A) The oxidation number of S in \[{{(N{{H}_{4}})}_{2}}{{S}_{2}}{{O}_{8}}\]is +6.
B) The oxidation number of Os in \[Os{{O}_{4}}\] is +8.
C) The oxidation number of S in \[{{H}_{2}}S{{O}_{5}}\] is +8.
D) The oxidation number of O in \[K{{O}_{2}}\] is -1/2.
Correct Answer: C
Solution :
[c] [a] \[{{\left( N{{\overset{+1}{\mathop{H}}\,}_{4}} \right)}_{2}}{{S}_{2}}{{O}_{8}}^{2-}\] \[\therefore \] Oxidation state of S=+6 (Since \[{{S}_{2}}{{O}_{8}}^{2-}\] has one peroxide bond) [b] Oxidation state of \[Os=+8\] [c] Oxidation state of S in \[{{H}_{2}}S{{O}_{5}}=+6\] (Since it has one peroxide bond) [d]\[{{K}^{1+}}{{O}_{2}}^{1-}\], oxidation state of \[O=-1/2\]
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