPTEMBER 30, 2014

CHEMISTRY SEPTEMBER 30, 2014. SI/ SIGNIFICANT FIGURES/SCIENTIFIC NOTATIONS. SCIENCE STARTER. Verbal Science Starter. OBJECTIVE. SWBAT Apply the SI units Apply the significant rules Apply the scientific notation rules. AGENDA. Science Starter SI units Significant Figures

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CHEMISTRY SEPTEMBER 30, 2014

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  1. CHEMISTRYSEPTEMBER 30, 2014 SI/SIGNIFICANT FIGURES/SCIENTIFIC NOTATIONS

  2. SCIENCE STARTER • Verbal Science Starter

  3. OBJECTIVE • SWBAT • Apply the SI units • Apply the significant rules • Apply the scientific notation rules

  4. AGENDA • Science Starter • SI units • Significant Figures • Scientific Notation

  5. IMPORTANT DATES • Makeup Quiz on Wednesday during 4th period or 9th period (Up to 4:15PM) • Lab – Thursday • Quiz 03 – Friday • Test 01 – Next Friday

  6. Solubility Curve

  7. Solubility

  8. PURE SUBSTANCE

  9. Particle Diagram

  10. PARTICLE DIAGRAMS - ELEMENTS

  11. PARTICLE DIAGRAMS - COMPOUND

  12. PARTICLE DIAGRAMS - HOMOGENEOUS

  13. PARTICLE DIAGRAMS - HETEROGENEOUS

  14. Separation Techniques

  15. SEPARATION TECHNIQUES • Chromatography • Filtration • Evaporation • Distillation • Magnetism

  16. CHROMATOGRAPHY • Definition: Method in which components of a mixture is separated based on how quickly different molecules dissolved in a mobile phase solvent move along a solid phase • One type is called Paper Chromatography • Usually used to identify chemicals (coloring agents) • Example: Identifying the chemicals in a marker

  17. CHROMATOGRAPHY

  18. FILTRATION • Method for separating an insoluble solid from a liquid • Popularly used in water treatment • Example: Separating river water

  19. FILTRATION

  20. EVAPORATION • Method used to separating a homogeneous (solution) mixture of a soluble solid and a solvent • Involves heating the solution until the solvent evaporates • Examples: Sugar water solution • Heat the solution until the water (solvent) dissolve leaving behind the sugar

  21. EVAPORATION

  22. DISTILLATION • Method used to separate a liquid from a solution • Similar to evaporation but the vapor is collected by condensation • Example: Sugar Water solution

  23. DISTILLATION

  24. MAGNETISM • Method used to separate two solids with one having magnetic properties • Example: Separating iron filings and dirt mixture

  25. MAGNETISM

  26. SEPARATING FUNNEL • Method for separating two immiscible liquids (liquids that do not dissolve well) • Example: Oil and water

  27. SEPARATING FUNNEL

  28. Miscible vs. Immiscible • Miscible: Forming a homogeneous solution when added together • Immiscible: do not form a homogeneous solution when added together. Do not dissolve well

  29. SI UNITS INTERNATIONAL SYSTEM OF UNITS

  30. SI UNITS • standard system of measurements used in chemistry • enable scientists to communicate with one another • there are 7 base units • all other units are derived from these 7 base units

  31. 7 SI base units • ampere (A) – measures electric current • kilogram (kg) – measure mass • meter (m) – measure length • second (s) – measure time • kelvin (K) – measure thermodynamic temperature • mole (mol) – measure amount of substance • candela (cd) – measure luminous intensity

  32. CONVERSION BETWEEN UNITS • Step 1: Draw the picket fence • Step 2: Identify the given • Step 3: Identify what you are looking for • Step 4: Identify the equivalent relationship • Step 5: Get rid of the units • Step 6: Do the math • Step 7: Check for the final unit(s)

  33. EXAMPLE • 10 m = __________________cm • Step 1: Draw the picket fence

  34. EXAMPLE – CONT’ • Step 2: Identify the given • 10 m • Step 3: Identify what you are looking for • cm • Step 4: Identify the equivalent relationship • 1cm = 0.01 m

  35. EXAMPLE – CONT’ • Step 5: Set up the problem

  36. EXAMPLE – CONT’ • Step 6: Get rid of the units

  37. EXAMPLE – CONT’ • Step 7: Do the math • Step 8: Check for the final unit(s)

  38. SIGNIFICANT FIGURES

  39. DEFINITION • a prescribed decimal place that determines the amount of rounding off to be done based on the precision of the measurement • consist of all digits known with certainty and one uncertain digit.

  40. RULES FOR DETERMINING SIGNIFICANT FIGURES • nonzero digits are always significant • example: 46.3 m has 3 significant figures • example: 6.295 g has 4 significant figures

  41. RULE – CONT’ • Zeros between nonzero digits are significant • example: 40.7 m has 3 significant figures • example: 87,009 m has 5 significant figures

  42. RULE – CONT’ • Zeroes in front of nonzero digit are not significant • example: 0.009587 m has 4 significant figures • example: 0.0009 g has 1 significant figure

  43. RULE – CONT’ • Zeroes both at the end of a number and to the right of a decimal point are significant • example: 85.00 g has 4 significant figures • example: 9.0700 has 5 significant figures

  44. EXAMPLE • 1. Give the number of significant figures in each of the following.  •  a)  10.0005 g   ______ • Do the next 3 problems

  45. EXAMPLES - answers • b)  0.003423 mm  __4____ •  c)  67.89 ft___4___ •  d)  78.340 L  __5____

  46. MULTIPLICATION/DIVISION RULES • The number of significant figure for the answer can not have more significant figures than the measurement with the smallest significant figures

  47. EXAMPLES 12.257 x 1.162 = 14.2426234 • 12.257 = 5 significant figures • 1.162 = 4 significant figures • Answer = 14.24 (4 significant figures)

  48. EXAMPLE - Answer • 12.257 = 5 significant figures • 1.162 = 4 significant figures

  49. EXAMPLE – Answer cont’ • Answer = 14.24 (4 significant figures)

  50. ADDITION/SUBSTRATION RULES • The number of significant figure for the answer can not have more significant number to the right of the decimal point

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