lecture13 - Lecture 13: Lecture 13: Redox; titrations;...

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Lecture 13: Redox; titrations; reactions in solution Oxidation-Reduction Reactions Oxidation Oxidation Originally: add oxygen . 2 Cu(s) + O 2 (g) 2 CuO(s) 2 CO(g) + O 2 (g) 2 CO 2 (g) Cu and CO are oxidized. O 2 is the oxidizing agent for both. Reduction Reduction Originally: reduce ore to metal ; reverse of oxidation . CuO(s) + H 2 (g) Cu(s) + H 2 O SnO 2 (s) + 2 C(s) Sn(s) + 2 CO(g) CuO and SnO 2 are reduced. H 2 and C are the reducing agents (note: H 2 is oxidized, so CuO is an oxidizing agent)
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Oxidation-Reduction Reactions In all cases: If something is oxidized, something must be reduced. • Redox reactions move e - . 2 Ag + (aq) + Cu(s) 2 Ag(s) + Cu 2+ (aq) • Ox Ox idation-red red uction = redox redox . Here: • Cu changes to Cu 2+ . • Cu loses 2 e - ; each Ag + gains one e - •A g + is reduced (ore turned to metal) Gain of e - = reduction (so, loss of e - = oxidation) +2 e - -2 e - Loss of electrons is oxidation Gain of electrons is reduction Leo says ger ger Oxidation is loss Reduction is gain Redox Reactions and Electron Transfer Oil Oil rig rig
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M is a reducing agent X is an oxidizing agent MX e - M loses electron(s) X gains electron(s) M is oxidized X is reduced Redox Reactions and Electron Transfer Oxidizing Agent Reaction Product O 2 (oxygen) O 2 - (oxide ion) H 2 O 2 (hydrogen peroxide) H 2 O( l ) F 2 , C l 2 , Br 2 , I 2 (halogen) F - , C l - , Br - , I - (halide ion) HNO 3 (nitric acid) nitrogen oxides (NO, NO 2 ..) Cr 2 O 7 - (dichromate ion) Cr 3+
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lecture13 - Lecture 13: Lecture 13: Redox; titrations;...

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