1. Types of Reactions Six Types

2. Single Replacement  A free element replaces one of the ions in a compound  A metal replaces a metal OR a nonmetal replaces a nonmetal  The single element replaces one of the ions in the solution and a new element appears from the ion in solution  Element + Compound yields element + compound

3. Examples  2 KI + Cl 2 → 2 KCl + I 2  2 AgNO 3 + Cu → Cu(NO 3 ) 2 + 2 Ag

4. Double Replacement  The cations switch places OR anions switch places  A metal replaces a metal AND a nonmetal replaces a nonmetal  Compound + Compound yields Compound + Compound

5. Examples  AgNO 3 + KCl → AgCl + KNO 3  Barium chloride + potassium sulfate yields barium sulfate + potassium chloride  Make sure to switch the names and then write the formula accordingly, balancing charges  BaCl 2 + K 2 SO 4 → BaSO 4 + 2 KCl

6. (Acid-Base) Neutralization  Special double displacement reaction  Acids: compounds that begin with hydrogen  Bases: compounds that end with hydroxide  Acid + hydroxide compound → Salt (ionic compound) + H 2 O

7. Example  HCl + NaOH → NaCl + H 2 O  NaCl is not the only salt!!!!  H 2 SO 4 + 2 NH 4 OH → (NH 4 ) 2 SO 4 + 2 H 2 O

8. Synthesis  Two elements or compounds come together to make a single product  A + B → AB  Element or compound + element or compound yields a single compound

9. Examples  2 H 2 + O 2 → 2 H 2 0  H 2 0 + SO 3 → H 2 SO 4

10. Decomposition  A coming apart; a single reactant comes apart into 2 or more products  AB → A + B  Compound yields two or more smaller substances (elements and/or compounds)

11. Examples  2 KClO 3 → 2 KCl + 3O 2  2 HgO → 2 Hg + O 2

12. Combustion (of hydrocarbon)  Hydrocarbon + oxygen → water + carbon dioxide  C x H y + O 2 → H 2 O + CO 2  Coefficients will change according to your hydrocarbon subscripts  C 6 H 12 + 9 O 2 → 6 H 2 O + 6 CO 2