Strontium
Strontium granules
CAS: 7440-24-6
Molecular Formula: Sr
Strontium - Names and Identifiers
Strontium - Physico-chemical Properties
| Molecular Formula | Sr |
| Molar Mass | 87.62 |
| Density | 2.6 g/mL at 25 °C (lit.) |
| Melting Point | 757 °C (lit.) |
| Boling Point | 1384 °C (lit.) |
| Water Solubility | reacts quickly with H2O; soluble alcohol [HAW93] |
| Solubility | H2O: soluble |
| Appearance | random pieces |
| Specific Gravity | 2.54 |
| Color | White to pale yellow |
| Exposure Limit | ACGIH: TWA 2 ppm; STEL 4 ppmOSHA: TWA 2 ppm(5 mg/m3)NIOSH: IDLH 25 ppm; TWA 2 ppm(5 mg/m3); STEL 4 ppm(10 mg/m3) |
| Merck | 13,8915 |
| Storage Condition | 2-8°C |
| Sensitive | Air & Moisture Sensitive |
| Physical and Chemical Properties | Silvery white soft metal. The relative density was 2.63. Melting point 769 °c. Boiling point 1384 °c. Face-centered cube. Chemical properties between calcium and barium, active strong, rapid oxidation in the air, the surface of the formation of a yellow oxide film. Spontaneous combustion can occur when it is pulverized in air. Heating can combine with hydrogen to form strontium hydride. It is also easy to react with halogen elements and phosphorus. Resistivity (20 ℃)23 μ Ω? cm, heat of fusion 7.43kJ/mol; Heat of vaporization 136.9 kJ/tool. Electronegativity 1.10. When water is decomposed to release hydrogen and a lot of heat, so that the hydrogen causes combustion, a deep red flame. Soluble in acids and produce hydrogen to cause combustion, soluble in alcohol. |
Strontium - Risk and Safety
| Risk Codes | R37/38 - Irritating to respiratory system and skin. R41 - Risk of serious damage to eyes R38 - Irritating to the skin R14 - Reacts violently with water R11 - Highly Flammable R36/38 - Irritating to eyes and skin. R34 - Causes burns R23/24/25 - Toxic by inhalation, in contact with skin and if swallowed. R36 - Irritating to the eyes R14/15 - |
| Safety Description | S26 - In case of contact with eyes, rinse immediately with plenty of water and seek medical advice. S45 - In case of accident or if you feel unwell, seek medical advice immediately (show the label whenever possible.) S36/37/39 - Wear suitable protective clothing, gloves and eye/face protection. S27 - Take off immediately all contaminated clothing. S23 - Do not breathe vapour. |
| UN IDs | UN 3264 8/PG 3 |
| WGK Germany | 3 |
| RTECS | WK8400000 |
| TSCA | Yes |
| Hazard Class | 4.3 |
| Packing Group | II |
Strontium - Reference Information
| resistivity (resistivity) | 23 μΩ-cm, 20°C |
| EPA chemical information | Information provided by: ofmpub.epa.gov (external link) |
| Introduction | The symbol of strontium is Sr, and the atomic number is 38. It is the fourth member of the second main group of the periodic table. Strontium is a typical alkaline earth element. The electronic structure is a structure with two additional external 5s electrons. Strontium is an alkaline earth metal, a soft silvery white or yellowish metal element with high chemical reactivity. Due to its extremely strong reactivity with oxygen and water, this element only exists naturally in compounds with other elements. When exposed to air, the metal turns yellow. Isotope 90Sr exists in radioactive dust with a half-life of 28.90 years. Strontium is usually present in nature and is the 15th most abundant element on the earth, accounting for an average of 0.034% of all igneous rocks. It is mainly found in the form of sulfate minerals celestite (SrSO4) and carbonate strontium ore (SrCO3). |
| Discovery history | Strontium and strontium mines are named after a village in Scotland, and minerals were discovered for the first time from ore mined by lead mines nearby. In 1787, an interesting mineral came to Edinburgh from a lead mine located in a small village on the shore of Lake Sunat, Argyll Lake, in the highlands of western Scotland. At the time, the substance was thought to be some kind of barium compound. Three years later, Adair Crawford, Scott's Irish chemist, published a paper claiming that the mineral possessed a new species that included new chemical elements. Other chemists later prepared a number of compounds with this element, noting that it caused the candle's flame to burn red and the barium compound to emit green. Thomas Hope, another professor of medicine at the University of Glasgow, named this new mineral strontium in 1793. In studying the electrolysis of various alkaline soils containing molten chlorides such as SrCl2 and mercury oxide, Humphrey Davy finally separated them in 1808. He announced his work in a lecture at the Royal Society on 30 June 1808. In keeping with the naming of other alkaline soils, he renamed it strontium. |
| Source | Strontium metal is not found in nature. Its salts and oxides account for only 0.025% of the earth's crust. There are 29 isotopes of strontium, ranging from Sr-75 to Sr-102. The four natural forms of strontium are stable rather than radioactive. These stable isotopes are Sr-84, accounting for 0.56% of the elements on the earth; Sr-86, accounting for 9.86%; Sr-87, accounting for 7.00% of the total; Sr-88, accounting for 82.58% of strontium on the earth. The remaining isotopes are radioactive, with half-lives ranging from a few microseconds to minutes, hours, days or years. Most, but not all, are produced in nuclear reactors or nuclear explosions. Two important radioisotopes are Sr-89 and Sr-90. |
