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II. Five basic types of chemical reactions:

II. Five basic types of chemical reactions:. Synthesis (composition) Decomposition Single Replacement Ionic or Double Replacement Combustion. A. Synthesis (composition):. two or more elements or compounds may combine to form a more complex compound. Basic form: A  +  X   AX.

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II. Five basic types of chemical reactions:

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  1. II. Five basic types of chemical reactions:

  2. Synthesis (composition) • Decomposition • Single Replacement • Ionic or Double Replacement • Combustion

  3. A. Synthesis (composition): • two or more elements or compounds may combine to form a more complex compound. • Basic form: A  +  X   AX

  4. Examples of synthesis reactions • Metal  +  oxygen  metal oxide • ex. 2Mg  +  O2  2MgO

  5. Nonmetal  +  oxygen  nonmetallic oxide • ex. C  +   O2  CO2

  6. Metal oxide  +  water   metallic hydroxide • ex. MgO  +   H2O   Mg(OH)2

  7. Nonmetallic oxide  +  water   acid • ex. CO2  +  H2O    H2CO3

  8. Metal + nonmetal   salt • ex. 2 Na  +  Cl2  2NaCl

  9. A few nonmetals combine with each other. ex. 2P  +  3Cl2  2PCl3

  10. What do all of these have in common? 2Mg  +  O2  2MgO • C  +   O2  CO2 CO2  +  H2O    H2CO3 MgO  +   H2O   Mg(OH)2 2 Na  +  Cl2  2NaCl 2P  +  3Cl2  2PCl3 Only one product is formed.

  11. Example(from Chemistry Interactive 2.0 CD, disk 1) Zinc + Iodine zinc iodide Oxygen + Hydrogen  Water

  12. Practice Predicting Products of Synthesis Reactions

  13. B. Decomposition: • A single compound breaks down into its component parts or simpler compounds. • Basic form: AX  A  +  X

  14. Examples of decomposition reactions: • Metallic carbonates, when heated, form metallic oxides and CO2 . • ex. CaCO3  CaO  +  CO2

  15. Most metallic hydroxides, when heated, decompose into metallic oxides and water. • ex. Ca(OH)2  CaO  +  H2O

  16. Metallic chlorates, when heated, decompose into metallic chlorides and oxygen. • ex. 2KClO3  2KCl  +  3O2

  17. Some acids, when heated, decompose into nonmetallic oxides and water. • ex. H2SO4  H2O  +  SO3

  18. Some oxides, when heated, decompose. • ex. 2HgO   2Hg  +  O2

  19. Some decomposition reactions are produced by electricity. • ex. 2H2O   2H2  +  O2 • ex. 2NaCl   2Na  +  Cl2

  20. What do all of these have in common? • CaCO3  CaO  +  CO2 • Ca(OH)2  CaO  +  H2O • 2KClO3  2KCl  +  3O2 • H2SO4  H2O  +  SO3 • 2HgO   2Hg  +  O2 • 2H2O    2H2  +  O2 They have only one reactant.

  21. Example • Decomposition of ammonium dichromate

  22. Practice Predicting Products of Decomposition Reactions

  23. C. Single Replacement: • a more active element takes the place of another element in a compound and sets the less active one free. • Basic form: A  +  BX AX  +  B •  or • AX  +  Y  AY + X

  24. Examples of replacement reactions: • Replacement of a metal in a compound by a more active metal. • ex. Fe  +  CuSO4FeSO4  +  Cu

  25. Replacement of hydrogen in water by an active metal. • ex. 2Na  +  2H2O   2NaOH  +  H2 • ex. Mg  +  H2O MgO  +  H2

  26. Replacement of hydrogen in acids by active metals. • ex. Zn  +  2HCl ZnCl2  +  H2

  27. Replacement of nonmetals by more active nonmetals. • ex. Cl2  +  2NaBr  2NaCl  +  Br2

  28. Examples(use Disk 2)

  29. Practice Predicting Products of Replacement Reactions

  30. D. Ionic or Double Replacement: • occurs between ions in aqueous solution. • A reaction will occur when a pair of ions come together to produce at least one of the following: • a precipitate • a gas • water or some other non-ionized substance. • Basic form: AX  + BY    AY  +  BX

  31. Examples of ionic reactions: • Formation of precipitate. • ex. NaCl  +  AgNO3  NaNO3  +  AgCl  • ex. BaCl2  +  Na2 SO4   2NaCl  +  BaSO4 

  32. Formation of a gas. • ex. HCl  +  FeS -  FeCl2  +  H2S 

  33. Formation of water. (If the reaction is between an acid and a base it is called a neutralization reaction.) • ex. HCl  +  NaOH   NaCl  +  H2O

  34. Formation of a product which decomposes. • ex. CaCO3  +  HCl   CaCl2  +  CO2  +  H2O

  35. Ammonium chloride + barium hydroxide Example

  36. Practice Predicting Products of Ionic Reactions

  37. Combustion of Hydrocarbons: • When a hydrocarbon is burned with sufficient oxygen supply, the products are always carbon dioxide and water vapor. • If the hydrocarbon has an even number of carbons, start with a coefficient of 2 CxHy • Balance in this order: C, H, O

  38. If the supply of oxygen is low or restricted, then carbon monoxide will be produced. • This is why it is so dangerous to have an automobile engine running inside a closed garage or to use a charcoal grill indoors.

  39. NOTE: • The phrase "To burn" means to add oxygen unless told otherwise.

  40. (CxHy)  +  O2  CO2  +  H2O • ex. CH4  +  2O2  CO2  +  2H2O • ex. 2C4H10   13O2  8CO2  + 10H2O

  41. Analyzing Chemical Reactions • One Reactant? yes no Decomposition Next slide

  42. 2 Ionic Compounds or Acid and Ionic Compound? yes no Double Replacement Next slide Precipitate Neutralization Gas

  43. yes no • Element and Compound? Single Replacement Hydrocarbon and O2 yes Metal Halogen Metallic oxide no no Combustion Synthesis

  44. yes Decomposition no • One Reactant? 2 Ionic Compounds or Acid and IonicCompound? yes no Double Replacement Element and Compound? yes no Precipitate Gas Neutralization Hydrocarbon and O2? Single Replacement yes no yes no Combustion Metal Halogen Metallic oxide Synthesis

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