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Types of Chemical Reactions Classifying Chemical Changes The products of a chemical reaction may often be predicted by applying known facts about common reaction types Five general types of reactions: Single displacement Double displacement Decomposition Synthesis Combustion Single Displacement (aka single replacement) One element displaces another element in a compound Metal replaces metal (+) Nonmetal replaces nonmetal (-) General form: element + compound element + compound A + BC B + AC General types of single displacement reactions: An active metal will replace the metallic ion in a compound of a less active metal. Ex: Fe + Cu(NO3)2 Fe(NO3)2 + Cu Some active metals such as sodium and calcium will react with water to give a metallic hydroxide and hydrogen gas. Ex: Ca + 2H2O Ca(OH)2 + H2 Active metals such as zinc, iron, and aluminum will displace the hydrogen in acids to give a salt and hydrogen gas. Ex: Zn + 2HCl ZnCl2 + H2 An active nonmetal will displace a less active nonmetal. Ex: Cl2 + 2NaBr 2NaCl + Br2 Double Displacement (aka double replacement) Ions in two compounds “change partners” Cation of one compound combines with the anion of the other compound General form: AB + CD AD + CB compound + compound compound + compound General types of double displacement reactions: A reaction between an acid and a base yields a salt and water. Such a reaction is a neutralization reaction. Ex: 2KOH + H2SO4 K2SO4 + 2H2O Reaction of a salt with an acid forms a salt of the acid and a second acid that is volatile. Ex: 2KNO3+ H2SO4 K2SO4 + 3HNO4 Reactions of some soluble salts produce an insoluble salt and a soluble salt. Ex: AgNO3 + NaCl AgCl + NaNO3 Decomposition A compound breaks down into 2 or more simpler substances Only one reactant General form: compound two or more substances AB A + B General types of decomposition reactions: When some acids are heated, they decompose to form water and an acidic oxide. Ex: H2CO3 CO2 + H2O When some metallic hydroxides are heated, they decompose to form metallic oxide and water. Ex: Ca(OH)2 CaO + H2O When some metallic carbonates are heated, they decompose to form a metallic oxide and carbon dioxide. Ex: Li2CO3 Li2O + CO2 Most metallic oxides are stable, but a few decompose when heated. Ex: 2HgO 2Hg + O2 Some compounds cannot be decomposed by heat, but can be decomposed into their elements by electricity. Ex: 2NaCl 2Na+ Cl2 Synthesis The combination of 2 or more substances to form a compound Only one product General form: element or compound + element or compound compound A + B AB General types of synthesis reactions: Two or more elements combine to form a compound. Ex: Fe + S FeS An acid anhydride, nonmetallic oxide, combines with water to give an acid. Ex: SO2 + H2O H2SO3 A basic anhydride, metallic oxide, combines with water to form a base. Ex: Na2O + H2O 2NaOH A basic oxide combines with a nonmetallic oxide to form a salt. Ex: CO2 + Na2O Na2CO3 Combustion Contains oxygen (O2) Usually contains hydrocarbons (H and C molecules) combine with oxygen to produce a large amount of energy, which produce CO2 + H2O General form: Hydrocarbon + oxygen carbon dioxide + water CxHy + O2 CO2 + H2O Ex: The burning of propane C3H8 + 5O2 3CO2 + 4H2O You Try! Balance and classify the following chemical reactions: 1 Na3PO4 + __ 3 KOH ___ 3 NaOH + __ 1 K3PO4 1. __ double displacement 1 P4 + __ 3 O2 __ 2 P2O3 2. __ synthesis 2 NO __ 2 O +1__ N 3. __ 2 2 2 decomposition 2 AgNO3 + 1 1 Cu(NO3)2 + __ 2 Ag 4. __ __ Cu __ single displacement 1 C3H6O + __ 4 3 3 2 + __ H2O 5. __ O2 __ CO combustion