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  2. Sulfurous acid - Wikipedia

    en.wikipedia.org/wiki/Sulfurous_acid

    Sulfurous acid is commonly known to not exist in its free state, and due to this, it is stated in textbooks that it cannot be isolated in the water-free form. [4] However, the molecule has been detected in the gas phase in 1988 by the dissociative ionization of diethyl sulfite. [5]

  3. Bisulfite - Wikipedia

    en.wikipedia.org/wiki/Bisulfite

    The bisulfite anion exists in solution as a mixture of two tautomers. One tautomer has the proton attached to one of the three oxygen atoms. In the second tautomer the proton resides on sulfur. The S-protonated tautomer has C 3v symmetry. The O-protonated tautomer has only C s symmetry.

  4. Hyposulfite - Wikipedia

    en.wikipedia.org/wiki/Hyposulfite

    The sulfoxylate anion (SO 2− 2) The thiosulfate anion (S 2 O 2− 3) Sodium thiosulfate, a salt containing the thiosulfate anion; S 2 O 2− 2, a reported sulfur oxyanion. However salts containing S 2 O 2− 2 and HS 2 O − 2 are not well characterized; they would be conjugate bases derived from the parent thiosulfurous acid (H 2 S 2 O 2 ...

  5. Oxyacid - Wikipedia

    en.wikipedia.org/wiki/Oxyacid

    The suffix -ite occurs in names of anions and salts derived from acids whose names end to the suffix -ous. On the other hand, the suffix -ate occurs in names of anions and salts derived from acids whose names end to the suffix -ic. Prefixes hypo-and per-occur in the name of anions and salts; for example the ion ClO − 4 is called perchlorate. [8]

  6. Sulfoxylic acid - Wikipedia

    en.wikipedia.org/wiki/Sulfoxylic_acid

    The complementary base is the sulfoxylate anion SO 2− 2 which is much more stable. In between these states is the HSO − 2 ion, also somewhat stable. Sulfoxylate ions can be made by decomposing thiourea dioxide in an alkaline solution. [4] To do this, thiourea dioxide first forms an amidine-sulfinic acid tautomer, H 2 NC(=NH)SO 2 H, which ...

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  8. Bisulfide - Wikipedia

    en.wikipedia.org/wiki/Bisulfide

    Bisulfide (or bisulphide in British English) is an inorganic anion with the chemical formula HS − (also written as SH −). It contributes no color to bisulfide salts, and its salts may have a distinctive putrid smell. It is a strong base. Bisulfide solutions are corrosive and attack the skin.

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