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Rubidium chloride

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Rubidium chloride
Rubidium chloride's NaCl structure
Rubidium chloride's CsCl structure
Names
Other names
rubidium(I) chloride
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.029.310
PubChem CID
RTECS number
  • VL8575000
UNII
  • InChI=1S/ClH.Rb/h1H;/q;+1/p-1 checkY
    Key: FGDZQCVHDSGLHJ-UHFFFAOYSA-M checkY
  • InChI=1/ClH.Rb/h1H;/q;+1/p-1
  • [Rb+].[Cl-]
Properties
RbCl
Molar mass 120.921 g/mol
Appearance white crystals
hygroscopic
Density 2.80 g/cm3 (25 °C)
2.088 g/mL (750 °C)
Melting point 718 °C (1,324 °F; 991 K)
Boiling point 1,390 °C (2,530 °F; 1,660 K)
77 g/100mL (0 °C)
91 g/100 mL (20 °C)
130 g/100 mL (100 °C)
Solubility in methanol 1.41 g/100 mL
−46.0·10−6 cm3/mol
1.5322
Thermochemistry
52.4 J K−1 mol−1
Std molar
entropy
(S298)
95.9 J K−1 mol−1
−435.14 kJ/mol
Hazards
NFPA 704 (fire diamond)
1
0
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
4440 mg/kg (rat)
Safety data sheet (SDS) Fisher Scientific
Related compounds
Other anions
Rubidium fluoride
Rubidium bromide
Rubidium iodide
Rubidium astatide
Other cations
Lithium chloride
Sodium chloride
Potassium chloride
Caesium chloride
Francium chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Rubidium chloride is the chemical compound with the formula RbCl. This alkali metal halide salt is composed of rubidium and chlorine, and finds diverse uses ranging from electrochemistry to molecular biology.

Structure

In its gas phase, RbCl is diatomic with a bond length estimated at 2.7868 Å. This distance increases to 3.285 Å for cubic RbCl, reflecting the higher coordination number of the ions in the solid phase.

Depending on conditions, solid RbCl exists in one of three arrangements or polymorphs as determined with holographic imaging:

Sodium chloride (octahedral 6:6)

The sodium chloride (NaCl) polymorph is most common. A cubic close-packed arrangement of chloride anions with rubidium cations filling the octahedral holes describes this polymorph. Both ions are six-coordinate in this arrangement. The lattice energy of this polymorph is only 3.2 kJ/mol less than the following structure's.

Caesium chloride (cubic 8:8)

At high temperature and pressure, RbCl adopts the caesium chloride (CsCl) structure (NaCl and KCl undergo the same structural change at high pressures). Here, the chloride ions form a simple cubic arrangement with chloride anions occupying the vertices of a cube surrounding a central Rb+. This is RbCl's densest packing motif. Because a cube has eight vertices, both ions' coordination numbers equal eight. This is RbCl's highest possible coordination number. Therefore, according to the radius ratio rule, cations in this polymorph will reach their largest apparent radius because the anion-cation distances are greatest.

Sphalerite (tetrahedral 4:4)

The sphalerite polymorph of rubidium chloride has not been observed experimentally. This is consistent with the theory; the lattice energy is predicted to be nearly 40.0 kJ/mol smaller in magnitude than those of the preceding structures.

Synthesis and reaction

The most common preparation of pure rubidium chloride involves the reaction of its hydroxide with hydrochloric acid, followed by recrystallization:

RbOH + HCl → RbCl + H2O

Because RbCl is hygroscopic, it must be protected from atmospheric moisture, e.g. using a desiccator. RbCl is primarily used in laboratories. Therefore, numerous suppliers (see below) produce it in smaller quantities as needed. It is offered in a variety of forms for chemical and biomedical research.

Rubidium chloride reacts with sulfuric acid to give rubidium hydrogen sulfate.

Radioactivity

Every 18 mg of rubidium chloride is equivalent to approximately one banana equivalent dose due to the large fraction (27.8%) of naturally-occurring radioactive isotope rubidium-87.

Uses


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