Predicting Products of Chemical Reactions. Identify the type of reaction. Two elements: One compound: One compound, One element: Two compounds Hydrocarbon + O2 Synthesis Decomposition Synthesis or Single replacement Synthesis or Double replacement Combustion

The product is always!!!!!!!!! CO2 + H2O Combustion reaction The product is always!!!!!!!!! CO2 + H2O

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: BaCl2 + K2O MgF2 + Li2O KI + Pb(NO3)2 FeS + HCl

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: BaCl2 + K MgF2 + O2 K + Pb(NO3)2 FeS + Cl2

Synthesis If there are only two elements: Ba + S  BaS Combine them into a binary compound. Check oxidation number Examples: Rb + S  Rb2S Ba + S  BaS

Practice these: H2 + O2 Mg + Cl2 K + N Ca + S

Synthesis If there are three or more elements: Ca + SO2 + O2  CaSO4 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: NH3 +H2O  H2SO3 + O2 CaO + SO2  MgO + PO3 

Decomposition: MgCl2  Mg + Cl2 Products depends on the compound decomposing: Binary compounds simply break into individual elements: Examples: H2O  H2 + O2 MgCl2  Mg + Cl2

Practice these: NH3 SO2 CaO MgO

Hydroxides: Metal hydroxide + H2O NaOH  Na2O + H2O Examples: NaOH  Na2O + H2O Ca(OH)2  CaO + H2O

Practice these: Al(OH)3  LiOH Fe(OH)3 CuOH

Carbonates: PbCO3  PbO + CO2 Metal oxide + CO2 Examples: CaCO3  CaO + CO2 PbCO3  PbO + CO2

Practice these: Li2CO3 SrCO3 Cu2CO3 MgCO3

Chlorates Metal Chloride + O2 Examples: Ba(ClO3)2  BaCl2 + O2 NaClO3  NaCl + O2 Fe(ClO3)3  FeCl3 + O2

Practice these: LiClO3 Sr(ClO3)2 CuClO3 Mg(ClO3)2