1. Identify reaction type Agenda  review balancing  Check equations I  Write explaining how to balance.  Class notes: ID reaction types  Demos  Homework: Equation II

2. Provide symbol or ratio of coefficients  Solid  Reacts to form  Mg (s) + SiO 2(s)  MgO (s) + Si (s)  C 6 H 6(l) + O 2(g)  CO 2(g) + H 2 O (g)  Al 2 S 3(s) + H 2 O (l)  Al(OH) 3(aq) + H 2 S (g)

3. 1. copper + nitric acid  copper (II) nitrate + hydrogen  Cu (s) + 2 HNO 3(aq)  Cu(NO 3 ) 2(aq) + H 2(g)  1:2:1:1

4. 2. zinc + copper (I) sulfate  zinc sulfate + copper  Zn (s) + Cu 2 SO 4(aq)  ZnSO 4(aq) + 2Cu (s)  1:1:1:2

5. 3. silver nitrate + sodium bromide  sodium nitrate + silver bromide  AgNO 3(aq) + NaBr (aq)  NaNO 3(aq) + AgBr (aq)  1:1:1:1

6. 4. iron + sulfur  iron (III) sulfide  2 Fe (s) + 3 S (s)  Fe 2 S 3(s)  2:3:1

7. 5. iron (III) chloride + ammonium hydroxide  iron (III) hydroxide + ammonium chloride  FeCl 3(aq) + 3NH 4 OH (aq)  Fe(OH) 3(s) + 3NH 4 Cl (aq)  1:3:1:3

8. 6. potassium chlorate  potassium chloride + oxygen  2KClO 3  2KCl + 3O 2  2:2:3

9. 7. magnesium chloride + ammonium nitrate  magnesium nitrate + ammonium chloride  MgCl 2(aq) + 2NH 4 NO 3(aq)  Mg(NO 3 ) 2(aq) + 2NH 4 Cl (aq)  1:2:1:2

10. 8. water  hydrogen + oxygen  2H 2 O (l)  2H 2(g) + O 2(g)  2:2:1

11. 9. aluminum + sulfuric acid  aluminum sulfate + hydrogen  2Al (s) + 3H 2 SO 4(aq)  Al 2 (SO 4 ) 3(aq) + 3H 2(g)  2:3:1:3

12. 10. mercury (II) oxide  mercury + oxygen  2HgO (s)  2Hg (l) + O 2(g)  2:2:1

13. 11. potassium iodide + lead (II) nitrate  lead (II) iodide + potassium nitrate  2KI (aq) + Pb(NO 3 ) 2(aq)  PbI 2(s) + 2KNO 3(aq)  2:1:1:2

14. 12. aluminum + oxygen  aluminum oxide  4Al (s) + 3O 2(g)  2Al 2 O 3(s)  4:3:2

15. 13. sodium peroxide + water  sodium hydroxide + oxygen  2Na 2 O 2(aq) + 2H 2 O (l)  4NaOH (aq) + O 2(g)  2:2:4:1

16. 14. iron (III) chloride + potassium hydroxide  potassium chloride + iron (III) hydroxide  FeCl 3(aq) + 3KOH (aq)  3KCl (aq) + Fe(OH) 3(s)  1:3:3:1

17. 15. zinc + hydrochloric acid  zinc chloride + hydrogen  Zn (s) + 2HCl (aq)  ZnCl 2(aq) + H 2(g)  1:2:1:1

18. 16. hydrogen peroxide  water + oxygen  2H 2 O 2(aq)  2H 2 O (l) + O 2(g)  2:2:1

19. 17. copper (II) nitrate + aluminum  aluminum nitrate + copper  3Cu(NO 3 ) 2(aq) + 2Al (s)  2Al(NO 3 ) 3(aq) + 3Cu (s)  3:2:2:3

20. 18. barium hydroxide + ammonium chloride  barium chloride + ammonia + water  Ba(OH) 2(aq) + 2NH 4 Cl (aq)  BaCl 2(aq) + 2NH 3(g) + 2H 2 O (l)  1:2:1:2:2

21. 19. hydrochloric acid + sodium hydroxide  sodium chloride + water  HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l)  1:1:1:1

22. 20. lithium + water  lithium hydroxide + hydrogen  2Li (s) + 2H 2 O (l)  2LiOH (aq) + H 2(g)  2:2:2:1

23. Write  Explain how to balancing selecting one of the questions on this worksheet.  You are teaching one of the freshmen in physical science.

24. Identifying Reaction Type Date

25. How many reactants? 12 Decomposition 1 reactant  2 products comBustion Hydrocarbon + O 2  CO 2 + H 2 O Single Replacement 1 element + 1 compound  1 element + 1 compound Double Replacement 2 compound  2 compound Combination 2 reactant  1 compound

26. Identification of Reactions  Sparklers  Methane bubbles  Nickel (II) nitrate plus phosphoric acid  Alkali metals with water  Sugar