How to find the Oxidation Number for in S (Elemental Sulfur)

To find the correct oxidation state of in S (Sulfur) we use a few rules and some simple math. In addition to elemental Sulfur (S), we’ll also look at several possible oxidation states the Sulfur atoms has when bonded to other atoms.

First, since the S molecule doesn’t have an overall charge (like NO3- or H3O+) we could say that it is a neutral (not an ion). When finding oxidation numbers, neutral elements will have oxidation numbers of zero. So for Sulfur the oxidation number will be zero.

When Sulfur bonds to other atoms it can have different oxidation numbers depending on what it is bonded to. The general rules below will help determine the oxidation state on S.
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GENERAL RULES
Free elements have an oxidation state of zero (e.g. Na, Fe, H2, O2, S8).
In an ion the all Oxidation numbers must add up to the charge on the ion.
In a neutral compound all Oxidation Numbers must add up to zero.
Group 1 = +1
Group 2 = +2
Hydrogen with Non-Metals = +1
Hydrogen with Metals (or Boron) = -1
Fluorine = -1
Oxygen = -2 (except in H2O2 or with Fluorine)
Group 17(7A) = -1 except with Oxygen and other halogens lower in the group

Additional Rule: The more electronegative element in a binary compound is assigned
the number equal to the charge it would have if it were an ion.
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