RedOx reactions(Single Replacement)

2 Mg (s) + O2 (g) 2 MgO (s)

0 0 +2 -2

Mg = oxidized more positive

O2 = reduced more negative

(reducing agent)

(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)

0 +1 +2 0

Zn = oxidized more positive

H = reduced more negative

(reducing agent)

(oxidizing agent)

Oxidation of Metals by Acids and Salts

H2SO4 (aq) + Fe (s) FeSO4 (aq) + H2 (g)

+1 0 +2 0

Fe = oxidized more positive

H = reduced more negative

(reducing agent)

(oxidizing agent)

Oxidation of Metals by Acids and Salts

Ni(NO3)2 (aq) + Fe (s) Ni (s) + Fe(NO3)2 (aq)

Net Ionic:

+2 0 0 +2

Fe = oxidized more positive

Ni = reduced more negative

(reducing agent)

(oxidizing agent)

Ni+2 (aq) + Fe (s) Ni (s) + Fe+2 (aq)

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:

0 +1 +2 0

Cu = oxidized more positive

Ag = reduced more negative

(reducing agent)

(oxidizing agent)

Cu (s) + 2Ag+1(aq) Cu+2

(aq) + 2Ag(s)

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:

0 +1 +2 0

Ni = oxidized more positive

H = reduced more negative

(reducing agent)

(oxidizing agent)

Ni (s) + 2H+1(aq) Ni+2

(aq) + H2 (g)

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)