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What sulphur species would most likely disproportionate: so42- so32- s2o3 s s42- hs-
Accepted Answer
The most likely species to disproportionate is SO32-.
Disproportionation is a redox reaction where the same element is both oxidized and reduced. Here's why SO32- is the most likely candidate:
SO32- can be oxidized to SO42-: The sulfur in SO32- has an oxidation state of +4. It can be oxidized to +6 in SO42-.
SO32- can be reduced to S or S2O32-: The sulfur in SO32- can be reduced to 0 in elemental sulfur (S) or to +2 in thiosulfate (S2O32-).
The other species are less likely to disproportionate because:
SO42-: Sulfur in SO42- is already in its highest oxidation state (+6), so it cannot be further oxidized.
S: Elemental sulfur (S) is already in its standard oxidation state (0), so it cannot be further reduced.
S42-: This species is not typically encountered in common chemistry.
HS-: The sulfur in HS- is in a lower oxidation state (-2) and is likely to be oxidized, not disproportionated.
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