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Classification of Chemical Reactions

Learn about synthesis, decomposition, single replacement, double replacement, combustion, exothermic, endothermic reactions with examples and energy change distinctions. Understand important concepts and reactions in chemistry.

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Classification of Chemical Reactions

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  1. Classification of Chemical Reactions

  2. Types of Chemical Reactions • Synthesis • Decomposition • Single Replacement • Double Replacement • Combustion

  3. Synthesis Reactions • A reaction in which two or more simple substances (elements or compounds) react to form one new substance. • A + B  AB • Example: 2H2 + O2  2H2O CaO + CO2 CaCO3

  4. Decomposition Reactions • A reaction in which one substance breaks down into two or more simple substances • AB  A + B • Example: 2H2O2  2H2O + O2 2KClO3  2KCl + 3O2

  5. Single Replacement Reactions • A reaction in which an uncombined element replaces another element in a compound • A + BC  AC + B • “Like replaces like” – metals replace metals and nonmetals replace nonmetals

  6. Single Replacement Reactions (continued) • Examples: Mg + CuSO4 MgSO4 + Cu (Mg and Cu are both metals) Cl2 + NaBr  NaCl + Br2 (Cl and Br are both nonmetals) • In order for the reaction to take place, the uncombined element must be more reactive than the ion it is replacing.

  7. Reactivity Table Most Active Metals Li Rb K Ca Na Mg Al Mn Zn Fe Ni Sn Pb Cu Ag Least Active Metals Pt Au Most Active Nonmetals F Cl Br I Least Active Nonmetals

  8. Which of the following reactions can take place? I2 + NaF  F2 + NaI Mg + HCl  MgCl2 + H2 Cu + MgSO4  CuSO4 + Mg K + NaOH  KOH + Na

  9. Double Replacement Reactions • A reaction in which two positive ions replace each other in compounds • AB + CD  AD + CB • In order for this type of reaction to occur, one of the following must happen: a precipitate is formed, a gas is formed, or one of the products must be covalent.

  10. Double Replacement Reactions (continued) • Examples: Na2S + Cu(NO3)2 CuS+ 2NaNO3 (a precipitate is formed) 2NaCN + H2SO4 2HCN + Na2SO4 (a gas is formed) NaOH + HCl  NaCl + H2O (a covalent compound is formed)

  11. Combustion Reaction • A reaction in which a hydrocarbon reacts with oxygen to produce carbon dioxide and water • CxHy + O2 CO2 + H2O • Example: CH4+ 2O2 CO2 + 2H2O C6H12O6 + 6O2 6CO2 + 6H2O

  12. Review Classify each of the following reactions by type and then balance the equation: Pb(NO3)2 + K2CrO4PbCrO4+ KNO3 Cl2 + KI  KCl + I2 C3H6 + O2  CO2 + H2O Al(OH)3  Al2O3 + H2O Li + O2  Li2O HCl + Fe2O3  FeCl3 + H2O MgCO3  MgO + CO2 Ba(CN)2 + H2SO4  HCN + BaSO4

  13. Classifying Reactions Based on Energy Changes • Exothermic reactions are reactions in which heat/energy is released • Example: 2C4H10 + 13O2 8CO2 + 10H2O • The container often feels warm during exothermic reactions • reactions involving explosions and burning are examples

  14. Classifying Reactions Based on Energy Changes (continued) • Endothermic reactions are reactions in which heat/energy is absorbed • Example: 6CO2 + 6H2O C6H12O6 + 6CO2 (photosynthesis) NaHCO3 + HCl  NaCl + H2O + CO2 • The container often feels cold during endothermic reactions • Reactions involving cooking or heating are often examples

  15. Review • Identify each of the following as either exothermic or endothermic: Baking a cake Exploding dynamite Burning a piece of paper A chemical ice pack Hand warmers

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