$H_{2} S$ acts only as a reducing agent while $S O_{2}$ can act both as a reducing and oxidizing agent because

S in $H_{2} S$ has - 2 oxidation state

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S in $S O_{2}$ has oxidation state + 4

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Hydrogen in $H_{2} S$ more +ve than oxygen

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Oxygen is more - ve in $S O_{2}$

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Solution

The correct option is B
S in $S O_{2}$ has oxidation state + 4

In $H_{2} S$ , Sulphur atom exhibits (-2) oxidation state, which is the least for the pnictogen.
As for its highest oxidation state - Sulphur exhibits (+6) in $H_{2} S O_{4}$ .
In $S O_{2}$ , sulphur exhibits a (+4) oxidation state, which is in between the extremes.
Hence $S O_{2}$ shows both oxidising and reducing properties.

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