1. Chem Catalyst 1) Balance the following: Cu(s) + S(s)  Cu 2 S(s) Be(s)+ O 2 (g)  BeO(s) K(s) + Cl 2 (g)  KCl(s) 2) What do these equations have in common?

2. Today’s Agenda: 1. Catalyst 2. Notes: Types of Chemical Reactions 3. Reaction analogies 4. P. 339 #24

3. Unit 5: Chemical Reactions BIG Questions 1. How does a chemical equation represent a chemical reaction? 2. Why do chemical reactions occur? 3. Why is balance essential when working with chemical reactions?

4. Combination (Synthesis) - Two or more substances combine to form a single compound - A + B  AB - 2 Reactants, 1 Product - Ex: 2 Zn + O 2  2 ZnO

5. Decomposition Reaction - A single compound splits into two (or more) substances - XY  X + Y - 1 Reactant, 2 Products - Ex: 2HgO (s)  2Hg(l) + O 2 (g)

6. Single-Replacement Reaction - An element replaces one of the ions in an ionic compound - A + BC  AC + B - 2 Reactants, 2 Products - Ex: Cu(s) + AgNO 3 (aq)  Ag(s)+ CuNO 3 (aq)

7. Double-Replacement Reaction - Ionic compounds exchange cations to form new ionic compounds - AB + XY  AY + XB - 2 Reactants, 2 Products - Ex: FeCl 3 + 3 NaOH  Fe(OH) 3 + 3 NaCl

8. Combustion - A hydrocarbon reacts with oxygen to form carbon dioxide and water - C x H y O z + O 2  CO 2 + H 2 O - 2 Reactants (hydrocarbon & O 2 ), 2 Products (CO 2, H 2 O) - Ex: C 2 H 5 O (l) + O 2 (g)  CO 2 (g) + H 2 O (l)

9. Examples: 2 C 8 H 18 (l) + 25 O 2 (g)  16 CO 2 (g) + 18 H 2 O (l) 2HgO(s)  2Hg(l)+ O 2 (g) CaI 2 + Hg(NO 3 ) 2  HgI 2 + Ca(NO 3 ) 2 2Mg + O 2  2MgO Fe(s) + Pb(NO 3 ) 2 (aq)  Pb(s) + Fe(NO 3 ) 2 (aq)