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You can do it.

5. You can do it. Chapter 1 Matter and Measurement. States of Matter. Solid. Liquid. Gas. Plasma. Matter. Pure substances (homogeneous composition). Mixtures of two or more substances. Elements. Compounds. Solutions (homogeneous composition – one phase).

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  1. 5

  2. You can do it.

  3. Chapter 1Matter and Measurement

  4. States of Matter

  5. Solid

  6. Liquid

  7. Gas

  8. Plasma

  9. Matter Pure substances (homogeneous composition) Mixtures of two or more substances Elements Compounds Solutions (homogeneous composition – one phase) Heterogeneous mixtures (two or more phases) Figure 3.2 (page 48)

  10. Classifying Substances

  11. Mixtures • Homogeneous • Heterogeneous

  12. Pure substance • A particular kind of matter with a definite, fixed composition • Elements • Compounds

  13. Compounds • Two or more elements • New • Definite • Can be

  14. Gatorade Caesar salad Water Coffee An iron nail Air Milk How would you classify?

  15. Methods of Separation Do not cause chemical changes

  16. Filtration • Used for • Gravity • Vacuum

  17. Sublimation

  18. Evaporation • Solutions…

  19. Distillation • Relies on

  20. Chromatography • Relies on

  21. Decantation

  22. Crystallization

  23. 5

  24. The Metric SystemThe International System of Units • Standards of measurement • Base units (7) – see Table 1.4 pg 14 • MASS: • LENGTH: • TIME: • COUNT, QUANTITY: • TEMPERATURE: • ELECTRIC CURRENT: • LUMINOUS INSTENSITY:

  25. The Metric System • Derived Units: • AREA: • VOLUME: • ENERGY: • FORCE: • PRESSURE: • POWER: • VOLTAGE: • FREQUENCY: • ELECTRIC CHARGE:

  26. Common ratio used in chemistry Physical property of a substance D = SI units: kg/m3 Solid g/cm3 Liquid g/mL Gas g/L Density Can change due to temperature and/or pressure changes

  27. Density • Find the density of a piece of metal with a volume of 2.7 cm3 and a mass of 10.8 g. 2. Determine the mass of an object with a density of 0.24 g/cm3 and a volume of 2 cm3.

  28. The Metric System • Metric Prefixes – make base unit larger or smaller • Table 1.5 – pg 14 • Based on 10 • Math method vs. “Stairs”

  29. Conversion Practice • Convert a volume of 12 microliters into centiliters • Express a distance of 15 meters in kilometers • Convert 83 cm into meters • Which is the longer amount of time, 1351 ps or 1.2 ns? • Convert 16 dL into L

  30. Uncertainty in Measurement • Why are digits in measurements uncertain? • Instruments never completely free of flaws • Always involves estimation • Choose the right instrument for the job • May be estimated for you (electronic scales) • Scale is marked but you estimate the in-between

  31. Uncertainty in Measurement • Precision: getting the same result again and again under same conditions • Accuracy: close to accepted value

  32. Significant Digits • All digits known with certainty plus one final digit which is uncertain (or estimated) • All non-zeros • A zero is significant when : • It is • It is • A zero is not significant when: • It is • It is

  33. Significant Digits - PRACTICE How many significant digits? • 54.23 • 23.00005 • 0.0004 • 35000 • 0.000504 • 45.623200 • 5,000,000 • 4,000,000.1

  34. Significant Digits - Calculations • Addition and Subtraction • Round answer to have final digit in the SAME PLACE as the last digit in the LEAST ACCURATE MEASUREMENT • 1.21 + 5.002 + 10. = • 34.5 + 12.45 + 23.0505 = • 186.31 + 11.1 = • 12.0231 + 3.86 = • 0.100012 + 120. = • 1200 + 12 + 15 + 0.5 =

  35. Significant Digits - Calculations • Multiplication and Division • The answer has as many sig figs as the number with the fewest sig figs • 14.8 x 3.1 = • 18.2 x 3.0 = • 52/1.5 = • 321.868783 x 1 = • 2400 x 2.123 = • 15000/12.354 =

  36. Scientific Notation • Convenient way of writing very large or very small numbers and showing only significant figures • Number between 1 & 10 with a power of ten • 5120 becomes 5.12 x 103 • Move decimal point in original number to make number 1-10 • Move left = +; move right = -

  37. Scientific Notation Practice • 123,000 = • 0.000045 = • 23.45 = • 0.0000000003 = • 1,000,000 =

  38. Scientific Notation • Math with: • Use the EE or EXP button on your calculator. • For example: • (1.25 x 105) (5.25 x 102) • Keystrokes are: • Or:

  39. Types of Measurements • Mass – • Expressed in • Does • Weight – • Expressed in same units

  40. Types of Measurements • Volume – • Cubic • Many instruments to measure • Temperature – • Kelvin • Degrees Celsius • Degress Farenheit

  41. Conversion Factors • Enable movement between metric system and “English” system • See back cover of book and Appendix III • Common conversions you should memorize • 1 inch = 2.54 cm • 1 mile = 1.609 km • 1 kg = 2.20 pounds • 1 mL = 1 cm3 • 0 K = -273.15 0C • 0F = 1.8(0C) + 32

  42. 5

  43. Dimensional Analysis(Problem Solving) • Remember: ALWAYS use UNITS OF MEASUREMENT in your work!!! • A technique of converting between units • Same system (metrics) • Different systems (inches to meters) • Chemical equations….later chapters…

  44. Dimensional Analysis(Problem Solving) • Conversion Factors: ratio derived from the equality between 2 different units 3 feet = 1 1 dollar = 1 1 yard 4 quarters • CF can be written either way 1 minute = 1 60 seconds = 1 60 seconds 1 minute

  45. The “t” method Dimensional Analysis(Problem Solving) unit given unit wanted = unit wanted unit given Conversion Factor Example: How many liters are in 125.6 gallons?

  46. Dimensional Analysis(Problem Solving) Dimensional Analysis(Problem Solving) How many seconds are in 4.15 hours? If a student needs 1.5 mL of water, how many cups does he need?

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