RedOx reactions (Single Replacement) 2 Mg (s) + O2 (g)  2 MgO (s) +2 -2 Mg = oxidized  more positive (reducing agent) O2 = reduced  more negative (oxidizing agent) LEO the lion goes GER OIL…RIG

Oxidation of Metals by Acids and Salts Zn (s) + 2 HCl (aq)  ZnCl2 (aq) + H2 (g) +1 +2 Zn = oxidized  more positive (reducing agent) H = reduced  more negative (oxidizing agent)

Oxidation of Metals by Acids and Salts H2SO4 (aq) + Fe (s)  FeSO4 (aq) + H2 (g) +1 +2 Fe = oxidized  more positive (reducing agent) H = reduced  more negative (oxidizing agent)

Oxidation of Metals by Acids and Salts Ni(NO3)2 (aq) + Fe (s)  Ni (s) + Fe(NO3)2 (aq) Net Ionic: +2 +2 Ni+2 (aq) + Fe (s)  Ni (s) + Fe+2 (aq) Fe = oxidized  more positive (reducing agent) Ni = reduced  more negative (oxidizing agent)

Activity Series Use to predict if a reaction will occur Single Replacement Any metal can be OXIDIZED by any metal below it on the series

Activity Series

Examples Cu (s) + 2AgNO3 (aq)  Cu(NO3)2 (aq) + 2 Ag (s) Net Ionic: +1 +2 Cu (s) + 2Ag+1(aq)  Cu+2 (aq) + 2Ag(s) Cu = oxidized  more positive (reducing agent) Ag = reduced  more negative (oxidizing agent)

Examples Cu (s) + 2FeNO3 (aq)  No Reaction Based on the Activity Series Cu can’t be oxidized by Fe Meaning that Cu is below Fe on the activity series

Examples Ni (s) + 2 HCl (aq)  NiCl2 (aq) + H2 (g) Net Ionic: +1 +2 Ni (s) + 2H+1(aq)  Ni+2 (aq) + H2 (g) Ni = oxidized  more positive (reducing agent) H = reduced  more negative (oxidizing agent)

Types of RedOx reactions Single replacement in acid Mg(s) + HCl(aq)  Single replacement in H2O Ca(s) + H2O(l)  Single replacement in aqueous salt Cu(s) + AgNO3(aq)  Single replacement of nonmetals F2(g) + LiBr(aq) 