Finding the oxidation state of each element in a compound is a fundamental skill in Class 11 Redox Chemistry. CO (Carbon Monoxide) is a common example.
Carbon monoxide (CO) is a colourless, odourless, and highly toxic gas. It binds to haemoglobin ~240 times more strongly than oxygen, preventing oxygen delivery to tissues — causing CO poisoning.
In CO (Carbon Monoxide):
Rule: Oxidation state of Oxygen = -2 (standard rule for oxygen in compounds)
Let oxidation state of Carbon = x
For a neutral molecule, sum of all oxidation states = 0:
x + (-2) = 0
x = +2
Oxidation state of Carbon in CO = +2
| Compound | Oxidation state of C |
|---|---|
| CO | +2 |
| CO₂ | +4 |
| CH₄ | -4 |
| C | 0 |
As carbon bonds with more oxygen, its oxidation state increases (becomes more positive).
Because C is in +2 state in CO and can be oxidised further to +4 (in CO₂), CO acts as a powerful reducing agent in metallurgy:
Fe₂O₃ + 3CO → 2Fe + 3CO₂
Here, CO reduces iron oxide to iron metal in blast furnaces.
Let x be OS of C. x + 3(-2) = -2. x - 6 = -2. x = **+4**
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