Question

Oxygen has an oxidation state of +2 in

• A. \(H_2O_2\)
• B. \(H_2O\)
• C. \(F_2O\)
• D. \(SO_2\)

Hint:

Oxygen usually exhibits -2 oxidation state. It shows positive oxidation states only when combined with fluorine, the most electronegative element.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept:
Oxidation state is determined by electronegativity differences. Fluorine is the most electronegative element.
Step 2: Detailed Explanation:
\begin{itemize} \item (A) \(H_2O_2\): Let O.N. of O be x. \(2(+1) + 2x = 0 \Rightarrow 2 + 2x = 0 \Rightarrow x = -1\). \item (B) \(H_2O\): \(2(+1) + x = 0 \Rightarrow x = -2\). \item (C) \(F_2O\): F has O.N. -1. \(2(-1) + x = 0 \Rightarrow -2 + x = 0 \Rightarrow x = +2\). \item (D) \(SO_2\): Let O.N. of O be x. S has O.N. +4. \(4 + 2x = 0 \Rightarrow 2x = -4 \Rightarrow x = -2\). \end{itemize}
Step 3: Final Answer:
Oxygen has +2 oxidation state in \(F_2O\), option (C).