| Application | The two main minerals of strontium are carbonate, strontium strontium SrCO3 and celestite SrSO4 with higher sulfate content. Since most applications involve calcium and barium, the element strontium has only a small use. Strontium alloys are used as "getter" for vacuum tubes ". It was incorporated into glass to make a picture tube for a color television set. Strontium compounds are used in tracer rounds and fireworks to produce red flares. Strontium titanate is a gem. Radioactive strontium 90 with a half-life of 29 years is a high-energy beta emitter. It is the product of nuclear fission. This isotope is a light nuclear power source in spacecraft and long-range weather stations. |
| Preparation | Strontium was found in the ores of strontium ore (SrCO3) and celestite (SrSO4) in Mexico and Spain. When these ores are treated with hydrochloric acid (HCl), they produce strontium chloride (SrCl2), which, together with potassium chloride (KCl), forms a eutectic mixture to lower the melting point of SrCl2 as a molten electrolyte in the graphite dish-shaped electrolysis device. The Sr cations produced by this process are collected at the cathode, where they acquire electrons to form the strontium metal. At the same time, Cl-ions release electrons at the anode and release them in the form of chlorine Cl2. |
| Hazardous | Strontium metal may explode spontaneously in powder form. Strontium and some of its compounds explode when heated. Some compounds can explode if struck with a hammer. Strontium and some of its compounds react with water to form strontium hydroxide [Sr(OH)2] and release hydrogen. The heat generated by the exothermic reaction may cause hydrogen to burn or explode. [Sr 2H2O → Sr(OH)2 H2 ↑] Some compounds, such as strontium chromate and strontium fluoride, are carcinogens and can be poisoned if ingested. Strontium 90 is particularly dangerous because it is a radioactive bone searcher that replaces calcium in bone tissue. Radiation poisoning and death may occur in people exposed to overdose Sr-90. Far from the source of the explosion, animals and plants may inhale strontium 90 and some other radioactive isotopes produced by the explosion of nuclear weapons, and then transport them to the atmosphere. This and other factors have led to the prohibition of atmospheric testing of nuclear and thermosenuclear weapons. |
| toxicity | strontium powder is easy to cause fire and explosion hazards when exposed to fire. Heating above the melting point can also ignite spontaneously. Because strontium reacts with water to release hydrogen; when strontium metal is stored in wet conditions, there may be a danger of gas explosion. It also easily reacts with halogen and phosphorus. When encountering acids, it will react violently and release hydrogen. The toxicity of strontium is between calcium and barium. Mistaking can cause gastrointestinal symptoms, limb pain convulsions, and a few cases can involve the myocardium. Radioactive strontium 89 and strontium 90 are highly toxic, and animals are injected intraperitoneally with metal strontium LD50:88~247 mg/kg. Patients should be removed from the contaminated area, placed to rest and keep warm. If you accidentally splash your eyes, you need to wash them with a lot of water for 15 min. In severe cases, you can see a doctor for diagnosis and treatment. Skin contact first rinse with water, and then wash thoroughly with soap. If there is burns, see a doctor for diagnosis and treatment. Wash your mouth immediately after taking it by mistake and rush to the hospital for treatment. |
| use | getter for alloys and vacuum tubes. It is used to make alloys, as a getter for electronic tubes, as well as chemical analysis, flue gas production, etc. |
| production method | the thermo-reduction method first thermally decomposes strontium nitrate to produce strontium oxide, uses fine-grained aluminum as reducing agent, the batching ratio is carried out according to 3SrO:2AI, strontium oxide and aluminum are first made into group ore, and the group ore is loaded into a steel distiller for vacuum degassing treatment. the treatment temperature is 90 ℃, and the vacuum degree should finally be 10mmHg. The inner cylinder made of thin iron plate is put into the whole distiller, and the reduction reaction is carried out at 1150 ℃ for 12h to obtain strontium deposit with a purity of 99%. Reduce the distiller to below 500 ℃, then take out the inner sliver and cut it, peel off the sediment, and make a finished product of strontium metal. |
| toxic substance data | information provided by: pubchem.ncbi.nlm.nih.gov (external link) |
Last Update：2024-04-09 02:00:04
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