7.3 Classifying Reactions

A combustion reaction is a chemical reaction that occurs when a substance combines with oxygen, releasing energy in the form of light and heat. Example: CH₄ + 2O₂ ⟶ CO₂ + 2H₂O.

A single replacement reaction is a type of chemical reaction where one element replaces another element in a compound. Example: Zn + 2HCl ⟶ ZnCl₂ + H₂.

A decomposition reaction is a chemical reaction where a single compound breaks down into two or more simpler products. Example: 2H₂O ⟶ 2H₂ + O₂.

A synthesis reaction is a type of chemical reaction where two or more simple substances combine to form a more complex product. Example: 2H₂ + O₂ ⟶ 2H₂O.

A double replacement reaction is a chemical reaction where two compounds exchange ions or bonds to form two new compounds. Example: AgNO₃ + NaCl ⟶ AgCl + NaNO₃.

The products of the combustion of propane are carbon dioxide (CO₂) and water (H₂O). Reaction: C₃H₈ + 5O₂ ⟶ 3CO₂ + 4H₂O.

The general form of a synthesis reaction is A + B ⟶ AB, where A and B are reactants that combine to form a single product AB.

The general form of a decomposition reaction is AB ⟶ A + B, where a single compound AB breaks down into its components A and B.

The general form of a single replacement reaction is A + BC ⟶ AC + B, where element A replaces element B in compound BC.

The general form of a double replacement reaction is AB + CD ⟶ AD + CB, where the ions of two compounds exchange places.