Step by step
- Known values: K = +1 (group 1 metals are +1); CN = −1 (cyanide ion CN⁻ is −1).
- Let the oxidation number of Fe be x. The sum over all atoms equals the overall charge, 0 for a neutral compound.
- 3(+1) + 6(−1) + x = 0
- −3 + x = 0, so x = +3
- x = +3
Potassium ferricyanide.
Check any other formula with the oxidation number calculator.
Common oxidation numbers
| Element in compound | Oxidation number |
|---|---|
| Mn in KMnO4 | +7 |
| Cr in K2Cr2O7 | +6 |
| Cr in Cr2O72− | +6 |
| Cr in CrO42− | +6 |
| Mn in MnO42− | +6 |
| Mn in MnO2 | +4 |
| S in H2SO4 | +6 |
| S in SO2 | +4 |
| S in SO3 | +6 |
| S in H2S | −2 |
| S in Na2S2O3 | +2 |
| S in S4O62− | +5/2 |
| S in H2SO5 | +6 |
| N in HNO3 | +5 |
| N in NH3 | −3 |
| N in NH4+ | −3 |
| N in NO3− | +5 |
| N in NO2 | +4 |
| N in HNO2 | +3 |
| N in N2O | +1 |
| N in N2O5 | +5 |
| N in N2H4 | −2 |
| N in NH2OH | −1 |
| N in HN3 | −1/3 |
| P in H3PO4 | +5 |
| P in H3PO3 | +3 |
| P in H3PO2 | +1 |
| Cl in HClO4 | +7 |
| Cl in HClO | +1 |
| Cl in KClO3 | +5 |
| Cl in CaOCl2 | 0 |
| Fe in Fe3O4 | +8/3 |
| Fe in K4[Fe(CN)6] | +2 |
| Fe in K3[Fe(CN)6] | +3 |
| Cr in CrO5 | +6 |
| O in H2O2 | −1 |
| O in OF2 | +2 |
| O in KO2 | −1/2 |
| O in Na2O2 | −1 |
| H in NaH | −1 |
| Pb in Pb3O4 | +8/3 |
| C in CO2 | +4 |
| C in CO | +2 |
| C in CH4 | −4 |
| C in C6H12O6 | 0 |
| C in HCOOH | +2 |
| Ni in Ni(CO)4 | 0 |
| Cu in [Cu(NH3)4]2+ | +2 |
| Co in [Co(NH3)6]Cl3 | +3 |
| Xe in XeF6 | +6 |
| Os in OsO4 | +8 |
| Al in LiAlH4 | +3 |
Questions students ask
What is the oxidation number of Fe in K₃[Fe(CN)₆]?
+3. Potassium ferricyanide.
How do you find the oxidation number of iron in K₃[Fe(CN)₆]?
Known values: K = +1 (group 1 metals are +1); CN = −1 (cyanide ion CN⁻ is −1). Let the oxidation number of Fe be x. The sum over all atoms equals the overall charge, 0 for a neutral compound. 3(+1) + 6(−1) + x = 0 −3 + x = 0, so x = +3 x = +3