1. Starter S-105 1.How many grams of copper (II) chloride are in 3.83 x 10 21 formula units?

2. Chemical Reactions Chapter 11

3. 11.1 Describing Chemical Reactions Chapter 11

4. Writing Chemical Reactions Word Equations – gives the names of compounds and elements in the equation reactants  products Reactants – compounds and elements before the reaction Products – compounds and elements after the reaction 11.1 Describing Chemical Reactions

5. Different compounds, or elements are separated by a plus sign Copper + Oxygen  Copper (II) Oxide These are often converted from descriptions of the reaction 11.1 Describing Chemical Reactions

6. When antiseptic hydrogen peroxide is put in an open cut bubbles of oxygen form rapidly. Water is also produced. Reaction – reactants hydrogen peroxide 11.1 Describing Chemical Reactions

7. When antiseptic hydrogen peroxide in an open cut bubbles of oxygen from rapidly. Water is also produced. Reaction – products hydrogen peroxide 11.1 Describing Chemical Reactions

8. When antiseptic hydrogen peroxide in an open cut bubbles of oxygen form rapidly. Water is also produced. Reaction – products hydrogen peroxide  oxygen + water 11.1 Describing Chemical Reactions

9. When a stove burner is lit, methane gas reacts with oxygen to form carbon dioxide and water. Reaction – reactants methane gas + oxygen 11.1 Describing Chemical Reactions

10. When a stove burner is lit, methane gas reacts with oxygen to form carbon dioxide and water. Reaction – products methane gas + oxygen 11.1 Describing Chemical Reactions

11. When a stove burner is lit, methane gas reacts with oxygen to form carbon dioxide and water. Reaction – products methane gas + oxygen  carbon dioxide + water 11.1 Describing Chemical Reactions

12. Chemical Equations – replace the names of compounds and elements with the chemical formula hydrogen peroxide  oxygen + water H 2 O 2  O 2 + H 2 O Remember diatomic elements 11.1 Describing Chemical Reactions

13. methane gas + oxygen  carbon dioxide + water CH 4 + O 2  CO 2 + H 2 O 11.1 Describing Chemical Reactions

14. Usually the state of each compound or element is given beside the formula CH 4(g) + O 2(g)  CO 2(g) + H 2 O (g) Solid(s) Liquid(l) Gas(g) Aqueous(aq) 11.1 Describing Chemical Reactions

15. Starter S-106 When solutions of potassium iodide and lead (II) nitrate are mixed in a beaker, a brilliant yellow solid is formed. This solid when analyzed turns out to be lead (II) iodide. Further analysis shows that potassium nitrate is now dissolved in the water. A.Write the word equation. B.Write the chemical equation

16. Balancing Chemical Equations – both sides of a chemical equation have the same number of each atom Mass is conserved 11.1 Describing Chemical Reactions Balancing Demo

17. Example Al +O 2  Al 2 O 3 1. Write elements on each side and how many of each are present 11.1 Describing Chemical Reactions

18. Example Al +O 2  Al 2 O 3 Al – 1Al – 2 O – 2O – 3 2. Add one element at a time to the side that doesn’t have enough 11.1 Describing Chemical Reactions

19. Al Al +O 2  Al 2 O 3Al – 2 O – 2O – 3 11.1 Describing Chemical Reactions

20. AlO 2 Al +O 2  Al 2 O 3Al – 2 O – 4O – 3 11.1 Describing Chemical Reactions

21. AlO 2 Al 2 O 3 Al +O 2  Al 2 O 3 Al – 2Al – 4 O – 4O – 6 11.1 Describing Chemical Reactions

22. Al,Al,Al O 2 Al 2 O 3 Al +O 2  Al 2 O 3Al – 4 O – 4O – 6 11.1 Describing Chemical Reactions

23. Al,Al,Al O 2,O 2 Al 2 O 3 Al +O 2  Al 2 O 3Al – 4O – 6 Balanced 3. Count the number of each compound or element – write a coefficient for each 11.1 Describing Chemical Reactions

