Rubidium fluoride

Rubidium fluoride
Names
Other names
Rubidium(I) Fluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.262 Edit this at Wikidata
RTECS number
  • VL8740000
UNII
  • InChI=1S/FH.Rb/h1H;/q;+1/p-1 checkY
    Key: AHLATJUETSFVIM-UHFFFAOYSA-M checkY
  • InChI=1/FH.Rb/h1H;/q;+1/p-1
    Key: AHLATJUETSFVIM-REWHXWOFAO
  • [Rb+].[F-]
Properties
RbF
Molar mass 104.4662 g/mol
Appearance white crystalline solid
Density 3.557 g/cm3
Melting point 795 °C (1,463 °F; 1,068 K)
Boiling point 1,408 °C (2,566 °F; 1,681 K)
130.6 g/100 mL (18 °C)
Solubility in acetone 0.0036 g/kg (18 °C)
0.0039 g/kg (37 °C)
−31.9·10−6 cm3/mol
1.398
Structure
Fm3m (No. 225)
a = 565 pm
4
Thermochemistry
113.9 J·mol−1·K−1
−552.2 kJ/mol
−520.4 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Toxic
GHS labelling:
GHS06: ToxicGHS07: Exclamation markGHS08: Health hazard
Danger
H301, H302, H311, H312, H315, H319, H331, H332, H335, H351
P203, P261, P262, P264, P264+P265, P270, P271, P280, P301+P316, P301+P317, P302+P352, P304+P340, P305+P351+P338, P316, P317, P318, P319, P321, P330, P332+P317, P337+P317, P361+P364, P362+P364, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Flash point Non-flammable
2.5 mg/m3, as F
NIOSH (US health exposure limits):
PEL (Permissible)
 2.5 mg/m3, as F
Related compounds
Other anions
 Rubidium chloride
Rubidium bromide
Rubidium iodide
Rubidium astatide
Other cations
 Lithium fluoride
Sodium fluoride
Potassium fluoride
Caesium fluoride
Francium fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Rubidium fluoride (RbF) is the fluoride salt of rubidium. It is a white crystalline solid with a cubic crystal structure, similar to common salt. It forms two different hydrates, a sesquihydrate with the stoichiometric composition 2RbF·3H2O and a third hydrate with the composition 3RbF·H2O.

Synthesis

There are several methods for synthesising rubidium fluoride. One involves reacting rubidium hydroxide with hydrofluoric acid:

RbOH + HF → RbF + H2O

Another method is to neutralize rubidium carbonate with hydrofluoric acid:

Rb2CO3 + 2HF → 2RbF + H2O + CO2

Another possible method is to react rubidium hydroxide with ammonium fluoride:

RbOH + NH4F → RbF + H2O + NH3

The least used method due to expense of rubidium metal is to react it directly with fluorine gas, as rubidium reacts violently with halogens:

2Rb + F2 → 2RbF

Properties

The enthalpy of solution of rubidium fluoride was determined to be −24.28 kJ/mol.

Rubidium fluoride has a purple or magenta red flame test.

In addition to simple rubidium fluoride, an acidic rubidium fluoride with the molecular formula HRbF2 is also known, which can be produced by reacting rubidium fluoride and hydrogen fluoride. The compounds H2RbF3 and H3RbF4 were also synthesized.

References

  1. 1 2 Aterton Seidell (1940). Solubilities Of Organic Compounds Vol - I. Carnegie-Mellon University Hunt Library, N.Sathyanarayanan. D.Van Nostrand Co.
  2. 1 2 Ans, Jean d'; Lax, Ellen (1998). Taschenbuch für Chemiker und Physiker (in German). Springer. ISBN 978-3-540-60035-0.
  3. ↑ Dickerson, Richard E. (1988). Prinzipien der Chemie (in German). Walter de Gruyter. ISBN 978-3-11-009969-0.
  4. ↑ PubChem. "Rubidium fluoride". pubchem.ncbi.nlm.nih.gov. Retrieved 2026-01-19.
  5. ↑ texte, Académie des sciences (France) Auteur du (1911-01-01). "Comptes rendus hebdomadaires des séances de l'Académie des sciences / publiés... par MM. les secrétaires perpétuels". Gallica. Retrieved 2023-12-24.
  6. 1 2 3 "WebElements". Archived from the original on 2008-04-18. Retrieved 23 February 2006.
  7. ↑ texte, Académie des sciences (France) Auteur du (1911-01-01). "Comptes rendus hebdomadaires des séances de l'Académie des sciences / publiés... par MM. les secrétaires perpétuels". Gallica. Retrieved 2023-12-24.
  8. 1 2 3 Eggeling, Hans; Meyer, Jullius (1905-08-19). "Über die Fluoride des Rubidiums". Zeitschrift für anorganische Chemie. 46 (1): 174–176. doi:10.1002/zaac.19050460111. ISSN 0863-1778.
  9. ↑ A Text-Book of Inorganic Chemistry. Forgotten Books. ISBN 978-1-4510-0469-4.