1. Add to table of contents: Naming FlowchartPg. 46 Chemical nomenclaturePg. 47 Naming IonicPg. 48 Naming acidsPg. 49 % comp gum labPg. 50 Chemical ReactionsPg. 51 Classifying reactionsPg. 52 Types of Chemical ReactionsPg. 53

2. Types of Chemical Reactions

3. Spontaneous reactions—occur naturally, the process is unaided. Example: – Decomposition of dead matter = spontaneous endothermic reactions. (absorbs heat energy) – Forest fire = spontaneous exothermic reactions. (releases heat energy)

4. Non-spontaneous reactions—can only occur when linked to an energy source. Example: – Striking a match book: Match: head contains KClO 3 Book: sand paper strip contains phosphorus. *Need energy (to strike the match for it to light!)

5. Reaction Types

6. Synthesis (Combination) Reactions the combination of 2 or more substances to form a compound only one product A + B  AB

7. Synthesis (Combination) Reactions Examples: N 2 (g) + 3 H 2 (g)  2 NH 3 (g) C 3 H 6 (g) + Br 2 (l)  C 3 H 6 Br 2 (l) 2 Mg (s) + O 2 (g)  2 MgO (s) Two or more substances react to form one product

8. 2 Mg (s) + O 2 (g)  2 MgO (s)

9. Decomposition Reactions a compound breaks down into 2 or more simpler substances only one reactant AB  A + B

10. Decomposition Reactions Examples: CaCO 3 (s)  CaO (s) + CO 2 (g) 2 KClO 3 (s)  2 KCl (s) + O 2 (g) 2 NaN 3 (s)  2 Na (s) + 3 N 2 (g) One substance breaks down into two or more substances

11. Combustion Reactions CH 4(g) + 2O 2(g)  CO 2(g) + 2H 2 O (g) the burning of any substance in O 2 to produce heat A + O 2  CO 2 +H 2 O

12. Combustion Reactions Examples: CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O (g) C 3 H 8 (g) + 5 O 2 (g)  3 CO 2 (g) + 4 H 2 O (g) Rapid reactions that produce a flame Most often involve hydrocarbons reacting with oxygen in the air

13. Whoosh Bottle Demo is a Combustion Reaction 13

14. C. Johannesson Single Replacement one element replaces another in a compound – metal replaces metal (+) – nonmetal replaces nonmetal (-) A + BC  B + AC

15. C. Johannesson Single Replacement Cu (s) + 2AgNO 3(aq)  Cu(NO 3 ) 2(aq) + 2Ag (s)

16. C. Johannesson AB + CD  AD + CB Double Replacement ions in two compounds “change partners” cation of one compound combines with anion of the other

17. C. Johannesson Double Replacement Pb(NO 3 ) 2(aq) + K 2 CrO 4(aq)  PbCrO 4(s) + 2KNO 3(aq)

18. 18 Practice—Classify the Following Reactions as Synthesis, Decomposition, Single Replacement, or Double Replacement. 3 Mg(s) + 2 FeCl 3 (aq)  3 MgCl 2 (aq) + 2 Fe(s) CO 2 (g) + H 2 O(l)  H 2 CO 3 (aq) 3 KOH(aq) + H 3 PO 4 (aq)  K 3 PO 4 (aq) + 3 H 2 O(l) Single Replacement. Double Replacement. Decomposition. Synthesis.