Talk:Sulfur difluoride

S2F4

Does sulfur difluoride really form a dimer S₂F₄, or is this formula a typing error (instead, S₂F₂ and SF₄ could be meant)? By now, I haven't found much about this compound, so I can't say if this statement is true or if someone (not necessarily the Wikipedia author) has mistaken the formulas... --79.243.249.124 (talk) 20:54, 4 August 2013 (UTC)

I expanded this part, taking material from the Greenwood and Earnshaw. Main group halides in low oxidation states behave strangely. --Smokefoot (talk) 22:30, 4 August 2013 (UTC)

Postive Charges on Fluorine

One of the way for producing SF2 is given as OF2 + H2S → SF2 + H2O. This indicates fluorine atoms carry positive oxidation charges. Is this possible? Anyways, 2p orbitals are strange. Most of the elements achieve highest oxidation state when they are bonded to oxygen, not fluorine. In general, oxides are thermally more stable than fluorides and/ or nitrides.Anoop Manakkalath (talk) 08:37, 27 April 2022 (UTC)