We will study 5 types of reactions Decomposition Synthesis Combustion Single-Replacement Double-Replacement

Decomposition Reactions (split) One substance breaks into 2 or more substances AB  A + B Examples H2O  MgCl2  Mg (s) + Cl2(g)

Synthesis Reactions (combine) 2 reactants  1 product A + B  AB Examples Na + Cl2  Fe + O2 

Combustion reactions A substance combines with oxygen and produces heat/energy There are 2 types combustion reactions Synthesis metal plus oxygen  oxide Mg + O2  Fuel + O2  CO2 + H2O C2H6 + O2  CO2 + H2O CxHy coefficient is 1 for odd x and 2 for even x

Practice 1) predict product 2) type of reaction 3) balance the equation Hydrogen (g) + chlorine (g)  Decane (C10H22) (l) + oxygen (g)  Magnesium chlorate (s)  Iron (III) + oxygen (g) 

Single displacement reactions Atoms of an element switch places with atoms of another element in a compound. A + BX  AX + B Not all replacements are possible The single element must be higher on the activity series than the element in the compound

Underline the element that would replace the other in a single replacement reaction. a. calcium, tin b. bromine, fluorine c. aluminum, potassium d. zinc, sodium e. iron, copper f. iodine, chlorine g. silver, lead

Single Replacement (displacement) reactions Al (s) + CuCl2  Cu + NaCl  Zn + SnCl2  K (s) + ZnCl2 (aq)  Cl2 (g) + HF (aq)  Pb (s) + H2O (aq) 

Double (displacement) Replacement Exchange of ions between 2 compounds AX + BY  AY + BX Can form a precipitate (solid), determined by solubility rules PbSO4 + HCl  Hg(NO3)2 + KI 

Classify These Reactions 1) CH4 (g) + O2 (g)  CO2 (g) + H2O (l) 2) Mg (s) + AlCl3(aq)  Al (s) + MgCl2(aq) 3) Al (s) + S (s)  Al2S3 (s) 4) H2 (g) + O2(g)  H2O (g) 5) F2(g) + NaBr(aq)  NaF (aq) + Br2 (l) 6) NaN3 (s)  Na (s) + N2 (g)