Statement (A): Oxidation number of fluorine is −1.
Statement (B): Oxidation number of sodium is +1.
Statement (C): In peroxides, oxygen exhibits +1/ 2 oxidation state.

see full answer

High-Paying Jobs That Even AI Can’t Replace — Through JEE/NEET

🎯 Hear from the experts why preparing for JEE/NEET today sets you up for future-proof, high-income careers tomorrow.

An Intiative by Sri Chaitanya

All the above statements are correct

All the above statements are incorrect

A and B are correct but C is incorrect

A and B are incorrect but C is correct

answer is C.

(Unlock A.I Detailed Solution for FREE)

Best Courses for You

JEE

NEET

Foundation JEE

Foundation NEET

CBSE

Detailed Solution

Fluorine Always Shows -1 Oxidation Number
The oxidation number of fluorine is always -1 in its compounds. This is because fluorine is the most electronegative element in the periodic table. It always pulls electrons towards itself in chemical bonds.
- Example 1: In HF (hydrogen fluoride), fluorine has an oxidation number of -1 because it attracts the shared electron pair from hydrogen.
- Example 2: In OF₂ (oxygen difluoride), fluorine still shows an oxidation number of -1, even though oxygen is less electronegative than fluorine. In this compound, fluorine's dominance keeps its oxidation number fixed at -1.
This unique property makes the oxidation number of fluorine a constant -1 in all its compounds.
Sodium Shows +1 Oxidation Number
Sodium, being an alkali metal, belongs to Group 1 of the periodic table and has the electronic configuration ns¹. It easily loses one electron to form a +1 charge, making its oxidation number +1 in compounds.
- Example 1: In NaH (sodium hydride), sodium has an oxidation number of +1, while hydrogen has an oxidation number of -1.
- Example 2: In Na₂S (sodium sulfide), sodium again shows an oxidation number of +1, while sulfur takes a -2 oxidation state to balance the compound.
Oxygen in Peroxides Shows -1 Oxidation Number
Oxygen usually has an oxidation number of -2, but in peroxides, such as H₂O₂ (hydrogen peroxide) or Na₂O₂ (sodium peroxide), it shows an oxidation number of -1. This is because the peroxide ion (O₂²⁻) consists of two oxygen atoms bonded together, with each oxygen atom contributing to the overall -2 charge of the ion.
- Example 1: In Na₂O₂, the peroxide ion (O₂²⁻) splits the -2 charge equally, giving each oxygen an oxidation number of -1.
- Example 2: In H₂O₂, the same principle applies, where each oxygen atom in the peroxide ion has an oxidation number of -1.