Rubidium hydride

Crystal structure
__ Rb +      __ H -
Crystal system	cubic
Space group	Fm 3 m (No. 225)
Lattice parameters	a = 604.9 pm
General
Surname	Rubidium hydride
Ratio formula	RbH
Brief description	colorless prismatic needles
External identifiers / databases
CAS number 13446-75-8 PubChem 171411 Wikidata Q219571
properties
Molar mass	86.48  g · mol -1
Physical state	firmly
density	2.65 g cm −3
Melting point	Decomposes at 300  ° C
solubility	reacts with water
safety instructions
GHS hazard labeling no classification available
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Rubidium hydride is a chemical combination of rubidium and hydrogen .

Manufacturing

Rubidium hydride can be produced by reacting rubidium and hydrogen.

${\displaystyle {\ce {2Rb + H2 -> 2RbH}}}$

It is also created when heating with magnesium in a hydrogen stream.

${\displaystyle {\ce {Rb2CO3 + Mg + H2 ->[\Delta] 2RbH + MgO + CO2 ^}}}$

properties

Physical Properties

Rubidium hydride crystallizes in the cubic crystal system in the space group Fm 3 m (space group no. 225) with the lattice parameters a = 604.9 pm, and 4 formula units per unit cell .

Chemical properties

When heated in a vacuum , rubidium hydride decomposes into the elements . The connection is extremely reactive.

Rubidium hydride reacts with water to form hydrogen gas.

${\displaystyle {\ce {RbH + H2O -> RbOH + H2 ^}}}$

The reaction with hydrogen chloride also releases hydrogen.

${\displaystyle {\ce {RbH + HCl -> RbCl + H2 ^}}}$

Rubidium formate is formed with carbon dioxide .

${\displaystyle {\ce {RbH + CO2 -> HCOORb}}}$

With sulfur dioxide formed during reaction under reduced pressure Rubidiumdithionit .

${\displaystyle {\ce {2RbH + 2SO2 -> Rb2S2O4 + H2 ^}}}$

Rubidium hydride burns with elemental fluorine to form hydrogen fluoride and rubidium fluoride . The reaction mixture ignites even with elemental chlorine , but the reaction does not take place completely and a green mixed salt remains. Bromine and iodine react less violently.

${\displaystyle {\ce {RbH + F2 -> RbF + HF ^}}}$

With liquid ammonia , rubidium amide is formed with evolution of hydrogen ; at room temperature the reaction with gaseous ammonia takes place only very slowly.

${\displaystyle {\ce {RbH + NH3 -> RbNH2 + H2 ^}}}$

Rubidium hydride reduces lead (II) oxide to elemental lead when heated , copper (II) oxide is reduced to elemental copper .

${\displaystyle {\ce {2RbH + PbO -> RbOH + Pb + H2O}}}$

Individual evidence

1. ↑ ^{a b c d e f} Jean D'Ans, Ellen Lax: Pocket book for chemists and physicists. 3. Elements, inorganic compounds and materials, minerals, Volume 3. 4. Edition, Springer, 1997, ISBN 978-3-540-60035-0 , p. 688 ( limited preview in the Google book search).
2. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. CRC Press, 2009, ISBN 978-1-4200-9084-0 .
3. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
4. ↑ ^{a b c d} R. Abegg, F. Auerbach: Handbuch der inorganic Chemie. Verlag S. Hirzel, Vol. 2, 1908. P. 425. Full text
5. ^ JW Mellor: "A comprehensive treatise on inorganic and theoretical chemistry", Volume 2, Verlag Wiley 1962, p. 2186. ( limited preview in the Google book search).
6. ↑ ^{a b c d} H. Moissan: "Preparation et propriétés des hydrures de rubidium et de césium" in Compt. Rend. Hebd. 1903 , 136 , p. 587. Full text