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how to calculate the oxidation number of. sulphur in Na2S4O6​

Answer 1

As a consequence, this compound must have sulfur atoms with mixed oxidation states. Since it is normal for sulfur to have oxidation states of -2, 0, +2, +4, and +6, it is most likely that there are three sulfurs with a +2 oxidation state and one sulfur that is +4. The average of these is +2.5. plz mark as brainiest

Answer 2

Let sulfur's oxidation number be X.

So we know based on prior knowledge that sodium, Na when it exists as an ion, it is Na+. Oxygen is 0(2-).

Now this compound is neutral and has an overall oxidation state of 0.

Now that we have got these information, let's use them to construct a mathematical equation.

(2*1), sodium ion charge + 4x, unknown oxidation state of sulfur + (6*-2), oxygen ion charge = 0

2 + 4x - 12=0

4x - 10 = 0

4x = +10

x = +2.5

Hence sulfur has an oxidation state of +2.5.