In peroxides, the oxidation number of oxygen is:
Correct answer: A. -1
- A. -1
- B. 2
- C. -2
- D. 1
Explanation
In peroxides, the oxidation number of oxygen is -1. This is due to the peroxide ion (O2²⁻), where two oxygen atoms are bonded together, sharing a -2 charge, which results in each oxygen having an oxidation state of -1. For example, in hydrogen peroxide (H2O2), the oxidation number of each oxygen atom is -1, balancing the +1 oxidation state of the hydrogen atoms.Options B (2) and D (1) are incorrect because oxygen typically does not have a positive oxidation state in compounds due to its high electronegativity. Option C (-2) is incorrect in the context of peroxides, as this is the oxidation number for oxygen in most other compounds but not in peroxides.
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Electrochemistry describes electron transfer through oxidation and reduction, identifies oxidizing and reducing agents, and applies oxidation numbers to balance redox equations. It also covers electrode potential and the standard hydrogen electrode, which provides the reference for comparing the reduction tendencies of other electrodes.
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