Barium sulfide

Crystal structure
__ Ba 2+      __ S 2−
Crystal system	cubic
Space group	Fm 3 m (No. 225)
Coordination numbers	Ba [6], S [6]
General
Surname	Barium sulfide
Ratio formula	Bas
Brief description	colorless cubic crystals with a rotten egg smell
External identifiers / databases
CAS number 21109-95-5 EC number 244-214-4 ECHA InfoCard 100.040.180 PubChem 6857597 ChemSpider 5256933 Wikidata Q411656
properties
Molar mass	169.39 g mol −1
Physical state	firmly
density	4.25 g cm −3
Melting point	2227 ° C
boiling point	decomposition
solubility	hydrolysis in water
safety instructions
GHS hazard labeling from  Regulation (EC) No. 1272/2008 (CLP) , expanded if necessary danger H and P phrases H: 290-301-332-314-400 EUH: 031 P: 260-280-301 + 330 + 331-310-303 + 361 + 353-304 + 340 + 310-305 + 351 + 338
MAK	0.5 mg m −3
Thermodynamic properties
ΔH f 0	−460.0 kJ / mol
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Barium sulfide is the sulfide of barium .

Extraction and presentation

Barium sulfide is made from barium sulfate ( heavy spar ); To do this, BaSO ₄ is reduced to BaS with carbon at 1000 ° C in a rotary kiln:

${\displaystyle \mathrm {BaSO_{4}+2\ C\rightarrow BaS+2\ CO_{2}} }$

Barium sulfide of high purity can be obtained in small quantities by heating barium carbonate at around 1000 ° C in a sufficiently strong stream of hydrogen sulfide and hydrogen .

${\displaystyle \mathrm {BaCO_{3}+H_{2}S\longrightarrow BaS+H_{2}O+CO_{2}} }$

properties

Physical Properties

Barium sulfide is a colorless to gray solid that oxidizes easily in air and decomposes when damp. It crystallizes cubically in the sodium chloride structure with a lattice parameter of a  = 6.39 Å and four formula units per unit cell . Impure barium sulfide phosphoresces after exposure to light. This was discovered in Bologna in 1602 (Bolognese light stone) by Vincentio Casciorolo and at that time attracted a great deal of attention from alchemists. Since the discovery preceded that of phosphor, this is the first observation of phosphorescence.

Chemical properties

Barium sulfide releases hydrogen sulfide when exposed to acids :

${\displaystyle \mathrm {BaS+2\ H^{+}\rightarrow Ba^{2+}+H_{2}S\uparrow } }$

use

Barium sulfide is used to make barium salts. It is converted into the corresponding salts with acids. Example:

${\displaystyle \mathrm {BaS+2\ HCl\rightarrow BaCl_{2}+H_{2}S\uparrow } }$

Individual evidence

1. ↑ ^{a b c d} Entry on barium sulfide. In: Römpp Online . Georg Thieme Verlag, accessed on July 14, 2014.
2. ↑ ^{a b c d e f} entry to barium sulfide in the GESTIS database of IFA , retrieved on July 23, 2016(JavaScript required) .
3. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Physical Constants of Inorganic Compounds, pp. 4-50.
4. ↑ Entry on barium sulphide in the Classification and Labeling Inventory of the European Chemicals Agency (ECHA), accessed on February 1, 2016. Manufacturers or distributors can expand the harmonized classification and labeling .
5. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Standard Thermodynamic Properties of Chemical Substances, pp. 5-6.
6. ↑ ^{a b} Georg Brauer (Ed.), With the collaboration of Marianne Baudler u a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 927.