PRODUCT IDENTIFICATION

75.13

H.S. CODE

TOXICITY

CLASSIFICATION

EXTRA NOTES

PHYSICAL AND CHEMICAL PROPERTIES

white crystalline powder

MELTING POINT

SOLUBILITY IN WATER

Soluble (soluble in ethanol)

REFRACTIVE INDEX

250 C

EXTERNAL LINKS & GENERAL DESCRIPTION

Wikipedia Linking

Google Scholar Search

Drug Information Portal (U.S. National Library of Medicine) - Thioacetamide

PubChem Compound Summary - Thioacetamide

KEGG (Kyoto Encyclopedia of Genes and Genomes) -  Thioacetamide

http://www.ebi.ac.uk/ -  Thioacetamide

http://www.ncbi.nlm.nih.gov/ -  Thioacetamide

Material Safety Data Sheet

Local:
Thioacetamide is used as a sulfur source in the synthesis organic compounds ( rubber chemicals, curing agents, crosslinking agents, metallurgy, pesticides, pharmaceuticals). It is used as a stabilizer of motor fuels. It is used in purification of hydrochloric and sulfuric acids. It is used in leather processing. It is used in laboratories as a substitute for hydrogen sulfide.

The first chemical contrast of thiols and sulfides with alcohols and ethers is acidity which is important in organic reactions. Thiols are stronger acids than relevant alcohols and phenols. Thiolate conjugate bases are easily formed, and are excellent nucleophiles in SN2 reactions of alkyl halides and tosylates. The nucleophilicity of sulfur is much greater than that of oxygen, resulting in a number of useful electrophilic substitution reaction that are rare by oxygen. For example, sulfides form (with alkyl halides) ternary sulfonium salts, in the same alkylattion of tert-amines quaternary ammonium salts, whereas ternary oxonium salts are prepared only under extream conditions. Without exception, sulfoxides, sulfinate salts and sulfite anion also alkylate on sulfur, despite of the partial negative formal charge on oxygen and partial positive charge on sulfur. The second character is the oxidation states of sulfur. Oxygen has only two oxidation states, whereas sulfur covers from –2 to +6 as follows:

• -2: Hydrogen Sulfide (H₂S), sulfides, sulfonium ions
• -1: disulfides
• 0: S elemental, sulfoxides, sulfenic acids
• +2: sulfones, sulfinic acids
• +4: sulfonic acids, sulfite esters
• +6: sulfate esters

One more sulfur compound's contrast with oxygen analog is in oxidation chemistry. Oxidation of sulfur compounds changes the oxidation state of sulfur rather than carbon, whereas, oxidation of  alcohols to aldehydes and ketones changes the oxidation state of carbon not oxygen. Thiols is oxidized to S-S single bond (disufide) which is stronger than O–O bond in peroxide. Disufide forms sulfenyl chlorides (with chlorine in mild condition) or sulfonic acids under harder condition. Oxidation of sulfides with hydrogen peroxide (or peracids) yields sulfoxides and then to sulfones. A certain sulfoxide compound such as dimethyl sulfoxide can be used as an effective oxygen source in the oxidation reaction of primary and secondary alcohols to aldehydes and ketones. DMSO easily is reduced to dimethyl sulfide and water is taken up by the electrophile. oxidation procedure is very mild and tolerates a variety of other functional groups, including those having oxidizable nitrogen and sulfur atoms.

APPEARANCE

white crystalline powder

ASSAY

99.0% min

MELTING POINT

HAZARD OVERVIEW

OSHA Hazards:Carcinogen, Target Organ Effect, Toxic by ingestion, Irritant. Target Organs:Liver

GHS

PICTOGRAMS

HAZARD STATEMENTS

H302-H315-H319-H350-H412

P STATEMENTS

P201-P273-P305 + P351 + P338-P308 + P313

RISK PHRASES

45-22-36/38-52/53

SAFETY PHRASES

53-45-61