Boron sulfide

Names
IUPAC name

Boron sulfide

Other names

Boron sesquisulfide, Diboron trisulfide

Identifiers

CAS Number

* 12007-33-9 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 23349327

ECHA InfoCard | 100.031.355
EC Number |

* 234-504-9

PubChem CID

* 123269

CompTox Dashboard (EPA)

* DTXSID50923210

InChI

* InChI=1S/B2S3/c3-1-5-2-4

Key: ZVTQDOIPKNCMAR-UHFFFAOYSA-N

SMILES

* S=BSB=S

Properties

Chemical formula

| 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

Solubility in water

| decomposes
Solubility | soluble in ammonia
Structure

Crystal structure

| monoclinic, mP40, SpaceGroup = P21/c, No. 14

Coordination geometry

| B: planar, sp2
Thermochemistry

Heat capacity (C)

| 111.7 J/mol K

Std molar
entropy (S⦵298)

| 327 J/mol K

Std enthalpy of
formation (ΔfH⦵298)

| -240.6 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):

Main hazards

| source of H2S
GHS labelling:

Pictograms

Signal word

| Danger

Hazard statements

| H225, H260, H301, H311, H315, H318, H335

Precautionary statements

| P210, P223, P231+P232, P280, P302+P352, P303+P361+P353, P305+P351+P338, P312, P402+P404, P405
NFPA 704 (fire diamond)  |

[1]

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).

Y verify (what is YN ?)

Infobox references

Chemical compound

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. It is the parent member of the thioborates.

## 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 10060436.70-73&rft.date=1996&rft_id=info:pmid/10060436&rft_id=info:doi/10.1103/physrevlett.76.70&rft_id=info:bibcode/1996PhRvL..76...70K&rft.aulast=Kincs&rft.aufirst=Joseph&rft.au=Martin,+Steve+W.&rft_id=https://lib.dr.iastate.edu/mse_pubs/67&rfr_id=info:sid/en.wikipedia.org:Boron+sulfide" class="Z3988">
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.19080590116.127-135&rft.date=1908&rft_id=info:doi/10.1002/zaac.19080590116&rft.au=Hoffmann,+J.&rft_id=https://zenodo.org/record/1428114&rfr_id=info:sid/en.wikipedia.org:Boron+sulfide" class="Z3988">
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: 46–98.46-98&rft.date=1824&rft.au=Berzelius,+J.&rft_id=https://books.google.com/books?id=pJlPAAAAYAAJ&pg;=PA46&rfr_id=info:sid/en.wikipedia.org:Boron+sulfide" class="Z3988">
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.18240781002.113-150&rft.date=1824&rft_id=info:doi/10.1002/andp.18240781002&rft_id=info:bibcode/1824AnP....78..113B&rft.au=Berzelius,+J.+J.&rft_id=http://gallica.bnf.fr/ark:/12148/bpt6k150878/f123.image.r=Annalen%20der%20Physic.langEN&rfr_id=info:sid/en.wikipedia.org:Boron+sulfide" class="Z3988"> 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.18581050109.67-73&rft.date=1858&rft_id=info:doi/10.1002/jlac.18581050109&rft.au=Wöhler,+F.&rft.au=Deville,+H.+E.+S.-C.&rft_id=https://books.google.com/books?id=muE2AAAAYAAJ&pg;=PA67&rfr_id=info:sid/en.wikipedia.org:Boron+sulfide" class="Z3988">
7. ^ Wöhler, F.; Deville, H. E. S.-C. (1858). "Du Bore". Annales de Chimie et de Physique. 52: 62–93.62-93&rft.date=1858&rft.au=Wöhler,+F.&rft.au=Deville,+H.+E.+S.-C.&rft_id=http://gallica.bnf.fr/ark:/12148/bpt6k347939/f62.table&rfr_id=info:sid/en.wikipedia.org:Boron+sulfide" class="Z3988">
8. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

