Transcript Slide 1

REDOX REACTIONS
OiL
RiG
Oxidation is Losing electrons
(becomes more positive)
Reduction is Gaining electrons
(becomes less positive)
more positive (Lost e-s)
0
2+
Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)
1+
Less positive (Gained e-s) 0
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
Assign oxidation numbers for each element below
MgC2O4
H2SO4
H2SO3
Cr2O72-
Co(NO3)2
Assign oxidation numbers for each element below
MgC2O4
+2
Mg
+
2x
C
4(-2)
O
+
=
0
overall charge
x = +3 (the assigned charge for carbon in this compound)
H2SO4
2(+1)
+
H
x
S
4(-2)
O
+
=
0
overall charge
x = +6 (the assigned charge for sulfur in this compound)
H2SO3
2(+1)
+
H
x
S
3(-2)
O
+
=
0
overall charge
x = +4 (the assigned charge for sulfur in this compound)
Cr2O72-
Co(NO3)2
2x
+
Cr
7(-2)
O
=
-2
overall charge
x = +6 (the assigned charge for chromium in this compound)
+2
2x
6(-2)
0
+
+
=
Co
N
O
overall charge
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.
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+ is oxidized from a ______
+2 charge to a ________
+7 charge. (OiL)
______
+4 charge to a ________
Pb4+ is reduced from a ______
+2
_______
charge. (RiG)
MnO
____________
is the reducing agent.
PbO2
____________
is the oxidizing agent.
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.
0
+3
+2
Fe (s) + FeCl3 (aq) → FeCl2 (aq)
0 charge to a ________
+2
Fe
______
is oxidized from a ______
charge. (OiL)
Fe3+ is reduced from a ______
+3 charge to a ________
+2
_______
charge. (RiG)
Fe ____ is the reducing agent.
_______
FeCl3
____________
is the oxidizing agent.
+2
0
+5
+4
Cu (s) + 4 HNO3 (aq) → 2 NO2 (g) + 2 H2O (l) + Cu(NO3)2 (aq)
Cu is oxidized from a ______
0 charge to a ________
+2
______
charge. (OiL)
N+5
+5 charge to a ________
+4
_______
is reduced from a ______
charge. (RiG)
Cu
____________
is the reducing agent.
HNO3
____________
is the oxidizing agent.