REDOX REACTIONS

OiL

Oxidation is Losing electrons(becomes more positive)

RiG

Reduction is Gaining electrons(becomes less positive)

Cu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s)

Put in charges and look at changes

0 2+

more positive (Lost e-s)

Cu is oxidized from 0 to 2+

1+ 0Less positive (Gained e-s)

Ag1+ is reduced from 1+ to 0

Cu is the reducing agent and AgNO3 is the oxidizing agent

MgC2O4

H2SO4

H2SO3

Cr2O72-

Assign oxidation numbers for each element below

Co(NO3)2

MgC2O4

H2SO4

H2SO3

Cr2O72-

Assign oxidation numbers for each element below

Co(NO3)2

+2 2x 4(-2) 0 + + =

Mg C O overall charge

x = +3 (the assigned charge for carbon in this compound)

2(+1) x 4(-2) 0 + + =

H S O overall charge

2(+1) x 3(-2) 0 + + =

H S O overall charge

2x 7(-2) - 2 + =

Cr O overall charge

+2 2x 6(-2) 0 + + =

Co N O overall charge

x = +6 (the assigned charge for sulfur in this compound)

x = +4 (the assigned charge for sulfur in this compound)

x = +6 (the assigned charge for chromium in this compound)

x = +5 (the assigned charge for nitrogen in this compound)

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.

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. (OiL)

_______ is reduced from a ______ charge to a ________ charge. (RiG)

____________ is the reducing agent.

____________ is the oxidizing agent.

+2 +7

More positive (Lost electrons) OiL

Mn2+ +2 +7

+4 +2

Less positive (Gains electrons) RiG

Pb4+ +4 +2

MnO

PbO2

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.

Fe (s) + FeCl3 (aq) → FeCl2 (aq)

______ is oxidized from a ______ charge to a ________ charge. (OiL)

_______ is reduced from a ______ charge to a ________ charge. (RiG)

_______ ____ is the reducing agent.

____________ is the oxidizing agent.

0 +3 +2

Fe 0 +2

Fe3+ +3 +2

Fe

FeCl3

Cu (s) + 4 HNO3 (aq) → 2 NO2 (g) + 2 H2O (l) + Cu(NO3)2 (aq)

______ is oxidized from a ______ charge to a ________ charge. (OiL)

_______ is reduced from a ______ charge to a ________ charge. (RiG)

____________ is the reducing agent.

____________ is the oxidizing agent.

0 +2

Cu 0 +2

+5 +4

N+5 +5 +4

Cu

HNO3