The oxyacids of sulphur having direct S-S bonds are :
H2S2O3, H2S2O4, H2S2O6
Every acid listed contains two sulphur atoms, so the discriminating question is how those two sulphurs are joined: directly (S-S), or through a bridging oxygen (S-O-S) or peroxide link (S-O-O-S).
H2S2O3, thiosulphuric acid — has S-S. It is structurally sulphuric acid with one terminal oxygen replaced by sulphur, so the second sulphur is bonded straight to the central one.
H2S2O4, dithionous acid — has S-S. Both sulphurs are in the +3 state and are joined by an unusually long, weak S-S bond, which is why the dithionite ion is such a powerful reducing agent.
H2S2O6, dithionic acid — has S-S. Two SO3H units are linked directly sulphur to sulphur, each sulphur being +5.
H2S2O7, pyrosulphuric (disulphuric) acid, does not. It is formed by condensing two molecules of H2SO4 with loss of water, so the two sulphurs are joined through a bridging oxygen, S-O-S.
H2S2O8, peroxydisulphuric acid, also does not. Here the link is a peroxide bridge, S-O-O-S, which is the source of its strong oxidising power.
So the three acids with a genuine sulphur-sulphur bond are the thio, dithionous and dithionic acids.
Hence the answer is H2S2O3, H2S2O4, H2S2O6.
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