Chemical Reactions By: kyle and taylor

The 5 Reaction Types: Synthesis, decomposition, single replacement, double replacement, combustion reaction.

  • Synthesis- Several reactions combine to make a single product. It forms a binary compound. Ex: H2 + O2 -> H20
  • Decomposition- One reactant decomposes into two or more products. Ex: H2O -> H2 + O2
  • Single replacement- A reaction in which a single atom replaces an ion from another reactant. Ex: SrCl2 + F2 -> SrF2 + Cl2
  • Double replacement- A reaction where parts of the reactants replace each other, creating two new compounds. Ex: BaF2 + Na2O -> BaO + NaF
  • Combustion- When a hydrocarbon reacts with oxygen. The products for combustion are always water, carbon dioxide, and energy. Ex: C4H10 + O2 -> CO2 + H2O

Diagrams of the 5 Different reactions

Single replacement
Double Replacement
When determining if a metal will replace another metal in a single replacement reaction, one must look at the activity series of metals first. If the metal that is going to replace is below the metal that is being replace on the activity series, the chemical reaction can not occur.

Solubility Rules

Used to determine if a chemical will dissolve in water or not


  • All nitrates, acetates, ammonium, and Group 1 salts
  • All chlorides, bromides, and iodides, except silver, lead, and mercury (I)
  • All fluorides except Group 2, lead (II), and iron (III)
  • All sulfates except calcium, strontium, barium, mercury, lead (II), and silver


  • All carbonates and phosphates except Group 1 and ammonium
  • All hydroxides except Group 1, strontium, barium, and ammonium
  • All sulfides except Group 1, Group 2, and ammonium
  • All oxides except Group 1


Created with images by bdyczewski - "laboratory chemistry subjects"

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