Reason: The average oxidation number of sulfur in S4O2−6 is +2.5.
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The average oxidation number of sulfur in S4O62− is +2.
In the formula of ${{\text{S}}_{\text{2}}}{{\text{O}}_{\text{6}}}^{{\text{2 – }}}$ there are 2 sulfur atoms and 6 oxygen atoms and the charge on an ion is -2. Therefore, the oxidation state of sulfur is in ${{\text{S}}_{\text{2}}}{{\text{O}}_{\text{6}}}^{{\text{2} – }}}$ is +5.
so the oxidation state of sulfur is +2.
The tetrathionate anion, S4O62−, is a sulfur oxoanion derived from the compound tetrathionic acid, H2S4O6.
Now look at the terathionate ion (S4O6) which has an overall charge of 2-, we can see that something strange is happening with the oxidation numbers. The oxygen present in the molecule has a total charge of -12 (-2 x 6).
The oxidation states indicated by sulfur are – 2 , 2 , 4 , 6 .
∴x=+6.
S2O32– (thiosulfate) Lewis structure. The thiosulfate ion contains two sulfur atoms and three oxygen atoms. In the Lewis structure of the S2O32 ion, there is a charge of -2 and Oxygen atoms should hold you. The total valence electrons of sulfur and oxygen atoms are used to draw the structure.
Only tin can have a stable +4 oxidation state, while others cannot.
The molecular formula of thiosulfate is S2O32-. Thiosulfate has a central sulfur atom surrounded by three oxygen atoms and one sulfur atom.
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