24. 4Al + 3O 2  2Al 2 O 3 11.1 Describing Chemical Reactions

25. Balance the following equations A.Cu + AgNO 3  Cu(NO 3 ) 2 + Ag 11.1 Describing Chemical Reactions

26. Balance the following equations A.Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag B.FeCl 3 + NaOH  Fe(OH) 3 + NaCl 11.1 Describing Chemical Reactions

27. Balance the following equations A.Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag B.FeCl 3 + 3NaOH  Fe(OH) 3 + 3NaCl C.CS 2 + Cl 2  CCl 4 + S 2 Cl 2 11.1 Describing Chemical Reactions

28. Balance the following equations A.Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag B.FeCl 3 + 3NaOH  Fe(OH) 3 + 3NaCl C.CS 2 + 3Cl 2  CCl 4 + S 2 Cl 2 D.AgNO 3 + H 2 S  Ag 2 S + HNO 3 11.1 Describing Chemical Reactions

29. Balance the following equations A.Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag B.FeCl 3 + 3NaOH  Fe(OH) 3 + 3NaCl C.CS 2 + 3Cl 2  CCl 4 + S 2 Cl 2 D. 2AgNO 3 + H 2 S  Ag 2 S + 2HNO 3 E.Zn(OH) 2 + H 3 PO 4  Zn 3 (PO 4 ) 2 + H 2 O 11.1 Describing Chemical Reactions

30. Balance the following equations A.Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag B.FeCl 3 + 3NaOH  Fe(OH) 3 + 3NaCl C.CS 2 + 3Cl 2  CCl 4 + S 2 Cl 2 D. 2AgNO 3 + H 2 S  Ag 2 S + 2HNO 3 E. 3Zn(OH) 2 + 2H 3 PO 4  Zn 3 (PO 4 ) 2 + 6H 2 O F.Fe 2 O 3 + H 2  Fe + H 2 O 11.1 Describing Chemical Reactions

31. Balance the following equations A.Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag B.FeCl 3 + 3NaOH  Fe(OH) 3 + 3NaCl C.CS 2 + 3Cl 2  CCl 4 + S 2 Cl 2 D. 2AgNO 3 + H 2 S  Ag 2 S + 2HNO 3 E. 3Zn(OH) 2 + 2H 3 PO 4  Zn 3 (PO 4 ) 2 + 6H 2 O F.Fe 2 O 3 + 3H 2  2Fe + 3H 2 O 11.1 Describing Chemical Reactions

32. Starter S-107 1.Balance C 6 H 6 + O 2  CO 2 + H 2 O CH 3 CH 2 OH + O 2  CO 2 + H 2 O

33. 11.2 Types of Chemical Reactions Chapter 11

34. 11.2 Type of Chemical Reactions You will need to know and predict the product for 6 types of chemical reactions 1.Synthesis Form Example 11.2 Types of Chemical Reactions Synthesis

35. 11.2 Type of Chemical Reactions 2. Decomposition Form Example 11.2 Types of Chemical Reactions Decomposition

36. 11.2 Type of Chemical Reactions 3. Single Replacement Reaction Form Example For metals, the reactions occurs if the metal is more reactive than the the one in the compound 11.2 Types of Chemical Reactions Single

37. Activity Series for Single Replacement Reactions

38. 11.2 Type of Chemical Reactions 4. Double Replacement Reaction Form Example 11.2 Types of Chemical Reactions Double

39. 11.2 Type of Chemical Reactions 5. Combustion Reaction Form Example 11.2 Types of Chemical Reactions Combustion

40. 11.2 Type of Chemical Reactions 6. Acid/Base Neutralization Reaction Form Example The substance AB is called a Chemical Salt 11.2 Types of Chemical Reactions Acid Base

41. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reactions are predicted based on recognizing forms.

