Question

Calculate oxidation state of $Ag$ in $Ag\left[\right(S_2{O}_3{)}_2{]}^{3-}$ molecule

• A. $+1$
• B. $0.5$
• C. $-1$
• D. $-2$

Answer 1

The correct option is A $+1$

Let $x$ be the oxidation state of $Ag$ in $Ag\left[\right(S_2{O}_3{)}_2{]}^{3-}$ molecule

Overall charge on molecule is $=-2$

We know, Thiosulphate $\left(S_2{O}_3\right)$ ion has $-2$ charge
So,
$x+2\times (-2)=-3x=+1$
Oxidation state of $Ag$ is $+1$
Theory :
Here are some important radicals with their formulas.
$\text{Radicals}\text{Formula}$
$\text{Sulphite}S{O}_3^{2-}$
$\text{Acetate}C{H}_{3}CO{O}^{-}$
$\text{Thiosulphate}{S}_2{O}_3^{2-}$
$\text{Tetrathionate}{S}_4{O}_6^{2-}$
$\text{Carbonate}C{O}_3^{2-}$
$\text{Dichromate}C{r}_2{O}_7^{2-}$
$\text{Phosphate}P{O}_4^{3-}$
$\text{Oxalate}{C}_2{O}_4^{2-}$