Chapter 106 of 2363 min read

Oxidation number and balancing redox equations

Why this is asked: Oxygen isn't always −2: it's −1 in peroxides (H₂O₂), −1/2 in superoxides (KO₂), and +2 in OF₂, where fluorine is the more electronegative atom — NEET tests exactly these exceptions, not the default. Also watch for disproportionation, where the same element is simultaneously oxidised and reduced in one reaction, such as Cl₂ with cold dilute NaOH.

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Test yourself

•Consider the following compounds: $K O_{2}$ , $H_{2} O_{2}$ and $H_{2} S O_{4}$ . The oxidation states of the underlined elements (O in $K O_{2}$ , O in $H_{2} O_{2}$ , S in $H_{2} S O_{4}$ ) in them are, respectively:

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