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Chemical Reactions

Chemical Reactions. Types of Reactions. 5 Types of Reactions. Synthesis or Combination Decompostion Single Replacement Double Replacement Combustion. Synthesis or Combination Reaction. Two or more substances combine to form another substance Example: A + B  AB

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Chemical Reactions

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  1. Chemical Reactions Types of Reactions

  2. 5 Types of Reactions • Synthesis or Combination • Decompostion • Single Replacement • Double Replacement • Combustion

  3. Synthesis or Combination Reaction • Two or more substances combine to form another substance • Example: A + B  AB • 2H2 (g) + O2 (g)  2H2O (g)

  4. Decomposition Reaction • One substance breaks down or decomposes into two or more simpler substances • Example: AB  A + B • 2H2O  2H2 + O2 • Just the opposite of a synthesis reaction

  5. Single Replacement Reaction • Occurs when one element replaces another in a compound • Example: AB + C  AC + B • Ba (cr) + FeBr2(aq)  BaBr2 (aq) + Fe (cr)

  6. Double Replacement Reaction • Takes place if a precipitate, water, or a gas forms when two ionic compounds in solution are combined • A precipitate is an insoluble compound formed during this type of reaction • Example: AB + CD  AC + BD • AgNO3 (aq) + NaCl (aq)  AgCl (cr) + NaNO3 (aq)

  7. Combustion Reaction • A chemical change in which an element or a compound reacts with oxygen often producing energy in the form of heat and light • Often the other reactant is a hydrocarbon which is a compound composed of hydrogen and carbon • The products of a combustion reaction are usually CO2 and H2O

  8. Example • 2 C8H18(l) + 25 O2(g) 16 CO2(g) + 18 H2O(l) • Notice the reactants and products • Reactants – Hydrocarbon reacting with Oxygen • Products – CO2 and H2O • Is this a combustion reaction • 2 Mg(s) + O2(g)  2 MgO (s) • Yes, because it reacts with oxygen producing heat and light • It can also be classified as a synthesis or combination reaction

  9. Energy and Chemical Reactions • In all chemical reactions, energy is either released or absorbed • Bonds must be broken or formed • To break bonds energy is required • To form bonds energy is released

  10. Exothermic Reaction • In many chemical reactions, less energy is required to break the original bonds than is released with the formation of new bonds • Heat is given off • Examples: Burning of wood; Explosion • Reactants  Products + Energy

  11. Endothermic Reaction • More energy is required to break the original chemical bonds than is given off. • Heat is absorbed so the container feels colder • Reactants + Energy  Products

  12. What type of reaction? • 2 NaBr + 1 Ca(OH)22 CaBr2 + 2 NaOH • 2 NH3+ 1 H2SO41 (NH4)2SO4 • 3 Pb + 3 H3PO43 H2 + 1 Pb3(PO4)2

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