Question
In $KO_2$, the nature of oxygen species and the oxidation state of oxygen atom are, respectively
The correct answer is
Superoxide and -1/2
Analyzing $KO_2$ Oxygen Species and Oxidation State
The compound $KO_2$ is potassium superoxide.
When $KO_2$ dissociates, it forms potassium ions ($K^+$) and superoxide ions ($O_2^-$).
- Potassium Ion: Potassium ($K$) is an alkali metal and typically exists in the $+1$ oxidation state. Thus, we have $K^+$.
- Oxygen Species: The remaining part is the $O_2$ unit, which must carry a charge of $-1$ to balance the $K^+$ ion, forming the $O_2^-$ ion. This $O_2^-$ ion is known as the superoxide ion.
Calculating Oxygen Oxidation State in Superoxide
To find the oxidation state of a single oxygen atom within the superoxide ion ($O_2^-$):
- Let the oxidation state of one oxygen atom be $x$.
- Since there are two oxygen atoms in the $O_2^-$ ion, their total oxidation state is $2x$.
- The overall charge of the superoxide ion is $-1$.
- Therefore, the equation is: $2x = -1$
- Solving for $x$: $x = -\frac{1}{2}$
Thus, the nature of the oxygen species in $KO_2$ is superoxide, and the oxidation state of the oxygen atom is -1/2.
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