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Types of Chemical Reactions

Ch. 8 – Chemical Reactions. Types of Chemical Reactions. Describing Chemical Reactions. Evidence of a chemical change… Production of heat and light Formation of a gas Formation of a precipitate, a solid product. Color change. Describing Chemical Reactions. A+B  AB. PRODUCTS.

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Types of Chemical Reactions

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  1. Ch. 8 – Chemical Reactions Types of Chemical Reactions

  2. Describing Chemical Reactions • Evidence of a chemical change… • Production of heat and light • Formation of a gas • Formation of a precipitate, a solid product. • Color change

  3. Describing Chemical Reactions A+B AB PRODUCTS REACTANTS

  4. Describing Chemical Reactions

  5. A. Combination / Synthesis (marriage) • the combination of 2 or more substances to form a compound • only one product A + B  AB

  6. A. Combination / Synthesis • Product: • Must be a compound Mg(s) + O2(g)  MgO(s)

  7. B. Decomposition (divorce) • a compound breaks down into 2 or more simpler substances • only one reactant AB  A + B

  8. B. Decomposition • Products: • Can be elements or compounds H2O2 (aq)  H2O(l) + O2(g)

  9. C. Single Replacement (affair) • one element replaces another in a compound • Metal replaces metal • Nonmetal replaces nonmetal A + BC  B + AC

  10. C. Single Replacement Zn(s) + HCl(aq)  H2(g) + ZnCl2(aq)

  11. D. Double Replacement (Jerry Springer) • ions in two compounds “change partners” • cation of one compound combines with anion of the other AB + CD  AD + CB

  12. D. Double Replacement • Products: • Are compounds • Sometimes one of the products is water Pb(NO3)2(aq)+ NaI(aq)  PbI2(s)+ NaNO3(aq)

  13. E. Combustion • the burning of a hydrocarbon to produce heat CxHy + O2 CO2 + H2O

  14. E. Combustion • Products: • During complete combustion the products are CO2 + H2O C12H22O11 + 3O2 9C + 3CO2 + H2O

  15. Warm up (practice) Title: Reaction Types Number Page (1-5) 1. 2. 3. 4. 5.

  16. 1. Single Replacement Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)

  17. 2. Decomposition 2 H2O(l)  2 H2(g) + O2(g)

  18. 3. Combination / Synthesis H2(g) + Cl2(g)  2 HCl(g)

  19. 4. Double Replacement Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)

  20. 5. Combustion C2H6 + O2 CO2 + H2O

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