1. Oxidation- Reduction Topic 9 Review Book

2. Oxidation Numbers Oxidation is the loss of electrons; Reduction is the gain of electrons Oxidation and reduction go together. Whenever a substance loses electrons and another substance gains electrons Oxidation Numbers are a system that we can use to keep track of electron transfers

3. LEO says Loss of Electrons = Oxidation Gain of Electrons = R eduction GER!

4. Rules for Assigning Oxidation Numbers Free elements are 0 Ions have the charge indicated Metals : Group 1 = +1; Group 2= +2 Hydrogen is +1 unless in binary compound with metal, then it is -1 Halogens in binary compounds are usually -1, in ternary compounds move on and go back to do the algebra Oxygen is -2 unless in peroxide when it is -1 or with fluorine when it is +2 (FIMHHO)

5. Practice Assigning Oxidation Numbers NO 2 N2O5N2O5 HClO 3 HNO 3 Ca(NO 3 ) 2 KMnO 4

6. Practice Assigning Oxidation Numbers NO 2 N= +4, O = -2 N2O5N2O5 N = +5, O = -2 HClO 3 H=+1, Cl=+5, O = -2 HNO 3 H=+1, N = +5, O = -2 Ca(NO 3 ) 2 Ca=+2, N =+5, O= -2 KMnO 4 K=+1, Mn=+7, O= -2

7. Practice Assigning Oxidation Numbers CaCl 2 K 2 Cr 2 O 7 KH NaHCO 3 H2OH2O MgO

8. Practice Assigning Oxidation Numbers CaCl 2 Ca = +2, Cl = -1 K 2 Cr 2 O 7 K=+1, Cr=+6, O=-2 KH K = +1, H= -1 NaHCO 3 Na= +1, H= +1, C=+4, O= -2 H 2 O H= +1, O= -2 MgO Mg = +2, O = -2

9. Using Oxidation Numbers Careful examination of the oxidation numbers of atoms in an equation allows us to determine what is oxidized and what is reduced in an oxidation-reduction reaction

10. Using Oxidation Numbers An increase in the oxidation number indicates that an atom has lost electrons and therefore oxidized. A decrease in the oxidation number indicates that an atom has gained electrons and therefore reduced Example Mg + ZnSO 4  MgSO 4 + Zn

11. Exercise For each of the following reactions find the element oxidized and the element reduced Cl 2 + KBr  KCl + Br 2 Mg + HNO 3  Mg(NO 3 ) 2 + NO 2 + H 2 O HNO 3 + I 2  HIO 3 + NO 2

12. Exercise For each of the following reactions find the element oxidized and the element reduced Cl 2 + KBr  KCl + Br 2 Br increases from –1 to 0 -- oxidized Cl decreases from 0 to –1 -- Reduced K remains unchanged at +1

13. Exercise For each of the following reactions find the element oxidized and the element reduced Mg + HNO 3  Mg(NO 3 ) 2 + NO 2 + H 2 O Cu increases from 0 to +2. It is oxidized Only part of the N in nitric acid changes from +5 to +4. It is reduced The nitrogen that ends up in copper nitrate remains unchanged

14. Exercise For each of the following reactions find the element oxidized and the element reduced HNO 3 + I 2  HIO 3 + NO 2 N is reduced from +5 to +4. It is reduced I is increased from 0 to +5 It is oxidized The hydrogen and oxygen remain unchanged.

15. Balancing Redox Reactions There are several basic steps 1.Assign oxidation numbers to the species in the reaction 2.Find the substance oxidized and the substance reduced 3.Write half reactions for the oxidation and reduction 4.Balance the atoms that change in the half reaction 5.Determine the electrons transferred and balance the electrons between the half reactions 6.Check your work. Make sure that both the atoms and charges balance

16. Balancing Redox Equations 1 Zn + HCl  ZnCl 2 + H 2 1.Assign oxidation numbers to the species in the reaction 2.Find the substance oxidized and the substance reduced 3.Write half reactions for the oxidation and reduction 4.Balance the atoms that change in the half reaction 5.Determine the electrons transferred and balance the electrons between the half reactions 6.Check your work. Make sure that both the atoms and charges balance *It may be helpful to balance the equation before starting the redox process

17. Balancing Redox Equations 2 MnO 2 + HCl  MnCl 2 + Cl 2 + H 2 O 1.Assign oxidation numbers to the species in the reaction 2.Find the substance oxidized and the substance reduced 3.Write half reactions for the oxidation and reduction 4.Balance the atoms that change in the half reaction 5.Determine the electrons transferred and balance the electrons between the half reactions 6.Check your work. Make sure that both the atoms and charges balance

18. Balance, Assign, ID, write ½ rxns for the following 1. Mg + O 2  MgO 2. KClO 3  KCl + O 2 3. HCl + O 2  H 2 O + Cl 2

19. Balance the following ionic equations ____Cr +6 + ____ S  ___ Cr +3 +____ S +4 ____Sn 2+ + ____Hg + 2  ___Sn +4 + ___Hg +1 _____Cu + _____Ag +1  ___Cu +2 + ___Ag