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REDOX REACTION

CHAPTER 6. REDOX REACTION. REAKSI REDOKS. Teaching Learning Objectivers. The student can explain definition of redox reactions the first concept (the release and uptake of atoms concept) The student can explain definition of redox reactions the secon concept (the electrons transfer concept)

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REDOX REACTION

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  1. CHAPTER 6 REDOX REACTION REAKSI REDOKS

  2. Teaching Learning Objectivers • The student can explain definition of redox reactions the first concept (the release and uptake of atoms concept) • The student can explain definition of redox reactions the secon concept (the electrons transfer concept) • The student can explain definition of redox reactions the third concept (the change in oxidation number concept)

  3. 1.The First Redox Concept,The Release and Uptake of Oxygen atoms Concept • Oxidation reaction is subtance uptakes an oxygen molecule on the reaction. Example : Na(s) + O2(g)→ Na2O(s) 4 2 Cl2(g) + O2(g) → Cl2O3(g) 2 3 2 2 4 FeS2(s)+ O2(g)→ Fe2O3(s) + SO2(g) 11 8 2 C2H2(g) + O2(g) → CO2(g) + H2O 5 4 2

  4. Reduction reaction is subtance releases an oxygen molecule on the reaction. Example : 2 HgO(s)→ Hg(s)+ O2(g) 2 2 KClO3(s)→ KCl(s)+ O2(g) 2 3 6 CO2(g)+ H2O(l)→C6H12O6(s)+ O2(g) 6 6 3 2 Fe2O3(s)+ C(s)→ Fe(s)+ CO2(g) 4 3

  5. 2.The Second Redox Cncept,The Electrons Transfer Concept • Oxidation reaction is refers to the loss of electrons. Example : 11Na Na+ + e Na → Na+ + e 2 8 1 2 8 12Mg Mg2+ + 2e Mg → Mg+2 + 2e 2 8 2 2 8

  6. Reduction reaction is refers to the gain of electrons. Example : Cl2 + 2e 2Cl- 17Cl + e Cl- 2 8 7 2 8 8 8O + 2e O2- O2 + 4e 2O2- 2 6 2 8

  7. Reaksi oksidasi selalu diikuti reaksi reduksi : R. Oks: Na → Na+ + e 2Na →2Na+ +2 e x2 R. Red: Cl2+ 2e→2Cl- Cl2+ 2e→2Cl- x1 R.Redoks : 2Na + Cl2→2Na+ + 2Cl- 2NaCl R. Oks: Mg → Mg+2 + 2e 2Mg →2Mg+2 + 4e x2 R. Red: O2 + 4e→2O-2 x1 O2 + 4e → 2O-2 R.Redoks : 2Mg +O2 →2Mg+2 +2O-2 2MgO

  8. The oxidation numbers of free are zero The oxidation numbers of mono atomic ion are equals to its ionic charge, The sums of oxidation numbers of atoms in their coumpounds are zero. The sums oxidation numbers is poliatomic ions are equal to the charge of poliatomic ions. The oxidation numbers of group IA element in a compound is +1, while the oxidation numbers of group. IIA element in a compound is +2 6. The oxidation numbers of group VIIA element in a compound is -1. 7. The oxidation numbers of hydrogen atom in compound is +1, exept in metal hydride its the oxidation numbers is -1. 8. The oxidation numbers of oxygen atom in compound is -2, exept in peroxide, its oxidation numbers is -1. And the oxidation numbers in binary compound with flourine is +2. The Rules to determine the okxidation numbers

  9. The oxidation numbers of free are zero Example : Al BO = 0 F2 BO =0 S8 BO =0 Na BO = 0 2. The oxidation numbers of mono atomic ion are equals to its ionic charge, Example : O-2 BO = -2 Al+3 BO = +3 Cl- BO = -1 Na+ BO = +1 • 3. The sums of oxidation numbers of atoms in their coumpounds are zero. 5.The oxidationnumbers of group IA element in a compound is +1, while the oxidation numbers of group. IIA element in a compound is +2 6. The oxidation numbers of group VIIA element in a compound is -1. Example : NaCl MgBr2 Na +Cl = 0 Mg +2Br = 0 (+1) + (-1) = 0 (+2) + 2(-1) = 0

  10. 7.The oxidation numbers of hydrogen atom in compound is +1, exept in metal hydride its the oxidation numbers is -1. 8. The oxidation numbers of oxygen atom in compound is -2, exept in peroxide, its oxidation numbers is -1. Example : H2O Exept (7) : NaH Na + H = 0 2H + O = 0 (+1) + H = 0 2(+1) + (-2) = 0 H= -1 Exept (8) : CaH2 Ca + 2H = 0 (+2) + 2H = 0 H2O2 H= -1 2H + 2O = 0 2(+1) + 2O = 0 Na2O2 BaO2 2O = -2 O = -1

  11. 4.The sums oxidation numbers is poliatomic ions are equal to the charge of poliatomic ions. Example : Exept (6) : Gol VIIA yang mengandung atom O dalam senyawanya BO tidak -1 SO4-2 S + 4O = -2 KClO3 S + 4(-2) = -2 K + Cl + 3O = 0 S = -2 + 8 S = +6 (+1)+ Cl +3(-2) = 0 Cl = +5

  12. 3.The Third Redox Concept,The Change in Oxidation Number Concept • Oxidation reaction is the increasing oxidation number. • Reduction reaction is the decreasing oxidation number. • Oxidant : being reduced • Reductant : being oxidized Example: : 2Na + Cl2→2NaCl 0 0 +1 -1 R.Reduksi R.Oksidasi Cl2 Oksidator Na Reduktor

  13. Mg +2HCl → MgCl2 + H2 MgCl2 Hasil Oksidasi +1 -1 +2 -1 0 0 R. Oksidasi H2 Hasil reduksi R. Reduksi Mg Reduktor HCl Oksidator Cl2 + KOH→ KCl + KClO3 + H2O Reaksi Auto Redoks / Reaksi Disproporsionasi +1 -2 +1 +1 -1 +1 -2 0 +1 +5 -2 R. Oksidasi R. Reduksi KClO3 Hasil Oksidasi KCl Hasil reduksi

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