OK, let me start this off with oxygen, it oxidizes, hence the name. To oxidize, is to grab electrons, right? Regardless, I remember being taught in high school chem that elements in the same column of the periodic table follow mostly the same rules and have similar properties. Does that mean you could use sulfur as an oxidizer, since its right below oxygen? The table on this forum says both are capable of an oxidation state of -2, meaning they both can grab 2 electrons? So both would be equally good at oxidizing, right? So the more negative number the oxidation state is, the more violently its going to grab electrons, right? Now sulfur is also capable of having a positive oxidation state, so it can also donate electrons. This depends on the situation right? And does having this ability make sulfur a lousy oxidizer?
So lets pretend our atmosphere had no oxygen and a bunch of gaseous sulfur in it, if I'm right in sulfur being just as good an oxidizer as oxygen, I could light a candle in it right? But doesn't a hydrocarbon need oxygen for a reason, as opposed to anything else?