Question

What is the oxidation state of oxygen in \(O_{2}F_{2}\) and \(O_{3}\)?

• A. \(+1\) in \(O_{2}F_{2}\) and \(0\) in \(O_{3}\)
• B. \(-1\) in \(O_{2}F_{2}\) and \(+2\) in \(O_{3}\)
• C. \(+2\) in \(O_{2}F_{2}\) and \(-1\) in \(O_{3}\)
• D. \(0\) in both

Hint:

Remember these important oxidation states of oxygen: \[ \boxed{ \begin{aligned} O_2,\;O_3 &: 0\\ H_2O &: -2\\ H_2O_2 &: -1\\ OF_2 &: +2\\ O_2F_2 &: +1 \end{aligned} } \] Whenever oxygen combines with fluorine, oxygen has a positive oxidation state because fluorine is the most electronegative element.

Answer 1

The Correct Option is A

Fluorine is the most electronegative element and is always assigned $-1$; in $O_2F_2$ this forces each oxygen to an oxidation state of $+1$. In $O_3$ all atoms are identical oxygen, so no electronegativity difference exists and the oxidation state of oxygen is $0$.