1. CHEMISTRY SEPTEMBER 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 4 th period or 9 th 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

51. EXAMPLES 3.95 + 2.879 + 213.6 = 220.429

52. EXAMPLE - Answer – 3.95 = has 2 significant figures after the decimal points – 2.879 has 3 significant figures after the decimal points – 213.6 has 1 significant figures after the decimal points

53. EXAMPLE – ANSWER CONT’ – Answer = 220.4 (1 significant figure)

54. ROUNDING RULES – Below 5 – round down – 5 or above – round up

55. EXACT VALUES has no uncertainty – example: Count value – number of items counted. There is no uncertainty – example: conversion value – relationship is defined. There is no uncertainty do not consider exact values when determining significant values in a calculated result

56. CALCULATOR BEWARE CALCULATOR does not account for significant figures!!!!

57. SCIENTIFIC NOTATIONS

58. SCIENTIFIC NOTATION Use to write very large number and very small number (more manageable)

59. PARTS Before the decimal point = 1 number After the decimal points = can be more than 1 numbers (can be optional) Exponential number = the number of places the decimal is moved

60. EXAMPLES Change to Scientific Notation – 1,234,400 = 1.234400 x 10 6 Or = 1.234400 E 6 Do the next 2 problems

61. EXAMPLES 2. 0.1234400 = 1.234400 x 10 -1 = 1.234400 E -1 3. 0.0000123 = 1.23 x 10 -5 = 1.234400 E -5

62. STANDARD NOTATION 2.4 x 10 5 = 240,000 Do the next 3 problems

63. EXAMPLES - Answer 7.8 x 10 7 = 78,000,000 9.789 E 3 = 9,789 1.2 x 10 -2 = 0.012

64. CALCULATION RULES - EXPONENTS Exponents are count values

65. CALCULATIONS RULES – ADD/SUBTRACT For addition and subtraction, all values must have the same exponents before calculations

66. CALCULATIONS RULES - MULTIPLICATION For multiplication, the first factors of the numbers are multiplied and the exponents of 10 are added

67. CALCULATION RULES - DIVISION For division, the first factors of the numbers are divided and the exponent of 10 in the denominator is subtracted from the exponent of 10 in the numerator

68. EXAMPLE - ADDITION Problem: 6.2 x 10 4 + 7.2 x 10 3

69. EXAMPLE – ADD cont’ Step 1: make sure all values have the same number of exponents 62 x 10 3 + 7.2 x 10 3

70. EXAMPLE – ADD cont’ Step 2: Add the factor 69.2 x 10 3

71. Step 3: put into correct scientific notation 6.92 x 10 4

72. Step 4: check for significant figures 6.9 x 10 4 (Significant rule: can only have as many as the least significant figure to the right of the decimal)

73. EXAMPLE - Multiplication Problem: (3.1 x 10 3 )(5.01 x 10 4 )

74. EXAMPLE – Multiplication (cont’) Step 1: multiple the factors and add the exponents (3.1 x 5.01) x 10 4+3 16 x 10 7

75. EXAMPLE – Multiplication (cont’) Step 2: Put into correct scientific notation format 1.6 x 10 8

76. EXAMPLE – Multiplication (cont’) Step 3: Check for significant figures 1.6 x 10 8 (Significant rule: can only have as many as the least significant figure)

77. EXAMPLE – Division Problem: (7.63 x 10 3 ) / (8.6203 x 10 4 )

78. EXAMPLE – Division (cont’) Step 1: Divide the factors and subtract the exponents (7.63 / 8.6203) x 10 3-4 0.885 x 10 -1

79. EXAMPLE – Division (cont’) Step 2: Put into correct scientific notation format 8.85 x 10 -2

80. EXAMPLE – Division (cont’) Step 3: Check for significant figures 8.85 x 10 -2 (Significant rule: can only have as many as the least significant figure)