Multiple Oxidation States

[Jaden Nguyen 2A]

Because some elements have several different oxidation states, how do we determine which one to use when drawing the Lewis dot structures? Sulfur, for example, has three different oxidations states so which one would we use? Would it depend on the compound that we’re given?

[Gabriel McDonald 1J]

I think it would depend on the compound. Also, I'm pretty sure that most elements have an oxidation state that is more common than the others. Sulfur, for example, usually loses two electrons because it is in Group 16.

[Rachel Fox - 3F]

Elements such as transition metals do not always follow an octet rule, so when drawing Lewis dot structures for elements like those or for elements like Sulfur or Phosphorus, it would depend on the compound and how many valence electrons you have. For elements like sulfur that can have an expanded octet, we would use formal charge calculations to determine the molecular structure that is most stable, which could include an expanded octet for the sulfur atom. Overall, the oxidation state of a particular element would depend on the compound given and how many valence electrons you have.

[Kaya L]

I would just follow the formal charge and octet rule unless the question states otherwise(as in the question can give you the oxidation state). When drawing Lewis structures, usually when asked to draw a specific amount of resonance structures, the only time things may get weird is when the structures are the same and the bonds are different, leading to a formal charge that isn't zero on some atoms. When this happens, as long as the number of electrons remains the same, even when the valence electrons are not perfectly in the octet rule, it should be ok. Electrons aren't set in a fixed position.