Question

Peroxide linkage is present in:
A. ${{\text{H}}_2}{\text{O}}$
B. ${\text{Ba}}{{\text{O}}_2}$
C. ${\text{O}}{{\text{F}}_{\text{2}}}$
D. ${{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}$

Answer 1

Hint: Peroxide, any of the chemical compounds as in which the two oxygen atoms are bound together by a single covalent bond. Moreover, several organic and inorganic peroxides are used as bleaching agents and other oxygen compounds.

Complete step by step answer: As ${\text{Ba}}{{\text{O}}_2}$has a peroxide linkage. Since peroxides have oxidation state of $ - 1$.
${\text{ + 2 + (2x) = 0}}$
${\text{x = - 1}}$
Basically, peroxide linkage is simply ${\text{O - O}}$bond. And talking about the term oxidation number, also called oxidation state, it is the total number of electrons that an atom either gains or loses in order to form a chemical bond with the other atom. So, as a result the compound ${\text{Ba}}{{\text{O}}_2}$ is a peroxide and referred to as barium peroxide. Barium peroxide appears as a greyish-white granular solid. It is insoluble in water. Also, it is non combustible material and accelerates the burning of combustible material. Some finely divided combustible materials which are mixed may be very explosive.
So, the option B) is correct i.e. ${\text{Ba}}{{\text{O}}_{\text{2}}}$.

Additional Information:
Barium peroxide reacts with ozone to produce barium oxide and oxygen. This reaction, as given below takes place at a temperature of near ${\text{ - 8}}{{\text{0}}^{\text{o}}}{\text{C}}$ in the liquid.
${\text{Ba}}{{\text{O}}_2}{\text{ + }}{{\text{O}}_3}{\text{ = Ba(}}{{\text{O}}_3}{{\text{)}}_2}{\text{ + }}{{\text{O}}_2}$

Note: Barium peroxide is used as an oxidizer in ordnance and it can be used for bleaching animal substances, vegetable fibers and straw. Moreover, barium is a known poisonous ingredient. Also, it has the tendency to infuse into the blood and make it more poisonous. Hence, hair dyes containing barium must be avoided.