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REDOX REACTIONS

REDOX REACTIONS. Ri G Reduction is G aining electrons ( becomes less positive ). Oi L Oxidation is L osing electrons ( becomes more positive). more positive ( L ost e - s). 0. 2+. Cu(s) + 2AgNO 3 ( aq )  Cu(NO 3 ) 2 ( aq ) + 2Ag(s). 0. 1+.

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REDOX REACTIONS

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  1. REDOX REACTIONS RiG Reduction is Gaining electrons (becomes less positive) OiL Oxidation is Losing electrons (becomes more positive) more positive (Lost e-s) 0 2+ Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s) 0 1+ Less positive (Gained e-s) Put in charges and look at changes Cu is oxidized from 0 to 2+ Ag1+ is reduced from 1+ to 0 Cu is the reducing agent and AgNO3 is the oxidizing agent

  2. Assign oxidation numbers for each element below MgC2O4 H2SO4 H2SO3 Cr2O72- Co(NO3)2

  3. Assign oxidation numbers for each element below MgC2O4 x = +3 (the assigned charge for carbon in this compound) H2SO4 x = +6 (the assigned charge for sulfur in this compound) H2SO3 x = +4 (the assigned charge for sulfur in this compound) Cr2O72- x = +6 (the assigned charge for chromium in this compound) Co(NO3)2 x = +5 (the assigned charge for nitrogen in this compound)

  4. 2 MnO (s) + 5 PbO2 (s) + 10 HNO3 (aq) → 2 HMnO4 (aq) + 5 Pb(NO3)2 (aq) + 4 H2O (l) ______ is oxidized from a ______ charge to a ________ charge. _______ is reduced from a ______ charge to a ________ charge. _______ ____ is the reducing agent. ____________ is the oxidizing agent.

  5. More positive (Lost electrons) OiL +2 +7 +4 +2 2 MnO (s) + 5 PbO2 (s) + 10 HNO3 (aq) → 2 HMnO4 (aq) + 5 Pb(NO3)2 (aq) + 4 H2O (l) Less positive (Gains electrons) RiG Mn2+ +2 +7 ______ is oxidized from a ______ charge to a ________ charge. (OiL) _______ is reduced from a ______ charge to a ________ charge. (RiG) +4 Pb4+ +2 MnO ____________ is the reducing agent. ____________ is the oxidizing agent. PbO2

  6. Fe (s) + FeCl3 (aq) → FeCl2 (aq) ______ is oxidized from a ______ charge to a ________ charge. _______ is reduced from a ______ charge to a ________ charge ____________ is the reducing agent. ____________ is the oxidizing agent.

  7. 0 +3 +2 Fe (s) + FeCl3 (aq) → FeCl2 (aq) 0 +2 Fe ______ is oxidized from a ______ charge to a ________ charge. (OiL) _______ is reduced from a ______ charge to a ________ charge. (RiG) Fe3+ +3 +2 Fe _______ ____ is the reducing agent. ____________ is the oxidizing agent. FeCl3

  8. +2 0 +5 +4 Cu (s) + 4 HNO3 (aq) → 2 NO2 (g) + 2 H2O (l) + Cu(NO3)2 (aq) Cu 0 +2 ______ is oxidized from a ______ charge to a ________ charge. (OiL) _______ is reduced from a ______ charge to a ________ charge. (RiG) N+5 +5 +4 Cu ____________ is the reducing agent. ____________ is the oxidizing agent. HNO3

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