Question
What are the oxidation number of the underlined elements in each of the following and how do you rationalise your results?
Solution
By conventional method
+ 1 x - 2
H2 S4 O6
2(+1) + 4x + 6(-2) = 0
or x = +2.5 (wrong)
But it is wrong because all the four S atoms cannot be in the same oxidation state.
By chemical bonding method. The structure of H2S4O6 is'
H2S4O6 is'
The oxidation number of each of the S-atoms linked with each other in the middle is zero while that of each of the remaining two S-atoms is -5.
H2S4O6 is'
The oxidation number of each of the S-atoms linked with each other in the middle is zero while that of each of the remaining two S-atoms is -5.
