| Identification | More | [Name]
RUBIDIUM | [CAS]
7440-17-7 | [Synonyms]
37Rb
Rubidio
RUBIDIUM
Chebi:33322
rubidium atom
MUELLER HINTON
RUBIDIUM METAL
Rubidium powder
RUBIDIUM: 99.9%
RUBIDIUM STANDARD
Rb Standard Solution
RUBIDIUM ICP STANDARD
Rubidium Metal Ingots
RUBIDIUM INGOT 98+%
RUBIDIUM, INGOT, 99.6%
Rubidium, breakseal ampoule
Rubidium standard for ICP
Rubidium,99.75%(metalsbasis)
RUBIDIUM ISO 9001：2015 REACH
RUBIDIUM, AAS STANDARD SOLUTION
RUBIDIUM SINGLE ELEMENT STANDARD
RUBIDIUM PLASMA EMISSION STANDARD
Rubidium, Breakseal Ampoule 99.8%
RUBIDIUM, PLASMA STANDARD SOLUTION
RUBIDIUM ATOMIC ABSORPTION STANDARD
RUBIDIUM (99+%) (PRESCORED AMPOULE)
Rubidium, 99.75% trace metals basis
RUBIDIUM (99.9+%) (PRESCORED AMPOULE)
RUBIDIUM (99.9+%) (BREAKSEAL AMPOULE)
RUBIDIUM ICP STANDARD TRACEABLE TO SRM F
RubidiuM ingot, 99.6% trace Metals basis
Rubidium, AAS standard solution, Rb 1000μg/mL
RUBIDIUM PLASMA EMISSION SPECTROSCOPY STANDARD
Rubidium plasma standard solution, Rb 10000μg/mL
Rubidium, ampuled under argon, 99.75% trace metals basis
Rubidium, AAS standard solution, Specpure(R), Rb 1000μg/ml
Rubidium, plasma standard solution, Specpure(R), Rb 1000μg/ml
Rubidium, plasma standard solution, Specpure(R), Rb 10,000μg/ml | [EINECS(EC#)]
231-126-6 | [Molecular Formula]
Rb | [MDL Number]
MFCD00134055 | [Molecular Weight]
85.47 | [MOL File]
7440-17-7.mol |
| Chemical Properties | Back Directory | [Definition]
Metallic element of atomic num-
ber 37, group IA of the periodic table, aw 85.4678,
valence = 1. One stable form, principal natural
radioactive isotope is rubidium-87. It is the sec-
ond most electropositive and the second most alka-
line element, has low | [Appearance]
Soft, silvery-white solid. Easily oxidized
in air.High heat capacity and heat transfer
coefficient. Soluble in acids and alcohol.
| [Melting point ]
38-39 °C(lit.)
| [Boiling point ]
686 °C(lit.)
| [density ]
1.53 g/mL at 25 °C(lit.)
| [solubility ]
reacts with H2O | [form ]
ingot
| [color ]
Silver | [Specific Gravity]
1.532 | [Resistivity]
11.0 μΩ-cm, 20°C | [Water Solubility ]
soluble in acids and alcohol [HAW93] | [Sensitive ]
moisture sensitive | [Merck ]
13,8363 | [Exposure limits]
ACGIH: TWA 2 ppm; STEL 4 ppm
OSHA: TWA 2 ppm(5 mg/m3)
NIOSH: IDLH 25 ppm; TWA 2 ppm(5 mg/m3); STEL 4 ppm(10 mg/m3) | [History]
Rubidium was discovered in 1861 by
Bunsen and Kirchhoff in the mineral lepidolite by use of the
spectroscope. The element is much more abundant than was
thought several years ago. It is now considered to be the 16th
most abundant element in the Earth’s crust. Rubidium occurs
in pollucite, carnallite, leucite, and zinnwaldite, which contains
traces up to 1%, in the form of the oxide. It is found in lepidolite
to the extent of about 1.5%, and is recovered commercially from
this source. Potassium minerals, such as those found at Searles
Lake, California, and potassium chloride recovered from brines
in Michigan also contain the element and are commercial
sources. It is also found along with cesium in the extensive deposits
of pollucite at Bernic Lake, Manitoba. Rubidium can be
liquid at room temperature. It is a soft, silvery-white metallic element
of the alkali group and is the second most electropositive
and alkaline element. It ignites spontaneously in air and reacts
violently in water, setting fire to the liberated hydrogen. As with
other alkali metals, it forms amalgams with mercury and it alloys
with gold, cesium, sodium, and potassium. It colors a flame
yellowish violet. Rubidium metal can be prepared by reducing
rubidium chloride with calcium, and by a number of other
methods. It must be kept under a dry mineral oil or in a vacuum
or inert atmosphere. Thirty-five isotopes and isomers of rubidium
are known. Naturally occurring rubidium is made of two
isotopes, 85Rb and 87Rb. Rubidium-87 is present to the extent of
27.83% in natural rubidium and is a beta emitter with a half-life
of 4.9 × 1010 years. Ordinary rubidium is sufficiently radioactive
to expose a photographic film in about 30 to 60 days. Rubidium
forms four oxides: Rb2O, Rb2O2, Rb2O3, Rb2O4. Because rubidium
can be easily ionized, it has been considered for use in
“ion engines” for space vehicles; however, cesium is somewhat
more efficient for this purpose. It is also proposed for use as a
working fluid for vapor turbines and for use in a thermoelectric
generator using the magnetohydrodynamic principle where rubidium
ions are formed by heat at high temperature and passed
through a magnetic field. These conduct electricity and act like
an armature of a generator thereby generating an electric current.