* v
* t
* e

Boron compounds

Boron pnictogenides|

* BAs
* BN
* BP

Boron halides|

* BBr3
* BCl3
* BF
* BFO
* BF3
* BI3
* B2F4
* B2Cl4

Acids|

* B(NO3)3
* B(OH)3
* BPO4
* B2(OH)4
* BH3O

Boranes|

* BH3
* B2H4
* B2H6
* BH3NH3
* B4H10
* B5H9
* B5H11
* B6H10
* B6H12
* B10H14
* B18H22

Boron oxides and sulfides|

* BO
* B2O3
* B2S3
* B6O

Carbides|

* B4C

Organoboron compounds|

* (BH2Me)2
* BMe3
* BEt3
* Ac4(BO3)2
* COBH3

* v
* t
* e

Sulfides (S2−)

| H2S |  |  |  | He

|
|
|
|

Li2S | BeS | B2S3
+BO3 | CS2
COS | (NH4)SH | O  | F  | Ne
Na2S | MgS | Al2S3 | SiS
SiS2
-Si | PxSy
-P | -S2−
2 | Cl  | Ar
K2S | CaS |  | ScS
Sc2S3 | TiS
TiS2
Ti2S3
TiS3 | VS
VS2
V2S3 | CrS
Cr2S3 | MnS
MnS2 | FeS
Fe3S4 | CoxSy | NixSy | Cu2S
CuS | ZnS | GaS
Ga2S3 | GeS
GeS2
-Ge | As2S3
As4S3
-As | SeS2
+Se | Br  | Kr
Rb2S | SrS |  | Y2S3 | ZrS2 | NbS2 | MoS2
MoS3 | TcS2
Tc2S7 | Ru  | Rh2S3 | PdS | Ag2S | CdS | In2S3 | SnS
SnS2
-Sn | Sb2S3
Sb2S5
-Sb | TeS2 | I  | Xe
Cs2S | BaS | *  | LuS
Lu2S3 | HfS2 | TaS2 | WS2
WS3 | ReS2
Re2S7 | OsS
4 | Ir2S3
IrS2 | PtS
PtS2 | Au2S
Au2S3 | HgS | Tl2S | PbS
PbS2 | Bi2S3 | PoS | At  | Rn
Fr  | Ra  | **  | Lr  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og

*  | LaS
La2S3 | CeS
Ce2S3 | PrS
Pr2S3 | NdS
Nd2S3 | PmS
Pm2S3 | SmS
Sm2S3 | EuS
Eu2S3 | GdS
Gd2S3 | TbS
Tb2S3 | DyS
Dy2S3 | HoS
Ho2S3 | ErS
Er2S3 | TmS
Tm2S3 | YbS
Yb2S3
**  | Ac2S3 | ThS2 | Pa  | US
US2 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No
*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
*[H225]: H225: Highly flammable liquid and vapour
*[H260]: H260: In contact with water releases flammable gases which may ignite spontaneously
*[H301]: H301: Toxic if swallowed
*[H311]: H311: Toxic in contact with skin
*[H315]: H315: Causes skin irritation
*[H318]: H318: Causes serious eye damage
*[H335]: H335: May cause respiratory irritation
*[P210]: P210: Keep away from heat, hot surfaces, sparks, open flames and other ignition sources. No smoking.
*[P223]: P223: Do not allow contact with water.
*[P231+P232]: P231+P232: Handle and store contents under inert gas. Protect from moisture
*[P280]: P280: Wear protective gloves/protective clothing/eye protection/face protection.
*[P302+P352]: P302+P352: IF ON SKIN: Wash with soap and water.
*[P303+P361+P353]: P303+P361+P353: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water [or shower].
*[P305+P351+P338]: P305+P351+P338: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do. Continue rinsing.
*[P312]: P312: Call a POISON CENTER or doctor/physician if you feel unwell.
*[P402+P404]: P402+P404: Store in a dry place. Store in a closed container.
*[P405]: P405: Store locked up.
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