RUBIDIO

Rubidio

Biological role

Safety and precautions

Degradation

Uses

Applications

Alloys

Compounds

Productios

Characteristics

Abundance on earth

History

Index

Rubidium was discovered in 1861 by Robert Bunsen and Gustav Kirchhoff in lepidolite using a spectroscope by detecting the two red streaks characteristic of the emission spectrum of this element and which are the reason for its name.

HISTORY

Rubidium is a fairly abundant element in the Earth's crust and is present at up to 310 parts per million (ppm). Because of its abundance, it occupies a place precisely because of the low carbon and chlorine and above fluorine and strontium.

ABUNDANCE ON EARTH

Alkaline metallic element. It has an atomic symbol Rb, atomic number 37 and atomic weight 85.47. It is used as a chemical reagent in the manufacture of photoelectric cells.

CHARACTERISTICS

The metal is obtained by electrolysis of the halide, although it can be obtained on a small scale by heating the chloride with calcium metal and distilling the metal. The metal spontaneously burns in the air and reacts violently with the water.

PRODUCTION

It has the atomic symbol Rb, atomic number 37 and atomic weight 85.47. It is used as a chemical reagent in the manufacture of photoelectric cells. An element that is an alkali metal. It has the atomic symbol Rb, atomic number 37 and atomic weight 85.47.

COMPOUNDS

Rubidium is an alkali, reactive, lightweight, low-melting metal.

ALLOYS

It is mainly used in the manufacture of special crystals for fiber optic telecommunication systems and night vision equipment. Other uses include: Tellurium-rubidium photoemitting coatings on photoelectric cells and electronic detectors.

APPLICATIONS

Rubidium is used in:Photocells Collector (trace gas eliminator) in vacuum tubes Working fluid in steam turbines Rock dating (rubidium-87) Fireworks (rubidium compounds give a purple color) Laser cooling, which is used to cool molecular and atomic samples Make certain types of glass and ceramic products (rubidium salts)

USES

DEGRADATION

reducing rubidium chloride with calcium in vacuum, or heating its hydroxide with magnesium in hydrogen stream

Skin: Remove the material and rinse with soap and water. Dispose of contaminated clothing. Get medical attention quickly. Inhalation: Go outdoors immediately. If irritation persists, get medical attention. Ingestion: Do not induce vomiting. Get medical attention right away.

PRECAUTIONS

Rubidium reacts violently with water and can cause inflammation of the hydrogen released in the reaction: 2 Rb + 2 H2O → 2 RbOH + H. To ensure the purity of the metal and safe handling, it is stored under dry mineral oil, in a vacuum or in an inert atmosphere.

SAFETY

Rubidium has no biological role, and it is not toxic. Your body contains about one-third of a gram of rubidium, and treats it almost exactly the same as potassium

BIOLOGICAL ROLE

END

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ainhoa garcía vergara