1. Unit VI: CHEMICAL REACTIONS I.5. Types Of Chemical Reactions

2. Types of Reactions 1. Synthesis 2. Decomposition 3. Single Replacement 4. Double Replacement Neutralization (Water Forming) 5. Combustion 1. Combustion of hydrocarbons 2. Combustion of metals

3. Synthesis Two or more substances combine to form a compound A + B AB

4. Synthesis

5. Often: elements a compound 2Al + 3F 2 2AlF 3

6. Synthesis Examples 2H 2 + O 2 2H 2 O 2Mg + O 2 2MgO CaO + CO 2 CaCO 3

7. Synthesis potassium + oxygen calcium + phosphorous

8. Synthesis A special type of synthesis CoCl 2 + 6H 2 O CoCl 2 6H 2 O

9. Synthesis A compound + an element a bigger compound 2SO 2 + O 2 2SO 3

10. Synthesis - Overview Always m mm more than 1 reactant Usually forms only 1 product

11. Decomposition One substance breaks down into more than one substance AB A + B

12. Decomposition

13. EXAMPLES: 2HgO 2Hg + O 2 2H 2 O 2H 2 + O 2 MgCl 2 Mg + Cl 2

14. Decomposition Note: Unless otherwise told, break all compounds COMPLETELY down to its elements. (Even break up PAIs)

15. Decomposition Note: Unless otherwise told, break all compounds COMPLETELY down to its elements. (Even break up PAIs)

16. Decomposition Note: Unless otherwise told, break all compounds COMPLETELY down to its elements. (Even break up PAIs)

17. Decomposition A special type of decomposition CuSO 4 5H 2 O CuSO 4 + 6H 2 O

18. Decomposition Also A Bigger Compound Smaller Compound + An Element 2KClO 3 2KCl + 3O 2

19. Single Replacement One substance replaces another in a compound Metals replace metals Non-metals replace non-metals AB + C A + BC

20. Single Replacement

21. Two Types 1. Metal Single Replacement 2. Non-metal Single Replacement

22. Single Replacement Examples of Metal SR Zn + CuSO 4 Cu + ZnSO 4 Fe + 3AgNO 3 3Ag + Fe(NO 3 ) 3

23. Single Replacement Metal SRs

24. Single Replacement Metal SRs

25. Single Replacement Some Non-Metal SRs

26. Single Replacement Some Non-Metal SRs

27. Single Replacement The catch some elements are not strong enough to replace others Plan: 1. Predict Products 2. Fix Formulas 3. Balance Equation 4. Determine from Activity Series if Reaction will Proceed

30. Double Replacement Both compounds change partners Again refer to the activity series to see if reaction will proceed AB + CD AD + BC

31. Double Replacement

32. Refer to the activity series to determine the relative reactivity of elements. For example, calcium is more reactive than hydrogen; therefore, calcium can replace hydrogen in a reaction.activity series Ca(s) + 2 HOH(l) Ca(OH) 2 (s) + H 2 (g)

34. Double Replacement Examples: 2KI (aq) + Pb(NO 3 ) 2 (aq) 2KNO 3 (aq) + PbI (s) AgNO 3 + KCl AgCl(s) + KNO 3

35. Double Replacement

38. Neutralization Sub-type of Double Replacement Reaction Sometimes called water forming ACID + BASE WATER + SALT

39. Neutralization

41. Combustion (aka Burning Stuff) Substance reacts with oxygen (fast enough to produce heat and light) Two Types of Combustion 1. Combustion of hydrocarbons 2. Combustion of metals

42. Combustion Hydrocarbons ALWAYS A REACTANT NOTE: O 2 is ALWAYS A REACTANT! ASSUME When burning hydrocarbons ASSUME the products are CO 2 + H 2 O

43. Combustion C x H y + O 2 CO 2 + H 2 O

44. Combustion

46. Combustion of Metals = Synthesis

47. Combustion Combustion of Metals = Synthesis

48. Combustion Combustion of Metals = Synthesis

49. Assignments Do Problem Set #3 and #4 on page in your Student Workbook Do Exercises 65 (a, c, e), 66 (b, d, f, h, j, l, n, p, r, t, v, x), 67 (a, c, e, h, j, l, n, p, r) on page 118 [Hebden] Do Hand-In Assignment # 8

50. Lab Do Experiment 5C – page 71-73[Heath] before This experiment will take most of the class your pre-lab must be complete before the lab begins Fill in the Blank Lab Format you are only responsible for the questions asked in the lab handout