A) \[~0,+6,-2\]
B) \[0,+4,-2\]
C) \[0,+1,+2\]
D) \[0,+1,-2\]
Correct Answer: B
Solution :
The oxidation state of an element in its free state is zero, ie, oxidation state of S in \[{{\text{S}}_{\text{8}}}\]is O. Let the oxidation state of S in \[\text{S}{{\text{O}}_{2}}\]and \[{{\text{H}}_{\text{2}}}\text{O}\]is \[x\]. \[\underset{\begin{smallmatrix} x+(-2)\,\times \,2\,=\,0 \\ \,\,\,\,\,\,\,\,\,\,\,x-4=0 \\ \,\,\,\,\,\,\,\,\,\,x=+\,4 \end{smallmatrix}}{\mathop{S{{O}_{2}}}}\,\] \[\underset{\begin{smallmatrix} (1)\,\times \,2+x=0 \\ \,\,\,\,\,\,\,\,\,\,\,\,2+x=0 \\ \,\,\,\,\,\,\,\,\,\,x=-2 \end{smallmatrix}}{\mathop{{{H}_{2}}S}}\,\] Thus, the oxidation states of S, in \[{{\text{S}}_{\text{8}}}\text{,S}{{\text{O}}_{\text{2}}}\]and \[{{\text{H}}_{\text{2}}}\text{S}\]are respectively 0, + 4 and - 2.
You need to login to perform this action.
You will be redirected in
3 sec
