Question

The species that contain peroxide ions is/are:
(This question has multiple correct options)
\[
 A.{\text{ }}K{O_2} \\
  B.{\text{ }}Sr{O_2} \\
  C.{\text{ }}Ba{O_2} \\
  D.{\text{ }}N{a_2}{O_2} \\
\]

Answer 1

Hint: In order to deal with this question first we will define the term peroxide ion then using its property and definition we will try to find out the required species out of the given options which contain peroxide ions.

Complete step by step solution:
> Peroxide: Any of a class of chemical compounds in which a single covalent bond binds two oxygen atoms together.
> The peroxide ion $\left( {O_2^{2 - }} \right)$ which is negatively charged is mostly found in the inorganic compounds so they can be considered as the salts of the very weak acid namely hydrogen peroxide;
- Examples of such species are a bleaching agent, and barium peroxide $\left( {Ba{O_2}} \right)$, sodium peroxide $\left( {N{a_2}{O_2}} \right)$ , previously used for obtaining hydrogen peroxide.
- Hence, the species that contain peroxide ions are $\left( {Ba{O_2}} \right)$ and $\left( {N{a_2}{O_2}} \right)$
So, the correct answer is options C and D.
- Additional information- Hydrogen peroxide, known colloquially simply as "peroxide," is the most toxic peroxide. This is sold at varying amounts as a solution of liquids. Because hydrogen peroxide is almost colorless, these solutions are as they are. This is used mainly as an oxidant and blanching agent. Nevertheless, hydrogen peroxide is also generated biochemically in the human body, due in large part to a number of oxidase enzymes. When in contact with organic compounds condensed solutions are extremely harmful.

Note:As bleaching agents, as initiators of polymerization reactions, and in the preparation of hydrogen peroxide (q.v.) and other oxygen compounds, various organic and inorganic peroxides are useful. Hydrogen peroxide has a bitter flavor and is a colorless liquid at room temperature. Large amounts of gaseous hydrogen peroxide naturally exist in the soil. The hydrogen peroxide is unstable and readily decomposes to oxygen and water with heat release.