1 / 67

Drill: Name & describe each of the 7 crystal structures

Drill: Name & describe each of the 7 crystal structures. Drill: Draw LDDs for:. BF 3 NH 3 BeCl 3 C 3 H 6 H 3 PO 4 H 2 CO 3. Drill: Draw LDDs for:. C 6 H 8. Drill: Draw LDD for:. C 3 H 5 NO. CHM II. Test Friday. CHM II HW. Read: Chapter 14 Work Problems 25 & 29 on page 585.

rudyard-mathis
Télécharger la présentation

Drill: Name & describe each of the 7 crystal structures

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Drill: Name & describe each of the 7 crystal structures

  2. Drill: Draw LDDs for: BF3 NH3 BeCl3 C3H6 H3PO4 H2CO3

  3. Drill: Draw LDDs for: C6H8

  4. Drill: Draw LDD for: C3H5NO

  5. CHM II • Test Friday

  6. CHM II HW • Read: Chapter 14 • Work Problems 25 & 29 on page 585

  7. Solutions

  8. Solution • Homogeneous mixture made up of at least one solute dissolved in the solvent

  9. Solute • Substance being dissolved • Portion in lesser molar amount

  10. Solvent • Substance doing the dissolving • Portion in greatest molar amount

  11. Colloid • Slightly larger particles • Light passes & particles stay suspended

  12. Suspension • Even larger particles • Particles block or reflect light

  13. Tyndall Effect • Because light reflects off suspended particles, the light ray can be seen from the side

  14. Size Comparison • Solution < Colloid • Colloid < Suspension

  15. Soluble • When one substance (solute) dissolves in another (solvent)

  16. Solubility • The amount of one substance (solute) dissolved in another (solvent)

  17. Concentration • The amount of solute dissolved into solution

  18. ConcentratedSolution • A solution with a relatively large amount of solute dissolved

  19. Dilute Solution • A solution with a relatively small amount of solute dissolved

  20. Saturated Solution • A solution with the maximum amount of solute dissolved in the solution

  21. Unsaturated Solution • A solution with less than the maximum amount of solute dissolved in solution

  22. Supersaturated Solution • A solution with greater than the maximum amount of solute dissolved in solution

  23. Solution Measures • Concentration • Molarity • Molality • Mole Fraction

  24. Percent Solution • Mass of one portion per the total mass, all times 100 % • %soln = ma/mtotal x 100 %

  25. Drill: • Define & give units for: • Molarity • Molality • Mole Fraction

  26. Molarity • Moles of solute per liter of solution • M = molessolute/Lsoln

  27. Molality • Moles of solute per kilogram of solvent • mo = molessolute/kgsolvent

  28. Mole Fraction • Moles of one portion per total number of moles in the solution • X = molesa/molessoln

  29. Calculate the molarity of a 250 mL solution containing 5.0 g NaOH dissolved in water

  30. Calculate the molality of 69 g of C2H5OH dissolved in 500.0 mL of water

  31. Calculate the mole fraction of each portion when 92 g of C2H5OH dissolved in 144 mL of water

  32. Drill: • Calculate the mass of KI required to make 250 mL of 0.500 M KI.

  33. Review DrillReview HW

  34. Calculate the molality & mole fraction of a solution containing 46 g of C2H5OH dissolved in 1782 mL of water

  35. Chm II HW Problems: 31 & 38 Page: 585 & 586

  36. AP Chm HW Problems: 31 & 35 Page: 298

  37. Colligative Properties • Properties dependent only on the concentration of particles in solution

  38. Examples • Vapor pressure • Boiling & Freezing points • Osmotic pressure

  39. Vapor Pressure • VPsolution = (VPsolvent)(Xsolvent) • X = mole fraction • VP = vapor pressure

  40. Boiling & Freezing DT = imoK DT = change in BP or FP i = ionic activity K = BP or FP constant

  41. Osmotic Pressure p = iMRT p = osmotic pressure i = ionic activity M = Molarity

  42. Calculate the vapor pressure of a solution containing 150 g C5H10O5 in 162 mL of water at 30oC

  43. Drill: • Calculate the VP of a solution containing 36 % m/m glucose (C6H12O6) in water at 29oC: • (VPwater = 30.0 mm Hg)

  44. Calculate BP & FP of 60.0 g of NaOH in 250 mL waterKBP = 0.512oC/moKFP = -1.86oC/mo

  45. Calculate the osmotic pressure of a solution containing 12 g of NaOH dissolved in 250 mL solution at 27oC

  46. Chm II Homework: Problems: 47 & 87 Page: 585 - 587

  47. AP Chm HW: Problems: 31, 35, & 39 Page: 298

  48. Calculate the vapor pressure of a solution containing 120 g C3H7OH in 144 mL of water at its BP.

More Related