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

Concept: The oxidation state of an element is the apparent charge assigned to it in a compound according to the oxidation number rules. Some important rules are:

• Fluorine always has oxidation state \(-1\).

• The oxidation state of an element in its free state is \(0\).

• The algebraic sum of oxidation states of all atoms in a neutral molecule is zero.
Since fluorine is the most electronegative element, oxygen exhibits a positive oxidation state in compounds containing fluorine.

Step 1: Find the oxidation state of oxygen in \(O_{2}F_{2}\).
Let the oxidation state of oxygen be \(x\). Since fluorine has oxidation state \(-1\), \[ 2x+2(-1)=0. \] Therefore, \[ 2x-2=0, \] \[ 2x=2, \] \[ x=+1. \] Hence, \[ \boxed{\text{Oxidation state of oxygen in }O_{2}F_{2}=+1.} \]

Step 2: Find the oxidation state of oxygen in \(O_{3}\).
Ozone is an allotrope of oxygen. Since it exists in the elemental state, \[ \boxed{\text{Oxidation state of oxygen}=0.} \]

Step 3: Identify the correct option.
Thus, \[ O_{2}F_{2}\rightarrow +1, \] \[ O_{3}\rightarrow 0. \] Hence, \[ \boxed{\textbf{Option (A)}} \] is the correct answer.