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Predicting Products of Chemical Reactions. Identify the type of reaction. Two elements: Synthesis One compound: Decomposition One compound, One element: Synthesis or Single replacement Two compounds Synthesis or Double replacement Hydrocarbon + O2 Combustion Combustion reaction The product is always!!!!!!!!! CO2 + H2 O Double Replacement Switch the positive ions: Check Oxidation numbers: Examples: HOH + KCl HCl + KOH Al2(SO4)3 + NH4ClO3 (NH4)2SO4 + Al(ClO3)2 Practice these: 3. BaCl2 + K2O MgF2 + Li2O KI + Pb(NO3)2 4. FeS + HCl 1. 2. Single Replacement Determine if the single element is positive or negative. Replace the same charged element in the compound. Examples: Al + Pb(NO3)2 Al(NO3)3 + Pb Mg + HCl MgCl2 + H2 Practice these: 3. BaCl2 + K MgF2 + O2 K + Pb(NO3)2 4. FeS + Cl2 1. 2. Synthesis If there are only two elements: Combine them into a binary compound. Check oxidation number Examples: Rb + S Rb2S Ba + S BaS Practice these: 3. H2 + O2 Mg + Cl2 K+N 4. Ca + S 1. 2. Synthesis If there are three or more elements: THERE WILL BE AT LEAST ONE POLYATOMIC ION. ARRANGE THE ELEMENTS INTO A COMMON POLYATOMOC ION. THE OTHER ION IS THE ELEMENT LEFT OVER. Examples: H2O + SO2 H2SO4 Ca + SO2 + O2 CaSO4 Practice these: 1. 2. 3. 4. NH3 +H2O H2SO3 + O2 CaO + SO2 MgO + PO3 Decomposition: Products depends on the compound decomposing: Binary compounds simply break into individual elements: Examples: H2O H2 + O2 MgCl2 Mg + Cl2 Practice these: 1. 2. 3. 4. NH3 SO2 CaO MgO Hydroxides: Metal hydroxide + H2O Examples: NaOH Na2O + H2O Ca(OH)2 CaO + H2O Practice these: 1. 2. 3. 4. Al(OH)3 LiOH Fe(OH)3 CuOH Carbonates: Metal oxide + CO2 Examples: CaCO3 CaO + CO2 PbCO3 PbO + CO2 Practice these: 1. 2. 3. 4. Li2CO3 SrCO3 Cu2CO3 MgCO3 Chlorates Metal Chloride + O2 Examples: Ba(ClO3)2 BaCl2 + O2 NaClO3 NaCl + O2 Fe(ClO3)3 FeCl3 + O2 Practice these: 1. 2. 3. 4. LiClO3 Sr(ClO3)2 CuClO3 Mg(ClO3)2