A) The oxidation number of S in \[{{(N{{H}_{4}})}_{2}}{{S}_{2}}{{O}_{8}}\]is +6.
B) The oxidation number of Os in \[{{O}_{S}}{{O}_{4}}\]is +8.
C) The oxidation nu mber 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] : Oxidation state of S in \[{{(N{{H}_{4}})}_{2}}{{S}_{2}}{{O}_{8}}=+6\] (Since \[{{S}_{2}}.{{O}_{8}}^{2-}\]has one peroxide bond) Oxidation state of Os in \[Os{{O}_{4}}=+8\] Oxidation state of S in \[{{H}_{2}}S{{O}_{5}}=+6\] (Since it has one peroxide bond) Oxidation state of O in \[K{{O}_{2}}=-1/2\]
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