Rubidium is used as a getter in vacuum tubes and as a photocell
component. It has been used in making special glasses.
RbAg4I5 is important, as it has the highest room-temperature
conductivity of any known ionic crystal. At 20°C its conductivity
is about the same as dilute sulfuric acid. This suggests use in
thin film batteries and other applications. The present cost in
small quantities is about $50/g (99.8% pure). | [CAS DataBase Reference]
7440-17-7(CAS DataBase Reference) | [EPA Substance Registry System]
Rubidium (7440-17-7) |
| Hazard Information | Back Directory | [Chemical Properties]
Soft, silvery-white solid. Easily oxidized
in air.High heat capacity and heat transfer
coefficient. Soluble in acids and alcohol.
| [General Description]
A soft silvery metal. Shipped in very limited quantities sealed in a copper tube and over packed in a wooden box. Used in electronics. | [Reactivity Profile]
RUBIDIUM METAL is a strong reducing agent. Burns spontaneously in dry oxygen [Mellor 2:468 1946-47]. Readily catches fire in air when molten or with a sulfur vapor [Mellor 2: 469 1946-47]. Causes explosive decomposition of maleic anhydride. [Chem Safety Data Sheet SD-88 1962; Chem. Haz. Info. Series C-71 1960] Burns in chlorine [Mellor 2, Supp. 1:380 1956]. Interaction with mercury is exothermic and may be violent, [Mellor, 1941, Vol. 2, 469]. | [Air & Water Reactions]
Tarnishes rapidly upon exposure to air. Reacts violently with water to form corrosive RUBIDIUM(7440-17-7) hydroxide and hydrogen, a flammable gas. The heat of the reaction usually ignites the hydrogen. | [Hazard]
Reacts vigorously with air and water, must
be stored under kerosene or similar liquid, danger-
ous fire and explosion risk. Metal causes serious
skin burns.
| [Health Hazard]
Inhalation or contact with vapors, substance or decomposition products may cause severe injury or death. May produce corrosive solutions on contact with water. Fire will produce irritating, corrosive and/or toxic gases. Runoff from fire control may cause pollution. | [Fire Hazard]
Produce flammable gases on contact with water. May ignite on contact with water or moist air. Some react vigorously or explosively on contact with water. May be ignited by heat, sparks or flames. May re-ignite after fire is extinguished. Some are transported in highly flammable liquids. Runoff may create fire or explosion hazard. | [Isotopes]
There are 30 isotopes of rubidium, ranging from Rb-75 to Rb-98. Rb-85 is theonly stable form of rubidium and constitutes 72.17% of all rubidium isotopes found inthe Earth’s crust. Rb-87 is radioactive (a half-life of 4.9×1010 years) and makes up about27.83% of the remainder of rubidium found in the Earth’s crust. All the other 28 isotopes make up a tiny fraction of all the rubidium found on Earth and are radioactive withvery short half-lives. | [Origin of Name]
Rubidium is named for the Latin word rubidus, meaning “reddish. | [Occurrence]
Rubidium does not exist in its elemental metallic form in nature. However, in compoundforms it is the 22nd most abundant element on Earth and, widespread over most land areasin mineral forms, is found in 310 ppm. Seawater contains only about 0.2 ppm of rubidium,which is a similar concentration to lithium. Rubidium is found in complex minerals and untilrecently was thought to be a rare metal. Rubidium is usually found combined with other Earthmetals in several ores. The lepidolite (an ore of potassium-lithium-aluminum, with traces ofrubidium) is treated with hydrochloric acid (HCl) at a high temperature, resulting in lithiumchloride that is removed, leaving a residue containing about 25% rubidium. Another processuses thermochemical reductions of lithium and cesium ores that contain small amounts ofrubidium chloride and then separate the metals by fractional distillation. | [Characteristics]
Rubidium is located between potassium and cesium in the first group in the periodic table.It is the second most electropositive alkali element and reacts vigorously and explosively in airor water. If placed on concrete on a sunny day, it would melt and then react violently withmoist air to release hydrogen with enough heat to burn the hydrogen. If a chunk of rubidiummetal is left on a table exposed to the air, it combusts spontaneously. Rubidium must be storedin oil, such as kerosene. | [Preparation]
