Question

Hydrogen peroxide molecules are:
A.Monatomic and form $X_2^{2 - }$ ions
B.Diatomic and form $X_{}^ - $ ions
C.Diatomic and form $HO_2^ - $ ions
D.Monoatomic and form $X_{}^ - $ ions

Answer 1

Hint:To answer this question, you should recall the properties of hydrogen peroxide. The chemical formula for hydrogen peroxide is ${H_2}{O_2}$. It is symmetrical and each OH ion has a negative charge.

Complete step by step solution:
We know that peroxide is a compound which has two oxygen atoms bonded together. And Hydrogen Peroxide is the simplest peroxide. The structure of the molecule can be drawn as:

Hydrogen peroxide is a colorless liquid and is used as a bleaching agent and disinfectant due to its property to produce free radicals on decomposition. Hydrogen peroxide decomposes when exposed to sunlight, hence it is stored in wax-lined glass or plastic containers and kept in dark. This process is catalyzed and accelerated by traces of alkali metals. It should also be kept away from dust particles because dust can induce explosive decomposition of this compound. Hydrogen peroxide is both acidic and the basic medium acts as an oxidizing as well as the reducing agent\[{H_2}{O_2}\] is a monatomic molecule as it contains only one atom. It can be simply represented as \[HO - OH.\] It forms \[{\left( {OH} \right)_2}^{2 - }\] ions on breakage.
That is, it forms \[{X_2}^{2 - }\] ​ ions. \[HO - OH \rightleftharpoons {\left( {OH} \right)_2}^{ - 2}\].

Hence, the correct option is option A.

Note:
You should know about the preparation of Hydrogen Peroxide:
\[N{a_2}{O_2}\left( s \right) + {H_2}S{O_4} \to N{a_2}S{O_4}\left( s \right) + {H_2}{O_2}\left( l \right)\].
We can see that here \[{H_2}{O_2}\]is being produced. This is indeed a preparation method of laboratory preparation of hydrogen peroxide by the action of ice-cold, dilute sulphuric acid on sodium peroxide or hydrated barium peroxide. A calculated quantity of sodium peroxide is added in small quantities to $20\% $an ice-cold solution of sulphuric acid. Most of the sodium sulphate separates on cooling as crystals of \[N{a_2}S{O_4}.10{H_2}O\]. From this reaction, we obtain a \[30\% \] hydrogen peroxide yield containing a small amount of sodium sulphate.