Types of reactions

AgNO3 (aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq) Double Replacement A rxn in which the cations switch places. AB + CD  CB + AD Precipitate rxns – formation of a solid Silver nitrate + sodium chloride  AgNO3 (aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq) silver chloride + sodium nitrate

B) Neutralization Rxns Any ionic compound Acid + base  water + salt HCl (aq) + NaOH(aq)  H2O(l) + NaCl(aq) Special case: Acid plus carbonate, CO3 2- HCl(aq) NaHCO3(s)  H2O(l) + NaCl(aq) + CO2(g) Bubbles as additional product

Oxidation-Reduction Rxns (Redox) This a rxn in which elements change their charges. Oxidation – become more positive Pb (s)  Pb 2+ (aq) + 2 e- Reduction – become more negative Cl2(g) + 2 e-  2 Cl– (aq) All elements are neutral +2 Ions just match their charge -1

Decomposition When one reactant decomposes into 2 or more products. AB  A + B Example: Nitrogen triiodide  nitrogen + iodine 2 NI3 (s)  N2 (g) + 3 I2 (g) Ox: I (-1 to 0) Red: N (+3 to 0) +3 -1 (-3)

Single Replacement A rxn in which an element replaces another element in a compound. A + BC  AC + B (if A is a would be cation) D + EF  ED + F (If D is a would be anion) Zinc + hydrochoric acid  ????? Zn(s) + HCl(aq)  2 ZnCl2(aq) + H2(g) +1 -1 +2 -1 So is the Zn going to have a positive or negative charge when it becomes an ion? Ox: Zn (0 to +2) Red: H (+1 to 0) +

Combination A + B  AB2 Hydrogen + oxygen  ???? 2 or more reactants combine to for a single product. A + B  AB2 Hydrogen + oxygen  ???? 2 H2(g) + O2(g)  2 H2O(g) -2 +1 Ox: H (0 to +1) Red: O (0 to -2)

Combustion The burning of a hydrocarbon to produce carbon dioxide and water. Butane + oxygen  2 C4H10(g) + 13 O2(g)  8 CO2(g) + 10 H2O(g) Balance the C’s first, H’s second and O’s last. You need to have the 2 in front of butane because you are not allowed to half fractions.