1. Warm up 11-10-15 1. Why do we have to balance chemical equations? 2. Balance these chemical equations: a) Sb + O 2 → Sb 4 O 6 b) FeCl 3 + KF → KCl + FeF 3 c) HCl + CaCO 3 → H 2 O + CO 2 + CaCl 2 Agenda -Turn in Lab -Notes Unit 5-3 -One-on-One grade check -WS Practice Unit 5-3 Homework Dec 9 - Deadline for quiz retake

2. a) Sb + O 2 → Sb 4 O 6 b) FeCl 3 + KF → KCl + FeF 3 c) HCl + CaCO 3 → H 2 O + CO 2 + CaCl 2

3. Unit 5-3 Types of Chemical Reactions

4. Types of Chemical Reactions Synthesis or Combination A + B → AB Ex: 2Na (s) + Cl 2 (g) → 2NaCl (s) The love story

5. Types of Chemical Reactions Decomposition AB → A + B Ex: 2H 2 O → 2H 2 + O 2 The break-up

6. Types of Chemical Reactions Single Replacement or Single Displacement AX + B → BX + A Ex: CuSO 4 + Zn (s) → ZnSO 4 + Cu (s) The complication

7. Types of Chemical Reactions Double Replacement or Double Displacement AB + CD → CB + AD Ex: Pb(NO 3 ) 2 + 2KI → PbI 2 + 2KNO 3

8. Types of Chemical Reactions Combustion Carbon compound + O 2 → CO 2 + H 2 O Ex: CH 4 + 2O 2 → CO 2 + 2H 2 O

9. Check In Name the reaction type for the following equations: NH 3 + H 2 SO 4 → (NH 4 ) 2 SO 4 HgO → Hg + O 2 CH 4 + O 2 → H 2 O + CO 2 CuCl 2 + H 2 S → CuS + HCl BaCl 2 + Na 2 SO 4 → NaCl + BaSO 4 Synthesis Decomposition Combustion Double Replace.

10. Percent Yield Analysis of the efficiency for chemical reaction Percent Yield calculation

11. Percent Yield Theoretical yield – The maximum amount of products that can be formed in a reaction based on calculation

12. Percent Yield The actual yield – Real amount produced in a reaction (usually less than the expected theoretical yield).

13. Percent Yield Example A reaction should have produced 1.44g of MgO. After the experiment, only 1.23g of magnesium oxide was present. What is the percent yield?

14. Assignments Summary Practice Worksheet due next class One-on-One grade check