2. H 2 CO 3

3. Carbonic Acid

4. F2F2

5. Fluorine

6. P3O2P3O2

7. Triphosphorus dioxide

8. K 3 SO 4

9. Potassium sulfate

10. Chromic Acid

11. H 2 CrO 4

12. Chlorine

13. Cl 2

14. Sulfur dioxide

15. SO 2

16. Ammonium phosphate

17. (NH 4 ) 3 PO 4

18. 2NaCl + F 2 2NaF + Cl 2

19. Sodium chloride and Fluorine

20. 4KMnO 4 2K 2 O+4MnO+5O 2

21. Potassium oxide Manganese (II) oxide Oxygen gas

22. Al (s) + HCl (aq) The Works Explosion

23. 2Al (s) +6HCl (aq) 3H 2(g) +2AlCl 3(aq)

24. C 6 H 12 O 6 +6O 2 6CO 2 +6H 2 O

25. Combustion

26. Fe (s) +2HCl (Aq) FeCl 2(Aq) +H 2(g)

27. Single Replacement- Cationic

28. 8 Fe + S 8 → 8 FeS

29. Synthesis

30. AgNO 3 +NaCl →AgCl+NaNO 3

31. Double Replacement

32. Br 2 + 2KI → 2KBr + I 2

33. Single Replacement- Anionic

34. A. State the coefficients in order B. How many atoms of iodine are in the reactants? C. List the subscripts in order D. What type of reaction occurred?

35. A. 1:2:3:2 B. 6 atoms C. 2, 3, 2, 3 D. Single Replacement- Anionic F 2 + 2NiI 3  3I 2 + 2NiF 3

36.  Does the following reaction occur? Cu (II) + 2NaCl  CuCl 2 + 2Na  How do you know?

37.  No reaction  How do you know? ◦ You looked at your PURPLE reactivity chart and saw that copper is less reactive than sodium.

38.  What happens in the presence of:  CO 2  H 2  O 2

39.  What happens in the presence of:  CO 2 -Flame goes out  H 2 - Popping noise  O 2 - Flame gets bigger

41.  You didn’t wait long enough.  You waited too long.  The pop was too quiet to hear.

43.  Not waiting long enough  Not mixing  Not feeling for a temperature change

45.  Subscripts are the small numbers showing the number of atoms in the compound. They cannot be changed within the compound.  Coefficients are the large number in front that state the number of molecules. These numbers can be changed.

46. AgNO 3 + NaCl 

47. AgNO 3 + NaCl  AgCl + NaNO 3

48. Na +Br 2 

49. 2 Na +Br 2  2NaBr

50. KI + Br  KBr + I 2

51.  Bromine is a dirty seven element.

52. Fe (s) + HCl (Aq)  FeCl 2(Aq) +H 2(g)

53. Fe (s) + 2HCl (Aq)  FeCl 2(Aq) +H 2(g)

54.  Potassium bromide reacts with sodium (II) chloride to produce potassium chloride and sodium bromide.

55.  Sodium has a positive one charge.

56.  What are the possible products of a double replacement reaction?

57.  Gas, water or precipitation (PPT)  If none of the above are produced, it is not a reaction!

58.  For the following reaction:  A. Predict products in words  B. Write a balanced chemical equation with states  C. Write a balanced complete ionic equation. Circle spectators.  D. Write a balanced net ionic equation.  Iron (III) chloride + ammonium hydroxide 

59.  Iron (III) chloride + Ammonium hydroxide  iron (III) hydroxide + Ammonium chloride

60.  FeCl 3(aq) + 3NH 4 OH (aq)  Fe(OH) 3(s) + 3NH 4 Cl (aq)

61.  Fe +3 (aq) + 3Cl - (aq) + 3NH 4 + (aq) + 3OH - (aq)  Fe(OH) 3(s) + 3NH 4 + (aq) +3Cl - (aq)

62.  Fe +3 (aq) + 3OH - (aq)  Fe(OH) 3(s)