Oxidation & Reduction
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1 Oxidation & Reduction Definition of Redox Reaction Oxidation Reduction Reaction (Redox): A reaction in which electrons are from one substance to another. Definition of Redox Reaction Oxidation cannot occur without Definition of Oxidized: 1. Losing of (LEO) 2. Increasing the oxidation charge, ie: 0 to +1 2 to 1 3. Gaining Definition of Reduced: 1. of electrons (GER) 2. Reducing the oxidation charge, ie: 1 to 2 1 to 0 3. Losing Example of an electron transfer reaction 2Mg + O 2 2MgO Mg atom two electrons to each oxygen atom. As a result 2 Mg atoms become Mg 2+ and two oxygen atoms become Mg two electrons O two electrons Examples of Oxidation Reduction When an electron is (An electron is found on the product side) there is X 0 X +1 + e When an electron is (An electron is found on the reactant side) there is e +Y +1 Y 0 1
2 Examples: start finish Oxidation or Reduction Ex5 Na 0 Na +1 Ex6 Fe +3 Fe +2 Ex7 N +1 N +2 Ex8 Mg +2 Mg 0 Vocabulary Whatever is is called the reducing agent Whatever is is called the oxidizing agent Real Examples: start finish Oxidizing agent or reducing agent Ex5 Na 0 Na +1 Ex6 Fe +3 Fe +2 Ex7 N +1 N +2 Ex8 Mg +2 Mg 0 1. What is a redox reaction? Redox Homework #1: 2. Can oxidation occur without reduction? Explain. 3. Define oxidation and reduction in terms of the gain or loss of oxygen. 4. Define oxidation and reduction in terms of the gain or loss of electrons. 5. How is a change in oxidation number related to the process of oxidation and reduction? 2
3 HalfReactions for Oxidation/Reduction A halfreaction is an equation just showing just the oxidation or just the reduction reaction that takes place in a redox reaction. State whether the halfreaction is oxidation or reduction. 6. K + +e K 7. Ca Ca e 8. 2Br Br 2 + 2e 9. S + 2e S F 2 + 2e 2F Write where the electron(s) is lost or gained. Then determine if each equation is oxidation or reduction. 11. Na Na Mg 2+ Mg 13. K K Fe 2+ Fe Ag + Ag 16. I 2 2I 17. Zn 2+ Zn 18. 2F F Al 3+ Al 20. Cl 2 2Cl Redox Rules: Redox Rules to Learn for Ionic and Covalent Bonds Electronegativity and Redox Rules Definition: Electronegativity is the atom s ability to electrons. is the most electronegative element Electronegativity Trend EN More protons to attract electrons EN electrons get further away from protons 3
4 Rule #1 Oxidation number of an atom = zero (no compounds or ions) i.e. Mg, H 2, Na ie. All H 2 O 2 N 2 Cl 2 Br 2 I 2 F 2 s ox. # are zero Rule #2 Oxidation number of a ion = charge of the ion i.e. Mg 2+, O 2, Al 3+, Br Rule #3 The sum of the oxidation numbers of a compound = 0 i.e. H 2O CO 2 CO NaCl Rule #4 The oxidation number for H is Exception: when bonded to a electronegative element (metal), then it is. i.e. LiH NaH MgH 2 i.e. HF Cl Rule#5 Oxygen s oxidation number is, in a compound Two exceptions: peroxides and fluorine in H 2O 2 with OF 2 where O is where O is Rule#6 Oxidation number of polyatomic = 0 (same as rule #3) polyatomic = the charge of the ion i.e. compounds: i.e. ions: NH 3 SiCl 4 K 3PO 4 NH 4 + CO 3 2 SO 4 2 NO 3 4
5 Rule#7 Oxidation numbers for in: Group 1A metal compound +1 2A metal compound +2 3A Aluminum compound+ +3 i.e. NaCl MgSO 4 AlPO 4 Rule#8 The most electronegative element ALWAYS has an oxidation number of 1 when it is bonded to another element. i.e. HF Question Time Assign oxidation numbers to each element 1. Cl 2 2. Cl 3. MgCl 2 4. NaH 5. HCl 6. K 3PO 4 7. CaSO 4 8. KF Classwork: Redox Rules 1. Give the oxidation numbers of all the elements in the following molecules and ions: a. N 2 O b. NO c. N 2 O 4 d. N 2 O 5 e. NO 2 f. NO 3 2. Determine the oxidation number of the sulfur atom: a. H 2 S b. S c. H 2 SO 4 d. S 2 e. HS f. SO 2 g. SO 3 3. Indicate the oxidation number of phosphorus in each of the following compounds: a. HPO 3 b. H 3 PO 2 c. H 3 PO 3 d. H 3 PO 4 e. H 4 P 2 O 7 f. H 5 P 3 O 10 5
