Sulfur dichloride

• Sulfur (II ) chloride
• Dichlormonosulfan

Red - brown liquid with a pungent odor

Liquid

1.62 g · cm -3 ( at 15 ° C )

-122 ° C

59.5 ° C

218 hPa ( 20 ° C)

Reacts with water

1.557 (14 ° C)

Risk

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Sulfur is a dark red, toxic, hydrolysis liquid with a characteristic reminiscent of the smell of chlorine.

History

One of the first applications of sulfur was 1846. At that time Alexander Parkes used in carbon disulfide (CS2 ) dissolved sulfur for cold vulcanization of rubber. During the First World War sulfur was used for the production of the chemical warfare agent sulfur mustard.

Production and representation

Laboratory sulfur is produced by reacting sulfur monochloride with chlorine gas. Also possible is the direct reaction of sulfur with a chlorine, wherein a mixture of sulfur monochloride and sulfur dichloride is obtained. Separation of the two liquids can be carried out by distillation in an inert gas atmosphere.

Properties

Physical Properties

Sulfur you Lord is with an enthalpy of formation of -49 kJ / mol a moderately exothermic connection. It is not stable at room temperature and divided into an equilibrium reaction to sulfur monochloride and chlorine. Stabilization is possible by the addition of phosphorus trichloride or phosphorus pentachloride.

Sulfur has C2v symmetry. The sulfur atom is tetrahedrally surrounded by two chlorine atoms and the two free electron pairs. The bond angle between Cl -S -Cl is about 103 degrees, the bond length d ( Cl -S) = 2.01 Å.

Use

Sulfur can be used as chlorinating agent and sulfidation in the synthesis. It reacts with unsaturated compounds such as Allylphenylethern or allyl phenols to the corresponding Thiaheterocyclen or sulfones.

Safety

As with sulfur in a relatively simple manner, the representation of mustard gas is possible, production, use and in particular export are regulated and monitored by law.