1. Organize these equation into types: Which #’s seem to describe similar patterns? 1) 2 HCl → H 2 + Cl 2 1) 2 HCl → H 2 + Cl 2 2) 2 K + Br 2 → 2 KBr 2) 2 K + Br 2 → 2 KBr 3) CH 4 + 2 O 2 → CO 2 +2 H 2 O 3) CH 4 + 2 O 2 → CO 2 +2 H 2 O 4) 2Al + 3 F 2  2 AlF 3 4) 2Al + 3 F 2  2 AlF 3 5) 2 NI 3 (s)  N 2 + 3 I 2 5) 2 NI 3 (s)  N 2 + 3 I 2 6) 2 C 2 H 6 +7 O 2 → 4 CO 2 +6 H 2 O 6) 2 C 2 H 6 +7 O 2 → 4 CO 2 +6 H 2 O

2. Reactions Problem Set For the 6 reaction types in Unit 3, this problem set will include: Notes A Demo Practice Problems It is vital for understanding this unit!

3. Homework 3-3 SynthesisNotes: A + B  C element + element  compound element + element  compound Use periodic table to determine charges of elements. Use periodic table to determine charges of elements. Write product using criss-cross or balancing of charges to determine subscripts. Write product using criss-cross or balancing of charges to determine subscripts. Balance equation. Balance equation.

4. Demo:Al (s) + I 2 (s)  Video Link Video Link 1) Na (s) + O 2 (g)  2) Al (s) + F 2 (g) 

5. 3) Sr (s) + O 2 (g)  4) K (s) + S 8 (s)  5) Na (s) + N 2 (g) 

6. What synthesis reaction is depicted below? Note the two diatomic reactants: Note the two diatomic reactants: oxygen and hydrogen.

7. DecompositionNotes: C  A + B compound  element + element compound  element + element Reactants will consist of just one compound. Reactants will consist of just one compound. Write compound’s elements as the products. Write compound’s elements as the products. Remember the 7 diatomics! Remember the 7 diatomics! Balance the equation. Balance the equation.

8. Demo:NI 3 (s)  Video Link Video Link Video Link

9. 6) AlCl 3 (l)  7) HgO (s)  8) H 2 O (l)  9) Al 2 O 3 (s)  10) FeBr 3 (s) 

10. CombustionNotes: C x H y ( or C x H y O z ) + O 2  CO 2 + H 2 O Rapid burning; one of the reactants will be O 2. Rapid burning; one of the reactants will be O 2. For hydrocarbons (see above), the products are For hydrocarbons (see above), the products are CO 2 + H 2 O CO 2 + H 2 O

11. Example: CH 4 + O 2 Video link Video link Video link Video link CH 4 + O 2 → CO 2 + H 2 O CH 4 + O 2 → CO 2 + H 2 O CH 4 + O 2 → CO 2 +2 H 2 O CH 4 + O 2 → CO 2 +2 H 2 O CH 4 + 2 O 2 → CO 2 +2 H 2 O CH 4 + 2 O 2 → CO 2 +2 H 2 O

12. 11) C 2 H 4 O 2 (l) + O 2 (g)  12) C 6 H 12 O 6 (g) + O 2 (g)  13) C 2 H 2 (g) + O 2 (g)  14) C 2 H 6 (g) + O 2 (g) 