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Measurement

Measurement. Metric System Prefixes Conversions Scientific Notation Writing Calculating Significant Figures Definition Counting Calculating Dimensional Analysis. Metric System. AKA : International System (SI) 1960 : international agreement set up to use this system of units

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Measurement

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  1. Measurement • Metric System • Prefixes • Conversions • Scientific Notation • Writing • Calculating • Significant Figures • Definition • Counting • Calculating • Dimensional Analysis

  2. Metric System • AKA: International System (SI) • 1960: international agreement set up to use this system of units • Our “English system” is used within our boundaries, but we use the metric system in international trade. • 1999: NASA $125 million dollar mistake

  3. Metric System • Graphic organizer for prefixes • Mnemonic device: The good man King Henry died by drinking chocolate milk Monday night, poor fellow. • Prefixes • Powers of Ten • Place holders • Conversions • Temperature • Kelvin & Celsius Oops!

  4. Moving the Decimal T // G // M // k h D base d c m // µ // n // p // f

  5. Metric System Practice. • 33 km = _____________ mm • 175 nm = ____________ Dm • 0.5 GL = _____________ cL Evaluate. (True or false?) • 453 µg = 0.00453 hg • 16 Mbytes = 0.016 Gbytes

  6. 33 km = ________ mm iRespond Question Multiple Choice F A.) 0.000033 mm B.) 0.033 mm C.) 33,000 mm D.) 33,000,000 mm E.)

  7. 175 nm = _______ Dm iRespond Question Multiple Choice F A.) 0.000 000 175 B.) 0.0 000 000 175 C.) 1,750,000,000 D.) 1,750,000,000,000 E.)

  8. 0.5 GL = ______ cL iRespond Question Multiple Choice F A.) 5,000,000 cL B.) 50,000,000 cL C.) 50,000,000,000 cL D.) 0.000 000 000 005 cL E.)

  9. 453 micrograms = 0.00453 hectograms iRespond Question Multiple Choice F A.) True B.) False C.) D.) E.)

  10. 16Mbytes = 0.016Gbytes iRespond Question Multiple Choice F A.) True B.) False C.) D.) E.)

  11. Metric HW • Complete the 1-4 Practice Problems (1-10) tonight. • Metric System Quiz - Friday

  12. Sample Element Quiz Questions • Co _______________________ • Cr ________________________ • Sn _______________________ • Copper ____________________ • Sodium ____________________ • Iron ________________________

  13. 1-4 PP#1 Convert 83 cm into meters. iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 0.83;.83; B.) 0.83 meters C.) D.) E.)

  14. 1-4 PP #2 Convert 459 L into milliliters. iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 459000;; B.) 459,000 mL C.) D.) E.)

  15. 1-4 PP #3 Express 1123 pg in nanograms. iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 1.123;; B.) 1.123 ng C.) D.) E.)

  16. 1-4 PP #4 Express 0.032 m3 in liters. iRespond Question Fill-In F TRICKY! 1 cm3 = 1 mL Steps: Convert 0.032 m3 to cm3. This equals mL. Convert mL to L. TRY IT. A.) 32;; B.) C.) D.) E.)

  17. HOW TO CONVERT 0.032m3 to L • Convert 0.032 m3 to cm3. • Cubed conversions are different from simple meter to centimeter conversions. • Move the decimal 2 spaces to the right to go from meter to centimeter, correct? NOT SO FAST! • Move the decimal 2 spaces for EACH dimension. Since the unit is cubed, we’ll move the decimal 2 spaces to the right X 3! • 0.032 m3 = 32,000 cm3 • Convert mL to L. • Since cm3 = mL, 32,000cm3 = 32,000 mL. • Move the decimal 3 spaces to the left to go from milli to liters. • 32,000 mL = 32 L

  18. 1-4 PP #5 Express 2.5 mm in micrometers. iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 2500;; B.) 2,500 micrometers C.) D.) E.)

  19. 1-4 PP #6 Which is the longer amount of time: 1351 ps or 1.2 ns? iRespond Question Multiple Choice F A.) 1351 ps B.) 1.2 ns T // G // M // k h D base d c m // µ // n // p // f C.) D.) 1351 ps E.)

  20. 1-4 PP #7 Which is the larger pressure: 232.1 kPa or 125,487 Pa? iRespond Question Multiple Choice F A.) 232.1 kPa B.) 125,487 Pa C.) T // G // M // k h D base d c m // µ // n // p // f D.) 232.1 kPa E.)

