Fe + 3AgNO3 → 3Ag + Fe(NO3)3
Step
Assign oxidation numbers then figure what was oxidized
Fe = 0, Rule 1 under oxidation states
AgNO3 = NO3 is a polyatomic ion N = 5, O = -6 so -1 overall.
+1
-1
Rule 3
Ag = 0, Rule 1 under oxidation states
Fe(NO3)3 = NO3 is still -1 but the 2nd subscript is multiplied by
+3 -3
-1 to equal -3 overall. Rule 3
Fe + 3Ag[N(O3)] → 3Ag + Fe[(NO3)3]
0
+1 +5 -2
0
+3 +5 -2
-1
-3
N+(Ox3) = -1
[N+(Ox3)]x3 = -3
5+(-2x3) = -1
[5+(-2x3)]x3 = -3
Fe + 3AgNO3 → 3Ag + Fe(NO3)3
0
1 5 -2
0
3 5 -2
Iron in oxidized, it increased in oxidation value.