Sodium disulfide
Crystal structure | ||||||||||||||||
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__ Na + __ S - | ||||||||||||||||
General | ||||||||||||||||
Surname | Sodium disulfide | |||||||||||||||
other names |
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Ratio formula | Na 2 S 2 | |||||||||||||||
Brief description |
yellow solid |
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External identifiers / databases | ||||||||||||||||
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properties | ||||||||||||||||
Molar mass | 110.11 g mol −1 | |||||||||||||||
Physical state |
firmly |
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Melting point |
470 ° C |
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safety instructions | ||||||||||||||||
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As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Sodium disulfide is a chemical compound from the group of sulfides .
Extraction and presentation
Sodium disulfide can be obtained by reacting sodium with sulfur .
The reaction of sodium tetrasulfide dissolved in alcohol with sodium or tetraphenylphosphonium chloride is also possible .
When sodium trisulfide is heated to 100 ° C, it decomposes to a 1: 1 mixture of sodium disulfide and sodium tetrasulfide.
The reaction of sodium sulfide with sulfur is also possible
or sodium with sulfur in liquid ammonia .
properties
Sodium disulfide is a light yellow, very hygroscopic solid. When heated, it gradually turns darker in color and is light red-brown at 400 ° C. Above 475 ° C the color deepens towards dark brown, and the substance begins to sinter strongly and from 490 ° C to melt into a deep dark brown liquid. The products made from an alcohol solution are always olive green in color after melting. It occurs in two allotropic forms, with the α-form below 160 ° C and the β-form irreversibly above. Both have a hexagonal crystal system.
use
Sodium disulfide is used to make other chemical compounds (e.g. diallyl disulfide ).
Individual evidence
- ↑ a b c d e f g Ralf Steudel : Elemental sulfur and sulfur-rich compounds, Volume 2 . 2003, ISBN 3-540-40378-7 , pp. 130 ( limited preview in Google Book search).
- ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
- ↑ a b c d Georg Brauer (Ed.), With the collaboration of Marianne Baudler a . a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 374.