2. Click Once to Begin JEOPARDY! Chemistry Final Review Chapters 6.1-6.4 and 6.7 Juliann Frenette

3. JEOPARDY! 100 200 300 400 500 Vocab.pHSolublity Vapor Pressure Boiling and Freezing Misc.

4. Daily Double Graphic and Sound Effect! DO NOT DELETE THIS SLIDE! Deleting it may cause the game links to work improperly. This slide is hidden during the game, and WILL not appear. In slide view mode, copy the above (red) graphic (click once to select; right click the border and choose “copy”). Locate the answer slide which you want to be the daily double Right-click and choose “paste”. If necessary, reposition the graphic so that it does not cover the answer text. Daily Double!!!

5. Define strong and weak electrolytes.

6. Strong electrolytes are ionic compounds that almost completely dissociate into ions when dissolved in water. Weak electrolytes only partially dissociate.

7. Define a solution, solute and solvent.

8. A solution is composed of the substance that is dissolved. The solute is what is being dissolved. The solvent is the liquid in which the solute is dissolved.

9. Write the equations for the 3 main ways to express concentration: %W/V, molarity and molality.

10. %W/V= (mass solute/volume)(100) Molarity= moles of solute/L of solution Molality= moles of solute/kg of solvent

11. State the differences between unsaturated, saturated and supersaturated.

12. Unsaturated solutions have room to hold more solute particles and saturated solutions are holding all the solute particles it can. Supersaturated one are created by heating to increase the amount of solute in the solution then cooled down to a temp. that ordinarily wouln’t allow the solution to hold that much solute

13. Explain how well strong and weak electrolytes can conduct electricity and why that is.

14. Strong electrolytes conduct electricity better than weak ones because there is a greater sea of electrons when strong electrolytes are dissolved in water

15. What is the equation used to calculate pH?

16. pH= -log[H+ or H30+]

17. The normal pH of human blood is 7.4. Human blood is…

18. Slightly basic

19. What is the relationship between the concentration of hydronium ions and pH?

20. As the concentration of the hydronium ions increases, the pH decreases.

21. Strong acids are to strong ________, as weak acids are to weak _________.

22. Electrolytes

23. What is the [H+] of a solution whose pOH = 2.86 ?

24. 7.24 x 10-12 M

25. When does a precipitate form?

26. When two compounds mix to form a product that is insoluble

27. True or false? All acetates are soluble

28. True

29. Which of the following salts are insoluble? A: LiCl B: NaCl C: AgCl D: KCl

30. AgCl

31. Which is always soluble: Ammonium or Ammonia?

32. Ammonium

33. 2 KCl(aq) + Pb(NO3)2(aq) → 2 KNO3(?) + PbCl2(?)

34. 2 KCl(aq) + Pb(NO3)2(aq) → 2 KNO3(aq) + PbCl2(s)

35. Define vapor pressure.

36. The pressure created by liquid molecules with enough energy to break them free from the surface and become gas molecules.

37. What is the relationship between vapor pressure and temperature?

38. As temp. increases, the vapor pressure of a liquid increases.

39. What does vapor pressure have to do with boiling point?

40. The boiling point is when the vapor pressure of the liquid and the atmospheric pressure of he surroundings are equal.

41. A solution always has a vapor pressure that is ______ than that of the original solvent. Why?

42. It’s less than the original solvent because there are fewer solvent molecules on the surface available for evaporation.

43. Connect all these terms in a sentence: average kinetic energy, temperature, imfs and vapor.

44. When temp. increases, so does the average kinetic energy. When the average increases, the # of molecules that have the min. energy needed the break the imfs of the liquid and become vapor also increases.

45. What are the equations to calculate boiling point and freezing point and what do the variable stand for?

46. Boiling point: T=KB(M) where KB is the boiling point elevation constant and M is molarity. Freezing point: T=KF(M) where KF is the freezing point depression constant and M is molarity.

47. A substance is at its freezing point when…

48. The solid phase and liquid phase are in equilibrium.

49. _______ always have a higher boiling point than a pure ______.

50. Solutions always have a higher boiling point than a pure solvent.

51. What is the normal boiling and freezing point of water in K and C?

52. Tb= 373.15 K or 100C TF= 273.15 K or 0C

53. Explain what happens at the molecular level when a substance freezes. Daily Double!!!

54. At a lower temp., the solid molecules are leaving the solid phase at a slower rate which can then be matched by the liquid molecules joining the solid.

55. What is the pH if the pOH is 4?

56. 10

57. If 62.0 g of ZnCl2 is added to 0.100 L of water, what is the molarity of the solution (with correct significant digits)?

58. 4.45 M

59. Given the Kf for water is 1.86°C/m, what will be the freezing point of a 2.2 m solution of glucose?

60. -4.09 degrees Celsius

61. For a 0.262M solution of sucrose in water with a KB of.512 degrees Celsius/M calculate the boiling point of the solution.

62. .134 degrees Celsius

63. If the KB for water at sea level is.52 degrees Celsius/M, what is the molarity of it when the boiling point is raised 100 degrees Kelvin?

64. .4 M

65. Final Jeopardy

66. Click Once to Begin Recite all the Solubility Rules from memory!