1. Chemical Reactions

2. PARTS OF A CHEMICAL EQUATION 2Mg + O 2  2MgO ReactantsProducts Coefficient “Produces Yields Forms” Subscript

3. TYPES OF CHEMICAL REACTIONS

4. SYNTHESIS REACTION When two or more substances combine to form ONE product A + B  AB Ex. H 2 + O 2  H 2 O

5. DECOMPOSITION When ONE substance breaks down into simpler substances AB  A + B Binary Ex. H 2 O  H 2 + O 2

6. Decompostion-Ternary (polyatomics) Metal Carbonates  metal oxide + carbon dioxide CaCO 3  CaO + CO 2 Metal Chlorates  metal chloride + oxygen KClO 3  KCl + O 2 Metal Hydroxides  metal oxide + water Ca(OH) 2  CaO + H 2 O Metal Sulfates  metal oxide + sulfur trioxide gas Cu(SO) 4  CuO + SO 3

7. SINGLE REPLACEMENT Think – “Single Man” A single element replaces another element in a compound A + BC  B + AC

8. SINGLE REPLACEMENT (continued) Examples: Li + CaCl 2  Ca + LiCl Cl 2 + MgBr 2  Br 2 + Mg Cl 2

9. SINGLE REPLACEMENT (continued) Balanced Examples: 2Li + CaCl 2  Ca + 2LiCl - NOTE: LIKE can only replace LIKE Cl 2 + MgBr 2  Br 2 + Mg Cl 2 - NOTE: LIKE can only reploace LIKE

10. DOUBLE REPLACEMENT Think: “2 compounds = double” AB + CD  CB + AD Only with ionic compounds NOTE: + ions can only “kick out” other + ions - ions can only “kick out” other - ions

11. Double Replacement (continued) Example: Kl + Pb(NO 3 ) 2  KNO 3 + PbI 2 Remember: Like can only replace like! Balanced example: 2Kl + Pb(NO 3 ) 2  2KNO 3 + PbI 2

12. COMBUSTION A hydrocarbon C x H y reacts with oxygen (O 2 )to form carbon dioxide and water CH 4 + O 2  CO 2 + H 2 O

13. COMBUSTION (continued) Balanced examples: 2Mg + O 2  2MgO CH 4 + 2O 2  CO 2 + 2H 2 O

14. NEUTRALIZATION Reaction between an ACID and a BASE A salt and water are formed as products Ex. HCl + NaOH  NaCl + H 2 O acid base saltwater