Chem Unit1

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Chem Unit1

  1. 1. If you’ve ever used nonstick pans Thank a chemist
  2. 2. If you’ve ever used Velcro Thank a chemist
  3. 3. If you’ve ever used sweeteners Thank a chemist
  4. 4. If you’ve ever used Tylenol or Advil Thank a chemist
  5. 5. If you’ve ever used dyed clothing Thank a chemist
  6. 6. If you’ve ever used Nylon Thank a chemist
  7. 7. If you’ve ever used gasoline Thank a chemist
  8. 8. If you’ve ever had an MRI Thank a chemist
  9. 9. If you’ve ever baked a cake Thank a chemist
  10. 10. Physical vs. Chemical Change
  11. 11. Physical vs. Chemical Change
  12. 12. Physical vs. Chemical Change
  13. 13. Physical vs. Chemical Change
  14. 14. Physical vs. Chemical Change
  15. 15. Physical vs. Chemical Change
  16. 16. Physical vs. Chemical Change
  17. 17. Physical vs. Chemical Change
  18. 18. Describing Matter UNITS Quantity Symbol Unit Abbreviation Length L Meter m Mass m Kilogram kg Time t Second S Temperature T Kelvin K Amount of Substance n mole mol Electric current I Ampere A Luminous intensity Iv Candela cd
  19. 19. Measurements SI units Système Internationale des Unités
  20. 20. Describing Matter Prefixes Prefix Abbreviation Exponential multiplier Value example Yotta Y 10 24 septillion Zetta Z 10 21 sextillion Exa E 10 18 quintillion exabyte peta P 10 15 quadrillion tera T 10 12 trillion terabyte giga G 10 9 billion gigaHertz mega M 10 6 million Kilo K 10 3 thousand kilometer Base - 10 0 1
  21. 21. Describing Matter Prefixes Prefix Abbreviation Exponential multiplier Value example deci d 10 -1 tenth decibel centi c 10 -2 hundredth centimeter milli m 10 -3 thousandth milligram micro μ 10 -6 millionth microsecond nano n 10 -9 billionth nanometer pico p 10 -12 trillionth picoHertz femto f 10 -15 quadillionth femtosecond atto a 10 -18 quintillionth attometer zepto z 10 -21 Sextillionth
  22. 22. Measurements: Temperature Fahrenheit Celsius Kelvin 212° F 100°C 373 K Boiling point of water 32°F 0°C 273 K Freezing point of water -459.67°F -273°C 0 K Lowest possible temperature
  23. 23. Derived Units Volume
  24. 24. What is Matter? Anything that has mass and volume
  25. 25. Pure or Mixture?
  26. 26. Elements The Ancient Greeks recognized four different earthly elements
  27. 27. Elements Pure Substance that contains only one type of atom
  28. 28. Allotropes Different Molecular Form of Same Elemen; diamond and graphite
  29. 29. Compounds Pure substances made of more than one type of atom Cl H
  30. 30. Mixtures Heterogeneous Oil and water Milk
  31. 31. Mixtures Homogeneous Salt water Sugar water
  32. 32. Energy ENERGY is neither created nor destroyed .
  33. 33. Energy .
  34. 34. Heat Transfer . Energy transfer due to a difference in temperature
  35. 35. Measurements: Temperature Fahrenheit Celsius Kelvin 212° F 100°C 373 K Boiling point of water 32°F 0°C 273 K Freezing point of water -459.67°F -273°C 0 K Lowest possible temperature
  36. 36. Energy . Exothermic VS. Endothermic
  37. 37. Specific Heat Capacity Q = m x C p x Δ T
  38. 38. Specific Heat Capacity Specific Heat substance 4.18 J/gK water 0.9 J/gK Aluminum 0.126 J/gK Gold 0.51 J/gK Steel 2.9 J.gK Paraffin wax 1.0 J/gK Air
  39. 39. Accuracy vs. Precision
  40. 40. Accuracy How close is your measurement to the actual value??
  41. 41. Precision How close is your measurements to each other?
  42. 42. Significant Figures Any non-zero digit is Significant Any zero between non-zero digits is Significant All zeros to the left of the first non-zero digit are NOT significant Zeros that occur without a decimal point are NOT significant Zeros AFTER the decimal point are Significant

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