Question

Calculate oxidation number of $Br$ in $B{r}_3{O}_8$ and $S$ in $S_4{O}_6^{2-}$.

Answer 1

(i) $\stackrel{x}{B}{r}_3{O}_8\Rightarrow 3x+4\times (-2)=0$

$\Rightarrow 3x=+8$

$\Rightarrow x=\frac{+8}{3}$

Oxidation state of $Br=\frac{+8}{3}$

(ii) $S_4{O}_6^{2-}\Rightarrow 4x+6\times (-2)=-2$

$\Rightarrow 4x-12=-2$

$\Rightarrow 4x=-2+12=+10$

$\Rightarrow x=+2.5$

Oxidation state of $S=+2.5$