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Boron sulfide
Names
IUPAC name
Boron sulfide
Other names
Boron sesquisulfide, Diboron trisulfide
Identifiers
3D model (JSmol)
ECHA InfoCard 100.031.355 Edit this at Wikidata
EC Number
  • 234-504-9
  • InChI=1S/B2S3/c3-1-5-2-4
    Key: ZVTQDOIPKNCMAR-UHFFFAOYSA-N
  • S=BSB=S
Properties
B2S3
Molar mass 117.80 g/mol
Appearance colorless crystals
Density 1.55 g/cm3, solid
Melting point 563 °C (1,045 °F; 836 K)
Boiling point decomposes at high T
decomposes
Solubility soluble in ammonia
Structure
monoclinic, mP40, SpaceGroup = P21/c, No. 14
B: planar, sp2
Thermochemistry
111.7 J/mol K
327 J/mol K
-240.6 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 source of H2S
GHS labelling:
GHS02: FlammableGHS06: ToxicGHS07: Exclamation mark
Danger
H225, H260, H301, H311, H315, H318, H335
P210, P223, P231+P232, P280, P302+P352, P303+P361+P353, P305+P351+P338, P312, P402+P404, P405
NFPA 704 (fire diamond)
[1]
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineInstability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazards (white): no code
2
3
3
Flash point 18°C (64.4°F)
Safety data sheet (SDS) trc-canada.com
Related compounds
Related compounds
 BCl3
Lawesson's reagent
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Boron sulfide is the chemical compound with the formula B2S3. It is a white, moisture-sensitive solid. It has a polymeric structure. The material has been of interest as a component of "high-tech" glasses and as a reagent for preparing organosulfur compounds.

Reactions[edit]

Like the sulfides of silicon and phosphorus, B2S3 reacts with traces of water, including atmospheric moisture to release H2S. This hydrolysis is described by the following idealized equation:

B2S3 + 3 H2O → B2O3 + 3 H2S

B2S3 readily forms glasses when blended with other sulfides such as P4S10. Such glasses do not absorb mid-frequencies of Infra-red energy relative to conventional borosilicate glasses. Some of these ternary phases that are fast ion conductors.[2]

B2S3 converts ketones into the corresponding thiones. For example, the conversion of benzophenone to its thione proceeds as follows:

B2S3 + 3 (C6H5)2C=O → B2O3 + 3 (C6H5)2C=S

In practice, B2S3 would be used in excess.[3]

Synthesis[edit]

An early synthesis involved the reaction of iron and manganese borides with hydrogen sulfide at temperatures of 300 °C. The conversion is shown for the monoborides in the following idealized equation:[4]

2 FeB + 4 H2S → B2S3 + FeS + 4 H2

The first synthesis was done by Jöns Jakob Berzelius in 1824 by direct reaction of amorphous boron with sulfur vapor.[5]

2 B + 3 S → B2S3

Another synthesis was favoured by Friedrich Wöhler and Henri Etienne Sainte-Claire Deville first published in 1858, starting from boron and hydrogen sulfide.[6][7]

2 B + 3 H2S → B2S3 + 3 H2

Structure[edit]

The boron atoms in B2S3 are trigonal planar, and are arranged in B3S3 and B2S2 rings with bridging S atoms forming a layer structure with an interlayer distance of 355 pm. This is different from boron trioxide which has a three dimensional structure.[8] The molecular, monomeric, form of B2S3 has a planar V shape with the central B-S-B angle of approximately 120°.[8]

References[edit]

  1. ^ Material Safety Data Sheet, VWR, 2010, retrieved November 11, 2023
  2. ^ Kincs, Joseph; Martin, Steve W. (1996). "Non-Arrhenius Conductivity in Glass: Mobility and Conductivity Saturation Effects". Physical Review Letters. 76 (1): 70–73. Bibcode:1996PhRvL..76...70K. doi:10.1103/physrevlett.76.70. PMID 10060436.
  3. ^ Sato, R. (2004). "Boron Trisulfide". In L. Paquette (ed.). Encyclopedia of Reagents for Organic Synthesis. New York: J. Wiley & Sons. doi:10.1002/047084289X.rb255. ISBN 0471936235.
  4. ^ Hoffmann, J. (1908). "Synthese von Borsulfid aus Ferro- und Manganbor". Zeitschrift für anorganische Chemie. 59 (1): 127–135. doi:10.1002/zaac.19080590116.
  5. ^ Berzelius, J. (1824). "Undersökning af flusspatssyran och dess märkvärdigaste föreningar" [Investigation of hydrofluoric acid and of its most noteworthy compounds]. Kongliga Vetenskaps-Academiens Handlingar [Proceedings of the Royal Science Academy]. 12: 46–98.
    Reprinted in German as:
    Berzelius, J. J. (1824). "Untersuchungen über die Flußspathsäure und deren merkwürdigsten Verbindungen". Annalen der Physik und Chemie. 78 (10): 113–150. Bibcode:1824AnP....78..113B. doi:10.1002/andp.18240781002. see especially pages 145–147.
  6. ^ Wöhler, F.; Deville, H. E. S.-C. (1858). "Neue Beobachtungen über das Bor und einige seiner Verbindungen" [New observations concerning boron and some of its compounds]. Liebigs Annalen der Chemie und Pharmacie. 105 (1): 67–73. doi:10.1002/jlac.18581050109.
  7. ^ Wöhler, F.; Deville, H. E. S.-C. (1858). "Du Bore". Annales de Chimie et de Physique. 52: 62–93.
  8. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
source: https://en.wikipedia.org/wiki/Boron_sulfide

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