  21. 1-4 PP #8 Which is the smaller mass: 285.0 cg or 23.78 dg? iRespond Question Multiple Choice F A.) 285.0 cg B.) 23.78 dg C.) T // G // M // k h D base d c m // µ // n // p // f D.) 23.78 dg E.)

  22. 1-4 PP #9 Which is shorter: 175.6 mm or 38.4 cm? iRespond Question Multiple Choice F A.) 175.6 mm B.) 38.4 cm C.) T // G // M // k h D base d c m // µ // n // p // f D.) 175.6 mm E.)

  23. 1-4 PP #10a 0.7824 mg to grams iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 0.0007824;.0007824; B.) 0.000 782 4 grams C.) D.) E.)

  24. 1-4 PP #10b 345,000 ng to grams iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 0.000345;.000345; B.) 0.000 345 000 grams C.) D.) E.)

  25. 1-4 PP #10c 0.00378 kg to grams iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 3.78;; B.) 3.78 grams C.) D.) E.)

  26. 1-4 PP #10d 34,981 micrograms to grams iRespond Question Fill-In F T // G // M // k h D base d c m // µ // n // p // f A.) 0.034981;.034981; B.) 0.034 981 grams C.) D.) E.)

  27. Scientific Notation • Lazy way to report really BIG or small numbers • Uses powers of ten rather than long strings of zeros • + powers mean BIG numbers • - powers mean small numbers

  28. Scientific Notation Expand or contract. • 250 = ______________ • 13,210,000 = ________ • 0.00150 = ___________ • 14 = ________________ • 0.00005 = ____________ • 1.6x10-4 = ____________ • 2.15x105 = ____________ • 1.0x101 = _____________ • 4.3x10-2 = ____________

  29. Scientific Notation Check your answers. • 250 = 2.5 x 102 • 13,210,000 = 1.321 x 107 • 0.00150 = 1.5 x 10-3 • 14 = 1.4 x 101 • 0.00005 = 5 x 10-5 • 1.6x10-4 = 0.00016 • 2.15x105 = 215,000 • 1.0x101 = 10 • 4.3x10-2 = 0.043

  30. Scientific Notation • Use the EE or EXP button to enter scientific notation. • NEVER use the ^ or x10. • Example: • Enter 6.02 x 1023 into your calculator. • Punch 6.02 as normal. • Then push the EE or EXP button. It replaces the x10. • Lastly, enter 23. • Summary: 6.02EXP23

  31. Scientific Notation • 6.02x1023 x 18.998 = ____________ • 5.6x10-8 / 3.2x10-3 = _____________ • 2.5x101 + 3.5x102 = _____________ • 8.45x10-3 x 2.1x101 = ____________ 1. 1.144x1025 2. 1.75x10-5 3. 375 4. 0.17745

  32. Density • Density is used to identify substances found in nature. • Density = mass/volume • Common units: g/mL or g/cm3 • mL measures the volume of a liquid. It is NOT a cubed unit. • cm3 measures the volume of a solid where length, width, and height were multiplied together.

  33. Density Example of Density: A rectangular sample is found. What is the density? 1. Measure the mass with a balance. 2. Measure the volume with a ruler since it has a normal (regular) shape. 3. Calculate.

  34. Density Another Example of Density: A strangely shaped sample is found. What is the density? 1. Measure the mass with a balance. 2. Measure the volume with a graduated cylinder using the water displacement method. 3. Calculate.

  35. Density A truth about the density of water: • A 1 cm3box will hold EXACTLY 1 mL of water, and the 1 mL of water will weigh EXACTLY 1 gram! • Therefore, 1 cm3 = 1 mL = 1 gram. • You are going to have a chance to prove this in your lab today using a small blue solid (not hollow) cube.

  36. Density Density of a Metal Cube Lab Goals: Test the 1 mL = 1 cm3 rule and determine the type of metal that makes up your group’s cube using density. Steps: Follow the lab steps carefully, and be sure to record any measurements on your paper. You’ll have a very small lab report due on Monday. The specifics of the report are described on your lab handout. If you get stuck, send a group rep to Mrs. Tarvin. NOTE: The copy of the lab at your station should not leave the station. A copy of the lab is on the blog for your use at home.

  37. iRespond Question Multiple Choice F A student determines that a piece of an unknown material has a mass of 5.854 g and a volume of 7.57 cm3. What is the density of the material? (Density Practice Problems #1) A.) 0.773 g/cm3 B.) 1.29 g/cm3 C.) 44.4 g/cm3 D.) none of these E.)