42. Starter S-110 What type of reaction is this? CaCl 2 + Pb(NO 3 ) 2  Write the complete balanced equation

43. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction AgNO 3 + NaCl  Type: Double Replacement Products: AgNO 3 + NaCl  AgCl + NaNO 3 Balanced: AgNO 3 + NaCl  AgCl + NaNO 3

44. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction Pb + AgNO 3  Type: Single Replacement Products: Pb + AgNO 3  Ag + Pb(NO 3 ) 2 Balanced: Pb + 2AgNO 3  2Ag + Pb(NO 3 ) 2

45. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction FeCl 3 + KOH  Type: Double Replacement Products: FeCl 3 + KOH  Fe(OH) 3 + KCl Balanced: FeCl 3 + 3KOH  Fe(OH) 3 + 3KCl

46. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction NaOH + H 2 SO 4  Type: Acid Base Neutralization Products: NaOH + H 2 SO 4  Na 2 SO 4 + H 2 O Balanced: 2NaOH + H 2 SO 4  Na 2 SO 4 + 2H 2 O

47. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction C 2 H 8 + O 2  Type: Combustion Products: C 2 H 8 + O 2  CO 2 + H 2 O Balanced: C 2 H 8 + 4O 2  2CO 2 + 4H 2 O

48. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction NH 3  Type: Decomposition Products: NH 3  N 2 + H 2 Balanced: 2NH 3  N 2 + 3H 2

49. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction Bi(NO 3 ) 3 + H 2 S  Type: Double Replacement Products: Bi(NO 3 ) 3 + H 2 S  Bi 2 S 3 + HNO 3 Balanced: 2Bi(NO 3 ) 3 + 3H 2 S  Bi 2 S 3 + 6HNO 3

50. Starter S-111 What type of reaction is Fe + CuCl 2  Write and balance the reaction

51. 11.3 Reactions in Aqueous Solutions Chapter 11

52. 11.2 Type of Chemical Reactions Many reactions take place in water – aqueous For example, the reaction of Silver Nitrate and Sodium Chloride But in a solution, most ionic compounds have dissociated to form ions 11.3 Reactions in Aqueous Solution

53. 11.2 Type of Chemical Reactions That is they are really in this form This is called the Complete Ionic Equation Notice – the solid is not broken into ions, only what is in solution 11.3 Reactions in Aqueous Solution

54. 11.2 Type of Chemical Reactions Look carefully at the equation There are Na + and NO 3 - ions that stay the same These are called Spectator Ions A Net Ionic Equation shows only ions that actually do something in a reaction 11.3 Reactions in Aqueous Solution

55. 11.2 Type of Chemical Reactions Net Ionic Equation Try this one 11.3 Reactions in Aqueous Solution

56. 11.2 Type of Chemical Reactions Practice Equation Compete Ionic Equations Net Ionic Equation 11.3 Reactions in Aqueous Solution

57. Starter S-112 Write the complete ionic and net ionic equations for Fe(NO 3 ) 3(aq) + 3NaOH (aq)  Fe(OH) 3(s) + 3NaNO 3(aq) Complete Ionic Fe +3 (aq) +3NO 3 - (aq) + 3Na + (aq) +3OH - (aq)  Fe(OH) 3(s) + 3Na + (aq) +3NO 3 - (aq) Net Ionic Fe +3 (aq) +3OH - (aq)  Fe(OH) 3(s)

58. 11.2 Type of Chemical Reactions Precipitate – separates from a solution as a solid Predicted using a solubility chart In the reaction Is either product a solid? 11.3 Reactions in Aqueous Solution Chart

59. 11.2 Type of Chemical Reactions AgCl – insoluble NaNO 3 11.3 Reactions in Aqueous Solution

60. 11.2 Type of Chemical Reactions AgCl – insoluble - solid NaNO 3 11.3 Reactions in Aqueous Solution

61. 11.2 Type of Chemical Reactions AgCl – insoluble - solid NaNO 3 – soluble 11.3 Reactions in Aqueous Solution

62. 11.2 Type of Chemical Reactions AgCl – insoluble - solid NaNO 3 – soluble - aqueous 11.3 Reactions in Aqueous Solution