1. New Stuff 2014… The Saga Continues!!!

2. Law of Conservation of Matter Law of Conservation of Mass Law of Conservation of Energy None of these can be created nor destroyed

3. Balancing a Chemical Reaction There are two parts –Reactants: What we start with –Products: What we end with They must be equal!!! THEY MUST BE EQUAL!!!

4. Symbols in a Reaction +Separates products and reactants →Separates reactants from products ↔,  Separates reactants from products and indicates a reversible reaction (s)Solid (l)Liquid (g)Gas (aq)Water solution

5. Water H 2 O H 2 + O 2 → H 2 O Reactants Products

6. Balance The Reaction You can NOT change a subscript!!!!! If you change a subscript, you change the chemical. You can NOT change a subscript!!!!!

7. Balance the Reaction Look at this reaction: H 2 + O 2 → H 2 O That gives us: 2 H + 2 O → 2 H + 1 O 2 H + 2 O ≠ 2 H + 1 O

8. Balance the Reaction To get the reaction to balance, we need to add a coefficient to the reaction. A coefficient changes the amount of material you put into the reaction.

9. Balance the Reaction When I put a coefficient in front of a chemical, I have added additional “buckets” of stuff. H 2 + O 2 → H 2 O If I place the #2 in front of H 2 O… H 2 + O 2 → 2 H 2 O

10. Balance the Reaction It means that I have 2 “Buckets” of water. H 2 + O 2 → 2 H 2 O 2 H + 2 O → 4 H + 2 O 2 H + 2 O ≠ 4 H + 2 O Closer… But not quite…

11. Balance the Reaction I need to increase the number of hydrogen molecules. If I add a coefficient to the H 2, I can balance it out. 2 H 2 + O 2 → 2 H 2 O 4 H + 2 O = 4 H + 2 O (The peasants rejoice)

12. Balance K Cl → K + Cl 2 2 K Cl → 2 K + Cl 2

13. Balance Be Cl 2 + H 2 O → Be O + H Cl Be Cl 2 + H 2 O → Be O + 2 H Cl

14. Balance Na Cl → Na + Cl 2 2 Na Cl → 2 Na + Cl 2

15. Balanced? H Cl + Na O H → H 2 O + Na Cl 2Fe 2 O 3 + 3C → 4Fe + 3C O 2

16. Balance Ca Cl 2 → Ca + Cl 2 Al Cl 3 → Al + Cl 2 Al 2 O 3 + H 2 → Al + H 2 O

17. More New Stuff!!! 1-8-14

18. Types of Reactions Synthesis Decomposition Single replacement Double replacement Combustion

19. Types of Reactions Synthesis A + B → A B

20. Types of Reactions Decomposition A B → A + B

21. Types of Reactions Single replacement A B + C → A C + B

22. Types of Reactions Double replacement A B + C D → A D + C B

23. Types of Reactions Combustion A + O 2 → Stuff + Heat + Light

24. Think about H2 O as H (O H) for most of the reactions.

25. Balance K Cl → K + Cl 2 H Cl + Na O H → H (O H) + Na Cl Fe 2 O 3 + C → Fe + C O 2 H 2 + O 2 → H (O H)

26. Balance 2 K Cl → 2 K + Cl 2 H Cl + Na O H → H (O H) + Na Cl 2 Fe 2 O 3 + 3 C → 4 Fe + 3 C O 2 2 H 2 + O 2 → 2 H (O H)

27. K Cl → K + Cl 2 Decomposition H Cl + Na O H → H 2 O + Na Cl Double replacement Fe 2 O 3 + C → Fe + C O 2 Single replacement H 2 + O 2 → H (O H) Synthesis

28. 2K Cl → 2K + Cl 2 Decomposition H Cl + Na O H → H 2 O + Na Cl Double replacement 2Fe 2 O 3 + 3C → 4Fe + 3C O 2 Single replacement 2H 2 + O 2 → 2H (O H) Synthesis

29. 1-9-14 Additional New Stuff!!!

30. Types of Reactions Synthesis Decomposition Single replacement Double replacement Combustion

31. Balance and Identify K 3 N → K + N 2 32 6

32. Balance and Identify In your notes for practice: K (O H) + H Cl → K Cl + H (O H) Ca (O H) 2 + H Br → Ca Br 2 + H (O H) B 2 O 3 → B + O 2 C 6 H 12 O 6 + O 2 → C O 2 + H 2 O H (O H) + Na → Na (O H) + H 2 Al + Cl2 → Al Cl 3

33. Balance and Identify K (O H) + H Cl → K Cl + H (O H) Double Replacement Ca (O H) 2 + 2H Br → Ca Br 2 + 2H (O H) Double Replacement 2 B 2 O 3 → 4 B + 3 O 2 Decomposition C 6 H 12 O 6 + 3 O 2 → 6 C O 2 + 6 H 2 O Combustion 2 H (O H) + 2 Na → 2 Na (O H) + H 2 Single replacement 2 Al + 3 Cl 2 → 2 Al Cl 3 Synthesis

34. Balance and Identify Quiz: New page in notebook… Na (O H) + H I → Na I + H (O H) Li 2 S + K (O H) → Li (O H) + K 2 S Cu Cl 2 + Na → Na Cl + Cu C 6 H 12 O 6 → C + H 2 O Ag Cl + Na 2 (S O 4 ) → Ag 2 (S O 4 ) + Na Cl

35. Answers Na (O H) + H I → Na I + H (O H) Double Replacement Li 2 S + 2 K (O H) → 2 Li (O H) + K 2 S Double Replacement Cu Cl 2 + 2 Na → 2 Na Cl + Cu Single Replacement C 6 H 12 O 6 → 6 C + 6 H 2 O Decomposition 2 Ag Cl + Na 2 (S O 4 ) → Ag 2 (S O 4 ) + 2 Na Cl Double Replacement