Although rubidium metals have been prepared by fused salt electrolysis, the highly reactive nature of the metals complicates the collection step and favors the use of other preparative methods where the metals can be removed in vapor form from the reaction mixture. The oxides, hydroxides, carbonates, halides, sulphates, chromates and nitrates of rubidium have been reduced to the metals by strong reducing metals such as sodium, calcium, magnesium, barium, iron, zirconium, aluminum or silicon at moderately high temperatures. The preferred method, however, involves the reduction of the anhydrous metal chlorides with calcium metal under vacuum. Anhydrous rubidium chloride is mixed with a large excess of calcium chips and heated under vacuum at 700- 800°C. As the chloride is reduced, metal vapors issue from the reaction mixture and are led under the vacuum to a cooler portion of the vessel where they condense and drop into a collection vessel. | [Production Methods]
Rubidium is recovered from its ore lepidolite or pollucite. Mineral lepidolite is a lithium mica having a composition: KRbLi(OH,F)Al2Si3O10. The ore is opened by fusion with gypsum (potassium sulfate) or with a mixture of barium sulfate and barium carbonate. The fused mass is extracted with hot water to leach out water-soluble alums of cesium, rubidium, and potassium. The solution is filtered to remove insoluble residues. Alums of alkali metals are separated from solution by fractional crystallization. Solubility of rubidium alum or rubidium aluminum sulfate dodecahydrate, RbAl(SO4)2?12H2O falls between potassium and cesium alum.
Alternatively, the mineral is opened by prolonged heating with sulfuric acid. Often calcium fluoride (fluorspar) is added for removal of silicon. Alkali metals are converted into water-soluble sulfates. After filtering residual solid, the solution is treated with ammonium or potassium carbonate or carbon dioxide. Lithium precipitates as lithium carbonate. Alkali metal carbonates are converted back to alums and separated by fractional crystallization.
Rubidium alum obtained by either method above is decomposed by treatment with alkali solutions for removal of aluminum and sulfate. Aluminum is precipitated as aluminum hydroxide. Addition of barium hydroxide to the filtrate removes sulfate, precipitating barium sulfate. Evaporation of the solution crystallizes rubidium as hydroxide.
Rubidium also may be recovered by the chlorostannate method. In this method the alkali metal carbonate solution obtained from the mixed alum is treated with carbon dioxide. Most potassium is precipitated as bicarbonate, KHCO3. Addition of hydrochloric acid converts the carbonates to chlorides. The chlorides are converted to chlorostannates by carefully adding stoichiometric quantities of stannic chloride at pH just below 7:
2RbCl + SnCl4 → Rb2SnCl6
Cesium chlorostannate, Cs2SnCl6, more insoluble than the rubidium salt, precipitates before any rubidium starts to precipitate. Under such controlled addition of stannic chloride, potassium chloride remains in solution in chloride form. Rubidium chlorostannate complex, on thermal decomposition, forms rubidium chloride, RbCl.
Rubidium metal may be obtained from its carbonate, hydroxide or chloride by reduction with magnesium or calcium at high temperatures in the presence of hydrogen:
Rb2CO3 + 3Mg → 2Rb + 3MgO +C
2RbOH + Mg → 2Rb + Mg(OH)2
2RbCl + Ca → 2Rb + CaCl2
Rubidium is a flammable solid. It is stored in dry hexane, isooctane or other saturated hydrocarbon liquids. Alternatively, the metal may be packaged and stored in well-sealed borosilicate glass ampules or stainless-steel containers under vacuum or an inert atmosphere. |
| Safety Data | Back Directory | [Hazard Codes ]
Xi,C,F | [Risk Statements ]
R36/37/38:Irritating to eyes, respiratory system and skin .
R36/38:Irritating to eyes and skin .
R34:Causes burns.
R14/15:Reacts violently with water, liberating extremely flammable gases . | [Safety Statements ]
S26:In case of contact with eyes, rinse immediately with plenty of water and seek medical advice .
S36/37/39:Wear suitable protective clothing, gloves and eye/face protection .
S43:In case of fire, use ... (indicate in the space the precise type of fire-fighting equipment. If water increases the risk add-Never use water) .
S45:In case of accident or if you feel unwell, seek medical advice immediately (show label where possible) .
