Lesson Day Date Topic
1. Synthesis and Decomposition Reactions
2. Single Replacement Reactions
3. Double Replacement Reactions
4. Reactions Combined
5. Formula and Ionic Equations
6. Reactions Practice Test
Worksheet #1 Synthesis and Decomposition Reactions
Predict and balance the following synthesis and decomposition reactions. Assume that all reactions will occur. Use abbreviations to indicate the phase of reactants and products: (aq) (s) (l) (g).
1. A sample of mercury II oxide is heated.
2. Sulfur dioxide gas is heated.
3. Aluminum is reacted with iodine.
4. Liquid hydrogen peroxide H2O2 is warmed and decomposes into water and other common gas.
5. Solid lithium reacts with sulphur.
6. Molten aluminum chloride is electrolyzed.
7. Sodium is added to a container of iodine vapor.
8. Molten calcium chloride is electrolyzed.
Worksheet #2 Single Replacement Reactions
Using the activity series, predict and balance the following single replacement reactions. Use abbreviations to indicate the appropriate phase of reactants and products. For those that do not react, write no reaction.
1. A piece of copper is dropped into a container of water.
2. Liquid bromine is added to a container of sodium iodide crystals.
3. An aluminum strip is immersed in a solution of silver nitrate.
4. Zinc pellets are added to a sulfuric acid solution.
5. Fluorine gas is bubbled into a solution of aluminum chloride.
6. Magnesium turnings are added to a solution of lead (II) acetate.
7. Iodine crystals are added to a solution of sodium chloride.
8. Calcium metal is added to a solution of nitric acid.
9. A pea-sized piece of lithium is added to water.
10. A solution of iron (III) chloride is poured over a piece of platinum wire.
Worksheet #3 Double Replacement Reactions
Predict and balance the following Double Replacement reactions. Include all phase symbols. Use your solubility table to predict.
1. Silver nitrate + Potassium sulphate
2. Ammonium chloride + Cobalt (II) sulphate
3. Lead II nitrate + Sodium chloride
4. Zinc bromide + Cesium hydroxide
5. Ammonium sulfide + Lead II nitrate
6. Iron III sulfate + Barium iodide
7. Chromium III bromide + Sodium nitrate
8. Rubidium phosphate + Titanium IV nitrate
9. Ammonium carbonate + Nickel II chloride
10. Tin IV nitrate + Potassium sulfite
11. Ammonium sulfate and Potassium hydroxide
12. Cobalt II chloride is combined with Silver nitrate
Complete the following combustion reactions. Include all phase symbols.
13. C4H10(g) + O2(g) →
14. C6H12(l) + O2(g) →
15. C22H42(l) + O2(g) →
16. C6H12O6(s) + O2(g) →
17. C12H24O11(s) + O2(g) →
Complete the following acid carbonate reactions. Include all phase symbols.
18. HCl(aq) + CaCO3(s) →
19. H2SO4(aq) + BaCO3(s) →
20. H3PO4(aq) + Na2CO3(s) →
Worksheet 4 Reactions Combined
1. Zinc is reacted with phosphorus.
2. A solution of cobalt (II) nitrate is reacted with a solution of sodium carbonate.
3. Magnesium metal is placed in a solution of zinc chloride.
4. Iron (III) oxide is decomposed.
5. Octane, C8H18, is burned as a fuel in cars.
6. Lithium reacts with water.
7. Sodium hydroxide solution is reacted with sulphuric acid.
8. Phosphoric acid reacts with barium hydroxide.
9. Hydrochloric acid reacts with barium carbonate.
10. The decomposition of sodium sulphide using electrolysis.
11. Calcium reacts with water.
12. Barium reacts with phosphoric acid.
13. Barium nitrate and Aluminum sulphate react in solution.
Worksheet 5 Formula and Ionic Equations
Write dissociation Equations for the following.
Complete the formula equation, complete ionic equation, and net ionic equation:
1. AgNO3(aq) + Na2SO4(aq) →
2. H3PO4(aq) + Sr(OH)2(aq) →
3. Fe(NO3)3(aq) + Zn(s) →
4. H2SO4(aq) + NaOH(aq) →
5. H3PO4(aq) + Sr(OH)2(aq) →
6. Ca(NO3)2(aq) + Na3PO4(aq) →
7. Zn(s) + HCl(aq) →
8. Sr(OH)2 (aq) + ZnSO4 (aq) →
9. Ca(s) + H2O(l) →
10. AlCl3(aq) + Zn(s) →
11. SrCl2(aq) + CaS(aq) →
Worksheet 6 Reactions Practice Test
Simplify each and round off to the correct number of significant digits.
1. 19.239 + 5.37
2. 2.6699 - 1.27
3. 156.3 x 277.3 x 45.3 x 0.0445687 0.82569 x 19.235 x 2654
4. 9.66 x 10 24 x 5.37894 x 10-15 x 4.532 x 1015
2.059 x 10 -20 5.343250 x 1015 5.37894 x 10-12
Convert using unit analysis
5. 627 g to mg
6. 4.05 x 106 um to m
7. 8.148 ML to mL
8. 235.2 mg to kg
9. 6.55 x 1014 mL to ML
Complete, include all phase symbols, and balance each equation. Write formula, complete, and net ionic equations.
10. Ca(s) + H2O(l) →
11. ZnCl2(aq) + Al(s) →
12. SrCl2(aq) + BaS(aq) →
13. H3PO4(aq) + Ca(OH)2(aq) →
14. Ba(NO3)2(aq) + Na3PO4(aq) →
15. AgNO3(aq) + Na2SO4(aq) →
16. Fe(NO3)3(aq) + Zn(s) →
17. HCl(aq) + CaCO3(s) →
18. H2SO4(aq) + BaCO3(s) →
Complete each formula equation only.
19. C10H22(l) + O2(g) →
20. C24H46(l) + O2(g) →
21. C12H22O11(s) + O2(g) →
22. Chlorine gas is bubbled into a solution of aluminum iodide.
23. Magnesium turnings are added to a solution of lead (II) chloride.
24. Barium metal is added to a solution of nitric acid.
25. Lead II nitrate and Sodium chloride are mixed both in solution.
26. Zinc bromide and Cesium hydroxide are mixed in solution.
27. Zinc is reacted with phosphorus.
28. Iron (II) oxide liquid is decomposed by electrolysis.
29. Octane, C8H18, is burned as a fuel in cars.