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Ch 4_Lecture 13_020612

Ch 4_Lecture 13_020612 - 1 Demo Activity Series Mg(s 2...

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Unformatted text preview: 2/6/2012 1 Demo: Activity Series Mg(s) + 2 HCl(aq) → Mg 2+ (aq) + 2 Cl – (aq) + H 2 (g). Mg is a very active metal (reduces H in both water and acid). Zn(s) + 2 HCl(aq) → Zn 2+ (aq) + 2 Cl – (aq) + H 2 (g). Zn is an active metal (reduces H in acid but not in water). Cu(s) + HCl(aq) → no reaction Cu is an inactive metal (does not reduce H in acid nor water). Activity Series Lab 3: You use Mg instead of Zn 2/6/2012 2 A “Classic” Redox Example Solid copper is immersed in aqueous silver nitrate. Cu(s) + 2Ag + (aq) Cu 2+ (aq) + 2Ag(s) Ox. #: 0 +1 +2 0 oxidation reduction Balanced Net Ionic eqn.: Blue color is formation of Cu 2+ Ag is formed from solution of Ag + net charge = net charge = +2 +2 At the particulate level… Before rxn occurs... During rxn 2/6/2012 3 Writing Half-Reactions Cu(s) + 2 Ag + (aq) Cu 2+ (aq) + 2 Ag(s) Cu(s) Cu 2+ (aq) + 2e- Ag + (aq) + e- Ag(s) We can separate an electron-transfer reaction between Cu(s) and Ag + (aq) into two “half-reactions,” where the electron loss or gain is explicitly stated. The half-reaction idea provides us with a reliable method of balancing redox reactions in aqueous solution. + x 2 Electrons just change places… charge is conserved!!! net charge = net charge = +2 +2 Balancing by Half-Reactions • Recall, a properly balanced redox reaction means both mass and charge are conserved. • Oftentimes the solvent (in this course, we will only consider water) will be explicitly involved in the redox reaction....
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Ch 4_Lecture 13_020612 - 1 Demo Activity Series Mg(s 2...

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