Question

Consider the following balanced reaction, $A{O}_2^{x-}+2H_{2}O⟶4O{H}^{-}+3O_2$ the $x$ is?

• A. $-1$ and species is super oxide
• B. $-2$ and species is peroxide
• C. $-4$ and species is oxide
• D. $-1$ and species is peroxide

Answer 1

The correct option is B $-2$ and species is peroxide

Option C is correct

$O_2^{x-}+2H_{2}O\to 4O{H}^{-}+3O_2$

In RHS the total charge is $-4$

so in LHS also the the charge should be $-4$

so $x=-4$

now the oxidation state of $O$ is

$2x=-4$

$x=-2$

so it is oxide