Rubidium sulfide

Rubidium sulfide
Rubidium sulfide
Are common
Systematic ; name	Rubidium sulfide
Traditional names	Rubidium sulphide
Chem. formula	Rb 2 s
Physical properties
condition	Dark red crystals
Molar mass	203.00 g / mol
Density	2,912 g / cm³
Thermal properties
T. melt.	530 ° C
Classification
Reg. CAS number
PubChem
Smiles
Inchi

Rubidium sulfide is a neutral binary inorganic chemical compound of rubidium with sulfur with the chemical formula Rb ₂ S. Dark red crystals. Forms crystalline hydrate Rb ₂ S • 4H ₂ O.

Content

Getting

Direct synthesis of elements:

{\mathsf {2\ Rb+S\ {\xrightarrow {100-130^{o}C}}\ Rb_{2}S}}

{\ displaystyle {\ mathsf {2 \ Rb + S \ {\ xrightarrow {100-130 ^ {o} C}} \ Rb_ {2} S}}}

By passing hydrogen sulfide through an alkali solution:

{\mathsf {2\ RbOH+H_{2}S\ {\xrightarrow {\ }}\ Rb_{2}S+2\ H_{2}O}}

{\ displaystyle {\ mathsf {2 \ RbOH + H_ {2} S \ {\ xrightarrow {\}} \ Rb_ {2} S + 2 \ H_ {2} O}}}

The interaction of excess rubidium and mercury sulfide , followed by distillation of metals:

{\mathsf {2\ Rb+HgS\ {\xrightarrow {\ }}\ Rb_{2}S+Hg}}

{\ displaystyle {\ mathsf {2 \ Rb + HgS \ {\ xrightarrow {\}} \ Rb_ {2} S + Hg}}}

The decomposition of crystalline hydrate when heated:

{\mathsf {Rb_{2}S\cdot 4H_{2}O\ {\xrightarrow[{-H_{2}O}]{200-250^{o}C}}\ Rb_{2}S\cdot 2H_{2}O\ {\xrightarrow[{-H_{2}O}]{>T}}\ Rb_{2}S}}

{\ displaystyle {\ mathsf {Rb_ {2} S \ cdot 4H_ {2} O \ {\ xrightarrow [{- H_ {2} O}] {200-250 ^ {o} C}} \ Rb_ {2} S \ cdot 2H_ {2} O \ {\ xrightarrow [{- H_ {2} O}] {> T}} \ Rb_ {2} S}}}

Physical Properties

Rubidium sulfide Rb ₂ S - dark red (colorless according to other sources) crystals of cubic syngony , space group F m3m , cell parameters a = 0.767 nm, Z = 4.

Anhydrous powdery Rb ₂ S is pyrophoric in air.

Well soluble in water (with hydrolysis ). Hygroscopic, forms tetrahydrates Rb ₂ S • 4H ₂ O - white or pale yellow crystals.

Chemical Properties

In aqueous solutions it has an alkaline reaction due to hydrolysis by anion :

{\mathsf {S^{2-}+H_{2}O\ {\xrightarrow {\ }}\ HS^{-}+OH^{-}}}

{\ displaystyle {\ mathsf {S ^ {2 -} + H_ {2} O \ {\ xrightarrow {\}} \ HS ^ {-} + OH ^ {-}}}}

Reacts with diluted strong acids:

{\mathsf {Rb_{2}S+2\ HCl\ {\xrightarrow {\ }}\ 2\ RbCl+H_{2}S\uparrow }}

{\ displaystyle {\ mathsf {Rb_ {2} S + 2 \ HCl \ {\ xrightarrow {\}} \ 2 \ RbCl + H_ {2} S \ uparrow}}}

In the reaction with concentrated sulfuric acid, the reducing properties of rubidium sulfide are manifested:

{\mathsf {Rb_{2}S+3\ H_{2}SO_{4}\ {\xrightarrow {\ }}\ 2\ RbHSO_{4}+SO_{2}\uparrow +S\downarrow +2\ H_{2}O}}

{\ displaystyle {\ mathsf {Rb_ {2} S + 3 \ H_ {2} SO_ {4} \ {\ xrightarrow {\}} \ 2 \ RbHSO_ {4} + SO_ {2} \ uparrow + S \ downarrow + 2 \ H_ {2} O}}}

Aqueous solutions are slowly oxidized by atmospheric oxygen to form various products:

{\mathsf {Rb_{2}S\ {\xrightarrow[{-RbOH}]{O_{2}}}\ {\begin{matrix}{\mathsf {S\downarrow }}\\{\mathsf {RbS_{n}}}\\{\mathsf {Rb_{2}S_{2}O_{3}}}\end{matrix}}}}

{\ displaystyle {\ mathsf {Rb_ {2} S \ {\ xrightarrow [{- RbOH}] {O_ {2}}} \ {\ begin {matrix} {\ mathsf {S \ downarrow}} \\ {\ mathsf {RbS_ {n}}} \\ {\ mathsf {Rb_ {2} S_ {2} O_ {3}}} \ end {matrix}}}}}

In solid state it is oxidized to sulfate:

{\mathsf {Rb_{2}S+2\ O_{2}\ {\xrightarrow {500^{o}C}}\ Rb_{2}SO_{4}}}

{\ displaystyle {\ mathsf {Rb_ {2} S + 2 \ O_ {2} \ {\ xrightarrow {500 ^ {o} C}} \ Rb_ {2} SO_ {4}}}}

When boiling the solution with sulfur , polysulfides are formed:

{\mathsf {Rb_{2}S+{\mathit {n}}S\ {\xrightarrow {100^{o}C}}\ Rb_{2}S_{n+1}}}

{\ displaystyle {\ mathsf {Rb_ {2} S + {\ mathit {n}} S \ {\ xrightarrow {100 ^ {o} C}} \ Rb_ {2} S_ {n + 1}}}}

where n = 2 ÷ 5.

When hydrogen sulfide is passed through a solution, hydrosulfide is formed:

{\mathsf {Rb_{2}S+H_{2}S\ {\xrightarrow {\ }}\ Rb_{2}S_{n+1}}}

{\ displaystyle {\ mathsf {Rb_ {2} S + H_ {2} S \ {\ xrightarrow {\}} \ Rb_ {2} S_ {n + 1}}}}

Literature

Lidin R.A. and other Chemical properties of inorganic substances: Textbook. manual for universities. - 3rd ed., Rev. - M .: Chemistry , 2000 .-- 480 p. - ISBN 5-7245-1163-0 .
Chemistry Handbook / Editorial: Nikolsky B.P. et al. - 2nd ed., rev. - M.-L.: Chemistry, 1966. - T. 1. - 1072 p.
Chemistry Handbook / Editorial: Nikolsky B.P. et al. - 3rd ed., rev. - L .: Chemistry, 1971. - T. 2. - 1168 p.

Plyushchev V. E., Stepin B. D. Chemistry and technology of compounds of lithium, rubidium and cesium. - M .: "Chemistry", 1970. - 408 p.