S36:Wear suitable protective clothing . | [RIDADR ]
UN 2031 8/PG 2
| [WGK Germany ]
3
| [RTECS ]
VL8500000
| [TSCA ]
Yes | [HazardClass ]
8 | [PackingGroup ]
III | [HS Code ]
2805199090 | [Safety Profile]
Moderately toxic by intraperitoneal route. A very reactive alkali metal (more reactive than potassium or cesium). In the body, rubidlum substitutes for potassium as an intracellular ion. The ratio of Rb/K intake is important in the toxicology of rubidium. A ratio above 40% is dangerous. In rats, a failure to gain weight is the first symptom, followed by ataxia and hyperirritabhty. Symptoms include: skin ulcers, poor hair coat, sensitivity, and extreme nervousness leading to convulsions and death.
hazard when exposed to heat or flame or by chemical reaction with oxidlzers. Igmtes on contact with air, oxygen, and halogens. A very dangerous fire and explosion
RUBIDIUM HYDROXIDE RPZOOO 121 5
Ignites spontaneously on contact with water. Reaction with water, moisture, or steam forms explosive hydrogen gas, whch then ignites. Explodes in contact with liquid bromine. Can react explosively with air, halogens, mercury, nonmetals, vanadium chloride oxide, moisture, acids, oxidizers. Violent reaction with vanadium trichloride oxide (at 60℃C), Cl202, P. Molten rubidium ignites in sulfur vapor and reacts vigorously with carbon. RbOH is more basic than KOH. Storage and handling: Keep under benzene, petroleum, or other liquids not containing gaseous O2. When heated to decomposition it emits toxic fumes of RbzO. See also SODIUM and SODIUM POTASSIUM ALLOY. |
| Questions And Answer | Back Directory | [Physical Properties]
Silvery-white metal; body-centered cubic crystals; ductile; soft and very light (the fourth lightest metallic element); Mohs hardness 0.3; density 1.522 g/cm3 at 18°C; melts at 39.3°C; density of the liquid metal 1.472 g/mL at 39°C; vaporizes at 689°C producing a blue vapor; vapor pressure 1 torr at 294°C and 10 torr at 387°C; electrical resistivity 11.6 microhm-cm at 0°C and 13.1 mirohm-cm at 25°C; viscosity 0.484 centipoise at 100°C; magnetic susceptibility 0.09×10–6 cgs units at 18°C; thermal neutron absorption cross section 0.73 barns; reacts violently with water.
| [History and Occurrence]
Rubidium was discovered in 1861 by Kirchoff and Bunsen. They observed new lines in the dark red spectral region of a sample extract of mineral lepidolite. The element got its name from the Latin word rubidus, which means dark red. Bunsen later succeeded in preparing metallic rubidium in low yield by heating rubidium hydrogen tartrate with carbon. The metal was obtained in higher yield by Hevesy and later by Beketov, Hevesy electrolyzing a melt of rubidium hydroxide and Beketov reducing the hydroxide with aluminum at red heat.
Rubidium is widely distributed in nature. Its abundance in the earth’s crust is estimated to be 90 mg/kg. Rubidium occurs at trace levels in many potassium minerals. Often it is associated with cesium. Some rubidium-containing minerals are lepidolite, leucite, petalite, feldspars, pollucite, beryl, and amazonite. The metal is never found as a major constituent in any mineral. Rubidium also occurs in many rocks such as basalts, granites and clay shales. Rubidium is found in seawater at an average concentration of 0.12 mg/L.
| [Uses]
Rubidium metal and its salts have very few commercial applications. They are used in research involving magnetohydrodynamics and thermoionic experiments. Rubidium is used in photocells. The metal also is a getter of oxygen in vacuum tubes. The beta-emitter rubidium –87 is used to determine age of some rocks and minerals. Radioisotopes of rubidium have been used as radioactive tracers to trace the flow of blood in the body. The iodide salt treats goiters. Rubidium salts are in pharmaceuticals as soporifics, sedatives, and for treating epilepsy.
| [Reactions]
Rubidium is a highly reactive metal, more reactive than sodium or potassium. Most reactions are similar to sodium or potassium (see Potassium). The metal ignites spontaneously in air forming oxides. It is coated rapidly with a gray-blue oxide film. It forms four oxides, Rb2O, Rb2O2, Rb2O3, and Rb2O4. It reacts violently with water to form rubidium hydroxide, RbOH:
2Rb + 2H2O → 2RbOH + H2
Reaction with dilute mineral acids can proceed with explosive violence, releasing hydrogen.
Rubidium combines with hydrogen and nitrogen forming hydride, RbH and nitride, Rb3N, respectively.
| [Hazard]
As a highly reactive metal, its contact with water or acids can produce violent reactions. Skin contact can cause serious burns.
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