  38. A student determines that a piece of an unknown material has a mass of 5.854 g and a volume of 7.57 cm3. What is the density of the material? (Density Practice Problems #1) Steps: Density = mass / volume Mass = 5.854 grams; Volume = 7.57 cm3 Notice that the units will be grams/cm3. The problem doesn’t specify certain units, so I can use these. 5.854 gram/7.57 cm3 = 0.773 g/cm3

  39. iRespond Question Multiple Choice F Iron has a known density of 7.87 g/cm3. What would be the mass of a 2.5 dm3 piece of iron? Density Practice Problem #2 A.) 1.9675 grams B.) 19.675 grams C.) 196.75 grams D.) 19, 675 grams E.)

  40. Iron has a known density of 7.87 g/cm3. What would be the mass of a 2.5 dm3 piece of iron? Density Practice Problem #2 Steps: Density = mass / volume Density = 7.87 g/cm3; Since the units are given for density, I am stuck with them. I cannot plug in a mass unless it is in grams. I cannot plug in a volume unless it is in cm3. Convert 2.5 dm3 to cm3. Move the decimal to the right THREE spaces. 7.87g/cm3 = mass / 2500 cm3 ; mass = 19,675 grams

  41. iRespond Question Multiple Choice F Mercury has a density of 13.5 g/cm3. How much space (in mm3) would 50.0 g of mercury occupy? Density Practice Problem #3 A.) 3.70 mm3 B.) 37.0 mm3 C.) 370.0 mm3 D.) 3,700 mm3 E.)

  42. Mercury has a density of 13.5 g/cm3. How much space (in mm3) would 50.0 g of mercury occupy? Density Practice Problem #3 Steps: Density = mass / volume Density = 13.5 g/cm3; The mass MUST be in grams, and the volume MUST be in cm3. 13.5 g/cm3 = 50.0 g / volume; REMEMBER – The volume will be in cm3 because of the density units. ALGEBRA HELPFUL HINT: Put a 1 under the density & cross multiply. 13.5 g/cm3 = 50.0 grams 1 volume (13.5 g/cm3)(volume) = (50.0 grams)(1) (13.5 g/cm3) (13.5 g/cm3) volume = 3.70 cm3 = 3,700 mm3

  43. iRespond Question Multiple Choice F A sample has a mass of 1.02g and a volume of 1.35cm3, what is the density of the nickel? Density Practice Problems #4 A.) 0.756 g/cm3 B.) 1.38 g/cm3 C.) 1.32 g/cm3 D.) 7.56 g/cm3 E.)

  44. A sample has a mass of 1.02g and a volume of 1.35cm3, what is the density of the nickel? Density Practice Problems #4 No conversions needed. 3 sig figs If you are not setting up the algebra, Then you are setting up for a mistake.

  45. iRespond Question Multiple Choice F What is the density of a material if its mass 2.02g and its volume is 0.500cm3? Density Practice Problem #5 A.) 1.01 g/cm3 B.) 4.04 g/cm3 C.) 0.248 g/cm3 D.) 4.48 g/cm3 E.)

  46. What is the density of a material if its mass 2.02g and its volume is 0.500cm3? Density Practice Problem #5 No conversions needed. 3 sig figs If you are not setting up the algebra, Then you are setting up for a mistake.

  47. iRespond Question Multiple Choice F Pure gold has a density of 19.32 g/cm3. How large (in dm3) would a piece of gold be if it had a mass of 318.97 g? Density Practice Problems #6 A.) 16.51 dm3 B.) 1.651 dm3 C.) 0.1651 dm3 D.) 0.01651 dm3 E.)

  48. Pure gold has a density of 19.32 g/cm3. How large (in dm3) would a piece of gold be if it had a mass of 318.97 g? Density P P #6 Plugging into equation will give cm3. Convert to dm3 at the end. If you are not setting up the algebra, Then you are setting up for a mistake. 4 sig figs

  49. iRespond Question Multiple Choice F How many cm3 would a 55.932 g sample of copper occupy if it has a density of 8.92 g/cm3? Density Practice Problems #7 A.) 0.159 cm3 B.) 499 cm3 C.) 6.27 cm3 D.) 48.9 cm3 E.)

  50. How many cm3 would a 55.932 g sample of copper occupy if it has a density of 8.92 g/cm3? Density PP #7 Plugging into equation will give cm3. If you are not setting up the algebra, Then you are setting up for a mistake. 4 sig figs

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