1. Section 4.4 Oxidation Reduction Reactions Redox Reactions Electron-Transfer Reactions

2. In this section: a.oxidation and reduction b.oxidation numbers c.recognizing redox reactions d.predicting redox reactions Not from this section: a. Organic reactions

3. Oxidation-Reduction Reactions Oxidation = loss of electrons Reduction = gain of electrons Zn(s) + Cu 2+ (aq)  Zn 2+ (aq) + Cu(s) Oxidation Half-Reaction: Zn(s)  Zn 2+ (aq) + 2 e - Reduction Half-Reaction: Cu 2+ (aq) + 2 e -  Cu(s)

4. Oxidation-Reduction Reactions Oxidation = loss of electrons Reduction = gain of electrons Zn(s) + Cu 2+ (aq)  Zn 2+ (aq) + Cu(s) Oxidizing agent = oxidant = gains electrons Reducing agent = reductant = loses electrons

5. Balancing Simple Redox Reactions Cu(s) + Ag + (aq)  Cu 2+ (aq) + 2 Ag(s)

6. Oxidation Numbers Electron tracking method. Oxidation numbers do not imply charges.

8. Examples: N in N 2 Fe in Fe 3+ N in NO 2 - O in H 2 O Cl in NaOCl Mn in MnO 4 -

9. Recognizing Oxidation-Reduction Reactions Oxidation = loss of electrons = increase in ox # Reduction = gain of electrons = decrease in ox # 4 Fe + 3 O 2  2 Fe 2 O 3

10. CuO(s) + H 2 (g)  Cu(s) + H 2 O( ) CaCO 3 (s)  CaO(s) + CO 2 (g)

11. MnO 4 - (aq) + 5 Fe 2+ (aq) + 8 H + (aq)  Mn 2+ (aq) + 4 H 2 O( ) + 5 Fe 3+ (aq)

12. Predicting Redox Reactions

13. Organic Reactions A. Combustion Reactions Reaction with oxygen gas to form CO 2 and H 2 O. C 3 H 8 (g) + 5 O 2 (g)  3 CO 2 (g) + 4 H 2 O(l) B. Substitution Reactions Exchange of one atom or molecular fragment.

14. C. Addition Reactions Addition of two molecules together. D. Elimination Reactions Ejection of a small molecule from a larger one.

15. E. Isomerization (Rearrangement) Reactions Change of shape of a molecule without gain or loss of any atoms.