1. Ionic Equations Most ionic compound dissociate (or break apart) when dissolved in water to form its component ions For example: NaCl (aq) really looks like Na + (aq) and Cl - (aq)

2. Soluble Vs. Precipitate Soluble means that the compound breaks down into its ions in water Ex) NaCl is soluble so it forms Na + and Cl - Insoluble means that the compound doesn’t break down in water

3. Precipitate Reactions In double replacement reactions, often one of the product will be insoluble The insoluble product is referred to as a precipitate.

4. AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) What happens when you put AgNO 3 and NaCl in water?

5. AgNO 3 NaCl

6. AgNO 3 NaCl

7. AgNO 3 NaCl

8. AgNO 3 NaCl

9. AgNO 3 NaCl

10. AgNO 3 NaCl

11. AgNO 3 NaCl

12. Ag NO 3 Na Cl

13. Ag + NO 3 - Na + Cl -

14. Ag + NO 3 - Na + Cl -

15. Ag + NO 3 - Na + Cl -

16. Ag + NO 3 - Na + Cl -

17. Ag + NO 3 - Na + Cl -

18. Ag + NO 3 - Na + Cl -

19. Ag + NO 3 - Na + Cl -

20. Ag + NO 3 - Na + Cl -

21. Ag + NO 3 - Na + Cl -

22. Ag + NO 3 - Na + Cl -

23. Ag + NO 3 - Na + Cl -

24. Ag + NO 3 - Na + Cl -

25. Ag + NO 3 - Na + Cl -

26. AgCl NO 3 - Na +

27. AgCl NO 3 - Na +

28. AgCl NO 3 - Na +

29. AgCl NO 3 - Na + AgCl(s) precipitate

30. AgCl NO 3 - Na + AgCl(s) precipitate

31. AgCl NO 3 - Na +

32. AgCl NO 3 - Na +

33. AgCl NO 3 - Na +

34. AgCl NO 3 - Na +

35. AgCl NO 3 - Na +

36. AgCl NO 3 - Na +

37. AgCl NO 3 - Na +

38. AgCl NO 3 - Na +

39. AgCl NO 3 - Na +

40. AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaClAgNO 3 NaCl AgNO 3 NaCl

41. AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaClAgNO 3 NaCl AgNO 3 NaCl

42. AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaClAgNO 3 NaCl AgNO 3 NaCl

43. Ag + NO 3 - Na + Cl - AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl AgNO 3 NaCl

44. Ag + NO 3 - Na + Cl - NaCl AgNO 3 NaCl AgNO 3 NaClAgNO 3 Ag + NO 3 - Na + Cl - Ag + NO 3 - Na + Cl - AgCl

45. Ag + NO 3 - Na + Cl - Ag + NO 3 - Na + Cl - Ag + NO 3 - Na + Cl - Ag + NO 3 - Na + Cl - Ag + NO 3 - Na + Cl - Ag + NO 3 - Na + Cl - Ag + AgCl Ag + Cl - Ag +

46. NO 3 - Na + Cl - NO 3 - Na + Ag + NO 3 - Na + Ag + NO 3 - Na + Cl - Na + NO 3 - Na + Cl - Ag + NO 3 - Na + NO 3 - Na + Cl - NO 3 - Na + AgCl Ag + Cl - Ag + Cl - Ag + Cl - Ag +

47. NO 3 - Na + NO 3 - Na + Ag + NO 3 - Na + Ag + NO 3 - Na + Cl - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + Cl - NO 3 - Na + Ag + Cl - Ag + Cl -

48. NO 3 - Na + NO 3 - Na + Ag + NO 3 - Na + Ag + NO 3 - Na + Cl - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + Cl - NO 3 - Na +

49. NO 3 - Na + NO 3 - Na + Ag + NO 3 - Na + Ag + NO 3 - Na + Cl - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + Cl - NO 3 - Na +

50. NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na +

51. NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + AgCl(s)

52. NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + AgCl(s)

53. NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + NO 3 - Na + AgCl(s)

54. Ionic Equations Continued To write a Complete Ionic Equation: Write the aqueous substances as ions (leave any substances in gas, liquids, & solids alone) Example: AgNO 3 (aq) + NaCl (aq)  AgCl (s) + NaNO 3 (aq)

55. Spectator Ions Spectator Ions-Ions that are not directly involved in a reaction Spectator ions show up on both sides of the equation Spectator Ions cancel out

56. NET Ionic Equations Net Ionic Equation-Indicate the particles that actually take part in a reaction The Net Ionic Equation does NOT include spectator ions Net Ionic Equations must be balanced according to atoms and charge

57. AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) ionic equation

58. AgNO 3 NaCl

59. Ag NO 3 Na Cl

60. Ag + NO 3 - Na + Cl -

61. Ag + NO 3 - Na + Cl -

62. Ag + NO 3 - Na + Cl -

63. Ag + NO 3 - Na + Cl -

64. Ag + NO 3 - Na + Cl -

65. Ag + NO 3 - Na + Cl -

66. Ag + NO 3 - Na + Cl -

67. Ag + NO 3 - Na + Cl -

68. Ag + NO 3 - Na + Cl -

69. Ag + NO 3 - Na + Cl -

70. Ag + NO 3 - Na + Cl -

71. Ag + NO 3 - Na + Cl -

72. Ag + Cl - NO 3 - Na + Reaction

73. NO 3 - Na + AgCl Reaction

74. NO 3 - Na + AgCl

75. NO 3 - Na + No Reaction

76. AgCl NO 3 - Na + No Reaction

77. AgCl NO 3 - Na + No Reaction

78. AgCl NO 3 - Na +

79. AgCl NO 3 - Na +

80. AgCl NO 3 - Na +

81. AgCl NO 3 - Na +

82. AgCl NO 3 - Na +

83. AgCl NO 3 - Na + These ions do not participate in the reaction. They are called SPECTATOR IONS

84. Ag + Cl -

85. Ag + Cl -

86. Ag + Cl -

87. Ag + Cl -

88. Ag + Cl -

89. Ag + Cl -

90. Ag + Cl -

91. Ag + Cl -

92. AgCl

99. The net ionic equation is constructed from the ionic equation:

104. No 3 - and Na + are not participating in the reaction

105. net ionic equation Ag + ( aq ) + Cl - ( aq )

106. net ionic equation Ag + ( aq ) + Cl - ( aq ) Ag + and Cl - are reacting to form

107. net ionic equation Ag + ( aq ) + Cl - ( aq ) Ag + and Cl - are reacting to form

108. net ionic equation