1. CH 8 Chemical Equations and Reactions Section 3 Classifying Chemical Reactions

2. 5 reaction types:  Single Replacement (displacement)  Double Replacement (displacement)  Combustion  Synthesis  Decomposition

3. Single Replacement  Also called “displacement” Generic form: A + BC  AC + B  A single element (A) reacts with a compound (BC), and replaces an element from the compound. [A kicks out B]

4. Single Replacement cont.  A pure metal may replace a metal (or H) in a compound. Cu + AgNO 3  identify the pure metal: identify the metal (or H) in the compound: Copper is a candidate to replace silver, and it will. Cu + AgNO 3  Ag + CuNO 3

5. Single Replacement: Activity Series  Not all metals are active enough to replace a metal (or H) in a compound.  The activity series ranks the elements in order of “strength”, those high on the list will replace those below.

6. Single Replacement Reactions  Identify the element in the compound to be replaced A) Li + CuCl 2 B) Fe + AgNO 3

7. 1. Li 2. K 3. Ba 4. Sr 5. Ca 6. Na 7. Mg 8. Al 9. Mn 10. Zn 11. Cr 12. Fe 13. Co 14. Ni 15. Sn 16. Pb 17. H 18. Cu 19. Hg 20. Ag 21. Pt 22. Au Activity Series of Metals

8. 1. Li 2. K 3. Ba 4. Sr 5. Ca 6. Na 7. Mg 8. Al 9. Mn 10. Zn 11. Cr 12. Fe 13. Co 14. Ni 15. Sn 16. Pb 17. H 18. Cu 19. Sn 20. Ag 21. Pt 22. Au 1.Li 2.K 3.Ba 4.Sr 5.Ca 6.Na 7.Mg 8.Al 9.Mn 10.Zn 11.Cr 12.Fe 13.Co 14.Ni 15.Sn 16.Pb 17.H 18.Cu 19.Hg 20.Ag 21.Pt 22.Au

9. Practice:  Will calcium replace Cobalt?  Will Sodium replace magnesium?  Will Lead replace Zinc?  Will Lithium replace…  Will gold replace…  Will sodium replace Potassium?

10. Practice equations  Aluminum is dipped into Zinc Nitrate solution.  Sodium is placed into cold water.  Gold is added to a solution of calcium chloride.  Magnesium is dipped into nickel (II) chloride solution.  Lead is placed into an iron (III) nitrate solution.  Zinc is added to a solution of copper (II) sulfate.

11. Predict the products of the following reactions:  Ca + CuSO 4   Al + KNO 3 

12. Single replacement the “other” activity series  A more active halogen will replace a less active halogen 1. F 2. Cl 3. Br 4. I 5. At Cl 2 + KI  Cl 2 + KF 

13. Decomposition Reactions  Binary Compounds Break into the elements 2 HgO  2 Hg + O 2  Ternary Compounds…escaping gas Metal Carbonate Metal Carbonate breaks into metal oxide and CO 2 CaCO 3  CaO + CO 2 Generic form : AB  A + B

14. Determine the reaction category, Predict the products and balance them. Br 2 + NaI  CH 4 + O 2  C 6 H 14 + O 2 

15. Combustion Reactions Generic form: C x H y + O 2  CO 2 + H 2 O  A hydrocarbon uses oxygen from the air to produce Carbon Dioxide and Water. C 2 H 6 + O 2  CO 2 + H 2 O Complete combustion always produces carbon dioxide and water. A “hydrocarbon” may also include an oxygen C 3 H 7 OH + O 2  CO 2 + H 2 O

16. Synthesis (Combination)  2 elements  2 elements combine to form an ionic compound. 2 K + Cl 2  2 KCl metal oxidewater  A metal oxide and water combine to form a base. (a base is a hydroxide compound) MgO + HOH  Mg(OH) 2 Li 2 O + HOH  2 LiOH Generic Form: A + B  AB

17. Synthesis (Combination) non-metal oxidewater A non-metal oxide and water combine to form an acid. (an acid starts with “H”)  CO 2 + H 2 O  H 2 CO 3  Carbon dioxide + water  Carbonic acid  SO 2 + H 2 O  H 2 SO 3  Sulfur Dioxide + water  Sulfurous acid

18. Double Replacement Reactions  2 ionic compounds  2 ionic compounds “switch + partners”. A solid precipitate, a gas, or water forms  Ba(NO 3 ) 2 + Na 2 SO 4  BaSO 4 + NaNO 3 Make sure the new ionic compounds have no net charge. Generic form: AB + CD  AD + CB

19. Types of Chemical Reactions Lab

20. Pb(NO 3 ) 2 + KI

21. Mg + HCl

22. H2O2 H2O2 

23. NaHCO 3  (+heat)

24. Electrolysis of H 2 O