Question

Peroxy linkage is present in-

• A. ${\mathrm{H}}_2{\mathrm{SO}}_5$
• B. ${\mathrm{H}}_2{\mathrm{SO}}_3$
• C. ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_7$
• D. ${\mathrm{H}}_2{\mathrm{SO}}_4$

Answer 1

The correct option is A

${\mathrm{H}}_2{\mathrm{SO}}_5$

The explanation for the correct option:

Option (A): ${\mathrm{H}}_2{\mathrm{SO}}_5$

• The peroxide bonds in a compound can be calculated by knowing the oxidation number of the central metal in a compound.
• If the oxidation number of central metal in a compound comes out to be greater than the maximum oxidation state of that central metal then that compound must contain peroxide bonds.
• In the case of In ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_5$, the oxidation state of sulfur can be calculated as:
  $$\begin{gathered} +2+x+(-10)=0 \\ x=+8 \end{gathered}$$
• But Sulfur has a maximum oxidation state of $+6$. hence, there will be one peroxide bond present in the given molecule, which can be given as

The explanation for the incorrect option:

Option (B): ${\mathrm{H}}_2{\mathrm{SO}}_3$

• ${\mathrm{H}}_2{\mathrm{SO}}_3$ has no peroxide bond present in the molecule.
• Hence, the option is the incorrect one.

Option (C):${\mathrm{H}}_2{\mathrm{SO}}_4$

• There is no peroxide bonding present in the ${\mathrm{H}}_2{\mathrm{SO}}_4$molecule.
• Thus, the given option does not represent the correct option.

Option (D): ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_7$

• ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_7$ has no peroxide bond present in the molecule.
• Hence, the given option does not coincide with the correct option.

Hence, peroxy linkage is present in ${\mathrm{H}}_2{\mathrm{SO}}_5$, option (A) is the correct answer.