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Download Unit 14.1 REDOX Reactions Objectives REDOX Reactions
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Transcript
Unit 14.1 REDOX Reactions Teacher: Dr. Van Der Sluys Objectives • REDOX – Oxidation – Reduction – Oxidizing agent – Reducing agent REDOX Reactions • REDOX reactions involve the transfer of electrons from one species to another. • A REDOX reaction involves both an oxidation of one species and a reduction of another. • REDOX reactions can be used to convert chemical potential energy into electrical energy. 1 Oxidation • A loss of electrons • An increase in the oxidation number • A half-reaction in which the electrons are products. Reduction • A gain of electrons • A decrease in the oxidation number • A half-reaction in which electrons are a reactant. Identifying the Oxidized and Reduced Species • Determine the oxidation number of an element on both the reactant and product side of the reaction. If the oxidation number increases, the atom was oxidized. Cu (s) + 2 AgNO3 (aq) --> Cu(NO3) 2 (aq) + 2 Ag (s) • Elemental copper has a zero oxidation state as a reactant, which increases to 2+ in the product Cu(NO3)2, hence the copper is oxidized. • The reactant AgNO3 has silver in the +1 oxidation state, which is reduced to 0 in the product, elemental silver. 2 Examples - Net Ionic Equations • Identify the species that is oxidized and reduced in the following. 2 Fe3+ (aq) + Zn (s) --> 2 Fe2+ (aq) + Zn2+ (aq) 4 H+ (aq) + MnO4- (aq) + Co2+ (aq) --> MnO2 (s) + Co3+ (aq) + 2 H2 O (l) 2 Cl- (aq) + F2 --> Cl2 (g) + 2 F - (aq) Examples - Molecular Formulas 2 H2 (g) + O2 (g) --> 2 H2O (l) 2 H2SO4 (aq) + 2 NaBr (aq) --> Br2 (l) + SO2 (g) + Na2SO4 (aq) + 2 H2O (l) I2O5 (s) + 5 CO (g) --> I2 (s) + 5 CO5 (g) Oxidizing and Reducing Agents • An oxidizing agent is the species that gets reduced in a REDOX reaction • A reducing agent is the species that gets oxidized in a REDOX reaction. 3 Examples - Identifying the Oxidizing and Reduxing Agents Cr2O7 2- (aq) + 14 H+ (aq) + 6 I- (aq) --> 2 Cr3+ (aq) + 3 I2 (s) + 7 H2O (l) Zn (s) + 2 H+ (aq) --> Zn2+ (aq) + H2 (g) 16 H+ (aq) + 2 MnO4 - (aq) + 5 C2O4 2- (aq) --> 2 Mn2+ (aq) + 8 H2O (l) + 10 CO2 (g) Conclusion • REDOX reactions involve oxidation and reduction and occur by the transfer of electrons from the reducing agent to the oxidizing agent. 4