6 Redox Homework #2: Oxidation Numbers and Rules Worksheet The oxidation number of an atom is the apparent charge assigned to it in a particular molecule, ion or compound. Certain rules are followed in assigning oxidation numbers. Use rules at the right to assign oxidation numbers to each element in each of the given formulas. Example OXIDATION NUMBER H2O H=+1, O= 2 N2 N=0 OXIDATION NUMBER 1. Cl2 2. Cl 3. Na 4. Na + 5. KCl 6. H2S 7. CaO 8. H2SO4 9. NO3 10. Cr2O NH4Cl 12. NH3 13. NO2 14. CaH2 (calcium hydride) 15. Na2O2 (sodium peroxide) Rule #1: Oxidation number of an uncombined atom = zero (no compounds or ions) Rule #2: Oxidation number of a monatomic ion = charge of the ion Rule #3: The sum of the oxidation numbers of a neutral compound = 0 Rule #4: The oxidation number for H is +1 except when bonded to a less electronegative element (metal), then it is 1. Rule#5: Oxygen s oxidation number is 2, 2 exceptions: peroxides and fluorine Rule#6: Oxidation number of polyatomic compound = zero, polyatomic ion = the charge of the ion Oxidation Number Rules Rule#7: Oxidation numbers for metals in: Group 1A metal compound= +1, 2A metal compound= +2, 3A metal compound= +3 Rule#8: The most electronegative element fluorine ALWAYS has an oxidation number of 1 when it is bonded to another element. Cw: Give oxidation numbers for the underlined atoms in these molecules and ions: a. Cs 2 O f. ClF 3 k. MoO 2 4 b. PtCl 6 2 g. H 3 AsO 3 l. MnO 4 c. CaI 2 h. SbF 6 m. PtCl 4 2 d. SnF 2 i. TiO 2 n. O 2 e. Al 2 O 3 j. P 4 o. O 3 6
7 Redox Homework #3: Oxidation Numbers Worksheet Directions: Use the Rules for Assigning Oxidation Numbers to determine the oxidation number assigned to each element in each of the given chemical formulas. Formula Element and Oxidation Number Formula Element and Oxidation Number 1. Cl 2 Cl 16. Na 2O 2 Na O 2. Cl Cl 17. SiO 2 Si O 3. Na Na 18. CaCl 2 Ca Cl 4. Na + Na PO 4 P O 5. O 2 O 20. MnO 2 Mn O 6. N 2 N 21. FeO Fe O 7. Al +3 Al 22. Fe 2O 3 Fe O 8. H 2O H O 23. H 2O 2 H O 9. NO 3 N O 24. CaO Ca O 10. NO 2 N O 25. H 2S H S 11. Cr 2O 2 7 Cr O 26. H 2SO 4 H S O 12. KCl K Cl 27. NH 4Cl N H Cl 13. NH 3 N H 28. K 3PO 4 K P O 14. CaH 2 Ca H 29. HNO 3 H N O SO 4 S O 30. KNO 2 K N O NT: Using the Rules (Last Lesson of the Year!) Oxidation Number If oxidation number goes it is. If oxidation number goes it is. Using the Rules Balance the reactions, write the oxidation numbers for each atom and write the oxidizing and reducing agents. Ex1 HCl + Zn ZnCl 2 + H 2 Ex2 Mg + N 2 Mg 3N 2 Ex3 H 2S + Cl 2 HCl + S Ex4 Fe + O 2 Fe 2O 3 7
8 Summary of Oxidation/Reduction There are three definitions of oxidation and reduction: Oxidation Reduction Two ways to remember oxidation/reduction is: L E O goes G E R or O I L R I G Classwork: Using Rules to Balance Equations Assign oxidation numbers for each element. Then, for the following balanced redox reactions answer the following questions: 1) Fe(aq) + H2O2(aq) Fe +2 (aq) + 2 OH 1 (aq) a. What is the oxidation state of oxygen in H2O2? b. What is the element that is oxidized? c. What is the element that is reduced? d. What is the oxidizing agent? e. What is the reducing agent? f. How many electrons are transferred in the reaction as it is balanced? 2) 4NaOH(aq) + Ca(OH)2(aq) + C(s) + 4ClO2(g) 4NaClO2(aq) + CaCO3(s) + 3H2O(l) a. What is the oxidation state of Cl in ClO2(g)? b. What is the oxidation state of C in C(s)? c. What is the element that is oxidized? d. What is the element that is reduced? e. What is the oxidizing agent? f. What is the reducing agent? g. How many electrons are transferred in the reaction as it is balanced? 8
9 3) 16 HCl(aq) + 5 SnCl2(aq) + 2 KMnO4(aq) 2 MnCl2(aq) 5 SnCl4(aq) + 8 H2O(l) + 2 KCl(aq) a. What is the oxidation state of Mn in KMnO4(aq)? b. What is the oxidation state of Sn in SnCl2(aq)? c. What is the element that is oxidized? d. What is the element that is reduced? e. What is the oxidizing agent? f. What is the reducing agent? g. How many electrons are transferred in the reaction as it is balanced? Redox Homework #4: Using Rules to Balance Equations Balance each equation. Assign oxidation numbers to each atom. Determine what is oxidized/reducing agent and what is reduced/oxidizing agent. Tell the number of electrons transferred. 1. Na + Cl 2 NaCl Oxidized (Reducing Agent) 2. C + O 2 CO 2 Oxidized (Reducing Agent) 3. Zn + CuSO 4 ZnSO 4 + Cu Oxidized (Reducing Agent) 4. Fe + O 2 + H 2 O Fe(OH) 2 Oxidized (Reducing Agent) 5. Cu + H 2 SO 4 CuSO 4 + SO 2 + H 2 O Oxidized (Reducing Agent) 6. Mg + HCl MgCl 2 + H 2 Oxidized (Reducing Agent) 9
10 Redox Homework #5: (Extra Practice) Assign oxidation numbers to each atom. Determine what is oxidized/reducing agent and what is reduced/oxidizing agent. Tell the number of electrons transferred. 1) 2 Na + FeCl 2 2 NaCl + Fe Oxidized (Reducing Agent) 2) 2 C 2H O 2 4 CO H 2O Oxidized (Reducing Agent) 3) 2 PbS + 3 O 2 2 SO PbO Oxidized (Reducing Agent) 4) 2 H 2 + O 2 2 H 2O Oxidized (Reducing Agent) 5) Cu + HNO 3 CuNO 3 + H 2 Oxidized (Reducing Agent) 6) AgNO 3 + Cu CuNO 3 + Ag Oxidized (Reducing Agent) 10
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