1. Chemical Reactions NC Essential Standard 2.2.2 Identifying Types of Chemical Reactions

2. Synthesis (Combination) Reactions Two or more substances combine to form a new compound. A + B  AB Formation of binary compounds A + B  AB Metal oxide and water MO + H 2 O  Base Nonmetal oxide and water (NM)O + H 2 O  Acid There are others not covered here! M= metal NM = Nonmetal

3. Decomposition Reactions A single compound undergoes a reaction that produces two or more simpler substances Decomposition of: Binary compounds H 2 O (l )  2H 2(g) + O 2(g) Metal carbonates CaCO 3(s)  CaO (s) + CO 2(g) Metal Hydrogen Carbonate MHCO 3  MO + H 2 O + CO 2 Metal hydroxides Ca(OH) 2(s)  CaO (s) + H 2 O (g) Metal chlorates 2KClO 3(s)  2KCl (s) + 3O 2(g) Oxyacids Acid  CO 2(g) + H 2 O(l ) AB  A + B M= metal NM = Nonmetal

4. Single Replacement Reactions Replacement of: Metals by another metal A + BC  AC + B Hydrogen in water by a metal M + H 2 O  MOH + H 2 Hydrogen in an acid by a metal M + HX  MX + H 2 Halogens by more active halogens D + BC  BD +C A + BX  AX + B BX + Y  BY + X

5. Double Replacement Reactions The ions of two compounds exchange places in an aqueous solution to form two new compounds. AB + CD  AD + CB Formation of a precipitate, gas from a solution, or a molecular compound, usually water. Acid-Base “Neutralization”

6. Combustion Reactions A substance combines with oxygen, releasing a large amount of energy in the form of light and heat. Hydrocarbon + oxygen  Carbon dioxide and water The burning of natural gas, wood, gasoline C 3 H 8(g) + 5O 2(g)  3CO 2(g) + 4H 2 O (g) Incomplete combustion 2C 3 H 8(g) + 7O 2(g)  6CO (g) + 8H 2 O (g)